CHAPTER 20

CHEMICAL BONDING

Stability in Bonding

bull Most matter is found in compounds ie air water salt

bull Compounds have properties unlike those of their individual elements

bull Salt NaCl= Na + Cl bull Na is a grey soft metal that

reacts violently w waterbull Cl is a greenish-yellow gas

that is toxic if inhaledbull 1 atom Na + 1 atom Cl = NaClbull NaCl is a chemical formula

bull Chemically combine to form something we put on our french fries

H2O ne H2O ne H2O

bull Numbers in some chemical formulas are called subscripts

bull Means ldquowritten belowrdquobull This tells how many atoms of

that element combine with the other element(s)

bull Ammonia NH3 = 1 N atom for every 3 H atoms 1N3H ratio

Try these

bull SiO2 silicon dioxide

bull C2H5OH ethanol

bull H2SO4 sulfuric acid

bull C6H12O6 sugar

bull KMnO4 potassium permanganate

Chemical bonds are forces that hold atoms together in a compound

bull Chemical Formula tells what elements it contains w symbols

bull Tells ratio of the atoms of those atoms w subscripts

bull Elements bond to become chemically stable (happy )

bull They become resistant to change

bull Outer E level completely filled with e- (usually 8 e-)

bull Gaining losing or sharing e- cause chemical change

20-2 Types of Bonds Ions are atoms that have lost or gained an e-bull This gives them a positive (+ lose e-) or

negative (- gain e-) chargebull Draw Lewis structures for each elementbull Put brackets around the symbol [ ]bull Then write a superscript + or ndash sign (see bottom

of pg 609 or top of pg 603) outside of the brackets

Ionic Bonds

bull Force of attraction between the opposite charges of the ions in an ionic compound

bull Atoms gain or lose e- to become stablebull Metals usually lose e- ( in outer E

level)bull Non-metals usually gain e- bull Now both atoms are stable (happy )

Ionic bondingbull NaCl

bull Whiteboard practice

bull MgF2

bull CaCl2bull LiBrbull KI

bull Mg3P2

Covalent bonding

bull Molecules are formed when e- are SHAREDbull Sharing e- to become stable (8 e-outer level) is more

common than losinggaining e-bull Diatomic molecules 2 atoms of the same element

bull Cl2 O2 H2 N2 F2

bull These would be nonpolar molecules they share e- equally

Covalent bonding contbull e- not always shared equally polar

molecules are between 2 different non-metal elements

bull Unequal sharing causes the molecule to have a (+) and a (ndash) end

bull e- spend more timenear the Othan the 2 H atoms

CHEMICAL BONDING REVIEWIonic bonding forms ions which can be positive or

negativeCovalent bonding forms molecules which can be polar or

non-polarElements that are close together on the periodic table

(non-metals) usually form covalent bondsElements far apart on the periodic table (metals amp non-

metals) form ionic bonds

Extra Credit Draw dot diagram for sugar

C6 H12 O6

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Stability in Bonding

bull Most matter is found in compounds ie air water salt

bull Compounds have properties unlike those of their individual elements

bull Salt NaCl= Na + Cl bull Na is a grey soft metal that

reacts violently w waterbull Cl is a greenish-yellow gas

that is toxic if inhaledbull 1 atom Na + 1 atom Cl = NaClbull NaCl is a chemical formula

bull Chemically combine to form something we put on our french fries

H2O ne H2O ne H2O

bull Numbers in some chemical formulas are called subscripts

bull Means ldquowritten belowrdquobull This tells how many atoms of

that element combine with the other element(s)

bull Ammonia NH3 = 1 N atom for every 3 H atoms 1N3H ratio

Try these

bull SiO2 silicon dioxide

bull C2H5OH ethanol

bull H2SO4 sulfuric acid

bull C6H12O6 sugar

bull KMnO4 potassium permanganate

Chemical bonds are forces that hold atoms together in a compound

bull Chemical Formula tells what elements it contains w symbols

bull Tells ratio of the atoms of those atoms w subscripts

bull Elements bond to become chemically stable (happy )

bull They become resistant to change

bull Outer E level completely filled with e- (usually 8 e-)

bull Gaining losing or sharing e- cause chemical change

20-2 Types of Bonds Ions are atoms that have lost or gained an e-bull This gives them a positive (+ lose e-) or

negative (- gain e-) chargebull Draw Lewis structures for each elementbull Put brackets around the symbol [ ]bull Then write a superscript + or ndash sign (see bottom

of pg 609 or top of pg 603) outside of the brackets

Ionic Bonds

bull Force of attraction between the opposite charges of the ions in an ionic compound

bull Atoms gain or lose e- to become stablebull Metals usually lose e- ( in outer E

level)bull Non-metals usually gain e- bull Now both atoms are stable (happy )

Ionic bondingbull NaCl

bull Whiteboard practice

bull MgF2

bull CaCl2bull LiBrbull KI

bull Mg3P2

Covalent bonding

bull Molecules are formed when e- are SHAREDbull Sharing e- to become stable (8 e-outer level) is more

common than losinggaining e-bull Diatomic molecules 2 atoms of the same element

bull Cl2 O2 H2 N2 F2

bull These would be nonpolar molecules they share e- equally

Covalent bonding contbull e- not always shared equally polar

molecules are between 2 different non-metal elements

bull Unequal sharing causes the molecule to have a (+) and a (ndash) end

bull e- spend more timenear the Othan the 2 H atoms

CHEMICAL BONDING REVIEWIonic bonding forms ions which can be positive or

negativeCovalent bonding forms molecules which can be polar or

non-polarElements that are close together on the periodic table

(non-metals) usually form covalent bondsElements far apart on the periodic table (metals amp non-

metals) form ionic bonds

Extra Credit Draw dot diagram for sugar

C6 H12 O6

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

H2O ne H2O ne H2O

bull Numbers in some chemical formulas are called subscripts

bull Means ldquowritten belowrdquobull This tells how many atoms of

that element combine with the other element(s)

bull Ammonia NH3 = 1 N atom for every 3 H atoms 1N3H ratio

Try these

bull SiO2 silicon dioxide

bull C2H5OH ethanol

bull H2SO4 sulfuric acid

bull C6H12O6 sugar

bull KMnO4 potassium permanganate

Chemical bonds are forces that hold atoms together in a compound

bull Chemical Formula tells what elements it contains w symbols

bull Tells ratio of the atoms of those atoms w subscripts

bull Elements bond to become chemically stable (happy )

bull They become resistant to change

bull Outer E level completely filled with e- (usually 8 e-)

bull Gaining losing or sharing e- cause chemical change

20-2 Types of Bonds Ions are atoms that have lost or gained an e-bull This gives them a positive (+ lose e-) or

negative (- gain e-) chargebull Draw Lewis structures for each elementbull Put brackets around the symbol [ ]bull Then write a superscript + or ndash sign (see bottom

of pg 609 or top of pg 603) outside of the brackets

Ionic Bonds

bull Force of attraction between the opposite charges of the ions in an ionic compound

bull Atoms gain or lose e- to become stablebull Metals usually lose e- ( in outer E

level)bull Non-metals usually gain e- bull Now both atoms are stable (happy )

Ionic bondingbull NaCl

bull Whiteboard practice

bull MgF2

bull CaCl2bull LiBrbull KI

bull Mg3P2

Covalent bonding

bull Molecules are formed when e- are SHAREDbull Sharing e- to become stable (8 e-outer level) is more

common than losinggaining e-bull Diatomic molecules 2 atoms of the same element

bull Cl2 O2 H2 N2 F2

bull These would be nonpolar molecules they share e- equally

Covalent bonding contbull e- not always shared equally polar

molecules are between 2 different non-metal elements

bull Unequal sharing causes the molecule to have a (+) and a (ndash) end

bull e- spend more timenear the Othan the 2 H atoms

CHEMICAL BONDING REVIEWIonic bonding forms ions which can be positive or

negativeCovalent bonding forms molecules which can be polar or

non-polarElements that are close together on the periodic table

(non-metals) usually form covalent bondsElements far apart on the periodic table (metals amp non-

metals) form ionic bonds

Extra Credit Draw dot diagram for sugar

C6 H12 O6

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Try these

bull SiO2 silicon dioxide

bull C2H5OH ethanol

bull H2SO4 sulfuric acid

bull C6H12O6 sugar

bull KMnO4 potassium permanganate

Chemical bonds are forces that hold atoms together in a compound

bull Chemical Formula tells what elements it contains w symbols

bull Tells ratio of the atoms of those atoms w subscripts

bull Elements bond to become chemically stable (happy )

bull They become resistant to change

bull Outer E level completely filled with e- (usually 8 e-)

bull Gaining losing or sharing e- cause chemical change

20-2 Types of Bonds Ions are atoms that have lost or gained an e-bull This gives them a positive (+ lose e-) or

negative (- gain e-) chargebull Draw Lewis structures for each elementbull Put brackets around the symbol [ ]bull Then write a superscript + or ndash sign (see bottom

of pg 609 or top of pg 603) outside of the brackets

Ionic Bonds

bull Force of attraction between the opposite charges of the ions in an ionic compound

bull Atoms gain or lose e- to become stablebull Metals usually lose e- ( in outer E

level)bull Non-metals usually gain e- bull Now both atoms are stable (happy )

Ionic bondingbull NaCl

bull Whiteboard practice

bull MgF2

bull CaCl2bull LiBrbull KI

bull Mg3P2

Covalent bonding

bull Molecules are formed when e- are SHAREDbull Sharing e- to become stable (8 e-outer level) is more

common than losinggaining e-bull Diatomic molecules 2 atoms of the same element

bull Cl2 O2 H2 N2 F2

bull These would be nonpolar molecules they share e- equally

Covalent bonding contbull e- not always shared equally polar

molecules are between 2 different non-metal elements

bull Unequal sharing causes the molecule to have a (+) and a (ndash) end

bull e- spend more timenear the Othan the 2 H atoms

CHEMICAL BONDING REVIEWIonic bonding forms ions which can be positive or

negativeCovalent bonding forms molecules which can be polar or

non-polarElements that are close together on the periodic table

(non-metals) usually form covalent bondsElements far apart on the periodic table (metals amp non-

metals) form ionic bonds

Extra Credit Draw dot diagram for sugar

C6 H12 O6

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Chemical bonds are forces that hold atoms together in a compound

bull Chemical Formula tells what elements it contains w symbols

bull Tells ratio of the atoms of those atoms w subscripts

bull Elements bond to become chemically stable (happy )

bull They become resistant to change

bull Outer E level completely filled with e- (usually 8 e-)

bull Gaining losing or sharing e- cause chemical change

20-2 Types of Bonds Ions are atoms that have lost or gained an e-bull This gives them a positive (+ lose e-) or

negative (- gain e-) chargebull Draw Lewis structures for each elementbull Put brackets around the symbol [ ]bull Then write a superscript + or ndash sign (see bottom

of pg 609 or top of pg 603) outside of the brackets

Ionic Bonds

bull Force of attraction between the opposite charges of the ions in an ionic compound

bull Atoms gain or lose e- to become stablebull Metals usually lose e- ( in outer E

level)bull Non-metals usually gain e- bull Now both atoms are stable (happy )

Ionic bondingbull NaCl

bull Whiteboard practice

bull MgF2

bull CaCl2bull LiBrbull KI

bull Mg3P2

Covalent bonding

bull Molecules are formed when e- are SHAREDbull Sharing e- to become stable (8 e-outer level) is more

common than losinggaining e-bull Diatomic molecules 2 atoms of the same element

bull Cl2 O2 H2 N2 F2

bull These would be nonpolar molecules they share e- equally

Covalent bonding contbull e- not always shared equally polar

molecules are between 2 different non-metal elements

bull Unequal sharing causes the molecule to have a (+) and a (ndash) end

bull e- spend more timenear the Othan the 2 H atoms

CHEMICAL BONDING REVIEWIonic bonding forms ions which can be positive or

negativeCovalent bonding forms molecules which can be polar or

non-polarElements that are close together on the periodic table

(non-metals) usually form covalent bondsElements far apart on the periodic table (metals amp non-

metals) form ionic bonds

Extra Credit Draw dot diagram for sugar

C6 H12 O6

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

20-2 Types of Bonds Ions are atoms that have lost or gained an e-bull This gives them a positive (+ lose e-) or

negative (- gain e-) chargebull Draw Lewis structures for each elementbull Put brackets around the symbol [ ]bull Then write a superscript + or ndash sign (see bottom

of pg 609 or top of pg 603) outside of the brackets

Ionic Bonds

bull Force of attraction between the opposite charges of the ions in an ionic compound

bull Atoms gain or lose e- to become stablebull Metals usually lose e- ( in outer E

level)bull Non-metals usually gain e- bull Now both atoms are stable (happy )

Ionic bondingbull NaCl

bull Whiteboard practice

bull MgF2

bull CaCl2bull LiBrbull KI

bull Mg3P2

Covalent bonding

bull Molecules are formed when e- are SHAREDbull Sharing e- to become stable (8 e-outer level) is more

common than losinggaining e-bull Diatomic molecules 2 atoms of the same element

bull Cl2 O2 H2 N2 F2

bull These would be nonpolar molecules they share e- equally

Covalent bonding contbull e- not always shared equally polar

molecules are between 2 different non-metal elements

bull Unequal sharing causes the molecule to have a (+) and a (ndash) end

bull e- spend more timenear the Othan the 2 H atoms

CHEMICAL BONDING REVIEWIonic bonding forms ions which can be positive or

negativeCovalent bonding forms molecules which can be polar or

non-polarElements that are close together on the periodic table

(non-metals) usually form covalent bondsElements far apart on the periodic table (metals amp non-

metals) form ionic bonds

Extra Credit Draw dot diagram for sugar

C6 H12 O6

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Ionic Bonds

bull Force of attraction between the opposite charges of the ions in an ionic compound

bull Atoms gain or lose e- to become stablebull Metals usually lose e- ( in outer E

level)bull Non-metals usually gain e- bull Now both atoms are stable (happy )

Ionic bondingbull NaCl

bull Whiteboard practice

bull MgF2

bull CaCl2bull LiBrbull KI

bull Mg3P2

Covalent bonding

bull Molecules are formed when e- are SHAREDbull Sharing e- to become stable (8 e-outer level) is more

common than losinggaining e-bull Diatomic molecules 2 atoms of the same element

bull Cl2 O2 H2 N2 F2

bull These would be nonpolar molecules they share e- equally

Covalent bonding contbull e- not always shared equally polar

molecules are between 2 different non-metal elements

bull Unequal sharing causes the molecule to have a (+) and a (ndash) end

bull e- spend more timenear the Othan the 2 H atoms

CHEMICAL BONDING REVIEWIonic bonding forms ions which can be positive or

negativeCovalent bonding forms molecules which can be polar or

non-polarElements that are close together on the periodic table

(non-metals) usually form covalent bondsElements far apart on the periodic table (metals amp non-

metals) form ionic bonds

Extra Credit Draw dot diagram for sugar

C6 H12 O6

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Ionic bondingbull NaCl

bull Whiteboard practice

bull MgF2

bull CaCl2bull LiBrbull KI

bull Mg3P2

Covalent bonding

bull Molecules are formed when e- are SHAREDbull Sharing e- to become stable (8 e-outer level) is more

common than losinggaining e-bull Diatomic molecules 2 atoms of the same element

bull Cl2 O2 H2 N2 F2

bull These would be nonpolar molecules they share e- equally

Covalent bonding contbull e- not always shared equally polar

molecules are between 2 different non-metal elements

bull Unequal sharing causes the molecule to have a (+) and a (ndash) end

bull e- spend more timenear the Othan the 2 H atoms

CHEMICAL BONDING REVIEWIonic bonding forms ions which can be positive or

negativeCovalent bonding forms molecules which can be polar or

non-polarElements that are close together on the periodic table

(non-metals) usually form covalent bondsElements far apart on the periodic table (metals amp non-

metals) form ionic bonds

Extra Credit Draw dot diagram for sugar

C6 H12 O6

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Covalent bonding

bull Molecules are formed when e- are SHAREDbull Sharing e- to become stable (8 e-outer level) is more

common than losinggaining e-bull Diatomic molecules 2 atoms of the same element

bull Cl2 O2 H2 N2 F2

bull These would be nonpolar molecules they share e- equally

Covalent bonding contbull e- not always shared equally polar

molecules are between 2 different non-metal elements

bull Unequal sharing causes the molecule to have a (+) and a (ndash) end

bull e- spend more timenear the Othan the 2 H atoms

CHEMICAL BONDING REVIEWIonic bonding forms ions which can be positive or

negativeCovalent bonding forms molecules which can be polar or

non-polarElements that are close together on the periodic table

(non-metals) usually form covalent bondsElements far apart on the periodic table (metals amp non-

metals) form ionic bonds

Extra Credit Draw dot diagram for sugar

C6 H12 O6

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Covalent bonding contbull e- not always shared equally polar

molecules are between 2 different non-metal elements

bull Unequal sharing causes the molecule to have a (+) and a (ndash) end

bull e- spend more timenear the Othan the 2 H atoms

CHEMICAL BONDING REVIEWIonic bonding forms ions which can be positive or

negativeCovalent bonding forms molecules which can be polar or

non-polarElements that are close together on the periodic table

(non-metals) usually form covalent bondsElements far apart on the periodic table (metals amp non-

metals) form ionic bonds

Extra Credit Draw dot diagram for sugar

C6 H12 O6

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

CHEMICAL BONDING REVIEWIonic bonding forms ions which can be positive or

negativeCovalent bonding forms molecules which can be polar or

non-polarElements that are close together on the periodic table

(non-metals) usually form covalent bondsElements far apart on the periodic table (metals amp non-

metals) form ionic bonds

Extra Credit Draw dot diagram for sugar

C6 H12 O6

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

bull Oxidation is a + or - assigned to an element to show its combining ability in a compound

bull It indicates how many e- an atom has lost gained or shared when bonding

bull NaCl Na loses 1 e- 1+ oxidation bull Cl gains 1 e- 1- oxidation bull Write the oxidation rsquos on your periodic

table from pg 616

203 Writing Formulas and Naming Compounds

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

bull Some elements have more than 1 oxidation

bull Usually the Transition elementsbull Use Roman numerals to show the

different oxidation rsquosbull Copy Table 2 from pg 616 onto the

back of your periodic tablebull Do the same for Table 3 pg 618

and Table 4 pg 619 and Table 5 pg 621

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

How to write binary ionic formulas

bull Binary compound composed of 2 different elements (ie NaCl)

bull 1) write the symbol for the elements w the (+) oxidation (H amp metals are +)

bull 2) then write the symbol of the element w the (-) oxidation (non-metals)

bull 3) add subscripts so the sum of the oxidation rsquos of the atoms are zero

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Letrsquos Practicebull Bromine and Potassiumbull 1) Potassium is + K1+

bull 2) Bromine is - Br1-

bull 3) (1+) + (1-) = 0 so no subscripts are neededbull 4) KBrbull Nitrogen and Magnesiumbull 1) Magnesium is + Mg2+

bull 2) Nitrogen is - N3-

bull 3) (2+) + (3-) ne 0 so you need to add subscriptsbull 4) Use crossover method the ox of Mg becomes the

subscript for N ox of N becomes the subscript for Mg Mg3N2

bull DO NOT USE + OR ndash SIGN IN SUBSCRIPT

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

PRACTICE WITH WHITEBOARDS

bull Flourine and Lithiumbull Chlorine and Aluminumbull Calcium and Oxygenbull Oxygen and Sodiumbull Potassium and Chlorinebull Strontium and Sulfurbull Beryllium and Nitrogenbull Iodine and Rubidium

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Naming chemical compounds

bull 1) Write the name of the (+) elementbull 2) If this element has more than 1 ox

(check the back of your periodic table) use the ox of the (-) element to figure out the ox of the (+) element use a Roman numeral after the elementrsquos name

bull 3) use Table 3 (back of your PT) to name the second element

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Letrsquos Practicebull CuIbull 1) Cu is (+) Copper (is it a lsquospecial

ionrsquo Look on the back of your PT)bull 2) I is (-) itrsquos ox is (1-) so we should

use Copper (I)bull 3) I is iodine which changes to iodide in

binary compoundsbull 4) Copper (I) iodide

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

WHITEBOARD PRACTICE

bull MgF2

bull PbO2

bull Na2O

bull LiBrbull BaSbull CuO

bull FeF3

bull Cr2O3

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Compounds with Polyatomic Ionsbull Poly many so polyatomic having many

atomsbull Polyatomic ion positively or negatively

charge group of atoms that act as one when bonding

bull Table 4 is just a short list

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Naming with polyatomic ions

bull 1) Write positive part firstbull 2) Use Table 4 from the back of your

PTbull Example NaOHbull 1) Na is positive sodiumbull 2) OH hydroxidebull 3) sodium hydroxide

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Whiteboard practice

bull Cu(OH)2

bull CaCO3

bull Al(C2H3O2)3

bull (NH4)3PO4

bull CuSO4

bull Ba(ClO3)2

bull NH4Cl

bull PbCO3

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Writing formulas w polyatomics

bull Same rules as for binary compoundsbull Plus step 4 write parentheses around

polyatomic ion when more than one of that ion is needed

bull Example iron III nitratebull 1) iron (III) = Fe3+

bull 2) nitrate = NO3 1-

bull 3) You will need 3 (NO3) to make ox rsquos = zerobull 4) Subscript is written outside the ( ) otherwise

it would look like FeNO33

bull Fe(NO3)3

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

WHITEBOARD PRACTICE

bull Potassium chloratebull Ammonium chloridebull Sodium sulfatebull Magnesium chloratebull Lead (II) carbonatebull Chromium (III) phosphatebull Lithium nitratebull Calcium acetate

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20

Compounds with added water

bull Hydrate is a compound that has water chemically attached to its ions

bull CoCl26H2O Cobalt chloride hexahydrate

bull Hexa= 6 hydrate= H2Obull Ca(NO3)23H2O bull Mg3(PO4)24H20