ch. 7 (con’t.) formula writing & naming of compunds
TRANSCRIPT
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Ch. 7 (Con’t.)Formula Writing &
Naming of Compunds
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Predicting Charges on Monatomic IonsPredicting Charges on Monatomic IonsKNOW THESE !!!!KNOW THESE !!!!
+1 +2 -3 -2 -1 0
Cd+2
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Chemical Formulas• Chemical formula-
– Consists of element symbols and subscripts C6H12O6
– Formula Units – simplest whole # ratios of ions present in a compound (for ionic compounds)
– Molecular Formulas- used for covalently bonded compounds.
• (show EVERY atom present in a molecule)
• Ex. H2O
Water has 2 hydrogen atoms and 1 oxygen atom
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Example: Aluminum ChlorideStep 1:
Step 2:
1 3
Step 3:
Al Cl
Al Cl
3+ 1-
write symbols & charge of elements
criss-cross charges as subscripts
combine as formula unit(“1” is never shown) (use smallest whole # ratio)Make sure you remove charges!!
Aluminum Chloride
AlCl3
Cation (metal) always written 1st!
Writing Balanced Chemical FormulasCriss-Cross Rule for Ionic Compounds
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InBr3BaS
charge on cation “becomes” subscript of anion charge on anion “becomes” subscript of cation
** Warning: Reduce subscripts to lowest terms.
Al2O3
Al3+ and O2–
Al2 O3
Ba2+ and S2–
Ba2 S2
In3+ and Br1–
In1 Br3
aluminum oxide barium sulfide indium bromide
Ones are not included in formulas!!
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Example: Magnesium Oxide
Step 1: Magnesium Oxide
Step 2: Mg2+ O2-
Step 3: Mg O2 2
Step 4: Mg2O2
Step 5: MgO
Criss-Cross Rule
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Putting Ions Together
Na+ + Cl- = NaCl
Ca+2 + O-2= CaO Na+ + O-2 = Na2O
Al+3 + S-2 = Al2S
3Ca+2 + N-3 = Ca
3N
2
Ca+2 + Cl- = CaCl2
You try these!
Mg+2 + F- =
K+ + Cl- = Al+3 + I- =
Sr+2 + P-3 =
Li+ + Br- =
Sr3P
2
AlI3
MgF2
KCl
LiBr
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Crisscross
• Switch the numerical value of the charges
Ba2+ N3-2 3
Ba3N2• Reduce ratio if possible
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Learning Check
Write the correct formula for the compounds containing the following ions:
1. Na+, S2-
a) NaS b) Na2S c) NaS2
2. Al3+, Cl-
a) AlCl3 b) AlCl c) Al3Cl
3. Mg2+, N3-
a) MgN b) Mg2N3 c) Mg3N2
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Solution
1. Na+, S2-
b) Na2S
2. Al3+, Cl-
a) AlCl3
3. Mg2+, N3-
c) Mg3N2
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Polyatomic IonsThere are some ions that are made up of more than one type of atom, these are called Polyatomic ions – groups of covalently bonded atoms with a charge
For example, the polyatomic ion known as ammonium NH4
+ has 4 atoms of hydrogen and one atom of nitrogen, HOWEVER, the whole “group” has an overall charge of +1
** you need to memorize the formulas & the charges of many polyatomic ions!
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NO3-
nitrate ion
NO2-
nitrite ion
Polyatomic Ions
Polyatomic Ions
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Naming Ternary Ionic Compoundscontain at least 3 elements & the 1st is a metal:there MUST be at least one polyatomic ion
(it helps to circle the ions)Examples:
NaNO3 Sodium nitrate
K2SO4 Potassium sulfate
Al(HCO3)3 Aluminum bicarbonate
or
Aluminum hydrogen carbonate
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What About. . .What if I have to put multiple polyatomic ions in a compound, for example, magnesium nitrate?
Magnesium has a charge of +2
Nitrate is polyatomic ion and has a charge of -1
Therefore, we need 2 nitrate ions for each magnesium
In this case, we put the entire polyatomic ion in parenthesis and put the subscript outside the parenthesis
Our answer would be Mg(NO3)2
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IONIC COMPOUNDSremember: they have oppositely-charged
ions in a rigid 3-D pattern
IONIC COMPOUNDSremember: they have oppositely-charged
ions in a rigid 3-D pattern
NH4+
Cl-
ammonium chloride, NHammonium chloride, NH44ClCl
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Ternary Ionic Nomenclature
Sodium SulfateNa+ and SO4 -2
Na2SO4
Iron (III) hydroxideFe+3 and OH-
Fe(OH)3
Ammonium carbonateNH4
+ and CO3 –2
(NH4)2CO3
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(NH4)3N
Fe2(Cr2O7)3
Sn(SO4)2
NH4ClO3
Mg(NO2)2
BaSO4
Writing Formulas w/Polyatomic Ions
Reminder! Parentheses are required only when you need more than one “bunch” of a particular polyatomic ion.
Ba2 and SO4
2–
Mg2+ and NO21–
NH41+ and ClO3
1–
Sn4+ and SO42–
Fe3+ and Cr2O72–
NH41+ and N3–
barium sulfate
magnesium nitrite
ammonium chlorate
tin (IV) sulfate
iron (III) dichromate
ammonium nitride
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Learning Check
1. aluminum nitrate
a) AlNO3 b) Al(NO)3 c) Al(NO3)3
2. copper(II) nitrate
a) CuNO3 b) Cu(NO3)2 c) Cu2(NO3)
3. Iron (III) hydroxide
a) FeOH b) Fe3OH c) Fe(OH)3
4. Tin(IV) hydroxide
a) Sn(OH)4 b) Sn(OH)2 c) Sn4(OH)
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• Many polyatomic ions with the same endings on their names have a different number of oxygen atoms attached to the central atom.
• For example
chlorate ClO3-1
sulfate SO4-2
phosphate PO4-3
acetate C2H3O2-1
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Polyatomic Ion: a group of atoms that stay together and have a single, overall charge.
BrO41-
Perbromate ion
BrO31-
Bromate ion
BrO21-
Bromite ion
BrO1-
Hypobromite ion
CO42- CO3
2-
Carbonate ion
CO22- CO2-
ClO41- ClO3
1-
Chlorate ion
ClO21- ClO1-
IO41- IO3
1-
Iodate ion
IO21- IO1-
NO41- NO3
1-
Nitrate ion
NO21- NO1-
PO53- PO4
3-
Phosphate ion
PO33- PO2
3-
SO52- SO4
2-
Sulfate ion
SO32- SO2
2-
1 more oxygen “normal” 1 less oxygen 2 less oxygen
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Salt metal polyatomic ion # Oxygen
atoms
________ per_____ate 1 more O ________ _____ate common ________ _____ite 1 less O
________ hypo_____ite 2 less O’s
________ _____ide 0 O’s
The table below shows the prefixes and suffixes that tell the number of oxygen atoms present in the negative ion.
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The oxy-ions of chlorine & bromine all have these trends in common. Look for them below……
perchlorate ClO4-1
chlorate ClO3-1
chlorite ClO2-1
Hypochlorite ClO-1
Perbromate BrO4-1
Bromate BrO3-1
Bromite BrO2-1
Hypobromite BrO-1
The most productive method of committing these ions to memory is first memorize the ones that have the -ate ending. This is the most common ending.
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Practice Problem #2sodium chlorite
Choose the correct formula for the compound
1. NaCl
2. NaClO
3. NaClO2
4. Na(ClO)2
5. none of the above
next problem
PrefixesPeriodic Chart
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Naming CompoundsNaming Compounds
What's in a name? That which we call a roseby any other name would smell as sweet." - William Shakespeare, Romeo and Juliet (II, ii)
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Naming CompoundsNaming Compounds
• 1. Cation first, then anion
• 2. Monatomic cation = name of the element
• Ca2+ = calcium ion
• 3. Monatomic anion = root + -ide
• Cl = chloride
• CaCl2 = calcium chloride
Binary Ionic Compounds (metal & nonmetal):Binary Ionic Compounds (metal & nonmetal):
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Name these ions
Cl1- Chloride ion N3- Nitride ion Br1- Bromide ion O2- Oxide ion Ga3+ Gallium ion
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Naming Binary Ionic Compounds
Examples:
NaCl
ZnI2
Al2O3
sodium chloride
zinc iodide
aluminum oxide
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Formulas to Names: Ternary Compounds
KMnO4
potassium
I’m a polyatomi
c ion
1. Write the names of the ions
Final Name permanganate
If the positive ion has a fixed charge, you are finished.
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Formulas to Names: Ternary Compounds
NH4NO3
ammonium
I’m a polyatomi
c ion
1. Write the names of the ions
Final Name
nitrate
If the positive ion has a fixed charge, you are finished.
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Learning Check
Match each set with the correct name:
1. Na2CO3 a) magnesium sulfite
MgSO3 b) magnesium sulfate
MgSO4 c) sodium carbonate
2 . Ca(HCO3)2 a) calcium carbonate
CaCO3 b) calcium phosphate
Ca3(PO4)2 c) calcium bicarbonate
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Practice Naming Ionic Compounds
• Na2CO3 -- • CaSO4 --
• KBr --
• MgS --
• BeCl2 --
• NH4F --
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Multiple Oxidation Numbers•When the metal in an ionic compound is
multi-valent (has more than 1 charge) there are 2 naming methods: – Latin & Stock Systems
•Latin is older (not useful for some compounds)
•The metal is named with it’s Latin or English root and ends in -ic or –ous to denote charge.
•E.g. Cu+1 is cuprous, E.g. Cu+2 is cupric•Lower = ous, Higher = ic
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Cu+2 + Cl-1 = CuCl2
= cupric chloride
Cu+1 + Cl-1 = CuCl = cuprous chloride
For Latin naming: know rules, possible charges, Latin names, & suffixes
Write the balanced formula for copper chloride & name it:
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Examples of Older Names of Cations formed from Transition Metals
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• The oxidation number (charge) of the metal is indicated in parentheses using Roman numerals
• E.g. Cu1+ is copper(I), Cu2+ is copper(II)• Numbers refer to charges not to #s of
atoms• Try: Cu2++Cl-1 & Cu1++Cl-1, • Cu+2++Cl-1 = CuCl2 = copper (II) chloride
Co+1 + Cl-1 = CuCl = copper (I) chloride
Multiple valence: Stock System
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Formula to Name:How do I figure out the Roman
Numeral??Hint: We’ve already learned this!
• 1) Assign the element with the unknown charge a charge of x
• 2) Multiply the charge of each element by the number of atoms of that element to get the total charge.
• 3) Add the products from step 2 and set them equal to zero because compounds are neutral- zero charge
• 4) Solve for the unknown charge.
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Binary CompoundsContaining a Metal of Variable Oxidation Number
To name these compounds, give the name of the metal (Type II cations) followed by Roman numerals in parentheses to indicate the oxidation number of the metal, followed by the name of the nonmetal, with its ending replaced by the suffix –ide.
Examples Stock System
FeCl2
(“ic” ending = higher oxidation state; “ous” is lower oxidation state)
SnO Tin oxideSnO2 Tin oxide
(II)(III)
(II)(IV)
Traditional (OLD) System
Ferrous chlorideFerric chloride
Stannous oxideStannic oxide
Iron chlorideIron chlorideFeCl3
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Ternary Ionic Nomenclature
Writing Formulas
• Write each ion, cation first. Don’t show charges in the final formula.
• Overall charge must equal zero.– If charges cancel, just write symbols.– If not, use subscripts to balance charges.
• Use parentheses to show more than one of a particular polyatomic ion.
• Use Roman numerals indicate the ion’s charge when needed (Stock System)
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How do I figure out the Roman Numeral?
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Solving for the roman numeral (charge) of Fe2O3
• (2x) + (3)(-2) = 0– # of Fe atoms times charge of Fe + number of
O atoms times charge of O = zero because compounds are neutral, no charge
• 2x + (-6) = 0• 2x – 6 = 0• 2x = 6• x= 3• Answer for the name: Iron (III) oxide
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Examples #6- Formulas to Names
Cu2S
copper
I’m not a polyatomi
c ion
2. Determine the charge of the positive ion
1. Write the names of the ions
Final Name
sulfide(I)
2Cux (S)-2 = 0
2X + (-2) = 0
X = +1
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Examples #1- Formulas to Names
CuSO3
copper
I’m a polyatomi
c ion
1. Write the names of the ions
Final Name
sulfite(II)
x
X + (- 2) = 0
X = +2
Cu SO3
= 0
You must know the charge on the sulfite ion is -2
The sum of the positive and negative charges must equal zero
2. Determine the charge of the positive ion
-
2
+2 +2
Next
+2
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Examples #4- Formulas to Names
SnF2
tin
2. Determine the charge of the positive ion
1. Write the names of the ions
Final Name
fluoride(II)
Snx (F-1)2 = 0
X + 2(-1) = 0
X = +2
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Example #3-Names to Formulas
nickel(III) acetate
Ni C2H3O2
2. Determine number of ions
1. Write symbols of elements
Final Formula
(Ni+3)x(C2H3O2-1)y
= 0
3X = 1y
X(+3) + y(-1) = 0
X 1Y 3=
1Choose the lowest set of integers that
satisfies the equation
(C2H3O2)3
If there is only one atom the “1” is not shown
Next
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Practice Problem #1Fe(NO3)3
Choose the correct name for the compound
1. Iron trinitrate
2. iron(I) nitrate
3. iron(III) nitrite
4. iron(III) nitrate
5. none of the abovenext
problemPolyatomic
IonsPeriodic Chart
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Learning Check
Complete the names of the following binary
compounds with variable metal ions:
FeBr2 iron (_____) bromide
CuCl copper (_____) chloride
SnO2 ___(_____ ) ______________
Fe2O3 ________________________
Hg2S ________________________
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Nomenclaturefor molecular (Covalent) binary
compounds (two nonmetals)• Uses a Prefix System
• 1 .Less electronegative atom comes first. (towards left side of P.T.)
•2. Add numerical prefixes to indicate # of atoms of each element.
3. Change the ending of the second element to –ide (since it’s binary)
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mono- 1 hepta- 7 di- 2 octa- 8 tri- 3 nona- 9 tetra- 4 deca- 10 penta- 5 hexa- 6
In order to be effective in using prefixes to name compounds containing two non-metals, these prefixes must be committed to memory:
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Naming covalent compounds1 mono
2 di
3 tri
4 tetra
5 penta
6 hexa
7 hepta
8 octa
9 nona
10 deca
• prefix refers to # of atoms - not chargeN2O4 = dinitrogen tetroxide
• Exception: don’t use mono for first element
CO2 = carbon dioxide• The first vowel is often dropped to
avoid the combination of “ao” or “oo”.CO = carbon monoxide
(monooxide)P4O10= tetraphosphorus decoxide
(decaoxide)
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Covalent Compounds: Name to FormulaYou’ll like this!
For covalent compounds, simply use the numerical prefixes to tell you the number (subscript) of each element (No charges, No criss-cross, No balancing needed!):What is the formula for dinitrogen trioxide?
N2O3
dinitrogen monoxide?
N2O
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Example #1-Names to Formulas
Sulfur trioxide
S O1 3
I’m a Binary Compound
2. Write number of atoms
1. Write symbols of elements
Final Formula
If no prefix, then 1 is implied and not written
Two Non metals:
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Example #2-Names to Formulas
dichlorine heptaoxide
Cl O2 7
I’m a Binary Compound
2. Write number of atoms
1. Write symbols of elements
Final Formula
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Example #3-Names to Formulas
oxygen difluoride
O F1 2
I’m a Binary Compound
2. Write number of atoms
1. Write symbols of elements
Final FormulaIf no prefix, then 1 is
implied and not written
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Example #4-Names to Formulas
dinitrogen tetraoxide
N O2 4
I’m a Binary Compound
2. Write number of atoms
1. Write symbols of elements
Final Formula
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Example #5-Names to Formulas
phosphorus pentachloride
PCl1 5
I’m a Binary Compound
2. Write number of atoms
1. Write symbols of elements
Final FormulaIf no prefix, then 1 is
implied and not written
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Examples #2- Formulas to Names
XeF3
xenonmono
tri
I’m a Binary
Compound
2. Write prefix for number of atoms
1. Write names of elements –last element ends in -ide
Final Name
fluorideIf first prefix is mono, it is implied and not written
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Example - Formulas to Names
AsI3
arsenic
mono
tri
I’m a Binary
Compound
2. Write number of atoms
1. Write names of elements
(-ide on last)
Final Name
iodideIf first prefix is mono, it is implied and not written
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Examples #1- Formulas to Names
CCl4
carbon
mono
tetra
I’m a Binary
Compound
2. Write number of atoms
1. Write names of elements
Final Name
chlorideIf first prefix is mono, it is implied and not written
Two Non metals:
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Write and name the following covalent compounds (IUPAC)
carbon tetrachloride
diphosporus trioxide
iodine heptafluoride
CCl4
P2O3
IF7
For more lessons, visit www.chalkbored.com
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• CF4
• N2O
• SBr6
–carbon tetrafluoride
–dinitrogen monoxide
–sulfur hexabromide
Molecular Nomenclature: Examples
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• arsenic trichloride
• dinitrogen pentoxide
• tetraphosphorus decoxide
–AsCl3
–N2O5
–P4O10
More Molecular Examples
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Learning Check
Fill in the blanks to complete the following names of covalent compounds.
CO carbon ______oxide
CO2 carbon _______________
PCl3 phosphorus _______chloride
CCl4 carbon ________chloride
N2O _____nitrogen _____oxide
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Learning Check
1. P2O5 a) phosphorus oxide
b) phosphorus pentoxide
c) diphosphorus pentoxide
2. Cl2O7 a) dichlorine heptoxide
b) dichlorine oxide
c) chlorine heptoxide
3. Cl2 a) chlorine
b) dichlorine
c) dichloride
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Practice Problem #1ClF3
Choose the correct name for the compound
1. carbon iodine trifluoride
2. chlorine trifluorine
3. chlorine trifluoride
4. chlorine tetrafluoride
5. none of the above
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Practice Problem #2arsenic pentabromide
Choose the correct formula for the compound
1. AsBr5
2. ArBr5
3. AsBr7
4. As5Br5. none of the above
next problem
PrefixesElement List
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Practice Problem #3N2O3
Choose the correct name for the compound
1. nitrogen trioxide
2. dinitride trioxide
3. dinitrogen trioxygen
4. dinitrogen trioxide
5. none of the abovenext
problemPrefixes
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Practice Problem #6dichlorine monoxide
Choose the correct formula for the compound
1. ClO
2. Cl2O
3. ClO2
4. Cl2O2
5. none of the above
next problem
Prefixes
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Acid Nomenclature• AcidsAcids
– Compounds that form HCompounds that form H++ in water. in water.
– Formulas usually begin with ‘H’.Formulas usually begin with ‘H’.
– In order In order to be considered an acidto be considered an acid, , they they
must be aqueous (dissolved in water – must be aqueous (dissolved in water –
formulas end in aq)formulas end in aq)
• Examples:Examples:
– HCl HCl (aq)(aq) – hydrochloric acid – hydrochloric acid
– HNOHNO3 3 (aq)(aq) – nitric acid – nitric acid
– HH22SOSO4 4 (aq)(aq) – sulfuric acid – sulfuric acid
We will look at binary & ternary acids!
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Naming Binary Acids
• H + 1 other element HX(aq)
• If the anion attached to hydrogen ends in -ide, add the prefix hydro- and change -ide to -ic acid
• HCl - hydrogen chloride becomes• hydrochloric acid
• H2S - hydrogen sulfide becomes
• hydrosulfuric acid
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Naming Ternary Acids
• H + a polyatomic ion – HXO(aq)
• change the suffix -ate to -ic acid
• HNO3(aq) not hydrogen nitrate, but
– nitric acid• change the suffix -ite to -ous acid
• HNO2(aq) not hydrogen nitrite, but
– nitrous acid• Ternary Acid names DO NOT begin with
“hydro-”!
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Anion Ending Acid Name
-ide hydro-(stem)-ic acid
-ate (stem)-ic acid
-ite (stem)-ous acid
Acid Nomenclature
Binary Binary
Ternary Ternary
To remember which goes with which…To remember which goes with which…
““In the cafeteria, you ATE something ICky”In the cafeteria, you ATE something ICky”
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Salt
Hydrogen + polyatomic ion
hydrogen per_____ate
hydrogen _____ate
hydrogen _____ite
hydrogen hypo_____ite
hydrogen _____ide
Aqueous Acid hydrogen polyatomic ion
per_____ic acid
_____ic acid
_____ous acid
hypo______ous acid
hydro______ic acid
To transform the hydrogen _____ide salt into its corresponding aqueous acid name: 1) The name hydrogen is replaced with the prefix hydro- 2) The -ide ending is replaced with ____ic 3) The word acid is added to the name
For example: hydrogen bromide > hydrobromic acid HBr(s) > HBr(aq)
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To transform the hydrogen _____ate salt into its corresponding aqueous acid name:
1) The name hydrogen is dropped 2) The -ate ending is replaced with –ic3) The word acid is added to the name
For example: hydrogen acetate > acetic acid HC2H3O2(s) > HC2H3O2(aq)
SaltHydrogen + polyatomic ion
hydrogen per_____ate
hydrogen _____ate
hydrogen _____ite
hydrogen hypo_____ite
hydrogen _____ide
Aqueous Acid hydrogen + polyatomic ion
per_____ic acid
_____ic acid
_____ous acid
hypo______ous acid
hydro______ic acid
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To transform the hydrogen per____ate salt into its corresponding aqueous acid name:
1) The name hydrogen is dropped 2) The -ate ending is replaced with –ic3) The word acid is added to the name
For example: hydrogen perchlorate > perchloric acid HClO4(s) > HClO4 (aq)
Aqueous Acid hydrogen polyatomic ion
per_____ic acid
_____ic acid
_____ous acid
hypo______ous acid
hydro______ic acid
Salt
Hydrogen + polyatomic ion
hydrogen per_____ate
hydrogen _____ate
hydrogen _____ite
hydrogen hypo_____ite
hydrogen _____ide
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Salt
Hydrogen + polyatomic ion
hydrogen per_____ate
hydrogen _____ate
hydrogen _____ite
hydrogen hypo_____ite
hydrogen _____ide
Aqueous Acid hydrogen polyatomic ion
per_____ic acid
_____ic acid
_____ous acid
hypo______ous acid
hydro______ic acid
To transform the hydrogen _____ite salt into its corresponding aqueous acid name:
1) The name hydrogen is dropped 2) The -ite ending is replaced with –ous3) The word acid is added to the name
For example:hydrogen nitrite > nitrous acidHNO2(s) > HNO2(aq)
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Salt
Hydrogen + polyatomic ion
hydrogen per_____ate
hydrogen _____ate
hydrogen _____ite
hydrogen hypo_____ite
hydrogen _____ide
Aqueous Acid hydrogen polyatomic ion
per_____ic acid
_____ic acid
_____ous acid
hypo______ous acid
hydro______ic acid
To transform the hydrogen hypo_____ite salt into its corresponding aqueous acid name:
1) The name hydrogen is dropped 2) The -ite ending is replaced with –ous3) The word acid is added to the name
For example: hydrogen hypoiodite > hypoiodous acid HIO (s) > HIO (aq)
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Examples #1- Formulas to Names
2. Determine the ion and it’s acid ending.
1. The hydrogen out front & the (aq) subscript indicates an acid
Final Name
HBrO2(aq)
bromous acid
bromite
____________ acid
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Practice Problem #1HIO4(aq)
Choose the correct name for the compound
1. iodoic acid
2. iodous acid
3. periodoic acid
4. hydrogen periodate
5. none of the abovenext
problemIon list
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Writing Acid Formulas
• Hydrogen will always be first• The name will tell you the anion
• If it starts with hydro- it’s binary -• H + a non-metal, • If it doesn’t start with hydro-, it’s
ternary – H + a polyatomic ion.• Remember: -ate comes from -ic, -ite
comes from –ous• Balance charges.
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Example #1-Names to Formulas
HClO3
2. Add hydrogen ions
1. Determine the formula & charge of the polyatomic ion
Final Formula
chloric acid
(aq)
chlorate
-1+1
3. Balance charge with ions
4. Add the subscript: (aq)
=0
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• hydrofluoric acidhydrofluoric acid
• sulfuric acidsulfuric acid
• nitrous acidnitrous acid
– 2 elements2 elements
– 3 elements, 3 elements, -ic-ic
– 3 elements, 3 elements, -ous-ous
HF HF (aq)(aq)
HH22SOSO44
HNOHNO22
Acid Nomenclature
HH++ F- F-
HH++ SO SO442-2-
HH++ NO NO22--
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• HBr HBr (aq)(aq)
• HH22COCO33
• HH22SOSO33
– 2 elements, 2 elements, --ideide
– 3 elements, 3 elements, -ate-ate
– 3 elements, 3 elements, -ite-ite
hydrohydrobromic bromic
acidacid
carboncarbonicic
acidacid
sulfursulfurousous
acidacid
Acid Nomenclature
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Practice Problemhydrobromic acid
Choose the correct formula for the compound
1. HBrO(aq)
2. HBr(aq)
3. HBrO3(aq)
4. HBrO2(aq)
5. none of the above
next problem
Ion list
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Acid Nomenclature Flowchart
h yd ro - p re fix-ic en d in g
2 e lem en ts
-a te en d in gb ecom es-ic en d in g
-ite en d in gb ecom es
-o u s en d in g
n o h yd ro - p re fix
3 e lem en ts
AC ID Ss ta rt w ith 'H '
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A flow chart for naming binary compounds.
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Mixed Review
Name the following compounds:
1. CaOa) calcium oxide b) calcium(I) oxidec) calcium (II) oxide
2. SnCl4
a) tin tetrachloride b) tin(II) chloride
c) tin(IV) chloride
3. N2O3
a) nitrogen oxide b) dinitrogen trioxidec) nitrogen trioxide
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Solution
Name the following compounds:
1. CaO
2. SnCl4
3. N2O3
a) calcium oxide
c) tin(IV) chloride
b) Dinitrogen trioxide
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Mixed Practice
1. Dinitrogen monoxide
2. Potassium sulfide
3. Copper (II) nitrate
4. Dichlorine heptoxide
5. Chromium (III) sulfate
6. Iron (III) sulfite
7. Calcium oxide
8. Barium carbonate
9. Iodine monochloride
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Mixed Practice
1.1. BaIBaI22
2.2. PP44SS33
3.3. Ca(OH)Ca(OH)22
4.4. FeCOFeCO33
5.5. NaNa22CrCr22OO77
6.6. II22OO55
7.7. Cu(ClOCu(ClO44))22
8.8. CSCS22
9.9. BB22ClCl44
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Name ‘Em!
• HI HI (aq)(aq)
• HClHCl
• HH22SOSO33
• HNOHNO33
• HIOHIO44
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Write the Formula!
• Hydrobromic acidHydrobromic acid
• Nitrous acidNitrous acid
• Carbonic acidCarbonic acid
• Phosphoric acidPhosphoric acid
• Hydrotelluric acidHydrotelluric acid
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Naming Ternary Compounds from Oxyacids
The following table lists the most common families of oxy acids.
one moreoxygen atom
most“common”
one lessoxygen
two lessoxygen
HClO4
perchloric acid
HClO3
chloric acid
HClO2
chlorous acid
HClOhypochlorous acid
H2SO4
sulfuric acid
H2SO3
sulfurous acid
H3PO4
phosphoric acid
H3PO3
phosphorous acid
H3PO2
hypophosphorous acid
HNO3
nitric acid
HNO2
nitrous acid
(HNO)2
hyponitrous acid
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Naming Simple Chemical Compounds
Ionic (metal and nonmetal) Covalent (2 nonmetals)
Metal
Formsonly onepositive
ion
Formsmore than
one positiveion
Nonmetal
Use the name of element
Use elementname followed
by a Romannumeral to
show the charge
Firstnonmetal
Secondnonmetal
Beforeelement name
use a prefixto matchsubscript
Use a prefixbefore
element name and end with ide
SingleNegative
Ion
Polyatomic Ion
Use the nameof the
element, butend with ide
Use thename of
polyatomicion (ate or
Ite)
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NomenclaturePOPO44
3-3-
phosphate ionphosphate ion
CC22HH33OO22--
acetate ionacetate ion
HC2H3O2
Acetic Acid
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Two nonmetals Multiple-charge cation Everything else
Romannumeral
Polyatomic ions OK
Roman numeralfor name only
Polyatomic ions
Greek prefixes
Charge
Criss-CrossRule
Romannumeral
OK
Where would you file this?
VCrO4
BaO
CBr4
Nb(ClO4)5
SCl2Rb2SO4
dinitrogen pentoxide
platinum (IV) iodate
ammonium chlorate
potassium iodide
nitrogen trichloride
manganese (V) sulfide
vanadium (II) chromate
VCrO4
N2O5
dinitrogen pentoxide
barium oxide
BaO
Pt(IO3)4
platinum (IV) iodate
carbon tetrabromide
CBr4
NH4ClO3
ammonium chlorate
niobium (V) perchlorate
Nb(ClO4)5
KI
potassium iodide
sulfur dichloride
SCl2
NCl3
nitrogen trichloride
rubidium sulfate
Rb2SO4
Mn2S5
manganese (V) sulfide
PRACTICE
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Learning Check
Complete the names of the following binary compounds:
Na3N sodium ________________
KBr potassium ________________
Al2O3 aluminum ________________
MgS _________________________
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- calcium hydroxide
- copper(II) sulfate
- ammonium nitrate
- cobalt(III) carbonate
Ca(OH)2
CuSO4
NH4NO3
Co2(CO3)3
Compounds containing polyatomic ions