NomenclatureChapter 9

Do Now #1Which statement is true?A. Elements in the same group has the same #

of val. e-B. Elements in the same period has the same #

of val. e-

Write the formula for each of the following compounds.1. Ammonium sulfate2. Vanadium (V) fluoride3. Copper (III) nitrate4. Aluminum oxide

Answers:5. (NH4)2SO4

6. VF5

7. Cu(NO3)3

8. Al2O3

Do Now #2

Do Now #3

What is the difference between CuSO4 and CuNO3?

Answer:Contain different polyatomic anion CuSO4: copper 2+

CuNO3: copper 1+

Name the following compounds:1. CO2. SiO2

3. P4O6

Write the formula for the below compounds:4. Arsenic tribromide

Answer:5. Carbon monoxide6. Silicon dioxide7. Tetraphosphorus hexoxide

Answer: AsBr3

Do Now #4

Types of Chemical BondsIonic Compounds: Formed by the opposite attraction between

cations & anions. (btwn metals & non-metals)

Salt - scientific name given to many different ionic compounds

75102.swf

Transfer of electrons creates ions

Formation of Sodium Chloride

+1 +

2+3

+/-4 -3 -2 -1

0

Hydrogen can be 1+ or 1-, most common is 1+

CATIONS (alkalai = +1, alkaline earth = +2, aluminum = +3, zinc = +2, silver = +1)

sodium ion _______

beryllium ion _______

aluminum ion _____

strontium ion ______

cesium ion _________

silver ion _____

Na 1+

Be 2+

Al 3+

Sr2+

Cs+

Ag+

TRANSITION/POST TRANSITION METALS (variable)

copper (I) ion _____

copper (II) ion _____

cobalt (II) ion ______

manganese (VII) ion ______

iron (II) ion ______

iron (III) ion _____

Cu+

Cu2

+

Co2

+

Mn7+

Fe3+

Fe2+

ANIONS (monoatomic anions all end in –ide)

nitride ______

fluoride _______

oxide ______

chloride _____

iodide _______

phosphide ______

N3-

F1-

O2-

Cl1

-

I1-

P3-

BINARY IONIC COMPOUNDS (Salts)

Naming rule:Metal name______________ ide

(root of non-metal)

Ex: AlCl3 = Aluminum Chloride

a. Li2O

b. MgF2

c. Ca3P2

d. SrI2

Lithium Oxide

Magnesium Fluoride

Calcium Phosphide

Strontium Iodide

Formula writing

Al +3 Cl -1

Al1Cl3 = AlCl3

Sodium chlorideCalcium chloride

Ionic Compound subscripts must be reducedTi+4O-2 Sn+2O-2 Ti2O4 reduces to TiO2 Sn2O2 reduces to

SnO

NaCl

CaCl2

Write the FORMULA for:

a. lithium fluoride b. calcium bromide

LiF CaBr2

c. magnesium phosphide d. barium oxide

Mg3P2 BaO

e. iron(III) chloride f. lead (II) nitrideFeCl3 Pb3N2

g. potassium nitride h. tin(IV) oxideK3N SnO2

Ions made up of 2 or more atomsCharge is spread across the group of bonded

atoms

Polyatomic ion

You do not need to memorize them. They will be given to you during the test

Write the FORMULA for:

a. lithium sulfate b. calcium hydroxide  Li2SO4 Ca(OH)2

  c. copper(II) cyanide d. strontium nitrate

Cu(CN)2 Sr(NO3)2

  e. chromium(III) phosphate f. manganese (IV) carbonate

CrPO4 Mn(CO3)2

  g. barium chlorate h. aluminum permanganate

Ba(ClO3)2 Al(MnO4)3

NAME the following compounds:a. NH4Cl b. Ca(CN)2

Ammonium Chloride Calcium Cyanide  c. Na3PO4 d. Al(OH)3

Sodium Phosphate Aluminum Hydroxide  e. ZnSO4 f. Cs2CO3

Zinc Sulfate Cesium Carbonate

  

g. KClO3 h. Mg3(PO4)2

Potassium Chlorate Magnesium Phosphate

TRANSITION/POST TRANSITION METALS (charge varies)

WHAT ABOUT THE METALS THAT HAVE MORE THAN ONE OXIDATION # (CHARGE)?

a. Write in the charges for the ions you are sure of (anion)b. Work backwards to find the charge of the metal ion (cation)Which metals DO NOT need Roman Numerals?

Column I (alkali) Column II (alkaline earth)   Silver (always +1): Ag+

 Zinc (always +2): Zn2+

 Aluminum (always +3): Al3+

NAME the following compounds(Roman numerals shows the charge of the metal)

a. CuS b. FeP copper (II) sulfide iron (III) phosphide

c. FeSO4 d. CuNO3

 iron (II) sulfate copper (I) nitrate

e. NiI3 f. Cr(MnO4)4

nickel (III) iodide chromium (IV) permanganate g. Pb(NO3)2 h. Pb(SO4)2

lead (II) nitrate lead (IV) sulfate i. Sn(CO3)2 j Sn(NO3)2

tin (IV) carbonate tin (II) nitrate 

k. Cu3(PO4)2 l. Cu3PO4

copper (II) phosphate copper (I) phosphate

Covalent CompoundsFormed when atoms share one or more pairs of electronsBonds between nonmetals

Prefix # of Atoms Prefix # of Atomsmono- 1 hexa- 6di- 2 hepta- 7tri- 3 octa- 8

tetra- 4 nona- 9penta- 5 deca- 10

Examples:SO2 → Sulfur dioxide

SO3 → Sulfur trioxide

NO → Nitrogen monoxide NOT Mononitrogen monooxideN2O5 → Dinitrogen pentoxide NOT dinitrogen pentaoxide

Some compounds are always referred to by their common namesH2O Water

NH3 Ammonia

CH4 Methane

C3Cl6

Si2O7

C5F10

PCl5

Prefix # of Atoms Prefix # of Atomsmono- 1 hexa- 6di- 2 hepta- 7tri- 3 octa- 8

tetra- 4 nona- 9penta- 5 deca- 10

tricarbon hexachloride

Disilicon heptoxide

pentacarbon decafluoride

phosphorous pentachloride

Writing the formula of molecular/covalent compounds:

a) dinitrogen pentaoxide

b) Boron triflouridec) Carbon monoxided) Carbon tetrachloridee) dinitrogen monoxidef) nitrogen dioxideg) dichlorine monoxideh) carbon tetrafluoridei) tetracarbon

octabromide

N2O5

BF3

COCCl4

N2ONO2

Cl2OCF4

C4Br8

BINARY: Contains exactly two elements. (without oxygen)

1. prefix hydro- to name the hydrogen part of the acid

2. add the suffix –ic EXAMPLES:

HCl HBrhydrochloric acid hydrobromic acid

Naming Acids (hint: acids start with “H”)

Naming Acids CONT…

Oxyacids: (contain oxygen) (H & polyatomic ion with O)

1. use the root of the anion2. if it is an –ate anion, use the –ic ending3. if it is an –ite anion, use the –ous ending

H2SO4 HNO3

sulfuric acid nitric acidH2SO3 HNO2

sulfurous acid nitrous acid

FORMULA ANION NAME

H2CO3

HC2H3O2

H2SO3

H3P

H2S

Carbonate Carbonic acid

Acetate Acetic acid

Sulfite Sulfurous acid

Phosphide Hydrophosphoric acid

Sulfide Hydrosulfuric acid

FORMULA ANION NAMEhydronitric acid

nitrous acid

permanganic acid

sulfuric acid

hydrofluoric acid

phosphoric acid

hydrophosphoric acid

H3N N3-

HNO2 NO2-1

HMnO4 MnO4-1

SO4-2H2SO4

HF F1-

PO4-3

P3-

H3PO4

H3P