starter s-73

Starter S-73

Give the scientific name for three chemical compounds.

Chemical Names and Formulas

Chapter 9

9.1 Naming Ions

Chapter 9

Monatomic Ions – only one atom

Review

Cations (metals) form positive charges

9.1 Naming Ions


Review

Group 1: +1

9.1 Naming Ions


Review

Group 2: +2

9.1 Naming Ions

8.1 Molecular Compounds

Some metals have more than one charge (oxidation number)

They are named using the name and the charge

9.1 Naming Ions

Symbol Name Classical Name

Cu+ Copper (I) Cuprous

Cu2+ Copper (II) Cupric

Fe2+ Iron (II) Ferrous

Fe3+ Iron (III) Ferric

Pb2+ Lead (II) Plumbous

Pb4+ Lead (IV) Plumbic


Review

Anions – negative ions

9.1 Naming Ions


Review

Group 17: -1

9.1 Naming Ions


Review

Group 16: -2

9.1 Naming Ions


Review

Group 15: -3

9.1 Naming Ions

Polyatomic Ions – a charged group of atoms bonded covalently

Examples – Ammonium

9.1 Naming Ions


Examples – Hydrogen Sulfate

9.1 Naming Ions


Examples – Carbonate

9.1 Naming Ions

See page 257 for a list of polyatomic ions.

There will be a quiz.

9.1 Naming Ions

9.2 Naming & Writing Formulas: Ionic

Chapter 9

Binary Compounds – composed of two elements and can be ionic or covalently bonded

For Ionic names

1. Write the name of the cation first

2. Write the name of the anion

3. Change the ending of the anion to -ide


NaBrSodium BrSodium BromineSodium Bromide

If the compound has a metal with more than one charge, we must calculate the charge

Write out the formula and the charge of the anion

Calculate the total negative charge

This is the total charge on the cation, so divide the charge by the number of atoms

PbCl4PbCl4

-1

414 x 414


Name the cation

Name the anion

Change the ending to -idePbCl4

414


Lead (IV) Cl4Lead (IV) ChlorineLead (IV) Chloride

Example 1:

Example 2:

Example 3:

Example 4:

Na2S


Sodium SSodium SulfurSodium Sulfide

CuOCopper (II) OCopper (II) OxygenCopper (II) Oxide

ZnI2Zinc I2Zinc IodineZinc Iodide

Fe2S3Iron (III) S3Iron (III) SulfurIron (III) Sulfide

Starter S-74

Write the names of the following ionic compounds

A. FeCl2B. V3N4

C. K2O

D. Cu2S

E. AgF

To write the formula from the name

1. Write the ions

2. Cross the values of the charges

3. Confirm it is the smallest ratio


Nickel (III) FluorideNi+3 F-NiF3

Example 1:

Example 2:

Example 3:

Example 4:


Calcium Bromide Ca+2 Br- CaBr2

Lead (IV) Oxide Pb+4 O-2 Pb2O4 PbO2

Magnesium Sulfide Mg+2 S-2 Mg2S2 MgS

Vanadium (V) OxideV+5 O-2V2O5

Polyatomic Ions – Use the same rules as other ionic compounds

The endings do not change

So to write the formula for

1. Write the formula and charge for Ammonium

2. Write the formula and charge for Carbonate


Ammonium CarbonateNH4+1 CarbonateNH4

+1 CO3-2

Polyatomic Ions – Use the same rules as other ionic compounds

The endings do not change

So to write the formula for

3. Criss Cross

4. If the polyatomic ion has a subscript, parenthesis are placed around the polyatomic ion


Ammonium CarbonateNH4+1 CarbonateNH4

+1 CO3-2NH42CO3(NH4)2CO3

Example 1

Example 2

Example 3

Example 4


Sodium PhosphateNa+ PO4-3Na3PO4

Iron (III) Dihydrogen PhosphateFe+3 H2PO4-Fe(H2PO4)3

Ammonium OxideNH4+ O-2(NH4)2O

Copper (II) PerchlorateCu+2 ClO4-Cu(ClO4)2

So to write the name for

1. Name the first ion (check charges if it needs a roman numeral)

2. Name the second ion


Ag2SO4Silver SO4Silver Sulfate

Pb(NO3)4Lead (IV) (NO3)4Lead (IV) Nitrate

Example 1

Example 2

Example 3

Example 4


(NH4)2Cr2O7Ammonium Dichromate

Ni2(C2O4)3Nickel (III) Oxalate

CaSiO3Calcium Silicate

CoHPO4Cobalt (II) Hydrogen Phosphate

Starter S-76

Give the names for the following

A. Pt(NO2)2

B. Mg(ClO)2

Give the formula for the following

A. Cesium Carbonate

B. Copper (I) Suflite

Starter S-77

Name

A. Pb(ClO4)4

B. Pb(NO3)2

Give the Formula

A. Iron (III) Silicate

B. Nickel (II) Fluoride

9.3 Naming & Writing Molecular Compounds

Chapter 9


Molecular Compounds (two non-metals)

Prefixes are used to name the subscript in the molecular formula

So to name

1. Never use mono on the first element

2. Prefix and element

Prefix Number

Mono 1

Di 2

Tri 3

Tetra 4

Penta 5

Hexa 6

Hepta 7

Octa 8

Nona 9

Deca 10

SiO2Silicon O2Silicon Dioxide


Example 1

Example 2

Example 3

Example 4

NCl3Nitrogen Trichloride

N2H4Dinitrogen Tetrahydride

Cl2O7Dichlorine Heptaoxide

P4S3TetraPhosphorus Trisulfide


Writing formulas invloves just writing the symbols and the prefixes

1. Write the first element with the proper subscript

2. Second element and subscript

Prefix Number

Mono 1

Di 2

Tri 3

Tetra 4

Penta 5

Hexa 6

Hepta 7

Octa 8

Nona 9

Deca 10

Carbon TetrabromideC TetrabromideCBr4


Example 1

Example 2

Example 3

Example 4

Diphosphorus TrioxideP2O3

Iodine HeptafluorideIF7

Nitrogen MonoxideNO

Tetraphosphorus HexoxideP4O6

9.4 Naming & Writing Acids

Chapter 9

9.4 Naming & Writing Formulas for Acids

Acid – a compound that has one or more hydrogen atoms and produces hydrogen ions (H+) in solution

The basic formula is

Three rules for naming

1. When the anion (X) does not have Oxygen in it

a. The name begins with hydro

b. The anion’s name ends in –ic

c. And the word acid is added to the end

HnX

HClHydro ClHydrochloricHydrochloric Acid

Starter S-78

Name

A. N2O3

B. SO3

C. HF

Give the Formula

A. Dihydrogen monoxide

B. Carbon Monoxide


2. When the anion (X) does have Oxygen and the polyatomic ion ends in -ite

a. Use the name of the anion, but change the ending to –ous

b. Add the word acid

H2SO3SulfurousSulfurous Acid


3. When the anion (X) does have Oxygen and the polyatomic ion ends in -ate

a. Use the name of the anion, but change the ending to –ic

b. Add the word acid

H2SO4SulfuricSulfuric Acid

Oxygen?NO YES

--ous acid

Ending of Polyatomic Ion?

-ite -ateHydro—ic acid

--ic acid


Example 1

Example 2

Example 3

Example 4

HClO3Chloric Acid

HCNHydrocyanic Acid

HNO3Nitric Acid

HClO2Chlorous Acid


To write the formulas, we go backwards through our list

Acids always have an H+ ion

Hydro means no Oxygen – so Fluoric means Fluoride

Hydrofluoric Acid

Oxygen?NO YES

--ous acid



--ic acid

H+ Hydrofluoric AcidH+ F-HF




ous means the ion ended in ite, so phosphite

Phosphorous Acid

Oxygen?NO YES

--ous acid



--ic acid

H+ Phosphorous AcidH+ PO3-3H3PO3




ic means the ion ended in ate, so phosphate

Phosphoric Acid

Oxygen?NO YES

--ous acid



--ic acid

H+ Phosphoric Acid


Example 1

Example 2

Example 3

Example 4

Hydroiodic AcidHI

Acetic AcidHC2H3O2

Hypochlorous AcidHClO

Carbonic AcidH2CO3

9.5 The Laws Governing Formulas and Names

Chapter 9


The Law of Definite Proportions – in any chemical compound, the masses of the elements are always in the same proportion

The ratio of this molecule is always

Or (Same Ratio)

Carbon:Hydrogen2.98:1:001:00:0.34


The Law of Multiple Proportions – Whenever the same two elements form multiple compounds, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers

Huh?

For example one compound

A second compound might be

The ratio of the two masses would be

5 :10gA gA5g A2g B

10g A2g B1: 2

starter s-73

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