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Starter S-73. Give the scientific name for three chemical compounds. Chemical Names and Formulas. Chapter 9. 9.1 Naming Ions. Chapter 9. 9.1 Naming Ions. Monatomic Ions – only one atom Review Cations (metals) form positive charges. 9.1 Naming Ions. Monatomic Ions – only one atom Review

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starter s 73
Starter S-73

Give the scientific name for three chemical compounds.

9 1 naming ions1
9.1 Naming Ions

Monatomic Ions – only one atom

Review

Cations (metals) form positive charges

9 1 naming ions2
9.1 Naming Ions

Monatomic Ions – only one atom

Review

Group 1: +1

9 1 naming ions3
9.1 Naming Ions

Monatomic Ions – only one atom

Review

Group 2: +2

8 1 molecular compounds
8.1 Molecular Compounds

9.1 Naming Ions

Some metals have more than one charge (oxidation number)

They are named using the name and the charge

9 1 naming ions4
9.1 Naming Ions

Monatomic Ions – only one atom

Review

Anions – negative ions

9 1 naming ions5
9.1 Naming Ions

Monatomic Ions – only one atom

Review

Group 17: -1

9 1 naming ions6
9.1 Naming Ions

Monatomic Ions – only one atom

Review

Group 16: -2

9 1 naming ions7
9.1 Naming Ions

Monatomic Ions – only one atom

Review

Group 15: -3

9 1 naming ions8
9.1 Naming Ions

Polyatomic Ions – a charged group of atoms bonded covalently

Examples – Ammonium

9 1 naming ions9
9.1 Naming Ions

Polyatomic Ions – a charged group of atoms bonded covalently

Examples – Hydrogen Sulfate

9 1 naming ions10
9.1 Naming Ions

Polyatomic Ions – a charged group of atoms bonded covalently

Examples – Carbonate

9 1 naming ions11
9.1 Naming Ions

See page 257 for a list of polyatomic ions.

There will be a quiz.

9 2 naming writing formulas ionic1
9.2 Naming & Writing Formulas: Ionic

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

For Ionic names

  • Write the name of the cation first
  • Write the name of the anion
  • Change the ending of the anion to -ide

NaBr

Sodium Br

Sodium Bromine

Sodium Bromide

9 2 naming writing formulas ionic2
9.2 Naming & Writing Formulas: Ionic

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

PbCl4-1

PbCl4

9 2 naming writing formulas ionic3
9.2 Naming & Writing Formulas: Ionic

Name the cation

Name the anion

Change the ending to -ide

PbCl4

Lead (IV) Cl4

Lead (IV) Chlorine

Lead (IV) Chloride

9 2 naming writing formulas ionic4
9.2 Naming & Writing Formulas: Ionic

Example 1:

Example 2:

Example 3:

Example 4:

Na2S

Sodium S

Sodium Sulfur

Sodium Sulfide

Copper (II) O

CuO

Copper (II) Oxide

Copper (II) Oxygen

ZnI2

Zinc I2

Zinc Iodine

Zinc Iodide

Iron (III) Sulfide

Iron (III) Sulfur

Iron (III) S3

Fe2S3

starter s 74
Starter S-74

Write the names of the following ionic compounds

  • FeCl2
  • V3N4
  • K2O
  • Cu2S
  • AgF
9 2 naming writing formulas ionic5
9.2 Naming & Writing Formulas: Ionic

To write the formula from the name

  • Write the ions
  • Cross the values of the charges
  • Confirm it is the smallest ratio

Nickel (III) Fluoride

Ni+3 F-

NiF3

9 2 naming writing formulas ionic6
9.2 Naming & Writing Formulas: Ionic

Example 1:

Example 2:

Example 3:

Example 4:

Calcium Bromide

Ca+2 Br-

CaBr2

Pb+4 O-2

Pb2O4

PbO2

Lead (IV) Oxide

Magnesium Sulfide

Mg+2 S-2

Mg2S2

MgS

Vanadium (V) Oxide

V+5 O-2

V2O5

9 2 naming writing formulas ionic7
9.2 Naming & Writing Formulas: Ionic

Polyatomic Ions – Use the same rules as other ionic compounds

The endings do not change

So to write the formula for

  • Write the formula and charge for Ammonium
  • Write the formula and charge for Carbonate

NH4+1 Carbonate

NH4+1 CO3-2

Ammonium Carbonate

9 2 naming writing formulas ionic8
9.2 Naming & Writing Formulas: Ionic

Polyatomic Ions – Use the same rules as other ionic compounds

The endings do not change

So to write the formula for

  • Criss Cross
  • If the polyatomic ion has a subscript, parenthesis are placed around the polyatomic ion

NH4+1 Carbonate

NH4+1 CO3-2

NH42CO3

(NH4)2CO3

Ammonium Carbonate

9 2 naming writing formulas ionic9
9.2 Naming & Writing Formulas: Ionic

Example 1

Example 2

Example 3

Example 4

Sodium Phosphate

Na+ PO4-3

Na3PO4

Fe(H2PO4)3

Iron (III) Dihydrogen Phosphate

Fe+3 H2PO4-

(NH4)2O

Ammonium Oxide

NH4+ O-2

Cu(ClO4)2

Copper (II) Perchlorate

Cu+2 ClO4-

9 2 naming writing formulas ionic10
9.2 Naming & Writing Formulas: Ionic

So to write the name for

  • Name the first ion (check charges if it needs a roman numeral)
  • Name the second ion

Ag2SO4

Silver SO4

Silver Sulfate

Lead (IV) (NO3)4

Lead (IV) Nitrate

Pb(NO3)4

9 2 naming writing formulas ionic11
9.2 Naming & Writing Formulas: Ionic

Example 1

Example 2

Example 3

Example 4

Ammonium Dichromate

(NH4)2Cr2O7

Ni2(C2O4)3

Nickel (III) Oxalate

CaSiO3

Calcium Silicate

Cobalt (II) Hydrogen Phosphate

CoHPO4

starter s 76
Starter S-76

Give the names for the following

  • Pt(NO2)2
  • Mg(ClO)2

Give the formula for the following

  • Cesium Carbonate
  • Copper (I) Suflite
starter s 77
Starter S-77

Name

  • Pb(ClO4)4
  • Pb(NO3)2

Give the Formula

  • Iron (III) Silicate
  • Nickel (II) Fluoride
9 3 naming writing molecular compounds1
9.3 Naming & Writing Molecular Compounds

Molecular Compounds (two non-metals)

Prefixes are used to name the subscript in the molecular formula

So to name

  • Never use mono on the first element
  • Prefix and element

SiO2

Silicon O2

Silicon Dioxide

9 3 naming writing molecular compounds2
9.3 Naming & Writing Molecular Compounds

Example 1

Example 2

Example 3

Example 4

Nitrogen Trichloride

NCl3

Dinitrogen Tetrahydride

N2H4

Cl2O7

Dichlorine Heptaoxide

TetraPhosphorus Trisulfide

P4S3

9 3 naming writing molecular compounds3
9.3 Naming & Writing Molecular Compounds

Writing formulas invloves just writing the symbols and the prefixes

  • Write the first element with the proper subscript
  • Second element and subscript

Carbon Tetrabromide

C Tetrabromide

CBr4

9 3 naming writing molecular compounds4
9.3 Naming & Writing Molecular Compounds

Example 1

Example 2

Example 3

Example 4

P2O3

Diphosphorus Trioxide

IF7

Iodine Heptafluoride

NO

Nitrogen Monoxide

P4O6

Tetraphosphorus Hexoxide

9 4 naming writing formulas for acids
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

  • 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

Hydro Cl

Hydrochloric

Hydrochloric Acid

HCl

starter s 78
Starter S-78

Name

  • N2O3
  • SO3
  • HF

Give the Formula

  • Dihydrogen monoxide
  • Carbon Monoxide
9 4 naming writing formulas for acids1
9.4 Naming & Writing Formulas for Acids

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

Sulfurous

Sulfurous Acid

H2SO3

9 4 naming writing formulas for acids2

Oxygen?

NO

YES

Hydro—ic acid

Ending of

Polyatomic Ion?

-ate

-ite

--ous acid

--ic acid

9.4 Naming & Writing Formulas for Acids

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

H2SO4

Sulfuric

Sulfuric Acid

9 3 naming writing molecular compounds5
9.3 Naming & Writing Molecular Compounds

Example 1

Example 2

Example 3

Example 4

Chloric Acid

HClO3

Hydrocyanic Acid

HCN

Nitric Acid

HNO3

Chlorous Acid

HClO2

9 4 naming writing formulas for acids3

Oxygen?

NO

YES

Hydro—ic acid

Ending of

Polyatomic Ion?

-ate

-ite

--ous acid

--ic acid

9.4 Naming & Writing Formulas for Acids

To write the formulas, we go backwards through our list

Acids always have an H+ ion

Hydro means no Oxygen – so Fluoric means Fluoride

H+ Hydrofluoric Acid

H+ F-

HF

Hydrofluoric Acid

9 4 naming writing formulas for acids4

Oxygen?

NO

YES

Hydro—ic acid

Ending of

Polyatomic Ion?

-ate

-ite

--ous acid

--ic acid

9.4 Naming & Writing Formulas for Acids

To write the formulas, we go backwards through our list

Acids always have an H+ ion

ous means the ion ended in ite, so phosphite

H+ Phosphorous Acid

Phosphorous Acid

H+ PO3-3

H3PO3

9 4 naming writing formulas for acids5

Oxygen?

NO

YES

Hydro—ic acid

Ending of

Polyatomic Ion?

-ate

-ite

--ous acid

--ic acid

9.4 Naming & Writing Formulas for Acids

To write the formulas, we go backwards through our list

Acids always have an H+ ion

ic means the ion ended in ate, so phosphate

H+ Phosphoric Acid

Phosphoric Acid

9 3 naming writing molecular compounds6
9.3 Naming & Writing Molecular Compounds

Example 1

Example 2

Example 3

Example 4

HI

Hydroiodic Acid

HC2H3O2

Acetic Acid

Hypochlorous Acid

HClO

Carbonic Acid

H2CO3

9 5 the laws governing formulas and names1
9.5 The Laws Governing Formulas and Names

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:Hydrogen

2.98:1:00

1:00:0.34

9 5 the laws governing formulas and names2
9.5 The Laws Governing Formulas and Names

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

5g A

10g A

2g B

2g B