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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
Monatomic Ions – only one atom
Review
Cations (metals) form positive charges
9.1 Naming Ions
Monatomic Ions – only one atom
Review
Group 1: +1
9.1 Naming Ions
Monatomic Ions – only one atom
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
Monatomic Ions – only one atom
Review
Anions – negative ions
9.1 Naming Ions
Monatomic Ions – only one atom
Review
Group 17: -1
9.1 Naming Ions
Monatomic Ions – only one atom
Review
Group 16: -2
9.1 Naming Ions
Monatomic Ions – only one atom
Review
Group 15: -3
9.1 Naming Ions
Polyatomic Ions – a charged group of atoms bonded covalently
Examples – Ammonium
9.1 Naming Ions
Polyatomic Ions – a charged group of atoms bonded covalently
Examples – Hydrogen Sulfate
9.1 Naming Ions
Polyatomic Ions – a charged group of atoms bonded covalently
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
9.2 Naming & Writing Formulas: Ionic
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
9.2 Naming & Writing Formulas: Ionic
Name the cation
Name the anion
Change the ending to -idePbCl4
414
9.2 Naming & Writing Formulas: Ionic
Lead (IV) Cl4Lead (IV) ChlorineLead (IV) Chloride
Example 1:
Example 2:
Example 3:
Example 4:
Na2S
9.2 Naming & Writing Formulas: Ionic
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
9.2 Naming & Writing Formulas: Ionic
Nickel (III) FluorideNi+3 F-NiF3
Example 1:
Example 2:
Example 3:
Example 4:
9.2 Naming & Writing Formulas: Ionic
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
9.2 Naming & Writing Formulas: Ionic
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
9.2 Naming & Writing Formulas: Ionic
Ammonium CarbonateNH4+1 CarbonateNH4
+1 CO3-2NH42CO3(NH4)2CO3
Example 1
Example 2
Example 3
Example 4
9.2 Naming & Writing Formulas: Ionic
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
9.2 Naming & Writing Formulas: Ionic
Ag2SO4Silver SO4Silver Sulfate
Pb(NO3)4Lead (IV) (NO3)4Lead (IV) Nitrate
Example 1
Example 2
Example 3
Example 4
9.2 Naming & Writing Formulas: Ionic
(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
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
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
9.3 Naming & Writing Molecular Compounds
Example 1
Example 2
Example 3
Example 4
NCl3Nitrogen Trichloride
N2H4Dinitrogen Tetrahydride
Cl2O7Dichlorine Heptaoxide
P4S3TetraPhosphorus Trisulfide
9.3 Naming & Writing Molecular Compounds
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
9.3 Naming & Writing Molecular Compounds
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
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
H2SO3SulfurousSulfurous 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
H2SO4SulfuricSulfuric Acid
Oxygen?NO YES
--ous acid
Ending of Polyatomic Ion?
-ite -ateHydro—ic acid
--ic acid
9.3 Naming & Writing Molecular Compounds
Example 1
Example 2
Example 3
Example 4
HClO3Chloric Acid
HCNHydrocyanic Acid
HNO3Nitric Acid
HClO2Chlorous 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
Hydrofluoric Acid
Oxygen?NO YES
--ous acid
Ending of Polyatomic Ion?
-ite -ateHydro—ic acid
--ic acid
H+ Hydrofluoric AcidH+ F-HF
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
Phosphorous Acid
Oxygen?NO YES
--ous acid
Ending of Polyatomic Ion?
-ite -ateHydro—ic acid
--ic acid
H+ Phosphorous AcidH+ PO3-3H3PO3
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
Phosphoric Acid
Oxygen?NO YES
--ous acid
Ending of Polyatomic Ion?
-ite -ateHydro—ic acid
--ic acid
H+ Phosphoric Acid
9.3 Naming & Writing Molecular Compounds
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
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:Hydrogen2.98:1:001:00:0.34
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
5 :10gA gA5g A2g B
10g A2g B1: 2