CompoundsCompounds

Know Your Periodic TableKnow Your Periodic Table

Transition Metals

Metals

Metals

Naming Ionic CompoundsNaming Ionic Compounds

Binary Ionic Compounds Consist of two elements: metal cation and a non-metal

anion

Metal is named first and says its own name

Non-metal is named second and changes its suffix to “ide”

For transition metals with more than one ionic chargeUse the anions to determine their charge

Indicate their charge with roman numerals Only Ag+, Zn2+, and Cd2+ have 1 charge. You do not need

Roman numerals for these

Binary Ionic Compounds Consist of two elements: metal cation and a non-metal

anion

Metal is named first and says its own name

Non-metal is named second and changes its suffix to “ide”

For transition metals with more than one ionic chargeUse the anions to determine their charge

Indicate their charge with roman numerals Only Ag+, Zn2+, and Cd2+ have 1 charge. You do not need

Roman numerals for these

ExamplesExamplesIonsIons Compound NameCompound Name

Sodium & chlorineSodium & chlorine Sodium chlorSodium chlorideide

Aluminum & chlorineAluminum & chlorine Aluminum chlorAluminum chlorideide

Aluminum & oxygenAluminum & oxygen Aluminum oxAluminum oxideide

Sodium & sulphurSodium & sulphur Sodium sulphSodium sulphideide

Iron (2 +) & OxygenIron (2 +) & Oxygen iron (II) oxideiron (II) oxide

Iron (3+) & OxygenIron (3+) & Oxygen iron (III) oxideiron (III) oxide

Formulas for Ionic CompoundsFormulas for Ionic Compounds

Binary Ionic CompoundsWrite down the symbols for each individual ion

side by side – cation first, anion secondBalance the charges by crossing them

(Swap & Drop)*Charges become subscripts*

Write the formulaNote:

You do not need to write the subscript 1 in the formula

You should reduce the subscripts if possible

Binary Ionic CompoundsWrite down the symbols for each individual ion

side by side – cation first, anion secondBalance the charges by crossing them

(Swap & Drop)*Charges become subscripts*

Write the formulaNote:

You do not need to write the subscript 1 in the formula

You should reduce the subscripts if possible

ExamplesExamples

Compound Compound NameName

IonsIons FormulaFormula

Sodium Sodium chlorchlorideide

NaNa++ & Cl & Cl-- NaClNaCl

Aluminum Aluminum oxoxideide

AlAl3+3+ & O & O2-2- AlAl22OO33

iron (III) oxideiron (III) oxide FeFe3+3+ & & OO2-2- FeFe22OO33

iron (II) oxideiron (II) oxide FeFe2+2+ & & OO2-2- FeFe22OO22 FeO FeO

Naming Ionic CompoundsNaming Ionic Compounds

Ternary Ionic CompoundsIonic compounds that contain polyatomic ions

Polyatomic ions act as a single unit (subscripts included)

Monatomic cations say their own name; monatomic anions end in the suffix “ide”

Polyatomic ions always say their own name

When more than one polyatomic ion is used in a formula, it will be placed in brackets

Ternary Ionic CompoundsIonic compounds that contain polyatomic ions

Polyatomic ions act as a single unit (subscripts included)

Monatomic cations say their own name; monatomic anions end in the suffix “ide”

Polyatomic ions always say their own name

When more than one polyatomic ion is used in a formula, it will be placed in brackets

ExamplesExamples

IonsIons Compound NameCompound Name

Ammonium & chlorineAmmonium & chlorine Ammonium chlorideAmmonium chloride

Potassium & sulfatePotassium & sulfate Potassium sulfatePotassium sulfate

Lead (2+) & phosphateLead (2+) & phosphate Lead (II) phosphateLead (II) phosphate

Ammonium & oxalateAmmonium & oxalate Ammonium oxalateAmmonium oxalate

Formulas for Ionic CompoundsFormulas for Ionic Compounds

Ternary Ionic CompoundsSame as binary ionic compounds

Make sure that when you balance the charges that the subscript for a polyatomic ion is OUTSIDE of the bracketsThis is because polyatomic ions act as a single unit and

the subscript applies to the entire unit

Remember, numbers WITHIN the brackets of a polyatomic ion CANNOT be reduced

Ternary Ionic CompoundsSame as binary ionic compounds

Make sure that when you balance the charges that the subscript for a polyatomic ion is OUTSIDE of the bracketsThis is because polyatomic ions act as a single unit and

the subscript applies to the entire unit

Remember, numbers WITHIN the brackets of a polyatomic ion CANNOT be reduced

ExamplesExamples

Compound Compound NameName

IonsIons FormulaFormula

Ammonium Ammonium sulphidesulphide

NHNH4+4+ & S & S2-2- (NH(NH44))22SS

Potassium Potassium carbonatecarbonate

KK++ & CO & CO332-2- KK22COCO33

Iron (II) nitrateIron (II) nitrate FeFe2+2+ & NO & NO33-- Fe(NOFe(NO33))22

Sodium sulfateSodium sulfate NaNa++ & SO & SO442-2- NaNa22(SO(SO44))

Acid StructureAcid Structure

Have a characteristic formula structure: “HX”Where “H” is a hydrogen cationWhere “X” is an anionSo generally, if you see a formula

for an ionic compound that starts with an “H” it is likely an acid

Have a characteristic formula structure: “HX”Where “H” is a hydrogen cationWhere “X” is an anionSo generally, if you see a formula

for an ionic compound that starts with an “H” it is likely an acid

Naming AcidsNaming Acids

Scenario 1 – The anion ends in the suffix “ide”Add the prefix “hydro” to the anion

Change the suffix to “ic”

Add the word “acid” to the end

i.e. HF hydrogen & fluoride hydrofluoric acid

i.e. HCN hydrogen & cyanide hydrocyanic acid

Scenario 1 – The anion ends in the suffix “ide”Add the prefix “hydro” to the anion

Change the suffix to “ic”

Add the word “acid” to the end

i.e. HF hydrogen & fluoride hydrofluoric acid

i.e. HCN hydrogen & cyanide hydrocyanic acid

Naming AcidsNaming Acids

Scenario 2 – The anion ends with the suffix “ate”Change the suffix of the anion to “ic”Add the word “acid” to the endNote: no need for the “hydro” prefixHint to remember – “If you ATE it, its Icky”

i.e. HNO3 hydrogen & nitrate nitric acid

i.e. H2SO4 hydrogen & sulfate Sulfuric acid

Scenario 2 – The anion ends with the suffix “ate”Change the suffix of the anion to “ic”Add the word “acid” to the endNote: no need for the “hydro” prefixHint to remember – “If you ATE it, its Icky”

i.e. HNO3 hydrogen & nitrate nitric acid

i.e. H2SO4 hydrogen & sulfate Sulfuric acid

Naming AcidsNaming Acids

Scenario 3 – The anion ends with the suffix “ite”Change the suffix on the anion to “ous”

Add the word “acid” to the end

Note: no need for the “hydro” prefix

i.e. HNO2 hydrogen & nitrite

nitrous acid

i.e. H2SO3 hydrogen & sulfite

sulfurous acid

Scenario 3 – The anion ends with the suffix “ite”Change the suffix on the anion to “ous”

Add the word “acid” to the end

Note: no need for the “hydro” prefix

i.e. HNO2 hydrogen & nitrite

nitrous acid

i.e. H2SO3 hydrogen & sulfite

sulfurous acid

Writing Acid FormulasWriting Acid Formulas

Use the prefix/suffix combinations to figure out the anion

Balance the charges with a H+ cation (s)

Write the formula

i.e. – permanganic acid permanganate anion MnO4

-

HMnO4

Use the prefix/suffix combinations to figure out the anion

Balance the charges with a H+ cation (s)

Write the formula

i.e. – permanganic acid permanganate anion MnO4

-

HMnO4

Naming Covalent CompoundsNaming Covalent Compounds

Prefixes are used to indicate the number of atoms

The prefix “mono” is only used for the second atom; no mono prefix needed for the first atom

The second atom named ends with the suffix, “ide”

Prefixes are used to indicate the number of atoms

The prefix “mono” is only used for the second atom; no mono prefix needed for the first atom

The second atom named ends with the suffix, “ide”

Prefixes: 1 – “mono” 2 – “di” 3 – “tri” 4 – “tetra” 5 – “penta” 6 – “hexa” 7 – “hept” 8 – “oct” 9 – “non” 10 - “deca”

Prefixes: 1 – “mono” 2 – “di” 3 – “tri” 4 – “tetra” 5 – “penta” 6 – “hexa” 7 – “hept” 8 – “oct” 9 – “non” 10 - “deca”

Examples of Naming Covalent CompoundsExamples of Naming Covalent Compounds

N2H4: Dinitrogen tetrahydride

SO3: Sulfur trioxide

CO2: Carbon dioxide

P2O5: Diphosphorus pentoxide

PCl3: Phosphorus trichloride

N2H4: Dinitrogen tetrahydride

SO3: Sulfur trioxide

CO2: Carbon dioxide

P2O5: Diphosphorus pentoxide

PCl3: Phosphorus trichloride

Formulas for Covalent CompoundsFormulas for Covalent Compounds

Read the prefixes to determine the amount of each atom

Examples:carbon tetrachloride:

CCl4 dinitrogen trioxide:

N2O3 carbon disulfide:

CS2 dihydrogen monosulfide:

H2Ssulfur hexafluoride:

SF6

Read the prefixes to determine the amount of each atom

Examples:carbon tetrachloride:

CCl4 dinitrogen trioxide:

N2O3 carbon disulfide:

CS2 dihydrogen monosulfide:

H2Ssulfur hexafluoride:

SF6

Number of Atoms in a FormulaNumber of Atoms in a Formula

The number of atoms in a formula is determined by the subscripts

If there is no subscript, this means that there is only one of a particular atomi.e.: NaCl

○ 1 Na atom and 1 Cl atom○ 2 atoms total

When you are dealing with polyatomic ions, remember that the subscript found outside of the brackets is applied to every atom inside the brackets by using the distributive property of multiplicationi.e.: Mg(NO3)2

○ 1 Mg atom, 2 N atoms, 6 O atoms○ 9 atoms total

The number of atoms in a formula is determined by the subscripts

If there is no subscript, this means that there is only one of a particular atomi.e.: NaCl

○ 1 Na atom and 1 Cl atom○ 2 atoms total

When you are dealing with polyatomic ions, remember that the subscript found outside of the brackets is applied to every atom inside the brackets by using the distributive property of multiplicationi.e.: Mg(NO3)2

○ 1 Mg atom, 2 N atoms, 6 O atoms○ 9 atoms total

Molar Mass of Molecules & CompoundsMolar Mass of Molecules & Compounds

To find the mass of a molecule/compound, simply add up all of the masses of the individual atoms in the compound

Value is known as the “Molar Mass” of a molecule/compound

i.e.: NaCl

i.e.: Mg(NO3)2

To find the mass of a molecule/compound, simply add up all of the masses of the individual atoms in the compound

Value is known as the “Molar Mass” of a molecule/compound

i.e.: NaCl

i.e.: Mg(NO3)2

Percent Composition by MassPercent Composition by Mass

The percent composition by mass of a molecule/compound is simply the percentage of mass for each element in the molecule/compound

To calculate the percent composition:

Examples: NaCl

Mg(NO3)2

The percent composition by mass of a molecule/compound is simply the percentage of mass for each element in the molecule/compound

To calculate the percent composition:

Examples: NaCl

Mg(NO3)2