Naming Naming &&

Writing FormulasWriting FormulasForFor

Molecular & Ionic CompoundsMolecular & Ionic Compounds

Naming Molecular Compounds

Non-metal + Non-metal

• Step 1: write the element name for the first

non-metal add a prefix ….(if there is more than

one atom)

• Step 2: Write the second element name and

add an ide ending Add a prefix

Exceptions

• DO NOT use any prefixes at all if the first element is hydrogen ……these are acids

Prefixes

1 = 6 =

2 = 7 =

3 = 8 =

4 = 9 =

5 = 10 =

mono

ditri

tetra

penta

hexa

hepta

octa

nona

deca

Examples

• P4O10 tetraphosphorus decaoxide

• bromine heptahydride

• H2S hydrogen sulfide

BrH7

Try the Following

• CO(g)

• CO2(g)

• N3F8

carbon monoxide

carbon dioxide

Trinitrogen octafluoride

Writing Formulas for Molecular Compounds

• Steps: Write each elements symbol Write the subscript number (the prefix)

• E.g. dinitrogen oxide N2O

Sulfur dioxide S20

Try the Following

• oxygen dibromide

• diphosphorus pentasulphide

• carbon tetraiodide

• phosphorus pentachloride

OBr2

P2S5

CI4

PCl5

Molecular Compounds that Must be memorized !!!

ammonia

water

NH3 ( g) =

H2O ( l) =H2S ( g) =

CH4 ( g) =

CH3OH ( l) =C2H6 ( g) =C2H5OH ( l) =

C6H12O6 ( s) =

hydrogen sulphide

methane

methanolethane

ethanol

glucosesucroseC12H22O11 ( s) =

hydrogen peroxideozoneO3 ( g) =

H2O2 ( l) =

Naming Binary Ionic Compounds

Metal + non-metal

• DO NOT USE PREFIXES

• Steps

1.Write the metal 1st

2. Write the non-metal 2nd with an ide ending

E.g. NaF

Na2Ssodium fluoride

sodium sulphide

two sodium ions are bonded with one sulphide ion… this doesn’t matter for naming ionic compound

Try the Following

• LiF

• KCl

• BeS

• Rb3P

• MgF2

• Na2O

• CsBr

lithium fluoride

potassium chloride

beryllium sulphide

rubidium phosphidemagnesium fluoride

sodium oxide

cesium bromide

Try the Following

• KCl

• MgBr2

• Ba3N2

• ScP

potassium chloride

magnesium bromide

barium nitride

scandium phosphide

Writing Formulas for Binary Ionic Compounds

• Steps

1.Look up the symbol for each…& write the metal first

2.Balance the charges (total + charges = total – charges)

3.Use subscripts to show the # of each element

sodium oxide

1+ Charge 2 Charge

1+ 2 = 2+ 2 1 = 2

Na2O

calcium phosphide

2+ Charge 3 Charge

2+ 3 = 6+ 3 2 = 6

Ca3P2

Try the Following

• magnesium chloride

• calcium chloride

• zinc sulphide

• silver sulphide

• germanium oxide

• calcium arsenide

• magnesium nitride

MgCl2

CaCl2

ZnS

Ag2S

GeO2

Ca3As2

Mg3N2

Try the Following

• lithium iodide

• zinc fluoride

• strontium phosphide

• silver oxide

• germanium arsenide

LiI

ZnF2

Sr3P2

Ag2O

Ge3As4

Naming Multivalent Ionic Compounds

• Transition metal ions have more than one possible charge

Cu2+, Cu+, Fe3+, Fe2+

transition metal + non-metal

• Steps

1. Write metal 1st with the charge in roman numerals

2.Write non-metal second

remember the charges have to balance

Roman Numerals (I,II,III,IV,V,VI,VII)

Examples

uranium (VI) fluoride

chromium (III) nitride

cobalt (II) chloride

U6+ F–

Cr3+ N3-

Co2+ Cl-

UF6

CrN

CoCl2

Try the Following

• AuBr

• CrCl2

• Co2O3

• VS2

• PuN2

gold (I) bromide

chromium (II) chloride

cobalt (III) oxide

vanadium (IV) sulphide

plutonium (VI) nitride

Naming Complex Ions

Metal + complex ion

• Steps:

1. Name the metal ion

2. Name the complex ion E.g.) PO43

Note: NH4+ (ammonium ion) is the

only positive complex ion…it will take the place of a metal

Examples

• CaCO3

• Ba(OH)2

• (NH4)3N

• CaCO3

• Ba(OH)2

• (NH4)3N

Solutions

Calcium carbonate

Barium hydroxide

Ammonium nitride

Try the Following

• KIO3

• NaCH3COO

• MgSO3

• NH4NO3

• Ca3(PO4)2

potassium iodate

sodium acetate

magnesium sulphite

ammonium nitrate

calcium phosphate

Writing Formulas For Complex Ions

• Steps:

1. Look up the symbol for each ion

2. Balance the charges

• Note: if you need more than 1 complex ion to balance the charges use brackets

• E.g. Ca(CH3COO)2

2+ 1 -

Try the Following

• aluminum phosphate

• calcium sulphite

• scandium acetate

• ammonium sulphate

• nickel (II) phosphate

• aluminum chlorate

AlPO4

Al(ClO3)3

CaSO3

Sc(CH3COO)3

(NH4)2SO4

Ni3(PO4) 2

SolubilitySolubility

Will the compound dissolve in water?Will the compound dissolve in water?

Soluble

• Refers to whether or not the compound dissolves in water

• If it is…. the compound is aqueous (aq)

• All acids are soluble

• Some ionic compounds are soluble… the rest are solids

Is It soluble?

• This will apply to ionic compounds (only)

• Steps

1. Find each ion in the boxes across the top

2. if it is soluble it will have (aq) aqueous

3. If it does not dissolve it will have (s) solid.

Determine if the following compounds are soluble in water. Use the proper subscript to indicate the state.

• AgCl• BaCO3

• LiOH• Ca2(PO4)3

• NaCl• CaI2

• Pb(NO3)2

• HMnO4

• AgCl

• BaCO3

• LiOH

• Ca2(PO4)3

• NaCl

• CaI2

• Pb(NO3)2

• HMnO4

(s)

(s)

(aq)

(s)

(aq)

(aq)

(aq)

(aq)

Acids & BasesAcids & Bases

Acids

• They are always soluble in water

• Conduct electricity

• Taste sour

• React with metals to produce hydrogen gas (H2(g))

• Neutralize a base

• they ALWAYS have hydrogen ….usually as the first element

• E.g. HCl(aq) , H3PO4(aq)

• There are three types: Binary Oxo Organic

Binary Acids

• contain only H and one other element (Cl, Br, etc.)

• E.g. HCl (aq)

Oxo Acids

• Contain H and Oxygen

• E.g. H3PO4(aq)

Organic Acids

• Contain C, H, & O

• The H is written at the end

• All have COO-

• E.g. CH3COOH(aq) – acetic acid

C6H5COOH(aq) - benzoic acid

HOOCCOOH(aq) – oxalic acid

Acid Indicators

• Turns blue litmus paper red

• Able to turn bromothymol blue to yellow

• Phenolphthalein remains colorless

• E.g. lemon juice

Bases

• Are usually soluble in water

• Conduct electricity (not weak ones)

• Neutralize acids

• Taste bitter

• Usually solids

• Feel slippery

Base Indicators

• Turns red litmus paper blue

• Bromothymol blue remains blue

• Turns phenolphthalein pink

• E.g. baking soda, Rolaids, soap, Draino crystals

Naming Acids

• Steps:

Hydrogen ____ide becomes hydro____ic acid

Hydrogen ____ate becomes _______ic acid

Hydrogen ____ ite becomes _______ ous acid

Examples

• HF (aq)       • H2SO3 (aq)

     

• H3BO3 (aq)

     

• HCl (g)   

hydrogen fluoride = hydrofluoric acid

hydrogen sulphite = sulphurous acid

hydrogen borate = boric acid

Hydrogen chloride (not an acid)

hydrosulphuric acid    phosphorus acid      

carbonic acid

hydrogen phosphite H3PO3 (aq)

1+ 3-

hydrogen carbonate H2CO3(aq)

1+ 2-

hydrogen sulphide H2S (aq)

1+ 2-

Try the Following

Writing Acid Formulas• Steps:

1. Use the naming rules in the opposite direction

• Example:

hydrosulphuric acid

hydrogen sulphide H2S(aq)

Try the Following

• carbonic acid

• chlorous acid

hydrogen carbonate

hydrogen chlorite

H2CO3(aq)

HClO2(aq)

Naming Bases

• Steps:

1. Write the metal name 1st

2. Write hydroxide or bicarbonate

E. g. NaOH sodium hydroxide

Try the Following

• KOH

• Ba(OH)2

• NaHCO3

potassium hydroxide

barium hydroxidesodium bicarbonate

Chemical Reactions• Can cause a physical or a chemical

change

• Always results in the formation of a new substance

• Evidence:

1. Temperature change

2. Formation of a precipitate

3. Colour change

4. Gas produces

states states

balancing

Reactants Products

1 H2 (g)+1 ZnCl2(aq)2 HCl(aq)1 Zn(s)+

Energy Changes

• Can occur in the form of heat, light, electrical, or mechanical

• There are two types: Endothermic Exothermic

• Endothermic Energy is absorbed (enters) Reactants + Energy products

• Exothermic Energy is released (leaves) Reactants product + energy

Balancing Equations

• There must be equal numbers of each element on both sides of the equation

Use lowest numbers

Example

____Mg(s) + ___ O2(g) ___ MgO(s)

____ H2O(l) ____H2(g) + ____ O2(g)

• When chemicals react they follow the Law of Conservation of Matter:

Matter can not be created or destroyed it only changes form

• Mass of reactants = mass of products

Counting Practice

• How many of each element are in the following compounds?

1. NaCl 5. NH4CH3COO

2. BaBr2 6. 3 (NH4)2S

3. (NH4)3P 7. 2 CaCl2

4. Ba(OH)2 8. 8 PbI2

9. 4 Zn(CH3COO)2

Balancing Practice

____ Cu(s) + ____ AgNO3(aq) ____ Ag(s) + ___Cu(NO3)2(g)

___ Cl2(g) + ____ NaBr(aq) ____ Br2(l) + ____ NaCl(aq)

____ KI(aq) + ___ Pb(NO3)2(aq) ___ PbI2(s) + ___KNO3(aq)

____ CH4(g) + ____ O2(g) ____ CO2(g) + ____ H2O(g)