1. Nomenclature

2. AlBr3 K2S ZnO Mg3N2 CCl4 CuO or Cu2O
We can determine the formula of a compound by completing Lewis diagrams or via the criss cross method
By knowing the valence of elements you can determine the formula of compounds
E.g. what compound would form from Ca + S?
Step 1 - write valences: Ca2+S2-
Step 2 - cross down valences: Ca2S2
Step 3 – reduce: CaS
a) Al,Br b) K,S c) Zn,O d) Mg,N e) C,Cl f) Cu,O
AlBr3
K2S
ZnO
Mg3N2
CCl4
CuO or Cu2O

3. Ionic compounds Rules for naming
Names end in -ide. Example: sodium chloride
Metal (cation) comes 1st (not chlorine sodide)
Do not capitalize (unless it’s the start of a sentence)
Give formulae & name: Ca + I, O + Mg, Na + S
= Ca2I1 = CaI2 = calcium iodide
= Mg2O2 = MgO = magnesium oxide
= Na1S2 = Na2S = sodium sulfide

4. Multiple valence: Latin naming
When the metal in an ionic compound is multivalent there are 2 methods: Latin or IUPAC
As before, the name ends in -ide & metal is first
The metal is named with it’s Latin or English root and ends in -ic or –ous to denote valence
E.g. Cu1 is cuprous, E.g. Cu2 is cupric
Lower = ous, Higher = ic
Give formulas and Latin names for:
Cu2+ + Cl- = CuCl2 = cupric chloride
= copper (II) chloride (IUPAC)
Cu+ + Cl = CuCl = cuprous chloride
= copper (I) chloride

6. Multiple valence: IUPAC naming
Name ends in -ide, positive/metal comes first
The valence of the metal is indicated in brackets using roman numerals
E.g. Cu1 is copper(I), Cu2 is copper(II)
Numbers refer to valences not to #s of atoms
Try:
Cu2+Cl, Zn2 + Cl, Co2+Cl, Hg+S (do both)
Cu2+Cl = Cu2Cl1 = CuCl2 = copper(II) chloride
Zn2+Cl = Zn2Cl1 = ZnCl2 = zinc chloride
Co2+Cl = Co2Cl1 = CoCl2 = cobalt(II) chloride
Hg+S = Hg1S2 = Hg2S = mercury(I) sulfide
Hg+S = Hg2S2 = HgS = mercury(II) sulfide

7. Compounds containing polyatomic ions
So far we have given valences to single atoms
Li + O
Li1O2  Li2O
Groups of atoms can also have valences
“Polyatomic ions” are groups of atoms that interact as a single unit.
E.g. OH1, (SO4)2. Ba3(PO4)2 =
barium phosphate
Naming compounds with polyatomic ions is similar to naming other ionic compounds
You should note that compounds with polyatomic ions have names ending in -ate or -ite not -ide
Note that most are negative, except ammonium
Name: Ca(OH)2, CuSO4, NH4NO3, Co2(CO3)3

8. Compounds containing polyatomic ions
Ca(OH)2
CuSO4
NH4NO3
Co2(CO3)3
- calcium hydroxide
- copper(II) sulfate
- ammonium nitrate
- cobalt(III) carbonate

9. Naming covalent compounds
-ide ending, each element has “prefix” 1
mono 2 di 3
tri 4
tetra 5
penta 6
hexa 7
hepta 8
octa 9
nona 10
deca
prefix refers to # of atoms - not valence
N2O4 = dinitrogen tetroxide
Exception: drop mono for first element
CO2 = carbon dioxide
The first vowel is often dropped to avoid the combination of “ao” or “oo”.
CO = carbon monoxide (monooxide)
P4O10= tetraphosphorus decoxide
SO2= sulfur dioxide (doxide)
Name: CCl4, P2O3, IF7

10. Write and name the following covalent compounds (IUPAC)
CCl4
P2O3
IF7
carbon tetrachloride
diphosporus trioxide
iodine heptafluoride

11. Working backwards: name to formula
It’s possible to determine a formula from a name
E.g. What is the formula of sodium oxide?
To get the answer, first write the valences:
Na1O2  Na2O
What is the formula of copper(II) oxide?
Cu2O2  Cu2O2  CuO
For covalent compounds, simply use the prefixes to tell you the number of each element:
What is the formula for dinitrogen trioxide?
N2O3
Give formulae for: lithium sulfide, dinitrogen monoxide, lead(IV) sulfate

12. Write and name the following covalent compounds (IUPAC)
lithium sulfide
dinitrogen monoxide
lead(IV) sulfate
Li1S2  Li2S
N2O
Pb4(SO4)2  Pb2(SO4)4  Pb(SO4)2

13. Assignment
Name each according to IUPAC rules: a) ZnS, b) FeCl3, c) CaCO3, d) P2O5, e) NaCN, f) N2F2, g) MgHPO4, h) Cu(BrO3)2, i) K2O, j) BF3
Give the valence of a) Fe in FeO, b) Mn in MnO2
3. Write formulas for: a) sodium oxide, b) potassium iodide, c) plumbic sulfide, d) mercury(I) oxide, e) ferrous oxide, f) iron(II) phosphate, g) copper(II) fluoride, h) dichlorine monoxide, i) silver sulfide, j) magnesium nitride, k) aluminum hypochlorite, l) iodine pentafluoride, m) calcium chromate, n) diphosphorus pentasulfide

14. Answers – 1, 2 zinc sulfide iron(III) chloride calcium carbonate
diphosporus pentoxide
sodium cyanide
dinitrogen difluoride
magnesium hydrogen phosphate
copper(II) bromate
potassium oxide
boron trifluoride
2 a) 2 b) 4

15. Answers – 3 Na2O KI PbS2 Hg2O FeO Fe3(PO4)2 CuF2 Cl2O Ag2S Mg3N2
Al(ClO)3
IF5
CaCrO4
P2S5

16. Naming Bases - calcium hydroxide Ca(OH)2 Bases contain an OH group
C6H12O6 does not have an OH group
If an OH group is present it will be clearly indicated: e.g. NaOH, Ca(OH)2
Also notice that bases have a metal (or positive ion such as NH4+ at their beginning)
Bases are named like other ionic compounds:
+ve is named first, followed by the polyatomic ion
- calcium hydroxide
- copper(I) hydroxide
- Al(OH)3
- NH4OH
Ca(OH)2
CuOH
aluminum hydroxide
ammonium hydroxide

17. Naming Acids: Binary acids
All acids start with H (e.g. HCl, H2SO4)
2 acids types exist: binary acids and oxyacids
Binary: H + non-metal. E.g. HCl
Oxy: H + polyatomic ion. E.g. H2SO4
Each have different naming rules.
Binary acids: naming depends on state of acid
If it’s not aqueous: hydrogen + non-metal
HCl(g) = hydrogen chloride
If it is aqueous: hydro + non-metal + ic acid
HCl(aq) = hydrochloric acid (aqueous hydrogen chloride)
HBr(s) HI(aq)
H2S(aq) H2S(g)
hydrogen bromide
hydroiodic acid
hydrosulfuric acid
hydrogen sulfide

18. Naming Acids: Oxyacids
Naming does not depend on the state (aq)
1) name the polyatomic ion
2) replace ate with ic, ite with ous
3) change non-metal root for pronunciation
4) add “acid” to the name
E.g. H2SO3
1) sulphite,
2) sulphous,
3) sulphurous,
4) sulphurous acid
HNO hypochlorous acid
H3PO4(aq) carbonic acid

19. Naming Acids: Oxyacids
HNO hypochlorous acid
H3PO4(aq) carbonic acid
- nitrous acid
- HClO
- phosphoric acid
- H2CO3

20. Assignment: give formula or name
a) chloric acid
b) hydrosulfuric acid
c) hydrobromic acid
d) phosphorous acid
e) iodic acid
f) HCl(g)
g) HCl(aq)
h) H2SO4(s)
i) H2SO4(aq)
j) HClO2
k) HF(aq)
a) HClO3
b) H2S(aq)
c) HBr(aq)
d) H3PO3
e) HIO3
f) hydrogen chloride
g) hydrochloric acid
h) sulfuric acid
i) sulfuric acid
j) chlorous acid
k) hydrofluoric acid

21. Hydrates
Some compounds contain H2O in their structure. These compounds are called hydrates.
This is different from (aq) because the H2O is part of the molecule (not just surrounding it).
The H2O can usually be removed if heated.
A dot separates water: e.g. CuSO4•5H2O is copper(II) sulfate pentahydrate.
A greek prefix indicates the # of H2O groups.
sodium sulfate decahydrate
nickel(II) sulfate hexahydrate
Na2CO3•H2O
BaCl2•2H2O
Na2SO4•10H2O
NiSO4•6H2O
sodium carbonate monohydrate
barium chloride dihydrate