1. 10/23/09
Naming Compounds
Day 2

2. Working backwards: name to formula
10/23/09
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

3. Write and name the following covalent compounds (IUPAC)‏
10/23/09
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

4. Assignment
10/23/09
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

5. Complete exercises on handout
10/23/09
Complete exercises on handout
Steps:
Determine if its ionic or covalent
If ionic, determine if its metal has one or more valence
Name according to appropriate rules

6. Answers – 1, 2 zinc sulfide iron(III) chloride calcium carbonate
10/23/09
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

7. Answers – 3 Na2O KI PbS2 Hg2O FeO Fe3(PO4)2 CuF2 Cl2O Ag2S Mg3N2
10/23/09
Na2O KI
PbS2
Hg2O
FeO
Fe3(PO4)2
CuF2
Cl2O
Ag2S
Mg3N2
Al(ClO)3
IF5
CaCrO4
P2S5

8. Naming Bases Bases contain an OH group
10/23/09
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

9. Naming Acids: Binary acids
10/23/09
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
hydr(o)iodic acid
hydrosulfuric acid
hydrogen sulfide

10. Naming Acids: Oxyacids
10/23/09
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

11. Naming Acids: Oxyacids
10/23/09
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
- nitrous acid
- HClO
- phosphoric acid
- H2CO3

12. Assignment: give formula or name
10/23/09
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

13. For more lessons, visit www.chalkbored.com
Hydrates
10/23/09
For more lessons, visit
Some compounds contain H2O in their struc-ture. 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