1. Chemical Nomenclature
Ionic Compounds
often a metal + nonmetal
anion (nonmetal), add “ide” to element name
BaCl2
barium chloride
Known as a subscript
K2O
potassium oxide
Mg(OH)2
magnesium hydroxide
KNO3
potassium nitrate

3. cation – ion with a positive charge
An ion is an atom, or group of atoms, that has a net positive or negative charge.
cation – ion with a positive charge
If a neutral atom loses one or more electrons
it becomes a cation. Na
11 protons
11 electrons
Na+
11 protons
10 electrons
anion – ion with a negative charge
If a neutral atom gains one or more electrons
it becomes an anion.
Cl-
17 protons
18 electrons Cl
17 protons
17 electrons

4. Forming Cations & Anions
A CATION forms when an atom loses one or more electrons.
An ANION forms when an atom gains one or more electrons
F + e- --> F-
Mg --> Mg e-

5. Do You Understand Ions? How many protons and electrons are in ? Al27 13 3+
13 protons, 10 (13 – 3) electrons
How many protons and electrons are in ? Se 78 34 2-
34 protons, 36 (34 + 2) electrons

6. A monatomic ion contains only one atom
Na+, Cl-, Ca2+, O2-, Al3+, N3-
A polyatomic ion contains more than one atom
OH-, CN-, NH4+, NO3-

8. Compound Names and Formulas
A. Naming ionic compounds
1. Ionic - transfer of electrons - causing one
element to become a positive ion (cation) and
one element to become a negative ion (anion)
2. the positive ion always come first
NaCl is never written as ClNa
3. The name is derived from the ions that make it up
a. naming binary ionic compounds - two
elements

9. i. the positive ion is simply the name ion the element
ii. Na+ is sodium
Ba++ is Barium
b. the negative ion’s ending is changed to ide
i. chlorine - Cl is changed to Cl- - chloride
c. some polyatomic ions are name according to
their oxygen content
Sulfate and sulfite
SO4-- and SO3--

10. d. Some cations must show their charge
Fe++ is known as the Iron II ion
Fe+++is known as the Iron III ion
e. when writing chemical formulas from their names
- the number of positive ions must equal the number
of negative ions
Sodium fluoride
Na+F these charges are balanced

11. Ca++Cl- - these charges are not balanced so we must adjust the
Calcium chloride
Ca++Cl- - these charges are not balanced so we must adjust the
subscripts so the number of + equals the number of -
Ca++Cl2-
Remember - Charges must be balanced - so you must
have 2 -1’s to balance the +2
Coefficient
subscript
2NH CO3-2 ==> (NH4+ ) 2 CO3-2
Ammonium
carbonate
carbonate
Ammonium
Use coefficients to balance the total number of atoms -
Always balance charges first using subscripts

12. +1 with -1
Ammonium with acetate
NH C2H3O ==> NH4+ C2H3O2-
Ammonium
acetate
Ammonium Acetate

13. Cu+1 + C2H3O2- => Cu+1C2H3O2-
copper (I)
acetate
copper (I) acetate

14. You must make the charges equal
+1 with -2
There is an issue 2
NH4+ +
CO3 -- (
NH4+ )
CO3 -- 2
Ammonium
Carbonate
Ammonium carbonate
You must make the charges equal
now you must balance it according to the conservation of
mass

15. - so must have 3 +1 with the -3
You must always have the charges equal
- so must have 3 +1 with the -3
3NH PO ==> (NH4+)3PO4-3
Ammonium
phosphate
Ammonium
phosphate
+2 with -1
You must always have the charges equal
- so must have 2 -1’s to equal the +2
Ca C2H3O ===> Ca+2(C2H3O2-)2
acetate
Calcium
acetate
Calcium

16. +2 with -2
Since the charges are equal - you simply put them together
Ca CO ===> CaCO3
Calcium
Carbonate
Calcium
Carbonate
+2 with -3
Since the charges are not equal - you must find the
LCD for 2 and 3 which is 6 so
3Ca PO ==> Ca+23(PO4 -3 )2
Calcium
Phosphate
Calcium
Phosphate

17. +3 with -1 Al+3 + 3 C2H3O2-  Al+3(C2H3O2-)3 Aluminum Acetate

18. Aluminum Carbonate Aluminum Carbonate +3 with -2
2Al CO  Al+32 (CO3 --)3
Aluminum
Carbonate
Aluminum Carbonate

19. +3 with -3 Al +++ + PO4 ---  Al+++PO4 --- Aluminum Phosphate

21. A molecular formula shows the exact number of atoms of each element in the smallest unit of a substance
An empirical formula shows the simplest
whole-number ratio of the atoms in a substance
H2O
molecular
empirical
H2O
C6H12O6
CH2O O3 O
N2H4
NH2

23. Molecular compounds nonmetals or nonmetals + metalloids common names
H2O, NH3, CH4, C60
element further left in periodic table is 1st
element closest to bottom of group is 1st
if more than one compound can be formed from the same elements, use prefixes to indicate number of each kind of atom
last element ends in ide

24. Molecular Compounds HI hydrogen iodide NF3 nitrogen trifluoride SO2
sulfur dioxide
N2Cl4
dinitrogen tetrachloride
TOXIC!
NO2
nitrogen dioxide
N2O
dinitrogen monoxide
Laughing Gas

25. Mixed Practice Dinitrogen monoxide Potassium sulfide
Copper (II) nitrate
Dichlorine heptoxide
Chromium (III) sulfate
Iron(III) sulfite
Calcium oxide
Barium carbonate
Iodine monochloride
N2O
K2S
Cu(NO3)2
Cl2O7
Cr2(SO4)3
Fe2(SO3)3
CaO
BaCO3
ICl

26. Mixed Practice BaI2 P4S3 Ca(OH)2 FeCO3 Na2Cr2O7 I2O5 Cu(ClO4)2 CS2
B2Cl4
Barium iodide
Tetraphosphorus trisulfide
Calcium hydroxide
Iron (II) carbonate
Sodium dichromate
Diiodine pentoxide
Cupric perchlorate
Carbon disulfide
Diboron tetrachloride

27. Examples of Older Names of Cations formed from Transition Metals (memorize these!!)
From Zumdahl

28. An acid can be defined as a substance that yields
hydrogen ions (H+) when dissolved in water.
HCl
Pure substance, hydrogen chloride
Dissolved in water (H+ Cl-), hydrochloric acid
An oxoacid is an acid that contains hydrogen, oxygen, and another element.
HNO3
nitric acid
H2CO3
carbonic acid
H2SO4
sulfuric acid
HNO3

29. Transition metal ionic compounds
indicate charge on metal with Roman numerals
FeCl2
iron(II) chloride
2 Cl- -2 so Fe is +2
FeCl3
3 Cl- -3 so Fe is +3
iron(III) chloride
Cr2S3
3 S-2 -6 so Cr is +3 (6/2)
chromium(III) sulfide

30. Oxidation and reduction
1. Oxidation and reduction (redox reactions)
A. Oxidation - loss of electrons
B. Reduction - gain of electrons
Oxidation-reduction reactions MUST
happen at the same time

31. C. Oxidation numbers - number of electrons
gained, lost or shared
1. how to assign oxidation numbers
a. free elements are assigned an
oxidation number of zero
i. free element - any un- combined
element - this includes the 7 diatomics
H2, N2, O2, F2, Cl2, Br2, I2
These 7 elements must be together if they are alone

32. b. mono atomic ion's charge equals their
oxidation number
i. Na+1= +1
ii. S-2 = -2
c. hydrogen's oxidation is =1
d. oxygen's oxidation number is -2
except in peroxides. In peroxides,
the oxidation is -1

33. e. the sum of the oxidation numbers of a
compound must add up to be zero
f. the sum of the oxidation numbers of a
polyatomic ion must add up to equal
its charge

34. The oxidation number of hydrogen is +1 except when it is bonded to metals in binary compounds. In these cases, its oxidation number is –1.
Group IA metals are +1, IIA metals are +2 and fluorine is always –1.
6. The sum of the oxidation numbers of all the atoms in a molecule or ion is equal to the charge on the molecule or ion.
Oxidation numbers of all the elements in HCO3- ?

35. +1 -2
HCO3- +1 ? +4 -6
= -1
H = +1
O = -2
C = +4

36. Li+, Li = +1; Fe3+, Fe = +3; O2-, O = -2
Oxidation number
The charge the atom would have in a molecule (or an
ionic compound) if electrons were completely transferred.
Free elements (uncombined state) have an oxidation number of zero.
Na, Be, K, Pb, H2, O2, P4 = 0
In monatomic ions, the oxidation number is equal to the charge on the ion.
Li+, Li = +1; Fe3+, Fe = +3; O2-, O = -2
The oxidation number of oxygen is usually –2. In H2O2 and O22- it is –1.

37. Try some
find the oxidation numbers for each element

38. Formula of Ionic Compounds
2 x +3 = +6
3 x -2 = -6
Al2O3
Al3+
O2-
1 x +2 = +2
2 x -1 = -2
CaBr2
Ca2+
Br-
1 x +2 = +2
1 x -2 = -2
Na2CO3
Na+
CO32-

39. NH4+Br-
Ca+2Cl-2
Na+C2H3O2-
Cu+2SO4-
K+HCO3-
Ba+2(NO3-)2

40. Zn+2S-2
Li+3PO4-3
Al+3(HSO4-)3
Fe+3 2O-2 3
Zn+2CO3-2
H+CN-

41. Ag+ 2 Cr2O7 -2
Fe+3PO3 -3
H2+ O2-2
Ca+2 HPO4-2
Cu+NO2-
Cu+2 (NO2- )2

42. Hg+2C2O4-2
Cr+3(OH- )3