Ionic and covalent bonding naming and formula guide provides comprehensive coverage of chemical bonding concepts essential for chemistry students. This resource explains the principles of naming ionic and covalent compounds, including the use of prefixes and polyatomic ions. It includes practice problems and detailed examples to help students master the material. Ideal for high school chemistry courses, this guide supports learners preparing for exams and enhancing their understanding of chemical formulas and nomenclature.

Key Points

  • Explains naming conventions for ionic and covalent compounds.
  • Includes practice problems for mastering chemical formulas.
  • Covers the use of prefixes in naming covalent compounds.
  • Details the role of polyatomic ions in chemical nomenclature.
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Unit 2: Chemistry
Name:
Block:
Science 9
Book 7: Naming & Writing
Chemical Formulas
1
NON-METALSMETALS
Ion charge(s)
47.9
Titanium
3+
Ti
4+22
Atomic Mass
Name
Symbol
Atomic Number
PERIODIC TABLE OF THE ELEMENTS
Alkaline
Earth
Metals
Alkali
Metals
Noble
Gases
Halogens
Based on mass of C-12 at 12.00.
Any value in parentheses
is the mass of the most
stable or best known isotope for
elements which do not occur naturally.
(262)
Lawrencium
Lr
3+103
(259)
Nobelium
3+
No
2+102
(258)
Mendelevium
3+
Md
2+101
(257)
Fermium
Fm
3+100
(252)
Einsteinium
Es
3+99
(251)
Californium
Cf
3+98
(247)
Berkelium
4+
Bk
3+97
(247)
Curium
Cm
3+96
(243)
Americium
Am
95
6+
5+
4+
3+
5+
3+
6+
4+
(244)
Plutonium
Pu
94
6+
4+
3+
5+
(237)
Neptunium
Np
93
5+
4+
6+
238.0
Uranium
U
92
231.0
Protactinium
4+
Pa
5+91
232.0
Thorium
Th
4+90
175.0
Lutetium
Lu
3+71
173.0
Ytterbium
2+
Yb
3+70
168.9
Thulium
2+
Tm
3+69
167.3
Erbium
Er
3+68
164.9
Holmium
Ho
3+67
162.5
Dysprosium
Dy
3+66
158.9
erbiumT
4+
Tb
3+65
157.3
Gadolinium
Gd
3+64
152.0
Europium
2+
Eu
3+63
150.4
Samarium
4+
Sm
3+62
(145)
Promethium
Pm
3+61
144.2
Neodymium
Nd
3+60
140.9
Praseodymium
4+
Pr
3+59
140.1
Cerium
4+
Ce
3+58
(266)
Meitnerium
Mt
109
(265)
Hassium
Hs
108
(262)
Bohrium
Bh
107
(263)
Sg
Seaborgium
106
(262)
Dubnium
Db
105
(2 61)
Rutherfordium
Rf
1 04
(227)
Ac t i ni u m
Ac
3+89
(226)
Radium
Ra
2+88
(223)
Francium
Fr
+87
(222)
Radon
Rn
086
(210)
Astatine
At
–85
(209)
Polonium
4+
Po
2+84
0209.
Bismuth
5+
Bi
3+83
207.2
Lead
4+
Pb
2+82
204.4
Thallium
3+
Tl
1+81
200.6
Mercury
1+
Hg
2+80
197.0
Gold
1+
Au
3+79
195.1
Platinum
2+
Pt
4+78
192.2
Iridium
4+
Ir
3+77
190.2
Osmium
4+
Os
3+76
186.2
Rhenium
7+
Re
4+75
183.8
ungstenT
W
6+74
180.9
antalumT
Ta
5+73
178.5
Hafnium
Hf
4+72
138.9
Lanthanum
La
3+57
137.3
Barium
Ba
2+56
132.9
Cesium
Cs
+55
131.3
Xenon
Xe
054
126.9
Iodine
I
–53
127.6
Tellurium
Te
2–52
121.8
Antimony
5+
Sb
3+51
118.7
Tin
2+
Sn
4+50
114.8
Indium
In
3+49
112.4
Cadmium
Cd
2+48
107.9
Silver
Ag
+47
106.4
Palladium
4+
Pd
2+46
102.9
Rhodium
4+
Rh
3+45
101.1
Ruthenium
4+
Ru
3+44
(98)
Technetium
Tc
7+43
95.9
Molybdenum
3+
Mo
2+42
92.9
Niobium
5+
Nb
3+41
91.2
Zirconium
Zr
4+40
88.9
Yttrium
Y
3+39
87.6
Strontium
Sr
2+38
85.5
Rubidium
Rb
+37
83.8
Krypton
Kr
036
79.9
Bromine
Br
–35
79.0
Selenium
Se
2–34
74.9
Arsenic
As
3–33
72.6
Germanium
Ge
4+32
69.7
Gallium
Ga
3+31
65.4
Zinc
Zn
2+30
63.5
Copper
1+
Cu
2+29
58.7
Nickel
3+
Ni
2+28
58.9
Cobalt
3+
Co
2+27
55.8
Iron
2+
Fe
3+26
54.9
Manganese
Mn
25
4+
3+
2+
52.0
Chromium
2+
Cr
3+24
50.9
Vanadium
4+
V
5+23
47.9
Titanium
3+
Ti
4+22
45.0
Scandium
Sc
3+21
40.1
Calcium
Ca
2+20
39.1
Potassium
K
+19
39.9
Argon
Ar
018
35.5
Chlorine
Cl
–17
32.1
Sulfur
S
2–16
31.0
Phosphorus
P
3–15
28.1
Silicon
Si
14
27.0
Aluminium
Al
3+13
24.3
Magnesium
Mg
2+12
23.0
Sodium
Na
+11
20.2
Neon
Ne
010
19.0
Fluorine
F
9 –
16.0
Oxygen
O
–8 2
14.0
Nitrogen
N
–7 3
12.0
Carbon
C
6
10.8
Boron
B
5
9.0
Beryllium
Be
+4 2
6.9
Lithium
Li
3 +
4.0
Helium
He
2 0
1.0
Hydrogen
H
1 –
1.0
Hydrogen
H
1 +
(294)
Ununoctium
Uuo
118
(?)
Ununseptium
Uus
117
(292)
Ununhexium
Uuh
116
(288)
Uup
Ununpentium
115
(289)
Ununquadium
Uuq
114
(2 84)
Ununtrium
Uut
1 13
(285)
Un u n bi u m
Uub
112
(272)
Roentgenium
Rg
111
(281)
Darmstadtium
Ds
110
1
2
3 4 5 6 7 8 9 10 11 12
13 14 15 16 17
18
2
Positive Ions
NAMES, FORMULAE AND CHARGES OF
SOME POLYATOMIC IONS
Negative Ions
NAMES AND FORMULAE OF
COMMON ACIDS
Hydrochloric acid
Sulfuric acid
Nitric acid
Acetic acid
NH
4
+
Ammonium CH
3
COO
–
Acetate
CO
3
2–
Carbonate
ClO
3
–
Chlorate
ClO
2
–
Chlorite
CrO
4
2–
Chromate
CN
–
Cyanide
Cr
2
O
7
2–
Dichromate
HCO
3
–
Hydrogen carbonate, bicarbonate
HSO
4
–
Hydrogen sulfate, bisulfate
HS
–
Hydrogen sulfide, bisulfide
HSO
3
–
Hydrogen sulfite, bisulfite
OH
–
Hydroxide
ClO
–
Hypochlorite
NO
3
–
Nitrate
NO
2
–
Nitrite
ClO
4
–
Perchlorate
MnO
4
–
Permanganate
PO
4
3–
Phosphate
PO
3
3–
Phosphite
SO
4
2–
Sulfate
SO
3
2–
Sulfite
PREFIXES
1
2
3
4
5
6
7
8
9
10
mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca
HCl
H
2
SO
4
HNO
3
HCH
3
COO
3
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End of Document
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FAQs

What are the rules for naming ionic compounds?
Ionic compounds are named by identifying the cation and anion. The cation retains its name, while the anion's name is modified to end in 'ide' if it is a single element. For polyatomic ions, the name remains unchanged. For example, NaCl is named sodium chloride, while Ca(NO3)2 is called calcium nitrate.

How do you name covalent compounds?
Covalent compounds are named using prefixes to indicate the number of atoms present. For instance, CO2 is named carbon dioxide, reflecting the presence of two oxygen atoms. The prefix 'mono-' is often omitted for the first element if there is only one atom. Therefore, N2O is named dinitrogen monoxide.

What is the significance of polyatomic ions in chemical formulas?
Polyatomic ions are groups of atoms that carry a charge and are treated as single entities in chemical formulas. They play a crucial role in ionic compounds, where they can combine with cations to form stable compounds. For example, ammonium sulfate consists of the ammonium ion (NH4+) and sulfate ion (SO4^2-), demonstrating how polyatomic ions contribute to the overall charge balance.

What are some common prefixes used in naming covalent compounds?
Common prefixes include mono- (1), di- (2), tri- (3), tetra- (4), penta- (5), hexa- (6), hepta- (7), octa- (8), nona- (9), and deca- (10). These prefixes help indicate the number of atoms of each element in a compound. For instance, in sulfur hexafluoride (SF6), 'hexa-' indicates that there are six fluorine atoms.

How can students practice naming and writing chemical formulas?
Students can practice by working through exercises that require them to name compounds based on their chemical formulas and vice versa. The guide includes numerous practice problems that reinforce the concepts of ionic and covalent bonding, helping students gain confidence in their skills. Additionally, reviewing examples of both types of compounds can aid in understanding the naming conventions.