Science 9 Unit 2 Chemistry focuses on naming and writing chemical formulas, essential for understanding chemical compounds. This resource provides comprehensive guidance on covalent and ionic compounds, including naming conventions and formula writing techniques. Students will learn about polyatomic ions, the use of prefixes in covalent compounds, and the significance of charge balancing in ionic compounds. Ideal for Grade 9 science students, this material prepares learners for exams and practical applications in chemistry.

Key Points

  • Explains naming conventions for ionic and covalent compounds.
  • Covers the use of prefixes in naming covalent compounds.
  • Includes practice problems for writing chemical formulas.
  • Discusses the significance of polyatomic ions in chemical naming.
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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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FAQs

What are the key differences between ionic and covalent compounds?
Ionic compounds consist of metal and non-metal ions that transfer electrons, resulting in charged ions. They typically have high melting and boiling points and conduct electricity when dissolved in water. In contrast, covalent compounds are formed by the sharing of electrons between non-metals, leading to the formation of molecules. These compounds usually have lower melting and boiling points and do not conduct electricity in solution.

How do you name a covalent compound?
To name a covalent compound, use prefixes to indicate the number of atoms of each element present in the molecule. For example, CO2 is named carbon dioxide, where 'di-' indicates two oxygen atoms. The first element retains its full name, while the second element's name is modified to end in '-ide.' If there is only one atom of the first element, the prefix 'mono-' is often omitted.

What is the significance of polyatomic ions in chemical formulas?
Polyatomic ions are groups of atoms that carry a charge and are treated as a single unit in chemical formulas. They play a crucial role in ionic compounds, where they can combine with metal ions to form stable compounds. For example, in calcium sulfate (CaSO4), the sulfate ion (SO4) is a polyatomic ion that allows for the formation of the compound. Understanding polyatomic ions is essential for correctly naming and writing chemical formulas.

What are the rules for writing chemical formulas for ionic compounds?
When writing chemical formulas for ionic compounds, the first step is to identify the ions involved and their charges. The total positive charge from the metal ions must balance the total negative charge from the non-metal ions. Use subscripts to indicate the number of each ion needed to achieve this balance. For example, in magnesium chloride (MgCl2), one magnesium ion (Mg2+) balances with two chloride ions (Cl-).

How do you determine the name of a compound from its chemical formula?
To determine the name of a compound from its chemical formula, first identify the elements present and their respective charges if applicable. For ionic compounds, the metal is named first, followed by the non-metal with an '-ide' suffix. For covalent compounds, use prefixes to indicate the number of atoms of each element. For example, the formula N2O4 translates to dinitrogen tetroxide, indicating two nitrogen atoms and four oxygen atoms.