Unit 1.1 Formulae and Equations Flashcards
1
Q
What does the chemical formula do?
A
A chemical formula tells us which elements make up a particular compound and how many atoms of each element there are in a molecule of that compound.
2
Q
formula of hydrogen ion
A
H+
3
Q
formula of lithium ion
A
Li+
4
Q
formula of sodium
A
Na+
5
Q
formula of potassium
A
K+
6
Q
formula of silver
A
Ag+
7
Q
formula of magnesium
A
Mg2+
8
Q
formula of calcium
A
Ca2+
9
Q
formula of barium
A
Ba2+
10
Q
formula of zinc
A
Zn2+
11
Q
formula of aluminium
A
Al3+
12
Q
formula of copper (I)
A
Cu+
13
Q
formula of copper (II)
A
Cu2+
14
Q
formula of iron (II)
A
Fe2+
15
Q
formula of iron (III)
A
Fe3+
16
Q
formula of tin (II)
A
Sn2+
17
Q
formula of tin (IV)
A
Sn4+
18
Q
formula of lead (II)
A
Pb2+
19
Q
formula of lead (IV)
A
Pb4+
20
Q
formula of chromium (III)
A
Cr3+
21
Q
formula of manganese (II)
A
Mn2+
22
Q
formula of fluoride
A
F-
23
Q
formula of chloride
A
Cl-
24
Q
formula of bromide
A
Br-
25
formula of iodide
I-
26
formula of oxide
O2-
27
formula of sulfide
S2-
28
formula of nitride
N3-
29
formula of phosphide
P3-
30
formula of hydride
H-
31
formula of hydroxide
OH-
32
formula of nitrate
NO3-
33
formula of carbonate
CO32-
34
formula of sulfate
SO42-
35
formula of phosphate
PO43-
36
formula of sulfite
SO32-
37
formula of hydrogen carbonate
HCO3-
38
formula of hydrogen sulfate
HSO4-
39
formula of ammonium
NH4+
40
formula of magnesium oxide
MgO
41
formula of sodium sulfide
Na2S
42
formula of calcium nitrate
Ca(NO3)2
43
formula of aluminium oxide
Al2O3
44
formula of iron (III) oxide
Fe2O3
45
formula of copper (II) sulfate
CuSO4
46
formula of sodium nitride
Na3N
47
formula of potassium sulfite
K2SO3
48
formula of calcium phosphide
Ca3P2
49
formula of sodium carbonate
NazCO3
50
formula of tin (II) oxide
SnO
51
What do oxidation numbers show? (What are oxidation numbers?)
Oxidation numbers (states) show the total number of electrons which have been removed (or partly removed) from an element or added (or partly added) to an element to get to its present state.
52
List the rules for working out oxidation numbers.
1. The oxidation number of an uncombined element is zero.
2. The sum of oxidation numbers of all the atoms or ions in a neutral compound is zero.
3. The sum of the oxidation numbers of all the atoms in an ion is equal to the charge on the ion.
4. The more electronegative element in a substance is given a negative oxidation number.
5. Some elements almost always have the same oxidation number in their compounds.
53
What is the usual oxidation state of group I elements?
always +1
54
What is the usual oxidation state of group II elements?
always +2
55
what is the usual oxidation state of oxygen?
usually -2,
except in peroxides (-1) and F2O(+2)
56
what is the usual oxidation state of hydrogen?
usually +1
except in metal hydrides where it is -1
57
what is the usual oxidation state of fluorine?
always -1
58
what is the usual oxidation state of chlorine?
usually -1
except in compounds with O or F.
59
What are oxidation numbers used for?
They are used to give unambiguous names to compounds.
60
How do you write an ionic equation?
1. Write the balanced equation, include state symbols
2. Split up any ionic solutions into separate positive and negative ions
3. Cross out any spectator ions (ions that appear on both sides of the equation)
4. Write the ionic equation by copying out the remaining substances
