Chemistry - chemical reactions, formulae, equations Flashcards
1
Q
conservation of mass
A
mass at start of reaction = mass at end of reaction
2
Q
formulae for bromine
A
Br2
3
Q
formula for buckminsterfullerene
A
C60
4
Q
formula for chlorine
A
Cl2
5
Q
formula for fluorine
A
F2
6
Q
formula for hydrogen
A
H2
7
Q
formula for iodine
A
I2
8
Q
formula for nitrogen
A
N2
9
Q
formula for oxygen
A
O2
10
Q
formula for ammonia
A
NH3
11
Q
formula for carbon dioxide
A
CO2
12
Q
formula for carbon monoxide
A
CO
13
Q
formula for methane
A
CH4
14
Q
formula for nitrogen dioxide
A
NO2
15
Q
formula for nitrogen monoxide
A
NO
16
Q
formula for sulfur dioxide
A
SO2
17
Q
formula for sulfur trioxide
A
SO3
18
Q
formula for water
A
H2O
19
Q
formula for lithium ion
A
Li+
20
Q
formula for sodium ion
A
Na+
21
Q
formula for potassium ion
A
K+
22
Q
formula for magnesium ion
A
Mg 2+
23
Q
formula for calcium ion
A
Ca 2+
24
Q
formula for barium ion
A
Ba 2+
25
formula for aluminium ion
Al 3+
26
formula for ammonium ion
NH4 +
27
formula for copper II ion
Cu 2+
28
formula for hydrogen ion
H+
29
formula for iron II ion
Fe 2+
30
formula for iron III ion
Fe 3+
31
formula for silver ion
Ag +
32
formula for zinc ion
Zn 2+
33
formula for oxide ion
O 2-
34
formula for sulfide ion
S 2-
35
formula for fluoride ion
F -
36
formula for chloride ion
Cl-
37
formula for bromide ion
Br -
38
formula for iodide ion
I -
39
formula for carbonate ion
CO3 2-
40
formula for hydroxide ion
OH-
41
formula for nitrate ion
NO3 -
42
formula for sulfate ion
SO4 2-
43
formula for hydrochloric acid
HCl
44
formula for nitric acid
HNO3
45
formula for sulfuric acid
H2SO4
46
formula for ethanoic acid
CH3COOH
47
soluble ions
K +
NH4 +
Na +
C -
B-
I-
F-
NO3 -
SO4 2-
48
soluble ions: exceptions
halides are soluble, except for halides of Ag +, Hg 2+, and Pb 2+
fluorides are soluble, except for fluorides of Mg 2+, Ca 2+, Sr 2+, Ba 2+, Pb 2+
sulfates are soluble, except for Sr 2+, Ba 2+, Pb 2+
49
insoluble ions (and exceptions)
carbonates (CO3 2-), exceptions are NH4 + salts, alkali metal salts
phosphate (PO4 3-), exceptions are NH4 + salts, alkali metal salts
metal hydroxides (OH-), exceptions are NH4 + salts, alkali metal salts
50
ionic equations
only include species which have changed state
51
neutralisation reaction of H+ and OH-
H+ (aq) + OH- (aq) --> H2O (l)
52
ammonia reactions
H+ (aq) + NH3 (aq) --> NH4 + (aq)
53
reactions with metals
2H+ (aq) + Mg (s) --> Mg 2+ (aq) + H2 (g)
54
what is precipitation reactions
forming solids from aqueous species
55
half equations
for displacement or electrolysis reactions
56
equilibrium
- reversible reactions in a closed system will reach equilibria
- forward reaction is at same rate as backward reaction
57
dynamic equilibrium
forward and backward reactions are occurring at same rate there is no overall effect, the number of reactants and products stay constant
58
changing equilibrium position
changing concentration, temperature and pressure of reversible reaction, the position of the equilibrium can be changed, it can be pushed either left or right
59
factors affecting equilibrium
- concentration of reactants / products
- pressure of gaseous reactants / products
- temperature
60
what happens to equilibrium when concentration of reactant increases
- increasing concentration of reactants cause equilibrium position to shift to right, so more products made
- equilibrium position tries to counteract the change and restore balance to the system
61
what happens to equilibrium when increasing concentration of products?
- equilibrium position shifts to the left so more reactants will be made
- equilibrium position tries to counteract the change and restore balance to the system
62
what happens to equilibrium when increasing the pressure of system (only affects gases)
when pressure increased, equilibrium position acts to counteract increase in pressure by decreasing pressure and moves to lower pressure which is the side with fewer gaseous molecules
63
what happens to equilibrium if you decrease the pressure of system (only affects gases)
pressure decreased, equilibrium position acts to counteract this decrease in pressure by increasing the pressure of the system and therefore moves to the side of greater pressure which is the side with a greater number of gaseous molecules
64
what happens to equilibrium if you increase temperature
shifts to direction of endothermic reaction
65
what happens to equilibrium if you decrease temperature
equilibrium position favours exothermic reaction
66
what impact do catalysts have on equilibrium
no effect
