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BMAT > Chemistry - chemical reactions, formulae, equations > Flashcards

Chemistry - chemical reactions, formulae, equations Flashcards

1
Q

conservation of mass

A

mass at start of reaction = mass at end of reaction

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2
Q

formulae for bromine

A

Br2

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3
Q

formula for buckminsterfullerene

A

C60

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4
Q

formula for chlorine

A

Cl2

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5
Q

formula for fluorine

A

F2

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6
Q

formula for hydrogen

A

H2

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7
Q

formula for iodine

A

I2

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8
Q

formula for nitrogen

A

N2

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9
Q

formula for oxygen

A

O2

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10
Q

formula for ammonia

A

NH3

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11
Q

formula for carbon dioxide

A

CO2

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12
Q

formula for carbon monoxide

A

CO

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13
Q

formula for methane

A

CH4

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14
Q

formula for nitrogen dioxide

A

NO2

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15
Q

formula for nitrogen monoxide

A

NO

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16
Q

formula for sulfur dioxide

A

SO2

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17
Q

formula for sulfur trioxide

A

SO3

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18
Q

formula for water

A

H2O

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19
Q

formula for lithium ion

A

Li+

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20
Q

formula for sodium ion

A

Na+

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21
Q

formula for potassium ion

A

K+

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22
Q

formula for magnesium ion

A

Mg 2+

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23
Q

formula for calcium ion

A

Ca 2+

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24
Q

formula for barium ion

A

Ba 2+

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25
Q

formula for aluminium ion

A

Al 3+

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26
Q

formula for ammonium ion

A

NH4 +

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27
Q

formula for copper II ion

28
Q

formula for hydrogen ion

29
Q

formula for iron II ion

30
Q

formula for iron III ion

31
Q

formula for silver ion

32
Q

formula for zinc ion

33
Q

formula for oxide ion

34
Q

formula for sulfide ion

35
Q

formula for fluoride ion

36
Q

formula for chloride ion

37
Q

formula for bromide ion

38
Q

formula for iodide ion

39
Q

formula for carbonate ion

40
Q

formula for hydroxide ion

41
Q

formula for nitrate ion

42
Q

formula for sulfate ion

43
Q

formula for hydrochloric acid

44
Q

formula for nitric acid

45
Q

formula for sulfuric acid

46
Q

formula for ethanoic acid

47
Q

soluble ions

A

K +
NH4 +
Na +
C -
B-
I-
F-
NO3 -
SO4 2-

48
Q

soluble ions: exceptions

A

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
Q

insoluble ions (and exceptions)

A

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
Q

ionic equations

A

only include species which have changed state

51
Q

neutralisation reaction of H+ and OH-

A

H+ (aq) + OH- (aq) –> H2O (l)

52
Q

ammonia reactions

A

H+ (aq) + NH3 (aq) –> NH4 + (aq)

53
Q

reactions with metals

A

2H+ (aq) + Mg (s) –> Mg 2+ (aq) + H2 (g)

54
Q

what is precipitation reactions

A

forming solids from aqueous species

55
Q

half equations

A

for displacement or electrolysis reactions

56
Q

equilibrium

A
  • reversible reactions in a closed system will reach equilibria
  • forward reaction is at same rate as backward reaction
57
Q

dynamic equilibrium

A

forward and backward reactions are occurring at same rate there is no overall effect, the number of reactants and products stay constant

58
Q

changing equilibrium position

A

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
Q

factors affecting equilibrium

A
  • concentration of reactants / products
  • pressure of gaseous reactants / products
  • temperature
60
Q

what happens to equilibrium when concentration of reactant increases

A
  • 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
Q

what happens to equilibrium when increasing concentration of products?

A
  • 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
Q

what happens to equilibrium when increasing the pressure of system (only affects gases)

A

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
Q

what happens to equilibrium if you decrease the pressure of system (only affects gases)

A

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
Q

what happens to equilibrium if you increase temperature

A

shifts to direction of endothermic reaction

65
Q

what happens to equilibrium if you decrease temperature

A

equilibrium position favours exothermic reaction

66
Q

what impact do catalysts have on equilibrium

BMAT (33 decks)

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