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Chemistry unit 1 > unit 1.1 - formulae and equations > Flashcards

unit 1.1 - formulae and equations Flashcards

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1
Q

Common compounds

A
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2
Q

Water?

A

H2O

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3
Q

Carbon dioxide?

A

C02

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4
Q

Sulfur dioxide?

A

SO2

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5
Q

Methane?

A

CH4

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6
Q

Hydrochloric acid?

A

HCL

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7
Q

Sulphuric acid?

A

H2SO4

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8
Q

Nitric acid?

A

HNO3

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9
Q

Ethanoic acid?

A

CH3CO2H

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10
Q

Ammonia

A

NH3

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11
Q

Ammonium chloride?

A

NH4CL

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12
Q

Sodium hydroxide?

A

NAOH

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13
Q

Sodium chloride

A

Nacl

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14
Q

Sodium carbonate

A

NA2CO3

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15
Q

sodium hydrogencarbonate

A

NAHCO3

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16
Q

sodium sulfate

A

Na2SO4

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17
Q

copper oxide

A

CUO

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18
Q

Copper sulfate

A

CUSO4

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19
Q

Calcium hydroxide

A

Ca(OH)2

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20
Q

Calcium carbonate

A

CaCO3

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21
Q

Calcium carbonate

A

CaCO3

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22
Q

Calcium chloride

A

CaCL2

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23
Q

Formulae of common ions

A

those in groups 1, 2 , 6 and 7

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24
Q

Ammonium

A

NH4+

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25
Q

Hydrogen

A

H+

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26
Q

Lithium

A

LI+

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27
Q

Potassium

A

K+

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28
Q

Sodium

A

Na+

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29
Q

Silver

A

Ag+

30
Q

Barium

A

Ba2+

31
Q

Calcium

A

Ca2+

32
Q

Magnesium

A

Mg2+

33
Q

Copper(11)

A

Cu2+

34
Q

Iron(11)

A

Fe2+

35
Q

Iron(111)

A

Fe3+

36
Q

Aluminium

A

Al3+

37
Q

Bromide

A

Br-

38
Q

Chloride

A

Cl-

39
Q

Flouride

A

F-

40
Q

Iodide

A

I-

41
Q

Hydrogencarbonate

A

HC03-

42
Q

Hydroxide

A

OH-

43
Q

Nitrate

A

N03-

44
Q

Oxide

A

O2-

45
Q

Sulfide

A

S2-

46
Q

Carbonate

A

CO32-

47
Q

Sulfate

A

SO42-

48
Q

Phosphate

A

PO43-

49
Q

Nitride

A

N3-

50
Q

what is the definition of oxidation number?

A

the number given to an atom in a molecule or an ion based on the number of electrons this atom uses in chemical bonding

51
Q

what are oxidation numbers used for?

A

the number of electrons that need to be added (or taken away
from) an element to make it neutral.

52
Q

for example?

A

calcium ion, Ca2+ needs two electrons added to it in order to make a neutral
calcium atom. Its oxidation number is therefore +2 (add 2 electrons). A sulphide ion,
S2-, needs to lose two electrons in order to make a neutral sulfur atom. Its oxidation
number is therefore -2 (take 2 electrons away).

53
Q

for example?

A

calcium ion, Ca2+ needs two electrons added to it in order to make a neutral
calcium atom. Its oxidation number is therefore +2 (add 2 electrons). A sulphide ion,
S2-, needs to lose two electrons in order to make a neutral sulfur atom. Its oxidation
number is therefore -2 (take 2 electrons away).

54
Q

oxidation rules

A
55
Q

rule number 1?

A

An uncombined element has an
oxidation number of zero

56
Q

rule number 2?

A

Group 1 elements in all compounds oxidation number = +1

57
Q

rule number 3?

A

Group 2 elements in all compounds the oxidation number =+2

58
Q

rule number 4?

A

Hydrogen in most compounds oxidation number is +1

59
Q

rule number 5?

A

Oxygen is most compounds oxidation number is -2

60
Q

rule number 6?

A

the sum of oxidation number of a compound must = 0

61
Q

rule number 7?

A

the sum of the oxidation number of a compound must = 0

62
Q

rule number 8?

A

the halide ions oxidation number in an ionic compounds equal -1 Br-1, cl -1

63
Q

Number line

A

oxidation - loss of electrons +
Reduction - gain of electrons -

64
Q

oxidation numbers practice

give the oxidation numbers for each atom

A
  • CO2 - (-2x2) = -4 so c has to be -4 to add up to 0
  • Cu20 - (-2) so cu has to be +2 so cu =+1
  • AlCl3 = cl = -1 x 3 = -3 so Al = +3
  • P4010 = P = -2x10 = 20 so P4 has to be +20 so p = 5
  • s04^2- = has to add up to -2 so -2x4 = -8 so s has to be +6
  • I2 = 0 uncombined element = 0
  • N03 - = has to add up to -1. O = -2 x3 = -6 N has to add up to +5
  • Mn04- has to add up to -1. O = -2 x 4 = -8. Mn = +7

stars represent italics which represent which represents which one i wa

65
Q

Ionic equations

A

written to sum up what happens in a chemical reaction using chemical formulae
a full complete equation can be converted into an ionic equation involves ionic compounds
when ions react with each other

66
Q

why are spectator ions omitted?

A

because they appear on both sides of the equation into equal amounts

67
Q

example of a neutralisation reaction

A

H2S04(aq) + 2NaOH(aq) ———– Na2SO4(aq) + 2H20(l)
2H+ + SO42 +2na+OH- ————- 2Na+ + S042- +2H20
2H+ 2OH- —— 2 H20
H+(aq) + OH-(aq) ——– H20(l)

68
Q

metal - acid questions

A

Mg(s) + 2HCl(aq) ———– MgCl2(aq) + H2(g)
Mg(s) +2H+ + 2Cl- ———Mg2+(aq) + 2Cl-(aq) +H2(g)
Mg(s) + 2H+(aq) ———— Mg2+(aq) +H2(g)

69
Q

Displacement questions

A

2KB(a q)r +Cl2(aq) ————- 2KCl(aq)+Br2(aq)
3K + 2Br- +Cl2 —————- 2K + 2Cl - +Br2
2Br-(aq) +Cl2(aq) ————–2Cl-(aq) + Br2(aq)

70
Q

ionic equations for example?

A

HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
H+(aq) + Cl- (aq) + Na+ (aq) + OH- (aq) → Na+ (aq) + Cl- (aq) + H2O (l)
H+ (aq) + OH- (aq) → H2O (l)

71
Q

note

A

state symbols have to be used in ionic equations. If you
look carefully at the state symbols for all of the ionic equations above, you will see
that: -
∙ The products are never aqueous – above you have a liquid and two solids.
∙ Spectator ions are the ones that remain in aqueous solution.

Chemistry unit 1 (4 decks)

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