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A level chemistry > module 2- foundations in chemistry > Flashcards

module 2- foundations in chemistry Flashcards

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1
Q

heavy water

A

contains two atoms of the 2^H [D] isotope

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2
Q

heavy water bp

A

101.40

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3
Q

heavy water mp

A

3.80

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4
Q

heavy water density

A

1.11

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5
Q

water bp

A

100.00

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6
Q

water mp

A

0.00

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7
Q

water density

A

1.00

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8
Q

group 1 (ion charge )

A

1+

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9
Q

group 2 (ion charge )

A

2+

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10
Q

group 5 (ion charge )

A

3-

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11
Q

group 6 (ion charge )

A

2-

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12
Q

group 7 (ion charge )

A

1-

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13
Q

ion group exceptions

A

Ag+, Zn2+

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14
Q

cation

A

positive ion

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15
Q

anion

A

negative ion

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16
Q

oil rig

A

oxidation is loss, reduction is gain [of electrons]

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17
Q

mass defect

A

the strong forces holding neutrons and electrons comes at the expense of the loss of mass {mass is lost to hold nucleus}

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18
Q

standard isotope

A

base all atomic masses on - carbon 12

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19
Q

mass spectrometer finds

A

the percentage abundances of in a sample of an element

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20
Q

mass spec method

A

sample is vaporised/ ionised to get positive ions, the ions are accelerated. heavier ions move slower and are harder to deflect so they are separated, depicted as mass to charge ratio. each ion reading adds to signal, greater abundance = greater signal

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21
Q

mass spec equation

A

mass/charge of ion

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22
Q

for an ion with one positive charge- m/z ratio

A

ratio is equivalent to the relative isotopic mass

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23
Q

metals on the left side of the periodic table (electrons )

A

lose electrons, to form cations

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24
Q

non- metals on the right side of the periodic table (electrons)

A

gain electrons, to form anions

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25
Q

binary compound

A

2 elements

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26
Q

poly atomic

A

ion may contain atoms of more than one element

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27
Q

ammonium (molecular formula )

A

NH4

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28
Q

ammonium (ion charge)

A

1+

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29
Q

hydroxide (mf)

A

OH

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30
Q

hydroxide (ion charge )

A

1-

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31
Q

nitrate (mf)

A

NO3

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32
Q

nitrate (ion)

A

1-

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33
Q

nitrite (mf)

A

NO2

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34
Q

nitrite (ion charge )

A

1-

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35
Q

hydrogen carbonate (ion)

A

1-

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36
Q

hydrogen carbonate (mf)

A

HCO3

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37
Q

mangante [VII] (mf)

A

Mno4

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38
Q

mangante [VII] (ion)

A

1-

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39
Q

carbonate (mf)

A

CO3

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40
Q

carbonate (ion)

A

2-

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41
Q

sulfate (mf)

A

SO4

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42
Q

sulfate (ion)

A

2-

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43
Q

sulfite (mf)

A

SO3

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44
Q

sulfite (ion)

A

2-

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45
Q

dichromate (mf)

A

Cr207

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46
Q

dichromate (ion)

A

2-

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47
Q

phosphate (mf)

A

PO4

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48
Q

phosphate (ion)

A

3-

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49
Q

molecular formula - (brackets)

A

poly atomic

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50
Q

molecular formula is (charge )

A

neutral, the charges cancels out

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51
Q

diatomic molecule

A

2 atoms bonded together

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52
Q

state symbols

A

(g) = gas
(s) = solid
(l) = liquid
(aq) = aqueous - dissolved in water

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53
Q

examples of diatomic molecules

A

H2,N2,O2,F2,Cl2,Br2,l2

54
Q

do covalent bonds have ions

A

do not

55
Q

amount (n)

A

particles measured in the units moles

56
Q

one mole [avogradros constant ]

A

6.02 x 10^23

57
Q

one mole is equal to

A

the number of atoms in carbon 12

58
Q

mass of one mole is equal to

A

atomic mass

59
Q

molecular mass (m)

A

mass in grams of each mol in a substance /g mol -1

60
Q

amount equation

A

amount = mass/molar mass

61
Q

molecular formula

A

number of atoms of each elements in a formula

62
Q

empirical formula

A

simplest ratio

63
Q

Mr

A

add the ram/ compared to carbon 12 molecular mass

64
Q

workout relative formula mass

A

add ram in emp formula

65
Q

hydrated salts

A

water molecules are apart of the crystalline structure- water of crystallisation, shown as dot between compound and water

66
Q

hydrated copper (II) sulfate [blue] is heated

A

is heated, the bond holding the water is broken, the water is evaporated, making white anhydrous copper sulfate- without water the crystalline structure is lost

67
Q

method- hydrated salt

A

Weigh an empty crucible
Add hydrated salt and weigh
Heat over bunsen burner until it turns white, using a tripod and a pipe - clay triangle - about 4 mins
Cool then weigh the anhydrous salt
Experimental formula - assumptions - all water is lost, no further decomposition

68
Q

cm =

A

ml

69
Q

dm=

A

1000cm= 1 litre

70
Q

concentration of solution

A

is the amount of solute in moles, dissolved in 1dm^3

71
Q

standard solution

A

solution of known concentration

72
Q

n=cxv

A

amount = conc x volume

73
Q

molar gas volume

A

is the volume per mole of gas molecules, at stated temperature and pressure

74
Q

room temperature and pressure (rtp)

A

20 degrees Celsius and 101 kpa

75
Q

at rtp, 1 mol of gas molecules have a volume of

A

24.0 dm^3 = 24000cm^3

76
Q

amount of mol =equation

A

volume/molar gas volume

77
Q

ideal gas assumptions for the molecules

A

random motion/elastic collisions/negligible size/no inter molecular forces

78
Q

pv = nrt

A

pressure x volume = amount x r x temperature

79
Q

ideal gas constant (r) for water

A

8.314 j mol-1 k-1

80
Q

cm^3 to m^3

A

x 10^-6

81
Q

dm^3 to cm^3

A

x 10^-3

82
Q

c to k

A

+ 273

83
Q

Kpa to pa

A

x10^3

84
Q

percentage yield

A

actual/theoretical x100

85
Q

limiting reagent

A

not in excess, used first and stops the reaction

86
Q

atom economy

A

based on balanced equation and assumes 100% yield

87
Q

high atom economy

A

Produce a large amount proportion of desired product and few unwanted waste products
Are important for sustainability as they make the best use of natural resources, better for environment

88
Q

atom economy equation

A

sum desired/ total sum x 100

89
Q

finding relative molecular mass-practical

A

Add sample of volatile liquid to a small syringe via a needle, weigh the small syringe
Inject the sample into a gas syringe through the self sealing rubber cap, reweigh the small syringe to find the mass of the volatile liuid ]
Place in a boiling water bath at 100 degrees, the liquid vaporises producing a gas , the pressure is recorded

90
Q

stoichiometry

A

balancing numbers give ratio of atoms in moles, of each substance

91
Q

identifying an unknown metal

A
92
Q

acid releases

A

H+

93
Q

alkali releases

A

OH-

94
Q

what is an acid

A

releases H+ ions when dissolved

95
Q

+ aq

A

excess of water

96
Q

hydrochloric acid

A

HCL

97
Q

sulfuric acid

A

H2SO4

98
Q

nitric acid

A

HNO3

99
Q

ethanoic acid (vinegar)

A

CH3COOH

100
Q

metal carbonates examples

A

Na2CO3, CaCO3, CuCO3

101
Q

metal oxides

A

MgO, CaO, CuO

102
Q

alkalis

A

NaOH, KOH, NH3

103
Q

strong acids [dissociation ]

A

completely dissociates, releases all h atoms into soloution as h+ ioms

104
Q

weak acids [dissociation ]

A

partially dissociates, only releases a small proportion of h+ ions

105
Q

bases

A

metal oxides, metal hydroxides, metal carbonates and ammonia are all bases

106
Q

base + acid –>

A

neutralises and forms a salt

107
Q

what is an alkali

A

releases OH- ions into solution

108
Q

carbonates + acid

A

salt + water + co2

109
Q

dissociation in sulphuric acid

A

Sulfuric acid H2SO4 is a strong acid but this is true for only one of the 2 hydrogen atoms, when sulfuric is mixed with water each H2SO4 molecule dissociates releasing just one of its two

110
Q

dissociation in sulphuric acid equations

A

hydrogen atoms, as an H+ ion :
H2SO4 (aq) → H+ (aq)+ HSO4- (aq)
The resulting hso4- (aq) ions then only partially dissociate
HSO4- (aq) ⇌ H+ (aq) + SO4 2- (aq)

111
Q

hydrochloric acid formula

A

HCl

112
Q

sulphuric acid formula

A

H2SO4

113
Q

nitric acid formual

A

HNO3

114
Q

ethanoic acid (vinega)

A

CH3COOH

115
Q

HCl forms

A

chlorides

116
Q

H2SO4 forms

A

sulfates

117
Q

HNO3

A

nitrates

118
Q

CH3COOH

A

ethanoate

119
Q

sodium chloride (f)

A

NaCl

120
Q

sodium sulfate

A

Na2SO4

121
Q

calcium nitrate

A

Ca(NO3)2

122
Q

ammonium ethanoate

A

CH3CO2NH4

123
Q

titrations

A

technique to accurately measure the volume of one solution that reacts exactly with another solution

124
Q

titration uses

A

1) find the concentrations of a solution
2) identification of unknown substances
3) purity of a substance

125
Q

impurities can cause ….

A

harm eg. in medication

126
Q

preparing a standard soloutionn- equipment

A

a volumetric flask is used to make up a standard solution accurately

127
Q

standard solution

A

a solution of a known concentration

128
Q

preparing a standard solution - method

A

1)The solid is first weighed accurately

2)The solid is dissolved in a beaker using less distilled water than will be needed to fill the volumetric flask.

3)The last traces of solution are rinsed into the solution with more distilled water

4) the flask is then carefully filled to the graduation line by adding distilled water a drop at a time until the bottom of the meniscus is lines up exactly with the mark. Care at this stage is essential - if too much water is added the solution will be to dilute and must be prepared again

5) the volumetric flask is slowly inverted several times to mix the solution thoroughly, makes consistent results

129
Q

acid base titrations

A

The solution of an acid is titrated against a solution of a base using a pipette and burette

130
Q

manufactured certainties - pipette and Burette

A

10cm3 pipette +- 0.04cm3
25cm3 pipette +_- 0.06cm3
50cm3 buirette +- 0.10 cm3

131
Q
A

A level chemistry (13 decks)

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