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chemistry test Flashcards

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1
Q

plum pudding model

A

sphere of positiv charge with small negative charges disrtibuted evently within it

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2
Q

rutherfords electron shell model

A

small dense central nucleus surrounded by orbiting electrons
nucleus = protons and neutrons giving overall pos charge

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3
Q

maximum number of orbiting elsesctons in a single shell

A

2n2

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4
Q

mass number

A

represented using a
protons and nuetrons

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5
Q

atomic number

A

z
number of protons in the atom

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6
Q

Ar

A

the mean mass of an atom of an element divided by one twelfth of the mean mass of an atom of the carbon 12 isotppe

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7
Q

isotope

A

atoms of the same elemtn with the same atomic number but diff neutron numbets resulting in diff mass number

react chemicaly in the same way as electron config is the same

diff mass number= diff physucal properties

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8
Q

ions

A

formed when an atom loses or gains electrons mesning it is no longer neutral and will have an overall charge

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9
Q

what is mass spectrometyr

A

this is an analytical techniques used to identify different isotpes and find the overall relatve atmic mass of an element

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10
Q

TOF steps

A

ionsiation
acceleration
ion drift
detection
analysis

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11
Q

ionisation

A

vapourised injected into mass spectrometer
high vltage
electron removed
+1 ion

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12
Q

acceleration

A

pod charged ions accelrated to neg charged detection plate

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13
Q

io drift

A

magnetic field deflects

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14
Q

detection

A

ion hits neg charged plate gain electron proudcong flow charge
greater abundance greater currwnt produce as they are propotional

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15
Q

analysis

A

flightimes to produce a spectra print out with relative abundance of eavh isotopes displayed

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16
Q

ar from spectra

A

m/z x abundance/ total abundance

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17
Q

orbitals

A

electeons are held in clouds of negative chsrge called orbitals
s p d f

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18
Q

s orbital shape

A

spherical

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19
Q

p orbital shape

A

dumbbell

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20
Q

d orbital

A

clover

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21
Q

electrons in s

A

2

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22
Q

electrons in p

A

6

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23
Q

electrons in d

A

10

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24
Q

spin

A

electrons pair up with opp spin so atom is as stavle
electrons same orbital opposite spin

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25
Q

ionisation energy

A

the minimum energy required to remove one mole of electrons from one mole of atoms in gaseous state

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26
Q

sucesseive ionisation energy

A

occurs when further elecons are removed
requires more energy because as electrons removed electrostatic forces of attraction between pos nucleus amd outer electron inc
more energy needed to overocme lo

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27
Q

ionisation energy along a period

A

increases due to decreasing atomic radius and greater electrostatic forces of attraction

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28
Q

ionisation energy down a group

A

firstnionisation energy decreases due to an increasing atomic radius and shielidng which reduces the effect of the electrostatic forces of attaraction

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29
Q

first ionisation of aluminium

A

lower than expected
single psir of electrons with opposite spin
natural repulsion
reduces amount of energy needed to be put to remove eletron

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30
Q

atomic radius a long a period

A

decreases
increased nc
outer electrons pulled in closer
greater attraction
more shells more shielding
nucleur attraction reduced

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31
Q

ionisation energy along a period

A

increases
decreasing atomic radius
inc nc
outershelll celectrons held more strongly and therefroew more energy required to remove them

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32
Q

ionisation energy downa group

A

decreases
nuclaur attraction between nucleus and outer slectron reduces
inc cheilding
less energy needed to remove

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33
Q

melting points in group 3

A

sod mag al -metallic bonding
mp inc due to pos charged ions
attractive forces increase from Na to Al

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34
Q

sillicon

A

macromolecuslr
stong covslrnt strucutre
lots
more energy do over come

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35
Q

phopshorus sulfur chlorine

A

simple covslnt
weak van der waals
dont require much energy to overcome
low similar mps

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36
Q

why argon is a gas at room temp

A

full outershell
stable
weak vdw
low mp
exists as gas at rtp

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37
Q

ionic bonding

A

metal and non
electron from metal to non
creates ions
oppositely charged afftravt thrpugh electrostatic forces to for, a giant ionic lattice

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38
Q

covalent bonding

A

two non metals
electrons shared

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39
Q

dative covalent bond

A

both electrons in the shared pair are supplied from a single atom
inducated using an arrow from lone pair

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40
Q

metallic bond

A

lattice of posotfily charged ions surrounded by sea delocalised electrons
strong forces of elecrtostatic attraction
larger ion larger radius weaker attraction

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41
Q

ionic properties

A

high mp and bp
lots energy needed to overvome electrostatic forces in alttice
moletn or aq sol conduct ekectricity
free moving ions
brittle

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42
Q

metallic properties

A

confuctors
sea
carry flow of charge
malleable
slide layers
solid at room temp

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43
Q

macromolcue properties

A

covalently bonded giant lattice
multiple covsneltn bofs
high mp
strong covalent latticr so rigid
diamond
bonded to four other carbon atoms

graphite
3 other carbons
flat sheets
free electrons
move betwen layers
conduct electricity

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44
Q

simple molecule

A

eg.iodine
covalnetly bonded
weak vdw
low mp and bp
poor cnducotrs

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45
Q

lone pair repulsion

A

additional repulsive forces changes bond angle reduced by 2.5

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46
Q

linear
bonding pairs
lone pairs
bond angle

A

2
0
180

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47
Q

v shaped
bonding pairs
lone pairs
bond angles

A

2
2
104.5

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48
Q

trigonal planar
bonding pairs]
lone pairs
bond angles

A

3
0
120

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49
Q

triagnular pyramid
bonding pairs
lone pairs
bond angles

A

3
1
107

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50
Q

tetrahedral bonding pairs
lone pairsn
bond angles

A

4
0
109.5

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51
Q

trigonal bipyramid
bonding pairs
lone pair
bond angles

A

5
0
90 and 120

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52
Q

octahedral
bonding pairs
lone pairs
bonf angles

A

6
0
90

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53
Q

electronegatvitiy

A

the power of an atom to attract negative charge towards itself in a covalent bond

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54
Q

permanant dipole

A

two atoms with diff electronegativities polar bond formed
more electroneg atom draws more neg charge towards itself away from other atom

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55
Q

induced dipole

A

when electron orbitalare influenced by another charged particles

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56
Q

vdw

A

weakest
induced dipole between molecules
larger mr stronger imf
straight chains stronger cdw pack closely together

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57
Q

permanant dipole

A

polar bond
attarct eachither
alltice structure

58
Q

hyrodgen bonding

A

fon
lone pair on these atoms forma. bond with a hydorgen atomfrom another molecule shown witha dotted line
high mp and bp

59
Q

The size of the first ionisation energy is affected by four factors:

A

Size of the nuclear charge
Distance of outer electrons from the nucleus
Shielding effect of inner electrons
Spin-pair repulsion

60
Q

between beryllium and boron

A

fifth electron in boron is in the 2p subshell, which is further away from the nucleus than the 2s subshell of beryllium
Beryllium has a first ionisation energy of 900 kJ mol-1 as its electron configuration is 1s2 2s2
Boron has a first ionisation energy of 800 kJ mol-1 as its electron configuration is 1s2 2s2 2px1

61
Q

between nitrogen and oxygen

A

decrease in IE1
spin-pair repulsion in the 2px orbital of oxygen
Nitrogen has a first ionisation energy of 1400 kJ mol-1 as its electron configuration is 1s2 2s2 2px1 2py1 2pz1
Oxygen has a first ionisation energy of 1310 kJ mol-1 as its electron configuration is 1s2 2s2 2px2 2py1 2pz1
In oxygen, there are 2 electrons in the 2px orbital, so the repulsion between those electrons makes it slightly easier for one of those electrons to be removed

62
Q

The successive ionisation energies of an element increas

A

As more electrons are removed, the attractive forces increase due to decreasing shielding and an increase in the proton to electron ratio

63
Q

oxides from period 3 elements

A

sodium oxide
magnesium oxides
aluminium oxides
sillicon dioxide
phopshopurs oxide
sulfur dioxide
sulfur trioxide

64
Q

sodium oxide oxidsiton state

A

1

65
Q

magneisum oxide oxidation state

A

2

66
Q

alumiunm oxide oxidation state

A

3

67
Q

sillicon dioxide oxidation statae

A

4

68
Q

sulfur trioxide oxidation state

A

6

69
Q

na2o structure and bonding and reactivity

A

ionic
vigorous

70
Q

mgo structure and reactivity

A

ionic
vigorous

71
Q

Al2o3

A

ionic
slow

72
Q

sio2

A

macromolecular
slow

73
Q

p4o10

A

simple covalent
vigorous

74
Q

so2 structure and ractivity

A

simple covalent
burns steadily

75
Q

period 3 and water

A

form alkaline solutions
10-14 ph
simple ocvalent oxides of sulfur and phosphorus combines with water to form acidic solutions witha ph around 0-2
when in solution these acids dissociate into h+ ions and ions of conjugate base

76
Q

acid base reaction

A

ionic oxides react with acid to produce salt and water
neutralisation

acid covalent oxides react with bases to produce a salt and water in a neutralsiation

77
Q

alumiunm oxide group 3 oxides

A

partially ionic and covalent
insoluble in water
ions dont dissociate
acts as an acid and base
amphoteric
produce salt and water in neutralisation reactions

78
Q

sodium vs mag

A

Both have high melting points, but magnesium has a higher melting point than sodium
This is because of the 2+ charge of magnesium, meaning that it is has a higher charge density

Both are silvery metals
Sodium is quite a soft, silvery metal which tarnishes quickly in air
Magnesium is harder than sodium and you will often see it as magnesium ribbon

79
Q

mag and water

A

extremely slow reaction - only a very small number of bubbles
magnesium hydroxide formed will have a pH of around 10 - it is less alkaline than sodium hydroxide because magnesium hydroxide is only partially soluble

80
Q

Sodium with cold water:

A

vigorous, exothermic
sodium floats on the surface of the water fizzing rapidly and melting as a result of the heat produced
colourless sodium hydroxide
13-14,

81
Q

Heated magnesium with steam:

A

faster than with cold wate
burns with a bright, white flame
magnesium oxide is produced

82
Q

na and oxygen

A

heated
vigorous
bright yellow flame
white solid

83
Q

mg and oxygen

A

heated
heated
vigorously
bright white flame
white solid

84
Q

al and oxygen

A

powdered al
fast
bright white flame
white powder

85
Q

si and oxygen

A

powdered si and heat
slowly
bright white sparkles
white powder

86
Q

p and oxygen

A

heated
heated
vigorous
yellow or white flame
white clouds

87
Q

s and oxygen

A

powdered s heated
gently
blue flame
tpxic fumes

88
Q

how sulfer tripxide is made

A

catalyst must be used and the reaction must take place at a very high temperature
The equation for this reaction is:
2S (s) + 3O2 (g) → 2SO3 (g)

88
Q

Ionic Oxides

A

Sodium oxide
Magnesium oxide
Aluminium oxide
These are ionic oxides because the bonding exists between metals and non metals
They have giant lattice structures and thus, high melting points

89
Q

Giant Covalent Oxides

A

Silicon dioxide
This is covalent because both silicon and oxygen are non metals
The millions of covalent bonds within this giant structure are extremely strong, and thus it has a high melting point
Giant covalent structures can also be called macromolecules or giant molecules

90
Q

Simple Covalent Oxides

A

Phosphorus(V) oxide
Sulfur dioxide
Sulfur trioxide
small molecules with only weak intermolecular forces of attraction between them

91
Q

why so3 has hgher m point

A

has a slightly higher melting point than sulfur dioxide, SO2, because of the increase in intermolecular forces between the slightly larger SO3 molecules

92
Q

na properties

A

solid
high mp
good condcutor
giant ionic
reacts and forms hydroxide ions in sol
13 ph

93
Q

mg properties

A

solid
high mp
good conductor
giant ionic
wlightly soluble dsissolved oxide forms a few hydroxide ions
8 ph

94
Q

al properties

A

solid
high mp
good conductor
giant ionic
sinoluble but amphoteric
7 ph

95
Q

si peoperties

A

solid
very high mp
no conductor
giant
insoluble but acidic
7 ph

96
Q

p properties

A

solid
low mp
not conductive
simple
acidic reacts and h+ in sol
2 ph

97
Q

so2 peoperties

A

gas
low mp
not conductor
simple
acidic h2so4 few h+ in sol
3 ph

98
Q

so3 properties

A

liquid
not conducotr
simple molecule
acidci reacts and forms h2so4
with h+ ions in sol
1 ph

99
Q

metal oxides and water

A

Sodium oxide, Na2O, and magnesium oxide, MgO, are made up of ions
They contain an oxide ion, O2-, which is a strong base and will readily produce hydroxide ions through reaction with water
This is why the solutions formed are strongly alkaline
Sodium oxide forms a more alkaline solution than magnesium oxide because it is far more soluble in water

100
Q

Non-metal oxides

A

Oxides of phosphorus and sulfur are simple covalent molecules
They will react with water to produce acidic solutions

101
Q

use of mgo

A

indeigstion tablers
neutralising excess acids in stomach

102
Q

Al2O3

A

Reacts with hot, concentrated alkali to form a salt

103
Q

SiO2

A

Reacts with hot, concentrated alkali to form a salt and water

104
Q

aluminium oxide

A

mphotenic
Ionic but also partially covalent
Small Electronegativity difference between al and o
Also al is a small ion with high charge so it can get close to the oxide ion and distorts the oxide charge cloud
Alumium metal is protected from corrosion in moist air by a thin layer of Al2o3
Insolubility in water impermeable to air and water
Ionic but binding is too strong to seperste ions

105
Q

collision theory

A

must have energy greater than or equal to the activation energy and correct particle orientation

106
Q

inc temp conc and pressure or maxwell disritubution

A

shifts ro the right

107
Q

effect of catalysts of maxwell disrtubtion

A

shifts to thr left no change on shape

108
Q

dynamic equillibrium

A

forward reaction rate is same and remains constant rate to bakcward
closed systems

109
Q

le chatellier

A

when a system is subject to change the system will alter to lessen the effect of that change
maximise yield

110
Q

increasing temp

A

favours endo
inc yield of endo products

111
Q

increasing pressures

A

favours side w fewer moles

112
Q

increasing conc

A

favour the reaction that produces the products

113
Q

hyrodgen oxidation state

A

+1

114
Q

oxygen oxidation stte

A

-2

115
Q

ha;ogens oxidation state

A

-1

116
Q

group 1 metals pxidation state

A

+1

117
Q

group 2 atomic radius

A

increases due to inc shells

118
Q

reactivity in group 2

A

increases
inc shielding

119
Q

ionisation energy

A

decreases
greater radius
greater sheilding

120
Q

group 2 melting point

A

metallic so larger the ions weaker the attractive fordes over greater distance so decrases

121
Q

group 2 and water

A

metal hydroxude and hydrogen
alkaline solution

mag reaction reacts very slowly
faster w steam bright whitw flame and powder

122
Q

solubility of hydroxides

A

increases down the group
mag hydroxide least soluble
barium hyrdoxide most soluble
mag hydroxide antaxid alaline neitslise acids

123
Q

solubility of sulfates

A

decreases
mag most
bar least

barium sulfate used in med
medical tracer
toic if enetr blood stream but insoluble so cannot be abosrbed into blood

124
Q

metal extraction

A

magnesium
from titanium chloride via dsiplacement

125
Q

flue gas removal

A

calcium oxide and sulfer dioxide
forms calcium sulfite and water

126
Q

atomic radius in group 7

A

increase
more shlls

127
Q

reactivity in group 7

A

dercreases
additional shielding
atomic radius inc

128
Q

ionisation energy in group 7

A

decreases

129
Q

bpiling point in group 7s

A

simple covalnt bonds
vdw
strength inc
higher bp

130
Q

oxidising power in group7

A

good oxidisng agents
decreases down goup

131
Q

silver nitratr

A

anoin halides testes using acified silver nitrat
acidified to remove other impurities that cpuld form a ppt removed

132
Q

agno3 with cl br i

A

white ppt
cream ppt
yellow ppt

133
Q

dilute nhs3 with cl- br- i-

A

ppt dissolves
no change
no change

134
Q

conc nh3 with cl- br- i-

A

ppt dissolves
dissolves
no chnage

135
Q

sulfate - anioins

A

bacl2
white ppts

136
Q

hydroxide anions on litmus paper

A

red limus ruen blue

137
Q

carbonate anions

A

hcl fizz co2
bubbles through limewater
cloudy

138
Q

calcium
strontium
barium
flames

A

brick red
red
green

139
Q

ammonium ions

A

redd litmus
blue

chem (34 decks)

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