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Chemistry > all of year 10 > Flashcards

all of year 10 Flashcards

1
Q

what are the different types of bonding

A
  • metallic
  • ionic (metal & non-metal)
  • covalent (non-metals)
  • giant covalent
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2
Q

define metalic bonding

A

eletrostation attraction between rows of metal cations and a sea of delocalised electrons

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3
Q

explain is metals are malleable or soft

A

malleable and ductile because the layers of cations can slide

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4
Q

define ionic bonding

A

eletrostatic attraction between positive metal and negative non-metal ions

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5
Q

are ionically bonded materials malleable or soft

A

brittle (hard but easy to break)

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6
Q

define covalent bonding

A

electrostatic attraction between the bonding pair of electrons and bonded nuclei with weak intermolecular forces between molecules

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7
Q

what is an alloy

A

a mixture of two or more elements one of which is a metal

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8
Q

why are alloys stronger than metals

A

because alloys have different sized atoms so the arrangement is more irregular so it is harder to bend / snap as the irregular atoms do not easily move over each other

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9
Q

describe the reactivity down group one

A

the get more reactive as you go down

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10
Q

how do group 1 elements react with air

A

they all instantly tarnish in air due to oxygen producing a white oxide

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11
Q

what is the name given to group one elements

A

alkali metals

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12
Q

describe how lithium reacts with water

A
  • moves on surface of water
  • fizzes
  • floats
  • squeaky pop with flame
  • universal indicator turns blue
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13
Q

describe how sodium reacts with water

A
  • moves on surface of water
  • fizzes
  • floats
  • squeaky pop with flame
  • universal indicator turns blue
  • melts into a ball
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14
Q

describe how potassium reacts with water

A
  • moves on surface of water
  • fizzes
  • floats
  • squeaky pop with flame
  • universal indicator turns blue
  • purple flame
  • melts into a ball
  • exploded
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15
Q

explain why group one metals get more reactive down the group

A
  • the outer electron is further away from the nucleus
  • there is less attraction = quicker transfer
  • the atos has more shells so the outer electron is more easily lost
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16
Q

what are the procucts of a group 1 element and water

A
  • metal hydroxide
  • hydrogen
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17
Q

what is the formula for hydroxide

A

OH -

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18
Q

what is the formula for nitrate

A

NO3 -

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19
Q

what is the formula for carbonate

A

CO3 2-

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20
Q

what is the formula for sulphate

A

SO4 2-

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21
Q

what is the formula for hyrdrochloric acid

A

HCl

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22
Q

what is the formula for sulfuric acid

A

H2SO4

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23
Q

what is the formula for nitric acid

A

HNO3

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24
Q

what is the name given to group 7 elements

A

halogens

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25
Q

what are the gases in group 7

A

fluorine and chlorine

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26
Q

what are the liquid(s) in group 7

A

bromine

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27
Q

what are the solid(s) in group 7

A

iodine

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28
Q

how many electrons do halogens have

A

7

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29
Q

explain the reactivity trend in group 7

A
  • less reactive down the group
  • more shells of electrons
  • outer shell electrons are less strongly attracted to the nucleus
  • it is harder to gain electrons
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30
Q

what colour is fluorine

A

pale yellow gas

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31
Q

what colour is chlorine

A

green gas

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32
Q

what colour is bromine

A

red-brown liquid

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33
Q

what colour is iodine

A

dark gray solid

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34
Q

describe displacement in the halogens

A

a more reactive halogen will displace a less reactive halogen from a solution of its compound

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35
Q

will chlorine displace bromine

A

yes

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36
Q

will bromine displace iodine

A

yes

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37
Q

will iodine displace chlorine

A

no

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38
Q

what is a redox reaction

A

when oxidation and reduction occur at the same time in a reaction

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39
Q

what is oxidation

A

when a substance gains oxygen or loses electrons

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40
Q

what is reduction

A

when a substance loses oxygen or gains electrons

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41
Q

what is the oxidising agent

A

the substance that is reduced (loses oxygen)

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42
Q

what is the reducing agent

A

the substance that is oxidised (gains oxygen)

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43
Q

define an acid

A

produces H+ when dissolved in water, they are proton donors

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44
Q

what pH do acidic soutions have

A

<7

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45
Q

define a base

A

can neutralise an acid; they are proton acceptors

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46
Q

define an alkali

A

a soluble producing OH- ions when disolved in water

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47
Q

what pH do alkali solutions have

A

> 7

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48
Q

when will an indicator not work

A

if the solution already has a colour

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49
Q

what is the alternative to an indicator

A

a pH meter

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50
Q

what are the indicators and their colour change from acid to alkali

A
  • litmus paper = red - blue
  • methyl orange = red - yellow
  • phenolphthalein = colourless - pink
  • universal = red - orange - green - blue - purple
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51
Q

what type of solutions will metal oxides form

A

alkaline

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52
Q

what type of solutions will non-metal oxides form

A

acidic

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53
Q

what is the difference between a base and an alkali

A

bases aren’t soluble in water, alkalis are soluble in water

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54
Q

what type of salt will be formed with hydrochloric acid

A

a chloride

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55
Q

what type of salt will be formed with sulfuric acid

A

a sulfate

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56
Q

what type of salt will be formed with nitric acid

A

a nitate

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57
Q

when are salts fromed

A

when an acid reacts

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58
Q

what are the products formed from a metal and an acid

A
  • salt
  • hydrogen
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59
Q

what are the products formed from a metal oxide and an acid

A
  • salt
  • water
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60
Q

what are the products formed from a metal carbonate and an acid

A
  • salt
  • carbon dioxide
  • water
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61
Q

what are the products formed from a metal hydroxide and an acid

A
  • salt
  • water
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62
Q

why don’t you react gorup 1 with acids

A

it is too dangerous

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63
Q

what are the two methods to form sulble salts

A
  • excess solid
  • titration
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64
Q

describe the excess solid method

A
  • heat the sulfuric acid
  • add balck copper oxide powder to excess and stir
  • filter out excess copper oxide
  • heat the blue copper sulfate solution until crystalisation point and leave to dry
  • filter out the crystals and wash with distilled water
  • leave to dry or dry between filter paper
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65
Q

describe a titration

A
  • pipette alkali solution into a cronicle flask
  • add a few drops of phenolphthalein indicator
  • put acid into the burette
  • acid is added to the alkali with swirling until the indicator changes colour from pink to colourless
  • record your burette volume and repeat until concordant results are achieved
  • repeat without indicator and heat till crystalisation etc for pure salt
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66
Q

what are concodant results

A

+ or - 0.1cm^2

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67
Q

how do you record a burette reading

A

with 2 decimal place

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68
Q

what is the equation fro neutrilisation

A

H+ (aq) + OH- (aq) -> H2O (l)

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69
Q

what is meant by the term precipitate

A

an insoluble salt made from two solutions

70
Q

are sodium salts soluble or insoluble

71
Q

are potassium salts soluble or insoluble

72
Q

are ammonium salts soluble or insoluble

73
Q

are nitrate salts soluble or insoluble

74
Q

are chloride salts soluble or insoluble

A

soluble except for silver chloride and lead chloride

75
Q

are sulfate salts soluble or insoluble

A

soluble except for lead, barium and calcium sulfate

76
Q

are carbonate salts soluble or insoluble

A

insoluble except for sodium, potassium and ammonium carbonate

77
Q

are hydroxide salts soluble or insoluble

A

insoluble excep for sodium, potassium and calcium hydroxide

78
Q

describe the method of making an insoluble salt

A
  • mix the two soluble salt solutions together
  • precipitate forms
  • filter out precipitate
  • wash with cold water
  • leave to dry in a warm oven
79
Q

what is the chemical test and result for hydrogen

A

lit split
= squeaky pop

80
Q

what is the chemical test and result for oxygen

A

glowing split
= relights

81
Q

what is the chemical test and result for carbon dioxide

A

add acid and bubble through lime water
= goes ‘cloudy white’

82
Q

what is the chemical test and result for chlorine gas

A

damp blue litmus paper
= may turn red then bleached white

83
Q

what is the chemical test and result for ammonia gas

A

damp red litmus paper
= turns blue

84
Q

what is the chemical test and result for water

A

white anhydrous copper sulfate
= turns blue

85
Q

how do you test for solid metal ions

A

carry out a flame test

86
Q

describe a flame test

A
  • dip a nichrome wire into an unreactive, colourless acid
  • dip it into ionic solid
  • put it in a roaring bunsen flame so the colour of flame will not interfere
87
Q

what colour flame will lithium produce

88
Q

what colour flame will sodium produce

89
Q

what colour flame will potassium produce

90
Q

what colour flame will calcium produce

A

red-orange

91
Q

what colour flame will copper produce

A

blue-green

92
Q

how do you test for metal ions in a solution

93
Q

what is the result of NaOH added to copper

A

blue precipitate

94
Q

what is the result of NaOH added to iron (II)

A

sludgy green precipitate

95
Q

what is the result of NaOH added to iron (III)

A

reddish brown precipitate

96
Q

how do you test for the halogen non-metal ions

A
  • add HNO3
  • add AgNO3
97
Q

what precipitate is formed from chloride

A

white precipitate

98
Q

what precipitate is formed from bromide

A

cream precipitate

99
Q

what precipitate is formed from iodine

A

yellow precipitate

100
Q

how do you test for sulphate non-metal ions and what is the result

A
  • add HCl
  • add BaCl2
    = white precipitate
101
Q

what are the rules when doing an ionic equation for a precipitate

A
  • write the formula of the precipitate on the right
  • write the ions that make it up on the left
  • balance and add state symbols
102
Q

what is the general formula of an alkane

103
Q

what is the general formula of an alkene

104
Q

what is the general fromula of an alcohol

105
Q

what is the meant by the term empricial formula

A

the simplest whole number ratio of atoms of each element in a compound

106
Q

what is the stem for a hydrocarbon with one carbon atom

107
Q

what is the stem for a hydrocarbon with two carbon atoms

108
Q

what is the stem for a hydrocarbon with three carbon atoms

109
Q

what is the stem for a hydrocarbon with four carbon atoms

110
Q

what is meant by the term hydrocarbon

A

a molecule made up of only carbon and hydrogen atoms

111
Q

what is meant by the term saturated

A

a molecule only containing single bonds between carbon atoms

112
Q

what is meant by the term unsaturated

A

a molecule containing carbon = carbon double bonds

113
Q

what is meant by the term isomer

A

molecule with the same molecular formula but different structual formulae

114
Q

what are the rules for drawing an isomer of a hydrocarbon

A
  • take one carbon off the long chain
  • re-bond that carbon to the orignal chain at least one carbon from the end
115
Q

what is crude oil

A

a mixture of molecules (mainly hydrocarbons)

116
Q

what is the process whihc spereates out crude oil

A

fractional distilation

117
Q

describe fractional distilation of crude oil

A
  • crude oil is heated up it vapourises
  • vapours ride up the column and condense at temperature just below their boiling point
  • they condense into different groups called fractions
  • they column is cooler at the top than the bottom
  • the larger molecules with higher boiling points condense at the bottom
118
Q

what are the products from fractional distilation from top of the column to the bottom

A
  • refinary gases
  • gasoline (petrol)
  • kerosene
  • diesel
  • fuel oil
  • bitumen
119
Q

what are the physical properties of the longer chain hydrocarbons

A
  • more viscous
  • more yellow/orange in colour
120
Q

why is catalytic cracking neccessary

A

because short-chain hydrocarbons are at higher demand as they are easily ignited so can be used for fuels but there is a greater supply of long-chain hydrocarbons

121
Q

what is catalystic cracking

A

the process of breaking down long-chain hydrocarbons into short-chain hydrocarbons

122
Q

what conditions are needed for catalytic cracking

A
  • 600-700 degrees celcius
  • catalyst
123
Q

what are the two options for a catalyst for catalytic cracking

A
  • alumina
  • silica
124
Q

what type of reaction is combustion

A

exothermic

125
Q

what are the two types of combustion

A
  • complete
  • incomplete
126
Q

what are the conditions and products for complete combustion

A
  • lots of O2
  • releases CO2 and H2O
127
Q

what are the conditions and products for incomplete combustion

A
  • limited O2
  • releases CO and H2O
128
Q

what is the apparatus for combustion

A

a u-tube with anydrous CuSO4

129
Q

what are the main pollutants from burning fuels and combustion

A
  • CO2 = greenhouse gas = global warming
  • CO = toxic = prevents blood carrying oxygen = death
  • NO, NO2 = acid rain
130
Q

are alkenes saturated or unsaturated

A

unsaturated

131
Q

when are alkene produced

A

when large hydrocarbon molecules are cracked into samller hydrocarbon molecules

132
Q

what are alkenes used to produce

133
Q

how can you distinguish between an alkane and alkene

A

by reacting it with bromine water

134
Q

how does an alkene react with bromine water

A

it rapidly decolourises from orange to colourless
- the c=c breaks
- the Br joins the molecule

135
Q

what type of reaction is an alkene with bromine water

A

addition reaction

136
Q

how does an alkane react with bromine water

A

with intense UV light
- one H substitutes for one Br
- producing the molecule and HBr

137
Q

what type of reaction is an alkane with bromine water

A

substitution reaction

138
Q

what is a monomer

A

a small molecule that can be added together by breaking the double bond

139
Q

what is a polymer

A

long, saturated molecule formed from monomers

140
Q

explain the problems wiht using polymers

A
  • they are inert (unreactive) as they have strong covalent bonds
  • they do not biodegrade
  • when burnt they produce toxic gases
141
Q

desribe how you draw a polymer

A
  • take the functional group (c=c)
  • break the double bond
  • draw two horazontal lines to show continued
  • draw two brackets around
  • copy the atoms on the carbons
  • add an n outside the braket
142
Q

what must alcohols contain

143
Q

how do you purify ethanol from fermentation

A

by distilation

144
Q

what is distilation

A

evapouration followed by condensation to concerntrate ethanol

145
Q

what is ethanol used for

A
  • make alcoholic drinks
  • cars
146
Q

how can you make ethanol

A
  • fermentation
  • direct hydration
147
Q

what is the equation for fermentation

A

C6H12O6 -> 2C2H5OH + 2CO2
glucose -> ethanol + carbon dioxide

148
Q

what is the equation for direct hydration

A

C2H4 + H2O -> C2H8OH
ethene + water -> ethanol

149
Q

what is the functional group of a carboxylic acid

150
Q

what must a carboxylic acid contain

151
Q

what type of bonds do carboxylic acids have between their one oxygen

A

a double bond

152
Q

what do carboxylic acids end in

A

-anoic acid

153
Q

what is this molecule

A

ethanoic acid

154
Q

what is this molecule

A

methanoic acid

155
Q

when reacted what charge does a carboxylic acid have

156
Q

what forms when a carboxylic acid reacts with a metal, eg ethanoic acid

A

the metal ethanoate & hydrogen

157
Q

what is added as a catalyst when making esthers

A

sulphuric acid

158
Q

what colour pH would carboxylic acids be

159
Q

what are esthers used in the industry for

A

perfumes and flavourings

160
Q

what reacts together to form an esther

A

a carboxylic acid and an alcohol

161
Q

what would the esther be called made by propanoic acid and methanol

A

methly propanoate

162
Q

what conditions are used when making esthers

A

H2SO4 and heat

163
Q

what is the other product made when esthers are made

164
Q

how are carboxylic acids formed

A
  • by alcohols being oxidised
  • microbial oxidation
165
Q

what carboxylic acid does vinegar contain

A

ethanoic acid

166
Q

what does volatile mean

A

that they turn innto gases quickly

167
Q

are esthers volatile

168
Q

how do you make esthers in the lab

A
  • add a few drops of concentrated sulfuric acid to a boiling tube with a dropping pipette
  • add 10 drops of ethanoic aci
  • add equal volume of ethanol
  • place in beaker of water - on tripod
  • heat with bunsen burner into boiling
  • after 1 min remove tube and allow to cool
  • pour into test tube if sodium carbonate and mix
  • layer of esther will form on solution
169
Q

what is the oxidising agent for alcohols to carboxylic acids

A

potassium dichromate(VI) in diulte sulfuric acid

170
Q

what is the colour change when ethanol reacts with potassium dichromate in diulte sulfric acid

A

orange to green

Chemistry (22 decks)

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