all of year 10 Flashcards
(170 cards)
1
Q
what are the different types of bonding
A
- metallic
- ionic (metal & non-metal)
- covalent (non-metals)
- giant covalent
2
Q
define metalic bonding
A
eletrostation attraction between rows of metal cations and a sea of delocalised electrons
3
Q
explain is metals are malleable or soft
A
malleable and ductile because the layers of cations can slide
4
Q
define ionic bonding
A
eletrostatic attraction between positive metal and negative non-metal ions
5
Q
are ionically bonded materials malleable or soft
A
brittle (hard but easy to break)
6
Q
define covalent bonding
A
electrostatic attraction between the bonding pair of electrons and bonded nuclei with weak intermolecular forces between molecules
7
Q
what is an alloy
A
a mixture of two or more elements one of which is a metal
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
9
Q
describe the reactivity down group one
A
the get more reactive as you go down
10
Q
how do group 1 elements react with air
A
they all instantly tarnish in air due to oxygen producing a white oxide
11
Q
what is the name given to group one elements
A
alkali metals
12
Q
describe how lithium reacts with water
A
- moves on surface of water
- fizzes
- floats
- squeaky pop with flame
- universal indicator turns blue
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
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
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
16
Q
what are the procucts of a group 1 element and water
A
- metal hydroxide
- hydrogen
17
Q
what is the formula for hydroxide
A
OH -
18
Q
what is the formula for nitrate
A
NO3 -
19
Q
what is the formula for carbonate
A
CO3 2-
20
Q
what is the formula for sulphate
A
SO4 2-
21
Q
what is the formula for hyrdrochloric acid
A
HCl
22
Q
what is the formula for sulfuric acid
A
H2SO4
23
Q
what is the formula for nitric acid
A
HNO3
24
Q
what is the name given to group 7 elements
A
halogens
25
what are the gases in group 7
fluorine and chlorine
26
what are the liquid(s) in group 7
bromine
27
what are the solid(s) in group 7
iodine
28
how many electrons do halogens have
7
29
explain the reactivity trend in group 7
- 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
30
what colour is fluorine
pale yellow gas
31
what colour is chlorine
green gas
32
what colour is bromine
red-brown liquid
33
what colour is iodine
dark gray solid
34
describe displacement in the halogens
a more reactive halogen will displace a less reactive halogen from a solution of its compound
35
will chlorine displace bromine
yes
36
will bromine displace iodine
yes
37
will iodine displace chlorine
no
38
what is a redox reaction
when oxidation and reduction occur at the same time in a reaction
39
what is oxidation
when a substance gains oxygen or loses electrons
40
what is reduction
when a substance loses oxygen or gains electrons
41
what is the oxidising agent
the substance that is reduced (loses oxygen)
42
what is the reducing agent
the substance that is oxidised (gains oxygen)
43
define an acid
produces H+ when dissolved in water, they are proton donors
44
what pH do acidic soutions have
<7
45
define a base
can neutralise an acid; they are proton acceptors
46
define an alkali
a soluble producing OH- ions when disolved in water
47
what pH do alkali solutions have
>7
48
when will an indicator not work
if the solution already has a colour
49
what is the alternative to an indicator
a pH meter
50
what are the indicators and their colour change from acid to alkali
- litmus paper = red - blue
- methyl orange = red - yellow
- phenolphthalein = colourless - pink
- universal = red - orange - green - blue - purple
51
what type of solutions will metal oxides form
alkaline
52
what type of solutions will non-metal oxides form
acidic
53
what is the difference between a base and an alkali
bases aren't soluble in water, alkalis are soluble in water
54
what type of salt will be formed with hydrochloric acid
a chloride
55
what type of salt will be formed with sulfuric acid
a sulfate
56
what type of salt will be formed with nitric acid
a nitate
57
when are salts fromed
when an acid reacts
58
what are the products formed from a metal and an acid
- salt
- hydrogen
59
what are the products formed from a metal oxide and an acid
- salt
- water
60
what are the products formed from a metal carbonate and an acid
- salt
- carbon dioxide
- water
61
what are the products formed from a metal hydroxide and an acid
- salt
- water
62
why don't you react gorup 1 with acids
it is too dangerous
63
what are the two methods to form sulble salts
- excess solid
- titration
64
describe the excess solid method
- 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
65
describe a titration
- 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
66
what are concodant results
+ or - 0.1cm^2
67
how do you record a burette reading
with 2 decimal place
68
what is the equation fro neutrilisation
H+ (aq) + OH- (aq) -> H2O (l)
69
what is meant by the term precipitate
an insoluble salt made from two solutions
70
are sodium salts soluble or insoluble
soluble
71
are potassium salts soluble or insoluble
soluble
72
are ammonium salts soluble or insoluble
soluble
73
are nitrate salts soluble or insoluble
soluble
74
are chloride salts soluble or insoluble
soluble except for silver chloride and lead chloride
75
are sulfate salts soluble or insoluble
soluble except for lead, barium and calcium sulfate
76
are carbonate salts soluble or insoluble
insoluble except for sodium, potassium and ammonium carbonate
77
are hydroxide salts soluble or insoluble
insoluble excep for sodium, potassium and calcium hydroxide
78
describe the method of making an insoluble salt
- mix the two soluble salt solutions together
- precipitate forms
- filter out precipitate
- wash with cold water
- leave to dry in a warm oven
79
what is the chemical test and result for hydrogen
lit split
= squeaky pop
80
what is the chemical test and result for oxygen
glowing split
= relights
81
what is the chemical test and result for carbon dioxide
add acid and bubble through lime water
= goes 'cloudy white'
82
what is the chemical test and result for chlorine gas
damp blue litmus paper
= may turn red then bleached white
83
what is the chemical test and result for ammonia gas
damp red litmus paper
= turns blue
84
what is the chemical test and result for water
white anhydrous copper sulfate
= turns blue
85
how do you test for solid metal ions
carry out a flame test
86
describe a flame test
- 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
what colour flame will lithium produce
red
88
what colour flame will sodium produce
yellow
89
what colour flame will potassium produce
lilac
90
what colour flame will calcium produce
red-orange
91
what colour flame will copper produce
blue-green
92
how do you test for metal ions in a solution
add NaOH
93
what is the result of NaOH added to copper
blue precipitate
94
what is the result of NaOH added to iron (II)
sludgy green precipitate
95
what is the result of NaOH added to iron (III)
reddish brown precipitate
96
how do you test for the halogen non-metal ions
- add HNO3
- add AgNO3
97
what precipitate is formed from chloride
white precipitate
98
what precipitate is formed from bromide
cream precipitate
99
what precipitate is formed from iodine
yellow precipitate
100
how do you test for sulphate non-metal ions and what is the result
- add HCl
- add BaCl2
= white precipitate
101
what are the rules when doing an ionic equation for a precipitate
- 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
what is the general formula of an alkane
CnH2n+2
103
what is the general formula of an alkene
CnH2n
104
what is the general fromula of an alcohol
CnH2n+1OH
105
what is the meant by the term empricial formula
the simplest whole number ratio of atoms of each element in a compound
106
what is the stem for a hydrocarbon with one carbon atom
meth-
107
what is the stem for a hydrocarbon with two carbon atoms
eth-
108
what is the stem for a hydrocarbon with three carbon atoms
prop-
109
what is the stem for a hydrocarbon with four carbon atoms
but-
110
what is meant by the term hydrocarbon
a molecule made up of only carbon and hydrogen atoms
111
what is meant by the term saturated
a molecule only containing single bonds between carbon atoms
112
what is meant by the term unsaturated
a molecule containing carbon = carbon double bonds
113
what is meant by the term isomer
molecule with the same molecular formula but different structual formulae
114
what are the rules for drawing an isomer of a hydrocarbon
- take one carbon off the long chain
- re-bond that carbon to the orignal chain at least one carbon from the end
115
what is crude oil
a mixture of molecules (mainly hydrocarbons)
116
what is the process whihc spereates out crude oil
fractional distilation
117
describe fractional distilation of crude oil
- 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
what are the products from fractional distilation from top of the column to the bottom
- refinary gases
- gasoline (petrol)
- kerosene
- diesel
- fuel oil
- bitumen
119
what are the physical properties of the longer chain hydrocarbons
- more viscous
- more yellow/orange in colour
120
why is catalytic cracking neccessary
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
what is catalystic cracking
the process of breaking down long-chain hydrocarbons into short-chain hydrocarbons
122
what conditions are needed for catalytic cracking
- 600-700 degrees celcius
- catalyst
123
what are the two options for a catalyst for catalytic cracking
- alumina
- silica
124
what type of reaction is combustion
exothermic
125
what are the two types of combustion
- complete
- incomplete
126
what are the conditions and products for complete combustion
- lots of O2
- releases CO2 and H2O
127
what are the conditions and products for incomplete combustion
- limited O2
- releases CO and H2O
128
what is the apparatus for combustion
a u-tube with anydrous CuSO4
129
what are the main pollutants from burning fuels and combustion
- CO2 = greenhouse gas = global warming
- CO = toxic = prevents blood carrying oxygen = death
- NO, NO2 = acid rain
130
are alkenes saturated or unsaturated
unsaturated
131
when are alkene produced
when large hydrocarbon molecules are cracked into samller hydrocarbon molecules
132
what are alkenes used to produce
plastics
133
how can you distinguish between an alkane and alkene
by reacting it with bromine water
134
how does an alkene react with bromine water
it rapidly decolourises from orange to colourless
- the c=c breaks
- the Br joins the molecule
135
what type of reaction is an alkene with bromine water
addition reaction
136
how does an alkane react with bromine water
with intense UV light
- one H substitutes for one Br
- producing the molecule and HBr
137
what type of reaction is an alkane with bromine water
substitution reaction
138
what is a monomer
a small molecule that can be added together by breaking the double bond
139
what is a polymer
long, saturated molecule formed from monomers
140
explain the problems wiht using polymers
- they are inert (unreactive) as they have strong covalent bonds
- they do not biodegrade
- when burnt they produce toxic gases
141
desribe how you draw a polymer
- 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
what must alcohols contain
an OH
143
how do you purify ethanol from fermentation
by distilation
144
what is distilation
evapouration followed by condensation to concerntrate ethanol
145
what is ethanol used for
- make alcoholic drinks
- cars
146
how can you make ethanol
- fermentation
- direct hydration
147
what is the equation for fermentation
C6H12O6 -> 2C2H5OH + 2CO2
glucose -> ethanol + carbon dioxide
148
what is the equation for direct hydration
C2H4 + H2O -> C2H8OH
ethene + water -> ethanol
149
what is the functional group of a carboxylic acid
COOH
150
what must a carboxylic acid contain
COOH
151
what type of bonds do carboxylic acids have between their one oxygen
a double bond
152
what do carboxylic acids end in
-anoic acid
153
what is this molecule
ethanoic acid
154
what is this molecule
methanoic acid
155
when reacted what charge does a carboxylic acid have
-
156
what forms when a carboxylic acid reacts with a metal, eg ethanoic acid
the metal ethanoate & hydrogen
157
what is added as a catalyst when making esthers
sulphuric acid
158
what colour pH would carboxylic acids be
orange
159
what are esthers used in the industry for
perfumes and flavourings
160
what reacts together to form an esther
a carboxylic acid and an alcohol
161
what would the esther be called made by propanoic acid and methanol
methly propanoate
162
what conditions are used when making esthers
H2SO4 and heat
163
what is the other product made when esthers are made
water
164
how are carboxylic acids formed
- by alcohols being oxidised
- microbial oxidation
165
what carboxylic acid does vinegar contain
ethanoic acid
166
what does volatile mean
that they turn innto gases quickly
167
are esthers volatile
yes
168
how do you make esthers in the lab
- 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
what is the oxidising agent for alcohols to carboxylic acids
potassium dichromate(VI) in diulte sulfuric acid
170
what is the colour change when ethanol reacts with potassium dichromate in diulte sulfric acid
orange to green
