Gcse What You Got Wrong Flashcards
1
Q
Why are compounds always pure
A
Because they are always within a fixed ratio of atoms
2
Q
What is an element
A
A substance that consists of only one type of atom
That can not be broken down any simpler by chemical means
3
Q
Describe the arrangement of gases
A
A= random and widely spread out
M= move randomly in all directions and freely
P= rarely in contract with each other
4
Q
As the temperature increases, what happens to the solubility of a gas
A
It decreases
5
Q
In, the experiment for measuring solubility, state the word equation for the calculation at the end
A
Mass of crystals dissolved= (mass of crystals + basin) - (mass of basin)
Mass of water that evaporated (that the solvent was orignal dissolved in )= (mass of basin + solution )- (mass of basin + crystals)
6
Q
Explain how the diffusion of potassium permanganate (iv) happens in water
A
Particles move from a high concentration to a low concentration
This is because there are gaps in the liquid and particles in a liquid are able to Slide Over each other
Therefore they can easily mix together
7
Q
Explain why as temperature increases, solubility of a solid also increase
A
Because the solvent molecules have more kinetic energy
This means that they can more efficiently break apart solute molecules held together by intermolecular forces of attraction
8
Q
Describe the structure of ionic substances, giant covalent substances, and metallic substances
A
Ionic:
-giant ionic lattice
-ions are regularly arranged
-and positive and negative ions repeat in a pattern
Giant covalent:
-giant lattice structure
-number of atoms is invariable
- so repeats on in 3D
Metallic
-giant metallic lattice
- held together by electrostatic attraction between positive ions and sea of delocalized
9
Q
In the electrolysis of aluminum oxide, what deposits at the bottom
A
Molten aluminum
10
Q
Why is diamond hard
A
Because of the rigid tetrahedral structure
11
Q
How can you measure the initial volume of air, when measuring percentage of oxygen in the air using iron
A
Fill the connecting tube and the flask with water and then measure this out in a measuring cylinder
12
Q
Explain how the phosphorus experiment works when measuring the percentage of oxygen in the air
A
-phosphorus is placed on an evaporating dish, on top of a trough of water in a bell jar
- it reacts with the oxygen in the air to form phosphorous oxide, a white smoke, which dissolves in the water
-this makes the water levels rise, and so you can measure the water levels before, and then the water levels after
13
Q
What is the word equation for the thermal decomposition of metal carbonates
A
Metal carbonate—-) metal oxide + carbon dioxide
14
Q
Give 5 word equationexamples of how carbon dioxide can be produced
A
Copper carbonate —-) copper oxide + carbon dioxide (thermal decomposition)
Calcium carbonate —-) calcium oxide + carbon dioxide (thermal decomposition)
Calcium carbonate + hydrochloric acid ——) calcium chloride + carbon dioxide + water
Carbon + oxygen —-) carbon dioxide
Petrol + oxygen —-) carbon dioxide + water
15
Q
Give the balanced symbol equation for the reaction between calcium carbonate and hydrochloric acid
A
CaCO3(s) + HCL(aq) -—-) CaCl2 (aq) + CO2(g) + H2O(l)
16
Q
Give the balanced symbol equation, using petrol to make carbon dioxide
A
2CH8H18 + 2O2 ——) 16CO2 + 18H2O
(This is the complete combustion of fuels, which always make carbon dioxide and water)
17
Q
Describe an experiment to measur oxygen in the air, using iron WOOL
A
Soak iron wool on acetic acid to catalyse the reaction
Push into a measuring cylinder and then invert inside trough of water
Measure initial volume of air
As iron reacts with oxygen, the water level will rise to replace the space taken up by oxygen
Measure the final volume of oxygen
18
Q
Give the equation to test that carbon dioxide has been given off
A
Bubbled in lime water to produce a white précipite of calcium carbonate
Ca(OH)2 + CO2 ——-) CaCO3 + H2O
19
Q
When you keep bubbling carbon dioxide in a solution of calcium carbonate and water, give the balanced symbol equation of what happens and the colour change
A
CaCO3 + H2O + CO2 ——) Ca(HCO3)2(aq)
Colourless
20
Q
State three substances that can be used to show combustion reactions, and give the flame colours produced aswell
A
Magnesium —-) white flame
Sulfur —-) dark blue flame
Hydrogen—-) pale blue flame
21
Q
State the balanced symbol equation when magnesium oxide reacts with water, and when sulfur dioxide reacts with water
A
MgO+ H2O —-) Mg(OH)
SO2 + H2O —-) H2SO3 (SULFUROUS ACID)
22
Q
Metal oxides are… in water
Non metal oxides are…. In water
A
Insoluble
Soluble
23
Q
Describe the reaction between calcium and water
A
Slow reaction
Bubble form
White insoluble calcium hydroxide forms
In a colorless solution
24
Q
Describe the reaction with magnesium with water and or steam
A
Does not react with water, because insoluble magnesium hydroxide layer is formed
Reacts with steam, to form magnesium oxide, which burns with a bright white flame. Also produces hydrogen
25
General word equation for metal and steam
Metal + steam —) metal oxide + hydrogen
26
Describe what happens to zinc in steam, and then iron in steam, with the colours
Zinc oxide formed, which is yellow upon heating but white upon cooling
Iron tetroxide formed, which is a darker grey
27
Describe the reaction between aluminum and hot and cold acid
Cold acid:
Reacts slowly and then vigorously,
Forms a layer of aluminum oxide, so the reaction stops
Hot acid: aluminum oxide layer is formed so reacts more vigorously
28
Describe the reactions of magnesium, zinc, and iron in hydrochloric acid
Magnesium:
- vigorous reaction
- rapid fizzing
-becomes hot
-colourless solution
Zinc:
-steady reaction
-steady fizzing
-becomes warm
- colourless solution
Iron:
-slow reaction
- fizzing
-slightly warm
- pale green solution
29
When iron reacts with hydrochloric acid, what colour is formed
Green pale solution
30
What two types of displacement reactions can you use to determine the reactivity of metals,
And then for each type state what will happen to the more reactive metal and then the less reactive metal.
-Metals with metal oxides, upon heating
-Metals with aqueous solutions of metal salt.
With metal oxides, more reactive metal is oxidized (as it binds more strongly to oxygen,
and less reactive metal is reduced
With aqueous solutions of metal salts, more reactive metal dissolves as it forms a solution
Less reactive metal coats the surface of the more reactive metal
31
Oxidizing agent defintion
Substance that oxidizes something else
So is reduced
32
What does the reactivity of metals depend upon
Their ability to from positive ions and lose electrons
33
Give the symbol way of writing hydrated iron (iii) oxide
Fe2O3.xH2O
34
Balanced symbol equation for the process of rust
4Fe + 3O2 + H2O —-) 2Fe2O3.XH2O
35
Galvanizing utilisés which two methods
Sacrificial protection
And the barrier method
36
percentage of argon in the air
0.9%
37
give the colours of the flames produced with the combustion reactions of sulphur, magnesium, hydrogen
sulfur, blue
magnesium, bright white
hydrogen, pale blue
38
give the thermal decomposition word equation reaction for a metal carbonate
metal oxide + carbon dioxide
39
give the word equation for the reaction between metal carbonate and acid
salt + carbon dioxide + water
40
give three ways that carbon dioxide can be produced
thermal decomposition of metal carbonates.
metal carbonate and acid, (react to form co2, salt, water)
combustion of fossil fuels
41
thermal decomposition of calcium carbonate has occurred. it is bubbled through lime water. what colour will it turn and what is produced
white precipitate,
because the decomposition results in the formation of carbon dioxide, when this bubbles in calcium hydroxide, it forms calcium carbonate and water
42
state the word equation for carbon dioxide is continuously bubbled through calcium hydroxide for a long time
calcium carbonate + carbon dioxide + water------ calcium hydrogen carbonate
43
reaction between,
metal + water
metal oxide + water
metal + steam
metal hydroxide + hydrogen
metal hydroxide
metal oxide + hydrogen
44
give descriptions of the reaction between,
magnesium +hcl
zinc + hcl
iron +hcl
vigorous,hot test tube, colourless
rapid reaction, warm test tube, colourless
slow reaction,slightyl warm, pale blue
45
what are two types of displacement reactions that can occur
combustion of metal oxide
reaction of metals with aqueous metal salt solutions
46
what is an ore
a rock that contains enough of the metal to extract it
47
what is a mineral
element or compound that occurs naturally
48
what is the relationship between steel and iron
steels are alloys of iron, mixed with different amounts of carbon
49
properties and uses of copper
unreactive
conducts electricity
malleable
pots and pans
electrical wires
water pipes
50
properties and uses of aluminium
resists corrosion
conducts electricity
low density
pots and pans
electric wires
car bodies
51
properties and uses of mild carbon steel
corrodes easily,
malleable
nails
carbodies
52
properties and uses of high carbon steel
brittle and hard,
cutting tools,
bridges
53
properties and uses of stainless steel
resists corrosion
strong
cutlery
sinks
54
stainless steel is an alloy of what
carbon and nickel
55
what is an alloy. then explain why alloys are harder than pure metals
alloys are mixtures of a metal with one or more other elements.
hard because has different sized atoms
which disrupts the regular lattice structure
so harder for the layers of ions to slide over each other
56
what colour does phenolphthalein and methyl orange turn in acid, and alkali solutions
phenolpthalein;
acid-colourless
alkali-pink
methyl;
acid-red
alkali; yellow
57
give 5 things to do in a titration to ensure accuracy
and give the value for results to be concordant
-use a white tile underneath
-swirl the solution to mix
-use water to rinse the flask at the end
-use a pipette with a pipette filler for an accurate reading
-always measure burette reading from bottom of the meniscus
concordant results are 0.2 + or_
58
an acid base reaction occurs and effervescence occurs. explain what type the base used was
base was a metal carbonate
bc when metal carbonate reacts with acids, co2 is given off which produces effervescence
59
Give four example of bases
Metal Carbonates
Metal oxides
Metal Hydroxides
Ammonia in solution
60
An acid is a proton..A bass is a proton…
Donor
Acceptor
61
Why must a titration be used to make a soluble salt of potassium sodium or ammonium
Because they are soluble in water, so it would not be known when the reaction is finished, and so exactly how much acid to add
62
What is the flame test colour for calcium
Orange
63
Describe how to carry out a precipation reaction for cations, and then give the observations made for each cation
Dissolve the salt in distilled water to form a solution (needs to be a solution for it to occur)
Add dilute sodium hydroxide
Observe the precipitate
Copper 2+—) blue
Ammonium ions, in cold—-) a smell. Ammonia in hot—-) red litmus turns blue
Iron 2+——) green
Iron 3+—-) brown
64
Describe what will happen to the colour of the precipitate if left out for a while, in the precipitation reaction of iron 2+
The iron (ii)hydroxide formed from the reaction will react with oxygen in the air to form iron (iii) hydroxide
65
Give the test for chlorine gas
1)take DAMP blue litmus paper and place in solution
2)will first turn red as chlorine dissolves in water to form an acidic soltuion
3)but will then turn it white because it beaches the paper
66
Give the test for carbonates
-add hydrochloric acid to the salt solution
-if fizzing is given off, this means a gas is produced
-and so test that the gas is carbon dioxide by bubbling it through limewater, to turn milky
67
Give the test for sulfates
-add hydrochloric acid to a solution of barium chloride (added to get rid of any carbonate or sulfite ions which could also form a précipitate)
-add this solution to the salt solution which is dissolved in distilled water
-a white precipitate of barium sulfate will form
68
Give the test for halides and the different observations
-add nitric acid to a solution of silver nitrate (the acid is added to get rid of any traces of other anions such as carbonates of sulfates
-add this solution to the solution of the halide dissolved in distilled water
-for chlorides, a white precipitate will form
-for bromides, a cream precipitate will form
-for iodides, a yellow precipitate will for,
69
Give the formula for hydrated copper sulfate
CuSO4.5H2O
70
Give the test for ammonium ions
Add sodium hydroxide to the solution
A pungent gas of ammonia will be given off
Test the GAS with DAMP red litmus, should turn blue
71
Volatility…. As chain length increases (for hydrocarbons) and explain why
Melting + boiling….. as chain length increases (for hydrocarbons) explain why
Decreases, because longer chain length means greater atomic mass, and so stronger attraction between other molecules, so less able to evaporate
Increases, because longer chain length so greater atomic mass, so greater intermolecular forces of attraction, so more energy required to break apart
72
When nitrogen oxide reacts with rain water what forms
When nitrogen oxide react with rain water and more oxygen what forms
Give the chemical formula for each
Nitric acid (HNO3)and nitrous acid(HNO2)
Nitric acid (HNO3)
73
Give the word equation for the hydration of ethene
Ethene + steam —-) ethanol
74
Give three word equations that involve the oxidation of ethanol
Combustion : ethanol + oxygen —-) carbon dioxide + water
Aerobic oxidation: ethanol + oxygen. —-) ethanoic acid. + water
Oxidizing agent: ethanol + potassium dichromate (IV) in dilute sulfuric acid. —-) ethanoic acid. + water
75
Give two advantages and two advantages of using fermentation over hydration of ethene to produce ethanol
Adv: renewable, uses less energy
Dis: slower process, less efficient bc batch process
76
Why is fermentation to produce ethanol done in an absence of air
Because of air got in it would oxidize the ethanol and produce ethanoic acid
77
What is vinegar
An aqeous solution of ethanoic acid
78
Write the formula for ethyl ethanoate
CH3COOCH2CH3
79
When preparing an ester using distillation, why does the ester evaporate the quickest
Because it is volatile, so has a low boiling point
80
Give the word equation to make an ester and then explain a basic method to do so
Alcohol + carboxylic acid —-) ester + water
1) add alcohol and Carboxylic acid to a beaker, with sulfuric acid
2)heat in a water bath
3) add sodium carbonate to remove acidic impurities
4)add calcium chloride to remove alcoholic impurities
5)the alcohol and acid will dissolve and the ester will float on top and you’ll be able to waft the smell
81
Draw the monomer for poly(tetrafluroethene)
Two carbon atoms in the centre joined by a double bond, each attached to a single fluorine
82
What is a polymer
A large molecule made by joining many smaller molecules together (monomers)
83
Describe three conditions to occur for addition polymérisation to occur
-must be an alkene
-must use heat and Hugh pressures
-must use an initiator, not a catalyst
84
Give two advantages and three disadvantges of landfill
Give two advantges and two disadvantges of incineration
(In terms of disposing of addition polymers)
Adv land; cheap, doesn’t produce green houe gases
Disad landfill: smells, unpleasant appearance, takes up space
Adv inciner:fuel can be used to heat home, dosent take up space
Disad inciner: produces green house gases, ashes still need to be disposed of
85
Why are addition polymers non biodegradable
Because they have c-c bonds which makes them unreactive, and so they can not be broken down by other substances
86
What is a polyester.
How is an ester link formed
Polyester is a type of condensation polymer formed when many ester links join together.
An ester link forms when the dicarboxylic acid functional group reacts the diol functional group, and a water molecule is lost in the process
87
Give two conditions for condensation polymerization to occur
-two different functional groups must be present
-each monomer must have atleast two functional groups attached to it
88
Give the word equation for condensation polymérisation
Dicarboxylic acid + diol monomer —-) poly (ester) + 2 water molecules
89
Explain whether bond breaking is Exothermic or endothermic
Bond breaking is Endothermic,
Because amount of energy needed to break bonds,
Is greater than amount of energy released when bonds are formed
90
Explain whether bond making is endo or Exothermic
Bond making is Exothermic,
Because amount of energy released to make bonds,
Is greater than amount of energy needed when bonds are broken
91
Is displacement endo or Exothermic reaction
Can be both
92
Explain the effect of increasing temperture on rate of reaction
Increasing temp, increases rate of reaction
Because particles have more kinetic energy
So are able to move more quickly
Therefore more frequent successful collisions per second
AND ALSO bc each collision has more energy,
There is a greater number of particles which have more energy than the activation energy require,
Therefore there are more succeful collisons
93
Explain why the presence of a catalyst increases the rate of reaction
Because it decreases the activation energy required
By providing an alternative pathway with a lower activation energy
Therefore more particles have the minium amount of energy required for the reaction to occur
94
Describe the reversible reaction of the dehydration of hydrated copper (ii) sulfate
When hydrated (ii) copper sulfate is heated, the blue crystals turn into a white powder anyhdrous copper sulfate and water.
This is the forward reaction,an endothermic reaction because energy is absorbed by the surroundings.
When water is added to anhydrous copper ii sulfate, it becomes blue copper sulfate crystals again.
This is an Exothermic reaction because heat is given out.
95
Describe the reversible reaction of the decomposition of ammonium chloride
Ammonium chloride is a white solid. Upon heating, it breaks down into ammonia gas and hydrogen chloride. This is the forwards reaction whcih is endothermic, because energy is taken in.
If left to cool,the ammonia gas and hydrogen chloride reform to make the solid. This is the backwards reaction which is exothermic, because energy is released into surroundings
96
What are the two conditions for dynamic equilibrium to occur:
-must be a reversible reaction
-must be in a closed container
97
What happens at dynamic equilibrium
-The concentration of products and reacts remain constant, but not necessarily equal,
-because the forwards and backwards reactions happen at the same rate
98
In the haber process, so when nitrogen and hydrogen combine to make ammonia, which direction is endothermic and which direction is exothermic
Forwards reaction is exothermic
Backwards reaction is endothermic
99
Why does a catalyst not affect the position of equilibrium in a reversible reaction
Because a catalyst increases the overall rate of reaction.
So therefore, the rate of the the forward reaction increases at an equal rate as the backwards reaction does.
It only speeds p the reaction, and so does not have an effect on the position of equilibrium.
100
What does the position of equilibrium mean
The side of the reaction which contains more particles
101
What is the effect of temperture n the position of equilibrium
All reactions are endothermic in one direction and exothermic in the other direction.
If you increases the temperture, then the endothermic reaction will occur inorder to use more heat.
If you decrease the temperture, then the exothermic reaction will occur inorder to release more heat
102
What is the effect of pressure on equilibrium
In all reactions, one side of the equation has more moles than the other.
If pressure increases, then the reaction om the side with thr least amount of moles will be encouraged, and fewer moles will be produced.
If you decreases the pressure, then the reaction on the side with the greater amount of moles will be encouraged and so more moles will be produced.
103
Metal carbonate + acid =
Metal salt + co2 + water
104
Two ways to make sure that all the acid is reacted, when mixing aluminum hydroxide and sulfuric acid to make a salt
Use excess aluminium hydroxide; [1 mark]
Stir (thoroughly); [1 mark]
105
In an experiment to measure the value of x, in a water of crystallization, the value obtained is lower than what was expected. Explain why and how they could overcome this
The crystals were not heated for long enough so not all of the water was able to evaporate.
Can improve by reheating until your achieve a constant mass
106
What is a solute
The solid that dissolves in a solvent
107
What is a saturated solution
A solution in which the maximum amount of solute has dissolved as possible
AT A SPECFIC TEMPERATURE
108
How does dilution occur
Because of diffusion, because particles of colour move from a high conc to low conc
And so can mix with the water molecules
109
If comparing two setups of chromatography, what two things should be the same
Same solvent
Same chromatography paper
110
What is atomic number
The number of protons in the nucleus of an atom
111
Give six properties of metals
Good conductors pf electricity
Good conductors of heat
High density
High melting point
Malleable
Ductile
112
Metal oxides are…
Non métal oxides are…
Basic
Acidic
113
Why do ionic compounds have high melting points
Strong electrostatic forces of attraction
Between oppositely charged ions
So therefore large amounts of thermal energy needed to overcome these forces of attraction
114
Why covalent substances low boiling + melting
Because weak intermolecular forces of attraction
Between the molecules
Therefore small amount of thermal energy required to overcome this attraction
115
How many double bonds do alkenes have
Only one
116
What is thermal decomposition
The breaking down of a COMPOUND
using heat
117
How to calculate the solubility of a substance using experiment. Aka what formula could u use
Mass of solute/ mass of water removed
X100
118
Give example of weak acid and string acid
Give example of weak alakali and strong alkali
Ethanoic acid, hydrochloric acid
Ammonia, sodium hydroxide
119
Explain an experiment on how you can measure effect if catalyst on rate of reaction
Add certain volume of hydrogen peroxide to a conical flask
Measure certain mass of catalyst
Put a bung on
Measure time taken for certain volume of gas to be produced
Repeat with diff catalysts but with same mass, and same volume of hydrogène peroxide
120
How do catalysts reduce the rate of reaction
They lower the activation energy required for a reaction
By providing an alternative reaction pathway with a lower activation energy
Therefore more particles have at least the minimum amount of energy required for reaction to occur
121
What is the measurement that u take when measuring the effect of surface area on the rate of reaction
In a fixed amount of time, you are measuring the volume of gas produced
So every ten seconds, measure the amount of gas produced
122
What is the first step of the flame test
Dip a loop of unreactive wire such as (platinum or Nichrome) dip in HYDROHCLORIC ACID
123
In the flame test, what colour shows for the presence of sodium cations, and then for calcium cations
Sodium = yellow
Calcium =orange
124
Apart from the flame test, describe another test you can carry out to identity cations
Adding sodium hydroxide to see if a precipitate will form.
1)so dissolve the salt in distilled water
2)then add sodium hydroxide
3)observe color of precipitate
125
Why is sodium hydroxide specifically used to test for cations in the precipitate test
Because it is the only hydroxide that is soluble
Therefore when it reacts with a metal it forms a metal hydroxide
But metal hydroxides are all insoluble, so will form a precipate
126
Apart from iron2+ and iron 3+, what are two other cations you can test for in the cation precipitate test
Ammonia
Copper 2+
127
What is the chemical equation for the reaction between carbon dioxide and limewater
CO2 + CaOH2 ——-) CaCO3 + H2O
128
Give the solubility rules of carbonates hydroxides and sulfates in order of what you’ve memorized
Sulfates: barium, lead, calcium
Carbonates: sodium, potassium, ammonium (all others insoluble)
Hydroxides: sodium, potassium, calcium (all others insoluble)
129
Give the word equation to make a soluble salt.
Give the word equation to make an insoluble salt.
Insoluble base + acid—-) soluble salt + water
Soluble salt + soluble salt ——) insoluble salt + soluble salt
130
Give the steps to make an insoluble salt
1)add soluble salt to soluble salt
2)filter off the précipitate
3)add to distilled water
4)observe the precipitate formed
131
Give three examples of insoluble salts and the colour of the precipitates that they form
Lead sulfate
Barium sulfate (white precipitate)
Silver chloride (white precipitate)
132
An insoluble salt is made, how do U identify the two substances that it was made from
The metal part usually comes from a nitrate
The non metal part usually comes from sodium, potassium or ammonium
133
Give step one of making a soluble salt
Heat the acid under a Bunsen burner so that rate of reaction will also be sped up
134
When making a soluble salt, give the next few steps after filtering off the excess base so that you’re left with salt solution and water
Heat to evaporate SOME of the water to form concentrated solution
Keep heating until saturated solution is formed
Leave soltuion to cool and to crystallize
Filter off the soltuion so that left with crystals as residue
135
Why do you not evaporate off all the water when making a soluble salt
Because the water needs to be present for water of crystallization
And also to prevent it from decomposing
136
Which one of the metals in the reactivity series does not react with water
Aluminum
137
What happens when aluminum reacts with acid in the reactivity series
Slow to start, but eventually becomes more vigourous
(Aluminum oxide layer on top prevents reaction)
138
State the colour changes of the three metals when they react with hydrochloric acid
Magnesium —) colourless
Zinc——) colourless
Iron——) green
139
What are two types of displacement reaction that can occur, and what happens in them
Redox, with a metal and metal oxide (more reactive binds with oxygen)
An aqeous soltuion of a metal salt(more reactive displaces less reactive, less reactive coats the surface)
140
Apart from magnesium, what two other substances can be used in a combustion reaction and give the colour of the flames that they produce
Sulfur, which forms a dark blue flame
Hydrogen, forms a pale blue flame
141
What is an ore. What is a mineral. What is a native substance
Ore is a substance that contains enough of a wanted mineral in it
Mineral is a substance that occurs naturally
Native is s substance that occurs without any other minerals in it
142
Describe the structure of ionic compounds
A giant lattice structure
Closely packed and regular arrangement
Of a repeating pattern of positive and negative ions
Held together by strong electrostatic forces of attraction between the oppsitely charged ions
143
Graphite melting and boiling point
High melting and boiling point,
Bc although weak intermolecular forces of attraction holding the layers together
The individual atoms are held together by strong covalent bonds.
Require large amounts of heat energy to overcome
144
Can graphite conduct electricty and explain
Yes
Because
Each carbon atom forms three bonds with three other carbon atoms
Therefore each carbon atom has one delocalized electron
Which is free to move and conduct a charge
145
Describe a Metallic structure
Giant metallic lattice structure
Held together by positive ions
Surrounded by sea of delocalized electrons
146
Anode rule
Cathode rule
Anode rule. If halide is parents it will be discharged.otherwise OH- will be discharged
Cathode rule. Least reactive will be discharged (relative to hydrogen)
147
If OH- ions discharged at the anode, what produces will be produced
Oxygen and hydrogen
(Rmeber in the equation u also have to add 4e aswell tho)
148
Give the general word equation for an alkene + bromine,
Alkene + bromine —-) alkane(1,2 dibromoalkane)
149
General word equation for substitution
Alkane + halogen —) halogens alkane + hydrogen halide
150
Give the general word equation for when ethanol is oxidized using a reducing agent
Ethanol + 2(o) —) ethanoic acid + water
151
Give the general word equation when ethanol is oxidized used aerobic respiration
Ethanol + oxygen —-) ethanoic acid + water
152
Give the eternal word equation for hydration of ethene
Ethene + steam —-) ethanol
153
Give the general word equation for fermentation
Glucose —(yeast)—-)ethanol +co2
154
Give the structural formula of methanoic acid
And then of ethanoic acid
HCOOH
CH3COOH
155
Do carboxylic acids have a double bond or not
Yes
156
Give three conditions required for addition polymerization
-Hugh temperatures and pressures
-must be unsaturated
-an initiator required
157
Give the steps to make an ester
-Mix Carboxylic acid and alcohol together, and then add concentrated sulfuric acid as the catalyst
-add calcium carbonate to remove alcoholic impurities
-add sodium carbonate to remove acidic impurities
Ester will float on top
158
Give the general word equation for condensation polymerization
Dicarboxylic acid + diol monomer —) poly(ester) + water
159
When hydroxide ions are deposited at the anode, give the half equation
4OH~ ——) 2H2O + O2 + 4e~
160
Concordant results differ by..
O.2cm3 or less
161
How does a catalyst increase rate of reaction
Provides an alternative pathway
With a lower activation energy
Therefore more particles have more energy than the activation energy
162
Reaction of ammonia and sulfuric acid word equation
Reaction of ammonium and sulfuric acid
Ammonia + sulfuric acid —-) ammonium sulfate
Ammonium + sulfuric acid —-) ammonium sulfate + water
163
Metal oxide + water
Metal hydroxide
164
Metal + steam
Metal oxide + hydrogen
165
Metal + water
Metal hydroxide + hydrogen
166
Metal + oxygen
Metal oxide
167
Metal oxides are… (soluble/ insoluble)
Usually insoluble.
Except can form metal hydroxides sometimes
168
Non metal oxides are ..soluble/ insoluble
Soluble
