PPQ's Flashcards
1
Q
Which element is used to sterilise water? (1)
A
Chlorine (Cl)
2
Q
Name a metal that can be made by heating its oxide with carbon? (1)
A
Iron (Fe)
3
Q
Explain why a powdered form is used rather than large pieces to increase rate of reaction. (2)
A
They have a larger Surface Area
Leading to a faster reaction.
4
Q
When dilute HCl is added to a solid, a gas forms.
Which of these ions is present in the solid? (1)
A
Carbonate (CO3)
5
Q
In an experiment on the anaerobic respiration of yeast to produce ethanol.
State the purpose of the yeast. (1)
A
The yeast acts like a catalyst. The zymase enzyme acts as the catalyst.
6
Q
What method is used to obtain water from a mixture containing salt and water? (1)
A
Simple Distillation
7
Q
State why the solvent level should not be above the base line at the start of the experiment. (1)
A
To prevent the inks mixing in the solvent trough.
8
Q
(In paper chromatography), State why ink D does not move during the experiment. (1)
A
As the ink is insoluble in the solvent
9
Q
Water is the name used for H2O(l).
Give the two names used for H2O(g). (2)
A
Steam
Water Vapour
10
Q
Name the to gases that react to form nitrogen oxides. (1)
A
Nitrogen and Oxygen
11
Q
State a physical property of Na that shows it is a metal. (1)
A
Good conductor of electricity
12
Q
State an observation that can be made when adding Potassium (K) to a trough of water. (1)
A
A flame burns (as the hydrogen produced ignites)
13
Q
Name an element that is a liquid at room temperature. (1)
A
Bromine
14
Q
What element is used in fire extinguishers? (1)
A
Carbon Dioxide
15
Q
Name a hydrocarbon compound used as a fuel. (1)
A
Methane
16
Q
State the name of the mesh heating guard used above Bunsen Burners in heating. (1)
A
Gauze
17
Q
State the name of the equipment that holds a gauze above a bunsen burner. (1)
A
Tripod
18
Q
Name two elements in Period 2 that form acidic oxides. (2)
A
Carbon
Nitrogen
Fluorine
19
Q
What are the elements arranged by in the periodic table?
A
Atomic Number
20
Q
State what is meant by the term covalent bond? (2)
A
Attracted to the nuclei of both atoms.
Electrostatic attraction of bonding through sharing electrons.
21
Q
Explain why carbon dioxide has a low boiling point. (2)
A
There are weak intermolecular forces between molecules.
Little thermal energy is required to overcome forces.
22
Q
- Blast Furnace - - - - - - -
Give the name of the Iron ore that contains Fe2O3. (1)
A
Haematite
23
Q
State two condition required fir industry cracking. (2)
A
600 - 700 *C
Alumina or Silica
24
Q
State the molecular formula of Decane. (1)
A
C10 H22
25
State the general formula of the homologous series that includes Decane. (1)
Cn H2n+2
26
State the observation made when platinum is added to cold water. (1)
No Change - Platinum is not very reactive
27
- - - - - - - Haber Process - - - - - - -
| Name the type of reaction that occurs between ammonia and sulfuric acid. (1)
Nuetralisation
28
State the formula of Ammonium Sulfate. (1)
(NH4)2SO4
29
Nitric acid and ammonia are used to produce ammonium nitrate.
Explain why ammonium nitrate is used in agriculture.(2)
Ammonium nitrate contains nitrogen, which stimulates plant growth and development as a chemical fertiliser.
30
Give a test to show that the potassium nitrate solution in the test tube contains potassium ions. (2)
- Carry out a flame test.
| - Lilac colour given out.
31
Name the gas which is necessary for rusting to occur. (1)
Oxygen
32
Name the gas which bleaches moist litmus paper. (1)
Chlorine
33
Name the gas which has the highest percentage by volume in the air. (1)
Nitrogen
34
Explain how decreasing the concentration of the hydrochloric acid affects the rate of reaction.
Refer to particle collision theory in your answer. (3)
- As the concentration decreases, there are less particles per unit measure.
- Meaning there are less particle collisions per unit time.
- Therefore less successful collision per unit time, reaction rate has decreased.
35
In a titration, suggest why it is not necessary to dry the flask (after washing it) before repeating the titration. (1)
Water does not effect the number of moles.
36
What are concordant results? (1)
Those results within 0.20 cm^3 of each other.
37
What type of polymers are poly(ethene) and poly(chloroethene)
Addition Polymers
38
Name the polymerisation process used to form Nylon. (1)
Condensation
39
In titrations, state why zinc should not be used for the electrodes. (1)
Zinc is not an inert element and may react.
40
Name a process that takes place in a Hofmann voltameter. (1)
Electrolysis
41
Which particles is furthest from the centre of each atom. (1)
An electron
42
What makes two atoms neutral? (1)
Electrons and Protons
43
What method of separation is used to separate red ink from a mixture of coloured inks? (1)
Chromatography
44
What method of separation is used to separate ethanol from a mixture of ethanol and water? (1)
Fractional Distillation
45
What method of separation is used to separate a mixture of sand and water? (1)
Filtration
46
What method of separation is used to separate water from a copper (II) Sulfate solution? (1)
Simple Distillation
47
Describe a Chemical test to show that the colourless liquid contains water. (2)
Test ... Anhydrous Copper (II) Sulfate
| Result ... Changes to a blue colour (from white)
48
Describe a Physical test to show that the colourless liquid is pure water. (2)
Test ... Boiling point and Freeing point
| Result ... B.P = 100 *C, F.P = 0 *C
49
- - - - - - - Not on New Spec - - - - - - -
| Explain why Carbon Dioxide is sometimes used in fire extinguishers. (2)
The CO2 blankets the fire
| Stopping oxygen getting to the fire and developing it
50
Incomplete combustion of propane leads to the formation of a poisonous gas.
Identify this gas. (1)
Carbon Monoxide (CO)
51
During the combustion of propane at high temperatures, gases represented by the formula NOx can form.
Which two elements combine to form these gases? (1)
Nitrogen (N) and Oxygen (O)
52
The disposal of most addition polymers is a problem because they do not biodegrade.
What is meant by the term biodegrade? (2)
breaks down / decomposes / decays
by bacteria / microbes / microorganisms
53
Complete the sentence. (1)
Lithium reacts with water to form an ..........
Alkali
54
Which group contains the noble gases? (1)
0
55
Identify the group whose atoms form ions with a charge of +1. (1)
1
56
Identify the group whose atoms form ions with a charge of -1. (1)
7
57
State the process that occurs as ethene changes t poly(ethene). (1)
Deposition - Gas -> Solid
58
Describe what is done to the crude oil before it enters the fractionating column. (2)
Heated
| Until Vaporised
59
When potassium is heated in gas X, potassium chloride solid is formed. State Gas X. (1)
Chlorine
60
When water is added to Potassium, colourless solution Y forms. State Y. (1)
Potassium Hydroxide
61
When Potassium Hydroxide has acid Z added to it, potassium chloride solution forms. State acid Z. (1)
Hydrochloric Acid
62
Give a test to show that an aqueous solution of sodium iodide contains iodide ions. (3)
- Add dilute nitric acid.
- Add (aqueous) silver nitrate.
- Yellow precipitate formed.
63
Sulfur Dioxide dissolves in water to form an acidic solution.
Identify the ion that causes this solution to be acidic. (1)
H+
64
State how litmus paper can be used to tell your solution is acidic. (1)
Blue litmus paper will turn red in acid.
65
Give two observations that are made when a piece of magnesium ribbon is added to the acidic solution. (2)
Effervescence.
Dissolves into acid.
ACCEPT gas produced and named (H2).
66
State why metals such as titanium are good electricity conductors. (1)
Their delocalised electrons can flow.
67
Explain why metals such as titanium are malleable. (1)
(Cat)ion layers
| Can slide / slip over one another
68
Slaked Lime, Ca(OH)2, forms when water is added to calcium oxide.
Give the chemical name of Slaked Lime. (1)
Calcium Hydroxide
69
```
Which of these is the formula for a molecule of an element? (1)
H
H2
H2O
H2O2
```
H2
70
What method of separation is used to separate dyes from a food colouring? (1)
Chromatography
71
Describe how to carry out a test to show that an (aqueous) sample contains chloride ions. (3)
- add (dilute) nitric acid
- add silver nitrate (solution)
- white precipitate forms
72
A brown solid contains hydrated iron(III) oxide.
| What is the common name for this brown solid? (1)
Rust
73
Identify two substances that react with Iron to form rust. (2)
Water
| Oxygen
74
What process involves coating iron with zinc? (1)
Galvanisation
75
What is the correct name for the compound with formula CuSO4? (1)
Copper(II) Sulfate
76
What colour is NH4Cl(s)? (1)
White
77
What colour is NH4Cl(aq)? (1)
Colourless
78
What is formed when sodium hydroxide solution is added to a sample of iron(III) sulfate solution? (1)
Brown Precipitate forms - [Iron(III)]
79
What is the general formula of an Alkene? (1)
Cn H2n
80
T/F: (1)
| Halogens an be obtained by electrolysing molten metal halides.
True - Electrolysis
81
T/F: (1)
| The first Halogens are diatomic.
True
82
T/F: (1)
| The halogens form covalent bonds with other non-metals.
True
83
T/F: (1)
| All halogens are liquid at room temperature
False - based on boiling points
84
T/F: (1)
| The boiling points of group 7 elements decrease as the group develops.
False - B.P increases down the group
85
T/F: (1)
| Cracking is used because of different demands for each hydrocarbon.
True - Petrol is high demand
86
T/F: (1)
| Molecules used in cracking are all hydrocarbons.
True
87
T/F: (1)
| Catalytic cracking uses iron as a catalyst.
False
88
T/F: (1)
| Cracking reactions are addition reactions.
False
89
T/F: (1)
| Cracking produces molecules with shorter chains.
True
90
Explain why magnesium metal is malleable. (2)
(magnesium) ions in layers / rows
| that can slip / slide (over each other).
91
Explain why magnesium metal is a good electricity conductor. (2)
(sea of) delocalised electrons
| that can flow / move through metal.
92
In a reaction, Magnesium is ignited and placed in a jar of oxygen gas.
State two observations that would be made. (2)
Bright / white flame produced.
White solid collects at base
93
Name the state change from; (1)
| Solid to Liquid
melting
94
Name the state change from; (1)
| Liquid to Gas
evaporation
95
Name the state change from; (1)
| Solid to Gas
sublimation
96
What is the name of the equipment piece that that the filter paper fits in? (1)
Filter Funnel
97
Name the industrial process used to separate crude oil. (1)
Fractional Distillation
98
State a use for Kerosene and Bitumen. (2)
Kerosene - Aircraft fuel
| Bitumen - Road surfacing
99
State a catalyst used in the industrial cracking of eicosane. (1)
Silica (Silicon Dioxide);
or
Alumina (Aluminium Oxide).
100
A molecule of the hydrocarbon eicosane has the formula C20 H42.
Explain which homologous series eicosane belongs to. (2)
Alkanes;
| General formula Cn H2n+2.
101
The hydrocarbon eicosane has 20 Carbons, how many Hydrogens does it have? (2)
42;
| Cn H2n+2 -> H (2 x 20) + 2 = 42
102
Suggest what it means if a hydrocarbon is saturated. (1)
The hydrocarbon has no carbon-carbon double bonds.
103
Describe a chemical test used to distinguish between unsaturated and saturated hydrocarbons. (3)
test: Adding bromine water.
result: Decolourisation = alkene (unsaturated);
Stays orange = alkane (saturated).
104
Does the isomer;
| But-3-ene exist?
No: only But-1-ene, and But-2-ene.
105
Substance A and B are both covalently bonded, simple molecular structures. A has a much higher boiling point than B, suggest why. (1)
The molecular mass is greater.
106
Hot, molten sulfur reacts with oxygen to form sulfur dioxide gas.
Describe what is seen when a sample of hot, molten sulfur is lowered into a glass jar containing oxygen. (1)
(bright), blue flame is produced
107
State a use of silica gel. (1)
They are used to dry substances.
108
A sample of sulfur dioxide reacts with water to form an acidic solution.
Identify the acid formation. (1)
Sulfuric Acid
109
Describe how a scientist could make sure all the water has been lost. (2)
Heat the sample until the mass of the sample does not change.
110
Describe how the scientist could use a solution of the salt to find out if the negative ions are chloride ions. (3)
- Nitric acid
- Silver nitrate
- White precipitate
111
Describe how you could use a method of crystallisation to obtain a pure, dry sample of ammonium sulfate from a dilute solution of ammonium sulfate. (4)
- Boil until crystals begin to form;
- Leave to cool;
- Filter;
- Suitable drying method; eg window.
112
Deduce the formula of the compound that is formed when Magnesium (group 2), reacts with Fluorine (halogen). (1)
MgF2
113
SiF4 and SiCl4 have simple molecular structures.
SiO2 has a giant covalent structure.
Explain why the boiling point of SiCl4 is greater than the boiling point of SiF4. (2)
M1) intermolecular forces (of attraction) / forces (of attraction) between molecules;
M2) stronger in SiCl4 /weaker in SiF4.
114
SiF4 and SiCl4 have simple molecular structures.
SiO2 has a giant covalent structure.
Explain why the boiling point of SiO2 is very much greater than the boiling point of SiCl4. (2)
M1 SiO2 has strong covalent bonds (that must be broken);
M2 (whereas) SiCl4 has weak intermolecular forces (of attraction must be overcome).
115
Name the particles that move through the connecting wires to form an electric current. (1)
Electrons
116
The electrodes are made of Platinum, which is an inert metal.
State what is meant by inert. (1)
not (chemically) reactive / does not react (with the electrolytes/with the products of electrolysis)
117
Explain how you know structure B is being presented as a displayed formula. (1)
(because) it shows all the bonds (in the molecule)
118
Explain the meaning of Isomers; (in terms of structure not atomic number).
- (compounds/molecules that have the) same molecular formula;
- (but have) different structural formula (allow displayed).
119
State the full name of the polymer, PVC. (1)
poly(chloroethene) or Polyvinyl Chloride
120
A beaker contains dilute hydrochloric acid.
Litmus indicator is added to the acid.
What is the final colour of the litmus? (1)
Red - Litmus is red in acidic solution.
121
A conical flask contains potassium hydroxide solution.
Litmus indicator is added to this alkaline solution.
What is the final colour of the litmus? (1)
Blue - Litmus is blue in alkaline solution.
122
Name the two particles found in the nucleus. (2)
Proton
| Nuetron
123
State the name given to atoms with the same atomic number but different mass numbers. (1)
Isotopes
124
In a titration between dilute sulfuric acid and sodium hydroxide, what type of reaction occurs? (1)
Neutralisation
125
Ethanol and compound X are members of the homologous series of alcohols.
One property of members of a homologous series is that they have similar chemical reactions.
Give one other property of members of a homologous series. (1)
```
Any one from:
have a general formula
successive members differ by CH2
trends in physical properties
same functional group
```
126
Most chromium is extracted from the ore, chromite, FeCr2O4.
| State the names of all the present elements in chromite. (1)
```
Fe = Iron
Cr = Chromium
O = Oxygen
```
127
Give the formulae of the two ions in LiF. (1)
Li+ and F-
128
Calculate the relative formula mass (Mr) of MgO. (1)
2 x 16 = 32
129
Chlorine is used in the manufacture of the addition polymer poly(chloroethene).
Explain how an addition polymer is formed from its monomers. (2)
M1 monomers join together/ double bonds
broken (in monomers).
M2 to form a long chain (molecule)/large
molecule.
