Chemistry 2
Structure and bonding
1. What is ionic bonding?
2. Between which groups on the periodic
table does it occur?
3. What does the receiver form?
4. What does the giver form?
5. How are they held together?
6. Give an example of a giant ionic lattice
7. Why is a lot of energy required to break
up a giant ionic structure?
8. In the liquid state, molten or dissolved in
water they can do what?
9. Complete this: solid ionic compounds are
….. in a …… They vibrate but ….. move
around so ….. conduct ……
10. Complete this: ………. Ionic Compounds
are where high ….. provide …. to
overcome strong ….between ions. They
can …… so ….. electricity
11. Ionic compounds in a …… separate away
from the …… because of ….moleculees,
enabling them to ……around the …….
12. How are covalent bonds formed?
13. Between which groups does it occur?
14. What are simple molecules? Give three
examples
15. Why don’t they conduct electricity?
16. What are giant covalent structures?
17. What is diamond? Describe its structure
18. What is graphite? Describe its structure?
19. What is silicon dioxide?
20. What are giant metallic structures?
21. why are they malleable?
22. What are alloys?
23. How do they affect the properties in
terms of atoms?
24. How does liquid nitrogen cool metals?
What can they be used for?
25. When did chemists discover carbon
cages?
26. What are they called?
27. State three things that have been made
up of (answer to 26)
28. What is nanoscience?
29. State four ways that nanoscience can be
used to improve every day lives.
30. What are monomers?
31. How are low density polymers formed?
32. How are high density polymers formed?
33. What are thermosoftening polymers?
34. What are thermosetting polymers?
Rates of Reaction
35. How can the rate of chemical reaction be
found?
36. What equation can be use to represent
this?
37. When do chemical reactions occur?
38. What is activation energy?
39. If the reactants produce a gas what
happens to the mass?
40. What can measure the volume of gas
evolved?
41. If a cloud precipitate is formed what is
timed?
42. What will happen to particles if
temperature is increased?
43. What will happen to particles if pressure
increases?
44. What happens to collisions if there is an
increase in surface area?
45. Draw a graph showing A) a farily slow
reacition b) a quicker reaction but the
same initial amounts c) more product and
an increased rate
46. What are catalysts?
47. Give three examples of different catalysts
used in industry – not enzymes.
48. What happens to the surroundings in an
endothermic reaction? Why?
49. Give three examples of an endothermic
reaction
50. What happens to the surroundings in an
exothermic reaction? Why?
51. Give three examples of an exothermic
reaction
52. Show a reversible reaction of copper
sulphate
Atoms and Quantitative Chemistry
53. What is a positive particle in an atom’s
nucleus? What is its mass?
54. What is a neutral particle in an atom’s
nucleus? What is its mass?
55. What is a negative subatomic particle in
an atom’s energy shell called? What is its
mass?
56. What is the atomic number?
57. What is the mass number?
58. What is meant by the relative atomic
mass?
59. What are the relative atomic masses of a)
hydrogen, b)helium, c)nitrogen, d)oxygen,
d)iron
60. What is the relative formula/molecular
mass of a compound?
61. What is the relative formula mass of
ammonia?
62. What is a mole?
63. What is 1 mole of a) carbon, b)oxygen
atom, c)iron, d)potassium, e)calcium,
f)argon
64. What is half a mole of a)water, b)carbon
dioxide, c)ammonia, d)potassium
chloride?
65. What is the formula for working out the
total number of moles?
66. What is the formula for working out the
percentage of an element in a
compound?
67. What is the formula for working out
percentage yield?
68. What is meant by the term ‘isotope’
69. Why isn’t it always possible to obtain
calculated amounts?
70. What is the empirical formula?
71. Use the empirical formula to work out a)
copper oxide, b)sodium hydroxide
c)water
72. What is a reversible reaction?
73. What is gas chromatography?
74. How does it work?
75. Why do compounds in a mixture dissolve
better than ones in a solvent?
76. What are the advantages and
disadvantages of instrumental analysis?
Acids and Alkalis
77. Give four examples of an acid
78. Give four examples of a base
79. Give three examples of neutral solutions
80. If a substance is dissolved in water what is
it called?
81. What are soluble hydroxides known as?
82. What do acids form when added to
water?
83. What do soluble hydroxides form when
added to water?
84. Is pH higher further up the scale or lower?
85. Which indicator is used for showing this?
86. An acid + metal forms what? Give an
example using magnesium chloride and
hydrogen
87. An acid+base forms what? Give an
example using sulphuric acid and
magnesium oxide
88. An acid+alkali forms what? Give an
example using nitric acid and sodium
hydroxide
89. An acid+carbonate forms what? Give an
example using hydrochloric acid and
calcium carbonate
90. What do some acids and alkalis form
when they react?
91. Ammonium nitrates are formed by what?
92. What are ammonia salts used for and
how are they made?
93. If two solutions of soluble salts are added
to water what is formed?
94. In the example lead nitrate + potassium
iodide which are the isoluble salts?
Electrolysis
95. What is electrolysis?
96. What are electrodes?
97. To which electrode does a) cation b)anion
move to? Why?
98. Upon heating what happens to an ionic
substance?
99. Why may products vary?
100. What is oxidation? Give an example
101. What is reduction? Give an example
102. In an aqueous solution if two elements
can be produced at an electrode will the
more reactive or less reactive element
from?
103. At a positive electrode hydroxide ions are
usually discharged to form what?
104. When is this not the case?
105. What is electroplating?
106. Why is it done?
107. Describe the process of manufacturing
aluminium
108. What can sodium hydroxide and chlorine
be used for?
Chemistry 3
Periodic table
1. Who was John Dalton?
2. In which year did John Newlands build on
Dalton’s ideas?
3. Why was Newland’s theory flawed? Give
two reasons
4. Who was Dimitri Mendeleev and what did
he do?
5. Whose idea is the modern periodic table
based on?
6. How are they different?
7. How are elements organised?
8. What are group 1 elements known as?
9. What charged ions do they form?
10. What are their four properties?
11. Where are the transition elements found?
12. What are their densities like compared to
group 1 elements?
13. What are their properties like compared
to group 1 elements?
14. Give an example of a coloured compound
15. Which elements in this section can form
different ions?
16. What are group 7 elements known as?
17. What charged ions do they form?
18. What are their four properties?
Water
19. What does soft water form when
combined with soap?
20. What does hard water form when
combined with soap?
21. What is scale?
22. What is scum?
23. Do soapless detergents form scum and
scale?
24. Which ions does hard water contain?
25. What is gypsum?
26. Is calcium carbonate soluble in water?
27. Is calcium carbonate soluble in slightly
acidic water?
28. If these ions are removed what can soap
form?
29. What else does hard water cause
problems in? What are the effects?
30. What is temporary hardness?
31. How can it be removed?
32. Why can’t permanently hard water be
softened by boiling?
33. How can it be softened?
34. What is ion exchange resin?
35. What are the advantages and
disadvantages of hard water?
36. What does the solubility of a solute in
water depend on?
37. What is a substances solubility?
38. What is wrong with drinking distilled
water?
39. Describe the process of sedimentation
40. Describe the process of filtration
41. Describe the process of disinfection
42. What is a home filter jug used for?
43. Discuss the advantages and disadvantages
of using fluoride ions in water treatment?
Energy from Reactions
44. How can the relative amount of energy
released when a substance burns be
measured?
45. What does each letter stand for in the
formula Q=MxCxΔT
46. How can energy transfer be reduced in a
polystyrene cup?
47. In an exothermic reaction are products at
a lower energy level than the
surroundings or a higher energy level?
Why?
48. In an endothermic reaction are products
at a lower energy level than the
surroundings or a higher energy level?
Why?
49. Does a catalyst increase or decrease
activation energy?
50. If energy change = Δproducts –
Δreactants, work out the answer of N2 (g)
+ 3H2 (g) – 2NH3 (g)
51. What can be used as an alternative to
fuel?
52. What can fuel cells be fed with to produce
water and energy to power vehicles?
53. What needs to be matched to compare
these fuels with petrol?
Titrations
54. What are added together in a conical flask
in a neutralisation reaction with
phenolphthalein insulator?
55. Why is a biuret used?
56. 1dm3 = how many cm3?
57. What is the formula for the number of
moles ina solution?
58. In which areas of industry are unknown
substances needed to be analysed? Give
at least three
59. What colour do the metal ions in a flame
of a) lithium b) sodium c) potassium )d)
calcium e)borium f)magnesium turn?
60. Precipitation reactions of sodium
hydroxide turn a) aluminium ions b)
calcium ions c) magnesium ions d) iron 2+
ions e) iron 3+ ions f) copper ions into
what?
61. What do carbonate ions react with to
form carbon dioxide?
62. Sulphate ions in……produce a …..
precipitate in ….. chloride in
……hydrochloric……
63. Halide ions in a solution produce what
with silver nitrates in the presence of
what? what colour does a)silver chloride
b)silver bromide c)silver iodide turn?
64. If the concentration of the reactant is
unknown, how can the results be found
out?
Ammonia
65. What is equilibrium?
66. Where does equilibrium occur?
67. What is a closed system?
68. Are the reactions still taking place?
69. In a reversible reaction what does the
position of equilibrium depend on?
70. If temperature is raised what will happen
to the a)endothermic b)exothermic
reaction yield?
71. If temperature is lowered what will
happen to the a)endothermic
b)exothermic reaction yield?
72. If pressure is raised will the reaction
which produces less volume or more
volume be encouraged?
73. If pressure is lowered will the reaction
which produces less volume or more
volume be encouraged?
74. What happens to a reaction if a catalyst is
added?
75. What are the raw materials for the Haber
process and how are they obtained?
76. What type of catalyst is needed for the
Haber process?
77. What are the ideal conditions?
78. Do higher pressures favour the forward or
backward reaction?
79. Why is pressure set as high as possible,
but why is temperature not?
80. What is the problem with lower
temperatures?
81. Why is 450® chosen?
82. What would happen to the reaction
without the catalyst?
Alcohols, esters and carboxylic acids
83. What is the general formula for the
structure of an alcohol?
84. What are the first three homologous
alcohols?
85. What are their properties?
86. They dissolve in water to form what?
87. How is ethanol produced and what is its
most popular use?
88. Whare are methylated spirits used for?
89. If there is more ethanol in a fuel is there
more or less pollution formed?
90. How can ethanol be oxidised? State two
ways
91. What is the general formula for the
structure of a carboxylic acid?
92. When dissolved in water they form what?
93. Why are they known as weak acids?
94. What is the difference between strength
and concentration?
95. What can carboxylic acids with longer
chains form?
96. How are esters formed and what is their
functional group?
97. What are their properties?
98. Complete this example: ethanol+ethanoic
acid - ….
99. What are they commonly used for?
100. Why do some esters cause ethical issues?