Outwood Academy Bydales
AWA 2015
Starting CHEMISTRY Revision from Year 10 – Feb 2016
Unit C2 - Additional Science
*This booklet covers ALL Foundation & Higher Content
‘300 Simple Facts to Learn’
Name:
Class:
Chemistry C2 Unit 2 –Recall Questions on EVERY bit of the Syllabus
Part of your revision should be memorising key facts and words from the syllabus, before making sure you can then
applying your understanding to GCSE questions. Test yourself repeatedly on these questions, using friends, family until
you can do them all from memory! Put at least 1-2 hours a week ON TOP of your Science HW to do this.
C.2.1.1. Questions on Structure and Bonding
1. What do we a substance where two or more atoms are chemically combined?
2. Name the type of chemical bonding that involves completely transferring electrons.
3. Name the type of chemical bonding that involves sharing electrons in the outer shells.
4. What do all atoms want their outer shell to be?
5. What group of atoms do all other atoms try to achieve the same electronic structure of?
6. What is the name of the Group 0 gases?
7. When an atom loses or gains electrons, what do we call the resulting particle?
8. What charge does an electron have?
9. What charge do atoms that lose electrons end up with?
10. Is it metal or non-metal atoms that tend to lose electrons?
11. What charge do atoms that gain electrons end up with?
12. Is it metal or non-metal atoms that tend to gain electrons?
13. Do ions have a full outer shell of electrons?
14. What group of atoms in the period table already have full outer shells?
15. What is the name of Group 0 in the periodic table?
16. What charge do ions in Group 1 form?
17. What charge do ions in Group 7 form?
18. What charge do ions in Group 2 form?
19. What charge do ions in Group 6 form?
20. What charge do ions in Group 3 form?
21. What charge do ions in Group 6 form?
22. What is the name of the elements in Group 1?
23. Are Group 1 elements metals or non-metals?
24. Do Group 1 ions have a charge of +1, +2 or +3?
25. What is the name of the elements in Group 7?
26. Are Group 7 elements metals or non-metals?
27. Do Group 7 ions have a charge of -1, -2 or -3?
28. What name do we give to the ions of Group 7?
29. Do Group 7 elements react with Group 1 elements?
30. What do we call the bonding in a compound made of a giant structure of ions?
31. What holds ions together in an ionic structure?
32. Are these forces strong or weak?
33. What do oppositely charged ions do to each other?
34. Do the forces in an ionic compound act in all directions?
35. We call the structure in an ionic compound a ‘giant crystal l________’.
36. What bonds are formed when atoms share pairs of electrons?
37. Do metals or non-metal atoms tend to do this type of bonding?
38. When atoms share a pair of electrons is the bond strong or weak?
39. Most covalently bonded substances form simple ‘m____________’.
40. Some covalently bonded substances form ‘giant c__________ s___________’
41. What is another name for such a structure?
42. Name such a giant structure that involves carbon atoms.
43. Name such a giant structure that involves silicon and oxygen atoms.
44. Do metals from giant structures of atoms arranged in a giant structure?
45. What word describes what happens to the outer shell electrons of metals.
46. What charged ions do the metal atoms therefore form?
47. Can the electrons moves through the whole structure?
48. What property does this (answer to 47.) give to metals?
49. What ‘glues’ the metal ions together in a giant metallic structure?
50. We sometimes call the electrons in a metal a ‘s___ of electrons’.
Some drawing/sketching/working out questions from C2.1.1
You are expected to be able to do all of these from memory, but using the Periodic Table to help.
51. Draw the electron structure of a Sodium ion. (Tip: Na+ proton number = 11)
52. Draw the electron structure of a Chloride ion. (Tip: Cl- proton number = 17)
53. Draw the electron structure of a Magnesium ion. (Tip: Mg2+ proton number = 12)
54. Draw the electron structure of a Oxide ion. (Tip: O2+ proton number = 8)
55. Draw the electron structure of a Calcium ion. (Tip: Ca2+ proton number = 20)
56. Draw an outer orbital overlap diagram showing covalent bonding in water (H2O)
57. Draw an outer orbital overlap diagram showing covalent bonding in ammonia (NH3)
58. Draw an orbital overlap diagram showing covalent bonding in hydrogen chloride (HCl)
59. Draw an outer orbital overlap diagram showing covalent bonding in methane (CH4)
60. Draw an outer orbital overlap diagram showing covalent bonding in oxygen (O2)
61. Sketch a diagram of the bonding in the giant covalent structure of diamond (C)
62. Sketch a diagram of the bonding in the giant covalent structure of silicon dioxide (SiO2)
63. Draw a diagram showing the bonding structure of a metal such as sodium.
C.2.2.1. Questions on Molecules
64. Substances that are simple molecules are made of metal or non-metal atoms?
65. Name the bonding that creates molecules.
66. What three states can simple molecules be?
67. Do simple molecules have relatively low or high melting points?
68. Do simple molecules have relatively low or high boiling points?
69. Are the forces between molecules strong or weak?
70. What is the correct name for these forces between molecules?
71. Is it these forces, or the covalent bonds, that are overcome when a substance melts?
72. Do substances made of simple molecules conduct electricity?
73. Do molecules have an overall electric charge, like ions?
C.2.2.2. Questions on Ionic Compounds
74. Are ionic compound structures regular or irregular?
75. Name the forces in all directions in a giant ionic lattice.
76. Do ionic compounds have high or low melting points?
77. Do ionic compounds have high or low boiling points?
78. Are ionic compounds generally solid, liquid or gas at room temperature?
79. Are the electrostatic forces in an ionic solid strong or weak?
80. Describe the amount of energy needed to break these bonds in an ionic compound.
81. Can ionic compounds be dissolved in water?
82. Does it require lots of energy to melt an ionic compound and make it molten?
83. Are ions free to move when ionic compounds are dissolved or molten?
84. Do ionic compounds conduct electricity when molten or dissolved in water?
85. What carries the current in a dissolved or molten ionic compound?
C.2.2.3. Questions on Covalent Structures
86. Can atoms that share electrons also form giant structures?
87. Give another name for a giant covalent structure.
88. What two forms of carbon form giant covalent structures?
89. What is another name for silicon dioxide, that forms a giant covalent structure?
90. Another name for the structure part is a l_________.
91. Are the covalent bonds in a giant covalent structure strong?
92. Are all the atoms in a giant covalent lattice linked to other atoms?
93. Is the melting point of a giant covalent structure high or low?
94. Is the boiling point of a giant covalent structure high or low?
95. In diamond, how many covalent bonds does each carbon atom form with other carbons?
96. Because of this, is diamond hard or soft?
97. In graphite, how many covalent bonds does each carbon atom form with other carbons?
98. What does graphite form that can slide over each other?
99. Are there covalent bonds between these l______ in graphite?
100. Is graphite soft and slippery, or hard and rigid?
101. What are delocalised between the layers of carbon atoms in graphite?
102. What two things can these delocalised electrons conduct in graphite?
103. What other kind of bonding is graphite similar to, in terms of delocalised electrons?
104. Do fullerenes have different numbers of carbon atoms?
105. What can fullerenes deliver into the body?
106. What can fullerenes act as, to speed up reactions by lowering activation energy?
107. What can fullerenes act as, in between moving parts of engines?
108. What do we call the structures of fullerenes that can act as strengtheners?
109. Name a sport that has its rackets reinforced by fullerenes.
110. What shape polygon are fullerene carbon atom rings arranged in?
C.2.2.4. Questions on Metals
111. What two things can metals conduct?
112. It is due to delocalised what that allows metals to conduct?
113. Can the layers of atoms in metals slide over each other?
114. Because of this, what two things can metals do without breaking?
115. What do we call substances made from two or more metals?
116. What do the different sized atoms of the different metals do to the layers in these?
117. Is it easier or harder for the layers to slide over each other with this happening?
118. Are alloys harder or softer than pure metals?
119. What do we call alloys that can return to their original shape after being deformed?
120. Name the alloy specifically mentioned in the syllabus that can do this.
121. What device are such alloys used in?
C.2.2.5. Questions on Polymers
122. What two things can affect the properties of polymers?
123. What is the full name of LD poly(ethene)?
124. What is the full name of HD poly(ethene)?
125. What can you say about the reaction conditions when these two polymers are made?
126. What can you say about the catalysts used when these two polymers are made?
127. What word describes how thermosetting polymer chains are arranged together.
128. What are formed between the polymer chains in thermosetting polymers?
129. Which type of polymers do melt when heated?
130. Which type of polymers do not melt when heated?
131. What do we call the forces between polymer chains in thermosoftening polymers?
132. Are these forces strong or weak in thermosoftening plastics?
133. Do these forces make thermosoftening plastics have low or high melting points?
C.2.2.5. Questions on Nanoscience
134. Nanoscience structures have a size between 1 and how many nanometres? (nm)
135. Are nanoscience structures in the order of a few hundred, thousand or million atoms?
136. Do nanoparticles have different or similar properties to the same materials in bulk?
137. Does ‘bulk’ mean large quantities or small quantities?
138. Do nanoscience structures have a high or low surface area to volume ratio?
139. What electronic devices could be developed by nanoscience?
140. What industrial agents that lower activation energy might be developed by nanoscience?
141. What two useful properties might construction materials become with nanoscience?
142. Can nanoscience be used to develop new coatings on materials?
143. Give two cosmetics that nanoscience could be used to develop.
C.2.3.1 Questions on Atomic Structure
144. In the periodic table, what is the name of the top number against an atom’s symbol?
145. In the periodic table, what is the name of the bottom number against an atom’s symbol?
146. What is the other name of the bottom number against an atom’s symbol?
147. What is the relative mass of a proton?
148. What is the relative mass of an electron?
149. What is the relative mass of a neutron?
150. What two particles make up the nucleus of an atom?
151. What do we call the total number of protons and neutrons in an atom?
152. What do we call different ‘versions’ of the same element?
153. What is the only thing different about these different ‘versions’ of an atom?
154. The relative atomic mass of all atoms is compared with a twelveth of which element?
155. Which isotope of that element is the one used for this comparison?
156. What is the correct name for the weight of an atom?
157. What is the correct name for the weight of a compound?
158. What do you add together to get the relative formula mass of a compound?
159. What is Ar short for?
160. What is Mr short for?
161. What animal do we call the relative formula mass of a substance in grams?
C.2.3.2 Questions on Analysing Substances
162. What ‘d’ can instrumental methods do with regard to trace elements and compounds?
163. What ‘i’ can instrumental methods do with regard to unknown elements & compounds?
164. What three advantages are there of instrumental methods for detecting substances?
165. Instrumental methods are advantageous when samples are very small or very large?
166. What can chemical analysis detect in foods?
167. What type of chromatography can detect artificial colours in foods?
168. What does GC-MS stand for?
169. What does gas chromatography allow the separation of?
170. What is measured as a substance moves through the column in gas chromatography?
171. What part of the gas chromatography column is linked to a mass spectrometer?
172. What does a mass spectrometer do to substances leaving the end of the G-C column?
173. What is the gas chromatography column packed with?
174. What does the number of peaks on the output of a gas chromatograph show?
175. What does the position of the peaks on the output of a gas chromatograph show?
176. Give two advantages of a mass spectrometer with regard to gas chromatography.
177. Apart from identifying substances separated by the column, was else can a mass
spectrometer give with regard to separated substances using G-C?
178. What part of the chromatograph shows the molecular mass of separated substances?
C.2.3.3 Questions on Quantitative Chemistry
179. Can atoms be lost or gained in a chemical reaction?
180. What can happen to some of a product when it is separated from the reaction mixture?
181. What do we call a reaction that does not go to completion?
182. What do we call the ‘amount of product obtained’ in a chemical reaction?
183. What do we call the ‘amount of product compared with the maximum theoretical
yield’?
184. What do we call a reaction where some of the products can react to produce the
original reactants?
C.2.4 Questions on Rates of Reaction
185. Complete: Rate of reaction = amount of reactant used / ?
186. Complete: Rate of reaction = amount of product formed / ?
187. For a reaction to occur, the reacting particles much have sufficient e_________?
188. For a reaction to occur, the reacting particles must c________ with each other.
189. What is the specific name of the minimum energy needed by particles in order to react?
190. What does increasing temperature do to the speed of reacting particles?
191. What does increasing temperature do to the energy of reacting particles?
192. Does increasing temperature make particles collide more or less often?
193. Does increasing temperature therefore increase or decrease the rate of a reaction?
194. What does increasing the pressure do to the frequency of collisions in reacting gases?
195. Does increasing pressure of gases therefore increase or decrease the rate of reaction?
196. What does increasing the concentration of a solution do to the frequency of collisions?
197. Does increasing concentration therefore increase of decrease the rate of reaction?
198. What does increasing surface area of a solid reactant do to the number of collisions?
199. Does increasing surface area increase or decrease the rate of a reaction?
200. What do we call a substance that speeds up a reaction but is not used up?
201. Do different reactions need similar or different catalysts?
202. Do catalysts increase or decrease the rates of industrial reactions?
203. What can catalysts reduce in industrial reactions (that is beneficial!)
C.2.5.1 Questions on Energy Transfer in Chemical Reactions
204. What do we call a reaction where energy is transferred to the surroundings?
205. What do we call a reaction where energy is taken in from the surroundings?
206. Is combustion an example of an exothermic or endothermic reaction?
207. Is oxidation an example of an exothermic or endothermic reaction?
208. Is neutralisation an example of an exothermic or endothermic reaction?
209. Give an example of a food that is cooked by a self-heating can?
210. Does a self-heating can use an exothermic or endothermic reaction?
211. What part of the body can be kept warm by an exothermic reaction when on a trek?
212. Is thermal decomposition an example of an exothermic or endothermic reaction?
213. In the medical room, what might be used that involves an endothermic reaction?
214. If a reversible reaction is exothermic in one direction, what is it in the other direction?
215. Is the same amount of energy transferred in both directions in a reversible reaction?
C.2.6.1 Questions on Making Salts
216. What is represented by the state symbol (s)?
217. What is represented by the state symbol (g)?
218. What is represented by the state symbol (aq)?
219. What is represented by the state symbol (l)?
220. Can soluble salts be made by reacting acids with metals?
221. Do all metals react with acids to form soluble salts?
222. Name a metal that is too reactive for making salts with acids.
223. Name a metal that is not reactive enough for making salts with acids.
224. What do we call the opposite of an acid?
225. What type of base is added to an acid to make a salt, where it is filtered off as an
excess?
226. What do we call a soluble base?
227. What is used when reacting acids & alkalis, to show that they have completely reacted?
228. What word describes what is done to a salt solution, to create a solid salt.
229. Are insoluble salts made by mixing soluble or insoluble solutions of ions together?
230. What do we call an insoluble salt that ‘appears’ from a solution when mixing ions?
231. What type of water has unwanted ions removed from it by precipitation?
232. What do we call waste water from industry or sewage? (Clue: e______________)
C.2.6.2 Questions on Acids and Bases.
233. Hydroxides and metal o_______s are know an bases.
234. What are bases the ‘opposite’ of?
235.Give an example of soluble bases.
236. Name the surname of a salt produced using hydrochloric acid.
237. Name the surname of a salt produced using nitric acid.
238. Name the surname of a salt produced using sulphuric acid.
239. What gives the forename of a salt, when mixing acids and bases, a metal or non-metal?
240. Does ammonia gas dissolve in water to form an acid or alkaline solution?
241. Give the forename of a salt produced when ammonia solution is neutralised?
242. In farming, what are ammonium salts used as?
243. What do we call the scale that identifies acids and bases?
244. What is the pH of a neutral solution?
245. Is pH0 a strong or weak acid?
246. Is pH14 a strong or weak alkali?
247. Is pH6 a strong or weak acid or alkali?
248. Is pH8 a strong or weak acid or alkali?
249. What ions make a solution acidic?
250. What ions make a solution alkaline?
251. What is the name of this ion OH- ?
252. What is the name of this ion H+ ?
253. Which ion makes a solution alkaline, OH- or H+ ?
254. What do we call a reaction where hydrogen ions react with hydroxide ions?
255. Apart from a salt, what else is always made when acids react with alkalis?
256. Complete this neutralisation:
H+ (aq) + _______ (aq)  ______ (1)
C.2.7.1 Questions on Electrolyis
257. What type of bonding only conducts when molten or dissolved in water?
258. What are free to move about when this melting or dissolving happens?
259. What do we call a melted substance, a liquid or a solution?
260. What do we called a dissolved substance, a liquid or a solution?
261. What is passed through a molten ionic substance to break it into its elements?
262. What is passed through a solution of ionic substance to break it into its elements?
263. What do we call the process of breaking down a substance in this way?
264. What is the name given to any substance being broken down by electrolysis?
265. If lead bromide is molten, and electricity passed through, what elements are produced?
266. What charge do metal ions have in a solution or molten liquid?
267. What charge do non-metal ions have in a solution or molten liquid?
268. Which charged ions move to a negative electrode?
269. Which charged ions move to a positive electrode?
270. Give the names of two metals used to coat objects using electrolysis.
271. This coating of metals using electrolysis is sometime know as what?
272. At the negative electrode, do positive ions gain or lose electrons?
273. At the positive electrode, do negative ions gain or lose electrons?
274. Name a drilling platform at sea that can help remember about oxidation/reduction.
275. Is losing electrons at an electrode oxidation or reduction?
276. Is gaining electrons at an electrode oxidation or reduction?
277. If there is a mixture of ions, what determines which ion will go to an electrode?
278. Balance this:
____Cl- 
Cl2 + _____e-
279. Balance this:
____H+ + _____ e- 
280. Balance this:
____Cl- - _____e- 
H2
Cl2
281. What do we call the compound that aluminium is obtained from by electrolysis?
282. What substance is added to reduce the melting point in aluminium production?
283. Reducing the melting point during aluminium production also reduces what?
284. What is another word for something that has been melted, and is very hot?
285. In aluminium oxide, what charge do aluminium ions have?
286. In aluminium oxide, what charge do oxide ions have?
287. In the electrolysis of aluminium oxide, name the ion that goes to the negative electrode.
288. In the electrolysis of aluminium oxide, name the ion that goes to the positive electrode.
289. In aluminium production, what are the electrodes made from?
290. What element reacts with these electrodes during aluminium oxide electrolysis?
291. Does this happen at the positive or negative electrode?
292. What new gas is produced at the electrode when it reacts with the element produced
there?
293. What compound from the sea when electrolysed produces hydrogen and chlorine?
294. In sea water electrolysis, what ions get to the positive electrode?
295. In sea water electrolysis, which ions don’t make it to the positive electrode?
296. In sea water electrolysis, what ions get to the negative electrode?
297. In sea water electrolysis, which ions don’t make it to the negative electrode?
298. What solution is left behind during electrolysis of sodium chloride solution?
299. Name two products made from chlorine that is obtained from salt water electrolysis.
300. What is sodium hydroxide used in the manufacture of?
Now Mark, Correct in Red, and LEARN THEM!