C1 - Knowledge Test

Candidate Name:
1) What are the three states of matter?
2) How are the three states of nmatter represented when using solid spheres to represent particles?
3) What happens to a substance as it changes from a solid to a liquid?
4) Why do different substances have different melting and boiling points?
5) What are the limitations to using simple particle models used to represent the different states of matter?
6) What state would substance A be at room temperature (25oC) when substance A has a melting point of -10oC and a boiling point of 55oC?
7) Why does water boil at 100oC rather than 90oC, in terms of bonding and energy transfers?
8) (HT) What are the limitations of the particle theory in relation to changes of state?
9) What is the smallest part of an element that can exist?
10) How are atoms of elements represented on the periodic table?
11) How many different elements are there?
12) How are compounds formed?
13) How can chemical reactions be detected other than through the observation of new substances forming?
14) What is a compound and how is it respresented?
15) What type of reaction is needed to separate a compound into elements?
16) How are chemical reactions represented?
17) What are the names and symbols of elements in Groups 1 and 7?
18) What are the names of the following compounds: NaCl, KF, LiBr?
19) In a chemical equation, what do the symbols (s), (l), (g), and (aq) represent?
20) What state symbols are added to each part of the chemical equation below? C O2 -> CO2
21) What is a mixture?
22) What happens to the chemical properties of each substance in a mixture?
23) When mixtures are separated by physical processes how does this affect the chemical reactions and substances made?
24) How are mixtures separated using filtration?
25) How are mixtures separated using crystallisation?
26) How are mixtures separated using simple distillation?
27) How are mixtures separated using fractional distillation?
28) How are mixtures separated using chromatography?
29) How could we separare a mixture of sand, salt, iron and water into its individual components?
30) What can lead to a scientific model being changed or replace?
31) What is an atom?
32) What were the main features of the 'plum pudding' model of the atom?
33) How did the 'plum pudding' model describe the structure of an atom?
34) How did the Rutherford's alpha particle scattering experiment change our understanding of the structure of the atom?
35) What contribution did Niels-Bohr make in furthering our understanding of the structure of the atom.
36) Which subatomic particle gives the nucleus of the atom a positive charge?
37) What discovery did James Chadwick make that advanced our understanding of the structure of an atom?
38) How did the evidence of alpha particles scattering lead to a change in the atomic model?
39) Describe the currently accepted structure of the atom
40) What are the relative electrical charges of each sub-atomic particle?
41) Why do atoms have no overall charge?
42) If an atom has 9 protons, how many electrons would it have?
43) What does the atomic number of an element tell us?
44) What do all atoms of a particular element have in common?
45) What are the differences between an atom of Nitrogen and an atom of Carbon. What is it that makes them unique elements?
46) How does the current nuclear model describe an atom?
47) How large is the radius of the nucleus of an atom in comparison to its total radius?
48) Where is the majority of the mass of the atom found?
49) What are the relative masses of each subatomic particle (proton, neutron and electron)?
50) What does the mass number of an atom tell us about that atom?
51) What is an isotope?
52) What do the individual tiles of the periodic table tell us?
53) Calculate the number of protons, neutrons and electrons in an atom of Cobalt. Mass number = 59 and Atomic number = 27
54) How large are atoms? a) 1 × 10-6 m b) 1 × 10-8 m c) 1 × 10-10 m
55) Why does chlorine have a mass number of 35.5?
56) What is the relative atomic mass of bromine where there are two isotopes of Bromine, 50% Br-79 and 50% Br-81?
57) What is the maximum number of electrons that can be held by each of the three inner most shells?
58) What would a diagram of the electron structure of an atom of carbon look like?
59) Why is carbon found in group 4 of the periodic table?
60) How big is the total radius of an average atom?
61) How are elements ordered in the periodic table?
62) Metals react to form __________ charged ions
63) In terms of electron structure, how are elements in the same group similar?
64) Non-metals react to form __________ charged ions
65) What does the group and period of an element tell us about its electron structure?
66) Are there more metals or non-metal elements on the periodic table?
67) Predict how the reactivity of caesium would compare to lithium
68) How were elements in early periodic tables ordered?
69) Why were early attempts at ordering the periodic table by atomic mass unsuccessful?
70) How did Mendeleev predict the existence of several undiscovered elements when designing his periodic table?
71) How are metals and non-metal elements arranged on the periodic table
72) What steps were involved in the development of the periodic table?
73) Which group of the periodic table are also named the nobel gases?
74) Describe in terms of electron structure as to why all of the nobel gases are unreactive
75) What is the same about the electron structure for all elements in Group 0 (noble gases)?
76) Describe the trend in boiling point down group 0
77) What is the common name given to the group 1 elements?
78) Give 4 common properties of transition metal elements.
79) Write a word equation for the reaction of sodium with chlorine.
80) Describe the trend in reactivity in group 1 as you go down the group
81) For elements in Group 1, what do the properties depend on?
82) Explain why elements become more reactive the further you go down group 1
83) What are the transition elements?
84) Compare the properties of transition metal elements with those of the group 1 elements.
85) Give examples of 3 transition metals
86) What is the common name given to the group 7 elements?
87) Describe the trend in boiling point and melting point of elements as you go down group 7?
88) Describe the trend in reactivity of elements as you go down group 7?
89) Write a word equation for the reaction between sodium chloride and fluorine. What type of reaction is this?
90) In terms of electron structure, whAt do all group 7 elements share in common?
91) List the elements of group 7 in order of reactivity.
92) Many transition elements are also useful as catalysts. What is a catalyst?
93) List the general properties of compounds of transition elements
94) How can different atoms interact with each to gain a full outer shell of electrons.
95) What are the three types of chemical bonding?
96) Name the type of attraction between particles in an ionic bond
97) In terms of electrons, how are covalent bonds formed?
98) Metallic bonds have delocalised electrons. What are delocalised electrons?
99) Ionic bonding occurs in compounds formed from ________ combined with ___________.
100) Covalent bonding occurs when _____________ atoms bond together.
101) Metallic bonding occurs between atoms of __________ elements.
102) What is chemical bonding?
103) Describe the transfer of electrons in an ionic bond
104) When a metal atom become an ion it loses electrons. How does this effect its charge?
105) When a non-metal atom bonds ionically it gains electrons. How does this effect its charge?
106) What is the electronic structure of ions produced by group 1,2 metals and group 6,7 non metals?
107) How could you show the formation of an ionic compound using a dot and cross diagram?
108) Draw a dot cross diagram to show the ionic bond in sodium chloride.
109) What charge do ions of elements from the following groups form 1) Group 1 2) Group 2 3) Group 6 4) Group 7
110) Explain why potassium chloride is KCl but potassium oxide is K2O
111) What is an ionic compound?
112) What do we call the attraction between oppositely charged ions?
113) Describe the structure of a giant ionic lattice.
114) What two models can be used to represent giant ionic structures?
115) Give a limitation of each the ball and stick model and charged ion ionic lattice models for representing ionic bonds.
116) Determine the empirical formulae of a compound given the ions: a) Na+ and N3- b) Al3+ and O2-
117) Draw out a dot cross diagram to show the ionic bond formed in the compound sodium chloride.
118) What are covalent bonds?
119) What type of substances have covalent bonds?
120) What are the names of the following substances CO2 H2O H2 Cl2
121) Give an example of large molecules with covalent bonds
122) Give two examples of substances that have giant covalent structures
123) List three ways to represent covalent bonds in molecules
124) How are polymers commonly represented?
125) Draw dot and cross diagrams for the molecules of hydrogen, chlorine, oxygen, nitrogen, hydrogen chloride, water, ammonia and methane look like?
126) How would you draw a single covalent bond?
127) What are the limitations of using dot and cross, ball and stick, 2D and 3D diagrams to represent substances?
128) What is the structure of a metal like?
129) How are the electrons in the outer shell of metal atoms arranged?
130) Why are metallic bonds so strong?
131) Describe the structure of metallic bonding?
132) When compared with the properties of materials, do atoms have the same bulk properties?
133) 1. How do a metal and non-metal bond? 2. How do two non-metals bond?
134) Why are metals good conductors of electricity?
135) In pure metals atoms are arranged in layers. What property does this give them?
136) Why are metals good conductors of thermal energy?
137) Why are pure metals often mixed with other metals or carbon?
138) Why are alloys harder than pure metals?
139) Describe the structure of an ionic compound?
140) Explain why ionic compounds have high melting and boiling points?
141) Under what conditions are ionic compounds able to conduct electricity?
142) What are the structures of different ionic compounds?
143) Substances that consist of small molecules are most commonly which states of matter at room temperature?
144) How does the size of a molecule affect the size of its intermolecular force?
145) Explain why substances that consist of small molecules often have low boiling and melting points
146) Why are covalent compounds unable to conduct electricity?
147) What is the difference between intermolecular forces and intramolecular forces?
148) Which is stronger: A covalent bond or intermolecular force?
149) Why is diamond so hard, in terms of its structure and bonding?
150) Why do metals tend to have high melting and boiling points?
151) How many bonds does each carbon atom form in graphite and how does this impact it's structure?
152) What happens to the spare electron that remains unused in a covalent bond in graphite?
153) Why do giant covalent structures have very high melting and boiling points?
154) Why is graphite soft and slippery?
155) How is graphite similar to metals?
156) What makes graphene useful in electronics and composites?
157) What are the properties of carbon nanotubes and what do their properties make them useful for?
158) What are the properties of graphene in terms of its structure and bonding?
159) What are fullerenes and what is their structure?
160) Name three uses of fullerenes?
161) Diamond, graphite and fullerenes are all examples of what type of structure?
162) How many bonds can an individual atom of carbon form? How many bonds does each carbon form in an atom of a) Diamond b) Graphite
163) Molecules of diamond, graphite and fullerenes are all held together by what type of bonds?
164) Which giant covalent structures are made only from carbon?
165) What was the first fullerene to be discovered and what is its shape?
166) What sort of structures does nanoscience refer to?
167) What is the size of a fine particle and which is smaller, nanoparticles or fine particles?
168) What is the diameter of coarse particles, such as dust?
169) What happens to the size of the surface area to volume ratio of a cube is you decrease the size of the sides by a factor or 10?
170) Why are the properties of nanoparticles different from those for the same materials in bulk?
171) How do nanoparticles compare in size to individual atoms?
172) What are the main applications of nanoparticles?
173) What are the advantages and disadvantages of using nanoparticles?
174) What sort of molecules are polymers?
175) What two monomers form polyester?
176) What type of bond links individual monomers together when forming a polymer?
177) What type of hydrocarbons are used to make polymers?
178) Why are polymers solids at room temperature?
179) What happens in an addition polymerisation reaction?
180) How is a polymer of poly(ethene) produced from ethene? (Show using a diagram)
181) (Chem only) How is the structure of the repeated unit of an addition polymer related to the monomer?
182) (Chem only) How can you identify if you have a polymer or a monomer structure?
183) (Chem only) What occurs during a condensation polymersiation reaction?
184) (Chem only) How many functional groups does each monomer have in the simplest condensation polymerisation reactions?
185) (Chem only) What are the basic principles of condensation polymersiation? (refer to functional groups and repeating units in your answer)
186) (Chem only) When does condensation polymerisation occur?
187) (Chem only) What are the monomers that form the following naturally occuring polymers? 1. proteins 2. starch 3. cellulose
188) (Chem only) What type of polymerisation reaction occurs when amino acids react to form polypeptides? (Include a reason why)
189) (Chem only) What would the equation looks like for the polymerisation of glycine?
190) (Chem only) How are proteins an example of a condensation polymer?
191) (Chem only) What is DNA and what is its function?
192) (Chem only) Why is the structure of DNA described as a polymer?
193) (Chem only) What are the other naturally occuring polymers that are important for life processes?
194) What is the law of the conservation of mass?
195) Why must we ensure that chemical equations are balanced?
196) What do the multipliers in normal script before a chemical formula represent? Eg 2MgO
197) How do we calculate the relative formula mass (Mr) of a compound?
198) Why must the total relative formula mass of all of the reactants equal that of all of the products made?
199) When a gas is produced in a chemical reaction, why would the mass of the products appear to be less than that of the reactants?
200) Explain why in the reaction below the mass of the products would be greater than that of the reactants 2Mg (s) O2 (g) -> 2MgO (s)
201) What does the term uncertainty mean?
202) How would you represent the distrubtion of results to make estimations of uncertainty?
203) A pippette has an uncertainty of /-0.01mL. It is used three times in a practical. What is the mean measure of uncertainty?
204) (HT only) Chemical amounts are measured in moles. What is the symbol of the unit for moles?
205) (HT only)How can we calculate the mass of one mole of a substance?
206) (HT only)If you have one mole each of two different substances, what will they share in common?
207) (HT only)What does Avogadro's constant represent?
208) (HT only)What is the value of Avogadro's constant?
209) (HT only)Would there be any difference in the number of atoms in one mole of carbon (C) compared with the number of one mole of molecules of carbon dioxide (CO2)?
210) (HT only)Calculate the mass of one mole of C2H6
211) What units are used for the measurement of concentration of a solution?
212) What is the concentration of a solution that has 37g of solute dissolved in 100cm3? Give your answer in dm3.
213) (HT only) What is the equation that relates the mass of a solute, the volume of a solution and the concentration of the solution?
214) Why industrially is high atom economy important?
215) (HT only)Balance the equation and calculate the mass of the reactants and products of the balanced symbol equation: H2O2 --> H20 02
216) (HT only)In the following equation: Mg 2HCI --> MgCI2 H2 What is the ratio of magnesium (Mg) atoms react in comparison to that of hydrochloric acid (HCl)?
217) (HT only)CaCO3 2HCl ---> CaCl2 CO2 H2O Use the above equation to determine the mass of carbon dioxide produced if you react 10g of calcium carbonate with an excess of hydrochloric acid?
218) (HT only)Calculate the mass of iron produced when 32g of iron (III) oxide is completely reduced by aluminium. The reaction is shown in the symbol equation: Fe2O3 2Al ? 2Fe Al2O3
219) (HT only)How can you use the massess of reactants and products to balance a symbol equation?
220) (HT only) Reactants Sb = 488g Cl2 = 426g Products SbCl3= 914g Complete a symbol equation for the reaction above using the masses to balance the equation.
221) (HT only)How do you rearrange the moles equation to find the relative formulat mass? Moles = mass / RFM
222) (HT only)What is meant when a reactant is said to be in excess?
223) What is meant when a reactant is described as a limiting reactant?
224) (HT only) 2H2 O2 --> 2H2O You react 10g of oxygen with 10g of hydrogen. Only 11.25g of product is made the rest of the reactants remain unused. Suggest why the full mass of reactants did not react. What is the leftover unreacted substance?
225) (Chem only) Suggest why it is not always possible obtain the calculated amount of product from a reaction?
226) (Chem only) What does the term yield refer to?
227) (Chem only) What is percentage yield?
228) (Chem only) What is the formula for calculating percentage yield?
229) (Chem only) What mass of carbon dioxide is formed when 12 g of carbon is burned in air?
230) (Chem only) What is atom economy a measure of?
231) (Chem only) What is the formula for calculating percentage atom economy?
232) (Chem only) Hydrazine (N2H4) is used in some rocket fuels. Two different methods can be used to manufacture hydrazine. The reactions are: NH2Cl NH3 ? N2H4 HCl 2NH3 H2O2 ? N2H4 2H2O Calculate the atom economy for each reaction
233) (Chem only) How can a chemist in a chemical plant that makes rocket fuel prevent waste products being formed?
234) (Chem only) What is mol/dm3 the unit of measurement for?
235) (Chem only) How can we calculate the number of moles of solute in a given volume of a solution?
236) (Chem only) What technique can we use if the volumes of two solutions that react completely are known and the concentration of one solution is known, to calculate the concentration of the other solution.
237) (Chem only) How can we calculate the mass of a solute within a solution if we know the concentration in mol/dm3?
238) (Chem only) What is the difference between a strong and weak acid?
239) (Chem only) Do all gases occupy the same volume?
240) (Chem only) What volume does one mole of any gas occupy at room temperature and pressure?
241) (Chem only) How could you calculate the volume a gas would occupy if you were given the mass of gas made?
242) (Chem only) If you have 88g of CO2. What volume would it occupy?
243) (Chem only) In the reaction CH4 2O2 ? CO2 2H2O (at rtp) what volume of water vapour is produced when 2.4 dm3 of methane burns?
244) (Chem only) Rearrange the volume of gas equation to calculate the number of moles
245) What does the reactivity of a metal depend on?
246) How can the reactivity of group 1 metals be compared using a practical investigation?
247) What happens when a metal reacts with oxygen?
248) What happens to metals in an oxidation reaction?
249) What is meant by the term 'reduction'?
250) What happens in terms of electrons during reduction and oxidation reactions?
251) Why is potassium more reactive than lithium?
252) What happens during a displacement reaction?
253) What would the independent, dependent and control variables be for a quantitative investigation into the reactivity of metals?
254) Where in the reactivity series does carbon appear and which elements can be displaced by carbon?
255) What conditions are standard when investigating the reactivity of metals with water and acids?
256) What is the list of metals (and non-metals) in the reactivity series, from most reactive to least reactive?
257) How do each of the following metals react with each of water and dilute acids: potassium, sodium, lithium, calcium, magnesium, zinc, iron and copper?
258) Write the ionic equation for the displacement reaction between copper ions and magnesium
259) Why are metals such as gold found in the Earth as the metal itself?
260) How can metals less reactive than carbon be extracted from their oxides?
261) What is meant by 'reduction' in terms of oxygen?
262) What substance can be used to extract the lesser reactive metals?
263) What type of reaction is it when electrons are transferred from one species to another?
264) Identify the species that are oxidised and reduced in the half equations below: Cu2 Mg --> Mg2 Cu
265) What are the products when acids react with metals?
266) (HT only) What type of reaction occurs when acids react with metals?
267) (HT only) In a reaction between copper (II) oxide and carbon, where does each of oxidation and reduction happen?
268) When an acid (such as hydrochloric acid) reacts with an alkali or a base (such as sodium hydroxide), what will the two products be?
269) What products are made when an acid reacts with a metal carbonate?
270) What factors affect the type of salt produced in a reaction between an acid and a base or alkali?
271) What two products would be made when zinc oxide reacts with dilute hydrochloric acid?
272) What examples of solid insoluble substances react with acids to form soluble salts?
273) When an excess of metal oxide reactant is added to an acid, how can the pure salt solution be collected?
274) What process is used to produce solid soluble salts from salt solutions?
275) What are the typical steps are involved in preparing a pure, dry sample of silver chloride from silver nitrate and sodium chloride?
276) What would the formula be if the following ions reacted to form salts: a) Mg Cl- b) Cu2 S2- c) Fe2 I-
277) In what way can universal indicator be used to measure the approximate pH of a solution?
278) If a substance has the following pH is it classified as acid, alkali or neutral: 1) pH 3 2) pH 11 3) pH 7
279) What ions are produced in alkalis in aqueous solutions?
280) What happens to strong acids in an aqueous solution in terms of ionisation?
281) What happens to weak acids in an aqueous solution in terms of ionisation?
282) What ions are produced in acids in aqueous solutions?
283) When an acid is stronger, what effect does this have on the pH?
284) What happens to the hydrogen ion concentration of a solution when pH decreases by one unit?
285) What is meant by 'dilute' and 'concentrated' (in terms of amount of substance) and 'weak acid' and 'strong acid' (in terms of the degree of ionisation)?
286) How is the reaction between hydrogen ions and hydroxide ions to produce water presented as an equation?
287) How is water produced in a neutralisation reaction between an acid and an alkali in terms of ions?
288) What piece of digital equipment can be used to measure the pH of a solution?
289) What pH values do each of acidic, alkaline and neutral solutions have?
290) A sample of vinegar contains 0.1 mol/dm3 ethanoic acid. What is its concentration in g/dm3? (The relative formula mass, Mr, of ethanoic acid is 60)
291) 25 cm3 of dilute hydrochloric acid is neutralised by 20 cm3 of 0.5 mol/dm3 sodium hydroxide. What is the concentration of the hydrochloric acid?
292) How can the volumes of acid and alkali solutions that react with each other be measured?
293) What does conservation of energy mean?
294) In what circumstance is energy transferred to the surroundings during a chemical reaction?
295) What happens to the energy in an exothermic reaction?
296) What are three examples of exothermic reactions?
297) What is an example of an exothermic reaction in everyday life?
298) What happens to the energy in an endothermic reaction?
299) What are three examples of endothermic reactions?
300) What is an example of an endothermic reaction in everyday life?
301) When a chemical reaction occurs and the temperature of the surroundings has increased, is it an exothermic or endothermic reaction?
302) What are the advantages of using exothermic reactions for hand warmers?
303) What is the temperature change of the solution if the starting temperature was 20 degrees and the end temperature was -5 degrees. State if this is endothermic or exothermic.
304) Why do some collisions between reactant particles not result in a product forming?
305) What does the term activation energy mean?
306) What information can be shown in a reaction profile?
307) What would the simple reaction profile for an exothermic reaction look like?
308) What would the simple reaction profile for an endothermic reaction look like?
309) What information does the activation energy provide?
310) What energy transfers occur during breaking bonds of reactants and forming new bonds of products?
311) What information can bond energies provide?
312) How is the overall energy change of a reaction calculated?
313) What happens in an exothermic reaction in terms of energy, bond making and bond breaking?
314) What happens in an endothermic reaction in terms of energy, bond making and bond breaking?
315) What is the energy transferred in the following chemical reaction: hydrogen bromide decomposing to form hydrogen and bromine? 2 ? (H?Br) ? H?H Br?Br The bond energies relevant to this reaction are shown below: H?Br 366 kJ/mol H?H 436 kJ/mol Br?Br 193kJ/mol
316) How can the amount of energy transferred during a chemical reaction be measured using a practical?
317) Why are chemical cells useful?
318) What factors can affect the voltage produced by a chemical cell?
319) How can a simple chemical cell be made?
320) What is the structure of a battery like?
321) Why do re-chargeable cells and batteries stop working?
322) How can re-chargeable cells and batteries be re-charged?
323) Which cell would be the best choice to use to power a machine? Cell A produces 0.01V of energy and cell B produces 0.20V of energy. Give a reason for your answer.
324) What type of batteries are non-rechargeable?
325) How do fuel cells produce a potential difference?
326) What sort of reaction occurs in a hydrogen fuel cell?
327) What do hydrogen fuel cells offer alternatives to?
328) What are the advantages and disadvantages of using hydrogen fuel cells compared with rechargeable cells and batteries?
329) (HT only) What are the half equations for the electrode reactions in a hydrogen fuel cell?
330) When is an ionic compound able to conduct electricity?
331) (HT) What is the balanced half equation for H ? e??? H2
332) What happens at each of the electrodes in electrolysis when an electric current is passed through the electroytes?
333) (HT) What happens at the anode and cathode electrodes in the electrolysis of aqueous sodium chloride? (use half equations to help explain)
334) Which electrode as the metals and non metals products found during electrolysis?
335) What would the products be for the electrolysis of the following ionic compounds: 1. NaCl 2. PbBr2 3. NaOH 4. Al2O3
336) (HT) What would the half equations be for the electrolysis of NaCl?
337) What happens at the cathode during electrolysis? Is this an oxidation or reduction reaction?
338) What happens at the anode during electrolysis? Is this an oxidation or reduction reaction?
339) What would the half equations be during the electrolysis of PbBr2?
340) When is electrolysis used to extract metals from their ores?
341) What is the main drawback of using electrolysis to extract metals?
342) How is aluminium extracted from its metal ore (aluminium oxide)?
343) Why is a mixture used as the electrolyte in electrolysis?
344) Why does the positive electrode (the anode) need to be replaced regularly?
345) (HT)What are the missing reactants and products of the half equation shown below: Mg2 ___--> _____
346) Why is hydrogen produced instead of sodium in the electrolysis of NaCl solution?
347) When is hydrogen produced at the negative electrode in electrolysis?
348) When is oxygen not produced at the positive electrode?
349) Why are hydrogen and oxygen often discharged in the electrolysis of aqueous ionic solutions?
350) What are the three products made in the electrolysis of aqueous sodium chloride?
351) (HT)
352) How can you separate a solution of copper II sulfate to extract low grade copper ores? (include equipment)
353) How do the Big Ideas link to this topic?

a) Forces:

b) Particles:

c) Energy:

d) Cells: