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(a) Chemists recognise that atoms are made of three types of particle.
Complete the following table with their names and properties.
[Table_1]
(b) The relative atomic mass of an element can be determined using data from its mass spectrum.
The mass spectrum of element X is shown, with the percentage abundance of each isotope labelled.
(i) Define the terms relative atomic mass and isotope.
relative atomic mass ..........................................................
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isotope ................................................................................
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[3]
(ii) Use the data in the mass spectrum to calculate the relative atomic mass, $$A_r$$, of X. Give your answer to two decimal places and suggest the identity of X.
$$A_r$$ of X ..........................................................
identity of X ......................................................
[2]
(c) The element tellurium, Te, reacts with chlorine to form a single solid product, with a relative formula mass of 270. The product contains 52.6% chlorine by mass.
(i) Calculate the molecular formula of this chloride.
molecular formula ....................................................
[3]
(ii) This chloride melts at 224°C and reacts vigorously with water. State the type of bonding and structure present in this chloride and explain your reasoning.
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[2]
(iii) Suggest an equation for the reaction of this chloride with water.
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[1]
(d) Sodium and silicon also react directly with chlorine to produce the chlorides shown.
[Table_2]
(i) Describe what you would see during the reaction between sodium and chlorine.
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[2]
(ii) Explain the differences between the melting points of these two chlorides in terms of their structure and bonding. You should refer to the difference between the electronegativities of the elements in your answer.
NaCl structure and bonding ..........................................
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SiCl4 structure and bonding ........................................
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explanation .................................................................................
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[4]
555
579
501
The relationship $pV = nRT$ can be derived from the laws of mechanics by assuming ideal behaviour for gases.
(a) The graph represents the relationship between $pV$ and $p$ for a real gas at three different temperatures, $T_1$, $T_2$ and $T_3$.
(i) Draw one line on the graph to show what the relationship should be for the same amount of an ideal gas.
(ii) State and explain, with reference to the graph, which of $T_1$, $T_2$ or $T_3$ is the lowest temperature.
(iii) Explain your answer to (ii) with reference to intermolecular forces.
(iv) State and explain the effect of pressure on the extent to which a gas deviates from ideal behaviour.
(b) A flask with a volume of $100 \, \text{cm}^3$ was first weighed with air filling the flask, and then with another gas, Y, filling the flask. The results, measured at $26\, ^{\circ}C$ and $1.00 \times 10^5\, \text{Pa}$, are shown.
Mass of flask containing air = $47.930\, \text{g}$
Mass of flask containing Y = $47.989\, \text{g}$
Density of air = $0.00118\, \text{g cm}^{-3}$
Calculate the relative molecular mass, $M_r$, of Y.
(c) Although nitrogen gas makes up about $79\%$ of the atmosphere it does not easily form compounds.
(i) Explain why nitrogen is so unreactive.
(ii) Explain why the conditions in a car engine lead to the production of oxides of nitrogen.
(iii) Give an equation for a reaction involved in the removal of nitrogen monoxide, NO, from a car's exhaust gases, in the catalytic converter.
One of the main reasons for reducing the amounts of oxides of nitrogen in the atmosphere is their contribution to the formation of acid rain.
(iv) Write an equation for the formation of nitric acid from nitrogen dioxide, NO$_2$, in the atmosphere.
(v) Write equations showing the catalytic role of nitrogen monoxide, NO, in the oxidation of atmospheric sulfur dioxide, SO$_2$.
522
525
574
Ethanol reacts with hydrogen cyanide, in the presence of a small amount of NaCN, as shown.
CH$_3$CHO + HCN \rightarrow CH$_3$CH(OH)CN
(a) Use bond energies from the Data Booklet to calculate the enthalpy change for this reaction. Include a sign with your answer.
enthalpy change = ............................... kJ mol$^{-1}$ [3]
(b) The product of this reaction shows stereoisomerism as it contains a chiral centre. This reaction produces an equimolar mixture of two optical isomers.
(i) Explain the meanings of the terms stereoiomerism and chiral centre.
stereoisomerism ......................................................................................................................
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chiral centre .............................................................................................................................
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[2]
(ii) Suggest why the two optical isomers are produced in equal amounts by this reaction.
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[1]
(c) (i) Complete the diagram to show the mechanism of this reaction. Include all necessary charges, partial charges, lone pairs and curly arrows and show the structure of the intermediate.
[5]
(ii) With reference to your mechanism in (i), explain the role of the NaCN in this reaction.
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[1]
590
561
554
There are four alcohols, A, B, C and D, which are structural isomers with the molecular formula $C_4H_{10}O$.
Alcohol A does not react with acidified potassium dichromate(VI) solution but B, C and D do.
All four alcohols react with hot, concentrated sulfuric acid to form products with the molecular formula $C_4H_8$. A, C and D each give a single product in this reaction. B gives a mixture of two structural isomers, one of which shows stereoisomerism.
(a) Give the skeletal formula for each of the four alcohols and complete the diagram with the names of the types of structural isomerism shown by each linked pair of compounds.
(b) (i) Give the names of the two structural isomers produced by the reaction of B with hot, concentrated sulfuric acid
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(ii) State which of these two isomers shows stereoisomerism. Explain why this molecule is capable of showing stereoisomerism.
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(iii) Draw displayed formulae to show the two stereoisomers.
stereoisomer 1 stereoisomer 2 [2]
560
503
577
