Chemistry p2 Mark Scheme

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    PAHANG TRIAL 2009 EXAMINATION

    CHEMISTRY PAPER 2 MARKING SCHEMES

    SECTION A - Structural Questions:

    Question 1.

    (a) (i) The presence of isotopes 1M

    (ii) Let the abundance of 63X be a %.The % abundance of 65X. = ( 100 a ) 1M

    Relative atomic mass = ( 62.93 x a) + ( 64.93 x ( 100 -a) ) 1M

    100

    63.55 = 62.93a + 6493 -64.93a100

    6355 = -2a + 6500a = 69.0% 1M

    The % abundance of 65X = 100- 69.0

    = 31.0 %

    Relative abundance 63X : 65X1 : 2 1M

    (iii)

    RelativeAbundance

    63 64 65 Relative mass /m/e2M

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    Species protons neutrons Electrons

    20 Ne

    10

    10 10

    10

    16 O2-

    8

    8 8 10

    2 M

    The species have same number of electrons or isoelectronic. 1M----------------

    10M

    2. (a) (i) H2O2 + 2H+ + 2 I- 2H2O + I2 1M

    (ii) Rate = k [H2O2] [I-] 1M(iii) 0.2 1M

    0.1 1M

    (iv) second order 1M

    (b) (i) 12 1M

    (ii) 1s2 2s2 2p6 3s2 . 1M

    (iii) +2 , X has two valence electrons 2M(iv) X is a better electricity conductor. 1M

    ----------------

    10M

    3.(a) Atomic size increases, screening effect increases with more inner shells of

    electrons 1M

    effective nuclear charge decreases, ionisation energy lowered, valence

    electrons are more easily removed. 1M

    (b) i. Be2+ (aq) + 4H2O (l) [ Be (H2O)4 ]2+ (aq) 1M

    ii. It is acidic, acting as a Bronsted-Lowry acid 1M

    The Be2+ ion has a high charge density 1M

    and can strongly polarise large anions due to its smaller size. 1M

    The ions of other Group 2 elements have larger sizes and charge densities andweaker polarising power

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    (d) i. platinum and rhodium 1M

    ii. 4NH3(g) + 5O2(g) 4NO(g) + 6H2O (g) 1M

    iii. low temperature 1M

    low pressure 1M(Note : The reaction is exothermic reaction. According to le Chatelier

    principle, a low temperature will favour the formation of NO. For gaseous

    equilibrium, a decrease in pressure will favour the reaction which producesmore gaseous molecules. Thus in the above equilibrium a low pressure will

    favour the formation of NO.)

    ________

    10M

    4.(a) i. A is CH3CH2CH2COOH 1MB is CH3CH2CH2COCl 1M

    C is CH3CH2CH2COOCH2CH 1M

    ii. butanoyl chloride 1M

    iii. Formation of ester:

    CH3CH2CH2COCl + CH3CH2OH CH3CH2CH2COOCH2CH3 + HCl 1M

    (b) i. H3N

    +CH2COOH + H2NCH(CH3)COOH

    H2NCH2CONHCH(CH3)COOH + H2O 1M

    Glycylalanine 1M

    ( Note: Alanylglycine can also be formed )

    ii. The amino group NH2 which is basic group reacts with hydrochloricacid to form the ammonium chloride salt of alanine 1M

    HOOCCH(CH3)NH2 + HCl HOOCCH(CH3)NH3+Cl- 1M

    ___________

    10 M

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    SECTION B - ESSAY

    5.(a) (i) Orbitals with the same energy 1M

    Example : 2p or 3d s orbitals 1M

    (ii) Nitrogen atom has 7 electrons 1M

    Fill 1s orbital with 2 electrons 1MFill 2s orbital with 2 electrons 1M

    Fill 2px,2py and 2pz orbitals with 3 electrons 1M / 6

    1M

    (b) Fe 2+ 1s2 2s2 2p6 3s2 3p6 3d4 1M

    Fe 3+ 1s2 2s2 2p6 3s2 3p6 3d5 1M

    In terms of electronic configuration, Fe 3+ is more stable than Fe 2+ 1M

    Because it has half-filled 3d orbital which is more stable 1M./ 4

    (c ) The valence electronic configuration of the electrons for nitrogen atom

    is 2s2 2px1 2py1 2pz1 1MNitrogen atom uses sp3 hybrid orbitals for forming covalent bonds

    between N and H atoms.

    Energy

    2p

    sp3 hybrid porbitals

    N(ground state) 1M

    In sp3 hybrid orbitals of nitrogen atom,one of the orbitalsIs occupied by a lone pair of electrons and three sp3 orbitals

    are half filled 1M

    Each N-H atom is formed by the overlapping of the s orbital

    of hydrogen atom with one of the half filled sp3 orbitals

    to give the ammonia molecule 1M

    Diagram of the bond formation in NH3 molecule. 1M /.5

    -------------------Total : 15 M

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    6. (a) Dynamic equilibrium ....

    a reversible reaction , in a closed system

    forward and backward reactions have the same rate of reaction. 2M(b) (i) N2O4 2NO2

    Kc = [NO2]2

    = [0.12]2

    [N2O4] [0.04]

    = 0.36 mol dm-3 5M

    (ii) Using PV =nRT where n = 0.12 +0.04 = 0.16 mol

    P = 0.16 (8.31) (383)

    10 -3

    = 509.24 kPa .3M

    (c) N2(g) + 3H2(g) 2NH3(g)

    - at low temperatures, % NH3 is higher

    - forward reaction is exothermic

    - equilibrium position shifts to the right at higher temperature

    - forward reaction is accompanied by a reduction in volume of gas

    - at higher pressures, equilibrium position shifts to the right

    - at high pressures, % NH3 is higher 5M---------------

    Total : 15MNo. 7

    (a) (i) Aluminium metal is extracted by electrolysis

    The electrolyte is molten bauxite in sodium hexafluoroaluminate.The electroyte has aluminium ion and oxide ions.

    Anode : 2O2- --- > O2 + 4e

    Cathode : Al3+ + 3e --- > Al 5M

    (ii) (Any 2 points)light

    Resistant to corrosion

    Strong alloy 2M

    `(b) aluminium :

    A giant metallic structure, strong metallic bonf.

    Silicon : giant 3 D covalent structure.

    Strong covalent bond between silicon atomes.

    higher melting point

    Phosphorus and sulphur - Both are simple molecules.

    Weak van der waals between molecules

    Sulphur has a stronger intermolecular forces

    S8 larger than P4 8M

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    No 8. (a) chlorine strong oxidation agent

    Bromide is oxidized to bromine

    E of chlorine is more positive than that of bromine.Cl2 + 2Br

    - ---- > 2Cl- + Br2 4M

    (b) iodine forms triodes complex in KI.

    I2 + I- ---- > I3

    -

    Iodine does not form any complex ions in water.

    I2 + 2H2O --- > I- + HIO + H3O

    + 4M

    (c) HCl is released in cold acid

    NaCl + H2SO4 NaHSO4 + HCl

    If heated more HCl released.

    NaHSO4 + NaCl - Na2SO4 + HCl 4M

    (d) Iodide is oxidized to iodine

    Purple Iodine is releasedPungent smell of H2S is detected 3M

    --------------

    Total : 15M

    9.( a ) ( i ) order : W, Y, X

    W, Y, X act as Lewis bases.

    X is the strongest base because ethyl group is an electron donor byinductive effect.

    Y is more basic than W because the lone pair electron on the N atom

    is not delocalised.

    W is less basic than Y because the lone pair electron on the N atomis delocalised into the benzene ring. 5M

    ( ii ) pKb value > 9.39

    Z is a weaker base than W.

    Presence of Cl - an electron withdrawing group reduces the donating

    potential of lone pair electron on the N atom through inductive effect. 4M

    ( b ) Concentated H2SO4 and HNO3., 55C

    Mechanism: HNO3 + H2SO4 NO2+ + HSO4

    + H2O

    NO2+ is an electrophile.

    H+ NO2+ NO2

    H

    NO2 + HSO4 NO2 + H2SO4

    + HNO3 NO2 + H2O 6M

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    Total : 15 marks

    10.( a ) ( i ) Terylene/Dacron

    ~~~~O - CH2 - CH2 - O - C C - O - CH2 - CH2 - O - C C~~~~ 3M|| || || ||

    O O O O

    ( ii ) Condensation polymerisation

    To make cloth/sleeping bags, etc 2M

    ( b ) ( i ) K: functional group : -OH

    isomers : CH3CH2CH2OH and CH3CHCH3OH

    warm isomers separately with alkaline iodine,

    CH3CHCH3OH gives a yellow precipitate but CH3CH2CH2OH does not.

    CH3CH2CH2OH + 4I2 + 6OH

    CHI3 + 5I + 5H2O + CH3COO

    5M

    (ii ) L : functional group : C = O

    |

    Isomers : CH3CH2CHO and CH3COCH3

    warm isomers separately with Tollens reagent.

    CH3CH2CHO gives a silver mirror but CH3COCH3 does not.

    CH3CH2CHO + 2[Ag(NH3)2]2+ + OH CH3CH2COO

    + 2Ag + 2NH4+ + 2NH3

    5M

    Note: Can also accept other suitable chemical test.

    Total : 15 marks