Chemistry Semester 2 STPM Chapter 11 Reaction Kinetics189Chapter1124. The rate equation for the gaseous reaction between X and Y is: Rate = k[X]2[Y] When 0.20 mol gas X and 0.20 mol of gas Y are mixed in a 2.0 dm3 flask at 350 °C, the initial rate is 5.60 × 10–3 mol dm–3 s–1. Which of the following statement(s) is/are correct of the reaction?I The rate determining step is trimolecular.II The numerical value for the rate constant at 350 °C is 5.60.III The rate of reaction is 1.12 × 10–2 mol dm–3 s–1at 700 °C.A I onlyB II onlyC I and IID I, II and III25. Consider the following equation:X + Y + Z → ProductsIn a kinetic study of the above reaction, the following graphs are obtained.ConcentrationTime [Z][Y][X]What is the order of reaction with respect to X, Y and Z?X Y ZA 1 1 1B 1 2 0C 2 1 0D 0 1 226. The rate constant for a reaction at 30 °C is 5.60 × 10–4 s–1. What is the half-life of thisreaction?A 1237 sB 2209 sC 7487 sD Insufficient data27. Propanone reacts with iodine according to the equation: CH3COCH3 + I2 → CH2ICOCH3 + HI The reaction is catalysed by dilute sulphuric acid. The rate equation is: Rate = k[CH3COCH3][H+] Which statement(s) is/are correct?I Increasing the concentration of dilute sulphuric acid increases the rate of reaction.II The rate determining step involves the reaction of propanone and iodine.III The unit of the rate constant is s–1.IV Dilute sulphuric acid is consumed in the reaction.A I only C II and IIIB I and IV D II and IV28. Aqueous potassium iodide reacts with hydrogen peroxide in the presence of dilute sulphuric acid according to the following mechanism:H2O2 + I– → H2O + IO– FastIO– + H+ → HOI SlowHOI + H+ + I– → I2 + H2O FastWhich statement(s) is/are true of the reaction?I The rate equation is: Rate = k[IO–][H+].II The reaction is first order with respect to H2O2, I– and H+.III Dilute sulphuric acid acts as a catalyst.A I only C I and IIIB II only D I, II and III29. The rate constant of an exothermic reaction is 4.50 × 10–2 s–1 at 35 °C. Which statement is true of the reaction?A It is a second order reaction.B The half-life for the reaction is 15.4 s.C The rate constant at 50 °C is less than 4.50 ×10–2 s–1.D The reaction is non-reversible.30. The dissociation of dinitrogen pentoxide is as follows: 2N2O5(g) → 4NO2(g) + O2(g) The mechanism for the reaction is: N2O5Slow 2NO2 + O N2O5 + O Fast 2NO2 + O2
Chemistry Semester 2 STPM Chapter 11 Reaction Kinetics190Chapter11 What is the unit of the rate constant for the decomposition?A s–1 C mol–1 dm3 s–1B mol dm–3 s–1 D mol–2 dm6 s–131. Which statement about endothermic reactions is true?A They cannot occur at room conditions.B The rate of reaction decreases with increasing temperature.C The activation energy of the forward reaction is lower than that of the reverse reaction.D The rate of reaction increases with the addition of a catalyst.32. The initial rate of reaction between P and Q at different concentration is given in the table below:[P]/mol dm–3 [Q]/mol dm–3 Initial rate/mol dm–3 s–1x y r2x 2y 4r2x 4y 16r What is the initial rate if the concentration of Pand Q is 3x and 3y respectively? A rB 4rC 9rD Cannot be calculated because the rate constant is not given.33. Which statement about catalyst is not true?A The rate of reaction increases with the amount of catalyst used.B The catalyst lowers the activation energy for the forward reaction more than the rate of the reverse reaction.C The yield of the reaction does not depend on the amount of catalyst used.D The chemical nature of the catalyst before and after the reaction is the same.Structured and Essay Questions1. Ethyl ethanoate undergoes hydrolysis in the presence of dilute sulphuric acid according to the equation: CH3COOC2H5(l) + H2O(l) → CH3COOH(aq) + C2H5OH(aq) An investigation of the hydrolysis in an excess of acid at 300 K gives the following information.Time/min 0 10 40 50 80[Ester]/mol dm–3 1.0 0.72 0.24 0.18 0.06(a) What is the function of dilute sulphuric acid?(b) Why must it be in excess?(c) Plot a graph of [ester] against time. Use your graph to determine the half-life of the reaction at initial[ester] of (i) 1.0 mol dm–3(ii) 0.8 mol dm–3(d) What is the order of reaction with respect to hydrogen peroxide?2. Nitrogen monoxide burns in oxygen to produce nitrogen dioxide. 2NO(g) + O2 2NO2(g) The reaction is first order with respect to oxygen and second order with respect to nitrogen dioxide.(a) Write the rate law for the reaction.(b) Given that it is a two-step reaction, write the mechanism for the reaction.
Chemistry Semester 2 STPM Chapter 11 Reaction Kinetics191Chapter11(c) In a particular experiment, the initial rate of reaction is 9.6 × 10–3 mol dm–3 s–1 when the concentrations of nitrogen monoxide and oxygen are 0.80 mol dm–3 and 0.26 mol dm–3 respectively.(i) Calculate the rate constant(ii) Explain the effect on the reaction rate when [O2] is doubled and [NO] is decreased four times.3. (a) The Arrhenius equation is given as k = Ae–EaRT . Name the terms represented by the symbols, k, A, Ea and R.(b) The table below shows the variation of the rate constant of dinitrogen tetroxide with temperature.N2O4(g) → 2NO2(g)Temperature/°C 32 40 50 60k/s–1 0.182 0.466 1.35 3.31(i) Plot a suitable graph to obtain the value of the activation energy.(ii) State one way of reducing the activation energy of the reaction.(iii) What is the order of reaction? Explain how you arrived at your answer.4. The mechanism for the reaction between hydrogen peroxide and potassium iodide in the presence of dilute sulphuric acid is as follows:H2O2 + I– → H2O + IO– FastIO– + H+ → HOI SlowHOI + H+ + I– → I2 + H2O Fast(a) Write the equation for the overall reaction.(b) What is the role of dilute sulphuric acid in the reaction?(c) Derive the rate equation for the reaction.5. The decomposition of hydrogen peroxide can be accelerated by adding a small amount of dilute hydrochloric acid. The mechanism for the catalysed reaction is:2H+ + 2Cl– + H2O2 → Cl2 + 2H2OCl2 + H2O2 → 2Cl– + 2H+ + O2(a) Write an overall equation for the above exothermic reaction.(b) Sketch the energy profile for the catalysed and uncatalysed reaction.(c) Other than catalyst and concentration, state how you would increase the rate of decomposition of hydrogen peroxide.6. Sodium bromate(V), NaBrO3, reacts with sodium bromide in acidic solution according to the equation:BrO3– + 6H+ + 5Br– → 3Br2 + 3H2OA kinetic study of the reaction gives the following results.Experiment [BrO3–]/mol dm–3 [Br–]/mol dm–3 [H+]/mol dm–3 Initial rate/mol dm–3 s–1I 0.40 0.28 0.031 2.50 × 10–3II 0.60 0.28 0.031 3.75 × 10–3III 0.60 0.56 0.031 7.50 × 10–3IV 0.40 0.28 0.062 1.00 × 10–2(a) Determine the order of reaction with respect to BrO3–, Br– and H+.(b) Calculate the rate constant, k, for the reaction.
Chemistry Semester 2 STPM Chapter 11 Reaction Kinetics192Chapter117. Phosphorous(V) chloride undergoes thermal decomposition as follows:PCl5(g) → PCl3(g) + Cl2(g)The graph below refers to the above reaction at temperature T.100 200 300 400 500 600 7001.00.80.60.40.20Concentration/mol dm–3Time/min(a) Determine the half-life of the decomposition corresponding to the initial concentration of PCl5.Concentration of PCl5/mol dm-3 1.0 0.6Half-life/min(b) Write the rate equation for the reaction.(c) How would the half-life change if the reaction is carried out at a high temperature? Explain your answer.e Quiz 3
Chemistry Semester 2 STPM STPM Model Paper (962/2)294Section A [20 marks]Answer all questions in this section.1. 50.0 dm3 containers contain 50.0 g of carbon monoxide, 300 g of nitrogen and 550 g of hydrogen at 25 °C. What is the total pressure of the mixture?[Gas constant, R, is 8.31 J K–1 mol–1]A 1.42 × 107 Pa C 1.42 × 104 PaB 1.20 × 106 Pa D 1.20 × 103 Pa2. Which property of graphite does notcorrespond to its uses?Property UsesA Slippery Lubricant B Inert ElectrodeC High melting point Furnace lining D Good electrical conductorNeutron moderator in nuclear reactors3. The reaction equation of an ester is given below.X(aq) + Y(aq) L Z(aq) + H2O(l)A homogeneous mixture of 0.60 mol carboxylic acid, X, 0.50 mol of alcohol, Y, 0.60 mol of ester, Z, and 0.40 mol of 1 dm3 water is refluxed in the presence of hydrochloric acid. At equilibrium, only 0.40 mol of X remains. Which statement is true about the reaction?A The value of Kc is 6.7.B The amount of Z at equilibrium is 0.80 mol.C The concentration of water at equilibrium is 0.4 mol dm–3.D Hydrochloric acid could be replaced by concentrated sulphuric acid.4. The equation of a reaction at equilibrium is given below.2SO2(g) + O2(g) L 2SO3(g) ∆H = –y kJ mol–1Which condition increases the value of the equilibrium constant, Kp, and the amount of sulphur trioxide at equilibrium?A Adds oxygenB Increases the pressureC Decreases the temperatureD Adds vanadium(V) pentoxide5. The formation of SO3 is shown in the equilibrium equation below.2SO3(g) + O2(g) 2SO3(g)Which are the effects of a catalyst on the reaction?k1 Kc [SO3]A Increases No effect No effectB Increases Decreases DecreasesC Decreases No effect DecreasesD Decreases Increases Increases6. The acid dissociation constants pKa, for several monoprotic acids are shown in the table below.Acid X Y ZpKa 3.7 4.7 7.5 What can be deduced from the pKa of the acids?A X has the lowest degree of dissociation.B pH of Y is lower than pH of Z.C X, Y and Z are strong acids.D Z is the strongest acid.k1k–1STPM MODEL PAPER (962/ 2)
Chemistry Semester 2 STPM STPM Model Paper (962/2)2957. An aqueous solution of 0.25 mol dm–3aniline, C6H5NH2, has pH of 9.0. Which is the Kb value of the aniline?A 2.5 × 10–19 mol dm–3B 4.0 × 10–18 mol dm–3C 2.5 × 10–11 mol dm–3D 4.0 × 10–10 mol dm–38. The equilibrium equation for a saturated solution for magnesium hydroxide is shown below. Mg(OH)2(s) L Mg2+(aq) + 2OH–(aq) Which statement is true of the equilibrium equation?A The solubility product is Ksp = 2x2.B Mg(OH)2 is less soluble when NH4Cl is added.C Mg(OH)2 is more soluble when NaOH is added.D The pH of the saturated solution increases with temperature.9. A student carries out a series of experiments to study the kinetic of the reactionX + Y → ZThe data of the experiment at 360 K is given in the table below.Experiment [X]/mol dm–3[Y]/mol dm–3Initial rate/mol dm–3 s–11 0.10 0.50 0.0532 0.20 0.30 0.1273 0.30 0.40 p4 0.40 0.30 0.509 Which is not true about the kinetic of the reaction?A The rate constant of the reaction is 10.6 dm6 mol–3 s–1.B The reaction is second order with respect to X.C The overall reaction is second order.D The value of p is 0.38 mol dm–3 s–1.10. The iodination of propanone, CH3COCH3, in the presence of H+ occurs according to the equation below. H+ CH3COCH3 + I2 ⎯→ CH2ICOCH3 + HI The rate equation for the reaction is rate = k[CH3COCH3][H+]. At T °C and pH 5, the rate of reaction is r. Which is true about the reaction when the rate of reaction is 2r and the concentration of CH3COCH3 is constant?A The pH of the reaction is 6.B The concentration of I2 is doubled.C The temperature of the reaction is 2T °C.D The concentration of H+ is 2 × 10–5 mol dm–3.11. The equation for the reaction between SO2and O2 is given below. 2SO2(g) + O2(g) → 2SO3(g)The rate constant of the reaction at 47 °C and 112 °C is 5.70 × 10–6 s–1 and 2.15 × 10–3 s–1respectively. What is the activation energy of the reaction?[Gas constant, R, is 8.31 J K–1 mol–1]A 1.74 kJ C 40.58 kJB 3.99 kJ D 93.57 kJ12. A 2.0 kg hot iron bar is placed into a container that is filled with 5.0 kg of water. The temperature of water increases from 20 °C to 30°C. What is the initial temperature of the iron bar? [The specific heat capacity of the iron bar is 0.45 J g–1 °C–1 and the specific heat of water is 4.18 J g–1 °C–1]A 202 °C C 262 °CB 232 °C D 325 °C13. The thermochemistry data of HBr is given below. H2(g) → 2H(g) ∆H = +436.4 kJ Br2(g) → 2Br(g) ∆H = +192.5 kJ H2(g) + Br2(g) → 2HBr(g) ∆H = –72.4 kJ What is the bond energy of HBr?
Chemistry Semester 2 STPM STPM Model Paper (962/2)296A 278.2 kJ mol–1 C 556.5 kJ mol–1B 350.6 kJ mol–1 D 701.3 kJ mol–114. NaX and NaY are halides salts that have the lattice energies of –776 kJ mol-1 and –731 kJ mol-1 respectively. Which is true about the differences in the lattice energies?A The size of Y– is larger than that of X–.B The covalent character is present in NaY.C Hydrogen bonds exists between NaXmolecules.D The melting point of NaY is higher than that of NaX.15. The Born-Haber cycle of sodium chloride is shown below.Na(s)Na(g)++Na + +(g)CI(g)NaCI(s)CI–(g)CI2(g) 12ΔH2ΔH4 ΔH5ΔH3ΔH1Which enthalpy changes have negative values?A ∆H1 and ∆H2 C ∆H3 and ∆H4B ∆H1 and ∆H5 D ∆H4 and ∆H516. An electrochemical cell is shown below. Zn(s) | Zn2+(aq) ∥ Cl2(g) | Cl–(aq) | Pt(s) Which factor does not affect the e.m.f. of the cell?A TemperatureB Concentration of Zn2+C Volume of chlorine gasD Size of the platinum electrode17. The standard reduction potentials of cobalt, Co and iron, Fe, are given below.Standard reduction potential E°Co2+(aq) + 2e– → Co(s) –0.28 VFe2+(aq) + 2e– → Fe(s) –0.44 VFe3+(aq) + e– → Fe2+(aq) +0.77 V Which is true about the above standard reduction potential?A Fe2+ can reduce Co2+ to Co.B Fe has a stronger oxidising power than Co.C Co2+ has stronger reducing power than Fe2+.D The reaction between Co and Fe2+ is nonspontaneous.18. An aqueous solution of CuSO4 is electrolysed for one hour by using a constant current of 0.452 A. Graphite electrodes are used in the electrolysis. Which is not true about the electrolysis? [Faraday constant, F, is 96 500 C mol–1, 1 mole of gas occupies a volume of 24.4 dm3at room conditions]A The quantity of charge used is 1627 C.B The colour intensity of the solution decreases.C The mass of copper deposited at cathode is 0.535 g.D The volume of oxygen gas liberated at anode is 206 cm3.19. An aqueous solution of silver nitrate is electrolysed for two hours by using a constant current of 10.0 A. What is the mass of silver deposited at the electrode? [Faraday constant, F, is 96 500 C mol–1]A 1.34 gB 40.3 gC 80.6 gD 145 g20. The overall reaction of lead storage battery is shown below. Pb(s) + PbO2(s) + 2H+(aq) + 2HSO4–(aq) → 2PbSO4(s) + 2H2O(l) If the concentration of H2SO4 is 4.50 mol dm–3 and the E°cell is 2.04 V, what is the e.m.f. of the cell at 25 °C?A 1.96 VB 2.00 VC 2.08 VD 2.12 V
Chemistry Semester 2 STPM STPM Model Paper (962/2)297Section B [14 marks]Answer all questions in this section.21. (a) Iodine molecules crystallise in the face-centred cubic structure. Draw the lattice structure of solid iodine. [3 marks](b) The activation energy for the decomposition of HI is 60.0 kJ mol–1. Calculate the ratio of the rate constants for the decomposition of HI at 25.0 °C and 35.0 °C, by using the Arrhenius equation, k = Ae–Ea/RT. [4 marks][Gas constant, R, is 8.31 J K–1 mol–1]22. Thermochemical equations for the formation of MgO and Mg2N3 are given below. Mg(s) + 12 O2(g) → MgO(s) ∆H° = –601.7 kJ mol–1 3Mg(s) + N2(g) → Mg3N2(s) ∆H° = –401.2 kJ mol–1(a) What is meant by standard enthalpy formation of magnesium nitride? [2 marks](b) Which compound is more stable? Explain your answer. [2 marks](c) A complete combustion of Mg3N2 produces MgO and N2.(i) Write the thermochemical equation for the above reaction. [1 mark](ii) Calculate the standard enthalpy of combustion of Mg3N2. [2 marks]Section C [26 marks]Answer all questions.23. (a) A reversible reaction involving A, B and C is shown below.A + 2B L 2C(i) A mixture of 1.0 mol of A and 1.5 mol of B in a 2.0 dm3 vessel is allowed to reach equilibrium at 1000 K. At equilibrium, the concentration of C is 0.35 mol dm–3. Determine the value of the equilibrium constant for this reaction. [5 marks](ii) If the enthalpy change for the reaction in (b)(i) is –20 kJ mol–1, calculate the equilibrium constant of the reaction at 1300 K. [4 marks] [The gas constant, R, is 8.31 J K–1 mol–1]
Chemistry Semester 2 STPM STPM Model Paper (962/2)298(b) The results of a titration between aqueous ammonia and 0.050 mol dm–3 of a strong acid, HX, at 25 °C is shown in the graph below.pH00 5 10 15 20 25 3024681012Volume of HX / cm3(i) The titration mixture exhibits buffering capacity at a stage in the titration. Circle the buffer zone on the graph. [1 mark](ii) The pOH of the alkaline buffer which is formed in the titration is given by pOH = pKb + log [NH4+][NH3]Based on the graph, determine the value of the equilibrium constant, Kb, of ammonia at 25 °C. [3 marks]24. (a) The standard reduction potentials of oxygen, X, Y and Z are given in the table below.Half-cell reaction E°/VO2(g) + 2H2O(l) + 4e– → 4OH–(aq) +0.40X2+(aq) +2e– → X(s) +0.34Y2+(aq) + 2e– → Y(s) –0.44Z3+(aq) + 3e– → Z(s) –0.74(i) Which metal is the most resistant towards corrosion? Explain your answer. [2 marks](ii) Identify the metal that corrodes the fastest and write the overall chemical equation of the cell. [2 marks](iii) Calculate the e.m.f. of the cell produced in (a)(ii). [2 marks](b) An aqueous sodium sulphate is electrolysed using platinum electrodes. The volume of the gas collected at the cathode is 35.0 cm3 at room temperature and atmospheric pressure.(i) Determine the amount of current that flows for 30 minutes. [5 marks](ii) Calculate the volume of the gas collected at the anode. [2 marks]
299ANSWERSChapter9 States of Matter9.11.pV = nRTMr = pRTp= (2.615)(8.31)(298)(101)= 64.12.pV = nRTV = pRTp= 142(14.0) × 8.31 × (45 + 273)101000= 0.0131 m33. nr = 0.29 + 0.64 = 0.93 molpTV = nRTpT(5.0 × 10–3) = 0.93 × 8.31 × (25 + 273)pT = 4.6 × 105 PapN2 = XN2 × pT= 0.290.93 × 4.6 × 105= 1.4 × 105 Pa4. p1V1 = p2V2For hydrogen, (202)(5.00) = pH2 (10.0)pH2 = 101 kPaFor nitrogen, (250)(11.5) = pN2 (10.0)pN2 = 287.5 kPaFor oxygen, (101)(1.50) = pO2 (10.0)pO2 = 15.15 kPaTotal pressure = 101 + 287.5 + 15.15= 403.7 kPa5. pO2 = XO2 × pT0.20 = XO2 × 2.4XO2 = 0.202.4 = 0.083Percentage of oxygen required = 0.083 × 100%= 8.3%9.21. Liquid P is more volatile than liquid Q. It evaporates more readily than liquid Q. It has lower boiling point then liquid Q. It has weaker intermolecular force than liquid Q.2. Pressure/atmPropanone Water MercuryTemperature/°C56.5 100 3571.009.31. • Metallic solid. It exists as a giant metallic structureheld by strong metallic bonds between metal cations and delocalised electrons. • Ionic solid. It exists as a giant ionic structure held by strong ionic bonds between cations and anions. • Simple molecular solid. It exists as simple molecular structure held by weak intermolecular van der Waals forces. 2. • C atom in diamond is sp3 hybridised. • Each carbon is covalently bonded to 4 other carbon atoms in three-dimensional manner. • C atom in fullerene is sp2 hybridised. • Each carbon is bonded to 3 other carbon atoms in spherical form which causes the molecules to be slippery.3. (a) • Diamond has a giant covalent structure withstrong covalent bonds. • Each C atom undergoes sp3 hybridisation and is covalently bonded to four other C atoms in atetrahedral manner. • Diamond is hard and has a high melting point. • Diamond is an electrical insulator because all ofthe valence electrons are used in bonding and there are no delocalised electrons. • Diamond is used as cutting tools and asabrasives. (b) • Graphite has a layered lattice structure whichthe carbon atoms are arranged hexagonally. • Each carbon atom in graphite is sp2 hybridised and form strong covalent bonds to three other carbon atoms in the same plane. • The free delocalised electrons are able to movethroughout the layer. This makes graphite a good conductor of electricity. Graphite is usedas inert electrodes in electrolysis. • The layers are interconnected with weak van derWaals forces of attraction. This makes graphite soft and slippery and is used as pencil lead.
332Chemistry Semester 2 STPM AppendixAPPENDIX1HHydrogen11HHydrogen1Proton number 1234567Period3Li Lithium74 Be Beryllium911 Na Sodium 23 12 Mg Magnesium 2419KPotassium 3920 Ca Calcium 4037 Rb Rubidium 85.5 38 Sr Strontium 8855 Cs Caesium 133 56 Ba Barium 137 57 – 71 Lanthanoids 89 – 103 Actinoids 87 Fr Francium 88 Ra Radium 105 Db Dubnium 106 Sg Seaborgium 107 Bh Bohrium 108 Hs Hassium 109 Mt Meitnerium 110 Ds Darmstadtium 111 Rg Roentgenium 112 Cn Copernicium 113 Nh Nihonium 114 Fl Flerovium 115 Mc Moscovium 116 Lv Livermorium21 Sc Scandium 4539YYttrium 8922 Ti Titanium 4840 Zr Zirconium 9172 Hf Hafnium 178.5 23VVanadium 5141 Nb Niobium 9373 Ta Tantalum 18124 Cr Chromium 5242 Mo Molybdenum 9674WTungsten 18425 Mn Manganese 5543 Tc Technetium 9875 Re Rhenium 186 26 FeIron 5644 Ru Ruthenium 101 76 Os Osmium 190 27 Co Cobalt 5945 Rh Rhodium 103 77 Ir Iridium 192 28 Ni Nickel 5946 Pd Palladium 106 78 Pt Platinum 195 29 Cu Copper 6447 Ag Silver 108 79 AuGold 197 30 ZnZinc 6548 Cd Cadmium 112 80 Hg Mercury 201 31 Ga Gallium 7049 InIndium 115 81 Tl Thallium 20432 Ge Germanium 7350 SnTin 119 82 PbLead 207 33 As Arsenic 7551 Sb Antimony 122 83 Bi Bismuth 209 34 Se Selenium 7952 Te Tellurium 128 84 Po Polonium 209 35 Br Bromine 8053IIodine 127 85 At Astatine 210 117 Ts Tennessine 118 Og Organesson 36 Kr Krypton 8454 Xe Xenon 131 86 Rn Radon 2225BBoron 1113 Al Aluminium 276CCarbon 1214 Si Silicon 287NNitrogen 1415P Phosphoros 318OOxygen 1616SSulphur 329FFluorine 1917 Cl Chlorine 35.52 He Helium410 Ne Neon 2018 Ar Argon 4058 La Lanthanum 139 90 Ac Actinium 59 Ce Cerium 140 91 Th Thorium 232 60 Pr Praseodymium 141 92 Pa Protactinum 231 61 Nd Neodymium 144 93UUranium 23862 Pm Promethium 94 Np Nepturium 63 SmSamarium 150 95 Pu Plutonium 64 Eu Europium 152 96 Am Americium 65 Gd Gadolinium 157 97 CmCurium 66 Tb Terbium 159 98 Bk Berkelium 67 Dy Dysprosium 162 99 Cf Californium 68 Ho Holmium 165 100 Es Elinsteinium 69 Er Erbium 167 101 FmFermium 70 TmThulium 169 102 Md Mendelevium 71 Yb Ytterbium 173 103 No Nobelium 71 Lu Lutetium 175 103 Lr Lawrencium104 Rf RutherfordiumSymbol of element Name of element Relative atomic mass Transition elementsLantanide series Actinide seriesI1II23 4 5 6 7 8 9 10 Group 11 12 III 13 IV14V15 VI 16 VII 17VIII 18MetalsKey:Semi-metals Non-metalsPeriodic Table of Elements
W.M: RM38.95 / E.M: RM40.95AAEVSC2675031A2ISBN 978-629-498-727-2Purchaseebook here!Strategic STPM Chemistry Semester 2 is written based on the purified STPM Examination Syllabus by the Malaysian Examinations Council (MEC) and will be implemented starting from STPM Semester 1 in 2026. This book is carefully designed and well-organised, containing the following features to enhance students’ understanding of the concepts being studied.Strategic STPM Pre-U Text Titles:› Pengajian Am Semester 2 › Bahasa Melayu Semester 2 › Biology Semester 2 › Physics Semester 2 › Chemistry Semester 2 › Mathematics Semester 2 › Sejarah Semester 2 › Geografi Semester 2 › Ekonomi Semester 2 › Pengajian Perniagaan Semester 2Also available:› MUET My Way CHEMISTRYPre-U TextStrategicSTPMSEMESTER2REVISION★ Comprehensive Notes★ Learning Outcomes★ Concept Maps★ SummariesREINFORCEMENT & ASSESSMENT★ Quick Checks★ STPM Practices★ STPM Model Paper Semester 2★ AnswersEXTRA FEATURES ★ Examples★ Chemistry Info★ Exam Tips★ Digital Resources QR CODEFEATURES