CHEMISTRY EXAM QUESTIONS FOR SS2 SECOND TERM
SS2 CHEMISTRY EXAM QUESTIONS SECOND TERM – EDUDELIGHT.COM
SECOND TERM EXAMINATION
Examination malpractices may lead to a repeat of the subject or suspensions don’t be involved.
SUBJECT: CHEMISTRY DURATION: 2 ½ HRS CLASS: SSS 2
1. What type of reaction is represented by the equation: 3H2 (g) + N2(g) → 2NH3(g) ; ΔH = -92.6kj mol-1? a. catalytic reaction b. exothermic reaction c. endothermic reaction d. heterolytic reaction
2. Which of the following equation represents direct combination?
a. Fe3+ (aq) + e– —Fe2+ b. H+ (aq) +OH–—- H2O(aq) c. Zn +Cl2—–ZnCl2(s)
d. Ag (aq) + Cl– —–AgCl(s)
3.__________ is the number of moles of reactant converted or product formed per unit time (a) rate of reaction (b) temperature of reaction (c) mass of reaction (d) escape of reaction
4.Which of the following occurs when only a small fraction of the collision result in a reaction (a) effective collisio (b) defective collision (c) moderate collision (d) ineffective collision.
5. When an external constraint such as change in concentration, pressure is imposed on a chemical system in equilibrium, the equilibrium will shiff so as to annual or neutralize the constraint. The above statement is called (a) law of multiple proportion (b) Le Chatelier’s principle (c) reversible reaction (d) equilibrium reaction.
6. A reaction that goes in both forward and backward reactions is called (a) reversible reaction (b) thermal reaction (c) radioactive reaction (d) activation reaction
7. The following factors have effects on position of equilibrium except (a) temperature change (b) pressure change (c) catalyst (d) concentration change.
8.In the decomposition of CaCO3(s) CaO(s) + CO2(g) the reaction will attain dynamic equilibrium only (a) when the reaction is in open system (b) when the reaction is heated strongly (c) When the reaction is in a closed system (d) when the reaction is catalysed.
9. N2O4à 2NO2. The effect of increase in the total pressure of the system at equilibrium (a) decrease the formation of N2O4 (b) favours the formation of more N2O4 (c) favours the formation of more NO2 (d) makes the system to be static.
10. The equilibrium constant K of this reaction is xZ + bQ + M + nR. (a) K = {Z}x {Q}b (b) K = {M}t {R}n (c) K = {Q}b {M}t
{M}t {R}n {Z}x {Q}b {Z}x {R}n
K = {t}m {n}D
{x}z {Q}b\
11. The product of an endothermic reaction are
a. higher in enthalpy than the reactant b. lower in enthalpy than the reactant
c .the same in enthalpy as the reactant d. the change in enthalpy is less than zero
12.What happens if the temperature of this system is decrease? So2(g) + O2(g)
2So3(g). H – xkymol-1. (a) The reaction favours backward reaction (b) The reaction attains equilibrium fast (c) The reaction favours forward reaction (d) The reaction favours both forward and backward reactions.
13.All except one is not a condition for considering pressure in an equilibrium system (a)There must be concentration gradient between the reactants and the products (b) The reactants could be gases while the products may be solid (c) Both products and reactants must be gaseous (d) the reaction takes place in a closed system.
14.In the reaction H2(g) + I2(g) 2HI(g). The effect of pressure on this system is (a) to encourage forward reaction (b) to encourage backward reaction (c) to remove the energy barrier (d) pressure may not have any effect.
15. The collision theory proposes that
reactants collide more frequently to bring about reduction in the reaction rate
all collision of reactants are effective
reactants must collide with a certain minimum amount of energy to form products
d. the fewer the collisions, the faster the reaction rate.
16. When concentrated H2SO4 is added to NaCl(s) the gas evolved
a. bleaches damp blue litmus paper
b. forms a white precipitate with AgNO3(aq)
c. forms a white precipitate with BaCl2(aq)
d. turns moist red litmus paper blue.
17. When X is added with manganese (iv) oxide, oxygen is produced .X is
KCl b.KClO3 C.CaCO3 d.ZnCO3
18. A measure of degree of disorderliness in a chemical system is known as: (a)enthalpy (b) free energy (c) entropy (d) activation energy
19. H2(g)+ x2(g) 2HX(g) ΔH=positive. In the above reaction, a decrease in temperature will:
(a) decrease the concentration of HX
(b) favour the forward reaction
(c) favour the yield HX
(d) have no effect on the equilibrium position
20. The energy barrier that needs to be overcome for a reaction to occur is (a) activation energy (b) activation complex (c) reaction complex (d) absorption reaction.
21.If there is no observable change in the properties of the system with respect to time, the system is said to be _____– (a) in equilibrium (b) unbalanced (c) perfect (d) electrolytic
22. A system is in equilibrium when
a. ∆G is positive b.∆ G is negative c. ∆G is zero d. ∆G is constant.
23. Which of the following metals will react with cold water to produce hydrogen gas?
a. calcium b. aluminium c. copper d .magnessium
24.The following are physical properties of hydrogen except (a) it is a colourless gas (b) Neutral to litmus (c) very low boiling point (d) acidic to litmus.
25.The percentage by volume of oxygen in the atmosphere is (a) 21% (b) 31% (c) 41% (d) 51%
26.The following methods are used to prepare hydrogen industrially except (a) from water gas (b) from methane (c) by electrolysis (d) by electrochemical method.
27.Which of the following behaves as basic and acidic (a) ZnO (b) CaO (c) CuO (d) SO2
28.The following are examples of neutral oxides except (a) NO (b) H2O (c) N2O (d) NO2
29.The following are isotopes of hydrogen except (a) tritium (b) deuterium (c) neutrium (d) protium.
30.The following are uses of hydrogen except (a) for filling ballons (b) in oxy-hydrogen flames (c) in the manufacture of ammonia (d) in dehydrogenation.
31.An isotope of hydrogen commonly referred to as heavy water is (a) protium (b) deuterium (c) tritium (d) basic water.
32.All, except one metal, can displace hydrogen from water or acids (a) Zinc (b) silver (c) potassium (d) heated magnesium.
33.The oxidation state of hydrogen in the hydride of nitrogen is (a) +1 (b) +3 (c) -3 (d) -1.
34.Sodium hydride reacts with water to
(a) form an acidic solution (b) liberate hydrogen gas (c) form a salt (d) liberate oxygen (e) form a neutral solution.
35.From the reaction. Fe2O3 + 3H2(g) 2Fe(s) + 3H2O(g), hydrogen is behaving as an (a) oxidizing agent (b) reducing agent (c) steam donor (d) hydride.
Which
36. Which component of air is removed when air is bubbled through a solution of alkaline pyrogallol?
a. carbon (iv)oxide b. Nitrogen c. Oxygen d. Helium
37. Oygen is obtained from liquid air by
a. Fermentation b. Fractional distillation
c. Filtration d. Sublimation
38. Which of these gases has the following physical properties? (i) diatomic gas (ii) colourless, tasteless and odourless (iii) slightly soluble in water (iv) liquefies easily. (a) Co (b) N2 (c) O2 (d) H2.
39. Chlorine is best collected by
a. upward displacement of air b. downward displacement of air c. over water
d .over mercury
40. Which of the oxides of nitrogen is a neutral oxide? a. N2O4 b.NO2 C.N2O5 d .NO
41.Plastic sulphur is a. A crystalline allotrope of sulphur b. A super cooled form of sulphur
c. A form of sulphur rings packed together d. Forms monoclinic sulphur when left
42. Arrange the following elements in order of increasing electron affinity
Br2,Cl2,I2,F2 a.I2, Cl2, Br2, F2 b.I2,Br2, Cl2,F2 c. Cl2, I2 , Br2, F2 d. Br2,Cl2,I2,F2
43. The gas that can be best collected by downward displacement of air (a) chlorine (b) carbon(iv)oxide (c) sulphur (iv)oxide (d) ammonia
44. Which of these reactions with Oxygen is slowest? (a) Rusting (b) Fe + O2 (c) Petrol + O2 (d) Coal + O2.
45. One of these methods produces impure nitrogen. (a) NaNO2(aq) + NH4cl (b) (NH4)2 Cr2 On(s) (c) NH3(g) + Cuo (d) removing Co2 and O2 from dust free air.
46.Hydride of Nitrogen which is capable of turning red litmus paper blue makes nitrogen to have an oxidation state of (a) +2 (b) -2 (c) +3 (d) -3.
47. Which of the allotropes of sulphur has amber colour with needle shapes? (a) Rhombic sulphur (b) Plastic sulphur (c) Monoclinic sulphur (d) Flower of sulphur.
48. Sulphur reacts with many metals when heated in the absence of air but sulphur reacts with one of these without heating. (a) Fe (b) Hfeg (c) Na (d) Au.
49. Yellow paints are prepared (with the presence of Fe3+) by using (a) SbS3 (b) Mns (c) Zns (d) SnS2.
50. Name Y in the following reactions. Cu(s) + 2H2SO4(aq) Cuso4(aq) + 2H2O(l) + Y. (a) copper(ii) hydride (b) hydrogen sulphide (c) sulphur(vi)oxide (d) sulphur(iv) oxide.
SS2 CHEMISTRY EXAM QUESTIONS SECOND TERM – EDUDELIGHT.COM
THEORY
1a. Draw an energy profile diagram for the reaction of aluminium carbide and water. 2marks
b.State one factor you would employ to make the reaction in the above reaction faster. 2marks
c. Show the effects of this factor on the energy profile diagram. 3marks
d. The reaction C+O2(g)—–CO2(g) is carried out at a temperature of 570C.If the enthalpy change is -5000j and the entropy changes is +15j.Calculate the free energy change. Is the reaction spontaneous or not? 3marks
2. a. Consider the following equilibrium reaction:
N2O4(g)¬˾2NO2(g),ΔH=+58.2KJ/mol
What would be the effect of the following factors on the position of equilibrium on the reaction.?
I . increase in temperature
II. decrease in pressure
III. decrease in the volume of the reaction vessel. 6marks
b. write down the equilibrium constant for the reaction. 1marks
c. State the types of reaction written bellow:
| heat |
(i) H30+ + OH– 2H2O
| V205 |
(ii) 2Pb(NO3)2(s) 2PbO(s) + 4NO2(g) + O2(g)
2SO2(g) + O2(g) 2SO3(g) 3marks
3. a. Using relevant chemical equations, describe 2 methods of preparing oxygen in the laboratory. 4marks
b. State 3 chemical properties of hydrogen and use chemical equations to support your answer. 11/2marks
c. Describe the test for oxygen and Hydrogen. 3marks
d. State the isotopes of Hydrogen. 11/2marks
4. a. Using equations only, outline the process involved in the manufacture of tetraoxosulphate (vi)acid by the contact process. 3marks
b. Describe any chemical test to distinguish between the following:
Sulphur (iv)oxide and Hydrogen Sulphide. 2marks
c. Give three major use of H2SO4. 2marks
d. In the preparation of trioxonitrate(v) acid in the Laboratory from trioxonitrate(v) salts
i. What other reagent is required? 1mark
ii. State the reason why an all- glass apparatus must be used. 2marks
5.a.Write a balanced equation for the decomposition of each of the following trioxonitrate(v)salts on heating:
I. NaNO3
II. Zn(NO3)2
III.AgNO3 3marks
b. State what ould be observed if a piece of damp blue litmus paper is dropped into a gas jar of chlorine. 2marks
c. Name the type of reaction which occurs in b above. 1marks
d. Give the property of chlorine which is exhibited in the reaction in c above. 1marks
e. Draw and label a diagram to illustrate the preparation and collection of dry chlorine gas in the laboratory. 3marks
1. Which of the following decreases when a given mass of gas is compressed to half its initial volume?
a. average intermolecular distances b. frequency of collisions c. number of molecules present
d. atomic radius of each particle
2. Calculate the mass of chlorine gas which occupies a volume of 1.12dm3 at s.t.p.
(Cl=35.5,1 mole of gas occupies 22.4dm3 at s.t.p. a.1.80g b.3.55g c.7.10g d.15.50g
3. Determine the mass of sulphur (iv) oxide obtained when 91.0g of oxygen reacts completely with sulphur according to the following equations S(s)+O2——-SO2(g).(S=32,O=16)
a.123g b.139g c.155g d.182g
4. Which of the following elements form an ionic chloride? A.magnesium b .carbon c. phosphorus d. Hydrogen
5. The bond between two iodine molecules is
(a).co-ordinate bond (b) electrovalent bond (c).ionic bond (d) van derwaal’s forces
6. Bonds between a highly electronegative atom and a hydrogen from another molecule is called
(a).hydrogen bond (b).covalent bond (c).intermolecular forces (d).ligand.
7. The nitride ion is N-3.What is the formula of the nitride of an alkali metal X.
a.X3N5 B.XN3 C.X2N3 d.X3N
8. What type of chemical bonding is involved in the formation of NH4+ from a molecule of ammonia and a proton.
a. Hydrogen bonding b. co-ordinate covalent bonding c. electrovalent bonding d. covalent bonding
9. Which component of the air is removed when air is bubbled through a solution of alkaline pyrogallol? A. Carbon (iv) oxide b. helium c. nitrogen d. oxygen e. water vapour
10.Which law is obeyed when 1 volume of Hydrogen reacts with 1 volume of chlorine to form 2 volumes of Hydrogen chloride? a.Law of constant composition b. Boyle’s law c. Charle’s law d. Gay Lussac’s law e. law of reciprocal proportions
11.What volume of oxygen in dm3 is given off at s.t.p. When 17g of Hydrogen peroxide completely decomposes according to the following equation 2H2O2(l)——-2H2O(l)+O2(g)
(H=1 ,O=16 and the molar volume of a gas at s.t.p=22.4dm3)
a.32 b.22.4 c.11.2 d.5.6 e.2.8
12. One mole of a substance contains the atomic mass b. Avogadros number of particles c. mass number d.oxidation number e. quantum number
13.The gas law represented by the mathematical expression,p=p1+p2+p3 is…… a.. avogadro’s law b. Daltons law of partial pressure c. Grahams law of diffusion d. law of constant composition e. law of multiple proportion
14. What is the volume occupied by 3 moles of ammonia at S.T.P?
a. 44.8dm-3 b. 22.4dm-3 c. 11.2dm-3 d. 67.2dm-3
15. The volume occupied by 0.4g of hydrogen gas at STP is (H=1.00, molar volume at STP =22.4 dm3)
(a) 2.24 dm3 (b) 4.48dm3 (c) 22.4dm3 (d) 8.96 dm3
16 .What type of bond holds Hydrogen fluoride molecules together to form larger
aggregates? a. covalent b. dative c. hydrogen d. ionic e. metallic
17. What is the percentage by mass of sodium in a molecule of Na2CO3.10H2O?
(H=1 , C=12, O=16 , Na=23) A. 160 b. 187 C. 186 D. 250
18. The relative molecular mass of a gas which has a vapour density of 16 is
a. b.
c.8 d.32 e.64
19. What is the amount in mole of sodium trioxocarbonate (iv) in 5.3g of the compound?(CaCO3=106)
a. 0.05 b.0.10 c.0.20 d.0.50 e.2.00
20. Calculate the mass of chlorine gas which occupies a volume of 1.12dm3 at s.t.p.(Cl=35.5, 1 mole of gas occupies 22.4dm3 at s.t.p) a. 21.4 g b. 3.55g c. 31.7g d. 4.35g
21.Given that 32.0g of sulphur contains 6.02×1023 sulphur atoms, how many atoms are there in 2.7g of aluminium?(Al=27, s=32) a. 6.02 x1023 b.3.01×1023 c.6.02x 1022 d.5.08×1022 e.3.01×1022
22. Which of the following gives the products of the equation given below
Zn(s) +HCl (aq)——–
a.ZnCl2+H2 b. ZnCl2+H c. ZnCl+H2 d. ZnCl+H
23. The molar mass of HNO3 is….. (H=1, O=16, N=14). A. 53 b.73 c.63 d.5
24.What is the percentage by mass of copper in copper(i)oxide Cu2O. (O=16,Cu=64)
a.88.9% b.80.0% c.66.7 d.20.5 e.11.1%
25.If the volume of a given mass of a gas at 0oC is 27.3cm3,what will be the volume of the gas at 10oC, pressure remaining constant? a. 2.73cm3 b.28cm3 c.37.3 cm3 d.273 cm3 e.28.3 cm3
26.Which of these gases will have the highest rate of diffusion under the same condition?(H=1,C=12,O=16,S=32,Cl=35.5). a. O2 B.Cl2 c. HCl d.H2S e.CO2
27.A given volume of methane diffuses in 20seconds.How long will it take the same volume of sulphur(iv) oxide to diffuse under the same condition. (CH4=16,SO2=64)
a.5 seconds b.20 seconds c.40 seconds d.60 seconds e.80seconds
28.The ratio of reactants to products is 1:3:2 in the reactions represented by the equation:N2(g)+3H2——–2NH3(g). Which of the following laws is demonstrated by this?
a.Boyle’s law b. Law of multiple proportion c. Gay lussacs law d. Law of constant composition E. Avogadro’s law
29. A solid substances with high melting and boiling points is likely to be a/an
a. covalent compound b. dative covalent compound c. electrovalent compound
d. non-metal
30. If X is a group III element. Its oxide would be represented as a. X3O2 b. X3O c. X2O3 d. XO3
31. What is the volume occupied by 2 moles of ammonia at S.T.P?
a. 44.8dm-3 b. 22.4dm-3 c. 11.2dm-3 d. 5.6dm-3
32. An organic compound contains 40.0% carbon, 6.7% hydrogen and 53.3% oxygen. What is the empirical formula of the compound? [O = 16.0, C = 12.0, H = 1.0]
a.C2HO b. CHO c. CH2O d. CHO2
33. Which of the following statements about electrovalent compounds is not correct?
a. crystals are formed b. electrons are shared c. ions are formed d. strong electrostatic forces are involved
34. Which of the following pairs of elements form a compound by transfer of electrons?
a. carbon and chlorine b. carbon and oxygen c. hydrogen and chlorine d. potassium and chlorine
35. What is the value of X in the following equation? 2H2S + SO2→ 2H2O + XS
A. 6 B. 4 C.3 D. 2
36. The law which describes the relationship between volume of a fixed mass of gas and its absolute temperature at constant pressure is a. Boyle’s law b. Charles’s law c. Gay Lussac’s law d. Graham’s laws
37. The two types of bonds that exist in H3O+ are A. covalent and ionic B. dative covalent and covalent C. metallic and ionic D. polar covalent and metallic
38. Given that r is rate and p is density, the expression r a1/√P represents
a. Boyle’s law b. Charles’s law c. Dalton’s law d. Graham’s law
39.If the atomic number of an element X is 11 and that of oxygen is 8, the most likely formula of the oxide of X is? (a) X2O (b) X3O2 (c) XO2 (d) XO3
40.An element X1with electronic configuration 2,8,2 and element Y with electronic configuration 2,8,7 are likely to combine by (a) metallic bonding (b) covalent bonding (c) electrovalent bonding
(d) dative bonding
41.The relative molecular mass of limestone CaCO3 is [Ca =40, C=12, O=16]? (a) 65 (b) 105 (c) 100 (d) 312
42.All pure samples of a particular chemical compound contain similar elements combined in the same proportion by mass is the law of ? (a) conservation of mass (b) definite proportions (c) multiple proportions (d) reciprocal proportions
43.Which of the following compound is covalent? (a) CaCl2 (b) MgO (c) NaH (d) CH4
44. All these are cause of luminousity in flames except;
a. Solid particles b. Solid particles and increase temperature
c. Solid particles and increased pressures. d. Size of materials burnt.
45. The gases burn with blue flame except: a H2 b. CH4 c.2H2 d.CO
46. Which of these is not necessary for metallic corrosion?
a. Water b. Oxygen c. Heat d. Sulphur (iv) oxide
47. The most abundant nobles gas in nature is: a. Neon b. Radon c. Helium d. Argon.
48. Which type of bond exist between two atoms of an element with atomic number of 7.
49. Which of the following exist as a molecular solid? a. Silica b. sodium c. iodine d. diamond
50. If the atomic number of an element is 10, then the outermost shell will have
a. 2 electrons b.4electrons c.6electrons d.8electrons
THEORY: attempt any three questions)
1(i)What volume is occupied by 24.5g of dichlorofluoromethane CF2Cl2 at s.t.p?
(C=12 ,F=19 ,Cl=35.5 and 1 mole of gas at s.t.p occupies 22.4dm3) 4marks
(ii) Distinguish between Dative and covalent bond 4marks
(iii) State the type of intermolecular forces present in: Argon
2(i) State Dalton’s law of Partial Pressure 2marks
(ii) If 200cm3 of carbon (iv) oxide were collected over water at 18oC and 700 mmHg, determine the volume of the dry gas at s.t.p
(standard Vapour pressure of water at 18oC = 15mmHg] 4marks
(iii) A hydrocarbon with a vapour density of 29 contains 82.76% carbon and 17.24% hydrogen.
Determine the:
I. empirical formula
II. molecular formula of the hydrocarbon
[H = 1.00 C = 12.00] 4marks
3.(i) Two different sample, 1 and 2 of Zinc oxide were obtained from different sources. When heated in a stream of hydrogen they were reduced to yield the results below.
| Zinc Oxide | Mass of Oxide | Mass of Zinc left |
| Sample 1 | 20.0g | 16.22g |
| Sample 2 | 26.4g | 21.7g |
Show that the result above explains the law of constant composition. 4marks
ii. What happens when a beaker of air is inverted over trough of water containing dissolved alkaline pyrogallol left overnight? 3marks
iii. What are the products of the combustion of a candle? Describe an experiment to identify the products of the burning candle. 3marks
4a.State the law of multiple proportion. 2marks
b. ii. A metal M forms two chlorides P and Q. On analysis,2.00 g of p was found to contain 0.69g of M and 10.0g of Q was found to contain 4.41g of M.
I Calculate the mass of chlorine which combined with 1.00g M to form P and Q respectively.
II. Deduce whether the law of multiple proportions is obeyed.
III. Write the correct formula of P and Q. 5 marks
c. If 250cm3 of a gas at s.t.p is heated to 270C at constant pressure, calculate its new volume. 3marks
5.(a) State the type of chemical bonding which accounts for each of the following observations
Chlorine exists as discrete molecules
ii. Sodium chloride dissolves readily in water.
iii. CuSO4(aq) forms a deep blue complex ion with excess NH3(aq)
Name the type of bonds that exist in each of the following compounds:
iv.CaCl2
v.NH4Cl
vi.CCl4 3marks
(b).How many moles of calcium trioxocarbonate (iv) are there in 5.0g of calcium trioxocarbonate(iv)?(Ca=40, C=12,O=16) 1mark
c. Complete and balance this equation.
i. Mg(s)+O2——
ii. NaOH (aq)+H2SO4
iii.H2SO4+Al(OH)3—–
iv.KOH+H2SO4——– 6marks
SS2 CHEMISTRY EXAM QUESTIONS SECOND TERM – EDUDELIGHT.COM
CLASS: S S 2 SUBJECT: CHEMISTRY
- What is the electronic configuration of sodium? 1S2522P6352 (b)1522522P6352 (c)1522522P6351 (d) 1522522P6350 (e) 1522P63523p6451
- Which of the following statements is true?
(a)An increase in temperature increases number gas molecules. (b)Increase in temperature does not affect kinetic energy
©Increase in temperature is proportimal to volume
(d) decrease in pressure decrease number of gasmol.
- An element is said to be electronegative if a.If is an halogen
- If is an Alkali earth metal
- If is an Alkali
- What is the consequence of increasing the equilibrium reaction? Zn0(g)
+theg = Zn (g) + H20(L) a.Equilibrium is driven to the left b.Equilibrum is driven to the right c.There is no effect
d.More Zn0(s) is produces
- An isotope has an atomic number of 17 and a mass number of 36, which of the following gives the correct number of neutron and protons in an atom of the isotope?
| Neutrons | Protons | |
| A | 53 | 17 |
| B | 17 | 36 |
| C | 19 | 17 |
| D | 36 | 17 |
Use this information to answer the following questions
Four elements, P,Q,R,S, have atomic number 4,10,12 AND 14 Respectively. 6.Which is a notable gas a. P B. Q C. R D. S
- Which is an ALKALI-METAL a. P b. Q C. R d. S
- Which is an ALKALI- EARTH METAL A. P B. Q C. R D. S
- The element with electronic configuration 1s2,2S2,2P3 is a. oxygen b. Chlorine c. nitrogen d. calcium
- How many electron are in L shell a. 2 b. 5 c. 8 d. 16
- Which of the following reaction is endothermic a. C[s] + O2 [g] — CO2[g]
b. CaO(s) + H2O© → (a{OH]2cs) c.Ccs = H20 → C0(g) = H2(g)
d. HCIcag) + Na0Hcag) →NaCIcag0 + H20©
12.A catalyst speed up the rate of chemical reaction by a.Taking part in the reaction
b.lowering the activation energy of the reaction. c.increase the heat content
d.increase the activation energy
- The electronic configuration of two atoms X and Y are as follows: X –IS22522P63S2
Y- IS22522P63S23P64S2
Which of the following statement is correct about the position of elements X and Y in the periodic table
a.X belongs to group 1,Y belongs to period 2
b.X belongs to group 1.Y belongs to period 1
c.X belongs to group 2,Y belongs to period 1
d.X belongs to group 3,Y belongs to period 2
- The electronic configuration 1S2 2S2 2P6 3S2 3P6 is that of a. noble gas b. Group 11 element c.group 3 element d. group vi element
- Which of the following statements is not correct a. diatomic b. good oxidizing agents c. Highly electronegative d. have high electron affinity
- An element whose atomic number 19 has the electronic configuration
a. IS22522P63523P7
b.1522522P63523P23P63d1 c.1S22522P63S33P6 d.IS22512P63523P6452
- Chlorine is used in water treatment as a. a germicide b. decolorizing agent c.an antioxidant d. a coagulating agent
- The valency of chlorine is a. -1 b. -5 c. -3 d. +1
- Isotopy is observed in which of the following element a. chlorine b. carbon c. oxygen d. fluorine
- The position of an element on the periodic table is determined by its
a. its density b. its atomic radius c. atomic number d. neutron number
- What is the molar mass of alkyne with the formula CXH14 [H=1 C= 12] a. 86g b.92g c. 98g d. 110g e. 112g
- Which of the following is not a separation techniques a.distillation
b.propiation
- chromatography
- distillation
- Which of the following is not an halogen a. silicon b. fluorine c. astatine d. bromine e. iodine
- An atom X consist of 6 protons, 6 electrons and 7 neutrons, Which of the following representation of atom is correct
- 13 X
6
(b) 13 x
7
(c) 19 X
6
(d) 7 19 X
- The following atoms of carbon 126C,136C and 146C can be described as a. allostropes b. isomas c. isotopes d. isotones
- How many electrons are there in 4Be2+ a. 2 b. 4 c. 5 d. 6
- An atom of an element X gains two electrons.The symbol of the ion formed is a. X b. X+ c. X2+ D d.X2-
- In the periodic table,all the elements within the same group have the same.
A.number of neutron
- number of valency electron
- numbers of isotopes
- atomic number
- In the periodic table,alkaline earth metals can be found in group
- 1
- 11
- vi
- vii
- Which of the following instruments is used in detecting the presence of radiation
- cathode ray tube
- Greiger-Muller Counter c.
Mass spectrometer
d. X-ray tube
- Which of the following elements is a metalloid a. carbon b. oxygen c. silicon d. sodium
- The shape of graphite crystal is a. tetrahydra b. pyramidal c. hexagonal d. octahedral
- Which of the following ions has the electronic configuration 2,8,8 a. Na+
- g2+ c. F d. Cl—
- An element with electronic configuration of 1S,2S,2P would have the combining power of a. 0 b. 2 c. 6 d.8
- Which of the following has the electronic configuration; 1S 2S 2P 3S 3P[Na,Al,N,S] a.0 b. 2 c. 6 d. 8
| 21 |
Find the number of neutons in an atom represented by 46 X a. 21 b. 24 c. 45 d. 66
- The activation energy of a reaction can be altered by a. adding reduction agent b. applying a higher pressure c. using a catalyst d. changing the temperature
- The phenomenon observed when particlesof colloidal solutionblock the part of light rays and scatter them is known as a.diffusion b. tyndal effect c.dialysis d. Brownian movement
- Which of the following substances causes the depletion of the ozone layer in the atmosphere a. CO2 b. Chloroform carbon c.Sulphur [iv]oxide
d. hydrocarbon
- A consequence of global warming is a. air pollution b. water pollution
c. Increased humidity d. Flooding
SS2 CHEMISTRY EXAM QUESTIONS SECOND TERM – EDUDELIGHT.COM
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