1. Which of the following instrument is used in detecting the presence of radiation?

A. Cathode ray tube

B. Geiger-Muller counter

C. mass spectrometer

D. X-ray tube


2. The molecule which has linear shape is

A. CH4

B. NH3

C. H2S

D. CO2


3. The formula of the compound formed between a trivalent metal, M and a divalent on-metal, Y is 

A. M2Y3

B. M3Y2


D. M3Y


4. An atom of an element X gains two electrons. The symbol of the ions formed is

A. X+

B. X2+

C. X2–

D. X


5. Which of the following statements is correct?

A. atomic size decreases down the group

B. Atomic size increases across the group

C. Anions are similar than the present atom

D. Cations are smaller than the parent atom


6. Which of the following arrangement represents the correct order  of electronic energy level?

A. 1s 2p 2s 3p 3s 3d 4s

B. 1s 2s 2p 3s 3p 3d 4s

C. 1s 2s 2p 3s 3p 4s 3d

D 1s 2s 3s 2p 3p 4s 3d


7.The element with electron configuration 1s2 2s2 2p6 3s2 3p1 belongs to

A. s – block, period 3, group 1

B. p – block, period 3, group 2

C. s – block, period 3, group 3

D. p – block , period3,  group 3


8.In the period table, all the elements within the same group have the same

A. umber of neutrons

B. number of valence electrons

C. number of isotopes

D. atomic


9. Which of the following halogens is liquid at room temperature?

A. Iodine

B. Chlorine

C. Bromine

D. Fluorine


10. Rare gases are stable because they are

A. are chemical active

B. contain equal number of protons and neutrons

C. contain more electrons than protons

D. have octet structures


11. In the periodic table, alkaline earth metak ca be found in groups

A. I





12 which of the following series are the atoms arranged in order of increasing ionization energy?

A. Li, Na, K

B.B, Be, Li

C. O, F, Ne

D. Be, Mg, Ca


13. Which of the following bond types is responsible for high boiling of water?

A. Metallic bond

B. covalent bond

C. ionic bond

D. Hydrogen bond


14. In metallic solid, the forces of attraction is between the mobile valence electrons and the

A. atoms

B. neutrons

C. negative ions

D. positively charged nuclei


15.  The bonds in crystalline ammonium chloride are

A. covalent and dative

B. ionic and covalent

C. ionic, covalent and dative

D. ionic, covalent and hydrogen bond


16. Which of the following elements is diatomic?

A. Sodium


C. Iron

D. Neon


17. Noble gas molecules are held together by

A. Van dar waals forces

B. Hydrogen bonds

C. dative bonds

D. covalent bonds


18. Which of the following statements about nuclear reaction is correct? The reaction

A. Involves neutrons only

B. takes places inside the nucleus

C. is governed by temperature and pressure

D. involved protons and electrons


19. Consider the reaction represented by the following equation

${{C}_{2}}{{H}_{2}}+y{{H}_{2}}\to {{C}_{2}}{{H}_{6}}$

The value of y in the reaction is

A. 4

B. 3

C. 2

D. 1


20. The volume of 0.25 mol dm–3 solution of KOH that would yield 6.5g of solid KOH on evaporation is (K =39.0; O =16.0; H =1.00)

A. 464.30cm3

B. 625.00  cm3

C. 1000.00cm3

D. 2153.80cm3


21. The percentage by mass of calcium in Ca(OCl)2 is [ca = 40.0, Cl =35.5, O =16.0

 A. 28.0%

B. 31.6%

C. 43.8%

D. 44.5%


22. The gas law which describes the relationship between volume and temperature is

A. Boyle’s law

B. Charles’s law

C. Dalton law

D. Gramham’s law


23. Which of the following phenomena leads to decrease in volume of a liquid in a open container?

A. Brownian motion

B. Diffusion

C. Evaporation

D. Sublimation



24. The pressure exerted by a gas is a function of the

A. total volume of the gas

B. speed of the gaseous molecules

C. mass of each gaseous molecule

D. frequency of collision between gaseous molecules


25. Which of the following gases are arranged in increasing order of diffusion rate?

[H =1.0, C = 12, N=14, O =16, S =32]

A. SO2, O2, NH3, H2

 B. H2S, NH2, O2, SO2

C. CO2, N2O, O2, SO2

D. NH3, NO2, N2, CO2


26. Which of the following variables is a measure of the average kinetic energy of the molecules of a gas?

A. Density

B. Pressure

C. Temperature

D. Volume


27.When heat is absorded during a chemical reaction, the reaction is said to be

A. adiabatic

B. endothermic

C. exothermic

D. isothermal


28. The aqueous solution which has pH >7

A. FeCl2(aq)

B. CuSO4(aq)

C. KNO3(aq)

D. Na2CO3(aq)


29. Which of the following acid readily react with CaCO3 to liberate CO2?


B. H2SO4

C. H2SO3



30. Which of the following compound crystallizes without water of crystallization?

A. MgSO4


C. NaCl

D. FeSO4


31. A substance is said to be impure if

A. its melting point range is wide

B. it dissolves in water with difficulty

C> it has a low melting point

D. it is coloured


32 The following affect the solubility of a solid in a given solvent except

A.  nature of solute

B. nature of solvent

C. pressure

D. temperature


33. Consider the reaction represented by the equation:

${{N}_{2}}{{O}_{4(g)}}\rightleftharpoons 2N{{O}_{2(g)}}:\text{ }\Delta =+x\text{ }KJmo{{l}^{-1}}$

What happens when the temperature is reduced at equilibrium?

A. concentration of N2O4 decreases

B. concentration of N2O4 increases

C. Pressure exerted by the gases increases

D. pressure exerted by the gases remains constant


34.  Which of the following cells produce electrical energy from chemical reactios

I. Lead-acid battery

II. Dry cell

III. Daniel cell

IV. Electrolytic cell


35. What happens at the cathode during electrolysis?

A. anion is oxidized

B. anion loses electrons

C. cations is oxidized

D. cations is discharged


36. Which of the following substance are electrolytes?

I. PbBr2(l)

II.  NaCl(aq)

III. NaCl(s)

IV. C6 H12O6(aq)

A. I and II only

B. I, II and IV only

C. III and IV only

D. I and III only


37. Consider the redox reaction as represented by the following equation

${{I}_{2(aq)}}+2{{S}_{2}}O_{3(aq)}^{2-}\to 2I_{(aq)}^{-}+{{S}_{4}}O_{6(aq)}^{2-}$

Which of the species in the equation is reduced?

A. ${{S}_{4}}O_{6(aq)}^{2-}$

B. ${{S}_{2}}O_{3(aq)}^{2-}$

C. I2(aq)

D/ $I_{(aq)}^{-}$


38. The separation of petroleum fractions depends on the difference in their

A. melting points

B. molar mass

C. solubilities

D. boiling points


39. The major product formed by the reaction between ethanoic acid ad aqueous sodium hydroxide is

A. soap

B. Sodum ethanoate

C. sodium methoxide

D. water


40. Which of the following organic compounds would decolourize  bromine water?

A. Benzene

B. Cyclobutane

C. Hexane

D. Pentane


41. How many isomers has C3H6Cl2?

A. 2

B. 3


D. 5


42. The IUPAC name of the compound \[{{(C{{H}_{3}})}_{2}}CHCHC\underset{\underset{N{{H}_{2}}}{\mathop{|}}\,}{\mathop{H}}\,OOH\] is

A.2 – amino hexanoic acid

B.2–amino–4–methyl pentanoic acid

C. 2,4 – dimethyl butanoic acid

D.  4 – amino pentanoic acid


43. Which of the following reactions is common to all hydrocarbons?

A. combustion

B. Addition

C. polymerization

D. condensation



44.A hydrocarbon compound contains 92.3% carbon. Determine its empirical formula

[H =1.00, C =12.00]


B.  CH2

C. CH3

D. C2H2


45. The main function of limestone in the blast furnace is to

A. act as catalyst

B. act as reducing agent

C. remove impurity

D. supply carbon (IV) oxide


46. Which of the following raw material is used in a plastic industry

A. ethane

B. methane

C. calcium

D. hydrogen


47. Which of the following statement about thermoplastic material is correct? They j

A. do not melt on heating

B. harden on heating

C. decompose on heating

D. soften and melt on heating


48. Bronze is a mixture of

A. Cu and Mg

B. Cu and Sn

C. Cu and Zn

D. Cu and Pb


49. Which of the following statement about fine chemical is correct?

A. is injurious to health

B. has low degree of purity

C. is produced in relatively small amount

D. can be stored for a log time


50.Which of the following material is classified as a non – biodegradable pollution?

A. Animal hide

B. Paper

C. Plastic

D. Wood