CHEMISTRY EXAM QUESTIONS SS1 SECOND TERM
SECOND TERM SS1 CHEMISTRY EXAM QUESTIONS – 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 1
1. Which of the following decreases when a given mass of gas is compressed to half its initial volume?
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? 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
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 2 moles of ammonia at S.T.P? a. 44.8dm-3 b. 22.4dm-3
c. 11.2dm-3 d. 5.6dm-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.ʅ32/2 b. ʅ16 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 mas of chlorine gas which occupies a volume of 1.12dm3 at s.t.p.(Cl=35.5, 1 mole of gas occupie 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) 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 00C is 27.3cm,what will be the volume of the gas at 100C, 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
31. 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
32. 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
33. 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
34. What is the value of X in the following equation?
2H2S + SO2→ 2H2O + XS A. 6 B. 4 C.3 D. 2
35. 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
36. 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
SECOND TERM SS1 CHEMISTRY EXAM QUESTIONS – EDUDELIGHT.COM
THEORY
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:
a. hydrogen fluoride
b. argon 2marks
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
SECOND TERM SS1 CHEMISTRY EXAM QUESTIONS – EDUDELIGHT.COM
CHEMISTRY
SECOND TERM EXAM SS 1
(1).The atomic number of chlorine is 17 what is the number of electrons in a chloride? (a) 16 (b) 17 (c)18 (d) 19
(2) A hydrogen atom which has lost an election contains
(a) one electron only (b) one proton & one neutron (c) one proton only (d) one proton, one electron & one neutron
(3).The following atoms of carbon 12 C and 14 C can be described as (a)
Allotropes (b) Somers (c) Isotopes (d) Isotones
(4).How many electrons are present in 94be2+? (a) 2 (b) 4 (c) 5 (d) 6
(5). The general gas equation pv/t=K is a combination of
(a) Boyle’s and Charles laws (b) Boyle’s and grahams law (c) charle’s and graham laws (d) Dalton atomic theory
(6).The law which describe the relationship between volume and temperature is ? (a) boyle’s law (b) Charles law (c) dalton’s law (d) graham’s law
(7).An atom of an element X gains two electrons the symbol of the ion formed is (a) X4 (b) X24 (c) X2- X-
(8).The general gas equation was derived from
(a) Boyle’s and gay lussac’s law
(b) Boyle’s and grahams law
(c) Boyle’s and Charles laws
(d) Dalton atomic theory
(9) The compound formed between 14X and 16Y is?
(a) X7 (b) XY2 (c) X2Y (d)X4Y6
(10). The negatively charged particle in an atom is (a)electron (b)neutron (c)position (d)proton
(11).How many orbitals are contained in an atom with atomic number 13? (a)7 (b)6 (c)5 (3)
(12).H+ (ay) +OH(ay) H2O(1) the above equation represents?
(a)hydrolysis (b)hydration (c)neutralization (d)electron affinity
(13).pH of 0001m acid is (a)2 (b)3 (c)4 (d)1
(14) Which pH value indicates a basic solution? (a)-1 (b)3 (c)0 (d)9
(15) Temporary hardness of water is removed by the use of the following exept
(a) Boiling
(b) Use of CaCoHD2
(c) Use of Na co3
(d) Use of alum
(16).One of this is not a water pollutant (a) petroleum (b)domestic liquid and solid water (c) industrial effluents (d) biodegradable chemicals
(17).Temporary hardness is due to the presence of
(a) Calcium hydrogentrioxo carbonate(iv)
(b) Soldium trioxocarbonate
(c) Calcium trioxide
(d) Magnesium trioxide
(18).A pH scale of 7 shows that the solution is ? (a)basic (b)Acid (c)newtral (d) basicitic
19. Neutralization is defined as ?
(a) Reaction with acid & base to produce hydrogen and water
(b) Reaction with acid &salt to produce C02 and water. (c)Reaction between acid & base to produce salt and water
20. pH scale of between 8 – 14 represents ?
(a) Slightly Alkaline very Alkaline (b) Very Alkaline – Slightly Alkaline (c) Neutral solution
21. is a compound formed when all the ionizable hydrogen of an acid is replaced by a metallic or ammonium ions (a) Base (b) Alkaline (c) Salts
22. Which pH value represents a basic solution (a) – 1 (b) 3 (c) 9 (d) 0 (e) 7
23. PiVi = P2V2 supports (a) Charle’s law (b) Boyle’s law (c) Graham’s law (d) Avogadro’s law
24. Standard temperature and pressure is ? (a) 7600 C and 273 mmHg (b)3600 and 760mmHg
(c) 273k and 760 mmHg
25Which of the following elements undergo Isotopy? (a) Potassium (b) Chlorine (c) Hydrogen
26. Kelvin temperature can be converted into celcius by (a) 0c = k – 273(b) K + 273 (c) 0c +K273 (d) K + 273
K 0C
27. Which of the following is an Avogadro’s constant (a) 6. 02 x1025 (b) 6.02×1022 (c) 6. 02 x 1023
28. Which of the three statesie of matter has no fixed shape, no fixed volume and least dense.
(a) Gas(b) Liquid (c) solids
29. Na2804 is the chemical formula for
(a) Sodium trioxonitrate (v) (b) Sodium tetraoxonitrate (vi) (c) Sodium tetraoxonitrate (v)
30. Na2Co3 is the chemical formula for
(a) Sodium silicate (iii) (b) Sodium carbonoxygen(iv) (c) sodium trioxocarbonnate (v)
31. What is the electronic configuration of an element represent b 199X
(a) 1522522p6 (b) 1522523523P3 (c) 1522P22P3352 (d) 1522522P63523P6451
32. which of the following atoms contains the highest number of electronics in the outermost shell
(a)80 (b) 10Ne (c)15P (d)19K
33Which of the following electronics configuration represents an element in groups of the periodic table
(a)152252 2P3 (b) 1522522p6 (c) 1522522P63523P4 (d)1522522P63523P6451
34. How many protons does 40 Ca contain (a) 12 (b) 20` (c) 40
35. Which of the following is the d.block element ?
(a) Calcium (b) iron (c) Lithium (d)silicon
36. Which of the following elements is diatonic ?
(a) iron(b) Neon (c) Oxygen (d) sodium
37. Which of the following elements is a metalloid
(a) Carbon (b) oxygen (c) silicon (d) sodium
38. Electronic configuration of 26fe3+ is
(a) {Ar} 452 3d6 (b){Ar} 4523d3 (c) [Ar} 451 3d4 (d) [Ar] 450 3d5
39. An atom W has 17 electronics , 18 protons and 17 neutrons. it would be represented as ? (a)35 W (b) 35 W (c) 17 W (d) 17 W
40, The two elements iix and 19Y are in the same group because they have the same .
(a) Valence electronics (b) Ionization energy (c) number of shell (d) atomic size
41. The combining power of an element is called? (a) Valency
(a) Electron (c) mixture (d) Atom
42. An atom X consists of 6 protons, 6 electrons and 7 neutrons. Which of the following representation of the atom is correct?
(a) 13 x (b) 13 X (c) 19 X (d)19 X
43. Fluorine has number of protons?
(a) 12 (b) 9 (c) 14 (d) 13
b. Which is not a career in chemistry?
(a)Engineering (b) Electrophysics (c) Chemist (d) Technologist Use the information to answer the following question
44. X If an element X has an Atomic number of 15 and a molecular number 25
c. It would be represented by
(a) 25 X (b) 10 X (c) 25 X (d)35 X
45. It has number of neutrons?
(a) 10 (b)15 (c) 25 (d) 20
46. It has Number of protons
(a) 10 (b) 15 (c) 25 (d) 20
47. If the electronic configuration is 2, 8, 8, 7, what is the valency of this element (a) -2 (b) +3 (c) -1 (d)-4
48. The IUPAC name for Na2804 is?
(a) Sodium (iv) sulphate
(b) Sodium tetraoxosulphate(vi)
(c) Sodium tetraoxide
(d) Sodium (vi) sulphate
49. Precipitation is a separation technique that allows the use of a Burnsen Burner? (a)True (b) False (c) None of above
CHEMISTRY EXAM QUESTIONS SS1 SECOND TERM
THEORY
(1)(a) Define an acid, Base and a salt
b) Give the natural resources of the following organic acid
(i) Lactic acid (ii) Abscorbic acid iii)Amino acid
(c) define buffer solution, give two uses of buffer solution
(d) define basicity of an acid
(e) List three (3) types of salt and explain them
(f) State three (3) uses of salts
(2) define the following laws :
I. Charle’s Law
II. Avogadro’s Law
III. Gay-Lussac’s Law
(2)(b)(i) Define Atom (ii)Molecules (iii)Compounds (iv) Valency (v)Isotopy
(c) Give a diagrammatic representation of the pH scale
(d) If 12. 2 of lead (ii) Trioxonitrate (v) were discussed in 21g of distilled water at 200C. calculate the solubility of the solute in mol dn-3
(3) An atom X has an atomic number 5 and a molecular number 9, while an atom Y has an atomic number of 12 and a molecular number of 25, Determine :
I. The number of protons of X
II. The number of neutrons of atom Y
III. The valencies of X and Y
IV. The names of atom X and Y
V. Electronic configuration of X and Y {SPDF}
VI. The chemical reaction between X and Y
(b) Write the first 20 elements and their valencies, and their groups and periods. (c)Describe the common causes of water pollution in Nigeria
(4) Differentiate between hard and soft water.
(a) Differentiate between temporary and permanent hardness including the ions involved
(b) State how to treat hard water.
(5) Balance the following equation I. S02 + 02 = S02
II. A2 + B2 = AB
III. S20 + H ↔S02 + H20 +S
(b) Distinguish between strong and weak acid
(c) State the groups from 1-8, their common names and their chemical properties
CHEMISTRY EXAM QUESTIONS SS1 SECOND TERM
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