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Chemistry
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Paper Type: Objective (PT. 1-4)

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 JUPEB CHEMISTRY PAST QUESTIONS (PT. 4)

SECTION A A. proton acceptor.

B. proton donor.
MULTIPLE CHOICE QUESTIONS C. electron acceptor.
Time Allowed: 1 Hour D. electron donor.

Answer All Questions. 4. Isotopes of hydrogen differ from

one another in _____
1. The reproducibility or
repeatability of a measurement is A. atomic number.
termed _____ B. number of protons.
C. number of electrons.
A. Accuracy D. number of neutrons.
B. Precision
C. Range 5. A solution of known
D. Confidence Interval concentration is termed a _____

2. The alpha (α-) scattering A. standard solution.

experiment is synonymous with B. unsaturated solution.
_____ C. saturated solution.
D. supersaturated solution.
A. J. J. Thomson
B. Ernest Rutherford 6. Which of the following is the
C. James Chadwick reason why CCl4 is non-polar?
D. Henry Mosley
A. The polar bonds cancel each
3. According to Brønsted-Lowry, other.
an acid is a\an _____ B. The molecule is non-linear.
C. The molecule is covalent.

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D. Small electronegativity + 2+
9. 𝑋 𝑔 → 𝑋 + 𝑒−. The energy
𝑔
difference between C and Cl.
utilized in the equation is typical of
_____
7. In what period of the periodic
table can the element with the
A. 1st electron affinity
electronic configuration 1s2 2s2 2p6
B. 1st ionization energy
3s2 3p6 4s2 3d1 be found?
C. 2nd ionization energy
D. 2nd electron affinity
A. 4
B. 3
10. Which of these electronic
C. 2
configurations belong to an
D. 1
element in period 3 of the periodic
table?
8. When a proton and an electron
beam are subjected to the same
A. [Ne] 3s1
strong electric field, the electron
B. 1s2
beam is deflected at a greater
C. [He] 2s2 2p3
angle than the proton beam
D. [Ar] 4s2 3d3
because _____

11. 0.200mol of a hydrocarbon

A. electron beam has a negative
undergo complete combustion to
charge while proton beam has a
give 35.2g of carbon dioxide and
positive charge
14.4g of water as the only
B. an electron is heavier than a
products. What is the molecular
proton
formula of the hydrocarbon? (C =
C. the electron is lighter than the
12.0, H = 1.0, O = 16.0)
proton
D. an electron has more electrical
A. C2H4
energy than a proton
B. C2H6
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C. C4H4 14. Fucoserratene, a hydrocarbon
D. C4H8 usually identified as the sexual
pheromone of the brown seaweed
12. Which of the following is the Fucus serratus has an empirical
best evidence of the presence of formula of C2H3. If the
ionic bonding in an unknown experimentally determined
substance? The substance molecular weight of this substance
conducts electricity _____ is 108 g/mol, the molecular
formula of fucoserratene is _____
A. in the solid state and in aqueous
solution. A. 𝐶4𝐻6
B. when molten and in aqueous B. 𝐶6𝐻9
solution. C. 𝐶8𝐻12
C. in the solid state and when D. 𝐶10𝐻15
molten.
D. when molten but not in the solid 15. Atoms of elements principally
state. go into bonding in order to achieve
_____
13. Decomposition reaction has a
half-life that does not depend on A. stability
the initial concentration of the B. covalency
reactant. What is the order of the C. electrovalency
reaction? D. attraction

A. zero order 16. In a chemical reaction, the

B. first order heat change at constant pressure
C. second order is referred to as _____
D. pseudo-first order
A. Entropy

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B. Enthalpy
C. Gibbs free energy ln k

D. Bond energy

17. In a given chemical reaction,

1/T (K-1)
the exponent(s) of the
concentration terms with respect
Which of the following is a measure
to the reactant species as
of the slope?
determined experimentally is/are
called _____
𝐸𝑎
A.
𝑅
𝐸𝑎
A. Molecularity B. −
𝑅

B. Order of reaction E𝑎
C.
RT
C. Elementary step 𝑅
D. −
𝐸𝑎
D. Rate law

20. Equal numbers of moles of He

18. Which of the following is used
(g), Ar(g), and Ne(g) are placed in
as detector for radiations from
a glass vessel at room
nuclear processes?
temperature. If the vessel has a
pinhole-sized leak, which of the
A. Cyclotron
following will be true regarding the
B. Particle accelerator
relative values of the partial
C. Geiger counter
pressures of the gases remaining
D. Electron volts system
in the vessel after some of the gas
mixture has effused?
19. The following represents a plot
obtained from an experiment to
A. PHe > PNe > PAr
graphically determine the
B. PAr > PNe > PHe
activation energy of a reaction.
C. PNe > PAr > PHe
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D. PAr > PHe > PNe C. 6
D. 8
21. Sodium is not suitable as a
sacrificial anode to prevent 24. All the following will exhibit
corrosion of underground iron common ion effect except _____
pipes because _____
A. Addition of sodium acetate to a
A. It would react with groundwater solution of acetic acid.
quickly. B. Addition of sodium chromate to
B. It has less standard electrode a saturated solution of lead
potential than that of iron. chromate.
C. It will form an oxide coating that C. Addition of hydrochloric acid to
prevents further oxidation. a saturated solution of silver
D. It is not a transition metal. chloride.
D. Addition of hydrochloric acid to
22. A solid which contains more a saturated solution of silver
than one type of bonding is _____ nitrate.

A. Ice. 25. When white phosphorus burns

B. Diamond. in air, it produces phosphorus (V)
C. Iron. oxide. P4(s) + 5O2(g) → P4O10(s);
D. Calcium oxide. ΔH = – 3010 kJ
What is ΔH for the following
23. What is the coordination equation?
number of the coordination P4O10(s) → P4(s) + 5O2(g)
compound Pt(NH3)2C2O4?
A. +3010 kJ
A. 3 B. –3010 kJ
B. 4 C. +602 kJ

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D. –602 kJ A. They have a valency of -1
B. They belong to the p-block of
26. Water gas is a mixture of two the periodic table
gases namely _____ C. They are all non-metals
D. They are all reducing agents
A. 𝐶𝑂 𝑎𝑛𝑑 𝑁𝑂 with Fluorine having the highest
B. 𝐶𝑂2 𝑎𝑛𝑑 𝐻2 reducing power
C. 𝐶𝑂 𝑎𝑛𝑑 𝐻2
D. 𝐶𝑂 𝑎𝑛𝑑 𝐻2𝑂 29. Transition elements usually
exhibit variable oxidation states
27. Which of the following is/are mainly because _____
true of alkali metals
A. they are metals
(I) They have the largest size B. they are employed as catalysts
in their respective period C. their d-electrons are involved in
(II) They have weak metallic bonding
bonding D. they have high melting and
(III) They are soft and they boiling point
have low melting point
30. The highest oxidation number
A. I only of iodine is _____
B. II only
C. I, II and III A. -1
D. I and III only B. 0
C. +5
28. The following statements are D. +7
properties of group 17 elements
except _____ 31. Which of the following does not
exhibit allotropy?

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A. Sulphur 34. Which group of particles is in
B. Phosphorus order of increasing size?
C. Carbon
D. Nitrogen A. N, O, F
B. N3- , O2–, F–
32. Which of the following inter- C. Na+, Mg2+, Al3+
halogen compound below does not D. Na+, Ne, F–
exist?
35. Diagonal relationships exist
A. ClBr3 between the following pairs except
B. IF3 _____
C. ClF5
D. ICl3 A. Be and Al
B. B and Si
33. Why is the ionic radius of a C. Li and Mg
chloride ion larger than the ionic D. Mg and Al
radius of a sodium ion?
36. Chlorine react with methane in
A. A chloride ion has one more the presence of sunlight through a
occupied electron shell than a process known as free radical
sodium ion reaction, which equation
B. chlorine has a higher proton represents the propagation step?
number than sodium
C. Ionic radius increases regularly A. CH4 + Cl• → CH3• + HCl
across the third period B. CH3• + CH3• → C2H6
D. Sodium is a metal, chloride is a C. CH3• + Cl• → CH3Cl
non-metal D. Cl2 → 2Cl•

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37. What is the product of the 40. The hybridization of the carbon
reaction between bromine and atom in ethyne is _____
ethene gas?
A. sp4
A. 2-bromoethane B. sp
B. Bromoethane C. sp3
C. 1, 2-dibromoethane D. sp2
D. 1, 1-dibromoethane
41. The following types of
38. The IUPAC name of the isomerism are found in aliphatic
compound CH≡C-CH2-CH2-COOH alkanes EXCEPT _____
is _____
A. Geometric isomerism
A. 1-pentyn-4-oic acid B. Position isomerism
B. pentyn-1-oic acid C. Chain isomerism
C. 5-pentyn-1-oic acid D. Structural isomerism
D. pent-4-yn-1-oic acid
42. How many isomers are
39. A family of organic compounds possible for a hydrocarbon with
which follows a regular structural molecular formula C4H8?
pattern such that each successive
member differs from the preceding A. two
one by a −𝐶𝐻2− 𝑔𝑟𝑜𝑢𝑝 is termed B. three
_____ C. four
D. six
A. Homologue
B. Organic series 43. What compounds are formed
C. Homologous series when sodium metal reacts with
D. Isotopic series propanol?

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A. Sodium propoxide and solution to produce a mixture of 2-
hydrogen bromopropane and 1-
B. Sodium oxide and propene bromopropane?
C. Sodium hydroxide and propene
D. Sodium methoxide and water A. Addition
B. Substitution
44. Which of the following C. Elimination
chemical equations represents the D. Displacement
reaction of group 1 metal hydrides
(MH) with water? 47. How many counter ions are
there in the coordination
A. MH + H2O → MO + 3H compound [Co(NH3)5Cl]Cl2?
B. MH + H2O → MOH + H2
C. MH + H2O → MOH + 2H A. 1
D. MH + H2O → M + OH + H2 B. 2
C. 5
45. What are the geometric shape D. 6
and oxidation number of the cobalt
in the complex ion, 48. The product of oxidation of
[Co(NH3)4(H2O)2]3+? secondary alcohol with K2Cr2O7 /H+
is a/an _____
A. Tetrahedral, +3
B. Octahedral, -3 A. carboxylic acid
C. Octahedral, +3 B. ester
D. Tetrahedral, -3 C. aldehyde
D. a ketone
46. What type of reaction occurs
between propene and 49. The following are reducing
concentrated hydrogen bromide sugars EXCEPT _____

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A. Fructose
B. Sucrose
C. Maltose
D. Cellulose

50. How many isomeric forms are

there for the molecular formula
C3H6Br2?

A4
B1
C2
D3

CHECK YOUR ANSWERS

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the correct answer(s) to any or
all of these questions?

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 JUPEB CHEMISTRY PAST QUESTIONS (PT. 3)

SECTION A 3. Which states that no two

electron in an atom can have the
MULTIPLE CHOICE QUESTIONS same set of quantum numbers?
Time Allowed: 1 Hour
A. Hund’s rule
Answer All Questions. B. Aufbau’s principle
C. de Broglie hypothesis
1. Which of the following D. Pauli’s exclusion principle
statements is incorrect?
4. Calculate the relative molecular
A. An atom is electrically neutral mass of a gaseous compound if
B. The size of a cation is smaller 13.15g of the compound occupies
than that of the corresponding 4.80dm3 at STP.
atom
C. The size of an anion is bigger A. 61
than that of the corresponding B. 34
atom C. 24
D. An atom and its ion have an D. 29
unequal number of protons
5. Which of the following species
2. Bronsted-Lowry base is _____ has the same electronic
configuration as Al3+ ion?
A. an electron pair acceptor
B. a proton acceptor A. F-
C. an electron pair donor B. Cl-
D. a proton donor C. S2-
D. O-

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6. What is the volume of oxygen 9. The electronegativity value of Si
required to burn completely 45cm3 and H are 1.8 and 2.1 respectively.
of methane? What type of bond exist within
SiH4?
A. 400cm3
B. 180cm3 A. Ionic
C. 90cm3 B. Polar covalent
D. 22.5cm3 C. Coordinate covalent
D. Non-polar bond
7. Which of the following is TRUE
regarding a precipitation reaction? 10. When an atom is oxidized, its
oxidation number _____
A. both products must be soluble
in water A. decreases, as electrons are
B. At least one of the products will gained
be insoluble in water B. decreases, as electrons are lost
C. At least one of the reactants C. increases, as electrons are
must be insoluble in water gained
D. Spectator ion forms insoluble D. increases, as electrons are lost
salts
11. What mass of carbon dioxide is
8. Arrange the following in order of formed when 60.0g of carbon is
increasing boiling point: CH4, HCN, burned in 750.0g of oxygen? [C =
CaO 12, O = 16]

A. CH4 < HCN < CaO A. 60.0g

B. HCN < CH4 < CaO B. 160.0g
C. CH4 < CaO < HCN C. 220.0g
D. CaO < CH4 < HCN D. 1031g

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12. A solution capable of resisting 15. Calculate the standard e.m.f in
change in pH upon the small volts of a cell that uses the
addition of acid or base is _____ following half-cell reactions:

A. an aqueous solution Fe2+(aq)+2e- ⇌ Fe(s) E°Fe2+/Fe = -0.44v

Ni2+(aq) + 2e- ⇌ Ni(s) E°Ni2+/Ni = -0.25v
B. a colloidal solution
C. a buffer solution
A. 0.18
D. a super saturated solution
B. 0.69
C. 0.11
13. What is the percentage by
D. 0.19
mass of carbon present in 6.0g of
a hydrocarbon which burns
16. What is the oxidation number
completely in air to produce 11.0g
of oxygen in Na2O2?
of carbon dioxide? [C=12, O=16]

A. -1
A. 25%
B. +1
B. 33%
C. -2
C. 50%
D. +2
D. 75%

17. If the enthalpy of a given

14. In which of the following
2
reaction is -215 kJ mol-1 and the
species is sp hybrid orbitals NOT
entropy change of the reaction is
involved?
15.2 J mol-1K-1 at 30°C, then the
reaction will _____
A. PCl3
B. BF3
A. not be spontaneous
C. C2H4
B. be spontaneous
D. CO2
C. be irreversible
D. be at equilibrium
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18. The temperature and pressure D. 0.572
at which the three phases of pure
water coexist respectively are 21. At 17°C, a sample of hydrogen
_____ gas occupies 125cm3. What will the
volume be at 100°C, if the pressure
A. 273 K and 760 mmHg remains constant?
B. 298 K and 1 atm
C. 0.01°C and 4.5 mmHg A. 21cm3
D. 0.273°C and 0.1 mmHg B. 91cm3
C. 161cm3
19. The pH of buffer solution D. 735cm3
depends upon the concentration of
_____ 22. Why is the first ionization
energy of phosphorus greater than
A. conjugate acid that of silicon?
B. conjugate base
C. salt A. The outer electron in
D. conjugate acid and base phosphorus is paired
B. The atomic radius of a
20. What is the mole fraction of phosphorus atom is greater
oxygen gas in a mixture containing C. A phosphorus atom has one
32.0g oxygen gas, 32.0g of more proton in its nucleus
methane gas and 32.0g of sulphur D. The outer electron in
(IV) oxide? [C=12, O=16, H=1, phosphorus is more shielded
S=32]
23. Which of the following pairs
A. 0.143 exhibit the most similar chemical
B. 0.286 properties?
C. 0.333

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A. Li and Mg C. LiCl
B. Ca and Zn D. LiBr
C. B and C
D. N and O 27. The colligative properties of a
solution are affected by _____
24. Which of the following metals
is not a first row transition A. nature of the solute
element? B. concentration of solute molecule
C. amount of liquid
A. V D. surface area of solute
B. Cd
C. Cr 28. What is the coordination
D. Mn number and oxidation state of the
central atom in [NiCl2(en)2]?
25. The following ions have noble
gas electronic configuration A. 6, 2
EXCEPT _____ B. 6, 0
C. 4, 2
A. Sr2+ D. 4, 4
B. Rb+
C. I- 29. Excess soil acidity caused by
D. Sn2+ acid rain can be neutralized by
_____
26. Which of the following
compound is the anion most A. adding more fertilizers
polarized? B. adding molten cryolite
C. adding brime
A. LiF D. adding quick lime
B. Lil

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30. Which of the following is an s- 33. Which of these reactions in
block element? equilibrium is unaffected by a
change in pressure?
A. Cs
B. Ar A. 2O3(g) ⇌ 3O2(g)
C. Cl B. PCl5(g) ⇌ PCl3(g) + Cl2(g)
D. He C. N2O4 ⇌ 2NO2
D. 2HI(g) ⇌ H2(g) + I2(g)
31. Use the following data to
determine the standard enthalpy 34. The trihalides of phosphorus
change formulation for solid ICl3. react with water to form one of the
following acids.
I2(s) + Cl2(g) → 2ICl(s)
∆H°=+14 kJ mol
A. H3PO4
ICl(s) + Cl2(g) → ICl3(s)
B. H5P3O10
∆H°=-88 kJ mol
C. H3PO3
D. H4P2O6
A. -60 kJ mol
B. -74 kJ mol
35. Which of the following
C. -81 kJ mol
hydrogen halides is the most
D. -162 kJ mol
acidic: HF, HCl, HBr, HI?

32. The oxide of nitrogen used as

A. HF
a mild anaesthetic for surgery is
B. HI
_____
C. HBr
D. HCl
A. nitrogen (IV) oxide
B. dinitrogen (I) oxide
36. The IUPAC name for
C. dinitrogen tetraoxide
[FeF4(H2O2]- is _____
D. nitrogen (II) oxide
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A. diaquatetrafluoroiron (III) ion D. 3-ethyl-4-butamine
B. diaquatetrafluoroferrate (III) ion
C. diaquatetrafluoroiron (III) 40. Heterolytic bond fission results
D. diaquatetrafluoroferrate (III) in the formation of positively
charged carbon species known as
37. Reaction between a hydrazine _____
and a carbonxyl compound yields a
_____ A. free radicals
B. carbanions
A. hydrazone C. carbonium ions
B. diazonium salt D. carbenes
C. benzaldehyde
D. phenyl hydrazine 41. The following statements are
true of an electrolytic cell EXCEPT
38. Which of the following is _____
tertiary amine?
A. it converts electrical energy to
A. CH3CH2NH2 chemical energy
B. CH3CH2NHCH3 B. a porous partition is not needed
C. (CH3CH2)2NCH3 C. cathode is negative electrode
D. CH(NH2)3 while anode is positive electrode
D. electrodes are in separate
39. Name the following organic compartment
compound.
CH3 CH2 CH CH2 NH2 42. The oxidation of
CH3CH2CHOHCH3 with potassium
CH2 – CH3
tetraoxomanganate (VII) gives
A. 3-ethylbutanamines
_____
B. 3-methylamine pentane
C. 2-ethylbutanamine
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A. CH3CH2CH2COOH D. polymerization reaction
B. CH3CH2COOH
C. CH3CH2COCH3 46. The compound with molecular
D. CH3CH2CH2CHOH formula C5H12 has _____

43. Hydrogenation of vegetable A. 2 isomers

oils to produce margarine is an B. 3 isomers
example of _____ C. 4 isomers
D. 5 isomers
A. addition reaction
B. substitution reaction 47. Consider the structure
C. elimination reaction
D. redox reaction C9H19

44. The enzyme suitable for the C H

conversion of starch to maltose is
_____

A. maltase What electronic effect is likely to

B. zymase be observed?
C. lipase
D. diastase A. Inductive effect
B. Electromeric effect
45. CH3CH2CHCHCH2CH3 does not C. Steric effect
undergo _____ D. Tautomeric effect

A. addition reaction 48. The following compounds

B. substitution reaction C6H13NH2, C3H7NH2, CH3CH2NH2,
C. combustion reaction

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and CH3NHCH3 are all related as D. Lower boiling point, low melting
_____ point and low density

A. chain isomers CHECK YOUR ANSWERS

B. homologues
C. functional group isomers Would you like to get or confirm
D. primary amines the correct answer(s) to any or
all of these questions?
49. Which of the following
reactions is suitable for the Download it NOW!
synthesis of alkenes?

A. Dehydration of primary alcohols

B. Hydrolysis of primary alcohols
C. Reduction of primary alcohols
D. Oxidation of primary alcohols

50. Branched chain isomers have

the following properties when
compared with their linear
isomers.

A. Low boiling point, low melting

point and high density
B. Lower boiling point, high
melting point and lower density
C. Higher boiling point, high
melting point and low density

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 JUPEB CHEMISTRY PAST QUESTIONS (PT. 2)

SECTION A C. The electron does not emit

energy when in the orbits
MULTIPLE CHOICE QUESTIONS D. Transitions between orbits are
Time Allowed: 1 Hour accompanied by emission or
absorption of radiation
Answer All Questions.
3. The following factors influence
1. Precision in measurement is ionization energies EXCEPT _____
_____
A. shielding effects of inner
A. agreement between replicate electrons
measurements B. magnitude of the nuclear charge
B. closeness of measurement to C. shape of the orbital containing
the true value the valence electron
C. estimated in terms of absolute D. distance of outer electrons from
error the nucleus
D. difference between measured
value and true value 4. The energy associated with the
process below is called _____
2. Which of the following is NOT an
assumption of Bohr’s model of Li(g) → Li+(g) + e-
atom?
A. electron affinity
A. Emission spectra of atom are B. ionization energy
continuous C. lattice energy
B. Electron moves in allowed orbits D. binding energy
around the nucleus

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5. The condensed electronic D. Microwaves are not visible
configuration of Zn2+ (Z=30) is
_____ 8. A base is a proton acceptor,
according to _____
A. [Ar] 4s2 3d10
B. [Ar] 4s2 3d8 A. Arrhenius concept
C. [Ar] 4s1 3d10 B. Bronsted-Lowry concept
D. [Ar] 4s0 3d10 C. Lewis concept
D. Dalton’s concept
6. All the following are attributes of
light EXCEPT _____ 9. A bottle of concentrated
hydrochloric acid solution has been
A. it consists of perpendicular reading “37.8% HCl by mass”.
electric and magnetic fields Calculate the molarity of this
B. its frequency is directly solution if it has a density of
proportional to its wavelength 1.1919g cm-3. [H=1.0, Cl=35.5]
C. it is both a photon and a wave
D. its speed in vacuum is fastest A. 11.3 M
B. 14.5 M
7. Which of the following is NOT C. 12.0 M
true of electromagnetic spectrum? D. 12.3 M

A. Visible light makes up a small 10. State the change in oxidation

proportion of the spectrum number of sulphur in the redox
B. The wavelength of ultraviolet reaction below:
radiation is greater than that of the
infrared radiation I2 + 2S2O32- → 2I + S4O72-
C. Gamma rays have shorter
wavelength A. -2 to -4

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B. +2 to +3 When 4 mol of nitrogen dioxide
C. -4 to -2 was put into 1 dm3 container and
D. +3 to +2 heated to a constant temperature,
the equilibrium mixture contained
11. What is the percent of carbon 0.8 mol of oxygen. What is the
in the glutamic acid, C5H8NO4? numerical value of equilibrium
[C=12.01, H=1.01, N=14.0, constant, Kc, at the temperature of
O=16.00] the experiment?

A. 8.22 0.82 × 0.8

A.
42
B. 24.3 1.6 × 0.8
B.
2.4 2
C. 41.1
1.62 × 0.8
D. 48.2 C.
42
1.62 × 0.8
D.
2.4 2
12. Which of the following
elements exhibits diagonal
14. In which of the following
relationship with aluminium?
reactions is the change in entropy
positive?
A. beryllium
B. silicon
A. 2Ag+(aq) + Zn(s) ⇌ Zn2+(aq) +
C. carbon
2Ag(s)
D. germanium
B. 2SO2(g) + O2(g) ⇌ 2SO3(g)
C. 2HF(g) ⇌ H2(g) + F2(g)
13. Nitrogen dioxide decomposes
D. H2O(s) ⇌ H2O(l)
on heating according to the
following equation.
15. A system in which only energy
is transferred between the system
2NO2(g) ⇌ 2NO(g) + O2(g)
and the surrounding is _____

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A. open system B. Na > K > Cs > Rb
B. isolated system C. Cs > Rb > K > Na
C. closed system D. Cs > K > Na > Rb
D. adiabatic
19. Hydride of the halogens with
16. Which of these orbitals is the the highest stability to heat is
most stable? _____

A. 3d A. HCl
B. 4p B. HBr
C. 5p C. HF
D. 5d D. HI

17. Identify the species A in the 20. Hydrocarbons which react with
radioactive reaction represented ammonical copper (I) chloride
by the equation below: solution conform to the general
234 238 molecular formula _____
𝐶 𝑇ℎ + 𝐴 → 𝑈
90 92
0
A. 𝑛
1 A. CnHn
1
B. 𝑒 B. CnH2n
0
1 C. CnH2n+2
C. ɤ
1 D. CnH2n-2
4
D. 𝐻𝑒
2
21. In the coordination

18. Arrange the following elements compounds, [Co(NH3)6] [FeCl4]x, if

in order of decreasing reducing the primary valences of both Co

power: Na, Rb, K, Cs. and Fe are both +3, what is x?

A. Cs > K > Rb > Na A. 2

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B. 1 B. β-
C. 3 C. γ
D. 5 D. β+

22. Which of the following is TRUE 25. For a reaction that is second
about sodium chloride in the solid order with respect to a reactant, A,
state? how many times does the rate
increase as [A] increases by a
A. Its ions are linked by metallic factor of 2?
bonds
B. It exists as aggregate of ions A. 1 time
C. It conducts electricity B. 2 times
D. It exists as discrete molecules C. 3 times
D. 4 times
23. A method of preventing
corrosion that involves coating 26. What is the number of atoms
steel with zinc metal is called present in 21.6g of Ag? [Ag=108
_____ gmol-1, NA=6.023 × 1023 mol-]

A. painting A. 0.2 × 1024

B. enamelling B. 1.204 × 1023
C. electroplating C. 6.02 × 1022
D. galvanizing D. 1.08 × 1023

24. What type of radioactive decay 27. Transition metal atoms without
produces a daughter nucleus with unpaired electrons are said to be
a higher atomic number? _____

A. α A. diamagnetic

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B. paramagnetic D. Graphite is partially soluble in
C. ferromagnetic water
D. anti-ferromagnetic
30. The oxidation state of Au in
28. Strontium I an element in K[Au(OH)4] is _____
Group 2 of the Periodic Table.
Which of the following statement A. +1
about strontium is NOT correct? B. +2
C. +3
A. Its first ionization energy is D. +4
lower than that of calcium
B. Its atomic radius is smaller than 31. Which of the following is NOT
magnesium true of a catalyst?
C. It has two electrons in its
outermost energy level A. Catalysts will decrease the
D. It forms a chloride with the activation energy of a reaction
formula SrCl2 B. Catalysts will be influenced by
the pH of the substance
29. Why is the melting point of C. Catalysts do not change the
diamond much higher than that of thermodynamics of the reaction
graphite? D. Catalysts cause a change in the
equilibrium constant of the
A. Diamond consists of covalent reaction
bonds extending in all directions
B. The structural layers of graphite 32. Which of the following will
are too far apart always produce a spontaneous
C. Diamond has a higher density reaction?
than graphite
A. Positive ∆H and a positive ∆S

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B. Positive ∆H and a negative ∆S what is the standard enthalpy (kJ
C. Negative ∆H and a positive ∆S mol) change of the reaction?
D. Negative ∆H and a negative ∆S
TiO2(s) + 2C(s) → Ti(s) + 2CO(g)
33. In the electrolysis of brine
(concentrated NaCl) using mercury A. -830
as the cathode, the components B. -720
produced and resulting solution C. +720
are _____, _____, and _____ D. +830
respectively.
36. The reaction C12H20O10 + 2H2O
A. H2, Cl2, and basic → 2C6H12O6 represents _____
B. Na, O2, and neutral
C. H2, O2, and basic A. polymerization of glucose
D. Na, Cl2, and neutral B. hydrolysis of carbohydrate
C. fermentation of sugar
34. The IUPAC name of K2[PtCl6] is D. dehydration of starch
_____
37. The shape and bond angle of
A. Potassium hexachloroplatinate (II) the sp2 hybridized orbital are
B. Potassium hexachloroplatinate (IV) _____
C. Platinum hexachloroplatinate (I)
D. Potassium hexachloroplatinum (II) A. tetrahydral and 109.5°
B. trigonal and 120°
35. Given that the standard C. trigonal and 180°
enthalpy changes of formation of D. linear and 180°
TiO2(s) and CO(g) are -940 kJ mol-1
and -110 kJ mol-1 respectively, 38. Calculate the volume of
oxygen evolved at 285K and 0.91

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× 105 Nm-2 when a current of 2.5A C. CH3CHOHCHO
is passed through acidified water D. CH3COCH2OH
for 1.5mins. [Molar volume of a
gas=22.4dm3, standard pressure 41. Which of the following is the
= 1.01 × 105 Nm-2, 1Faraday = final product from the reaction of
96500C] ethyne with hydrogen bromide?

A. 12.34 cm3 A. CH3 – CHBr2

B. 23.12 cm3 B. CH2Br – CH2Br
C. 15.13 cm3 C. CH3 – CH3
D. 9.13 cm3 D. CH2 = CHBr

39. Which of the following groups 42. The IUPAC name for
of compound forms a layer of silver CH3CH2CH2CHClCH3 is _____
when reacted with silver
troxonitrate (V) in the presence of A. 2-Chloropentane
excess ammonia? B. 2-Chloropropane
C. 4-Chlorohexane
A. Alkanols D. 4-Chloropentane
B. Alkanals
C. Alkanones 43. In Benedict’s test, a positive
D. Alkanoic acids test is indicated by a colour change
from _____
40. Which of the following
compounds is NOT a functional A. brick red to blue
group isomer of CH2OHCH2CHO B. brown to purple
C. blue to red
A. CH2=COHCH2OH D. purple colour change
B. CH3OCH2CHO

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44. The IUPAC name for the B. there are only four hydrogen
compound below is _____ atoms in ethane
CH2CH2CH2CH3 CH3 C. the carbons in ethane are
smaller than those of ethane
H3C – C – CH2 – CH2 – CH2 – C – CH2CH3 D. the carbons in ethane are linked
by double bonds
CH3 CH3

47. H3C – Br → CH3+ + Br

A. 5,5,9,9-tetramethylundecane
B. 3,3,7,7-tetramethylundecane
The above equation shows _____
C.2,6,6-trimethyl-2-n-butyloctane
D.3,3,7-trimethyl-7-n-butyloctane
A. substitution reaction
B. homolytic fission
45. Given below are sets of
C. heterolytic fission
homologous series, identify the set
D. electrophilic reaction
that contains a carboxyl group.

48. Which group of compounds

A. alkanes, alkenes, alkynes
produce yellow crystals of CHI3 in
B. alcohols, carboxylic acids,
the presence of I2/NaOH?
ethers
C. aldehydes, ketones, amines
A. Alkane
D. carboxylic acids, aldehydes,
B. Alkanone
ketones
C. Carboxylic acid
D. Ester
46. There is free rotation about the
carbons of ethane but not that of
49. Identify P in the reaction
ethane. This is due to the fact that
H2O/H+
_____ C2H5MgBr + P C2H5C(OH)(CH3)C3H7

A. C3H7CHO
A. the carbons in ethane are round
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B. C3H7COCl
C. C3H7COCH3
D. C2H5COC2H5

50. An element with an atomic

number of 35 is _____ block
element.

A. s-block
B. p-block
C. d-block
D. f-block

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 JUPEB CHEMISTRY PAST QUESTIONS (PT. 1)

SECTION A 3. How many atoms of Cu are

present in 35.4 g of Cu? [Cu = 63.5
MULTIPLE CHOICE QUESTIONS gmol-1]
Time Allowed: 1 Hour
A. 1.08 x 1024 atoms of Cu
Answer All Questions. B. 3.27 x 1023 atoms of Cu
C. 6.02 x 1023 atoms of Cu
1. A normal body temperature is D. 1.20 x 1022 atoms of Cu
37°C, Kw = 2.4 x 10-14. Calculate
[H3O+] and [OH-] for the body fluid 4. How would you prepare 250cm3
at this temperature. of 0.25M aqueous solution of NaCl?
[Na= 23g mol-1; Cl = 35.5g mol-1]
A. [H3O+] = [OH-] = 2.5 x 10-7
B. [H3O+] = [OH-] = 1.5 x 10-8 A. Add 3.66g NaCl to 250cm3 of
C. [H3O+] = [OH-] = 1.5 x 10-6 distilled water
D. [H3O+] = [OH-] = 1.5 x 10-7 B. Weigh 3.66g NaCl into 250ml
flask and add distilled water up to
2. Atoms of elements in a group on the mark
the Periodic Table have similar C. Add 14.60g NaCl to 250cm3 of
chemical properties. This similarity distilled water
is most closely related to the D. Weigh 14.60g NaCl into 250ml
atoms'. flask and add distilled water up to
the mark
A. number of principal energy
levels 5. What is the shape of PCl3?
B. number of valence electrons
C. atomic numbers A. Trigonal planar
D. atomic masses B. Trigonal pyramidal

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C. Tetrahedral B. Sodium has higher ionization
D. V-shaped (bent) energy
C. Sodium has a stronger metallic
6. Uranium -233 (233U92) decays by bond
α – emission. What is the decay D. Caesium has a larger atomic
product? radius

229
A. Th90 9. Transition metals can form
231
B. Th90 complex ions because _____
231
C. Ac91
233
D. Ac91 A. they have paired electrons in
the d subshell
7. Arrange the following ions in B. they have unpaired electrons in
order of decreasing charge density the d subshell
Ca2+, Mg2+, Al3+ and Ba2+ C. they have empty d orbitals
D. they have small charge/size
A. Al3+> Mg2+>Ca2+>Ba2+ ratio
B. Ba2+>Ca2+> Mg2+> Al3+
C. Al3+< Mg2+<Ca2+<Ba2+ 10. How many equivalent hybrid
D. Mg2+>Al3+>Ba2+>Ca2+ orbitals are there in Sp2-hybridised
carbon?
8. Which of the following
statements explain why caesium A. four
has a lower melting point than B. two
sodium? C. three
D. one
A. Sodium is a more
electropositive metal 11. When common names are
used for acids, the underlined

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carbon atom in the molecule C.
shown would be designated as the
_____ C atom. mass
O
time
CH3CH2CH2 – C – OH D.

A. gamma mass
B. alpha
C. delta time
D. beta
13. Which gas closely approaches
12. Purification of a strip of impure ideal behaviour at room
copper metal in aqueous CuSO4 temperature and pressure?
was carried out using a steady
current. Which graph shows the A. helium
change in mass of the cathode with B. carbon dioxide
time? C. ammonia
D. oxygen
A.
mass 14. A sample of a brown gas, a
major air pollutant, is found to
time contain 2.34g N and 5.34g O.
B. Determine the empirical formula
for this substance. [N = 14, O =
mass 16]

time A. NO2
B. NO

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C. N2O 17. The first stage in the
D. N2O3 manufacture of nitric acid is the
oxidation of ammonia by oxygen.
15. Why does the rate of a gaseous wNH3(g) + xO2(g) → yNO(g) +
reaction increase when the zH2O(g).
pressure is increased at a constant What values for w, x, y and z are
temperature? needed to balance the equation?

A. More particles have energy that A. 4, 5, 4 and 6

exceeds the activation energy. B. 4, 6, 4 and 5
B. The particles have more space C. 5, 6, 5 and 4
in which to move. D. 6, 5, 6 and 4
C. The particles move faster.
D. There are more frequent 18. The reaction of chlorine with
collisions between particles. methane is carried out in the
presence of light. What is the
16. Why is gaseous nitrogen less function of the light?
reactive than gaseous fluorine?
A. to break the C – H bonds in
A. The boiling point of nitrogen is methane
lower than that of fluorine. B. to break up the chlorine
B. The relative molecular mass of molecules into atoms
nitrogen is lower than that of C. to break up the chlorine
fluorine. molecules into ions
C. The atomic radius of nitrogen is D. to heat up the mixture
greater than that of fluorine.
D. The bond strength in the 19. In the Solvay process,
molecule is greater in nitrogen
than in fluorine.

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NaCl(aq) + NH3(g) + H2O(l) + CO2(g) What will be precipitated following
→ NaHCO3(s) + NH4Cl(aq) the addition of calcium hydroxide?

What volume of carbon dioxide (at A. CaCl2

s.t.p) is required to produce 1.00 B. CaCO3
kg of sodium hydrogencarbonate? C. Ca(NO3)2
(1 mole of gas at s.t.p occupies D. Mg(NO3)2
22.4 dm3) [Na = 23, Cl = 35.5, C
= 12, O = 16, H = 1, N = 14] 22. The electronic configuration of
the Fe3+ ion is _____
A. 250 dm3
B. 762 dm3 A. 1s2 2s2 2p6 3s2 3p6 3d4
C. 267 dm3 B. 1s2 2s2 2p6 3s2 3p6 3d5
D. 462 dm3 C. 1s2 2s2 2p6 3s2 3p6 3d3
D. 1s2 2s2 2p6 3s2 3p6 3d6
20. Which group of particles is in
order of increasing size? 23. An element with an atomic
number of 35 is _____ block
A. N, O, F element.
B. N3–, O2–, F–
C. Na+, Mg2+, Al3+ A. s-block
D. Na+, Ne, F– B. p-block
C. d-block
21. River water in a chalky D. f-block
agricultural area may contain Ca2+,
Mg2+, CO32-, HCO3-, Cl-, NO3- ions. 24. Iodine trichloride, ICl3, is made
In a waterworks, such water is by reacting iodine with chlorine.
treated by adding a calculated I2(s) + Cl2(g) → 2ICl(s) ; ΔHɵ =
quantity of calcium hydroxide. +14 kJ mol–1

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ICl(s) + Cl2(g) → ICl3(s) ; ΔHɵ = – 26. The standard enthalpy
88 kJ mol–1 changes of formation of HCl and HI
are –93 kJ mol–1 and +25 kJ mol–1
By using the data above, what is respectively. Which statement is
the enthalpy change of the most important in explaining this
formation for solid iodine difference?
trichloride?
A. The bond energy of Cl2 is
A. –162 kJ mol–1 smaller than the bond energy of I2.
B. –81 kJ mol–1 B. The activation energy for the H2
C. –74 kJ mol–1 / Cl2 reaction is much less than
D. –60 kJ mol–1 that for the H2 / I2 reaction.
C. The bond energy of I2 is smaller
25. The standard enthalpy than the bond energy of Cl2.
changes of formation of TiO2(s) D. The bond energy of HI is smaller
and CO(g) are –940 kJmol–1 and than the bond energy of HCl.
-110 kJ mol–1 respectively.
27. What is the catalyst used in the
TiO2(s) + 2C(s) → Ti(s) + 2CO(g) Contact process?

What is the standard enthalpy A. Pd

change of this reaction? B. Pt
C.Fe2O3
A. –830 kJ mol–1 D.V2O5
B. –720 kJ mol–1
C. +720 kJ mol–1 28. The main purpose of adding
D. +830 kJ mol–1 cryolite to the ore (bauxite) during
the preparation of aluminium
metal by electrolysis is _____

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A. minimizes the release of oxygen 31. How many chiral centres does
at the graphite anode the compound below possess?
B. reduce the melting point of the
bauxite CH2CO2H
C. increase the melting point of the
C(OH)CO2H
bauxite
CH2CO2H
D. enable the aluminium discharge
at the anode A. 0
B. 1
29. What type of bond needs to be C. 2
broken for magnesium oxide to D. 3
melt?
32. 0.200 mol of a hydrocarbon
A. Co-ordinate undergo complete combustion to
B. covalent give 35.2g of carbon dioxide and
C. ionic 14.4g of water as the only
D. metallic products. What is the molecular
formula of the hydrocarbon?
30. A substance which contains the
following elements by mass: C, A. C2H4
17.8%; H, 1.5%; Cl, 52.6%; F, B. C2H6
28.1% has molecular mass of 135. C. C4H4
Determine the molecular formula. D. C4H8

A. C2H2FCl 33. One of the original postulates

B. C2H2F2Cl of Dalton’s Atomic Theory is:
C. C2H2F2Cl2
D. C2HFCl3

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A. An atom reacts to attain A. electron affinity
electronic configuration of the B. binding energy
noble gas closest to it. C. ionization energy
B. When atoms of different D. electronegativity
elements react to form chemical
compound, the atoms are 36. If the activation energy in the
combined in simple whole number forward direction of an elementary
ratio. step is 52 kJ and the activation
C. The isotopes of an element are energy in the reverse direction is
in whole number ratio. 74 kJ, what is the energy of
D. Atoms of different elements reaction ∆E for this step?
differ in terms of number of
protons in their nuclei. A. 22 kJ
B. -22 kJ
34. The ions in a mass C. 52 kJ
spectrophotometer are separated D. -52 kJ
based on their mass : charge ratio
by the _____ 37. Sodium peroxide dissolves in
water in accordance with the
A. ion source following reaction:
B. mass analyzer
C. deflector Na2O2(s) + 2H2O(l) NaOH
D. detector (aq) + H2O2(aq)

35. Which of the following terms The pH of the solution after

accurately describes the energy reaction will be _____
associated with the process:
A. 7-8
Li (g) → Li+(g) + e- B. 6-7

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C. < 2 B. addition
D. >10 C. condensation
D. elimination.
38. Gunpowder is a mixture of
saltpetre, sulphur and wood 41. The boiling point of water is
charcoal in the ratio of 6:1:1 by higher than that of methanol
mass. The mixture burns with because _____
explosion because it produces a
large volume of gases. Saltpetre in A. water is oxide while methanol is
the mixture acts as _____ an alcohol
B. inter molecular forces in water
A. modifier are stronger than those in
B. reducing agent methanol
C. oxidising agent C. water is an inorganic compound
D. Fuel while methanol is organic
D. water is an ionic compound
39. The oxidation state of Au in while methanol is covalent
K[Au(OH)4] is _____
42. In the Rutherford scattering
A. +1 experiment, Rutherford
B. +2 bombarded a thin piece of gold foil
C. +3 with a beam of _____.
D. +4
A. electrons
40. The most common type of B. neutrons
chemical reaction which alkanes C. protons
undergo is _____ D. alpha particles

A. substitution

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43. When azimuthal quantum 46. Which of the following is a
number (l = 2), what set of orbitals state function?
is designated?
A. enthalpy
A. p B. work
B. d C. heat
C. f D. power
D. g
47. The method that cannot be
44. Sodium hydroxide is an used for removing permanent
Arrhenius base because it contains hardness of water is _______.
_____.
A. adding sodium carbonate
A. Na+ B. boiling
B. OH- C. adding caustic soda
C. NaOH D. adding slaked lime
D. Na
48. In which of the following
45. The standard state of an characteristics does hydrogen
element or compound is resemble halogens?
determined at a pressure of and a
temperature of _____. A. Hydrogen is the lightest
B. Hydrogen forms ionic hydrides
A. 760 mmHg, 0oC with alkali metals
B. 1 atm, 273oC C. Hydrogen atom contains one
C. 760 mmHg, 0K electron each
D. 1 atm, 298K D. Hydrogen has three isotopes

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49. Which alkali metal react
directly with Nitrogen to form
nitride?

A. Na
B. K
C. Rb
D. Li

50. The isomerism which exists

between CH3CHCI2 and CH2CI.
CH2CI is _____

A. chain isomerism
B. functional group isomerism
C. positional isomerism
D. metamerism

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