Class 9 Chemistry MCQs Tests

This page contains all the online tests for Class 9 Chemistry MCQs. Students should do the practice of all these tests for getting good marks in FBISE board exams.

Chapter-wise MCQs Tests

Chapter 1
Fundamentals of Chemistry

Practice MCQs Test 1

Practice MCQs Test 2

Practice MCQs Test 3

Practice MCQs Test 4

Chapter 2
Structure of Atoms

Practice MCQs Test 1

Practice MCQs Test 2

Practice MCQs Test 3

Practice MCQs Test 4

Challenge Test 2

Chapter 3
Periodic Table & Periodicity of Properties

Practice MCQs Test 1

Practice MCQs Test 2

Practice MCQs Test 3

Practice MCQs Test 4

Challenge Test 3

Chapter 4
Structure of Molecules

Practice MCQs Test 1

Practice MCQs Test 2

Practice MCQs Test 3

Practice MCQs Test 4

Challenge Test 4

Chapter 5
Physical States of Matter

Practice MCQs Test 1

Practice MCQs Test 2

Practice MCQs Test 3

Practice MCQs Test 4

Challenge Test 5

Chapter 6
Solutions

Practice MCQs Test 1

Practice MCQs Test 2

Practice MCQs Test 3

Practice MCQs Test 4

Challenge Test 6

Chapter 7
Electrochemistry

Practice MCQs Test 1

Practice MCQs Test 2

Practice MCQs Test 3

Practice MCQs Test 4

Challenge Test 7

Chapter 8
Chemical Reactivity

Practice MCQs Test 1

Practice MCQs Test 2

Practice MCQs Test 3

Practice MCQs Test 4

Challenge Test 8

Atomic Numbers and Atructure tomic Masses
Practice MCQs Test No 1

/10

Class 9 Chemistry

Chapter 1

Atomic Numbers and Atomic Masses

MCQs Test No 1

1 / 10

The atomic number of Helium (He) is:

2 / 10

Atomic number, atomic mass and Symbol of Potassium are:

19, 39 and Po

20, 40 and Po

20, 40 and P

19, 39 and K

3 / 10

The nitrogen has 7 protons in its nucleus, its atomic number is:

4 / 10

The atomic mass of Carbon is:

5 / 10

The symbol of Sodium is:

6 / 10

Atomic number of Oxygen is 8, its atomic mass is:

7 / 10

Atomic number of Aluminum is 13, its atomic mass is:

8 / 10

The symbol of Hydrogen is H, its atomic number is 1, and its atomic mass is:

9 / 10

The atomic mass of Sodium is 23, its atomic number is:

10 / 10

The atomic number and atomic mass of Magnesium are ______ and _______.

12 , 24

10 , 20

11 , 23

13 , 27

Your score is

The average score is 66%

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Practice MCQs Test No 2

/16

Class 9 Chemistry

Chapter 1

Branches of Chemistry

Practice MCQs Test 2

1 / 16

Element radium decays by emitting α-particles and is converted into another element radon.

Inorganic chemistry

Industrial Chemistry

Biochemistry

Nuclear Chemistry

2 / 16

Calorimeter is a device that measures the amount of heat, a substance absorbs on heating or emits on cooling.

Analytical Chemistry

Organic Chemistry

Inorganic chemistry

Physical Chemistry

3 / 16

Some examples of complete protein food are meat, milk, and eggs.

Biochemistry

Organic Chemistry

Inorganic chemistry

Physical Chemistry

4 / 16

Photosynthesis produces glucose and oxygen from carbon dioxide and water in presence of chlorophyll and sunlight.

Inorganic Chemistry

Organic Chemistry

Biochemistry

Environmental chemistry

5 / 16

Gases can be compressed by applying pressure.

Organic Chemistry

Inorganic chemistry

Physical Chemistry

Biochemistry

6 / 16

Sulphuric acid (H₂ SO₄) is extremely corrosive to skin.

Biochemistry

Physical Chemistry

Analytical Chemistry

Inorganic chemistry

7 / 16

Ammonia is a colourless gas with a pungent irritating odour. It is highly soluble in water.

Biochemistry

Analytical Chemistry

Physical Chemistry

Inorganic chemistry

8 / 16

Haber’s process converts large quantities of hydrogen and nitrogen into ammonia (NH₃ ).

Industrial Chemistry

Biochemistry

Inorganic Chemistry

Environmental Chemistry

9 / 16

Chlorofluorocarbon compounds are responsible for the depletion of ozone layer.

Organic Chemistry

Environmental Chemistry

Physical Chemistry

Inorganic chemistry

10 / 16

α-particles (He⁺⁺) when bombard on nitrogen atom, a proton is emitted.

Analytical Chemistry

Biochemistry

Inorganic chemistry

Nuclear Chemistry

11 / 16

Acetylene is the simplest hydrocarbon that contains a carbon-carbon triple bond. Hydrocarbons are the compounds of carbon and hydrogen.

Organic Chemistry

Biochemistry

Inorganic chemistry

Physical Chemistry

12 / 16

A chemist performed an experiment to check the percentage purity of a sample of glucose (C₆ H₁₂ O₆).

Physical Chemistry

Inorganic chemistry

Organic Chemistry

Analytical Chemistry

13 / 16

An analyst determines that NO₂ is responsible for acid rain.

Industrial Chemistry

Environmental Chemistry

Physical Chemistry

Analytical Chemistry

14 / 16

Hair contain a special class of proteins called keratins, which are present in nails and wool. Proteins contain chains of C-atoms.

Inorganic chemistry

Physical Chemistry

Biochemistry

Analytical Chemistry

15 / 16

White lead is a pigment used by artists for centuries, the metal Pb in the compound is extracted from its ore, galena (PbS).

Industrial Chemistry

Biochemistry

Inorganic chemistry

Organic Chemistry

16 / 16

Plantation helps in overcoming the greenhouse effect.

Organic Chemistry

Industrial Chemistry

Environmental chemistry

Biochemistry

Your score is

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Practice MCQs Test No 3

Class 9 Chemistry

Chapter 1

Branches of Chemistry

Practice MCQs Test 3

1 / 10

Gasoline (a mixture of hydrocarbons) fumes are ignited in an automobile engine.

Organic chemistry

Physical chemistry

Inorganic chemistry

Biochemistry

2 / 10

Purple iodine vapour appears when solid iodine is warmed.

Inorganic chemistry

Physical chemistry

Analytical chemistry

Environmental chemistry

3 / 10

A silver article tarnishes in air.

Physical chemistry

Environmental chemistry

Biochemistry

Inorganic chemistry

4 / 10

Ice floats on water.

Biochemistry

Analytical chemistry

Physical chemistry

Environmental chemistry

5 / 10

Dynamite (C₃ H₅ N₃ O₉) explodes to form a mixture of gases.

Physical chemistry

Analytical chemistry

Inorganic chemistry

Environmental chemistry

6 / 10

A cornstalk grows from a seed.

Biochemistry

Environmental chemistry

Inorganic chemistry

Organic chemistry

7 / 10

In Pakistan, most of the factories use wet process for the production of cement.

Inorganic chemistry

Industrial chemistry

Environmental chemistry

Physical chemistry

8 / 10

Many other light chlorinated hydrocarbons in drinking water are carcinogens.

Organic chemistry

Inorganic chemistry

Environmental chemistry

Physical Chemistry

9 / 10

Carbon-14 is continuously produced in the atmosphere when high energy neutrons from space collide with nitrogen-14.

Physical chemistry

Industrial Chemistry

Nuclear chemistry

Inorganic chemistry

10 / 10

Sulphur dioxide is the major source of acid rain.

Environmental chemistry

Inorganic chemistry

Analytical chemistry

Physical chemistry

Your score is

The average score is 36%

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Practice MCQs Test No 4

/10

Class 9 Chemistry

Chapter 1

Practice MCQs Test No 4

1 / 10

How many moles of Na atoms are present in 2.3 g of Na?

1 mole

0.1 moles

1.5 moles

0.15 moles

2 / 10

How many atoms are there in 0.1 moles of Carbon?

6.022 × 10^22>/sup>

6.022 × 10^23>/sup>

6.022 × 10^21>/sup>

6.022 × 10^24>/sup>

3 / 10

The empirical formula for caffeine (C₈H₁₀N₄O₂) is:

C₅H₅N₂O

C₄H₅NO₂

C₄H₅N₂O

C₄H₅NO

4 / 10

A compound with chemical formula BaSX₄ has a formula mass 233 amu. Atomic mass of the element X is:

106

5 / 10

0.25 moles of SO₂ will contain:

3.5055 x 10²³ molecules

4.5055 x 10²³ molecules

2.5055 x 10²³ molecules

1.5055 x 10²³ molecules

6 / 10

A compound with chemical formula Na₂CX₃ has formula mass 106 amu. What is the atomic mass of the element X? [Atomic Masses: C=12, Na=23]

106

7 / 10

If molar mass of a compound is 90 g/mole, the number of its moles containing 3.011×10²³ molecules will be:

0.5

3.0

4.5

1.5

8 / 10

How many atoms are there in 1.25 moles of Zinc?

7.53 × 10²³ Zn atoms

8.53 × 10²³ Zn atoms

6.63 × 10²³ Zn atoms

9.53 × 10²³ Zn atoms

9 / 10

Atomic masses of H and O are 1 amu and 16 amu respectively. The molecular mass of hydrogen peroxide (H₂O₂) is:

32 amu

18 amu

34 amu

17 amu

10 / 10

Which of the following is the correct empirical formula of C₆H₄O(NO₂)₃?

C₃H₄O₃N

C₆H₄O₇N₃

C₃H₂O₃N₂

C₃H₂O₇N₃

Your score is

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Chapter 2

Practice MCQs Test No 1

/13

Class 9 Chemistry

Chapter 2

Practice MCQs Test No 1

1 / 13

Chlorine has two isotopes, both of which have:

same number of electrons

same number of neutrons

different number of protons

same mass number

2 / 13

Carbon has __________ isotopes.

3 / 13

₁₁Na has electronic configuration:

1s² 2s² 2p⁵ 3s²

1s² 2s² 2p⁷

1s² 2s² 2p⁶ 3s¹

1s² 2s² 3s¹

4 / 13

Value of Plank’s constant is:

6.626 x 10^-30 J.s

6.626 x 10^-36 J.s

6.626 x 10^-32 J.s

6.626 x 10^-34 J.s

5 / 13

According to Bohr atomic model:

The farther the electron is from the nucleus, the more energy it has.

Light is absorbed when an electron jumps a lower energy orbit.

The energy of the electron is inversely proportional to its distance from the nucleus.

Each orbit has fixed energy, so each orbit is called sub-energy level.

6 / 13

Number of neutrons in ²⁷M₁₃ are:

7 / 13

M shell has sub-shells:

3s, 3p, 3d

1s, 2s

1s, 2s, 3s

2s, 2p

8 / 13

A sub-shell that can accommodate 6 electrons is:

9 / 13

Rutherford used _____ particles in his experiments.

He^-2

He atoms

He⁺

He⁺²

10 / 13

Identify the number of electrons that f-sub shell can accommodate.

11 / 13

Which of the following is a defect of Rutherford atomic model?

Electrons do not fall into the nucleus

Most of the mass is present in nucleus

Most of the space in atom is empty

Electrons are negatively charged

12 / 13

Which one of the following sub shell is filled after filling of 3p sub shell?

13 / 13

Keeping in view Auf Bau Principle, identify the energy level which the elements fill first.

Your score is

The average score is 71%

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Practice MCQs Test No 2

/14

Class 9 Chemistry

Chapter 2

Practice MCQs Test No 2

1 / 14

Which of the following statement is not correct about isotopes?

they have same physical properties

they have same chemical properties

they have same atomic number

they have same number of protons

2 / 14

As the value of n increases:

energy of the shell decreases

the distance of electron from the nucleus increases

distance of electron from nucleus and energy of shell increases

energy of the shell increases

3 / 14

Which isotope of Uranium is rare?

U-234

U-238

U-239

U-235

4 / 14

The fission of uranium–235 yields:

smaller nuclei

All are correct

neutron

energy

5 / 14

Which isotope is commonly used to irradiate cancer cells?

Carbon-14

Iodine-131

Cobalt-60

Iodine-123

6 / 14

Chemical properties of an element depend upon the number of:

Protons and electrons

Neutrons

Electrons

Protons

7 / 14

Which isotope is used in nuclear reactors?

U-234

U-238

All of these

U-235

8 / 14

The nuclear energy released by the fission of one kilogram of uranium–235 is equivalent to chemical energy produced by burning more than:

1700 kg of coal

17000 kg of coal

17000 g of coal

1700 g of coal

9 / 14

Identify the isotope used as a Tracer in diagnosing Thyroid problem:

Iodine-123

Cobalt-60

Carbon-14

Iodine-131

10 / 14

Which isotope is used to trace the path of carbon in photosynthesis?

Iodine-131

Iodine-123

Carbon-14

Cobalt-60

11 / 14

_______ do not take part in ordinary chemical reactions.

Molecules

Atoms

Neutrons

Electrons

12 / 14

Which of the following isotopes is used to trace the flow of blood and detect possible constrictions or obstructions in the circulatory system?

C0-60

C-14

I-131

Na-24

13 / 14

When Uranium-238 decays into Thorium-234, it emits:

Electron

Alpha particle

Proton

Neutron

14 / 14

Isotopes of an element have similar:

Atomic masses

Physical properties

Chemical properties

All of these

Your score is

The average score is 37%

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Practice MCQs Test No 3

/15

Class 9 Chemistry

Chapter 2

Practice MCQs Test No 3

1 / 15

Which carbon is not black in colour?

Graphite

Coal

Buckey ball

Diamond

2 / 15

TRITIUM has number of neutrons

Zero

3 / 15

Formula for heavy water is:

H₃O

D₃O

H₂O

D₂O

4 / 15

Almost entire mass of an atom is concentrated in the

Neutrons

Protons

Nucleus

Electrons

5 / 15

Electrons revolve only in those orbits with angular momentum as an

Half integral multiple of

2\pi

Integral multiple of h

Half integral multiple of h

Integral multiple of

\frac { h }{ 2\pi }

6 / 15

Maximum number of electrons in a shell can be calculated by

2n²

2n+2

2l+1

7 / 15

Rutherford use ________ as a source of alpha particles.

Carbon

Polonium

Silver

Gold

8 / 15

The word isotopes was first used by scientist

Rutherford

Bohr

Moseley

Soddy

9 / 15

When an electron changes its orbit from higher to lower, energy is

No change

Remains constant

Absorbed

Released

10 / 15

All the isotopes of carbon are _______ in water.

Miscible

Insoluble

Soluble

Dissolve

11 / 15

The energy of an electron in an orbit is proportional to

Distance between two nuclei

Distance from nucleus

Distance between shells

Positive charge inside nucleus

12 / 15

_________ is highly inflammable gas.

Carbon dioxide

Chlorine

Hydrogen

Carbon gas

13 / 15

Alpha particles which were deflected backward in Rutherford's experiment were hit upon by

Electrons

Protons

Nucleus

Empty space

14 / 15

The value of Planks constant is

6.626×10⁻³⁴ J/s

6.626×10⁻³⁴ J.s

6.626×10³⁴ J.s

6.22×10²³ J.s

15 / 15

Which of the following is a defect of Rutherford atomic model?

Most of the mass is present in nucleus

Electrons are negatively charged

Electrons do not fall into the nucleus

Most of the space in an atom is empty

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Practice MCQs Test No 4

/15

Class 9 Chemistry

Chapter 2

Practice MCQs Test No 4

1 / 15

Which isotope can be used for radiotherapy for cancer patients?

P-32

Co-60

C-14

I-131

2 / 15

We can compare the activity of isotopes of carbon from skull and jaw bones of dead organism.

C-14

C-12

C-16

C-13

3 / 15

Correct increasing order of energy of sub shell is:

1s>2s>2p>3s>3p>4s>3d

1s<2s<3s<2p<3p<4s<3d

1s<2s<2p<3s<3p<3d<4s

1s<2s<2p<3s<3p<4s<3d

4 / 15

An element has two protons in its nucleus. The symbol of the element is _____.

5 / 15

Which of the following isotopes of uranium is most abundant?

U-235

U-238

U-236

U-237

6 / 15

An element is placed in second period of periodic table and have six protons and six neutrons in its nucleus. The element is _____.

7 / 15

Electronic configuration of an element is as shown: 1s², 2s², 2p⁶, 3s², 3p⁵ Identify the element which contains this electronic configuration.

8 / 15

Maximum number of electrons in d sub shell are:

9 / 15

Sub shells are also called as:

Orbitals

Orbits

None of the above.

Energy levels

10 / 15

Electronic configuration for an element is as shown. 1s², 2s², 2p⁶, 3s², 3p⁵ . Which of the following is correct regarding this electronic arrangement?

1s has high energy than 2s

1s has high energy than 3p

3p has higher energy than 2s

2s has high energy than 2p

11 / 15

Atomic number of Na is 11. electronic configuration of the Na is _____.

1s²,2s³,2p⁵,3s¹

1s²,2s²,2p⁶,3s¹

1s²,2s²,2p⁵,3s²

1s²,2s¹,2p⁵,3s²

12 / 15

Which of the following is true about the isotopes?

Isotopes have greater numbers of neutrons than protons

Isotopes have same numbers of protons but different numbers of neutrons.

Isotopes have same numbers of protons and neutrons.

Isotopes have greater numbers of protons than neutrons.

13 / 15

According to 2n² rule, L-Shell contains maximum___ electrons.

14 / 15

Energy released by the isotopes uranium - 235 is due to the process:

Demolution

Fission

Fusion

Sublimation

15 / 15

$_{ 17 }^{ 37 }{ Cl }$ has how many protons?

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Chapter 3

Practice MCQs Test No 1

Class 9 Chemistry

Chapter 3

Practice MCQs Test No 1

1 / 20

By 1925, ____ elements were known.

109

2 / 20

Last _____ periods are long periods.

3 / 20

A table showing systematic arrangement of elements is called:

Elements table

Periodic table

Periods

Groups

4 / 20

Atomic number was discovered by:

Neil Bohr

John Newland

Moseley

Mendeleev

5 / 20

Elements are arranged in the order of increasing:

Neutron number

Atomic mass

Atomic number

Nucleon number

6 / 20

Group IIA elements are called:

Alkali metals

Alkaline earth metals

Halogens

Noble gases

7 / 20

Metallic elements in Group 1A are called:

Alkali metals

Halogens

Noble gases

Alkaline earth metals

8 / 20

Elements of Group IA and Group IIA contain their valence electrons in:

f sub-shell

d sub-shell

p sub-shell

s sub-shell

9 / 20

Group B elements are called:

Transition elements

Main Group elements

Representative elements

Normal elements

10 / 20

The Group VIIIA elements are called:

Alkaline earth metals

Halogens

Noble gases

Alkali metals

11 / 20

By the end of 18th century, _______ elements were known.

109

12 / 20

Number of periods in the Periodic table are:

13 / 20

Group A elements are called:

All of these

Main group elements

Normal elements

Representative elements

14 / 20

The horizontal rows of the periodic table are called:

Groups

Actinides

Lenthanides

Periods

15 / 20

Each vertical column of elements in the periodic table is called a:

group

family

period

group or family

16 / 20

Elements with similar valance shell electronic configuration are placed in the same:

Block

Group

List

Period

17 / 20

On the basis of outermost valence sub-shell, elements in the periodic table can also be classified into:

6 blocks

4 blocks

8 groups

7 blocks

18 / 20

The atomic number was discovered in:

1918

1913

1900

1906

19 / 20

First _____ periods are called short periods.

20 / 20

The elements of Group VIIA are called:

Alkali metals

Noble gases

Halogens

Alkaline earth metals

Your score is

The average score is 66%

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Practice MCQs Test No 2

Class 9 Chemistry

Chapter 3

Practice MCQs Test 2

1 / 20

Because all the elements of a particular group have similar valence shell electronic configuration, they possess similar:

Chemical properties

Number of shells

Number of neutrons

Physical properties

2 / 20

Physical properties depend on the:

Sizes of atoms

Electronic configuration

Valence shell electronic configuration

Number of neutrons

3 / 20

The number of electrons in the valence shell of halogens are _____.

4 / 20

Chemical properties depend on the:

valence shell electronic configuration

first shell electronic configuration

Number of neutrons

Atomic mass

5 / 20

Across a period (left to right), shielding effect _____.

becomes zero

increases

decreases

remains constant

6 / 20

What is the period number of Nitrogen -7 ?

7 / 20

__________ of element indicates the number of electrons in the valence shell.

Block number

Atomic mass

Group number

Period number

8 / 20

Which of the following has the lowest shielding effect?

9 / 20

____________ of element indicates n value of the valence shell.

Period number

Atomic number

Block number

Group number

10 / 20

The number of electrons in the valence shell of alkali metals is _____

11 / 20

The number of elements in the first period is _____.

12 / 20

The elements of Group IIIA to VIIIA (except He) are known as:

f – block elements

p – block elements

s – block elements

d – block elements

13 / 20

Element having configuration 1s² belongs to group:

14 / 20

Elements in the same vertical group of the periodic table have same _____.

Atomic Number (Z)

Atomic Mass (A)

Number of valence electrons

Avogadro's number

15 / 20

Valence shell configuration of Na is:

3s¹

2p⁶ , 3s¹

2s² , 2p⁶

1s² , 2s², 2p⁶, 3s¹

16 / 20

The elements of B-group are called _____.

Transition elements

Alkali metals and alkaline earth metals

Alkaline Earth metals

Halogens

17 / 20

The horizontal rows in a periodic table are known as _____.

Periods

Rows

Groups

Columns

18 / 20

John Newland found the similarity in properties of every ________ element.

19 / 20

Which of the elements are not p-block representative elements?

Noble gases

Group V-A

Halogens

Alkali metals

20 / 20

Which of the following has the highest shielding effect?

Your score is

The average score is 64%

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Practice MCQs Test No 3

/15

Class 9 Chemistry

Chapter 3

Practice MCQs Test No 3

1 / 15

Which of the elements are not p-block representative elements?

Noblegases

Halogens

Alkalimetals

GroupV-A

2 / 15

Which of the following has the lowest shielding effect?

3 / 15

Across a period (left to right), shielding effect _____.

Becomeszero

Increases

Decreases

Remainsconstant

4 / 15

What is the period number of Nitrogen -7 ?

5 / 15

The horizontal rows in a periodic table are known as _____.

Groups

Columns

Periods

Rows

6 / 15

The number of elements in the first period is _____.

7 / 15

John Newland found the similarity in properties of every ------ element.

8 / 15

Element having configuration 1s² belongs to group

9 / 15

The number of electrons in the valence shell of alkali metals is _____.

10 / 15

Which of the following has the highest shielding effect?

11 / 15

Valence shell configuration of Na is

2p6,3s1

3s1

2s2,2p6

1s2,2s2,2p6,3s1

12 / 15

Atomic number is discovered by

Rutherford

Bohr

Moseley

Dalton

13 / 15

Elements in the same vertical group of the periodic table have same _____.

Avogadro'snumber

AtomicMass(A)

Numberofvalenceelectrons

AtomicNumber(Z)

14 / 15

The number of electrons in the valence shell of halogens are _____.

15 / 15

The elements of B-group are called _____.

Alkalineearthmetals

Alkalimetalsandalkalineearthmetals

Transitionelements

Halogens

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Practice MCQs Test No 4

/15

Class 9 Chemistry

Chapter 3

Practice MCQs Test No 4

1 / 15

Atomic radii decreases because of

Increas in number of valence electrons

Increase in attractive forces of the nucleus and valence electrons

Increase in number of protons

All of these

2 / 15

In general, ionization energy _____ going bottom to top within a group in the periodic table.

Becomes zero

Remains unchanged

Decreases

Increases

3 / 15

Ionization energy is measured in _____.

J/sec

kJ/h

kW/mol

kJ/mol

4 / 15

Which of the following has the highest electron affinity?

5 / 15

Electronegativity refers to _____.

the ability of an atom to attract the electrons in a chemical bond toward itself

the energy required to remove an electron from a gaseous atom in the ground state.

tendency of an atom to attract a shared electron pair towards itself

the ability of an atom to attract the electrons toward nucleus

6 / 15

Arrange the elements in decreasing ionization energy.

Li,Na,K

Li>Na>K

Li<Na<K

K>Na>Li

7 / 15

Element in group II A with smallest atomic radius is _____.

8 / 15

The state required for Chlorine to release energy and form a uninegative ion is _____.

Gaseous molecules

Gaseous atoms

Liquid atoms

Solid molecules

9 / 15

Electron affinity involves _____.

Addition of an electron to the outermost shell of an atom

Addition of an electron to the nucleus of an atom

Removal of an electron from the outermost shell an atom

Addition of a proton to the nucleus

10 / 15

Which element has the highest electronegativity?

11 / 15

Ionization energy is a/an _____.

Cation formation

Anion formation

Bond breaking process

Bond making process

12 / 15

When atomic radius increases, electron affinity _____.

Becomes zero

Increases

Decreases

Remains constant

13 / 15

Which of these represents an element with a large electron affinity?

Ability to gain an electron easily to form a positive ion

Ability to lose an electron easily to form a negative ion

Ability to lose an electron easily to form a positive ion

Ability to gain an electron easily to form a negative ion

14 / 15

Ionization results in the ejection of _____.

Protons

Electrons

Neutrons

Nucleus

15 / 15

Negative sign is given to electron affinity because energy is _____.

Released

Remain same

No effect

Gained

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Chapter 4

Practice MCQs Test No 1

/16

Class 9 Chemistry

Chapter 4

Practice MCQs Test No 1

1 / 16

Which of the following atoms obey duplet rule?

F₂

H₂

N₂

O₂

2 / 16

In Hydrogen Iodide (HI), the bond is:

Polar covalent bond

Co-ordinate covalent bond

Ionic bond

Non polar covalent bond

3 / 16

Which of the following is not true about the formation of Na₂S?

Sodium forms cation

Each sodium atom loses one electron

Each sulphur atom gains one electron

Sulphur forms anion

4 / 16

The covalent bond is formed by:

Donating an electron pair by one atom

Complete transfer of electrons

Mutual sharing of an electron pair by two atoms

Accepting electron pair by one atom

5 / 16

In the formation of AlF₃, aluminum atom loses _____________ electrons.

6 / 16

Which of the following atoms will form an ion of charge -2?

Atomic Number : 8 Mass Number : 16

Atomic Number : 14 Mass Number : 28

Atomic Number : 12 Mass Number : 24

Atomic Number : 10 Mass Number : 20

7 / 16

Which of the following substance has ionic bond?

CO₂

SO₂

MgO

H₂O

8 / 16

Identify the covalent compound:

MgO

H<sub>2</sub>O

NaCl

9 / 16

Phosphorus belongs to third period of Group VA. How many electrons it needs to complete its valence shell?

10 / 16

Hydrogen bonding is involved in:

Formation of crystals in NaCl

Conductance of electricity

Adhesive action of paints

Van der Waal's force

11 / 16

The bond which is formed by complete transfer of electrons from one atom to another is called:

Hydrogen bond

Covalent bond

Ionic bond

Co-ordinate bond

12 / 16

The melting point and boiling pint of water are higher due to:

Its covalent nature

Hydrogen bonding

Its higher density

Its higher molecular mass

13 / 16

Which of the following atoms will not form cation or anion?

D (Atomic No. 19)

B (Atomic No. 17)

A (Atomic No. 16)

C (Atomic No. 18)

14 / 16

Which of the following atoms will form cation?

Atomic number 15

Atomic number 17

Atomic number 20

Atomic number 18

15 / 16

Which of the following molecules has triple covalent bond between its atoms?

N₂

Class 9 Chemistry MCQs Tests