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 1

Atomic Numbers and Atomic Masses
Practice MCQs Test No 1

/10

Class 9 Chemistry

Chapter 1

Atomic Numbers and Atomic Masses

MCQs Test No 1

1 / 10

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

2 / 10

The symbol of Sodium is:

3 / 10

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

4 / 10

The atomic number of Helium (He) is:

5 / 10

The atomic mass of Carbon is:

6 / 10

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

10 , 20

12 , 24

11 , 23

13 , 27

7 / 10

Atomic number, atomic mass and Symbol of Potassium are:

19, 39 and K

20, 40 and Po

19, 39 and Po

20, 40 and P

8 / 10

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

9 / 10

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

10 / 10

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

Your score is

The average score is 71%

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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.

Nuclear Chemistry

Biochemistry

Inorganic chemistry

Industrial Chemistry

2 / 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

Organic Chemistry

Biochemistry

Inorganic chemistry

3 / 16

Gases can be compressed by applying pressure.

Biochemistry

Organic Chemistry

Inorganic chemistry

Physical Chemistry

4 / 16

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

Industrial Chemistry

Biochemistry

Inorganic Chemistry

Environmental Chemistry

5 / 16

An analyst determines that NO₂ is responsible for acid rain.

Environmental Chemistry

Analytical Chemistry

Industrial Chemistry

Physical Chemistry

6 / 16

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

Analytical Chemistry

Physical Chemistry

Inorganic chemistry

Biochemistry

7 / 16

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

Organic Chemistry

Inorganic chemistry

Physical Chemistry

Biochemistry

8 / 16

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

Inorganic chemistry

Physical Chemistry

Biochemistry

Analytical Chemistry

9 / 16

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

Biochemistry

Organic Chemistry

Environmental chemistry

Inorganic Chemistry

10 / 16

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

Inorganic chemistry

Analytical Chemistry

Physical Chemistry

Organic Chemistry

11 / 16

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

Analytical Chemistry

Organic Chemistry

Inorganic chemistry

Physical Chemistry

12 / 16

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

Inorganic chemistry

Nuclear Chemistry

Analytical Chemistry

Biochemistry

13 / 16

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

Physical Chemistry

Organic Chemistry

Biochemistry

Inorganic chemistry

14 / 16

Plantation helps in overcoming the greenhouse effect.

Biochemistry

Industrial Chemistry

Environmental chemistry

Organic Chemistry

15 / 16

Chlorofluorocarbon compounds are responsible for the depletion of ozone layer.

Organic Chemistry

Inorganic chemistry

Physical Chemistry

Environmental Chemistry

16 / 16

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

Inorganic chemistry

Biochemistry

Analytical Chemistry

Physical Chemistry

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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

Biochemistry

Inorganic chemistry

Physical chemistry

2 / 10

Many other light chlorinated hydrocarbons in drinking water are carcinogens.

Inorganic chemistry

Physical Chemistry

Environmental chemistry

Organic chemistry

3 / 10

A cornstalk grows from a seed.

Inorganic chemistry

Environmental chemistry

Biochemistry

Organic chemistry

4 / 10

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

Analytical chemistry

Inorganic chemistry

Physical chemistry

Environmental chemistry

5 / 10

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

Industrial chemistry

Environmental chemistry

Physical chemistry

Inorganic chemistry

6 / 10

Sulphur dioxide is the major source of acid rain.

Physical chemistry

Analytical chemistry

Inorganic chemistry

Environmental chemistry

7 / 10

Ice floats on water.

Analytical chemistry

Biochemistry

Physical chemistry

Environmental chemistry

8 / 10

Purple iodine vapour appears when solid iodine is warmed.

Environmental chemistry

Analytical chemistry

Inorganic chemistry

Physical chemistry

9 / 10

A silver article tarnishes in air.

Physical chemistry

Biochemistry

Environmental chemistry

Inorganic chemistry

10 / 10

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

Physical chemistry

Inorganic chemistry

Nuclear chemistry

Industrial Chemistry

Your score is

The average score is 0%

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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?

1.5 moles

0.15 moles

1 mole

0.1 moles

2 / 10

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

C₃H₄O₃N

C₃H₂O₇N₃

C₃H₂O₃N₂

C₆H₄O₇N₃

3 / 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

4 / 10

0.25 moles of SO₂ will contain:

1.5055 x 10²³ molecules

4.5055 x 10²³ molecules

3.5055 x 10²³ molecules

2.5055 x 10²³ molecules

5 / 10

How many atoms are there in 1.25 moles of Zinc?

7.53 × 10²³ Zn atoms

6.63 × 10²³ Zn atoms

8.53 × 10²³ Zn atoms

9.53 × 10²³ Zn atoms

6 / 10

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

4.5

1.5

3.0

0.5

7 / 10

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

106

8 / 10

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

17 amu

34 amu

18 amu

32 amu

9 / 10

The empirical formula for caffeine (C₈H₁₀N₄O₂) is:

C₄H₅NO₂

C₄H₅NO

C₄H₅N₂O

C₅H₅N₂O

10 / 10

How many atoms are there in 0.1 moles of Carbon?

6.022 × 10^24>/sup>

6.022 × 10^23>/sup>

6.022 × 10^22>/sup>

6.022 × 10^21>/sup>

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

Carbon has __________ isotopes.

2 / 13

According to Bohr atomic model:

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

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

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

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

3 / 13

Chlorine has two isotopes, both of which have:

same number of electrons

same number of neutrons

different number of protons

same mass number

4 / 13

Number of neutrons in ²⁷M₁₃ are:

5 / 13

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

6 / 13

₁₁Na has electronic configuration:

1s² 2s² 2p⁷

1s² 2s² 3s¹

1s² 2s² 2p⁵ 3s²

1s² 2s² 2p⁶ 3s¹

7 / 13

A sub-shell that can accommodate 6 electrons is:

8 / 13

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

9 / 13

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

10 / 13

M shell has sub-shells:

3s, 3p, 3d

2s, 2p

1s, 2s, 3s

1s, 2s

11 / 13

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

Most of the mass is present in nucleus

Most of the space in atom is empty

Electrons are negatively charged

Electrons do not fall into the nucleus

12 / 13

Rutherford used _____ particles in his experiments.

He^-2

He⁺

He atoms

He⁺²

13 / 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^-34 J.s

6.626 x 10^-32 J.s

Your score is

The average score is 65%

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Practice MCQs Test No 2

/14

Class 9 Chemistry

Chapter 2

Practice MCQs Test No 2

1 / 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 g of coal

1700 g of coal

17000 kg of coal

2 / 14

Which isotope of Uranium is rare?

U-234

U-238

U-239

U-235

3 / 14

The fission of uranium–235 yields:

All are correct

neutron

smaller nuclei

energy

4 / 14

Chemical properties of an element depend upon the number of:

Electrons

Protons

Protons and electrons

Neutrons

5 / 14

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

Neutron

Electron

Proton

Alpha particle

6 / 14

As the value of n increases:

energy of the shell decreases

the distance of electron from the nucleus increases

energy of the shell increases

distance of electron from nucleus and energy of shell increases

7 / 14

Which isotope is commonly used to irradiate cancer cells?

Iodine-131

Cobalt-60

Carbon-14

Iodine-123

8 / 14

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

Cobalt-60

Iodine-131

Iodine-123

Carbon-14

9 / 14

Which of the following statement is not correct about isotopes?

they have same chemical properties

they have same atomic number

they have same number of protons

they have same physical properties

10 / 14

Which isotope is used in nuclear reactors?

U-235

U-238

U-234

All of these

11 / 14

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

Iodine-123

Iodine-131

Cobalt-60

Carbon-14

12 / 14

_______ do not take part in ordinary chemical reactions.

Neutrons

Electrons

Molecules

Atoms

13 / 14

Isotopes of an element have similar:

Atomic masses

Chemical properties

All of these

Physical properties

14 / 14

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

I-131

C-14

C0-60

Na-24

Your score is

The average score is 35%

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Practice MCQs Test No 3

/15

Class 9 Chemistry

Chapter 2

Practice MCQs Test No 3

1 / 15

The word isotopes was first used by scientist

Moseley

Rutherford

Bohr

Soddy

2 / 15

Electrons revolve only in those orbits with angular momentum as an

Integral multiple of h

Half integral multiple of h

Half integral multiple of

2\pi

Integral multiple of

\frac { h }{ 2\pi }

3 / 15

The value of Planks constant is

6.626×10⁻³⁴ J.s

6.22×10²³ J.s

6.626×10⁻³⁴ J/s

6.626×10³⁴ J.s

4 / 15

Which carbon is not black in colour?

Diamond

Coal

Buckey ball

Graphite

5 / 15

TRITIUM has number of neutrons

Zero

6 / 15

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

Released

Absorbed

No change

Remains constant

7 / 15

_________ is highly inflammable gas.

Carbon dioxide

Hydrogen

Chlorine

Carbon gas

8 / 15

The energy of an electron in an orbit is proportional to

Distance between shells

Distance between two nuclei

Positive charge inside nucleus

Distance from nucleus

9 / 15

Almost entire mass of an atom is concentrated in the

Electrons

Protons

Neutrons

Nucleus

10 / 15

Rutherford use ________ as a source of alpha particles.

Silver

Gold

Polonium

Carbon

11 / 15

Maximum number of electrons in a shell can be calculated by

2n²

2l+1

2n+2

12 / 15

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

Most of the space in an atom is empty

Electrons are negatively charged

Most of the mass is present in nucleus

Electrons do not fall into the nucleus

13 / 15

Formula for heavy water is:

D₃O

D₂O

H₂O

H₃O

14 / 15

All the isotopes of carbon are _______ in water.

Soluble

Insoluble

Miscible

Dissolve

15 / 15

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

Nucleus

Electrons

Empty space

Protons

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Practice MCQs Test No 4

/15

Class 9 Chemistry

Chapter 2

Practice MCQs Test No 4

1 / 15

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

2 / 15

Which of the following is true about the isotopes?

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

Isotopes have greater numbers of neutrons than protons

Isotopes have same numbers of protons and neutrons.

Isotopes have greater numbers of protons than neutrons.

3 / 15

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

4 / 15

Maximum number of electrons in d sub shell are:

5 / 15

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

6 / 15

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

1s²,2s²,2p⁵,3s²

1s²,2s¹,2p⁵,3s²

1s²,2s²,2p⁶,3s¹

1s²,2s³,2p⁵,3s¹

7 / 15

Sub shells are also called as:

Orbits

Orbitals

None of the above.

Energy levels

8 / 15

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

9 / 15

Which isotope can be used for radiotherapy for cancer patients?

I-131

P-32

C-14

Co-60

10 / 15

Correct increasing order of energy of sub shell is:

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

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

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

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

11 / 15

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

2s has high energy than 2p

3p has higher energy than 2s

1s has high energy than 2s

1s has high energy than 3p

12 / 15

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

Fission

Fusion

Demolution

Sublimation

13 / 15

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

14 / 15

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

C-14

C-12

C-13

C-16

15 / 15

Which of the following isotopes of uranium is most abundant?

U-236

U-237

U-235

U-238

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Chapter 3

Practice MCQs Test No 1

Class 9 Chemistry

Chapter 3

Practice MCQs Test No 1

1 / 20

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

7 blocks

4 blocks

6 blocks

8 groups

2 / 20

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

s sub-shell

d sub-shell

f sub-shell

p sub-shell

3 / 20

Atomic number was discovered by:

Mendeleev

Moseley

John Newland

Neil Bohr

4 / 20

Number of periods in the Periodic table are:

5 / 20

Metallic elements in Group 1A are called:

Alkali metals

Alkaline earth metals

Noble gases

Halogens

6 / 20

The horizontal rows of the periodic table are called:

Groups

Actinides

Lenthanides

Periods

7 / 20

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

109

8 / 20

Group IIA elements are called:

Alkaline earth metals

Halogens

Alkali metals

Noble gases

9 / 20

Group B elements are called:

Representative elements

Transition elements

Main Group elements

Normal elements

10 / 20

First _____ periods are called short periods.

11 / 20

The Group VIIIA elements are called:

Alkaline earth metals

Halogens

Alkali metals

Noble gases

12 / 20

A table showing systematic arrangement of elements is called:

Groups

Periodic table

Periods

Elements table

13 / 20

The atomic number was discovered in:

1918

1906

1900

1913

14 / 20

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

group or family

period

family

group

15 / 20

By 1925, ____ elements were known.

109

16 / 20

Elements are arranged in the order of increasing:

Atomic number

Neutron number

Nucleon number

Atomic mass

17 / 20

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

Group

List

Block

Period

18 / 20

Group A elements are called:

Representative elements

Main group elements

Normal elements

All of these

19 / 20

The elements of Group VIIA are called:

Alkaline earth metals

Noble gases

Halogens

Alkali metals

20 / 20

Last _____ periods are long periods.

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The average score is 73%

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Practice MCQs Test No 2

Class 9 Chemistry

Chapter 3

Practice MCQs Test 2

1 / 20

Physical properties depend on the:

Electronic configuration

Number of neutrons

Sizes of atoms

Valence shell electronic configuration

2 / 20

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

remains constant

increases

becomes zero

decreases

3 / 20

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

4 / 20

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

Halogens

Alkali metals

Group V-A

Noble gases

5 / 20

The number of elements in the first period is _____.

6 / 20

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

Number of valence electrons

Avogadro's number

Atomic Number (Z)

Atomic Mass (A)

7 / 20

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

8 / 20

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

9 / 20

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

Block number

Group number

Period number

Atomic mass

10 / 20

Which of the following has the highest shielding effect?

11 / 20

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

Columns

Rows

Periods

Groups

12 / 20

____________ of element indicates n value of the valence shell.

Group number

Block number

Period number

Atomic number

13 / 20

Element having configuration 1s² belongs to group:

14 / 20

Which of the following has the lowest shielding effect?

15 / 20

What is the period number of Nitrogen -7 ?

16 / 20

Valence shell configuration of Na is:

2s² , 2p⁶

3s¹

1s² , 2s², 2p⁶, 3s¹

2p⁶ , 3s¹

17 / 20

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

Number of shells

Number of neutrons

Chemical properties

Physical properties

18 / 20

The elements of B-group are called _____.

Transition elements

Halogens

Alkaline Earth metals

Alkali metals and alkaline earth metals

19 / 20

Chemical properties depend on the:

valence shell electronic configuration

first shell electronic configuration

Number of neutrons

Atomic mass

20 / 20

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

s – block elements

d – block elements

f – block elements

p – block elements

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The average score is 95%

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Practice MCQs Test No 3

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Class 9 Chemistry

Chapter 3

Practice MCQs Test No 3

1 / 15

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

GroupV-A

Noblegases

Halogens

Alkalimetals

2 / 15

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

Rows

Periods

Columns

Groups

3 / 15

Atomic number is discovered by

Bohr

Dalton

Rutherford

Moseley

4 / 15

Valence shell configuration of Na is

1s2,2s2,2p6,3s1

2p6,3s1

3s1

2s2,2p6

5 / 15

Element having configuration 1s² belongs to group

6 / 15

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

7 / 15

The number of elements in the first period is _____.

8 / 15

Which of the following has the lowest shielding effect?

9 / 15

What is the period number of Nitrogen -7 ?

10 / 15

Which of the following has the highest shielding effect?

11 / 15

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

12 / 15

The elements of B-group are called _____.

Transitionelements

Alkalimetalsandalkalineearthmetals

Halogens

Alkalineearthmetals

13 / 15

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

Becomeszero

Remainsconstant

Increases

Decreases

14 / 15

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

15 / 15

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

AtomicMass(A)

Numberofvalenceelectrons

AtomicNumber(Z)

Avogadro'snumber

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Practice MCQs Test No 4

/15

Class 9 Chemistry

Chapter 3

Practice MCQs Test No 4

1 / 15

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

Liquid atoms

Gaseous atoms

Gaseous molecules

Solid molecules

2 / 15

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

3 / 15

Arrange the elements in decreasing ionization energy.

Li<Na<K

Li,Na,K

K>Na>Li

Li>Na>K

4 / 15

Which element has the highest electronegativity?

5 / 15

Electronegativity refers to _____.

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

the ability of an atom to attract the electrons toward nucleus

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

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

6 / 15

Electron affinity involves _____.

Removal of an electron from the outermost shell an atom

Addition of an electron to the nucleus of an atom

Addition of a proton to the nucleus

Addition of an electron to the outermost shell of an atom

7 / 15

Atomic radii decreases because of

Increase in number of protons

Increas in number of valence electrons

All of these

Increase in attractive forces of the nucleus and valence electrons

8 / 15

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

Increases

Decreases

Remains unchanged

Becomes zero

9 / 15

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

Released

Remain same

Gained

No effect

10 / 15

Ionization energy is measured in _____.

J/sec

kW/mol

kJ/mol

kJ/h

11 / 15

When atomic radius increases, electron affinity _____.

Increases

Decreases

Remains constant

Becomes zero

12 / 15

Which of the following has the highest electron affinity?

13 / 15

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

Ability to lose an electron easily to form a positive ion

Ability to gain an electron easily to form a negative ion

Ability to lose an electron easily to form a negative ion

Ability to gain an electron easily to form a positive ion

14 / 15

Ionization results in the ejection of _____.

Electrons

Protons

Neutrons

Nucleus

15 / 15

Ionization energy is a/an _____.

Anion formation

Bond making process

Cation formation

Bond breaking process

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Chapter 4

Practice MCQs Test No 1

/16

Class 9 Chemistry

Chapter 4

Practice MCQs Test No 1

1 / 16

The covalent bond is formed by:

Donating an electron pair by one atom

Complete transfer of electrons

Accepting electron pair by one atom

Mutual sharing of an electron pair by two atoms

2 / 16

Hydrogen bonding is involved in:

Formation of crystals in NaCl

Adhesive action of paints

Conductance of electricity

Van der Waal's force

3 / 16

Silicon belongs to Group IVA. It has ______ electrons in the valence shell.

4 / 16

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

5 / 16

Which of the following atoms obey duplet rule?

H₂

O₂

N₂

F₂

6 / 16

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

Its covalent nature

Hydrogen bonding

Its higher molecular mass

Its higher density

7 / 16

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

Each sodium atom loses one electron

Sulphur forms anion

Each sulphur atom gains one electron

Sodium forms cation

8 / 16

Identify the covalent compound:

H<sub>2</sub>O

NaCl

MgO

9 / 16

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

Atomic Number : 12 Mass Number : 24

Atomic Number : 10 Mass Number : 20

Atomic Number : 14 Mass Number : 28

Atomic Number : 8 Mass Number : 16

10 / 16

Which of the following atoms will form cation?

Atomic number 18

Atomic number 15

Atomic number 20

Atomic number 17

11 / 16

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

O₂

F₂

N₂

H₂

12 / 16

In Hydrogen Iodide (HI), the bond is:

Non polar covalent bond

Polar covalent bond

Ionic bond

Co-ordinate covalent bond

13 / 16

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

Ionic bond

Covalent bond

Hydrogen bond

Co-ordinate bond

14 / 16

Which of the following substance has ionic bond?

MgO

H₂O

SO₂

CO₂

15 / 16

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

16 / 16

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

A (Atomic No. 16)

C (Atomic No. 18)

D (Atomic No. 19)

B (Atomic No. 17)

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Practice MCQs Test No 2

/16

Class 9 Chemistry

Chapter 4

Practice MCQs Test No 2

1 / 16

Atoms other than the noble gases are reactive because they tend to gain stability by:

All of these

gaining electrons

loosing electrons

Sharing electrons

2 / 16

Which one of the following compounds is not having an ionic bond?

NaCl

CO₂

MgO

MgF₂

3 / 16

The noble gases are sometimes called the:

Inert gases

None of these

Reactive gases

Noble metals

4 / 16

In forming compounds, atoms tend to gain electronic configuration of a:

Noble metal

Hydrogen gas

Halogen gas

Noble gas

5 / 16

In a covalent bond, the atom that contributes more electrons for sharing is the:

Central atom

Positive atom

Smallest atom

Biggest atom

6 / 16

Ionic compounds as a whole are:

Electrically neutral

Positively charged

Negatively charged

None of these

7 / 16

Due to high ionization energies, which element do NOT lose electron?

Radioactive elements

Metals

Non-metals

Transition elements

8 / 16

Which substance is NOT covalent?

HCN

H₂O

CO₂

CaO

9 / 16

Which of the following elements will gain one electron to complete its octet?

_{ 17 }^{ 35 }{ X }

_{ 13 }^{ 27 }{ X }

_{ 16 }^{ 32 }{ X }

_{ 18 }^{ 40 }{ X }

10 / 16

Which substance does not have ionic bond?

NaF

MgO

CH₄

NaCl

11 / 16

Pairs of valence electrons which are not shared between atoms are called:

None of these

Shared pair

Electron pair

Lone pair

12 / 16

When atoms gain or lose electron they acquire the configuration of:

Next noble gas element

Next noble metal element

All of these

Next Halogen gas element

13 / 16

The metal atoms form:

None of these

Both Cations and Anions

Cations

Anions

14 / 16

Which one of the following molecules has a non-polar covalent bond?

N₂

NH₃

NO₂

N₂O₄

15 / 16

Non-metal atoms form:

Both Cations and anions

None of these

Anions

Cations

16 / 16

Which of the following makes hydrogen very electron-deficient?

All of these

Nitrogen

Fluorine

Oxygen

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Challenge MCQs Test

/32

Class 9 Chemistry

Chapter 4

Challenge MCQs Test

1 / 32

Which one of the following compounds is not having an ionic bond?

NaCl

CO₂

MgO

MgF₂

2 / 32

Pairs of valence electrons which are not shared between atoms are called:

Lone pair

Electron pair

None of these

Shared pair

3 / 32

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

H₂

N₂

O₂

F₂

4 / 32

Silicon belongs to Group IVA. It has ______ electrons in the valence shell.

5 / 32

Which of the following makes hydrogen very electron-deficient?

Oxygen

All of these

Nitrogen

Fluorine

6 / 32

Which substance does not have ionic bond?

NaCl

CH₄

MgO

NaF

7 / 32

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

Co-ordinate bond

Ionic bond

Covalent bond

Hydrogen bond

8 / 32

The noble gases are sometimes called the:

None of these

Reactive gases

Inert gases

Noble metals

9 / 32

Which of the following atoms will form cation?

Atomic number 18

Atomic number 15

Atomic number 17

Atomic number 20

10 / 32

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

11 / 32

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

Each sodium atom loses one electron

Each sulphur atom gains one electron

Sodium forms cation

Sulphur forms anion

12 / 32

When atoms gain or lose electron they acquire the configuration of:

Next Halogen gas element

Next noble gas element

Next noble metal element

All of these

13 / 32

Non-metal atoms form:

Cations

None of these

Anions

Both Cations and anions

14 / 32

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

Hydrogen bonding

Its higher density

Its higher molecular mass

Its covalent nature

15 / 32

The covalent bond is formed by:

Accepting electron pair by one atom

Mutual sharing of an electron pair by two atoms

Complete transfer of electrons

Donating an electron pair by one atom

16 / 32

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

Atomic Number : 14 Mass Number : 28

Atomic Number : 10 Mass Number : 20

Atomic Number : 12 Mass Number : 24

Atomic Number : 8 Mass Number : 16

17 / 32

Which substance is NOT covalent?

H₂O

CO₂

HCN

CaO

18 / 32

In forming compounds, atoms tend to gain electronic configuration of a:

Halogen gas

Noble metal

Noble gas

Hydrogen gas

19 / 32

Which of the following substance has ionic bond?

H₂O

MgO

CO₂

SO₂

20 / 32

Due to high ionization energies, which element do NOT lose electron?

Radioactive elements

Non-metals

Transition elements

Metals

21 / 32

Atoms other than the noble gases are reactive because they tend to gain stability by:

gaining electrons

Sharing electrons

All of these

loosing electrons

22 / 32

Which one of the following molecules has a non-polar covalent bond?

N₂

N₂O₄

NH₃

NO₂

23 / 32

Hydrogen bonding is involved in:

Formation of crystals in NaCl

Conductance of electricity

Van der Waal's force

Adhesive action of paints

24 / 32

Identify the covalent compound:

MgO

H<sub>2</sub>O

NaCl

25 / 32

In a covalent bond, the atom that contributes more electrons for sharing is the:

Positive atom

Central atom

Smallest atom

Biggest atom

26 / 32

Ionic compounds as a whole are:

Negatively charged

None of these

Electrically neutral

Positively charged

27 / 32

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

28 / 32

The metal atoms form:

Anions

None of these

Both Cations and Anions

Cations

29 / 32

In Hydrogen Iodide (HI), the bond is:

Non polar covalent bond

Ionic bond

Polar covalent bond

Co-ordinate covalent bond

30 / 32

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

B (Atomic No. 17)

A (Atomic No. 16)

D (Atomic No. 19)

C (Atomic No. 18)

31 / 32

Which of the following atoms obey duplet rule?

F₂

N₂

H₂

O₂

32 / 32

Which of the following elements will gain one electron to complete its octet?

_{ 13 }^{ 27 }{ X }

_{ 16 }^{ 32 }{ X }

_{ 18 }^{ 40 }{ X }

_{ 17 }^{ 35 }{ X }

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Chapter 5

Practice MCQs Test No 1

/10

Class 9 Chemistry
Chapter 5
Practice MCQs Test No 1

1 / 10

Melting points of amorphous solid will be in _____.

definite temperature value

a particular range of temperature

a single positive value of temperature

a single negative value of temperature

2 / 10

_____ phase of physical states that can never be achieved in sublimation process.

semisolid

solids

liquids

gases

3 / 10

Liquids with weak intermolecular forces

cannot diffuse

contain a lot of kinetic energy

easily evaporate

freeze easily

4 / 10

Evaporation causes _____ effect ,due to this effect water is contained in the pitcher.

increase in weight

heating

increase in density

cooling

5 / 10

Sublimation is usually used to purify _____ state of matter.

liquids

gases

semiliquid

solids

6 / 10

As pressure decreases, boiling point ___

decreases then increases

increases

increases then decreases

decreases

7 / 10

Water bubbles arising in the beaker provided with the temperature of 100 °C is an example of _____.

distillation

compression

boiling

evaporation

8 / 10

Which of the following changes decrease the vapour pressure of water kept in a sealed vessel?

Decreasing the quantity of water

Decreasing the volume of the vessel to one-half

Adding salt to water

Decreasing the temperature of water

9 / 10

By touch, glass imparts a hard appearance but microscopically atoms may be _____ arranged.

irregularly

uniformly

regularly

three dimensionally

10 / 10

The boiling point of water is 100 °C, where internal vapour pressure becomes equal to atmospheric pressure. What is that atmospheric pressure?

1 atm

all of the above

101.325 kpa

760 mm Hg

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Practice MCQs Test No 2

/10

Class 9 Chemistry
Chapter 5
Practice MCQs Test No 2

1 / 10

Amount of vapour pressure of liquid decreases _______

At sea level

Depth

None of the above

Above sea level

2 / 10

Melting points of crystalline solids are _____ due to strong intermolecular forces existing .

sharp

low

medium

least

3 / 10

The particles in ___ are always vibrating, but don't move past each other.

solids and liquids

solids

gases

liquid

4 / 10

When the atmospheric pressure equals the equilibrium vapor pressure ___ occurs.

melting

boiling

freezing

sublimation

5 / 10

Statement related to process of evaporation that is incorrect is _____.

no bubbles are formed in the liquid during evaporation

temperature may change during evaporation

evaporation takes place within the liquid

evaporation occurs at any temperature

6 / 10

________ is usually used to purify liquids.

evaporation

condensation

sublimation

distillation

7 / 10

Identify the figure (a) and ( b)

( a ) crystalline ( b) amorphous

( a ) amorphous ( b) crystaline

Both are amorphous

Both are crystalline

8 / 10

Which figure has a repetitive pattern in its structure?

Fig A

Both A and B

Fig B

None of the above

9 / 10

A person living in hill stations observed that cooking food without using pressure cooker takes more time. The reason for this observation is that at high altitude_____

Pressure increases

Temperature increases

Pressure decreases

Pressure remain constant

10 / 10

If surface area of liquid is large then evaporation will be _____.

minute

small

moderate

large

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Chapter 8

Practice MCQs Test No 1

/15

Class 9 Chemistry

Chapter 8

Practice MCQs Test No 1

1 / 15

Metallic bonding involves _____.

electrons between metal cations

sharing of electrons between metal atoms

gain and loss of electrons between metal atoms

gain and loss of electrons between metal and non-metal atoms

2 / 15

Choose the correct order for metallic character.

Na>Mg>Al>Si

Na>Mg<Al>Si

Na<Mg<Al<Si

Na<Mg>Al<Si

3 / 15

Potassium super oxide react with moisture and carbon dioxide and produce

Oxygen

All of these

Potassium

Water

4 / 15

Which of the following metals will have the lowest melting point?

5 / 15

Copper nickle alloy is used to make

Crockery

Aeroplanes

Keys

Coins

6 / 15

Among all the alkali metals, cesium has the lowest ionization energy. Which of these will then have the highest electropositive character?

7 / 15

Electropositive character is also known as _____.

Metallic character

Covalent character

Electrolytic character

Electronegative character

8 / 15

Which of the following metals is NOT an active metal?

9 / 15

Which alloy is used by dentists?

Silver

Gold

Copper

Platinum

10 / 15

Name the mixture to which gold and platinum can react.

Milk of magnesia

Aqua regia

Air

Aqua acid

11 / 15

Name the Property of elements to lose electron and become cation .

Ionization energy

Electronegative character

Electropositive character

Electronegativity

12 / 15

Which of the following does not represent a symbol for noble metal?

13 / 15

Which of the following will react with most ease with oxygen present in the air?

Barium

Calcium

Sodium

Iron

14 / 15

As we go from Li to Cs, electropositive character _____.

Becomes zero

Remains same because valency remains same

Decreases

Increases

15 / 15

Nature of oxides of aluminium are

Basic

Amphoteric

Acidic

None of these

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Practice MCQs Test No 2

/10

Class 9 Chemistry
Chapter 8
Practice MCQs Test No 2

1 / 10

The only non-metal that exists in liquid state is _____.

Bromine

Carbon

Boron

Mercury

2 / 10

Atoms with high electronegative character prefer to form _____.

Molecules

Cations

Alloys

Anions

3 / 10

When hydrogen halides dissolve in water , it will form

Halogenic acid

None of these

Hydrohalic acid

Halic acid

4 / 10

Which of the following halogens does NOT exist in diatomic form?

Iodine

None of these

Chlorine

Fluorine

Bromine

5 / 10

Which non metal is the most non metallic ?

6 / 10

When halogens and metals react , they form salts called

Halic Salts

Nitrides

None of these

Halides

7 / 10

The correct increasing acidic strength of acids of halogens is

HF>HCl>HBr>HI

HF>HI>HBr>HCl

HF<HBr<HCl<HI

HF<HCl<HBr<HI

8 / 10

Fluorine can oxidize all halide ions because of high

Oxidizing power

Electropositivity

Reducing power

All of these

9 / 10

Which of the following elements will have the highest electronegativity?

Sodium

Fluorine

Potassium

Calcium

10 / 10

Which of the following elements is NOT a non-metal?

Hydrogen

Halogens

Carbon

Boron

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Class 9 Chemistry MCQs Tests