Free Printable Chemistry Quiz

1.

How many new chemical compounds are estimated to be produced annually?

a)

100,000

b)

200,000

c)

500,000

d)

1,000,000

2.

What is the chemical formula for table salt mentioned in the text?

a)

NaCl

b)

C12H22O11

c)

NaClO

d)

H2O

3.

What is the main constituent of bleach according to the text?

a)

NaCl

b)

C12H22O11

c)

NaClO

d)

H2O

4.

Which of the following is used to sweeten coffee as mentioned in the text?

a)

NaCl

b)

C12H22O11

c)

NaClO

d)

H2O

5.

What are the electrons in the outermost shell of an atom called?

a)

Core electrons

b)

Valence electrons

c)

Inner electrons

d)

Reactive electrons

6.

Which type of electrons do not influence chemical reactions?

a)

Valence electrons

b)

Core electrons

c)

Reactive electrons

d)

Outer electrons

7.

Who established a simple and useful way to represent the electrons of an atom's valence shell by dots?

a)

Albert Einstein

b)

Isaac Newton

c)

Gilbert Newton Lewis

d)

Marie Curie

8.

According to the octet rule, how many electrons do atoms aim to have in their valence shell to achieve stability?

a)

2

b)

4

c)

6

d)

8

9.

Which element is an exception in Group A, having only 2 valence electrons?

a)

Helium (He)

b)

Hydrogen (H)

c)

Lithium (Li)

d)

Beryllium (Be)

10.

What is the electronic configuration of Sodium (Na)?

a)

1s²2s²2p⁶3s²

b)

1s²2s²2p⁶3s¹

c)

1s²2s²2p⁶3p⁵

d)

1s²2s²2p⁶3p⁶

11.

Which noble gas is closest to Chlorine (Cl) in terms of electronic configuration?

a)

Helium (He)

b)

Neon (Ne)

c)

Argon (Ar)

d)

Krypton (Kr)

12.

What is the result of the electrostatic attraction between the positive charge of the Na⁺ cation and the negative charge of the Cl⁻ anion?

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

d)

Hydrogen bond

13.

What does Na (sodium) need to do to become isoelectronic with Ne (neon)?

a)

Gain an electron

b)

Lose an electron

c)

Gain two electrons

d)

Lose two electrons

14.

What is the formula for lithium oxide?

a)

LiO

b)

Li₂O

c)

LiO₂

d)

Li₂O₂

15.

What is the electronic configuration of oxygen (O)?

a)

1s²2s²2p⁴

b)

1s²2s²2p⁶

c)

1s²2s¹2p⁴

d)

1s²2s²2p³

16.

What happens to chlorine (Cl) to become isoelectronic with argon (Ar)?

a)

It loses an electron

b)

It gains an electron

c)

It loses two electrons

d)

It gains two electrons

17.

What is the electronic configuration of lithium (Li)?

a)

1s²2s²

b)

1s²2s¹

c)

1s²2p¹

d)

1s¹2s²

18.

What is the charge of the lithium ion (Li⁺) after it loses an electron?

a)

-1

b)

+1

c)

-2

d)

+2

19.

What is the charge of the oxygen ion (O²⁻) after it gains two electrons?

a)

-1

b)

+1

c)

-2

d)

+2

20.

What is a covalent bond?

a)

$A) A pair of electrons shared between two atoms$

b)

$B) A transfer of electrons from one atom to another$

c)

$C) A bond formed by the attraction of opposite charges$

d)

$D) A bond that occurs only in metals$

21.

How is a covalent bond represented in the hydrogen molecule (H2)?

a)

$A) H-H$

b)

$B) H:H$

c)

$C) H+H$

d)

$D) H-H-H$

22.

What is the main characteristic of a covalent bond?

a)

$A) Both atoms need electrons$

b)

$B) One atom gives electrons to another$

c)

$C) It only occurs in metals$

d)

$D) It is weaker than ionic bonds$

23.

According to the Octet Rule, how many electrons does an atom tend to have in its outer shell to be stable?

a)

$A) 8$

b)

$B) 2$

c)

$C) 6$

d)

$D) 4$

24.

Who formulated the Octet Rule?

a)

$A) Lewis$

b)

$B) Newton$

c)

$C) Einstein$

d)

$D) Bohr$

25.

What is the first step in writing a Lewis structure for a substance?

a)

Determine the total number of valence electrons.

b)

Choose the central atom and write the skeleton of the compound.

c)

Connect the central atom to other atoms with single covalent bonds.

d)

Represent non-bonding electrons as lone pairs.

26.

In a Lewis structure, which atoms frequently occupy the central position?

a)

Hydrogen and halogens

b)

Atoms with lower electronegativity like C, N, P, and S

c)

Atoms with higher electronegativity like O and F

d)

Noble gases

27.

How many valence electrons are present in the NH₄⁺ ion?

a)

8

b)

9

c)

7

d)

6

28.

What should be done if the structure is for an anion?

a)

Subtract a number of electrons equal to the positive charge.

b)

Add a number of electrons equal to the negative charge.

c)

Subtract a number of electrons equal to the negative charge.

d)

Add a number of electrons equal to the positive charge.

29.

What are lone pairs in a Lewis structure?

a)

Electrons that participate in covalent bonding.

b)

Electrons that do not participate in covalent bonding.

c)

Electrons that are shared between atoms.

d)

Electrons that are lost during bond formation.

30.

How many valence electrons are present in the NO₃⁻ ion?

a)

24

b)

18

c)

8

d)

12

31.

What is the purpose of distributing remaining electrons in a Lewis structure?

a)

To complete the octet of all atoms.

b)

To form double bonds.

c)

To create lone pairs.

d)

To balance the charge.

32.

What is the total number of valence electrons in CH₄?

a)

4

b)

6

c)

8

d)

10

33.

Which of the following is an example of a molecule with a double bond?

a)

CH₄

b)

PCl₃

c)

C=C

d)

H₂O

34.

In the Lewis structure of PCl₃, how many valence electrons are there in total?

a)

8

b)

18

c)

26

d)

32

35.

What is the central atom in the Lewis structure of CH₄?

a)

H

b)

C

c)

O

d)

N

36.

How many valence electrons does each hydrogen atom contribute in CH₄?

a)

1

b)

2

c)

3

d)

4

37.

What type of bond is formed between the atoms in CH₄?

a)

Ionic bond

b)

Covalent bond

c)

Metallic bond

d)

Hydrogen bond

38.

In the Lewis structure of PCl₃, how many chlorine atoms are bonded to the phosphorus atom?

a)

1

b)

2

c)

3

d)

4

39.

What is the first step in drawing the Lewis structure of a molecule?

a)

Determine the total number of valence electrons

b)

Draw the skeleton structure

c)

Connect atoms with single bonds

d)

Add lone pairs to atoms

40.

How many valence electrons are represented in the initial structure of Cl-P-Cl?

a)

6

b)

20

c)

26

d)

18

41.

How many electrons does each Cl need to complete its octet in the Cl-P-Cl structure?

a)

2

b)

4

c)

6

d)

8

42.

What is the total number of valence electrons in the SO2 molecule?

a)

18

b)

20

c)

16

d)

14

43.

In the SO2 structure, how many electrons are needed to satisfy the octet rule for each oxygen atom?

a)

4

b)

6

c)

8

d)

2

44.

What is the final step to satisfy the octet rule for all atoms in the SO2 structure?

a)

Add more electrons

b)

Remove electrons

c)

Move a pair of electrons from one oxygen to form an additional bond with sulfur

d)

Change the structure

45.

How many valence electrons are represented in the final structure of SO2?

a)

14

b)

16

c)

18

d)

20

46.

What is the total number of valence electrons in the NO5 molecule?

a)

10

b)

12

c)

14

d)

16

47.

What is the first step in forming a chemical bond between nitrogen (N) and carbon (C)?

a)

Move 2 pairs of isolated electrons from O to N

b)

Connect each pair of atoms with a single bond

c)

Calculate the valence electrons

d)

Form a double bond between N and C

48.

How many valence electrons are represented in the final structure of the molecule?

a)

8

b)

10

c)

24

d)

6

49.

What is the term used to describe the phenomenon where a molecule can be represented by two or more valid Lewis structures?

a)

Resonance

b)

Octet Rule

c)

Valence Bond

d)

Ionic Bond

50.

According to the text, which type of bond is expected to be larger in size?

a)

Single bond (O - O)

b)

Double bond (O = O)

c)

Triple bond (N ≡ O)

d)

Ionic bond

51.

What is the term used to represent two or more Lewis structures for a single molecule?

a)

Resonance

b)

Octet Rule

c)

Valence Bond

d)

Hybridization

52.

What is the bond length of a double bond C=O in the given text?

a)

1.48 nm

b)

1.21 nm

c)

0.122 pm

d)

129 pm

53.

Which ion is used as an example of resonance in the text?

a)

Ozone (O₃)

b)

Carbonate (CO₃²⁻)

c)

Water (H₂O)

d)

Ammonium (NH₄⁺)

54.

What is the bond length of a single C-O bond mentioned in the text?

a)

1.48 nm

b)

1.21 nm

c)

143 pm

d)

129 pm

55.

What is the exception to the Octet Rule mentioned in the text?

a)

Molecules with more than eight electrons

b)

Molecules with exactly eight electrons

c)

Molecules with less than eight electrons

d)

Molecules with no electrons

56.

What is the Lewis structure for H₂Be as given in the text?

a)

H-Be-H

b)

H-Be-H₂

c)

H₂-Be-H

d)

H-Be

57.

In the example given, why is the Octet Rule not satisfied for the atom of Beryllium (Be)?

a)

Because Be shares four electrons with two Hydrogen (H) atoms.

b)

Because Be has more than eight electrons.

c)

Because Be is bonded to halogens.

d)

Because Be has an odd number of electrons.

58.

What are molecules with an atom that has more than eight electrons called?

a)

Molecules with expanded octet.

b)

Molecules with reduced octet.

c)

Molecules with odd number of electrons.

d)

Molecules with even number of electrons.

59.

Which atoms can frequently be the central atom in molecules with an expanded octet?

a)

P, S, Cl

b)

H, He, Li

c)

C, N, O

d)

Na, Mg, Al

60.

How many valence electrons does Phosphorus (P) have in the molecule PCl5?

a)

5

b)

7

c)

10

d)

8

61.

How many total valence electrons are there in PCl5?

a)

40

b)

35

c)

30

d)

25

62.

Why is the Octet Rule not satisfied for the atom of Phosphorus (P) in PCl5?

a)

Because P is surrounded by 10 valence electrons.

b)

Because P is surrounded by 8 valence electrons.

c)

Because P is surrounded by 6 valence electrons.

d)

Because P is surrounded by 4 valence electrons.

63.

What is the total number of valence electrons in Nitric Oxide (NO)?

a)

11

b)

10

c)

9

d)

8

64.

What is the total number of valence electrons in Nitrogen Dioxide (NO2)?

a)

17

b)

15

c)

13

d)

11

65.

Why is it impossible to draw Lewis structures with an odd number of electrons?

a)

Because they cannot satisfy the Octet Rule.

b)

Because they have too many electrons.

c)

Because they have too few electrons.

d)

Because they are unstable.

66.

Despite having an odd number of electrons, why are molecules like NO and NO2 stable?

a)

Because they can be approximated to Lewis structures.

b)

Because they have an even number of electrons.

c)

Because they are bonded to halogens.

d)

Because they have a reduced octet.

Chemistry Quiz

Total questions: 1

Worksheet time: 35mins

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