Chemistry 9th Chap 4 : Topic 19 - Maryam Publications

Chemistry Chapter 4 : Topic 19

Noble Gas Configuration

1 / 20

Which statement best explains why noble gases are chemically inert in terms of their electronic configuration?

A) Their electrons are loosely bound and easily shared with other atoms.

B) They have partially filled outer shells, but strong nuclear forces prevent reactions.

C) They possess unstable nuclei that discourage bonding.

D) Their outermost shell is completely filled, making them electronically stable and unreactive.

2 / 20

Which of the following electronic configurations corresponds to a noble gas and explains its lack of reactivity?

A) 2, 7

B) 2, 8, 1

C) 2, 6

D) 2, 8

3 / 20

Why does Helium behave differently from other noble gases in terms of its stable electronic configuration?

A) Its electrons are unstable and reactive.

B) It has more than eight electrons in its valence shell.

C) It has no electrons in its outer shell.

D) It follows the duplet rule instead of the octet rule.

4 / 20

Which conclusion can be drawn when comparing the electronic configurations of noble gases and alkali metals?

A) Both have completely filled outer shells.

B) Both easily gain electrons to become stable.

C) Alkali metals have more stable configurations than noble gases.

D) Noble gases have full valence shells, while alkali metals have one electron in the outermost shell.

5 / 20

Which statement correctly relates the stability of noble gases to their ionization energy?

A) Ionization energy is unrelated to electronic configuration.

B) Noble gases easily lose electrons due to full shells.

C) Noble gases have low ionization energy due to weak nuclear attraction.

D) Noble gases have very high ionization energy due to stable electronic configurations.

6 / 20

Why do noble gases rarely form ions under normal conditions?

A) They have very low atomic masses.

B) They cannot gain or lose electrons easily due to stable configurations.

C) They have incomplete valence shells.

D) They do not contain protons.

7 / 20

Which of the following best explains why Neon does not form compounds easily?

A) It has no electrons in the outer shell.

B) Its valence shell is incomplete.

C) It already has a stable octet configuration.

D) It has an unstable nucleus.

8 / 20

What would be the most likely behavior of an atom with electronic configuration 2, 8, 7 compared to noble gases?

A) It will gain one electron to achieve noble gas configuration.

B) It will lose seven electrons to become stable.

C) It will behave like a noble gas due to nearly complete shell.

D) It will remain completely inert.

9 / 20

Which property of noble gases is directly linked to their electronic configuration?

A) Chemical inertness

B) High reactivity

C) Tendency to form ionic bonds

D) Strong metallic character

10 / 20

Which statement explains why noble gases exist as monoatomic gases?

A) Their electronic configuration discourages bonding with other atoms.

B) Their nuclei are unstable.

C) Their atoms are strongly attracted to each other.

D) They form strong ionic bonds.

11 / 20

Which of the following comparisons best explains the trend in reactivity between noble gases and halogens?

A) Both have complete valence shells.

B) Both are equally reactive.

C) Halogens have one electron less than noble gases and are highly reactive.

D) Noble gases have one electron less than halogens.

12 / 20

Why is Argon less likely to participate in chemical reactions compared to Chlorine?

A) Chlorine has a complete outer shell.

B) Argon has unstable electrons.

C) Argon has a complete octet, while Chlorine needs one electron.

D) Argon has fewer electrons than Chlorine.

13 / 20

Which of the following electronic configurations represents an element that would behave similarly to noble gases?

A) 2, 8, 3

B) 2, 6

C) 2, 8, 2

D) 2, 8, 8

14 / 20

Which statement best explains why noble gases have almost zero electron affinity?

A) Their outer shell is complete, so they do not need extra electrons.

B) They readily form anions.

C) They strongly attract additional electrons.

D) They have empty valence shells.

15 / 20

Which factor is primarily responsible for the chemical inactivity of noble gases?

A) Complete valence shell

B) High density

C) Large atomic size

D) High melting point

16 / 20

Which noble gas does NOT follow the octet rule but is still stable?

A) Helium

B) Argon

C) Neon

D) Krypton

17 / 20

If an atom achieves the electronic configuration of a noble gas, what is its expected chemical behavior?

A) Moderately reactive

B) Chemically stable and unreactive

C) Highly reactive

D) Highly radioactive

18 / 20

Which of the following statements is TRUE about noble gases?

A) They tend to lose electrons easily.

B) They form strong covalent bonds readily.

C) They neither gain nor lose electrons under normal conditions.

D) They tend to gain electrons easily.

19 / 20

Why do noble gases have very low chemical reactivity compared to other groups in the periodic table?

A) They lack protons.

B) They have very large atomic radii.

C) Their electrons are highly mobile.

D) Their outermost shell is fully occupied, making them stable.

20 / 20

Which statement best summarizes the relationship between noble gas configuration and chemical stability?

A) Stability depends only on atomic mass.

B) Stability increases when atoms lose electrons completely.

C) Stability is achieved when atoms have a complete outer shell like noble gases.

D) Stability occurs when atoms form as many bonds as possible.

Your score is

0%