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) They possess unstable nuclei that discourage bonding.

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

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

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

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

C) 2, 6

D) 2, 8, 1

3 / 20

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

A) It has no electrons in its outer shell.

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

C) Its electrons are unstable and reactive.

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

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

5 / 20

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

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

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

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

D) Ionization energy is unrelated to electronic configuration.

6 / 20

Why do noble gases rarely form ions under normal conditions?

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

B) They have incomplete valence shells.

C) They do not contain protons.

D) They have very low atomic masses.

7 / 20

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

A) It has an unstable nucleus.

B) Its valence shell is incomplete.

C) It has no electrons in the outer shell.

D) It already has a stable octet configuration.

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 behave like a noble gas due to nearly complete shell.

C) It will lose seven electrons to become stable.

D) It will remain completely inert.

9 / 20

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

A) Strong metallic character

B) Chemical inertness

C) High reactivity

D) Tendency to form ionic bonds

10 / 20

Which statement explains why noble gases exist as monoatomic gases?

A) Their atoms are strongly attracted to each other.

B) They form strong ionic bonds.

C) Their electronic configuration discourages bonding with other atoms.

D) Their nuclei are unstable.

11 / 20

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

A) Both are equally reactive.

B) Noble gases have one electron less than halogens.

C) Both have complete valence shells.

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

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 fewer electrons than Chlorine.

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

13 / 20

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

A) 2, 8, 2

B) 2, 8, 3

C) 2, 8, 8

D) 2, 6

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 strongly attract additional electrons.

C) They have empty valence shells.

D) They readily form anions.

15 / 20

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

A) High melting point

B) Complete valence shell

C) High density

D) Large atomic size

16 / 20

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

A) Helium

B) Neon

C) Krypton

D) Argon

17 / 20

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

A) Moderately reactive

B) Highly radioactive

C) Highly reactive

D) Chemically stable and unreactive

18 / 20

Which of the following statements is TRUE about noble gases?

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

B) They tend to lose electrons easily.

C) They tend to gain electrons easily.

D) They form strong covalent bonds readily.

19 / 20

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

A) They lack protons.

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

C) Their electrons are highly mobile.

D) They have very large atomic radii.

20 / 20

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

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

B) Stability depends only on atomic mass.

C) Stability increases when atoms lose electrons completely.

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

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