Chemistry 9th Chap 4 : Topic 3 - Maryam Publications

Chemistry Chapter 4 : Topic 3

Group and Ionic Charge

1 / 15

An element belongs to Group 1 of the periodic table. It is observed that it readily forms a positively charged ion by losing one electron from its outermost shell. Which statement best explains this behavior in terms of its group number?

A) Group 1 elements form + 2 ions because they contain two energy levels.

B) Group 1 elements have one valence electron which is easily lost, forming + 1 ions.

C) Group 1 elements gain one electron to complete their octet and form negative ions.

D) Group 1 elements have completely filled outer shells, so they do not form ions.

2 / 15

An element from Group 17 shows a strong tendency to form a negatively charged ion. A student explains this by relating it to its outer shell configuration. Which explanation is most correct?

A) It loses one proton from the nucleus to become stable.

B) It shares electrons equally with metals only.

C) It loses seven electrons to achieve stability.

D) It gains one electron to complete its octet in the outermost shell.

3 / 15

An element in Group 2 forms a stable ion with a +2 charge. Which reasoning best connects group number with ionic charge?

A) Group number equals number of neutrons in nucleus.

B) Group 2 elements lose two outermost electrons to achieve stability.

C) Group 2 elements gain two electrons to complete inner shells.

D) Group number determines atomic mass and charge together.

4 / 15

A student states that Group 18 elements generally do not form ions under normal conditions. Which explanation best supports this idea?

A) They have unstable electronic configurations.

B) They have incomplete outer shells.

C) They have no electrons in outer shell.

D) Their outermost shells are already completely filled.

5 / 15

An element has electronic configuration ending in 3s² 3p¹ and belongs to Group 13. It forms a + 3 ion. What is the correct explanation?

A) It shares three electrons equally with non-metals.

B) It gains electrons to reduce nuclear charge.

C) It loses three valence electrons from outermost shell.

D) It gains three electrons to complete octet.

6 / 15

A chemistry student observes that elements in Group 16 often form - 2 ions. Which concept best explains this pattern?

A) They gain two electrons to complete their outermost shell.

B) They lose six electrons to achieve stability.

C) They lose two electrons because of high metallic character.

D) They do not follow octet rule.

7 / 15

An element in Group 15 can form an ion with a - 3 charge under certain conditions. What is the correct interpretation of this behavior?

A) It shares three electrons permanently.

B) It gains protons to balance charge.

C) It loses three electrons due to metallic nature.

D) It gains three electrons to complete its outermost shell.

8 / 15

A student generalizes that “for main group elements, ionic charge can be predicted from group number.” Which statement best supports this idea?

A) Group number relates to number of valence electrons and electron gain / loss tendency.

B) Group number determines atomic radius only.

C) Group number indicates number of energy levels.

D) Group number is unrelated to electronic configuration.

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An element has two electrons in its outermost shell and belongs to Group 2. Which statement correctly describes its ion formation?

A) It loses two electrons to form + 2 ion.

B) It gains two electrons to form - 2 ion.

C) It gains one and loses one electron simultaneously.

D) It shares electrons without forming ions.

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A student compares Group 1 and Group 17 elements and concludes they form ions with opposite charges. What is the best explanation of this observation?

A) Group 1 loses one electron while Group 17 gains one electron to complete octet.

B) Group 1 gains electrons and Group 17 loses electrons.

C) Both groups form neutral atoms only.

D) Both groups lose electrons equally.

11 / 15

Why do elements in the same group of the periodic table form ions with similar charges?

A) They have identical atomic masses.

B) They have similar number of valence electrons in outermost shell.

C) They have same number of energy levels.

D) They contain same number of neutrons.

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A student analyzes an unknown element that forms a + 1 ion and has one electron in its outer shell. Which group is most likely for this element?

A) Group 16

B) Group 1

C) Group 17

D) Group 2

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An element forms an ion by gaining electrons until its outer shell becomes stable. Which group is least likely to follow this behavior?

A) Group 17

B) Group 1

C) Group 16

D) Group 15

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A student states: “The ionic charge of main group elements is directly related to the number of electrons lost or gained to achieve noble gas configuration.” Which explanation is best?

A) Only metals form ions

B) Ionic charge is random for each element

C) Ionic charge depends only on atomic mass

D) Elements adjust electrons in outer shell to become stable like noble gases

15 / 15

An element from Group 14 can sometimes show + 4 or - 4 behavior. What does this indicate?

A) It only forms positive ions.

B) It belongs to noble gases.

C) It has no valence electrons.

D) It can either lose or gain electrons depending on bonding conditions.

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