Chemistry 9th Chap 4 : Topic 4 - Maryam Publications

Chemistry Chapter 4 : Topic 4

Group Chemical Similarities

1 / 20

Elements in the same group of the periodic table show similar chemical properties even though their atomic sizes increase down the group. A student explains this by linking it with electronic configuration. Which statement best supports this idea?

A) Elements in a group have different numbers of protons.

B) Elements in a group have the same number of shells.

C) Elements in a group have the same number of valence electrons.

D) Elements in a group have identical atomic masses.

2 / 20

Lithium (Li), Sodium (Na), and Potassium (K) belong to Group 1. They all react similarly with water. What is the most appropriate reason based on electronic configuration?

A) They all have one electron in their outermost shell.

B) They all have different numbers of neutrons.

C) They all belong to the same period.

D) They all have completely filled outer shells.

3 / 20

Fluorine, chlorine, and bromine belong to Group 17 and show similar reactivity. Which explanation best connects this behavior with their electronic configuration?

A) They all belong to transition elements.

B) They all have full outer shells.

C) They all have seven electrons in their outermost shell.

D) They all lose seven electrons easily.

4 / 20

Why do sodium and potassium behave similarly in chemical reactions despite being in different periods?

A) They have same number of valence electrons in outer shell.

B) They have identical atomic radii.

C) They have same number of shells.

D) They have different nuclear charges only.

5 / 20

Elements in Group 2 such as magnesium and calcium show similar chemical properties. What is the correct electronic explanation?

A) They both gain two electrons easily.

B) They both belong to noble gases.

C) They both have full p-orbitals.

D) They both have two valence electrons in outer shell.

6 / 20

A student compares chlorine and iodine and notes similar chemical behavior. What is the best explanation?

A) They both have seven valence electrons in outermost shell.

B) They both have complete octets.

C) They both have one valence electron.

D) They both are metals.

7 / 20

Why do elements in the same group form similar types of compounds?

A) Because they have same valence electron configuration.

B) Because they are in same period.

C) Because they have same atomic masses.

D) Because they have same number of neutrons.

8 / 20

Which of the following best explains why lithium, sodium, and potassium all form + 1 ions?

A) They all share electrons equally.

B) They all have full outer shells.

C) They all gain one electron.

D) They all have one electron in outermost shell which is easily lost.

9 / 20

A student observes that fluorine and chlorine both form - 1 ions. What is the correct electronic reason?

A) They both have one valence electron.

B) They both lose electrons easily.

C) They both are metals.

D) They both have seven valence electrons and gain one electron.

10 / 20

Why do noble gases show very low reactivity compared to other groups?

A) They have unstable electronic configuration.

B) They have completely filled valence shells.

C) They have incomplete outer shells.

D) They have high atomic masses.

11 / 20

Magnesium and calcium behave similarly when reacting with oxygen. What is the electronic reason?

A) Both have full octets.

B) Both are non-metals.

C) Both have one valence electron.

D) Both have two valence electrons in outer shell.

12 / 20

A teacher explains that chemical similarity in a group is due to periodic repetition of electronic configuration. What does this mean?

A) Elements repeat atomic mass values.

B) Elements repeat valence electron patterns.

C) Elements have same physical state.

D) Elements have same number of neutrons.

13 / 20

Why do halogens (Group 17) show similar ability to form salts?

A) They gain one electron to form halide ions.

B) They lose electrons easily.

C) They are all metals.

D) They have full outer shells already.

14 / 20

Which statement best connects electronic configuration with group properties?

A) Atomic mass determines chemical similarity

B) Physical state determines group behavior

C) Chemical behavior depends on valence electrons

D) Group properties depend on number of protons only

15 / 20

Elements in the same group behave similarly because they have:

A) Same atomic radius

B) Same number of energy levels

C) Same density

D) Same number of valence electrons

16 / 20

Why do sodium and potassium both form ionic compounds with chlorine?

A) They both are non-metals.

B) They both gain electrons.

C) They both have full octets.

D) They both have one valence electron to lose.

17 / 20

Which concept best explains similarity of elements in a group?

A) Similar number of shells

B) Similar atomic mass

C) Similar nuclear structure

D) Similar valence shell electronic configuration

18 / 20

A student notices that all Group 1 elements react vigorously with water. What is the best electronic explanation?

A) They are noble gases.

B) They have seven valence electrons.

C) They have full outer shells.

D) They have one loosely held valence electron.

19 / 20

Why do chlorine and bromine show similar bleaching and oxidizing properties?

A) They both are metals.

B) They both have two valence electrons.

C) They both have full shells.

D) They both have seven valence electrons.

20 / 20

What is the most important factor responsible for similarity in chemical properties of a group?

A) Number of shells

B) Density of elements

C) Number of valence electrons

D) Atomic mass

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