Chemistry 9th Chap 5 : Topic 3 - Maryam Publications

Chemistry Chapter 5 : Topic 3

Electropositive and Electronegative Nature

1 / 17

A student observes that metals tend to lose electrons during chemical reactions while non-metals tend to gain electrons. Which statement best explains this behavior?

A) Metals have loosely held valence electrons whereas non-metals strongly attract electrons.

B) Metals have high ionization energy while non-metals have low ionization energy.

C) Metals and non-metals both prefer to share electrons equally.

D) Metals have completely filled outer shells while non-metals have empty shells.

2 / 17

When sodium reacts with chlorine, sodium loses an electron and chlorine gains it. Which property of sodium is primarily responsible for this behavior?

A) Large number of neutrons

B) Electropositive nature

C) High electronegativity

D) High electron affinity

3 / 17

Which statement best explains why non-metals such as chlorine and oxygen readily gain electrons during reactions?

A) Their atoms are larger in size than metals.

B) They possess low nuclear charge.

C) Their valence shells are nearly filled and they attract electrons to complete the octet.

D) They contain more neutrons than protons.

4 / 17

Which of the following properties mainly causes metals to exhibit electropositive character?

A) High melting points

B) High density

C) Low ionization energy

D) Low thermal conductivity

5 / 17

Why do non-metals generally form negative ions during chemical reactions?

A) They lose protons easily.

B) Their outer shells are empty.

C) They tend to gain electrons due to strong attraction for electrons.

D) They have low electron affinity.

6 / 17

Which of the following periodic trends best explains why metals are electropositive?

A) Metals have larger atomic radii and weaker attraction for valence electrons.

B) Metals have higher electronegativity than non-metals.

C) Metals contain more neutrons than non-metals.

D) Metals are located on the right side of the periodic table.

7 / 17

A student claims that fluorine is highly electronegative. Which observation supports this claim?

A) Fluorine atoms contain equal numbers of electrons and protons.

B) Fluorine readily loses electrons to form positive ions.

C) Fluorine strongly attracts electrons in a chemical bond.

D) Fluorine atoms have very low nuclear charge.

8 / 17

Which pair of elements would most likely form an ionic compound due to electropositive and electronegative behavior?

A) Sodium and chlorine

B) Carbon and hydrogen

C) Oxygen and nitrogen

D) Chlorine and fluorine

9 / 17

Why do metals generally form cations while non-metals form anions?

A) Metals gain electrons while non-metals lose electrons.

B) Both metals and non-metals gain electrons.

C) Metals and non-metals both lose electrons equally.

D) Metals lose electrons while non-metals gain electrons.

10 / 17

A chemist compares magnesium and oxygen. Magnesium forms Mg²⁺ while oxygen forms O²⁻. Which explanation best accounts for this difference?

A) Magnesium has high electronegativity while oxygen has low electronegativity.

B) Both elements prefer to share electrons only.

C) Magnesium tends to gain electrons while oxygen tends to lose electrons.

D) Magnesium tends to lose electrons while oxygen tends to gain electrons.

11 / 17

Which statement best relates electronegativity with the position of elements in the periodic table?

A) Electronegativity decreases down a group and increases across a period.

B) Electronegativity depends only on the number of neutrons.

C) Electronegativity remains constant across the periodic table.

D) Electronegativity increases down a group and decreases across a period.

12 / 17

A metal atom loses two electrons during a reaction. What is the most likely reason for this behavior?

A) It has high electronegativity.

B) It tends to achieve a stable noble gas configuration by losing electrons.

C) Its valence shell is completely filled.

D) It has more neutrons than protons.

13 / 17

Which property directly measures the ability of an atom to attract electrons toward itself in a chemical bond?

A) Density

B) Atomic radius

C) Ionization energy

D) Electronegativity

14 / 17

A comparison between potassium and fluorine shows opposite chemical behavior. Which explanation best accounts for this?

A) Potassium has high electronegativity while fluorine has low electronegativity.

B) Potassium gains electrons easily while fluorine loses electrons.

C) Both elements equally share electrons.

D) Potassium readily loses electrons while fluorine strongly attracts electrons.

15 / 17

Why does the electropositive character of metals increase down a group in the periodic table?

A) The number of neutrons decreases.

B) Atomic size increases and outer electrons are farther from the nucleus.

C) Nuclear charge decreases.

D) Atomic size decreases and electrons are tightly held.

16 / 17

Which situation best demonstrates the electronegative nature of non-metals?

A) Chlorine gaining an electron to form Cl⁻.

B) Iron conducting electricity.

C) Sodium releasing energy during a reaction.

D) Calcium losing electrons to form Ca²⁺.

17 / 17

In a chemical bond between a metal and a non-metal, the electron density is usually shifted toward the non-metal. Why?

A) Both atoms repel electrons equally.

B) The non-metal has greater electronegativity.

C) The metal has a smaller atomic radius.

D) The metal nucleus attracts electrons more strongly.

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