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 and non-metals both prefer to share electrons equally.

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

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

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) High electron affinity

B) Large number of neutrons

C) High electronegativity

D) Electropositive nature

3 / 17

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

A) They contain more neutrons than protons.

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

C) Their atoms are larger in size than metals.

D) They possess low nuclear charge.

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

A) High melting points

B) Low ionization energy

C) High density

D) Low thermal conductivity

5 / 17

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

A) Their outer shells are empty.

B) They have low electron affinity.

C) They lose protons easily.

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

6 / 17

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

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

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

C) Metals contain more neutrons than non-metals.

D) Metals have higher electronegativity than non-metals.

7 / 17

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

A) Fluorine readily loses electrons to form positive ions.

B) Fluorine strongly attracts electrons in a chemical bond.

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

D) Fluorine atoms have very low nuclear charge.

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

A) Sodium and chlorine

B) Oxygen and nitrogen

C) Chlorine and fluorine

D) Carbon and hydrogen

9 / 17

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

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

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

C) Both metals and non-metals gain electrons.

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

10 / 17

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

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

B) Both elements prefer to share electrons only.

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

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

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

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

B) Electronegativity remains constant across the periodic table.

C) Electronegativity depends only on the number of neutrons.

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

12 / 17

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

A) Its valence shell is completely filled.

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

C) It has high electronegativity.

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) Electronegativity

B) Atomic radius

C) Density

D) Ionization energy

14 / 17

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

A) Both elements equally share electrons.

B) Potassium gains electrons easily while fluorine loses electrons.

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

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

15 / 17

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

A) Atomic size decreases and electrons are tightly held.

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

C) The number of neutrons decreases.

D) Nuclear charge decreases.

16 / 17

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

A) Iron conducting electricity.

B) Chlorine gaining an electron to form Cl⁻.

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) The metal has a smaller atomic radius.

B) The metal nucleus attracts electrons more strongly.

C) Both atoms repel electrons equally.

D) The non-metal has greater electronegativity.

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