Chemistry 9th Chap 4 : Topic 20 - Maryam Publications

Chemistry Chapter 4 : Topic 20

Metals and Non-Metals

1 / 20

Which statement best explains why metals are generally good conductors of heat compared to non-metals?

A) Metals contain loosely packed atoms that vibrate less and restrict heat flow.

B) Metals possess free-moving electrons that transfer kinetic energy efficiently.

C) Metals chemically react with heat, enhancing conduction.

D) Metals have lower density, allowing faster heat transfer.

2 / 20

A student observes that graphite conducts electricity while diamond does not, even though both are non-metals. What is the most appropriate explanation?

A) Graphite contains impurities that allow current flow.

B) Graphite is an alloy, while diamond is a pure substance.

C) Diamond is metallic in nature but lacks charge carriers.

D) Graphite has free electrons due to its layered structure, unlike diamond.

3 / 20

Which of the following statements correctly distinguishes electrical conductivity in metals and non-metals?

A) Both metals and non-metals conduct electricity equally under normal conditions.

B) Metals conduct electricity through free electrons, while non-metals generally lack mobile charge carriers.

C) Non-metals conduct electricity better because of stronger bonds.

D) Metals conduct electricity due to ions, while non-metals conduct due to electrons.

4 / 20

Which property allows metals to be beaten into thin sheets without breaking?

A) Malleability due to layers of atoms sliding over each other

B) Elasticity due to weak intermolecular forces

C) Brittleness due to strong covalent bonds

D) Ductility due to ionic bonding

5 / 20

A metal wire is stretched into a thin shape without breaking. Which property is being demonstrated and why?

A) Malleability, due to strong directional bonding

B) Elasticity, due to ionic lattice structure

C) Ductility, due to non-directional metallic bonding

D) Conductivity, due to free ions

6 / 20

Why are non-metals generally brittle compared to metals?

A) Non-metals have weak metallic bonds.

B) Non-metals contain free electrons that resist deformation.

C) Non-metals have high density.

D) Non-metals have directional covalent bonds that break easily under stress.

7 / 20

Which of the following best compares melting points of metals and non-metals?

A) Both metals and non-metals have identical melting points.

B) Non-metals always have higher melting points due to covalent bonding.

C) Metals generally have higher melting points due to strong metallic bonding.

D) Metals have lower melting points because of weak bonding.

8 / 20

A substance has a very low boiling point and does not conduct electricity. It is most likely:

A) A non-metal with weak intermolecular forces

B) A transition metal

C) A metallic oxide

D) An alloy

9 / 20

Which statement best explains why metals can conduct electricity in solid state but ionic compounds cannot?

A) Metals contain mobile electrons, while ions in ionic compounds are fixed in solid state.

B) Metals have ions that move freely.

C) Metals dissolve in water to conduct electricity.

D) Ionic compounds lack charged particles.

10 / 20

Which of the following observations would most strongly indicate that a substance is a non-metal?

A) It has high melting and boiling points.

B) It can be drawn into wires easily.

C) It is shiny and conducts heat efficiently.

D) It breaks when hammered and does not conduct electricity.

11 / 20

Which statement correctly compares thermal conductivity of metals and non-metals?

A) Metals conduct heat efficiently due to mobile electrons, unlike non-metals.

B) Non-metals are better conductors due to strong covalent bonds.

C) Both conduct heat equally due to atomic vibrations.

D) Metals are poor conductors because their atoms are tightly packed.

12 / 20

Why do metals generally have high boiling points compared to non-metals?

A) Metals have strong metallic bonds requiring more energy to break.

B) Non-metals have ionic bonds.

C) Non-metals have larger atomic sizes.

D) Metals contain weaker forces of attraction.

13 / 20

A material is found to be ductile, conducts electricity, and has high melting point. It is most likely:

A) A metalloid

B) A non-metal

C) A noble gas

D) A metal

14 / 20

Which statement best explains why metals are not brittle?

A) They contain no electrons.

B) Their atoms repel each other strongly.

C) Their layers of atoms can slide due to metallic bonding.

D) Their atoms are held by rigid covalent bonds.

15 / 20

Which property is NOT commonly associated with non-metals?

A) Low melting point

B) Brittleness

C) High ductility

D) Poor electrical conductivity

16 / 20

Why are metals suitable for making cooking utensils?

A) They conduct heat efficiently and have high melting points.

B) They are poor conductors of heat.

C) They react strongly with food.

D) They are brittle and break easily.

17 / 20

Which of the following is the best explanation for ductility in metals?

A) Weak intermolecular forces allow elongation

B) Free electrons allow atoms to slide past each other without breaking

C) Strong ionic bonds allow stretching

D) Covalent bonds rearrange under stress

18 / 20

A solid sample does not conduct electricity in solid form but becomes conductive when melted. It is most likely:

A) A noble gas

B) A non-metal

C) An ionic compound (non-metal behavior context)

D) A metal

19 / 20

Which statement best compares malleability in metals and non-metals?

A) Non-metals are more malleable due to covalent bonding.

B) Metals are malleable, while non-metals are brittle.

C) Both are equally malleable.

D) Metals are brittle due to strong bonds.

20 / 20

Which combination of properties correctly identifies a non-metal?

A) Malleability, conductivity, high boiling point

B) High conductivity, ductility, high melting point

C) Low conductivity, brittleness, low melting point

D) High ductility, high density, conductivity

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