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 is an alloy, while diamond is a pure substance.

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

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

D) Graphite contains impurities that allow current flow.

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 due to ions, while non-metals conduct due to electrons.

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

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

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) Brittleness due to strong covalent bonds

C) Ductility due to ionic bonding

D) Elasticity due to weak intermolecular forces

5 / 20

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

A) Conductivity, due to free ions

B) Elasticity, due to ionic lattice structure

C) Ductility, due to non-directional metallic bonding

D) Malleability, due to strong directional bonding

6 / 20

Why are non-metals generally brittle compared to metals?

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

B) Non-metals have weak metallic bonds.

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

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

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

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

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) An alloy

D) A metallic oxide

9 / 20

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

A) Ionic compounds lack charged particles.

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

C) Metals have ions that move freely.

D) Metals dissolve in water to conduct electricity.

10 / 20

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

A) It is shiny and conducts heat efficiently.

B) It has high melting and boiling points.

C) It can be drawn into wires easily.

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 are poor conductors because their atoms are tightly packed.

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

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

D) Both conduct heat equally due to atomic vibrations.

12 / 20

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

A) Non-metals have ionic bonds.

B) Metals contain weaker forces of attraction.

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

D) Non-metals have larger atomic sizes.

13 / 20

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

A) A non-metal

B) A metalloid

C) A noble gas

D) A metal

14 / 20

Which statement best explains why metals are not brittle?

A) Their atoms repel each other strongly.

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

C) They contain no electrons.

D) Their atoms are held by rigid covalent bonds.

15 / 20

Which property is NOT commonly associated with non-metals?

A) Brittleness

B) High ductility

C) Low melting point

D) Poor electrical conductivity

16 / 20

Why are metals suitable for making cooking utensils?

A) They are poor conductors of heat.

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

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) Covalent bonds rearrange under stress

D) Strong ionic bonds allow stretching

18 / 20

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

A) A non-metal

B) A noble gas

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

D) A metal

19 / 20

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

A) Both are equally malleable.

B) Metals are brittle due to strong bonds.

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

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

20 / 20

Which combination of properties correctly identifies a non-metal?

A) High ductility, high density, conductivity

B) High conductivity, ductility, high melting point

C) Malleability, conductivity, high boiling point

D) Low conductivity, brittleness, low melting point

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