Chemistry 9th Chap 5 : Topic 7 - Maryam Publications

Chemistry Chapter 5 : Topic 7

Bonding in Materials

1 / 15

Engineers commonly use copper wires for electrical transmission in houses and industries. Which explanation best relates this use to the type of bonding present in copper?

A) Copper atoms form ionic bonds that allow ions to move freely through the lattice.

B) Copper atoms are held by metallic bonding where delocalized electrons can move freely and carry electric current.

C) Copper contains weak intermolecular forces that allow electric charge to flow between atoms.

D) Copper atoms form simple covalent molecules that easily release electrons when heated.

2 / 15

Diamond is widely used in cutting tools and drilling equipment even though it is made only of carbon atoms. Which structural feature explains its exceptional hardness?

A) Carbon atoms are connected through weak intermolecular forces.

B) Diamond consists of small carbon molecules packed tightly together.

C) Carbon atoms are arranged in a giant covalent network with strong bonds in all directions.

D) Carbon atoms are held together by metallic bonding.

3 / 15

Graphite is used as a lubricant and also as electrodes in batteries. Which property of its bonding and structure explains these two uses?

A) Graphite forms simple molecules that move easily.

B) Graphite contains ionic bonds that produce free ions.

C) Graphite has metallic bonding similar to iron.

D) Graphite contains layered covalent structures with mobile electrons.

4 / 15

Aluminium is widely used in electrical cables even though it is lighter and less conductive than copper. Which property related to metallic bonding makes aluminium suitable for this purpose?

A) It forms a molecular structure that allows electricity to pass easily.

B) Its covalent bonds weaken when current flows through it.

C) It has mobile electrons and its atoms can slide without breaking bonds easily.

D) Its ions can move through the solid lattice.

5 / 15

Sodium chloride is not used as a conductor of electricity in solid form, but molten sodium chloride can conduct electricity. Which explanation best describes this behavior?

A) In solid NaCl electrons are trapped but become free when melted.

B) Ionic bonds disappear completely during melting.

C) In solid NaCl ions are fixed in a lattice but become mobile when melted.

D) NaCl molecules break into atoms during melting.

6 / 15

A scientist needs a material that can withstand extremely high temperatures without melting. Which type of bonding would most likely provide this property?

A) Simple covalent bonding

B) Giant covalent bonding

C) Metallic bonding

D) Ionic bonding

7 / 15

Plastic materials are often used as electrical insulators in wires and electronic devices. Which bonding characteristic explains this property?

A) Plastics consist of covalent molecules with no free charged particles.

B) Plastics contain metallic bonding that traps electrons.

C) Plastics contain free protons that block electric current.

D) Plastics contain ionic lattices with immobile ions.

8 / 15

Why are metals generally strong yet capable of being shaped into wires or sheets without breaking?

A) Metals contain weak ionic bonds that easily rearrange under pressure.

B) Metals consist of atoms that are not bonded to each other.

C) Metals contain small molecules that can move freely in solid state.

D) Metallic bonds allow layers of atoms to slide while maintaining attraction between ions and electrons.

9 / 15

A material is required for constructing cooking utensils because it must conduct heat efficiently. Which bonding type best explains the suitability of metals for this purpose?

A) Ionic bonding with mobile ions

B) Covalent bonding with strong directional bonds

C) Metallic bonding with mobile delocalized electrons

D) Molecular bonding with weak intermolecular forces

10 / 15

Silicon dioxide is widely used in glass and ceramics due to its hardness and resistance to heat. Which structural feature is responsible for these properties?

A) Formation of ionic bonds between silicon and oxygen ions

B) A giant covalent network of atoms connected by strong bonds

C) Presence of weak intermolecular forces between molecules

D) Metallic bonding with delocalized electrons

11 / 15

Why are ionic compounds generally unsuitable for making electrical wires even though they contain charged particles?

A) Their ions are too small to conduct electricity.

B) Their ions are fixed in position in solid crystals and cannot move.

C) They contain covalent bonds instead of ionic bonds.

D) They break down into atoms when current passes through them.

12 / 15

Steel is widely used in building structures due to its strength. Which bonding explanation best describes this property?

A) Steel consists of simple molecules held together by weak forces.

B) Steel contains ionic bonds that allow ions to move freely.

C) Steel forms a giant covalent network similar to diamond.

D) Metallic bonding produces strong attraction between positive ions and delocalized electrons.

13 / 15

Why are covalent molecular substances like methane or carbon dioxide rarely used as construction materials?

A) Their molecules repel each other strongly.

B) They form ionic lattices that dissolve easily.

C) They contain metallic bonds that break easily.

D) They contain weak intermolecular forces that cannot provide strong structures.

14 / 15

Which property makes graphite suitable for making electrodes in electrochemical cells?

A) It forms molecules that conduct electricity when heated.

B) It contains ionic bonds that release ions in circuits.

C) It has free electrons that can move along its layers.

D) It has metallic ions moving through its structure.

15 / 15

A material used in aircraft construction must be lightweight, strong, and resistant to corrosion. Which bonding type explains the suitability of metals such as aluminium for this application?

A) Hydrogen bonding between atoms

B) Covalent molecular bonding with weak forces

C) Ionic bonding with strong electrostatic attraction

D) Metallic bonding allowing strength and flexibility

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