Properties of Solids | Chemistry Quiz

Properties of Solids Quiz

Test your Chemistry knowledge with these challenging 17 multiple-choice questions on solids. Covering crystalline structures, lattice energy, and more.

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1. Amorphous solids are characterized by:

Long-range order of atoms/molecules.

Sharp melting points.

Isotropic properties.

Distinct cleavage planes.

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2. Crystalline solids have:

Irregular shapes.

A range of melting temperatures.

Distinct geometrical shapes.

No definite arrangement of particles.

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3. Cleavage planes in crystals are:

Planes of weakness along which a crystal tends to break.

Irregular fractures within a crystal.

Surfaces created by melting the crystal.

External faces of the crystal.

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4. The external shape of a crystal is known as its:

Habit

Polymorphism

Isomorphism

Allotropy

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5. Anisotropy refers to:

The property of a substance to exist in more than one crystalline form.

The variation of physical properties with direction within a crystal.

The ability of two different substances to crystallize in the same form.

The existence of an element in different forms in the same physical state.

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6. Isomorphism is the phenomenon where:

Two or more substances have the same crystal structure.

A single substance exists in different crystalline forms.

A substance changes its crystalline form with temperature.

An element exists in different forms in the same physical state.

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7. The low density of ice is due to:

Strong covalent bonds between water molecules.

Hydrogen bonding creating an open, tetrahedral structure.

Weak van der Waals forces between water molecules.

The small size of water molecules.

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8. The high heat of fusion of ice is due to:

The breaking of strong covalent bonds.

The breaking of hydrogen bonds.

The expansion of the crystal lattice upon melting.

The high kinetic energy of water molecules in ice.

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9. Molecular solids are held together by:

Strong covalent bonds.

Metallic bonds.

Weak intermolecular forces.

Ionic bonds.

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10. Metallic solids are characterized by:

Localized electrons.

A sea of delocalized electrons.

Strong ionic bonds.

Weak intermolecular forces.

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11. The unit cell of NaCl is:

Simple cubic

Body-centered cubic

Face-centered cubic

Hexagonal close-packed

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12. The unit cell is significant because:

It represents the smallest repeating unit of the crystal lattice.

It determines the color of the crystal.

It dictates the melting point of the crystal.

It determines the density of the crystal.

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13. Which is NOT a common type of packing arrangement in solids?

Simple cubic

Body-centered cubic

Face-centered cubic

Rhombohedral packing

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14. In simple cubic packing, the coordination number is:

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15. Which solid has the highest melting point generally?

Molecular solids

Metallic solids

Ionic solids

Covalent network solids

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16. Which solid is a good conductor of electricity?

Ionic solids in solid state

Molecular solids

Metallic solids

Covalent network solids

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17. Which of the following solids is likely to sublime readily?

Sodium chloride

Ice

Iodine

Diamond

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The topic included in the quiz are:

Lattice Energy
General Properties of Solids (diffusion, compression, expansion, molecular motion, intermolecular forces, kinetic energy)
Amorphous vs. Crystalline Solids
Properties of Crystalline Solids (geometric shape, melting point, cleavage planes, crystal habit, crystal growth, anisotropy, symmetry, isomorphism, polymorphism, allotropy, transition temperature)
Allotropes of Oxygen and Sulfur
Factors Affecting Ionic Crystal Shape
Properties of Ice (low density, high heat of fusion)
Molecular Solids
Metallic Solids
Unit Cell and Crystal Shape (using NaCl as an example)
Packing Arrangements in Solids
Comparison of Ionic, Covalent, Molecular, and Metallic Crystalline Solids