Quiz Crystalline Solids

Define crystalline solid

• A solid in which the atoms CANNOT be changed.

• A regular repeating, three-dimensional structure of atoms that form a crystal lattice.

• A pure solid that can conduct electricity.

• A pure solid that has a defined melting and boiling point.

One major difference between crystalline and amorphous solids is that

• crystalline solids have a true melting point, while amorphous solids do not.

• amorphous solids have a lattice structure.

• amorphous solids always behave consistently and uniformly.

• crystalline solids break unpredictably and can produce curved fragments.

Which is an example of an ionic crystal?

• Graphite (lead in a lead pencil)

• Sodium Chloride (NaCl)

• Ammonia (NH₃)

• Iron (Fe)

Tags

NGSS.HS-PS1-3

Which type of solid is hard, brittle, has a high melting point, but ONLY conducts electricity if dissolved in H₂O or melted.

• Ionic Crystal

• Covalent Molecular Crystal

• Metallic Crystal

• Covalent Network Crystal

Which type of solid typically has the lowest melting point of the four types of crystals?

• Ionic Crystal
• Covalent Molecular Crystal
• Metallic Crystal
• Covalent Network Crystal

Which type of solid has very strong covalent bonds between neighboring atoms?

• Ionic Crystal

• Covalent Molecular Crystal

• Metallic Crystal

• Covalent Network Crystal

Identify the covalent molecular solid crystal.

• Diamond (Carbon)

• Sodium chloride (NaCl)

• Ammonia (NH₃)

• Iron (Fe)

Identify the metallic crystal.

• Graphite (carbon)

• NaCl

• Ammonia (NH₃)

• Iron (Fe)

High melting points, good conductors of electricity in the solid state, does not dissolve in water.

• Ionic

• Metallic

• Covalent Network

• Covalent Molecular

Tags

NGSS.HS-PS1-3

Very hard, very high melting point, nonconductors of electricity, low density.

• Ionic

• Metallic

• Covalent Network

• Covalent Molecular

Tags

NGSS.HS-PS1-3