Crystalline solids

Which is an example of an ionic crystal?

• Quartz
• NaCl
• Ammonia
• Iron

Tags

NGSS.HS-PS1-3

Which is an example of an covalent network crystal?

• Quartz
• NaCl
• Ammonia
• Iron

What property gives metallic solids the ability to conduct electricity well, but not covalent network solids?

• Electrons in metallic solids are strongly bound in place
• Electrons in covalent network solids are freely moving around
• Covalent network solids are not bound to other atoms
• Metallic solids have many electrons that are not bound and can move about the solid

Tags

NGSS.HS-PS1-3

NGSS.HS-PS2-6

Which type of solid is hard, brittle, and nonconducting unless dissolved in H₂O?

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

Tags

NGSS.HS-PS1-3

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 strong covalent bonds between neighboring atoms?

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

Tags

NGSS.HS-PS2-6

Which is an example of an covalent molecular crystal?

• Quartz
• NaCl
• Ammonia
• Iron

Tags

NGSS.HS-PS1-3

Which is an example of an metallic crystal?

• Quartz
• NaCl
• Ammonia
• Iron

Solids have many different properties. ___________ solids are known for their ability to be flattened into a sheet, stretched into a wire, and to conduct energy well.

• Molecular

• Metallic

• Covalent Network

• Ionic

Which statement is true about the properties of solids?

• Metallic solids have a high melting point.

• Network solids are generally not soluble in water.

• Molecular solids do not dissolve easily in water.

• All ionic solids are similar in density.