Question

chemical bonding
jewelers use gems in jewelry because of their appearances and how they can be shaped. the metals used in jewelry have different uses and properties than gems. once you have viewed the investigative phenomenon video and worked on a first draft of a claim - evidence - reasoning exercise to explain the phenomenon you observed, answer the following reflection questions about the physical properties of gems and metals.
1 ccc patterns compare the properties of the gems and metals in the photo.
gems metals
2 sep construct an explanation metals usually bend without breaking, while gems usually break in a specific pattern. what might be happening to the bonds between the atoms in these materials that can explain this difference?

Explanation:

Step1: Compare properties for Q1

Gems are often hard, have high - luster, are brittle, and come in various colors. Metals are malleable, ductile, good conductors of heat and electricity, and usually have a metallic luster.

Step2: Explain bond differences for Q2

In metals, there are metallic bonds. The delocalized electrons in metallic bonds allow the metal ions to slide past one another when a force is applied, enabling bending without breaking. In gems (which often have ionic or covalent bonds), the bonds are more directional. When a force is applied, the bonds break along specific planes due to the fixed arrangement of atoms in the crystal lattice, resulting in a specific breaking pattern.

Answer:

1. Gems: Hard, high - luster, brittle, various colors. Metals: Malleable, ductile, good conductors, metallic luster.
2. In metals, metallic bonds with delocalized electrons allow bending. In gems, directional ionic or covalent bonds lead to specific breaking patterns.