Question
Both diamond and silicon dioxide have a GIANT COVALENT structure.Which characteristics do they share? [*BE CAREFUL; there are 2 versions of this question but with different answers]
Answer
4.1
(216 Votes)
Opal
Professional · Tutor for 6 years
Answer
### High melting and boiling points, Hardness, Electrical non-conductivity, Insolubility in water
Explanation
## Step 1: Understanding Giant Covalent Structures### Diamond and silicon dioxide both have giant covalent structures, meaning they consist of a vast network of covalently bonded atoms. This structure leads to certain shared characteristics.## Step 2: High Melting and Boiling Points### Due to the strong covalent bonds throughout the structure, both diamond and silicon dioxide have very high melting and boiling points. Breaking these bonds requires a significant amount of energy.## Step 3: Hardness### Both substances are extremely hard. Diamond is the hardest known natural material, and silicon dioxide (in its crystalline form, quartz) is also very hard. This is due to the strong covalent bonds in their giant lattice structures.## Step 4: Electrical Conductivity### Neither diamond nor silicon dioxide conducts electricity in their pure forms. This is because they do not have free electrons or ions that can move and carry charge.## Step 5: Insolubility in Water### Both diamond and silicon dioxide are insoluble in water and most other solvents. The strong covalent bonds do not break easily in the presence of solvents.#