Question: That “DIAMOND” on her finger is: i) an allotrope of carbon ii) a three-dimensional network of carbon atoms iii) has properties not dependent on London Forces iv) very hard with a high melting point and low vapor pressure v) the only reason she puts up with your ____. A) none of the above is true B) only i, iii, and iv are true C) only ii, iii, and iv are true D) only iv is true E) all of the above are true. Face facts, dude.

Q: Which of the following correctly describes the influence of intermolecular forces on the properties…

A: Intermolecular interactions between individual molecules in a chemical entities are important…

Q: Indicate the strongest force holding the crystals together in CH3OH and K2S.

A: The force of attraction present between the molecules of a substance is known as intermolecular…

Q: Question 9 options:  a  b c d 1. metallic 2. molecular 3. covalent network 4. ionic

A: These are the type of bonding in compounds or an element present in the field of chemistry.

Crystal Structures

Solids are present all around us. They have different properties and applications. Diamond and graphite are two well-known solids. Diamond is the hardest material in the world and is used in making jewelry. Graphite on the other hand is soft. The lead of your pencil is graphite. Why are they so different in appearance and properties despite the fact they are chemically the same? Both are allotropes of carbon. The answer lies in the structure, the way constituent particles are arranged in the solids.