Can you explain the forces that hold the bonds (ionic metallic and covalent) together?

Answer 1

Pretty much all chemical bonds are held together because of the electric force. Positive charges are attracted to negative charges and negative charges are repelled from each other.

It is because of that latter effect that all electrons don't just clump up next to the nucleus of an atom - they hate each other so they held away from the nucleus in a pattern of orbitals. This also exposes them to attraction to completely different nuclei. When one is pulled away completely, you end up with an ion or two.

But when two nuclei end up sharing attraction to one or more electrons, you get a bond.

Ionic bonds result from the overall attraction of a cation to an anion. Covalent bonds result from sharing of specific electrons in specific shared orbitals. Metallic bonds result from a sharing of a cloud of easily mobile electrons across generally non-specific directions.

Hope that helps!

Answer 2

a) Xenon has an more desirable atomic mass, meaning atoms of xenon have a greater advantageous allure to one yet another (van der Waals forces are proportional to atomic or molecular mass) b) Copper chloride is an ionic molecule, the place electrons are separated. steel copper is in a feeling atoms swimming in a sea of electrons. c) CO2 molecules are discrete, fascinated in one yet another by utilising brought about dipoles. SiO2 is a community stable, the place each atom is bonded to countless others. d) NF3 has a lone pair of electrons on the nitrogen, making the molecule a trigonal pyramid and giving it a dipole 2d. BF3 is electron-poor, with out lone pair on the B. as a consequence, it relatively is trigonal planar and non-polar.