Explain how the properties of ionic and covalent bonds vary?

Answer 1

I'm not totally sure how this helps, but I'll give it my best shot.

Ionic and covalent bonds are two different ways that different atoms can be held together in a molecule. As you probably know, most elements have a specific charge relating to their number of valance electrons and, subsequently, their position on the periodic table. Ionic bonds are held together by a fusion of these charges. All atoms naturally want to gain 8 electrons in their outer shell, making their charge zero. Because of this, they will attract eachother based on their charges. For example, hydrogen has a charge of -1 while chlorine has a charge of +1. These two are attracted and become HCl, hydrochloric acid. Because they involve charges, the bonds usually involve a metal and a non-metal.

Covalent bonds are a little more tricky. Like ionic bonds, atoms want to complete their outer shell by bonding with other atoms. If the charges do not equal zero, they come together and "share" electrons - the move closer together so they each have 8 electrons in their shell. Covalent bonds are stronger than ionic bonds and hold together most of our polyatomic ions - NO3-, CO3^2-. etc. Covalently bonded molecules can have an overall charge. I hope this helps.

Answer 2

Ionic bonds result from the transfer of electrons between atoms, leading to the formation of ions with opposite charges that are held together by electrostatic forces. Covalent bonds, on the other hand, involve the sharing of electrons between atoms to achieve a more stable electron configuration. Ionic bonds tend to be stronger than covalent bonds due to the attraction between ions, while covalent bonds can vary in strength depending on the atoms involved in the bond.