In an ionic bond electrons are transferred and the bond is due to electrostatic attrcation between oppositely charged ions. in a covalent bond the electrons are shared .
Compounds with covalent bonds form molecules. Compounds with ionic bonds form ionic lattices.
Molecules can be ionic OR covalent, but not both. PbI2 (lead iodine), however, is ionic.
Covalent. The electronegativity difference between N and O is small.
It is covalent due to the small electronegativity difference between hydrogen and sulfur.
MgCl2 is an ionic compound. there is a large difference in electronegativity between Mg and Cl.
Covalent compounds are more flammable when compared to ionic compounds.Ionic compounds are more soluble in water than covalent compounds.for more go to: difference between . net
Compounds with covalent bonds form molecules. Compounds with ionic bonds form ionic lattices.
Molecules can be ionic OR covalent, but not both. PbI2 (lead iodine), however, is ionic.
Covalent. The electronegativity difference between N and O is small.
It is covalent due to the small electronegativity difference between hydrogen and sulfur.
MgCl2 is an ionic compound. there is a large difference in electronegativity between Mg and Cl.
Ionic bonds are based on the electrostatic attraction of ions; covalent bonds are based on the sharing of electrons between two atoms.
If the electronegativity difference between two atoms is over 1.7, then ionic bond is formed and if it is below 1.7, then covalent bond is formed.
The major difference between the two is: - Ionic bonds occur between one metal and one non-metal (such as sodium and oxygen) - Covalent bonds occur between two non-metals.
It represents the boundary between what is considered to be an ionic or a covalent bond.
P2O5 is covalent compound as the difference in electronegativity between P and O is below 1.7
PCl3 has covalent bonds. The difference in electronegativity between P and Cl is not large enough. The electronegativity of P is 2.19 and for Cl it is 3.16, and so the difference is less than one, making it a polar-covalent bond.