H2O. Due to difference in electronegativity.
O2 is covalent, NaCl and KI are ionic, CH4 is usually considered to be simply covalent as the electronegatiicty difference is small.
N2 = covalentH2O = polar covalent bondMgS = ionic bondNaCl = ionic bond
NaCL is what compound
MgF2 and NaCl are ionic. NH3 and H2O contain polar covalent bonds. N2 contains non polar covalent bond.
no salt (NaCl) is an ionic compound
NH3 contains covalent bond
N2 = covalentH2O = polar covalent bondMgS = ionic bondNaCl = ionic bond
NaCL is what compound
MgF2 and NaCl are ionic. NH3 and H2O contain polar covalent bonds. N2 contains non polar covalent bond.
NaCl is an ionic compound, and these terms are generally reserved for covalent compounds. But by definition, all ionic compounds are polar.
no salt (NaCl) is an ionic compound
NH3 contains covalent bond
Salts do not usually contain covalent bonds e.g. NaCl doesn't.
no
NaCl is ionic, and polar/non-polar usually refers to covalent bonds. So, while it is polar in a sense (there are + and - parts) it is really ionic. It is, however, soluble in polar liquids, such a water.
Ionic bonds have stronger bonds than covalent but are easier to separate simply because Ionic Compounds are POLAR molecules. There electronegativity different between the Metal and Non metal is higher than 1.7 (Extremely polar). This means putting, example NaCl (Salt), in water, will easily dissolve the NaCl into the cation and anion. Hopefully this helps.
Because sodium chloride and water are polar compounds.
Miscible is not the correct word - probable you think to soluble; and because NaCl is a polar compound it is not soluble in these organic compounds (the formula C7H14 correspond to three compounds).