N2 = covalent
H2O = polar covalent bond
MgS = ionic bond
NaCl = ionic bond
no
MgF2 and NaCl are ionic. NH3 and H2O contain polar covalent bonds. N2 contains non polar covalent bond.
NH3 contains covalent bond
NaCl is ionic.
Ionic compounds generally are more soluble in polar solvents than in non-polar. Strictly polar compound is a term applied to compounds with a polar covalent bond
no
MgF2 and NaCl are ionic. NH3 and H2O contain polar covalent bonds. N2 contains non polar covalent bond.
NH3 contains covalent bond
NaCl is ionic.
No. It contains non-polar covalent bond.
Ionic compounds generally are more soluble in polar solvents than in non-polar. Strictly polar compound is a term applied to compounds with a 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.
Due to the polarity of water compounds that dissolve best in water contain polar bonds. It is a covalent bond between two atoms where the electrons forming the bond are unequally distributed.
H2 contains the strongest polar covalent bond.
There is no such compound as CH2OH. The compounds CH2O (formaldehyde) and CH3OH (methanol) do exist. Both contain carbon and are miscible in water for largely the same reason. Formaldehyde contains a highly polar C-O double bond while methanol contains both a polar C-O bond and a polar O-H bond. Polar bonds tend to make molecules water soluble.
Generally a polar molecules (as salts) have an ionic bond.
To classify a bond as polar or covalent, you must first find the Electronegativity difference. The electronegativity of Na is 0.93 and Cl is 3.16. Therefore we find the electronegativity difference by subtracting: 3.16 - 0.93= 2.23. Therefore NaCl is an ionic bond. For electronegativity differences >1.7, the bond is ionic. For electronegativity differences between 0.4-1.7, the bond is polar covalent For electronegativity differences < 0.4, the bond is non-polar covalent.