A electronegativity difference of about 2 between the elements is considered a prerequisite for an ionic bond.
Figure 2 is arbitrary and different authorities have slightly different views.
Chemical bonding cannot be solely explained with the concept of electronegativity. According to generality, it is said that a particular compound has a principal ionic character if it exceeds the electronegativity difference of 1.7 in Pauling's scale.
Calcium is a metal with an electronegativity of 1.0 and oxygen is a nonmetal with an electronegativity of 3.5. The electronegativity difference is 2.5, and anything over 1.7 indicates an IONIC BOND.
To calculate the the Energetics of Covalent Bonding and the Ionic character, you need to take into accot the difference in electronegativity of two atoms: Δχ = χB − χA.
Non polar covalent bonding. (Both atoms have the same electronegativity)
Sodium hydroxide is an ionic compound which disassociates in to Na+ and OH- ions in solution.
Not sure about your examples but electronegativity variance is a good rule of thumb for deciding ionic from covalent bonds. Electronegativity variance less than 1.4, generally much less, indicates a covalent bonding. Electronegativity variance greater than 1.4 indicates ionic bonding.
Chemical bonding cannot be solely explained with the concept of electronegativity. According to generality, it is said that a particular compound has a principal ionic character if it exceeds the electronegativity difference of 1.7 in Pauling's scale.
Calcium is a metal with an electronegativity of 1.0 and oxygen is a nonmetal with an electronegativity of 3.5. The electronegativity difference is 2.5, and anything over 1.7 indicates an IONIC BOND.
If this difference is under 2 the bond is covalent; if the difference is over 2 the bond is ionic.
To calculate the the Energetics of Covalent Bonding and the Ionic character, you need to take into accot the difference in electronegativity of two atoms: Δχ = χB − χA.
The electronegativity difference between the bonding atoms is concerned to determine it ionic behaviour.
Non polar covalent bonding. (Both atoms have the same electronegativity)
Sodium hydroxide is an ionic compound which disassociates in to Na+ and OH- ions in solution.
The difference in electronegativity between the atoms determines the nature of the bond. The larger the electronegativiity difference the more ionic character it will have, this ranges from polar covalent through to ionic bonding.In valence bond terms the ionic resonance forms become more important and make a bigger contribution as the electronegativity difference increases. The contribution of covalent bonding never really disappears.
To say that bonding is on a continuum means that the type of bonding changes gradually as the difference in electronegativity between atoms increases. There is no sharp distinction between polar covalent and ionic bonds.
CdS is about 15% ionic and the balance covalent, based on an equation that curve fits measured ionic character of compounds versus difference in electronegativity.
Ammonia is a covalent compound. It is a compound of two nonmetals, nitrogen and hydrogen, so the difference in electronegativity is not great enough to cause ionic bonding.