Question

If a covalent bond were to be formed between a nitrogen atom (electronegativity 3.0) and hydrogen atom (electronegativity 2.2), which of the following statements would best describe such a bond? *

1 point

Non-polar covalent

Polar covalent where the hydrogen atoms carried the partial negative charge

Polar covalent where the nitrogen atom carried the partial negative charge

Polar covalent where the nitrogen atom carried the partial positive charge​

Answer 1

Answer:

dont know..........???

Answer 2

Answer:

Polar covalent where the nitrogen atom carried the partial negative charge.

Explanation:

• The electrons in a covalent bond are not always shared equally between the two bonded atoms. Unless a bond connects two atoms of the same element, as in H2, there will always be one atom that attracts the electrons in the bond more  than the others, as in HCl. Covalent bonds with equal electron sharing and are called a non-polar covalent bond.
• Covalent bonds with unequal distribution of electrons, such as , are called  polar covalent bonds. The distribution of electron density in  polar bonds is uneven. This  electron density imbalance results in a  partial negative charge (represented by δ-) on one side of the bond (N) and a partial positive charge (represented by δ+) on the other side of the bond (H). is accumulated.
• An electric dipole is generated due to charge separation  in a polar covalent bond.
• If the electronegativity difference is 0.4 to 1.8 it is called polar covalent.

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