Question

Water (${H_2}O$) is polar, whereas $Be{F_2}$, is not because:
A.electronegativity of $F$is greater than that of $O$
B.${H_2}O$ involves H-bonding ,whereas $Be{F_2}$ is a discrete molecule
C.${H_2}O$ is angular and $Be{F_2}$ is linear
D.${H_2}O$ is linear and $Be{F_2}$ is angular

Answer 1

Hint: Polarity is defined as a separation of electric charge which leads a molecule or its chemical groups to have an electric dipole moment and also with a negatively charged end and a positively charged end. Polar molecules can contain polar bonds because of a difference in electronegativity between the bonded atoms.

Complete step by step solution:
If we first check about $Be{F_2}$, it has the dipole moment equal to zero because $Be{F_2}$ is linear in the shape. Whereas if we see ${H_2}O$ shape, it is V-shaped hence its net dipole moment which is produced due to the bond moment and the lone pair moment.
Therefore ${H_2}O$ is polar whereas $Be{F_2}$ is not.

So the correct answer is C.

Additional information:
Not every molecule pulls the electrons with a similar power towards them. The measure of pulling an iota on the electrons is known as its electronegativity. Iotas which have high electronegativities, for example, fluorine, oxygen, and nitrogen: apply a more bulging or pulling draw on electrons than the particles which have lower electronegativities. For example, salt metals and soluble earth metals which have low electro-negativity. In a bond, this stimulates inconsistent sharing of electrons between the iotas. As electrons will be moved closer to the particle having higher electronegativity.
Since electrons have a negative charge on it, the uneven sharing of electrons inside a bond encourages the development of an electric dipole which is a detachment of positive and negative electric charge. Then the measure of charge isolated in such dipoles is typically more uncertain than a key charge, these are known as halfway charges which are signified as \[\delta + \](delta in addition to) and \[\delta - \] (delta short). These images were offered by Sir Christopher In gold and Dr. Edith Hilda (Usher wood) in 1926. The security dipole second is calculated by duplicating the measure of charge isolated and the separation between the charges.

Note: Polar molecules can contain polar bonds due to a difference in the electronegativity between the bonded atoms. A polar molecule with two or more polar bonds has a geometry which is asymmetric in at least one of the directions, so that the bond dipoles do not cancel each other.