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28` while H-N-H bond angle in NH3 is 107? ,though both carbon and nitrogen are sp3 hybridized . Because of the presence of lone pair on N; there is a lone pair – bond pair repulsion between electrons. Hence it decreases the bond angle from 109◦ angle to 107 ◦ as bond angle.

The H—C—H bond angle in methane is the tetrahedral angle, 109.5°. This angle is obtained when all four pairs of outer electrons repel each other equally. The bond angles in ammonia and in water are less than 109.5° because of the stronger repulsion by their lone pairs of electrons.

So, the geometry of the methane is tetrahedral. So, the bond angles in methane are of 109.5∘ . As all surrounding atoms are hydrogen so, all bond angles in methane is H-C-H angles. So, all bond angles are the same.

It turns out that methane is tetrahedral, with 4 equal bond angles of 109.5° and 4 equal bond lengths, and no dipole moment.

It isn’t! Although it has a fluorine which you may associate with hydrogen bonding, there isn’t a hydrogen attached directly to it.) van der Waals dispersion forces (Although each C-H bond has a slight dipole, overall these cancel each other out to give no permanent dipole on the molecule as a whole.)

In F2 the bonding is pure covalent, with the bonding electrons shared equally between the two fluorine atoms.

Explanation: Ionic bonds are the strongest type of bonds, followed by covalent bonds, hydrogen bonds, and lastly, van Der waals forces.

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The London Dispersion Forces in I2 are strong enough to keep I2 solid at room temperature; where as, F2 is a gas at room temperature. In general London Dispersion Forces are considered to be the weakest intermolecular force; however, London Dispersion Forces become very important for larger molecules.

hydrogen- bonding interaction