Question

What hybridization is required for central atoms that have a tetrahedral arrangement of electron pairs? A trigonal planar arrangement of electron pairs? A linear arrangement of electron pairs?

Answer 1

Answer:

The required hybridization for a central atom that have:

a tetrahedral arrangement of electron pairs        is  $sp^3$

a trigonal planar arrangement of electron pairs   is  $sp^2$

a linear arrangement of electron pairs                 is   $sp$

Explanation:

From the given information:

The required hybridization for a central atom that have:

a tetrahedral arrangement of electron pairs        is  $sp^3$

a trigonal planar arrangement of electron pairs   is  $sp^2$

a linear arrangement of electron pairs                 is   $sp$

Hybridization is the mixing and blending of two or more pure atomic orbitals ( s, p and d) to forma two or more hybrid atomic orbitals that are identical in shape and energy e. sp ,sp² , sp³, sp³d hybrid orbitals.

Examples:

Tetrahedral

In CH₄ , carbon C is the central atom.

A 2s electron is excited from the ground state of boron 1s²2s²2p² to one of the empty orbitals to 2p to give the excited state 1s²2s²2p³.

In the excited state of carbon, the 2-s orbital can be mixed with the 2p orbitals in three ways : sp³, sp² and sp hybridization. For the formation of four sp³ hybrid orbitals, the 2s orbital are mixed with all the three p orbitals. The four sp³ hybrid orbitals are tetrahedrally arranged with a bond angle of 109.5⁰

Trigonal Planar

In BF₃ , Boron B is the central atom

A 2s electron is excited from the ground state of boron 1s²2s²2p¹ to one of the empty orbitals to 2p. The 2s orbital is then mixed with two orbitals of 2p to form three sp² hybrid orbitals that are trigonal planar arranged in the plane in order to minimize repulsion. They bonds between them form an equal strength and with bond angles of 120⁰

Linear arrangement:

In BeCl₂, Be is the central atom

To provide the unpaired electrons for covalent bonds a 2s electron is excited to a 2p orbital. Thereafter, the two atomic orbitals hybridize to give two identical orbitals called sp hybrid orbitals. The  sigma bond for,ed are equal in bond lengths and form a bond angle of 180°