Table of Contents
What is the bond angle present in phenol?
Lone pair – Lone pair > > Lone pair – Bond pair > Bond pair – Bond pair. In ideal case when there’s no lone pair present, the angle of sp3 hybridized (tetrahedral geometry) is 109°28′. Hope this helps.
Why is the bond angle of a tetrahedral 109.5 and not 90?
methane consists of four bonded pairs, i.e 4 C-H bonds. So as to minimize repulsion, the molecule adopts a tetrahedral shape, hence bond angle becomes 109.5. with bond angle of 90, the molecule would not be very stable.
What is the angle between any of the bonds in a tetrahedral carbon?
In a tetrahedral molecular geometry, a central atom is located at the center with four substituents that are located at the corners of a tetrahedron. The bond angles are cos−1(−1⁄3) = 109.4712206… ° ≈ 109.5° when all four substituents are the same, as in methane (CH 4) as well as its heavier analogues.
Why is methane tetrahedral?
The four C-H bonds in methane are held at an angle of 109∘-28′ because this is the only angle in space at which repuslions between the four shared pairs of electrons is minimum. That is why methane assumes tetrahedral geometry.
Which of the following is not a correct reason for the C-O bond length in phenol to be less than that in methanol?
The best explanation: The two lone pairs of electrons of oxygen are present in OH groups of both phenol and methanol and has an effect on the C-O-H bond angle and not the C-O bond length.
Why phenols are more acidic than aliphatic alcohols?
In phenoxide ion the negative charge is delocalized within the ring structure which makes it more stable than the aliphatic alcohols. In aliphatic alcohols there is no such delocalization stabilization. Therefore, phenols are more acidic and the resulting phenoxide ion is stabilized because of resonance.
What are the factors affecting bond angle?
(i) Repulsion between atoms or groups attached to the central atom may increase or decrease the bond angle. (ii) In hybridisation as the s character of the s hybrid bond increases, the bond angle increases. (iii) By increasing lone pair of electron, bond angle decreases approximately by 2.5\%.