Question

What orbitals are used to form each bond in methanol, ch3oh? be sure to answer all parts?

Answer 1

Orbitals that play a role in bonding to C atoms are sp³ hybridization orbitals, while O atoms, the orbitals used for binding are 2p orbitals

and the H atom, the orbitals used are 1s

Further explanation

Hybridization is a term used in the formation of chemical bonds or the determination of the geometric shape of a molecule. Hybridization is generally used to describe molecules that have C, N and O atoms

In the formation of bonds between 2 atoms, the valence electrons of the two atoms will play a role in the filling of empty orbitals that are shared and filled with electrons from both atoms.

Hybridization itself is merging of orbitals that have different energy levels so that it is expected to explain the resulting geometric shape according to the length, angle or bond energy

In the compound CH₃OH (methanol) which is one of the alcohols there are 3 atoms in it namely C, H, and O

The electron configurations of each of these atoms are:

C: 1s² 2s² 2p2²

H: 1s1¹

O: 1s² 2s² 2p⁴

In an atom, C hybridization occurs where the electrons in the 2s orbitals are excited into the 2p orbitals to form sp³ hybridization orbitals so that 4 single electrons can bind to other atoms

Whereas on the O atom there are 2 single electrons in the 2p orbitals so that they can bind with 2 other electron atoms to form bonds

Whereas the H atom, there is 1 single electron in 1s orbitals that can bind to 1 electron from another atom

Learn more

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Keywords: the electron configuration, orbitals, hybridization

Answer 2

All C-H bonds are formed from C $\boxed{s{p^3}}$ to H $\boxed{1s}$.

The C-O bond is formed from C   to O $\boxed{2p}$.

The O-H bond is formed from O $\boxed{2p}$ to $\boxed{1s}$.

Further explanation:

Hybridization

The process that involves the combination of atomic orbitals of the same atom to form an equal number of hybrid orbitals having the same energy and same shape is known as hybridization. Hybrid orbitals are supposed to be the mixtures of atomic orbitals.

There are three atoms, namely C, H and O that are involved in the formation of ${\text{C}}{{\text{H}}_3}{\text{OH}}$. The atomic number of carbon is 6 so it has a configuration of $1{s^2}2{s^2}2{p^2}$. The atomic number of hydrogen is 1 so its electronic configuration is $1{s^1}$. The atomic number of oxygen is 8 and its configuration is $1{s^2}2{s^2}2{p^4}$.

One of the 2s electrons in carbon atom gets excited to the 2p orbital and one 2s and three 2p orbitals combine with each other to form four   hybrid orbitals. So the hybridization of carbon is $s{p^3}$.

All C-H bonds are formed from $s{p^3}$ hybrid orbitals of C to 1s orbital of H. So the orbitals involved in C-H bonds are $s{p^3}$ hybrid orbitals of carbon and 1s orbitals of hydrogen.

The C-O bond is formed from $s{p^3}$ hybrid orbitals of C to 2p orbital of O. So the orbitals involved in C-O bonds are $s{p^3}$ hybrid orbitals of carbon and 2p orbital of oxygen.

The O-H bond is formed from 2p orbitals of O to the 1s orbital of H. So the atomic orbitals involved in O-H bond are 2p orbital of oxygen and 1s orbital of hydrogen.

Learn more:

1. Molecular shape around the central atoms in the amino acid glycine: brainly.com/question/4341225
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Answer details:

Grade: Senior School

Chapter: Covalent bonding and molecular structure

Subject: Chemistry

Keywords: hybridization, CH3OH, C, H, O, sp3, 1s, 2p, orbitals, C-H bond, O-H bond, C-O bond.