Construct the resonance structure for CSO, which has a formal charge of +2 on the central atom and +1 on the oxygen atom.
1 answer:
Answer:
The given condition is proved.
Explanation:
Given that,
Construct the resonance structure for CSO, which has a formal charge of +2 on the central atom and +1 on the oxygen atom.
We need to construct the resonance structure for CSO
The structure shown in figure
According to question,
A formal charge of +2 on the central atom and +1 on the oxygen atom.
Then tha structure shown in figure
The central atom in the structure is sulphur.
We need to calculate the formal charge on sulphur
Using figure,
A formal charge of +2 on the central atom.
This is proved.
Hence, The given condition is proved.
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There are 7 values of ml are allowed for an electron in a 5f subshell namely: -3 -2, -1, 0, +1, +2, +3
<h3>Further explanation</h3>In an atom, there are energy levels in the shell and subshell.This energy level is expressed in terms of electron configurations.
Writing the electron configuration starts from the lowest to the highest subshell's energy level. There are 4 sub-shells in an atom's shell, namely s, p, d, and f. The maximum number of electrons for each subshell is
- s: 2 electrons
- p: 6 electrons
- d: 10 electrons and
- f: 14 electrons
Electron filling in subshells using the following sequence:
1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.
Each sub-shell also has orbitals drawn in the form of a square box in which there are electrons symbolized by half arrows.
Each orbital in an atom consists of 4 quantum numbers
- n is the principal quantum number.
- l is the angular momentum / azimuthal quantum number
- ml, the magnetic quantum number
- ms, the electron-spin quantum number
Value of n: positive integer
value of l: s = 0, p = 1, d = 2, f = 3
ml value: between -l to + l
ms value: +1/2 or -1/2
Determination of electron configurations based on principles:
- 1. Aufbau: Electrons occupy orbitals of the lowest energy level
- 2 Hund: electron fills orbitals with the same energy level
- 3. Pauli: there are no electrons that have 4 equal quantum numbers
So for 5f orbitals, the value of a possible quantum number is
n = 5;
l = 3 (f = 3);
m = -3 -2, -1, 0, +1, +2, +3;
s = + - 1/2
<h3>Learn more</h3>the locations and properties of two electrons
It's sublevel
a possible full set of quantum numbers
Keywords: orbitals, subshells, quantum numbers
Reactions of Ethyl-3-pentenoate with all given reagents are given below.
Reaction with H₂ / Pd:
The non-polar double bond present in Ethyl-3-pentenoate is reduced to saturated chain. This reagent can not reduce the carbonyl group.
Reaction with NaBH₄:
Sodium Borohydride is a weak reducing agent at compared to LiAlH₄. It can only reduce aldehydes and Ketones to corresponding alcohols.
Reaction with LiAlH₄:
Lithium Aluminium hydride is a strong reducing agent. It can reduce all types of carbonyl compounds to corresponding alcohols, But, it can not reduce non-polar double bonds like alkenes and alkynes.
Result:
The correct answer is Option-A (Highlighted RED below).
Reaction with H₂ / Pd:
The non-polar double bond present in Ethyl-3-pentenoate is reduced to saturated chain. This reagent can not reduce the carbonyl group.
Reaction with NaBH₄:
Sodium Borohydride is a weak reducing agent at compared to LiAlH₄. It can only reduce aldehydes and Ketones to corresponding alcohols.
Reaction with LiAlH₄:
Lithium Aluminium hydride is a strong reducing agent. It can reduce all types of carbonyl compounds to corresponding alcohols, But, it can not reduce non-polar double bonds like alkenes and alkynes.
Result:
The correct answer is Option-A (Highlighted RED below).