Which among the following is colourless?a)Sc2+b)Zn2+c)Ti3+d)V3+Correct answer is option 'B'. Can you explain this answer?

Question

Answer

Zn²⁺ has completely filled d-orbitals and there are no vacant d-orbitals for the transition of electrons, hence it is colourless.

Answer

Zn2+ because of no unpaired electron

Answer

Colour can be shown by d block elements only if d-d transition is possible... Zn+2 has fully filled 3d orbital.. So no d-d transition so no colour

Answer

Since Zn2+ is a d10 ion, it does not absorb visible light even though the “d orbital” splittings are correct for absorbing visible wavelengths. Meaning that all d orbitals are full therefore there is no space for the electrons to move resulting in a colorless compound thanks!!!!!

Answer

Mostly Diamagnetic Elements are Colourless ___
[ Diamagnetic elements are those elements which have paired electrons only ]
A) Sc^2+ ( E. C. ==> [ Ar ] 4s^0 ,,,3d^1 )_________________
B) Zn^2+ ( E. C. ==> [ Ar ] 4s^0 ,,,,3d^10 {5-pairs of e. })____________
C) Ti ^3+ ( E. C. ==> [ Ar] 4s^0 ,,,3d^1 ) ________
D) V^3+ ( E. C.==> [ Ar ] 4s^0 ,,, 3d^2 {but are unpaired }) .................................
From above electronic configuration u can observe that only Zn^2+ have all paired electrons ( no any unpaired electron as in other elements) THEREFORE( B) OPTION IS CORRECT _______________
I hope this will help u to clear out ur doubt..

Answer

Answer:

Introduction:
In this question, we are asked to identify the compound that is colorless among the given options. To determine the correct answer, we need to understand the factors that contribute to the color of compounds.

Factors affecting the color of compounds:
The color of a compound is primarily determined by the presence of d-orbitals in the metal ions. When electrons in these d-orbitals absorb energy from light, they undergo transitions to higher energy levels. The energy absorbed corresponds to a specific wavelength of light, and the remaining light is transmitted or reflected, giving the compound its color.

Explanation:
Let's analyze each option and determine which one is colorless:

a) Sc2 (Scandium):
Scandium (Sc) is a transition metal with atomic number 21. It has an electronic configuration of [Ar] 3d1 4s2. Scandium compounds are known to be colorless. However, the given option 'Sc2' does not exist as a stable compound. Therefore, we can eliminate this option.

b) Zn2 (Zinc):
Zinc (Zn) is also a transition metal with atomic number 30. It has an electronic configuration of [Ar] 3d10 4s2. Zinc compounds are well known for their colorless nature. Therefore, option 'Zn2' is the correct answer as it represents a stable compound that is colorless.

c) Ti3 (Titanium):
Titanium (Ti) is another transition metal with atomic number 22. It has an electronic configuration of [Ar] 3d2 4s2. While titanium compounds can exhibit different colors, the given option 'Ti3' does not represent a stable compound. Hence, we can eliminate this option.

d) V3 (Vanadium):
Vanadium (V) is a transition metal with atomic number 23. It has an electronic configuration of [Ar] 3d3 4s2. Vanadium compounds often exhibit various colors, such as green, blue, or yellow. However, the given option 'V3' does not represent a stable compound. Therefore, we can eliminate this option.

Conclusion:
Among the given options, the correct answer is option 'B' (Zn2). Zinc compounds are known to be colorless, making it the only colorless compound among the given options.

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