Atomic Structure Test

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Atomic Structure Test - 11

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Weekly Quiz Competition

Question 1
1 / -0

Which of the following statements regarding quantum numbers is not correct?

A
Quantum numbers n, l, m and s are needed to describe an electron in an atom completely.

B
Quantum numbers n, l, m and s are obtained by solving the Schrödinger wave equation.

C
A sub-shell in an atom can be designated with two quantum numbers n and l.

D
The maximum value of l is equal to n – 1 and that of m is ± l.

Solution

The quantum number s is not the outcome of the solution of Schrödinger equation.
The spin quantum number was introduced by Pauli.
Question 2
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Which of the following is a correct statement in regard to the Aufbau principle?

A
(n – 1)d subshell is always lower in energy than ns subshell.

B
(n – 1)d subshell always has more energy than ns subshell.

C
5d is lower in energy than 4f.

D
5f is lower in energy than 7s.

Solution

Energy increases with increase in the value of n + l.
For (n - 1)d subshell, the n + l value is n - 1 + 2 = n + 1
For the ns subshell, the n + l value is n + 0 = n
Question 3
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The following question has four choices, out of which ONLY ONE is correct.

Two electrons in the same atomic orbital can be distinguished by their

A
principal quantum number

B
azimuthal quantum number

C
magnetic quantum number

D
spin quantum number

Solution

Two electrons in the same atomic orbital can be distinguished by their spin quantum number because two electrons in the same orbital have different spin quantum numbers.
Question 4
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Which of the following electronic configurations is not theoretically possible?

A
2d⁵

B
3p⁶

C
4s¹

D
4f¹²

Solution

For 2d orbital, l > n, which is not allowed.
Question 5
1 / -0

The maximum number of electrons in a subshell is given by the expression

A
4l - 2

B
4l + 2

C
2l + 1

D
2n²

Solution

The maximum number of electrons in a subshell is given by the expression 4l + 2.
Example:
For the s sub-shell, l = 0
Number of electrons it can accommodate = 4 × 0 + 2 = 2
For the p sub-shell, l = 1
Number of electrons it can accommodate = 4 × 1 + 2 = 6

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Atomic Structure Test - 11

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Atomic Structure Test - 11

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Question 1

Quantum numbers n, l, m and s are needed to describe an electron in an atom completely.

Quantum numbers n, l, m and s are obtained by solving the Schrödinger wave equation.

A sub-shell in an atom can be designated with two quantum numbers n and l.

The maximum value of l is equal to n – 1 and that of m is ± l.

Solution

Question 2

(n – 1)d subshell is always lower in energy than ns subshell.

(n – 1)d subshell always has more energy than ns subshell.

5d is lower in energy than 4f.

5f is lower in energy than 7s.

Solution

Question 3

principal quantum number

azimuthal quantum number

magnetic quantum number

spin quantum number

Solution

Question 4

2d5

3p6

4s1

4f12

Solution

Question 5

4l - 2

4l + 2

2l + 1

2n2

Solution

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2d⁵

3p⁶

4s¹

4f¹²

2n²