Hund's Rule

Q.

Write the ground-state electronic configuration for a neutral carbon atom, and for an excited state of carbon.

Q.

What is subshells?

Q. Which of the following electronic configuration represent a violation of Hund's rule for an atom in its ground state?

1. 
2. 
3. 
4. 

Q. The explanation for the presence of three unpaired electrons in the nitrogen atom is given by _____.

1. Paulis exclusion principle
2. Aufbau principle
3. Hunds rule
4. Heisenberg uncertainty principle

Q. According to the Hunds rule, which of the following is the correct electronic configuration of nitrogen atom?

1. $1s^{2}2s^{2}2{p_x}^{2}2{p_y}^{1}2{p_z}^0$
2. $1s^{2}2s^{2}2{p_x}^{0}2{p_y}^{1}2{p_z}^2$
3. $1s^{2}2s^{2}2{p_x}^{1}2{p_y}^{1}2{p_z}^1$
4. $1s^{2}2s^{2}2{p_x}^{1}2{p_y}^{0}2{p_z}^2$

Q. Which of the following rules have been violated while writing the following electronic configuration of oxygen atom?
$$\begin{array}{c}\upharpoonleft \downharpoonright \end{array}\begin{array}{c}\upharpoonleft \downharpoonright \end{array}\begin{array}{ccc}\upharpoonleft \downharpoonright & \upharpoonleft \upharpoonleft & \end{array}$$

1. Aufbau principle
2. Hund’s rule
3. Pauli’s exclusion principle
4. Heisenberg's Uncertainty principle

Q. According to Hund's rule of maximum multiplicity, all the electrons in singly occupied orbitals have the same spin.

1. True
2. False

Q. According to which principle/rule, electron pairing starts only when all the orbitals of same energy are singly occupied?

1. Pauli exclusion principle
2. Aufbau principle
3. Hund's rule
4. Heisenberg uncertainty principle

Q.

My sir told that while writing subshell configuration we 1st write 3d and then 4s. But the electrons fill first in 4s and then in 3d My doubt is that which will come first 4s or 3d??why??

Q.

Which of the following should be correct according to Hund's rule?

1. 

2. 

3. 

4. 

Q. Statement 1: Hydrogen atom just needs one extra electron to achieve its duplet configuration.
Statement 2: Hydrogen atom has the tendency to acquire duplet configuration so that it can become stable.

1. Statement 1 and 2 are correct, but statement 2 is not the correct reason for statement 1.
2. Statement 1 and 2 are correct and statement 2 is the correct reason for statement 1.
3. Statement 1 is correct and statement 2 is incorrect.
4. Statement 2 is correct, but statement 1 is incorrect.

Q. In a ccp structure of compound X, Y. X atom is present in octahedral voids.Calculate nearest neighbours upto 6th CN for X atom at body centre?

Q. Were write the electronic configuration of ele!ments like 3s3p3d3f ....... What are these spdf . are they sushells of an atom.. If not what are they and what are sub shells and how to write it please explain in detail.

Q.

In degenerate orbitals, unpaired electrons have ______ spin

Q. Noble gases could not fit into Newlands' octave pattern.

1. False
2. True

Q. The $Z_{eff}$ for
3d electron of Cr
4s electron of Cr
3d electron of ${Cr}^{3+}$
3s electron of ${Cr}^{3+}$ are __________ respectively.

1. none of these
2. 4.6, 2.95, 4.95, 8.05
3. 4.95, 2.05, 4.6, 8.05
4. 4.6, 2.95, 5.3, 12.75

Q. Above orbital diagram shows the electron configuration of nitrogen atom. Which rule does not support this?

1. Afbau Principle
2. Pauli's exclusion law
3. none of these
4. Hund's rule

Q.

Indicate the number of unpaired electrons in: Si

Q. Why He is placed in p block not in s block , it has a configuration of 2s² which is similar to 2 group element? Explain in detail either its a exception or a correct placement.

Q. Noble gases could not fit into Newlands' octave pattern.

1. True
2. False

Q. Which of the following are filled according to the Aufbau's Principle.

1. $1s^{2}2s^1$
2. $2p^{5}3s^1$
3. $2p^{6}3s^1$
4. $4s^{2}3d^5$
5. $4p^{5}3s^1$
6. $4p^{6}5s^2$
7. $4f^{1}45d^1$
8. $3s^{1}2p^5$

Q. The ground state electronic configuration of nitrogen atom can be represented by

1. 
2. 
3. 
4. 

Q. Noble gases could not fit into Newlands' octave pattern.

1. False
2. True

Q. Dobereiner laid down the___________rule

Q.

The electron identified by quantum number n and l

1. n=4, l=1 2. n=4, l=0

3. n=3, l=2 4. n=3, l=1

Can be placed in the order of increasing energy from the lowest to highest as

A) 4<2<3<1 B) 2<4<1<3

C) 1<3<2<4 D) 3<1<4<2