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Consider the following list of electron ...

Consider the following list of electron configurations:
(1) `1s^(2)2s^(2)3s^(2)` (2) `1s^(2)2s^(2)2p^(6)`
(3) `1s^(2)2s^(2)2p^(6)3s^(1)` (4) `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)`
(5) `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)3d^(6)`
Which one of the above configurations represents an excited state of a neutral atom?

A

1

B

3

C

2

D

4

Text Solution

AI Generated Solution

The correct Answer is:
To determine which of the given electron configurations represents an excited state of a neutral atom, we need to analyze each configuration based on the principles of electron filling order and the n + l rule. ### Step-by-Step Solution: 1. **Understanding the Ground State Configuration**: The ground state configuration of an atom is the arrangement of electrons in the lowest energy levels. Electrons fill the orbitals in the order of increasing energy, following the Aufbau principle. The order of filling is determined by the n + l rule, where n is the principal quantum number and l is the azimuthal quantum number. 2. **Analyzing Each Configuration**: - **Configuration (1)**: `1s^(2)2s^(2)3s^(2)` - This configuration fills the 1s, 2s, and 3s orbitals. It is a ground state configuration as it follows the correct order of filling. - **Configuration (2)**: `1s^(2)2s^(2)2p^(6)` - This configuration fills the 1s, 2s, and 2p orbitals completely. It is also a ground state configuration. - **Configuration (3)**: `1s^(2)2s^(2)2p^(6)3s^(1)` - Here, the 1s, 2s, and 2p orbitals are filled, but the 3s orbital has only one electron. This indicates that an electron from a lower energy level (possibly 3s) has been excited to a higher energy level. This configuration represents an excited state. - **Configuration (4)**: `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)` - This configuration fills the 1s, 2s, 2p, 3s, 3p, and 4s orbitals completely. It is a ground state configuration. - **Configuration (5)**: `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)3d^(6)` - This configuration fills the 1s, 2s, 2p, 3s, 3p, and 4s orbitals before filling the 3d orbital. It is also a ground state configuration. 3. **Conclusion**: The only configuration that represents an excited state is **Configuration (3)**: `1s^(2)2s^(2)2p^(6)3s^(1)`. ### Final Answer: The configuration that represents an excited state of a neutral atom is **(3) `1s^(2)2s^(2)2p^(6)3s^(1)`**.
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Knowledge Check

  • Consider the following list of electron configurations: (1) 1s^(2)2s^(2)3s^(2) (2) 1s^(2)2s^(2)2p^(6) (3) 1s^(2)2s^(2)2p^(6)3s^(1) (4) 1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2) (5) 1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)3d^(6) Which one of the above configuration represents a transition element?

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  • Consider the following list of electron configurations: (1) 1s^(2)2s^(2)3s^(2) (2) 1s^(2)2s^(2)2p^(6) (3) 1s^(2)2s^(2)2p^(6)3s^(1) (4) 1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2) (5) 1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)3d^(6) Which one of the above configuration represents a neutral atom that readily forms a singly charged positive ion?

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    B
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