Which of the following electron configurations represents an excited state of the indicated atom?A) Ne: 1s2 2s2 2p6B) Na: 1s2 2s2 2p6 3s2 3p2 4s1C) P: 1s2 2s2 2p6 3s2 3p2 4s1D) N: 1s2 2s2 2p

Complete question:

Which of the following electron configurations represents an excited state of the indicated atom?A) Ne: 1s2 2s2 2p6B) Na: 1s2 2s2 2p6 3s2 3p2 4s1C) P: 1s2 2s2 2p6 3s2 3p2 4s1D) N: 1s2 2s2 2p3

C) P: 1s² 2s² 2p⁶ 3s² 3p² 4s¹ → excited state

Explanation:

An excited state configuration is a higher energy arrangement of electrons.

A) Ne: (Neon has 10 electrons)

Ground state configuration:  1s² 2s² 2p⁶

Given configuration: 1s² 2s² 2p⁶ → ground state

B) Na: (sodium has 11 electrons)

Ground state configuration: 1s² 2s² 2p⁶ 3s¹

Given configuration: 1s² 2s² 2p⁶ 3s² 3p² 4s¹ → excess electrons

C) P: (Phosphorus has 15 electrons)

Ground state configuration: 1s² 2s² 2p⁶ 3s² 3p³

Given configuration: 1s² 2s² 2p⁶ 3s² 3p² 4s¹ → excited state

D) N: (Nitrogen has 7 electrons)

Ground state configuration: 1s² 2s² 2p³

Given configuration: 1s² 2s² 2p³ → ground state

hope this

explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)

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explanation: