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The electron configurations described in this chapter all refer to gaseous atoms in their ground states. An atom may absorb a quantum of energy and promote one of its electrons to a higher-energy orbital. When this happens, we say that the atom is in an excited state. The electron configurations of some excited atoms are given. Identify these atoms and write their ground-state configurations: (a) 1s12s11s^12s^1
(b) 1s22s22p23d11s^22s^22p^23d^1 (c) 1s22s22p64s11s^22s^22p^64s^1 (d) [Ar]4s13d104p4[\mathrm{Ar}]4s^13d^{10}4p^4 (e) [Ne]3s23p43d1[\mathrm{Ne}]3s^23p^43d^1

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PART A:

Determine the atomic number of the element represented by the electron configuration in its excited state by adding the superscripts of the subshells. Then use the periodic table to determine the identity of this element.

Z=1+1=2\begin{align*} Z &= 1+1\\ &=2 \end{align*}

This is the atomic number for helium (He).

Use the periodic table as a guide in writing down the correct electron configuration for helium in its ground state. Make sure to write the electron configuration in the order in which the subshells are filled.

He: 1s21s^2

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