Which of the following species have the same number and arrangement of electrons in their lowest energy states?
_{19}K^+
_{11}Na^+
_8O^–
_8O^{2–}
_{16}S^–
A. _8O^– and _8O^{2–}
B. _{19}K^+ and _{16}S^–
C. _{11}Na^+ and _8O^{2–}
D. _{19}K^+ and _{11}Na^+
E. _8O^– and _{16}S^–
_{19}K^+
To find the number of protons, find the atomic number (in this case it’s 19, so we have 19 protons here). In a neutral atom, protons = electrons. Now we know that a neutral K atom should have 19 electrons, however, we want to find K^+, so we are going to remove one electron (we are looking to write out the structure for K^+ so we will need to fill in 18 electrons.
1s^2 2s^2 2p^6 3s^2 3p^6
_{11}Na^+
10 electrons.
1s^2 2s^2 2p^6
_8O^{-}
9 electrons.
1s^2 2s^2 2p^5
_8O^{2-}
10 electrons.
1s^2 2s^2 2p^6
_{16}S^-
17 electrons.
1s^2 2s^2 2p^6 3s^2 3p^5
_{11}Na^+ and _8O^{2-} both have the same number of electrons and therefore the same electron structure.
It says ‘lowest energy state’.
Doesn’t that mean 1s?