Question

an atomic cation with a charge of +1 has the following electron configuration: 1s^2 2s^2 2p^6. what is the chemical symbol for the ion? na^+. how many electrons does the ion have? 11. how many 2s electrons are in the ion? 2

Explanation:

Step1: Analyze electron - configuration

The given electron - configuration $1s^{2}2s^{2}2p^{6}$ has a total of $2 + 2+6=10$ electrons.

Step2: Determine the neutral atom's electron number

Since it is a + 1 cation (lost 1 electron), the neutral atom had $10 + 1=11$ electrons. The element with 11 electrons is sodium (Na).

Step3: Identify number of 2s electrons

In the electron - configuration $1s^{2}2s^{2}2p^{6}$, the superscript of $2s$ is 2, so there are 2 electrons in the 2s orbital.

Answer:

What is the chemical symbol for the ion? $Na^{+}$
How many electrons does the ion have? 10
How many 2S electrons are in the ion? 2