Identify the electronic filling after known elements

The last known noble gas in the currently predicted sequence is element $Z=118$ with configuration ending in: $[Rn] \, 5f^{14} 6d^{10} 7s^2 7p^6$

Next elements after $Z=118$

After $7p$ is completely filled at $Z=118$, the next electrons are expected to enter the $8s$ subshell.

• For $Z=119$: $[Og] \, 8s^1$ This would be an alkali metal.

• For $Z=120$: $[Og] \, 8s^2$

Determine the group from valence configuration

An outer electronic configuration of $ns^2$ corresponds to Group 2 elements.

Group 2 elements are called alkaline earth metals.

Check options

• A: Alkaline earth metal $ightarrow$ Correct
• B: Alkali metal $ightarrow$ Incorrect, that would correspond to $ns^1$
• C: Transition metal $ightarrow$ Incorrect, transition metals involve filling of $d$ subshells
• D: Inner transition metal $ightarrow$ Incorrect, inner transition metals involve filling of $f$ subshells

Final answer

Therefore, the element with $Z=120$ will be an alkaline earth metal.