Question

consider the figure below: figure showing electron shell diagrams for elements in group 1 (h, li, na), group 14 (c, si), group 17 (f, cl), group 18 (he, ne, ar) across periods 1, 2, 3 how many electrons do elements in group 1 need to lose in order to achieve a stable electron configuration? options: 3, 2, 4, most atoms already have the most stable electron configuration by nature, 1 (with 1 selected).

Explanation:

Step1: Recall Group 1 Elements' Valence Electrons

Group 1 elements (alkali metals) have 1 valence electron (electron in the outermost shell). For example, H has 1 valence electron, Li has 1 valence electron in its outermost shell, and Na has 1 valence electron in its outermost shell.

Step2: Determine Stable Electron Configuration

A stable electron configuration (like that of noble gases) is achieved when the outermost shell is full. For group 1 elements, losing 1 valence electron will leave them with a full outermost shell (same as the previous noble gas configuration). For example, Li (2,1) loses 1 electron to become \(Li^+\) (2, which is stable like He's configuration), Na (2,8,1) loses 1 electron to become \(Na^+\) (2,8, which is stable like Ne's configuration). So they need to lose 1 electron.

Answer:

1 (corresponding to the option "1" or the option with the text "1" among the choices, which in the given options is the one marked with the blue dot: "1")