What is noticeable about all of the ionic charges in Group 1 2 15 16 and 17?

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The ionic charges of group 1 and 2 metals are +1 and +2 respectively. Group 15 & 16 the simple mono-atomic ions are -3 and -2. Group 17 ions are -1. This can be explained by the following elemnts in groups 1 and 2 lose 1 or 2 electrons respectively to achieve a noble gas configuration whereas groups 15, 16 and 17 gain electrons (3,2 1 respectively)
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How do the outer-shell electron configurations for ions of elements from groups 1 and 2 and 15 and 16 and 17 compare with those of the noble gases?

Answer . Elements in Group 1 have 1 more electron than the noble gas in the row above it. Elements in Group 2 have 2 more electrons than the noble gas in the row above it

Why groups 1 and 2 form many compounds with groups 16 and 17?

Group 1 and 2 elements have 1 and 2 valence electrons respectively. Removal of these electrons will result in stable noble gas electronic configuration. Group 17 and 16 elemen

Why do the elements in the group 1 and 2 react with group 17?

The group 1 and 2 elements have much lower electronegativity value than group 17 elements and therefore lose electrons to the group 17 elements. The group 17 elements require

What is the charge ionic of Group 5a?

Group 5A, which includes the common elements nitrogen and phosphorus, has a -3 charge in an ionic bonding scenario, which means they will gain three electrons.