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