Group 1 elements have an average electronegativity of 0.84 (not including hydrogen). Group 17 elements have an average electronegativity of 2.99. These two groups often form bonds. Given this information, which kind of bond will they likely form (ionic or covalent), and what evidence supports your claim? If it is ionic, then include which group gives up its electron to the other group. In three to five sentences, explain your reasoning. (4 points)

Group I elements combine with group 17 elements to form ionic compounds such NaF, NaCl, etc. When the electronegativity DIFFERENCE is above about 1.7 the bond will be ionic. 2.99-0.84 >> 2.15 and ionic is the game. Group I elements give up electrons and gorup 17 elements accept them.

is drbob answer right?

I sure hope he is .

Based on the electronegativity values of Group 1 and Group 17 elements, it is likely that they will form ionic bonds. Ionic bonds occur when there is a large difference in electronegativity between two elements, resulting in the transfer of electrons from one atom to another. In this case, the Group 1 elements have a lower electronegativity (0.84) compared to Group 17 elements (2.99). This indicates that Group 1 elements are more likely to give up their electrons to Group 17 elements, forming positive ions (cations) and negative ions (anions), respectively. The strong difference in electronegativity supports the formation of ionic bonds between these two groups.