Question

why do metals typically have low electronegativity values? 1 point they have many valence electrons they actively seek to gain electrons they tend to lose electrons to become more stable they have complex electron configurations what happens when the difference between electronegativity values is greater than 1.7? 1 point a partial electron transfer occurs no chemical bonding takes place a complete exchange of electrons happens atoms remain chemically inert

Explanation:

For the first question, metals have low electronegativity because they tend to lose electrons to achieve a stable electron - configuration. For the second question, when the electronegativity difference between atoms is greater than 1.7, a complete transfer of electrons (ionic bond) occurs which can be considered a complete exchange of electrons in the context of chemical bonding.

Answer:

First question: They tend to lose electrons to become more stable
Second question: A complete exchange of electrons happens