tendency to give up electron and become positive ion (+1) low electronegativity

1. He Ne Ar N F Be H O C B Li Na K • Describe the basic trend you see in the data. Relate it to the periodic table position of the elements. • Is it harder to remove an electron from an atom of lithium (Li) or fluorine (F)? • An atom of which element, Li or F, is more likely to give up an electron to form an ion (an atom from which 1 or more electrons has been removed)? What would be the charge on that ion? • By extension and contrast, an atom of which element, Li or F, is more likely gain an electron to form an ion? What would be the charge on that ion? • What would happen if an ion of Li approached an ion of Cl-? If an atom of Li approached an atom of Cl? • Explain using the diagram why Li, Na, and K have similar properties and are grouped together in Group 1 of the Periodic Table. What about He, Ne, and Ar? F and Cl?

2. little tendency to give up/take electron • extremely stable; pure element unreactive • don’t form bonds (filled outer shell) He Ne GP 8A F Ar N GP 7A Cl C H O Be B GP 1A Li Na K • tendency to give up electron and become positive ion (+1) • low electronegativity • pure element very reactive • 1 e outer shell, lose to haveflled outer shell • form ionic bonds with nonmetals • tendency to gain electron (from metals) and become negative ions (-1) • high electronegativity • pure element very reactive • form ionic bonds with metals • form covalent bonds (share electrons) with other nonmetals