What is the typical oxidation state of Group 1 metals in most compounds?

What is the typical oxidation state of Group 1 metals in most compounds?

• A. +1
• B. 0
• C. +2
• D. -1

Answer: (A)

Group 1 metals have one valence electron and readily lose it to reach a stable electron configuration like that of a noble gas. In compounds, that loss results in a +1 charge, so these elements form +1 cations in most cases (for example, NaCl, K2O, Na2O, etc.). Trying to remove a second electron to reach +2 is much less favorable for these elements, and in their elemental state the oxidation state is 0. The -1 state is not typical for metals. Therefore, the usual oxidation state of Group 1 metals in most compounds is +1.

Group 1 metals have one valence electron and readily lose it to reach a stable electron configuration like that of a noble gas. In compounds, that loss results in a +1 charge, so these elements form +1 cations in most cases (for example, NaCl, K2O, Na2O, etc.). Trying to remove a second electron to reach +2 is much less favorable for these elements, and in their elemental state the oxidation state is 0. The -1 state is not typical for metals. Therefore, the usual oxidation state of Group 1 metals in most compounds is +1.