Question

1. use a periodic table to choose the best answer.

____ is a period 4 element that is most likely to lose electrons to form a cation.
br
kr
k
ge

1. use a periodic table to choose the best answer.

which of these elements has the highest ionization energy?
br
f
i
at
cl

Explanation:

Question 6

• Br (Bromine): It is a non - metal in group 17. Non - metals tend to gain electrons to form anions.
• Kr (Krypton): It is a noble gas (group 18). Noble gases have a stable electron configuration and do not easily lose or gain electrons.
• K (Potassium): It is an alkali metal (group 1). Alkali metals have one valence electron and readily lose it to form a cation (\(K^{+}\)).
• Ge (Germanium): It is a metalloid. While it can form ions, it is not as likely as an alkali metal to lose electrons to form a cation.

• Ionization energy generally increases across a period (from left to right) and decreases down a group.
• Br (Bromine): In period 4, group 17.
• F (Fluorine): In period 2, group 17. It is the most electronegative element and has a very high ionization energy as it holds its electrons tightly.
• I (Iodine): In period 5, group 17. Its ionization energy is lower than F and Cl due to its larger atomic size.
• At (Astatine): In period 6, group 17. It has a lower ionization energy than the lighter halogens.
• Cl (Chlorine): In period 3, group 17. Its ionization energy is lower than F.

Answer:

K

Question 7