Question

using the periodic table and your knowledge of periodic trends, answer the following questions:
1 circle the best answer that has the:
a smallest electron affinity
n
p
as
sb
bi
b largest electronegativity
ga
ge
as
sc
c largest ionization energy
o
s
sc
te
po
d lowest ionization energy
o
s
sc
te
po
e smallest atomic radius
f
cl
br
i
at
f largest atomic radius
li
na
k
rb
cs

Explanation:

Step1: Analyze atomic radius trend

Atomic radius increases down a group and decreases across a period. Among the given elements, Cs (cesium) is in the lower - left part of the periodic table (Group 1, lower periods), so it has a large atomic radius. Li, Na, K, Rb are also in Group 1, but Cs is the lowest among them. For the non - metals in the upper part (like F), atomic radius is smaller.

Step2: Analyze electron - affinity trend

Electron affinity generally becomes more negative (more favorable) across a period (excluding noble gases). F (fluorine) is highly electronegative and has a high electron - affinity. Among the given non - metals (N, P, As, Sb, Bi, F, Cl, Br, I, At), F is in the upper right (excluding noble gases) and has a high tendency to gain an electron.

Answer:

a. F (smallest electron - affinity among the non - metals shown, as it has a high tendency to gain an electron and is in the upper right of the non - metals in the table).
f. Cs (largest atomic radius as it is in Group 1 and the lowest period among the given elements in that group).