Question

a. label the metals and the nonmetals.
b. for the vertical arrow, indicate the trend for atomic radius (ar), ionization energy (ie) and electron affinity (ea) by labeling next to the arrow whether each property increases or decreases.
c. repeat the instructions in b for the horizontal arrow.
d. for the diagonal arrow, indicate whether metallic character increases or decreases.
what conclusion can you draw about the ability of metals to hold on to and attract electrons, as compared to nonmetals?

Explanation:

Step1: Identify metals and non - metals

Metals are on the left - hand side and non - metals on the right - hand side of the periodic table (in a general sense).

Step2: Analyze vertical trend

As we move down a group (vertical arrow), atomic radius increases, ionization energy decreases, and electron affinity generally decreases.

Step3: Analyze horizontal trend

As we move across a period (horizontal arrow), atomic radius decreases, ionization energy increases, and electron affinity generally increases.

Step4: Analyze diagonal trend

As we move in the direction of the diagonal arrow, metallic character increases.

Step5: Compare metals and non - metals

Metals have a lower ability to hold on to and attract electrons compared to non - metals. Non - metals have higher electronegativities, ionization energies, and electron affinities, making them more likely to attract electrons.

Answer:

A. Metals are on the left - hand side of the periodic table representation in the grid, non - metals on the right.
B. Atomic radius: Increases; Ionization energy: Decreases; Electron affinity: Decreases.
C. Atomic radius: Decreases; Ionization energy: Increases; Electron affinity: Increases.
D. Metallic character: Increases.
Conclusion: Metals have a lower ability to hold on to and attract electrons compared to non - metals.