Question

periodic trends worksheet
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 se
c largest ionization energy o s se te po
d lowest ionization energy o s se te po
e smallest atomic radius f cl br i at
f largest atomic radius li na k rb cs
2 low ionization energy is a characteristic of a
3 what does atomic radius measure?
4 describe the change in the atomic size across a period and down a group.
5 which element has the largest atomic radius?
6 explain the main difference between metals and nonmetals.
7 determine if the listed pairs of elements have similar or different properties.
a potassium & rubidium b calcium & barium
c sodium & chlorine d helium & krypton
e phosphorus & oxygen f lithium & fluorine
8 which element has the largest electronegativity?
9 which group (name) would have the lowest ionization energies?
10 which group (name) has the highest ionization energies?

Explanation:

Step1: Recall electron - affinity trend

Electron - affinity generally increases across a period and decreases down a group. Among N, P, As, Sb, Bi, Bi has the smallest electron - affinity as it is the largest atom in this group and has the least tendency to gain an electron.

Step2: Recall electronegativity trend

Electronegativity increases across a period and decreases down a group. Among Ga, Ge, As, Se, Se has the largest electronegativity as it is the most right - hand element among them in the periodic table.

Step3: Recall ionization - energy trend

Ionization energy increases across a period and decreases down a group. Among O, S, Se, Te, Po, O has the largest ionization energy as it is the top - most and most right - hand element among them (excluding noble gases in this context).

Step4: Recall ionization - energy trend for lowest value

Ionization energy decreases down a group. Among O, S, Se, Te, Po, Po has the lowest ionization energy as it is the bottom - most element in this group.

Step5: Recall atomic - radius trend

Atomic radius decreases across a period and increases down a group. Among F, Cl, Br, I, At, F has the smallest atomic radius as it is the top - most element in this group.

Step6: Recall atomic - radius trend for largest value

Atomic radius increases down a group. Among Li, Na, K, Rb, Cs, Cs has the largest atomic radius as it is the bottom - most element in this group.

Step7: Answer question 2

Low ionization energy is a characteristic of metals. Metals have a tendency to lose electrons easily, so they have low ionization energies.

Step8: Answer question 3

Atomic radius measures the distance from the nucleus of an atom to the outermost shell of electrons.

Step9: Answer question 4

Across a period, atomic size decreases due to increasing nuclear charge pulling the electrons closer. Down a group, atomic size increases as the number of electron shells increases.

Step10: Answer question 5

Francium (Fr) has one of the largest atomic radii among elements, but among common elements, Cs has a very large atomic radius.

Step11: Answer question 6

Metals tend to lose electrons (form cations), are good conductors of heat and electricity, and are malleable and ductile. Non - metals tend to gain electrons (form anions), are poor conductors of heat and electricity (except some like graphite), and are often brittle.

Step12: Answer question 7

a. Potassium and Rubidium are in the same group (alkali metals), so they have similar properties.
b. Calcium and Barium are in the same group (alkaline earth metals), so they have similar properties.
c. Sodium is a metal and Chlorine is a non - metal, so they have different properties.
d. Helium and Krypton are noble gases, so they have similar properties.
e. Phosphorus and Oxygen are non - metals but in different groups, so they have different properties.
f. Lithium is a metal and Fluorine is a non - metal, so they have different properties.

Step13: Answer question 8

Fluorine has the largest electronegativity among all elements.

Step14: Answer question 9

Alkali metals (Group 1) have the lowest ionization energies as they have only one valence electron which is easily removed.

Step15: Answer question 10

Noble gases (Group 18) have the highest ionization energies as they have a stable electron configuration and do not want to lose electrons easily.

Answer:

1. a. Bi; b. Se; c. O; d. Po; e. F; f. Cs
2. Metals
3. The distance from the nucleus of an atom to the outermost shell of electrons
4. Across a period, atomic size decreases; down a group, atomic size increases
5. Cs
6. Metals tend to lose electrons, are good conductors, and are malleable/ductile; non - metals tend to gain electrons, are poor conductors, and are often brittle
7. a. Similar; b. Similar; c. Different; d. Similar; e. Different; f. Different
8. F
9. Alkali metals
10. Noble gases