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 sc
c largest ionization energy o s sc 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?
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Explanation:

Step1: Recall electron - affinity trend

Electron affinity generally decreases down a group. Among N, P, As, Sb, Bi (Group 15), Bi has the smallest electron affinity.

Step2: Recall electronegativity trend

Electronegativity increases across a period and decreases down a group. Among Ga, Ge, As, Sc, As has the largest electronegativity as it is further to the right in the periodic table compared to the others.

Step3: Recall ionization - energy trend

Ionization energy decreases down a group. Among O, S, Se, Te, Po (Group 16), O has the largest ionization energy.

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.

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.

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.

Step7: Low ionization energy characteristic

Low ionization energy is a characteristic of a metal. Metals tend to lose electrons easily.

Step8: Define atomic radius

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

Step9: Describe atomic - size change

Across a period, atomic size decreases due to increasing nuclear charge. Down a group, atomic size increases due to the addition of electron shells.

Step10: Identify element with largest atomic radius

Among all elements, Francium (Fr) has one of the largest atomic radii (not in the given list, but generally). In the context of common - known elements, Cs is a large - radius element.

Step11: Explain metal - nonmetal difference

Metals tend to lose electrons to form cations, are good conductors of heat and electricity, and are malleable and ductile. Non - metals tend to gain electrons to form anions, are poor conductors, and are brittle.

Step12: Determine element - pair properties

a. Potassium and Rubidium (both Group 1) have similar properties as they are in the same group.
b. Calcium and Barium (both Group 2) have similar properties as they are in the same group.
c. Sodium (metal) and Chlorine (non - metal) have different properties.
d. Helium and Krypton (both noble gases) have similar properties.
e. Phosphorus and Oxygen (both non - metals but different groups) have different properties.
f. Lithium (metal) and Fluorine (non - metal) have different properties.

Step13: Identify element with largest electronegativity

Fluorine has the largest electronegativity among all elements.

Step14: Identify group with lowest ionization energies

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

Step15: Identify group with highest ionization energies

The noble gases (Group 18) have the highest ionization energies as they have a full outer - shell electron configuration and are very stable.

Answer:

1a. Bi
1b. As
1c. O
1d. Po
1e. F
1f. Cs

1. Metal
2. Distance from nucleus to outermost electron shell
3. Across a period: decreases; Down a group: increases
4. Cs (or Fr in general)
5. Metals lose electrons, are good conductors, malleable and ductile; Non - metals gain electrons, are poor conductors, brittle

7a. Similar
7b. Similar
7c. Different
7d. Similar
7e. Different
7f. Different

1. F
2. Alkali metals
3. Noble gases