name
instructions: answer the following. refer to your periodic table.
1. a. which atom is smaller? si or cl? circle your answer.
b. what period do the 2 elements belong?
2. a. which atom is larger? ca or rn? circle your answer.
b. which group do the 2 elements belong?
3. a. which atom is smaller? k or br? circle your answer.
b. what period do the 2 elements belong?
4. a. which atom is smaller? be or ra?
b. what group do the 2 elements belong?
5. a. which atom is larger? n or br?
b. what period does oxygen belong?
c. what group does chlorine belong?
6. which of the following will have a larger radius than zinc? gallium, aluminum, magnesium, strontium?
7. the atomic radius across period: a. decrease from left to right b. increase from left to right c. decrease from right to left d. stay the same
8. as you move down a group on the periodic table, what happens to the size of the atoms? a. they stay the same b. they get larger c. they get smaller
9. a. which element has the lowest ionization energy? ne or cs?
b. what period does ne belong?
c. what group does cs belong?
10. a. which has a greater ionization energy? li or se? circle your answer.
b. what period does li belong?
c. what group does se belong?
11. a. which has a greater ionization energy? rb or o?
b. what period does rb belong?
c. what group does o belong?
12. which of these elements has the highest ionization energy? a. li b. k c. fr d. na
13. which of these elements has the lowest ionization energy? a. o b. b c. c d. f
14. which of the following lists of the atoms in order of increasing ionization energy?
a. calcium, iron, copper b. copper, iron, calcium c. calcium, copper, iron d. iron, copper, calcium
15. across a period, ionization energy ____a____
down a group, ionization energy ____b____
(options: a : increase, b : decrease; a : increase, b : increase; a : decrease, b : decrease)
16. which element has the greater ionization energy? mg or p?
17. which of the following is true about a sulfur atom and a chlorine atom?
(options: sulfur is larger and has higher ionization energy; sulfur is larger and has lower ionization energy; sulfur is smaller and has higher ionization energy; sulfur is smaller and has lower ionization energy)
circle the atom in each pair that has the greater electronegativity.
a. ca or ga
b. br or as
c. li or o
d. ba or sr
e. cl or s
f. o or s

Question

name
instructions: answer the following. refer to your periodic table.
1. a. which atom is smaller? si or cl? circle your answer.
   b. what period do the 2 elements belong?
2. a. which atom is larger? ca or rn? circle your answer.
   b. which group do the 2 elements belong?
3. a. which atom is smaller? k or br? circle your answer.
   b. what period do the 2 elements belong?
4. a. which atom is smaller? be or ra?
   b. what group do the 2 elements belong?
5. a. which atom is larger? n or br?
   b. what period does oxygen belong?
   c. what group does chlorine belong?
6. which of the following will have a larger radius than zinc? gallium, aluminum, magnesium, strontium?
7. the atomic radius across period: a. decrease from left to right b. increase from left to right c. decrease from right to left d. stay the same
8. as you move down a group on the periodic table, what happens to the size of the atoms? a. they stay the same b. they get larger c. they get smaller
9. a. which element has the lowest ionization energy? ne or cs?
   b. what period does ne belong?
   c. what group does cs belong?
10. a. which has a greater ionization energy? li or se? circle your answer.
    b. what period does li belong?
    c. what group does se belong?
11. a. which has a greater ionization energy? rb or o?
    b. what period does rb belong?
    c. what group does o belong?
12. which of these elements has the highest ionization energy? a. li b. k c. fr d. na
13. which of these elements has the lowest ionization energy? a. o b. b c. c d. f
14. which of the following lists of the atoms in order of increasing ionization energy?
    a. calcium, iron, copper b. copper, iron, calcium c. calcium, copper, iron d. iron, copper, calcium
15. across a period, ionization energy ____a____
    down a group, ionization energy ____b____
    (options: a : increase, b : decrease; a : increase, b : increase; a : decrease, b : decrease)
16. which element has the greater ionization energy? mg or p?
17. which of the following is true about a sulfur atom and a chlorine atom?
    (options: sulfur is larger and has higher ionization energy; sulfur is larger and has lower ionization energy; sulfur is smaller and has higher ionization energy; sulfur is smaller and has lower ionization energy)
circle the atom in each pair that has the greater electronegativity.
    a. ca or ga
    b. br or as
    c. li or o
    d. ba or sr
    e. cl or s
    f. o or s

Accepted Answer

Let's solve some of these problems step by step. We'll start with question 7 about atomic radius across a period.

### Question 7
# Explanation:
## Step 1: Recall periodic trend for atomic radius across a period
As we move from left to right across a period in the periodic table, the number of protons in the nucleus increases, which increases the effective nuclear charge. This pulls the electrons closer to the nucleus, decreasing the atomic radius.
## Step 2: Match with options
The options are: a. decrease from left to right, b. increase from left to right, c. decrease from right to left, d. stay the same. From the trend, atomic radius decreases from left to right across a period. So the correct option is a.
# Answer: a

### Question 8
# Explanation:
## Step 1: Recall periodic trend for atomic size down a group
As we move down a group in the periodic table, each element has an additional electron shell. The outermost electrons are further from the nucleus, so the atomic size (radius) increases.
## Step 2: Match with options
The options are: a. they stay the same, b. they get larger, c. they get smaller. From the trend, atoms get larger as we move down a group. So the correct option is b.
# Answer: b

### Question 15
# Explanation:
## Step 1: Trend for ionization energy across a period
Across a period (left to right), the effective nuclear charge increases, so it's harder to remove an electron. Thus, ionization energy increases.
## Step 2: Trend for ionization energy down a group
Down a group (top to bottom), the number of electron shells increases, so the outermost electron is further from the nucleus and easier to remove. Thus, ionization energy decreases.
## Step 3: Match with options
For part a (across a period), ionization energy increase. For part b (down a group), ionization energy decrease. So the first option with a: increase and b: decrease is correct.
# Answer: a: increase, b: decrease (the first set of options)

### Question 16: Which has greater ionization energy, Mg or P?
# Explanation:
## Step 1: Locate Mg and P on the periodic table
Mg is in period 3, group 2. P is in period 3, group 15.
## Step 2: Recall ionization energy trend across a period
Across a period (left to right), ionization energy generally increases (with some exceptions). P is to the right of Mg in period 3. Also, P has a half - filled p - subshell (3p³), which is relatively stable, but the general trend of increasing across the period (from left to right) still holds as the effective nuclear charge increases. So P has a greater ionization energy than Mg.
# Answer: P

### Question 17: About S and Cl atoms
# Explanation:
## Step 1: Atomic size trend
S and Cl are in the same period (period 3). As we move from S (group 16) to Cl (group 17) across the period, the atomic radius decreases. So S is larger than Cl.
## Step 2: Ionization energy trend
Across a period (left to right), ionization energy generally increases. Since S is to the left of Cl, S has a lower ionization energy than Cl. So the statement "Sulfur is larger and has lower ionization energy" is correct.
# Answer: Sulfur is larger and has lower ionization energy.

### Electronegativity questions (circle the atom with greater electronegativity)
#### Part a: Ca or Ga
# Explanation:
## Step 1: Locate Ca and Ga
Ca is in group 2, period 4. Ga is in group 13, period 4.
## Step 2: Electronegativity trend across a period
Across a period (left to right), electronegativity increases. Ga is to the right of Ca in period 4. So Ga has greater electronegativity.
# Answer: Ga

#### Part b: Br or As
# Explanation:
## Step 1: Locate Br and As
Br is in group 17, period 4. As is in group 15, period 4.
## Step 2: Electronegativity trend across a period
Across a period (left to right), electronegativity increases. Br is to the right of As in period 4. So Br has greater electronegativity.
# Answer: Br

#### Part c: Li or O
# Explanation:
## Step 1: Locate Li and O
Li is in group 1, period 2. O is in group 16, period 2.
## Step 2: Electronegativity trend across a period
Across a period (left to right), electronegativity increases. O is to the right of Li in period 2. So O has greater electronegativity.
# Answer: O

#### Part d: Ba or Sr
# Explanation:
## Step 1: Locate Ba and Sr
Ba is in group 2, period 6. Sr is in group 2, period 5.
## Step 2: Electronegativity trend down a group
Down a group (top to bottom), electronegativity decreases. Sr is above Ba in group 2. So Sr has greater electronegativity.
# Answer: Sr

#### Part e: Cl or S
# Explanation:
## Step 1: Locate Cl and S
Cl is in group 17, period 3. S is in group 16, period 3.
## Step 2: Electronegativity trend across a period
Across a period (left to right), electronegativity increases. Cl is to the right of S in period 3. So Cl has greater electronegativity.
# Answer: Cl

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Question 7

Step 1: Recall periodic trend for atomic radius across a period

Step 2: Match with options

Step 1: Recall periodic trend for atomic size down a group

Step 2: Match with options

Step 1: Trend for ionization energy across a period

Step 2: Trend for ionization energy down a group

Step 3: Match with options

Answer:

Question 8