Periodic Trends Part 2

Review Questions

Multiple Choice

As you move down the periodic table atoms get bigger.  This is because ____________.

• The atoms have more protons.
• The atoms have more energy levels

Multiple Choice

As you move across the periodic table atoms tend to get smaller because, ______________.

• the atoms have more protons.
• the atoms have less electrons.

Multiple Choice

Which of the following will have a larger radius than Zinc?

• Aluminum
• Strontium

Multiple Choice

The more protons there are, the  ____ .

• Weaker the pull
• Stronger the pull

Multiple Choice

Which one has the largest radius?

• Lithium (Li, atomic #3)
• Boron (B, atomic #5)
• Nitrogen (N, atomic #7)

Multiple Choice

Why is iodine larger than bromine?

• iodine has a greater number of electrons than bromine

• iodine has more occupied energy levels and greater shielding than bromine

• iodine has more valence electrons than bromine

e-

e-

Positive ions are smaller than the neutral atom from which they are formed.

The increased positive charge of the nucleus pulls electrons in
closer.

e-

e-
Valence

electrons are

removed.

More protons than
electrons causes the

nucleus to pull in electrons closer.

The resulting cation
is smaller than the
neutral atom.

​

anion

Negative ions are larger than the neutral atom from which they are formed.

e-

e-
Valence

electrons are

added

More electrons than protons causes the ion

to expand due to increased repulsive

forces.

The resulting anion
is larger than the
neutral atom.

The extra repulsion produced from the additional electrons cause the ion to expand.

e-

e-

Multiple Choice

As you look from left to right across a period, ionic radius

• increases

• decreases

Cations formed

from metal atoms are smaller than
the neutral atom.

Anions formed from nonmetal atoms are

larger than the neutral atom.

1. Which of the following elements have atoms with a

smaller atomic radius than sulfur?

a. silicon

b. carbon

c. sodium

d. chlorine

2. Which ion in each pair has the smaller radius?

a. K+or Ca2+

c. Al3+or P3-

b. K+or Cs+

d. O2-or F-

Ionization Energy: the energy required to
remove an electron from an atom

Multiple Choice

What is ionization energy?

• Energy needed to destroy an atom
• Energy required to remove an electron
• Energy needed to split an electron
• Energy required to add an electron

Period Trend:
Ionization energy increases across the period.

As the atomic radius decreases across the period, the valence electron being removed is closer to the nucleus.

(being held more tightly!)

​

t

t

t

As the atomic radius increases
down the group, the valence
electron being removed is
further from the nucleus.

​

(easier to remove!)

Group Trend: Ionization energy decreases down the group.

Multiple Choice

As you look down a group, ionization energy and electronegativity

• increases

• decreases

Electronegativity: a measure of the ability of
an atom in a chemical compound to attract
electrons from another atom

Multiple Choice

Electronegativity is...

• how good an atom is at attracting electrons
• the ability of an atom to lose electrons
• the energy required to remove an electron from a specific atom
• how easy it is to make friends. 

Period Trend:
Electronegativity increases across the period.

As the atomic radius decreases across the period, the positive nuclear charge increases, making the atom’s ability to “pull in” electrons much greater.

t

t

t

As the atomic radius increases down the group, valence electrons are further from the positive nuclear charge, making it difficult for the atom to “pull in” electrons.

​

Group Trend: Electronegativity decreases down the group.

The element with the highest electronegativity

is fluorine. The lowest - francium

1. Which atom has the least ability to attract electrons in

a compound?

a. S

b. O

c. Cl

d. F

2. Which atom has the greatest ability to attract

electrons in a compound (electronegativity)?

a. As

c. Ga

b. Se

d. Ge

Multiple Choice

Which has the greater electronegativity:

N or C?

• C

• N

Group Trends: (down the group)
Affected by shielding. Shielding increases down the
group due to increasing number of energy levels.

Period Trends: (across the period)
Affected by increasing nuclear charge. Increasing
number of protons, but same number of energy levels.

metals

nonmetals