Free Practice Quiz Question List

2 Periodic Trends Online Quiz Questions

Use this free practice quiz with 20 questions to review 2 Periodic Trends, test your knowledge, and prepare for your next test or exam.

20 questions

True or false

1 point

True or false: Across a period, effective nuclear charge on valence electrons generally increases.

A
True
B
False

True or false

1 point

True or false: Electronegativity is the energy change when an isolated gaseous atom gains an electron.

A
True
B
False

Choose one

1 point

An atom loses one or more electrons to form a cation. Which statement best explains the usual change in size?

A
A cation is usually larger than its parent atom because it has fewer electrons.
B
A cation is usually smaller than its parent atom because electron removal reduces electron–electron repulsion.
C
A cation is always the same size as its parent atom.
D
A cation is usually larger because its nucleus has fewer protons.

Choose one

1 point

Which sequence orders the isoelectronic ions from largest radius to smallest radius?

A
O²⁻ > F⁻ > Na⁺ > Mg²⁺
B
Mg²⁺ > Na⁺ > F⁻ > O²⁻
C
F⁻ > O²⁻ > Mg²⁺ > Na⁺
D
Na⁺ > Mg²⁺ > O²⁻ > F⁻

Choose one

1 point

Why does first ionization energy generally increase from left to right across a period?

A
It generally decreases because each added proton increases shielding enough to cancel the nuclear charge.
B
It remains constant because the added electron is in the same main energy level.
C
It generally increases because effective nuclear charge rises.
D
It generally increases because atoms gain additional electron shells.

Written response

1 point

What is the name of the radius defined as half the distance between the nuclei of two identical atoms joined by a covalent bond?

Written response

1 point

What property is the energy required to remove an electron from a ground-state gaseous atom?

Fill in the blank

1 point

Across a period, atomic radius generally because effective nuclear charge pulls electrons in the same general shell closer to the nucleus.

Fill in the blank

1 point

Using the energy-change convention for electron affinity, a negative value means when a gaseous atom gains an electron.

Choose all

1 point

Select all statements that correctly describe general periodic trends.

A
Atomic radius generally decreases across a period.
B
Atomic radius generally decreases down a group.
C
First ionization energy generally increases across a period.
D
Electronegativity generally decreases down a group.
E
First ionization energy generally decreases across a period.

Choose all

1 point

Select all statements about ionic size that are supported by periodic-trend principles.

A
A cation is usually smaller than its parent atom.
B
An anion is usually larger than its parent atom.
C
In an isoelectronic series, radius increases as proton number increases.
D
In an isoelectronic series, radius decreases as proton number increases.
E
A cation and its parent atom must have the same radius.

Choose one

1 point

A table reports an electron affinity of negative energy using the energy-change convention. What does the negative sign indicate for the process of a gaseous atom gaining an electron?

A
Energy must be absorbed when an atom gains an electron.
B
Energy is released when an atom gains an electron.
C
The atom's electronegativity has increased.
D
The atom has lost an electron.

Open ended

1 point

An element's successive ionization energies increase gradually for the first two electrons, then show a particularly large jump when the third electron is removed. What does this suggest about the number of valence electrons, and why does the large jump occur?

Written response

1 point

A researcher measures the distance between the nuclei of two identical atoms joined by a covalent bond, then takes half that distance. What radius measure is being determined?

Choose one

1 point

Sodium and potassium are in the same group, with potassium below sodium. Which prediction about their atomic radii is best supported by periodic trends?

A
The radius generally decreases because nuclear charge increases.
B
The radius generally increases because valence electrons occupy shells farther from the nucleus.
C
The radius stays constant because shielding exactly cancels the added nuclear charge.
D
The radius generally decreases because each step down removes an electron shell.

Choose one

1 point

Sodium and magnesium are neighboring elements in the same period. Which is expected to have the smaller atomic radius, and why?

A
Magnesium, because effective nuclear charge generally increases across a period.
B
Sodium, because each added proton is fully canceled by an added electron.
C
They have the same radius, because their valence electrons occupy the same shell.
D
Sodium, because its smaller nuclear charge pulls its electrons closer.

Choose one

1 point

A neutral atom loses one electron to form a cation, without losing an entire outer shell. What is the usual size change, and what is the main explanation given by periodic-trend reasoning?

A
The cation is larger because the remaining electrons have more space available.
B
The cation is the same size because the number of protons is unchanged.
C
The cation is smaller because electron removal reduces electron–electron repulsion.
D
The cation is larger because losing an electron increases shielding.

Written response

1 point

Several atoms or ions are being compared, and each has the same number of electrons. What concise term describes these species?

Choose one

1 point

In a Na–Cl bond, which explanation best accounts for the shared electrons being drawn toward chlorine?

A
Sodium's first ionization energy is greater, so it pulls the shared electrons toward itself.
B
Chlorine is more electronegative than sodium, so it attracts the shared electrons more strongly.
C
Chlorine's electron affinity directly determines every feature of the bond.
D
Sodium has more protons, so it must attract the shared electrons more strongly.

True or false

1 point

True or false: Removing an electron from a ground-state gaseous atom always requires an input of energy.

A
True
B
False