Atomic Structure and Periodic Patterns Practice Quiz (11 questions)

All questions and answers

1. An atomic diagram uses the Bohr model to show an electron around the nucleus. Which arrangement is consistent with this model?

A position within the nucleus
A three-dimensional region with no defined path
A circular path selected from the allowed paths
Any circular path chosen without restrictions

A circular path selected from the allowed paths

Explanation

In the Bohr model, electrons circle the nucleus only along allowed paths. A three-dimensional region describes the quantum mechanical model, while unrestricted paths are not part of the Bohr model.

2. A scientist replaces a Bohr-style diagram with the quantum mechanical model. How does the new model represent where electrons are located?

In three-dimensional areas around the nucleus
On fixed circular paths around the nucleus
In flat, two-dimensional rings around the nucleus
Within the nucleus itself

In three-dimensional areas around the nucleus

Explanation

The quantum mechanical model represents electrons in three-dimensional areas around the nucleus. Fixed paths are characteristic of the Bohr model, and the model does not place electrons in the nucleus.

3. A student is assigning electrons to orbitals and has already placed two electrons in one orbital. How many additional electrons can be placed in that same orbital?

Zero
Four
One
Two

Zero

Explanation

An orbital can hold up to two electrons, so an orbital that already contains two has no remaining capacity. The one-electron and larger capacities confuse orbital capacity with other configuration counts.

4. When identifying the first subshell in an atom's electron configuration, which description applies to 1s?

The lowest-energy subshell, containing two spherical orbitals
A higher-energy subshell, containing one spherical orbital
The lowest-energy orbital, containing two subshells
The lowest-energy subshell, containing one spherical orbital

The lowest-energy subshell, containing one spherical orbital

Explanation

The 1s subshell has the lowest energy and contains one spherical orbital. The two-orbital description and the two-subshell description confuse distinct configuration features.

5. What are valence electrons?

Electrons in an atom’s outermost energy shell that influence its chemical properties
Electrons emitted from an atom when it releases energy as light
Electrons distributed across all shells that set the atom’s atomic number
Electrons in an atom’s innermost energy shell that determine its mass

Electrons in an atom’s outermost energy shell that influence its chemical properties

Explanation

Valence electrons occupy the outermost energy shell and are responsible for an atom’s chemical properties and participation in reactions. Electrons in the innermost shell are not what the term valence electrons identifies.

6. Which pattern in outermost energy levels helps make the periodic table useful for predicting relative properties of elements?

Elements with similar outermost-electron patterns tend to show related properties.
Elements in the same row have identical numbers of occupied energy levels.
Elements in the same column have matching numbers of total electrons.
Elements with similar atomic masses tend to share the same reactivity.

Elements with similar outermost-electron patterns tend to show related properties.

Explanation

Patterns in electrons in the outermost energy levels help predict relative properties of elements. Elements in a column do not have matching total electron counts; their outermost-electron patterns are the relevant clue.

7. What is the purpose of distinguishing an atom’s mass number from its average atomic mass?

The mass number counts protons and neutrons, while average atomic mass is a weighted average of isotope masses.
The mass number gives the weighted average of isotope masses, while average atomic mass counts protons and neutrons.
The mass number counts protons and electrons, while average atomic mass counts neutrons in the most common isotope.
The mass number identifies the number of isotopes, while average atomic mass gives the number of protons in the atom.

The mass number counts protons and neutrons, while average atomic mass is a weighted average of isotope masses.

Explanation

The mass number is the total number of protons and neutrons in an atom, whereas average atomic mass reflects the weighted masses of its isotopes. Counting protons and electrons does not define mass number, since neutrons—not electrons—are included in that total.

8. How do the electron transitions in a flame test differ before and after an electron emits light?

Absorbing energy removes an electron from the atom, while emitting light restores it to its original level.
Absorbing energy moves an electron to a lower level, while emitting light accompanies its rise to a higher level.
Absorbing energy moves an electron to a higher level, while emitting light accompanies its return to a lower level.
Absorbing energy changes an electron’s orbital shape, while emitting light leaves its energy level unchanged.

Absorbing energy moves an electron to a higher level, while emitting light accompanies its return to a lower level.

Explanation

An electron absorbs energy to reach a higher energy state, then releases energy as light when it drops to a lower state. The reverse-transition distractor swaps the directions of the energy changes.

9. Why can shininess and electrical conductivity help identify an element as a metal?

These traits indicate that the element emits visible light when heated.
These traits demonstrate that the element has a high number of energy levels.
These traits are characteristic properties associated with metals.
These traits show that the element has a full outer electron shell.

These traits are characteristic properties associated with metals.

Explanation

Shininess and good electrical conductivity are properties that support identifying an element as a metal. A full outer electron shell is associated with low reactivity, not with these identifying metallic traits.

10. When sketching an atom using the Bohr model, how should its electrons be arranged?

Throughout three-dimensional regions around the nucleus
Along specific allowed paths around the nucleus
In a continuous cloud without defined energy levels
In subshells grouped by their relative energy

Along specific allowed paths around the nucleus

Explanation

The Bohr model depicts electrons moving around the nucleus in specific allowed paths. Three-dimensional regions around the nucleus describe the quantum mechanical model instead.

11. Which feature characterizes the second energy shell in an atom?

It is the highest energy level an atom can have.
It contains one spherical orbital in the 1s subshell.
It contains two subshells, labeled s and p.
It contains the same number of electrons as the first shell.

It contains two subshells, labeled s and p.

Explanation

The second energy shell is composed of s and p subshells. The single spherical orbital describes the first shell’s 1s subshell, not the second shell.

Study with flashcards

Lock in the answers with 10 flashcards on Atomic Structure and Periodic Patterns.

In the Bohr model, where may electrons circle the nucleus?

Only in allowed paths.

How does the quantum mechanical model represent electrons around the nucleus?

As three-dimensional areas.

How many electrons can one orbital hold at most?

Two electrons.

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