Electronic Configuration of Atoms Quiz

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

Which element has an electron configuration of 2,8,1?

Sodium (Na) (correct)

Lithium (Li)

Potassium (K)

Calcium (Ca)

What is the maximum number of electrons that can occupy the d-sublevel?

10 (correct)

Which sublevel is filled after the 4s sublevel?

3d (correct)

Which statement about valence electrons is correct?

They occupy the outermost shell of an atom. Signup and view all the answers

According to the Aufbau principle, which of the following electrons are filled first?

2 electrons in the s-sublevel Signup and view all the answers

What is the total number of electrons found in the valence shell of Argon (Ar)?

8 Signup and view all the answers

Which element has an electron configuration of 2, 8, 8?

Argon (Ar) Signup and view all the answers

How many orbitals does the p-sublevel have?

3 Signup and view all the answers

Which of the following correctly describes the filling order of the first four energy levels?

1s, 2s, 2p, 3s Signup and view all the answers

Which element will have a filled 4p sublevel when in its ground state?

Krypton (Kr) Signup and view all the answers

Which element has the electron configuration of 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d5?

Chromium Signup and view all the answers

According to Hund’s rule, how should electrons be distributed in orbitals of equal energy?

Occupying all orbitals singly before pairing Signup and view all the answers

What is the electron configuration of the Ni ion Ni2+?

[Ar] 3d6 Signup and view all the answers

Which of the following correctly describes the Pauli Exclusion Principle?

No more than two electrons may occupy an orbital, and they must have opposite spins. Signup and view all the answers

What is the electron configuration for the element Lead (Pb)?

[Xe] 5d10, 6s2, 6p3 Signup and view all the answers

Which element features the electron configuration of 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d8?

Nickel Signup and view all the answers

If one were to remove electrons to form a cation from the iron atom (Fe), in which order would they be removed?

4s, then 3d; Signup and view all the answers

What constitutes a monoatomic anion?

Formed by adding electrons to the highest occupied orbitals. Signup and view all the answers

Which of the following elements would have a filled 3s subshell?

Calcium Signup and view all the answers

Which statement accurately reflects Hund's rule?

Electrons will occupy each orbital singly before pairing up. Signup and view all the answers

Study Notes

Electronic Configuration of Atoms

Electronic configuration describes the number of electrons in each main energy level of an atom.
Example: Helium (He) has 2 electrons in its n=1 shell, therefore its electron configuration is 2.
Example: Nitrogen (N) has 7 electrons with the configuration: 2 electrons in the n=1 shell, 5 electrons in the n=2 shell, configuration 2,5.
Example: Sodium (Na): 2,8,1
Example: Argon (Ar): 2,8,8

Sublevels, Orbitals, and Electrons

s-sublevel: holds 2 electrons in 1 orbital
p-sublevel: holds 6 electrons in 3 orbitals (px, py, pz)
d-sublevel: holds 10 electrons in 5 orbitals
f-sublevel: holds 14 electrons in 7 orbitals

Aufbau Principle

Electrons occupy the lowest available energy states first when building up the electronic configuration of an atom in its ground state.
The 4s sublevel is lower in energy than the 3d sublevel and is always filled before the 3d sublevel.
Examples:
- Scandium (Sc): 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d1
- Vanadium (V): 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d3
- Chromium (Cr): 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d5
- Nickel (Ni): 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d8
- Copper (Cu): 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d10
- Zinc (Zn): 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10

Hund's Rule of Maximum Multiplicity

When filling orbitals with the same energy level, electrons first occupy each orbital individually before they pair up.
Example:
- Boron (B): 1s2, 2s2, 2px1, 2py0, 2pz0
- Carbon (C): 1s2, 2s2, 2px1, 2py1, 2pz0
- Nitrogen (N): 1s2, 2s2, 2px1, 2py1, 2pz1
- Oxygen (O): 1s2, 2s2, 2px2, 2py1, 2pz1
- Fluorine (F): 1s2, 2s2, 2px2, 2py2, 2pz1
- Neon (Ne): 1s2, 2s2, 2px2, 2py2, 2pz2

Pauli Exclusion Principle

No more than two electrons can occupy a single orbital, and they must have opposite spins.

Configuration of Ions

Cations: Formed by losing electrons. Electrons are removed in the order np, ns, (n-1)d, where n is the principal quantum number of the valence shell.
Example:
- Iron (Fe): [Ar]3d64s2
- Iron(III) ion (Fe3+): [Ar]3d5
Anions: Formed by gaining electrons. Monoatomic anions gain enough electrons in their valence shell to achieve a noble gas configuration.
- Nitrogen (N): [He]2s2, 2px1, 2py1, 2pz1
- Azide ion (N3-): [He]2s2, 2px2, 2py2, 2pz2

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Description

Test your knowledge on the electronic configurations of various atoms and the principles governing them. This quiz covers examples, sublevels, orbitals, and the Aufbau principle. Challenge yourself to understand how electrons are arranged in different atoms!