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Practice: Quantum Numbers and Electronic Configuration

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Wize University Chemistry Textbook > Quantum Numbers and Electron Configurations

Orbital Filling Diagrams

6 Activities

Wize University Chemistry Textbook > Quantum Numbers and Electron Configurations

Diamagnetic vs Paramagnetic Electron Configurations

3 Activities

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1. Which groups of atoms are diamagnetic in their ground electronic states?
2. What would be the electronic configuration of Na if each orbital could hold 3 instead of 2 electrons? Draw the electronic configuration assuming all other rules are valid.
3. What is the maximum number of electrons in an atom that has: n =3, ml = ±1, ms = + 1/2?
4. What are the 4 quantum numbers for the unpaired electron of Br?
More Orbital Filling Diagrams Questions:
Quantum Numbers
How many electrons can have the following quantum numbers:
a. n = 4
b. n = 4, ms = + 1/2
Filling Atomic Orbitals
Fill the atomic orbital diagram for scandium below to answer the following questions.
Filling Atomic Orbitals
Fill the atomic orbital diagram for vanadium below to answer the following questions.
Quantum model: Orbital filling
Draw an atomic orbital diagram for sulfur.
Atom: Electronic configuration
Which of the following orbital diagrams shows a valid ground state electron configuration for an uncharged atom?
Quantum model: Electron configuration
a) What is the full ground state electron configuration (spdf notation) of Al?
b) Draw the energy level diagram for Al.
c) Modify the energy diagram above to show the excited state that required the smallest amount of energy to move the highest energy valence electron to another orbital.
Quantum model: Ground and Excited States
In the energy diagram:
a) Identify all subshells by circling them.
b) Place the name of each subshell next to your circle.
Quantum model: Energy Level Diagram
Consider an atom of the alkali metal Potassium.
a) In the energy diagram given, fill in the required number of electrons for a potassium atom and name the occupied orbitals.
b) The valence electron of potassium can be excited to the next highest energy state in the same valence shell. Below, show how the energy level diagram for the excited atom of potassium has changed. Make sure to name all occupied orbitals.
Orbitals: Lowest energy configuration
Select the orbital diagram of P+ in its lowest energy configuration (ground state).
VSEPR: σ and π Frameworks with Consecutive Double Bonds
Answer the following questions about the species H2CN2, whose Lewis structure is shown below:
Quantum Model: Orbital filling
Which of the following is a correct energy diagram for all the electrons present in a ground state neutral nitrogen atom?
Quantum model: Filling orbitals
Which element has the orbital-filling diagram shown below?
Atom: Electronic configuration
Given the ground-state electronic configuration
[Ar] 4s23d3
1. What is the neutral atom with this electronic configuration?
More Diamagnetic vs Paramagnetic Electron Configurations Questions:
Write the electronic configuration of the following species, and label them as D diamagnetic or P paramagnetic
Cr2+
Write the shorthand electron configurations for the following species pairs, and state if they are paramagnetic or diamagnetic:
Cu and Cu+{\small \text{Cu and Cu}^+}
I and I−{\small \text{I and I}}^-
MOT
Similar to 2017, final exam, #50
Rank the following species in terms of increasing bond length and comment on their magnetic properties:
O22+, O2+, O2, O2―, and O22―.
Atomic Orbital Diagram
Draw the atomic orbital diagram of a neutral magnesium atom and determine the magnetism of the atom.
Periodic Table: Magnetism
Fill in the blanks using neutral atoms from the 4th period. Note there may be more than one answer.
____________ is diamagnetic
Which of the following is not paramagnetic?
Elements: Magnetism
Which of the following are paramagnetic? (Note: Answer Yes or No)
"The Periodic Table", image retrieved from Chemistry 2e (https://d3bxy9euw4e147.cloudfront.net/oscms-prodcms/media/documents/Chemistry2e-OP_QCzV58S.pdf) by Flowers, P et al., is licensed under CC BY.
Elements: Magnetism
Which of the following are diamagnetic? (select all that apply in your answer)
"The Periodic Table", image retrieved from Chemistry 2e (https://d3bxy9euw4e147.cloudfront.net/oscms-prodcms/media/documents/Chemistry2e-OP_QCzV58S.pdf) by Flowers, P et al., is licensed under CC BY.
Atom: Electron Configuration
Write the electronic configuration of the following species, and label them as D diamagnetic or P paramagnetic
a) Sc2+
b) Cr2+
According to MO theory, which of the following molecules would be diamagnetic?
Elements: Diamagnetic Diatomics
Which of the following diatomic molecules are paramagnetic? Use MO theory in your analysis.
i. O2
ii. N2
Elements: Magnetism
Which of the ground-state atoms in the table below have their magnetic behavior identified correctly?
AtomClassificationI.MgparamagneticII.SidiamagneticIII.Brdiamagnetic\begin{array}{c:c:c} &\rm Atom&\rm Classification\\ \hline \rm I. &\rm Mg&\rm paramagnetic \\ \hline \rm II. &\rm Si& \rm diamagnetic \\ \hline \rm III. &\rm Br&\rm diamagnetic \end{array}
paramagnetic
What is the electron configuration of Ni2+? Bonus: Is this diamagnetic or paramagnetic (see solutions for answer)
Atom: Electronic Configuration and Magnetism
Write the electronic configuration of the following species, and label them as D diamagnetic or P paramagnetic
Ni2-
Elements: Magnetism
Which of the following atoms or ions is paramagnetic?
Atom: Electron configuration and Magnetism
Write the electronic configuration of the following species, and label them as D diamagnetic or P paramagnetic
Mn5+
Atom: Electronic Configuration and Magnetism
Write the electronic configuration of the following species, and label them as D diamagnetic or P paramagnetic
Cr2+
Elements: Magnetism
Write the electronic configuration of the following species, and label it as diamagnetic or paramagnetic
Sc2+