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Questions and Answers
Helium has a total of 1 electron in its electronic configuration.
Helium has a total of 1 electron in its electronic configuration.
False
The electronic configuration of sodium is represented as 2,8.
The electronic configuration of sodium is represented as 2,8.
False
The p-sublevel can hold a maximum of 10 electrons.
The p-sublevel can hold a maximum of 10 electrons.
False
The Aufbau principle states that electrons fill the highest energy levels first.
The Aufbau principle states that electrons fill the highest energy levels first.
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Potassium has a total of 19 electrons in its electronic configuration.
Potassium has a total of 19 electrons in its electronic configuration.
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The 4s sublevel is filled after the 3d sublevel in an atom's electronic configuration.
The 4s sublevel is filled after the 3d sublevel in an atom's electronic configuration.
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The maximum number of electrons in the d-sublevel is 10.
The maximum number of electrons in the d-sublevel is 10.
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Valence electrons are those that occupy the innermost shell of an atom.
Valence electrons are those that occupy the innermost shell of an atom.
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Neon has an electronic configuration of 2,8.
Neon has an electronic configuration of 2,8.
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Beryllium has a total of 4 electrons in its electronic configuration.
Beryllium has a total of 4 electrons in its electronic configuration.
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According to Hund's rule, electrons fill orbitals in pairs before occupying them singly.
According to Hund's rule, electrons fill orbitals in pairs before occupying them singly.
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The electronic configuration of Copper (Cu) ends with 3d10.
The electronic configuration of Copper (Cu) ends with 3d10.
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The Pauli Exclusion Principle allows for three electrons to occupy the same orbital if they have the same spin.
The Pauli Exclusion Principle allows for three electrons to occupy the same orbital if they have the same spin.
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The electronic configuration for Scandium (Sc) is 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d1.
The electronic configuration for Scandium (Sc) is 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d1.
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The ion configuration for Fe3+ is [Ar]3d6.
The ion configuration for Fe3+ is [Ar]3d6.
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Zinc (Zn) has an electronic configuration that ends with 4s2, 3d10.
Zinc (Zn) has an electronic configuration that ends with 4s2, 3d10.
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For a nitrogen anion N3-, three additional electrons fill the 2s and 2p orbitals to achieve new noble gas configuration.
For a nitrogen anion N3-, three additional electrons fill the 2s and 2p orbitals to achieve new noble gas configuration.
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Element with atomic number 24 has its electronic configuration written as 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d5.
Element with atomic number 24 has its electronic configuration written as 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d5.
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In electronic configuration, the d orbitals are always filled before the s orbitals of the next principal energy level.
In electronic configuration, the d orbitals are always filled before the s orbitals of the next principal energy level.
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A cation configuration for element with atomic number 26 always loses electrons from the 3d subshell first.
A cation configuration for element with atomic number 26 always loses electrons from the 3d subshell first.
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Study Notes
Electronic Configuration
- Electronic configuration describes the distribution of electrons in an atom's energy levels.
- Each energy level (n=1, 2, 3, 4...) corresponds to a shell, containing sublevels (s, p, d, f) with differing energies.
- The Aufbau Principle dictates that electrons fill the lowest available energy states first.
Sublevels, Orbitals, and Electrons
- The s-sublevel has 1 orbital and can hold 2 electrons.
- The p-sublevel has 3 orbitals (px, py, pz) and can hold 6 electrons.
- The d-sublevel has 5 orbitals and can hold 10 electrons.
- The f-sublevel has 7 orbitals and can hold 14 electrons.
Filling Order and Exceptions
- The 4s sublevel is filled before the 3d sublevel due to lower energy.
- Hund's rule of maximum multiplicity states that electrons fill orbitals singly before pairing up in the same orbital.
- The Pauli Exclusion Principle states that an orbital can hold a maximum of two electrons with opposite spins.
Electronic Configuration of Elements
- Hydrogen: 1s1
- Sodium: 1s2, 2s2, 2p6, 3s1
- Scandium: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d1
- Vanadium: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d3
- Chromium: 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d5
- Nickel: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d8
- Copper: 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d10
- Zinc: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10
- Neodymium: [Xe] 4f4, 6s2
- Lead: [Xe] 4f14, 5d10, 6s2, 6p3
Electronic Configuration of Ions
- Cations are formed by removing electrons from the valence shell, following the order np, ns, (n-1)d.
- Example: Fe3+ (iron(III) ion) = [Ar]3d5
- Anions are formed by adding electrons to the valence shell to achieve the configuration of the next noble gas atom.
- Example: N3- (azide ion) = [He]2s2, 2px2, 2py2, 2pz2
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Description
Test your knowledge on electronic configuration, energy levels, and sublevels in atoms. This quiz covers key principles such as the Aufbau Principle, Hund's rule, and the Pauli Exclusion Principle. Challenge yourself to master the arrangement of electrons in various atomic orbitals.
