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The electronic configuration of elements indicates the arrangement of __________ in an atom.
electrons
The first energy level can hold a maximum of __________ electrons.
2
The electron configuration for sodium (Na) is __________.
2,8,1
The __________ shell is the outermost energy level of an atom.
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In electron configuration, the __________ principle states that electrons fill the lowest energy levels first.
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For argon (Ar), the electron configuration is __________.
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The maximum number of electrons that can fit in the p-sublevel is __________.
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The __________ sublevel is filled before the 3d sublevel because it has a lower energy.
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Lithium (Li) has an electron configuration of __________.
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The d-sublevel can accommodate a maximum of __________ electrons.
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The electronic configuration of sodium (Na) is 1s2, 2s2, 2p6, 3s______.
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According to the Pauli Exclusion Principle, no more than two electrons may occupy a ______ and they must have opposite spin.
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Hund's rule states that when orbitals of ______ energy are available, electrons occupy them singly before pairing up.
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The electronic configuration for chromium (Cr) is 1s2, 2s2, 2p6, 3s2, 3p6, 4s______, 3d5.
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Iron, when in a +3 oxidation state, has an electronic configuration of [Ar]3d______.
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Carbon forms a monoatomic anion (C4-) by adding enough electrons to achieve the configuration of the next noble gas atom, which is ______.
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The electronic configuration of cobalt (Co) is [Ar]3d______4s2.
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The electronic configuration of lead (Pb) can be written as [Xe]4f14, 5d10, 6s2, ______.
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In nitrogen (N), the electronic configuration is [He]2s2, 2px1, 2py1, and ______.
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Copper (Cu) has the electronic configuration of 1s2, 2s2, 2p6, 3s2, 3p6, 4s______, 3d10.
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Study Notes
Electronic Configuration of Atoms
- The number of electrons in each main energy level is called the electronic configuration.
- The outermost shell of an atom is called the valence shell. The electrons in this shell are called valence electrons.
- The arrangement of electrons in an atom can be represented using a shorthand notation with subscripts for each shell. For example, the electronic configuration of helium (He) is 1s2, indicating that there are two electrons in the first shell.
Sublevels and Orbitals
- There are four main sublevels in an atom: s, p, d, and f.
- Each sublevel contains a specific number of orbitals, which are three-dimensional regions of space where an electron is likely to be found.
- The number of electrons in each sublevel is limited:
- s: 2 electrons (1 orbital)
- p: 6 electrons (3 orbitals)
- d: 10 electrons (5 orbitals)
- f: 14 electrons (7 orbitals)
Aufbau Principle
- The Aufbau Principle states that electrons fill the lowest energy levels first.
- The 4s sublevel is lower in energy than the 3d sublevel, therefore the 4s sublevel is filled before the 3d sublevel.
Hund's Rule
- Hund's Rule states that when two or more orbitals of equal energy are available, electrons will fill them individually before pairing up.
Pauli Exclusion Principle
- The Pauli Exclusion Principle states that an orbital can only hold a maximum of two electrons, and these electrons must have opposite spins.
Electronic Configuration of Ions
- Cations: Positively charged ions, formed by removing electrons.
- Anions: Negatively charged ions, formed by adding electrons.
- The order of electron removal in cations is: np, ns, (n-1)d.
- Monoatomic anions are formed by adding enough electrons to the valence shell to achieve the configuration of the next noble gas atom.
###Examples:
- Nitrogen (N): 7 electrons, electronic configuration: 1s2 2s2 2p3
- Nitrogen anion (N3-): Gains three electrons to achieve the electronic configuration of neon: 1s2 2s2 2p6
Filling Orbitals:
- The order of filling orbitals can be illustrated by a diagram like this:
- 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6d, 7s...
Conclusion
- The electronic configuration of an atom describes the distribution of electrons in its various energy levels and sublevels.
- This concept is fundamental to understanding chemical bonding and other aspects of chemistry.
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Description
This quiz covers the electronic configuration of atoms, including the arrangement of electrons in various energy levels and sublevels. It also explains the Aufbau Principle, which dictates the filling order of electron orbitals. Test your understanding of these fundamental concepts in atomic structure.
