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What is effective nuclear charge (Zeff)?
What is effective nuclear charge (Zeff)?
The actual nuclear charge experienced by an electron, defined as the charge of the nucleus plus the charge of the shielding electrons.
What is the formula to calculate Zeff?
What is the formula to calculate Zeff?
Zeff = Z - S
What does 'location' refer to in the context of effective nuclear charge?
What does 'location' refer to in the context of effective nuclear charge?
The radius of the orbital.
What is the shielding effect?
What is the shielding effect?
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What are valence electrons?
What are valence electrons?
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Zeff increases as you move _____ and ____ along a periodic table.
Zeff increases as you move _____ and ____ along a periodic table.
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Atomic radius increases as you move ____ and ____ along a periodic table.
Atomic radius increases as you move ____ and ____ along a periodic table.
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Study Notes
Effective Nuclear Charge
- Effective nuclear charge (Zeff) is the net positive charge experienced by an electron in an atom.
- Defined as the actual nuclear charge of the nucleus adjusted for the shielding effect caused by inner electrons.
Calculation of Zeff
- The formula to calculate Zeff is Zeff = Z - S.
- Z represents the number of protons in the nucleus (atomic number).
- S denotes the number of non-valence (inner) electrons.
Location
- Refers to the radius of the orbital where the electrons are located within the atom.
Shielding Effect
- The shielding effect occurs when inner electron layers reduce the pull of the nucleus on outer electrons.
- The efficiency of shielding is ranked in the following order: S > P > D > F, with S orbitals being most effective.
Valence Electrons
- Valence electrons are found in the outermost energy level of an atom and are crucial for chemical bonding.
Trends in Effective Nuclear Charge
- Zeff increases when moving up and to the right on the periodic table, indicating stronger attraction between nucleus and outer electrons.
Trends in Atomic Radius
- Atomic radius increases when moving down and to the left on the periodic table, due to added energy levels and reduced effective nuclear charge at lower positions.
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Description
Test your understanding of effective nuclear charge and its implications in atomic structure. This quiz covers key concepts, calculations, and the influence of shielding on electron behavior. Perfect for students studying chemistry and atomic theory.
