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- https://chem.libretexts.org/Sandboxes/khaas/Inorganic_Chemistry_II_(CHEM4210)/01%3A_Basic_Inorganic_Concepts/1.02%3A_Atomic_Structure/1.2.02%3A_The_Schrodinger_equation_particle_in_a_box_and_atomic_wavefunctions/1.2.2.04%3A_ShieldingConsequently, when an electron is in the small inner lobe of the 2s orbital, it experiences a relatively large value of Z*, which causes the energy of the 2s orbital to be lower than the energy of the...Consequently, when an electron is in the small inner lobe of the 2s orbital, it experiences a relatively large value of Z*, which causes the energy of the 2s orbital to be lower than the energy of the 2p orbital. This is because as Z increases by a small interval, the shell number increases, and so the electrons in the valence shell are much farther from the nucleus and are more shielded by all the electrons in the lower shell numbers.
- https://chem.libretexts.org/Under_Construction/Purgatory/AUCHE_230_-_Structure_and_Bonding/02%3A_Atomic_Orbitals/2.06%3A_Slater's_RulesSlater's rules allow you to estimate the effective nuclear charge from the real number of protons in the nucleus and the effective shielding of electrons in each orbital "shell" (e.g., to compare the ...Slater's rules allow you to estimate the effective nuclear charge from the real number of protons in the nucleus and the effective shielding of electrons in each orbital "shell" (e.g., to compare the effective nuclear charge and shielding 3d and 4s in transition metals). Slater's rules are fairly simple and produce fairly accurate predictions of things like the electron configurations and ionization energies.
- https://chem.libretexts.org/Courses/East_Tennessee_State_University/CHEM_4110%3A_Advanced_Inorganic_Chemistry/02%3A_Atomic_Structure/2.03%3A_Aufbau_Principle/2.3.01%3A_Shielding
- https://chem.libretexts.org/Courses/Lebanon_Valley_College/CHM_311%3A_Physical_Chemistry_I_(Lebanon_Valley_College)/05%3A_Many_Electron_Atoms/5.03%3A_The_Variational_Method_ApproximationIn this section we introduce the powerful and versatile variational method and use it to improve the approximate solutions we found for the helium atom using the independent electron approximation.
- https://chem.libretexts.org/Under_Construction/Purgatory/AUCHE_212_General_Chemistry_II_Part_1_(Minhas)/03%3A_Periodic_Trends/3.04%3A_Periodic_Trends/3.4.07%3A_Slater's_Rules_for_Effective_Nuclear_ChargeEffective nuclear charge determines the size and energy of orbitals, which determine most properties of atoms. Slater's rules give a simple approximation of effective nuclear charge, which depends on ...Effective nuclear charge determines the size and energy of orbitals, which determine most properties of atoms. Slater's rules give a simple approximation of effective nuclear charge, which depends on the number of electrons that might get between, so it depends on the electron we are looking at. For any electron, to find the effective nuclear charge it feels, we need to know how many other electrons might get in the way, and how much time it spends near the nucleus.
- https://chem.libretexts.org/Courses/Ursinus_College/CHEM322%3A_Inorganic_Chemistry/01%3A_Atomic_Structure/1.04%3A_Periodic_Properties_of_the_Elements/1.4.01%3A_Effective_Nuclear_ChargeA modified form of Coulomb's Law is written below, where e is the charge of an electron, Z* is the effective nuclear charge experienced by that electron, and r is the radius (distance of the e...A modified form of Coulomb's Law is written below, where e is the charge of an electron, Z* is the effective nuclear charge experienced by that electron, and r is the radius (distance of the electron from the nucleus). This is because as Z increases by a small interval, the shell number increases, and so the electrons in the valence shell are much farther from the nucleus and are more shielded by all the electrons in the lower shell numbers.
- https://chem.libretexts.org/Courses/Ursinus_College/CHEM322%3A_Inorganic_Chemistry/01%3A_Atomic_Structure/1.03%3A_Multi-Electron_Atoms/1.3.04%3A_Slater's_RulesSlater's rules allow you to estimate the effective nuclear charge from the real number of protons in the nucleus and the effective shielding of electrons in each orbital "shell" (e.g., to compare the ...Slater's rules allow you to estimate the effective nuclear charge from the real number of protons in the nucleus and the effective shielding of electrons in each orbital "shell" (e.g., to compare the effective nuclear charge and shielding 3d and 4s in transition metals). Slater's rules are fairly simple and produce fairly accurate predictions of things like the electron configurations and ionization energies.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/General_Chemistry_Supplement_(Eames)/Periodic_Trends/Slater's_Rules_for_Effective_Nuclear_ChargeEffective nuclear charge determines the size and energy of orbitals, which determine most properties of atoms. Slater's rules give a simple approximation of effective nuclear charge, which depends on ...Effective nuclear charge determines the size and energy of orbitals, which determine most properties of atoms. Slater's rules give a simple approximation of effective nuclear charge, which depends on the number of electrons that might get between, so it depends on the electron we are looking at. For any electron, to find the effective nuclear charge it feels, we need to know how many other electrons might get in the way, and how much time it spends near the nucleus.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Descriptive_Chemistry/Periodic_Trends_of_Elemental_Properties/Periodic_Trends_in_Ionic_RadiiAn understanding of periodic trends is necessary when analyzing and predicting molecular properties and interactions. Common periodic trends include those in ionization energy, atomic radius, and elec...An understanding of periodic trends is necessary when analyzing and predicting molecular properties and interactions. Common periodic trends include those in ionization energy, atomic radius, and electron affinity. One such trend is closely linked to atomic radii -- ionic radii. Neutral atoms tend to increase in size down a group and decrease across a period. When a neutral atom gains or loses an electron, creating an anion or cation, the atom's radius increases or decreases, respectively.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Instrumental_Analysis_(LibreTexts)/19%3A_Nuclear_Magnetic_Resonance_Spectroscopy/19.02%3A_Environmental_Effects_on_NMR_SpectraIn this section we will consider why the location of a nucleus within a molecule—what we call its environment—might affect the frequency at which it absorbs and why a particular absorption line might ...In this section we will consider why the location of a nucleus within a molecule—what we call its environment—might affect the frequency at which it absorbs and why a particular absorption line might appear as a cluster of individual peaks instead of as a single peak.
- https://chem.libretexts.org/Courses/BethuneCookman_University/BCU%3A_CH_332_Physical_Chemistry_II/Text/7%3A_Approximation_Methods/7.01%3A_The_Variational_Method_ApproximationIn this section we introduce the powerful and versatile variational method and use it to improve the approximate solutions we found for the helium atom using the independent electron approximation.
