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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/Courses/University_of_Missouri/MU%3A__1330H_(Keller)/07._Periodic_Properties_of_the_Elements/7.3%3A_Sizes_of_Atoms_and_IonsIonic radii share the same vertical trend as atomic radii, but the horizontal trends differ due to differences in ionic charges. A variety of methods have been established to measure the size of a sin...Ionic radii share the same vertical trend as atomic radii, but the horizontal trends differ due to differences in ionic charges. A variety of methods have been established to measure the size of a single atom or ion. The covalent atomic radius (rcov) is half the internuclear distance in a molecule with two identical atoms bonded to each other, whereas the metallic atomic radius (rmet) is defined as half the distance between the nuclei of two adjacent atoms in a metallic element.
- https://chem.libretexts.org/Courses/Tennessee_State_University/CHEM_4210%3A_Inorganic_Chem_II_(Siddiquee)/04%3A_d-Block_Metal_Chemistry/4.01%3A_Properties_of_Transition_Metals/4.1.03%3A_General_Trends_among_the_Transition_MetalsTransition metals are characterized by the existence of multiple oxidation states separated by a single electron. Most transition-metal compounds are paramagnetic, whereas virtually all compounds of t...Transition metals are characterized by the existence of multiple oxidation states separated by a single electron. Most transition-metal compounds are paramagnetic, whereas virtually all compounds of the p-block elements are diamagnetic.
- https://chem.libretexts.org/Courses/City_College_of_San_Francisco/Chemistry_101A/Topic_E%3A_Atomic_Structure/08%3A_Periodic_Properties_of_the_Elements/8.02%3A_Shielding_and_Effective_Nuclear_ChargeThe calculation of orbital energies in atoms or ions with more than one electron (multielectron atoms or ions) is complicated by repulsive interactions between the electrons. The concept of electron s...The calculation of orbital energies in atoms or ions with more than one electron (multielectron atoms or ions) is complicated by repulsive interactions between the electrons. The concept of electron shielding, in which intervening electrons act to reduce the positive nuclear charge experienced by an electron, allows the use of hydrogen-like orbitals and an effective nuclear charge to describe electron distributions in more complex atoms or ions.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/Map%3A_Chemistry_-_The_Central_Science_(Brown_et_al.)/07%3A_Periodic_Properties_of_the_Elements/7.02%3A_Shielding_and_Effective_Nuclear_ChargeThe calculation of orbital energies in atoms or ions with more than one electron (multielectron atoms or ions) is complicated by repulsive interactions between the electrons. The concept of electron s...The calculation of orbital energies in atoms or ions with more than one electron (multielectron atoms or ions) is complicated by repulsive interactions between the electrons. The concept of electron shielding, in which intervening electrons act to reduce the positive nuclear charge experienced by an electron, allows the use of hydrogen-like orbitals and an effective nuclear charge to describe electron distributions in more complex atoms or ions.
- https://chem.libretexts.org/Courses/Lansing_Community_College/LCC%3A_Chem_151_-_General_Chemistry_I/Text/08%3A_Periodic_Properties_of_the_Elements/8.02%3A_Shielding_and_Effective_Nuclear_ChargeThe calculation of orbital energies in atoms or ions with more than one electron (multielectron atoms or ions) is complicated by repulsive interactions between the electrons. The concept of electron s...The calculation of orbital energies in atoms or ions with more than one electron (multielectron atoms or ions) is complicated by repulsive interactions between the electrons. The concept of electron shielding, in which intervening electrons act to reduce the positive nuclear charge experienced by an electron, allows the use of hydrogen-like orbitals and an effective nuclear charge to describe electron distributions in more complex atoms or ions.
- https://chem.libretexts.org/Courses/Widener_University/CHEM_145%3A_FA22_Van_Bramer/07%3A_Electronic_Structure_and_Periodic_Properties/7.05%3A_Periodic_Variations_in_Element_PropertiesElectron configurations allow us to understand many periodic trends. Covalent radius increases as we move down a group because the n level (orbital size) increases. Covalent radius mostly decreases as...Electron configurations allow us to understand many periodic trends. Covalent radius increases as we move down a group because the n level (orbital size) increases. Covalent radius mostly decreases as we move left to right across a period because the effective nuclear charge experienced by the electrons increases, and the electrons are pulled in tighter to the nucleus. Anionic radii are larger than the parent atom, while cationic radii are smaller.
- https://chem.libretexts.org/Under_Construction/Purgatory/AUCHE_212_General_Chemistry_II_Part_1_(Minhas)/03%3A_Periodic_Trends/3.04%3A_Periodic_Trends/3.4.03%3A_Effective_Nuclear_ChargeElectrons in s orbitals, even 4s or 5s, still spend some time right at the nucleus, and when they are there, they feel the full nuclear charge, so on average the s electrons feel a nuclear charge clos...Electrons in s orbitals, even 4s or 5s, still spend some time right at the nucleus, and when they are there, they feel the full nuclear charge, so on average the s electrons feel a nuclear charge closer to the actual nuclear charge.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/Map%3A_Chemistry_-_The_Central_Science_(Brown_et_al.)/07%3A_Periodic_Properties_of_the_Elements/7.03%3A_Sizes_of_Atoms_and_IonsIonic radii share the same vertical trend as atomic radii, but the horizontal trends differ due to differences in ionic charges. A variety of methods have been established to measure the size of a sin...Ionic radii share the same vertical trend as atomic radii, but the horizontal trends differ due to differences in ionic charges. A variety of methods have been established to measure the size of a single atom or ion. The covalent atomic radius (rcov) is half the internuclear distance in a molecule with two identical atoms bonded to each other, whereas the metallic atomic radius (rmet) is defined as half the distance between the nuclei of two adjacent atoms in a metallic element.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/07%3A_Approximation_Methods/7.03%3A_Trial_Functions_Can_Be_Linear_Combinations_of_Functions_That_Also_Contain_Variational_ParametersThis page explores variational methods in quantum mechanics, particularly the construction of wavefunctions using linear combinations of basis functions. It differentiates between normal and nonlinear...This page explores variational methods in quantum mechanics, particularly the construction of wavefunctions using linear combinations of basis functions. It differentiates between normal and nonlinear variational methods, emphasizing the computational advantages of the former. The significance of adjustable zeta parameters in modeling electron interactions, especially in multi-electron atoms, is highlighted.
- https://chem.libretexts.org/Courses/East_Tennessee_State_University/CHEM_3110%3A_Descriptive_Inorganic_Chemistry/02%3A_Atomic_Theory/2.02%3A_ShieldingThe presence of other electrons in an atom will shield an electron from feeling the full positive charge of the nucleus. The amount of screening is determined by the number other electrons and their l...The presence of other electrons in an atom will shield an electron from feeling the full positive charge of the nucleus. The amount of screening is determined by the number other electrons and their location.
