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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/Earlham_College/CHEM_361%3A_Inorganic_Chemistry_(Watson)/01%3A_Intro_Review_and_Effective_Nuclear_Charge/1.02%3A_Atomic_Structure/1.2.02%3A_The_Schrodinger_equation_particle_in_a_box_and_atomic_wavefunctions/1.2.2.04%3A_Shielding
- 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.
- https://chem.libretexts.org/Courses/Tennessee_State_University/Inorganic_Chemistry_(CHEM_5000_4200)/01%3A_Map-_Inorganic_Chemistry-I_(LibreTexts)/02%3A_Atomic_Structure/2.02%3A_The_Schrodinger_equation_particle_in_a_box_and_atomic_wavefunctions/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_California_Davis/Chem_124A%3A_Fundamentals_of_Inorganic_Chemistry/02%3A_Atomic_Structure/2.02%3A_The_Schrodinger_equation_particle_in_a_box_and_atomic_wavefunctions/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/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/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/Tennessee_State_University/CHEM_4210%3A_Inorganic_Chem_II_(Siddiquee)/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/Kutztown_University_of_Pennsylvania/CHM_320%3A_Advanced_Inorganic_Chemistry_textbook/02%3A_Atomic_Structure/2.02%3A_The_Schrodinger_equation_particle_in_a_box_and_atomic_wavefunctions/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/Centre_College/CHE_332%3A_Inorganic_Chemistry/02%3A_Atomic_Theory/2.03%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.
- https://chem.libretexts.org/Courses/Northern_Michigan_University/CH_215%3A_Chemistry_of_the_Elements_Fall_2023/01%3A_Atoms_and_Electronic_Structure/1.15%3A_Effective_Nuclear_Charge_and_ShieldingCoulomb's Law is from classical physics; it tells us that particles with opposite electrostatic charge are attracted to each other, and the larger the charge on either particle or the closer the dista...Coulomb's Law is from classical physics; it tells us that particles with opposite electrostatic charge are attracted to each other, and the larger the charge on either particle or the closer the distance between them, the stronger the attraction. Coulomb's law is insufficient for predicting the energies of electrons in multi-electron atoms and ions. To explain these things, we need to consider how both electron shielding and penetration result in variations in effective nuclear charge (Z*) that
