1. Ionization energy energy required to remove the least tightly bound electron
from a neutral atom in the gas phase
2. periodic trend of ionization energy ANS >>> highest at top right-smaller
electron=harder to remove
3. Why is a half filled subshell so stable? ANS >>> it serves to maximize the
stabilizing interactions while minimizing the destabilizing interactions among
electrons
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, 4. exchange interaction ANS >>> pie, stabilizing, result of electrons pairing in
degenerate orbitals with parallel spin
5. pairing energy ANS >>> destabilizing, coulomb interaction, pic, energy of
electron-elec- tron repulsion in a filled orbital
6. Is it easier to ionize a high energy or low energy electrons ANS >>> high
energy electron-already contains more energy so it requires less energy input
7. What happens when a 3d series metal is ionized? ANS >>> the first
electron to be ionized will come from the 4s orbital, the other s electron will
enter the d orbital (4s03dn+1)
8. lanthanide contraction ANS >>> reduction in atomic radius following the
lanthanide se- ries, contrary to the overall trend observed for the periodic table
9. lanthanides ANS >>> elements 57-71, first appearance of f orbitals, f orbitals are
poor at shielding so any electrons dded will have a higher Zeff, shrinking the
radius
10. Slater's rules ANS >>> tell us what the effective nuclear charge will be,
Zeff=Z-sigma, Z is the atomic number, sigma=sum of the number of electrons in
a given subtle multiplied by a weighting coefficient (page 1)
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, 11. Shielding ANS >>> the reduction in charge attraction between the nucleus and
electrons due to electrons between the nucleus and the electron in question, it is
considered the be between if it has a lower energy
12. penetration ANS >>> when an electron of a higher atomic orbital is found within
the shell of electrons of a lower atomic number, that is to say that an electron of
higher energy is found within an orbital of lower energy
13. electron affinity ANS >>> the difference in energy for a neutral gaseous
atom, and the gaseous anion. used interchangeably with electron gain enthalpy.
more posi- tive=more stable EA with the additional electron, more positive
EGE=more stable with extra electron
14. Combination of electron affinity and ionization energy ANS >>>
electronegativity, overall measure of an atoms ability to attract electrons to
itself when part of a compound, fluorine has highest electronegativity
15. polarizability ANS >>> an atoms ability to be distorted by an electric field,
regions of a molecule can take on partial positive or partial negative charge
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, 16. Why do we use the hydrogen system approximation ANS >>> systems
involving multiple electrons are much more complex, and they require the use of
quantum mechanics
17. What is the formula for the energy of a hydrogen orbital ANS >>> -
E=-13.6(eV)*(Z^2/n^2), h is plancks constant (background on pg 4)
18. Energy can be expressed in... ANS >>> Joules, wavenumber, inverse
centimeters
19. quantum number N ANS >>> principle quantum number, defines energy and
size of orbital
20. quantum number L ANS >>> orbital angular momentum quantum number,
defines the magnitude of the orbital angular momentum, as well as the angular
shape of the orbital, L can have values of 0 to n-1.
21. quantum number Ml ANS >>> magnetic quantum number, describes the
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from a neutral atom in the gas phase
2. periodic trend of ionization energy ANS >>> highest at top right-smaller
electron=harder to remove
3. Why is a half filled subshell so stable? ANS >>> it serves to maximize the
stabilizing interactions while minimizing the destabilizing interactions among
electrons
mailto:https://www.stuvia.com/en-us/user/techgrades
, 4. exchange interaction ANS >>> pie, stabilizing, result of electrons pairing in
degenerate orbitals with parallel spin
5. pairing energy ANS >>> destabilizing, coulomb interaction, pic, energy of
electron-elec- tron repulsion in a filled orbital
6. Is it easier to ionize a high energy or low energy electrons ANS >>> high
energy electron-already contains more energy so it requires less energy input
7. What happens when a 3d series metal is ionized? ANS >>> the first
electron to be ionized will come from the 4s orbital, the other s electron will
enter the d orbital (4s03dn+1)
8. lanthanide contraction ANS >>> reduction in atomic radius following the
lanthanide se- ries, contrary to the overall trend observed for the periodic table
9. lanthanides ANS >>> elements 57-71, first appearance of f orbitals, f orbitals are
poor at shielding so any electrons dded will have a higher Zeff, shrinking the
radius
10. Slater's rules ANS >>> tell us what the effective nuclear charge will be,
Zeff=Z-sigma, Z is the atomic number, sigma=sum of the number of electrons in
a given subtle multiplied by a weighting coefficient (page 1)
mailto:https://www.stuvia.com/en-us/user/techgrades
, 11. Shielding ANS >>> the reduction in charge attraction between the nucleus and
electrons due to electrons between the nucleus and the electron in question, it is
considered the be between if it has a lower energy
12. penetration ANS >>> when an electron of a higher atomic orbital is found within
the shell of electrons of a lower atomic number, that is to say that an electron of
higher energy is found within an orbital of lower energy
13. electron affinity ANS >>> the difference in energy for a neutral gaseous
atom, and the gaseous anion. used interchangeably with electron gain enthalpy.
more posi- tive=more stable EA with the additional electron, more positive
EGE=more stable with extra electron
14. Combination of electron affinity and ionization energy ANS >>>
electronegativity, overall measure of an atoms ability to attract electrons to
itself when part of a compound, fluorine has highest electronegativity
15. polarizability ANS >>> an atoms ability to be distorted by an electric field,
regions of a molecule can take on partial positive or partial negative charge
mailto:https://www.stuvia.com/en-us/user/techgrades
, 16. Why do we use the hydrogen system approximation ANS >>> systems
involving multiple electrons are much more complex, and they require the use of
quantum mechanics
17. What is the formula for the energy of a hydrogen orbital ANS >>> -
E=-13.6(eV)*(Z^2/n^2), h is plancks constant (background on pg 4)
18. Energy can be expressed in... ANS >>> Joules, wavenumber, inverse
centimeters
19. quantum number N ANS >>> principle quantum number, defines energy and
size of orbital
20. quantum number L ANS >>> orbital angular momentum quantum number,
defines the magnitude of the orbital angular momentum, as well as the angular
shape of the orbital, L can have values of 0 to n-1.
21. quantum number Ml ANS >>> magnetic quantum number, describes the
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