ACS INORGANIC CHEMISTRY STUDY GUIDE
Questions and Answers
1.Ionization energy
ANS 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
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)
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
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 orientation of the
angular momentum, ml can have values of 0 to +/-1
22.quantum number Ms
ANS spin magnetic quantum number, defines intrinsic angular
momentum of an electron, Ms can have values of either +1/2 or -1/2
23.Radial wavefunction
ANS (R(r)), along with the angular wavefunction, gives us the orbitals.
Questions and Answers
1.Ionization energy
ANS 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
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)
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
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 orientation of the
angular momentum, ml can have values of 0 to +/-1
22.quantum number Ms
ANS spin magnetic quantum number, defines intrinsic angular
momentum of an electron, Ms can have values of either +1/2 or -1/2
23.Radial wavefunction
ANS (R(r)), along with the angular wavefunction, gives us the orbitals.
