INORGANIC CHEMISTRY ACS: STUDY
GUIDE WITH COMPLETE SOLUTIONS
Ionization energy - Correct Answers -energy required to remove the least tightly bound
electron from a neutral atom in the gas phase
periodic trend of ionization energy - Correct Answers -highest at top right-smaller
electron=harder to remove
Why is a half filled subshell so stable? - Correct Answers -it serves to maximize the
stabilizing interactions while minimizing the destabilizing interactions among electrons
exchange interaction - Correct Answers -pie, stabilizing, result of electrons pairing in
degenerate orbitals with parallel spin
pairing energy - Correct Answers -destabilizing, coulomb interaction, pic, energy of
electron-electron repulsion in a filled orbital
Is it easier to ionize a high energy or low energy electrons - Correct Answers -high
energy electron-already contains more energy so it requires less energy input
What happens when a 3d series metal is ionized? - Correct Answers -the first electron
to be ionized will come from the 4s orbital, the other s electron will enter the d orbital
(4s03dn+1)
lanthanide contraction - Correct Answers -reduction in atomic radius following the
lanthanide series, contrary to the overall trend observed for the periodic table
lanthanides - Correct Answers -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
Slater's rules - Correct Answers -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)
Shielding - Correct Answers -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
,penetration - Correct Answers -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
electron affinity - Correct Answers -the difference in energy for a neutral gaseous atom,
and the gaseous anion. used interchangeably with electron gain enthalpy. more
positive=more stable EA with the additional electron, more positive EGE=more stable
with extra electron
Combination of electron affinity and ionization energy - Correct Answers -
electronegativity, overall measure of an atoms ability to attract electrons to itself when
part of a compound, fluorine has highest electronegativity
polarizability - Correct Answers -an atoms ability to be distorted by an electric field,
regions of a molecule can take on partial positive or partial negative charge
Why do we use the hydrogen system approximation - Correct Answers -systems
involving multiple electrons are much more complex, and they require the use of
quantum mechanics
What is the formula for the energy of a hydrogen orbital - Correct Answers -E=-
13.6(eV)*(Z^2/n^2), h is plancks constant (background on pg 4)
Energy can be expressed in... - Correct Answers -Joules, wavenumber, inverse
centimeters
quantum number N - Correct Answers -principle quantum number, defines energy and
size of orbital
quantum number L - Correct Answers -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.
quantum number Ml - Correct Answers -magnetic quantum number, describes the
orientation of the angular momentum, ml can have values of 0 to +/-1
quantum number Ms - Correct Answers -spin magnetic quantum number, defines
intrinsic angular momentum of an electron, Ms can have values of either +1/2 or -1/2
Radial wavefunction - Correct Answers -(R(r)), along with the angular wavefunction,
gives us the orbitals. With a wave function it is possible to completely characterize a
particle, goes to zero at infinity, produce characteristic shapes when graphed
Radial distribution function - Correct Answers -a plot of R^2(r)r^2, tells us probability of
finding an electron at a certain distance from the nucleus, every orbital has a different
radial distribution function and a node on the graph is a region of zero probability
, Bohr radius - Correct Answers -the most probably distance to find the electron in a one
proton, one electron system (52.9 pico-meters)
What orbitals correspond to l=0 through l=4 - Correct Answers -L=0=s, L=1=p, L=2=d,
L=3=f, L=4=g
Building up principle/Hund's rule - Correct Answers -when degenerate orbitals are
available for occupation, electrons occupy separate orbitals with parallel spin
Pauli exclusion principle - Correct Answers -no more than two electrons can occupy a
single orbital, and to do so, their spins must be paired
Descibe VSEPR - Correct Answers -purpose is to predict molecular geometries, basic
assumption is that regions of enhanced electron density take positions as far apart as
possible in order to minimize repulsive forces.
Relative repulsion strengths VSEPR - Correct Answers -lone pair> multiple bonds>
single bonds
Valence bond theory - Correct Answers -explains chemical bonding by considering the
overlap of tomic orbitals, wave patterns of atomic orbitals interfere constructively to form
a bond, sigma is formed when orbital overlap has cylindrical symmetry, pi bond forms
when they overlap side by side after the formation of a sigma bond
How is hybridization used in valence bond theory - Correct Answers -explains bonding
where the number of equivalent bonds exceeds the number of valence orbitals
Effect of a lone pair on geometry? - Correct Answers -it pushes strongly against all
other substituent. It is the strongest force governing the shape of a molecule
Molecular orbital theory - Correct Answers -an improvement over valence bond theory
in that the bonding description extends to all atoms in a molecule and handles
polyatomic molecules, atomic orbitals combine to form molecular orbitals which are
delocalized descriptions of electron distribution
MO theory assumptions - Correct Answers -orbital approximation, linear combinations
of atomic orbitals
Orbital approximation - Correct Answers -the wave function describing all of the
electrons of a molecule can be written as a product of the one electron avefunctions
linear combination of atomic orbitals - Correct Answers -the superposition of multiple
atomic orbitals of same type along with weighting coefficients
GUIDE WITH COMPLETE SOLUTIONS
Ionization energy - Correct Answers -energy required to remove the least tightly bound
electron from a neutral atom in the gas phase
periodic trend of ionization energy - Correct Answers -highest at top right-smaller
electron=harder to remove
Why is a half filled subshell so stable? - Correct Answers -it serves to maximize the
stabilizing interactions while minimizing the destabilizing interactions among electrons
exchange interaction - Correct Answers -pie, stabilizing, result of electrons pairing in
degenerate orbitals with parallel spin
pairing energy - Correct Answers -destabilizing, coulomb interaction, pic, energy of
electron-electron repulsion in a filled orbital
Is it easier to ionize a high energy or low energy electrons - Correct Answers -high
energy electron-already contains more energy so it requires less energy input
What happens when a 3d series metal is ionized? - Correct Answers -the first electron
to be ionized will come from the 4s orbital, the other s electron will enter the d orbital
(4s03dn+1)
lanthanide contraction - Correct Answers -reduction in atomic radius following the
lanthanide series, contrary to the overall trend observed for the periodic table
lanthanides - Correct Answers -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
Slater's rules - Correct Answers -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)
Shielding - Correct Answers -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
,penetration - Correct Answers -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
electron affinity - Correct Answers -the difference in energy for a neutral gaseous atom,
and the gaseous anion. used interchangeably with electron gain enthalpy. more
positive=more stable EA with the additional electron, more positive EGE=more stable
with extra electron
Combination of electron affinity and ionization energy - Correct Answers -
electronegativity, overall measure of an atoms ability to attract electrons to itself when
part of a compound, fluorine has highest electronegativity
polarizability - Correct Answers -an atoms ability to be distorted by an electric field,
regions of a molecule can take on partial positive or partial negative charge
Why do we use the hydrogen system approximation - Correct Answers -systems
involving multiple electrons are much more complex, and they require the use of
quantum mechanics
What is the formula for the energy of a hydrogen orbital - Correct Answers -E=-
13.6(eV)*(Z^2/n^2), h is plancks constant (background on pg 4)
Energy can be expressed in... - Correct Answers -Joules, wavenumber, inverse
centimeters
quantum number N - Correct Answers -principle quantum number, defines energy and
size of orbital
quantum number L - Correct Answers -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.
quantum number Ml - Correct Answers -magnetic quantum number, describes the
orientation of the angular momentum, ml can have values of 0 to +/-1
quantum number Ms - Correct Answers -spin magnetic quantum number, defines
intrinsic angular momentum of an electron, Ms can have values of either +1/2 or -1/2
Radial wavefunction - Correct Answers -(R(r)), along with the angular wavefunction,
gives us the orbitals. With a wave function it is possible to completely characterize a
particle, goes to zero at infinity, produce characteristic shapes when graphed
Radial distribution function - Correct Answers -a plot of R^2(r)r^2, tells us probability of
finding an electron at a certain distance from the nucleus, every orbital has a different
radial distribution function and a node on the graph is a region of zero probability
, Bohr radius - Correct Answers -the most probably distance to find the electron in a one
proton, one electron system (52.9 pico-meters)
What orbitals correspond to l=0 through l=4 - Correct Answers -L=0=s, L=1=p, L=2=d,
L=3=f, L=4=g
Building up principle/Hund's rule - Correct Answers -when degenerate orbitals are
available for occupation, electrons occupy separate orbitals with parallel spin
Pauli exclusion principle - Correct Answers -no more than two electrons can occupy a
single orbital, and to do so, their spins must be paired
Descibe VSEPR - Correct Answers -purpose is to predict molecular geometries, basic
assumption is that regions of enhanced electron density take positions as far apart as
possible in order to minimize repulsive forces.
Relative repulsion strengths VSEPR - Correct Answers -lone pair> multiple bonds>
single bonds
Valence bond theory - Correct Answers -explains chemical bonding by considering the
overlap of tomic orbitals, wave patterns of atomic orbitals interfere constructively to form
a bond, sigma is formed when orbital overlap has cylindrical symmetry, pi bond forms
when they overlap side by side after the formation of a sigma bond
How is hybridization used in valence bond theory - Correct Answers -explains bonding
where the number of equivalent bonds exceeds the number of valence orbitals
Effect of a lone pair on geometry? - Correct Answers -it pushes strongly against all
other substituent. It is the strongest force governing the shape of a molecule
Molecular orbital theory - Correct Answers -an improvement over valence bond theory
in that the bonding description extends to all atoms in a molecule and handles
polyatomic molecules, atomic orbitals combine to form molecular orbitals which are
delocalized descriptions of electron distribution
MO theory assumptions - Correct Answers -orbital approximation, linear combinations
of atomic orbitals
Orbital approximation - Correct Answers -the wave function describing all of the
electrons of a molecule can be written as a product of the one electron avefunctions
linear combination of atomic orbitals - Correct Answers -the superposition of multiple
atomic orbitals of same type along with weighting coefficients
