Electron Configuration And Lewis Structures Flashcards
binding energy depends on
n and l
difference in binding energy due to having a multi electron system
based on z effective, not z
Hunds Rule
when e- are added to states if the same energy, a single electron enters each state before a second does
paramagnetic
energy state has an unpaired electron
diamagnetic
no unpaired electron
most stable electron configurations
filled or 1/2 filled
aufbau principle
fill energy state 1 at a time, starting with fhe lowest energy
anion
ion that gained an electron and has a negative charge
cation
ion that lost an electron and is positively charged
transition metals lose what first
4s
relationship between IE2 and IE
IE2 is always greater than IE
when an ion is by itself charge =
oxidation state
isoelectronic
same electron configuration
Zeff
effective nuclear charge
Zeff trend (and why)
▪ increase across periodic table (bc more protons)
▪decrease down periodic table (bc n inc)
ionization energy is always a ______ value
positive
ionization energy trends
▪inc across periodic table
▪dec down periodic table
Electron affinity
ability of an atom to gain electrons
electron affinity = -______
change in energy
positive electron affinity means
atom wants an electron
electron affinity trends (and why)
▪inc across periodic table
▪dec going down
▪bc Zeff
electronegativity
the net ability of an atom to attract an electron from another atom
electron acceptor
atom with high electronegativity
electron donor
atom with low electronegativity
electronegativity trends
▪inc across
▪dec down
msot electronegative element
flourine
noble gas electronegativity
0
atomic radius trend (and why)
▪Dec across period table (bc Zeff inc)
▪inc down periodic table (bc n inc)
electronegativity inc by what amount across the periodic table?
.5
difference of electronegativity causes
a polar molecule
ionic bonds
transfer of one or more electrons from one atom to another with a bond
ionic bonds are caused by
coulombic attraction
covalent bonding
▪a pair of electrons are shared between 2 atoms
on covelnt bond graph, the x intercept =
bond length (sharing electrons at a good distance)
on covelent binding graph, difference between x intercept and asymptote =
dissociation energy
dissociation energy
energy required to seperate bonded atoms
deeper well in covalent bonding graph=
stronger bond
energy of interaction
nuclear-nuclear repulsion + electron-nucleur attraction + electron-electron repulsion
polar covalent
unequal sharing of electrons between 2 atoms w a different electronegativities
difference between electronegativities to form a polar covalent bond
.4 < x< 1.7
octet rule
electrons distributed in such a way that each element is surrounded by 8 electrons
coreect lewis structure has the ________ formal charge
least complicated
if a lewis structure only has single bonds it has no ______
resonance structures
octet rule exceptions
▪odd number of electrons
▪octet deficient molecules
▪valence shell expansion
radical species
molecules with an unpaired electron
valence shell expansion
element with n greater than or equal to 3 can have more than 8 electrons around the central atom
ionic bonds are between a
mental and nonmetal
less than an octet most often occurs with the elements
▪Boron (B)
▪Beryllium (Be)
▪aluminum (Al)
covalent bondimg occurs between
2 nonmetals
orbital filling exceptions
Cr, Cu
Cr electron configuration
▪6 total electrons
▪4s orbital filled with one
▪3d each filled with one
Cu electron configuration
▪11 total electrons
▪4s with 1
▪3d completely filled
group with the highest electron affinity
halides
methyl group
CH3
