ch 7 Flashcards
what does the pauli exclusion says
no 2 e can have the same 4 quantum numbers and the two e in an orbital must have opposite spins
when is the shell more stable
the smaller it is the more stable
1 is more stable than 2 and so on
subshell stability
s is more stable than p and so on
s>p>d>f
energy of shells get closer together as n gets
larger
effective nuclear charge Z*
the larger Z*
the more stable it is
what is Z*
is the net force attraction experinced by the outermost electron in an atom
how many orbitals in s
1
how many orbitals in p
3
how many orbitals in d
5
How many orbitals in f
7
How to find the total number of orbitals in a given shell
n^2
what is the exception with the transition metal and d subshell
d subshells prefer to be totally filled or half filled rather than partially filled
the exceptions include everything under Cr and Cu (Mo, Ag, Au)
electron configuration for anions
Write out the electron configuration for neutral element
Fill in the desired number of electrons by adding electrons to the highest energy subshell
electron configuration for cations
write out the electron configuration for neutral element
remove the desired number of e from first removing from the highest n level and highest energy subshell.
isoelectronic species
same number of electrons and same electron configuration
what are the most stable ions of atoms?
the most stable ions of atoms are isoelectronic with noble gases or half filled shells.
Diamagnetic
all electrons are paired
paramagnetic
unpaired electrons will be attracted to a magnetic field
z effective nuclear charge
nuclear charge that is felt by the valence electron
electrons are attracted to the
nucleus. the closer they are, the stronger the attraction to the nucleus
nuclear shielding
inner electrons shield outer electrons from the attractive force of the nucleus
core electrons
electrons in the inner shell
valence electrons
electrons in the outermost shell
valence electrons are attracted and repelled by what
valence electrons are attracted by the positively charged nucleus and repelled by the core electrons
Zeff formula
Zeff = Z - S
Z=atomic number
S= # of core electrons
How does Zeff increases?
Up and right
To the righ Zeff
as we move to the right in the periodic table , the # of protons increases so Zeff increases because protons are positively charged and so the pulling effect is higher
Moving down Zeff
As we move down a group, the number of core shells increases so shielding increases and Zeff decreases
total e formula
total electrons= core + valence
valence electrons can be found in periodic table in family
total electrons is the element #
Atomic radius trend
Atomic radius increases down and to the left because as we go down the number of shells increases, Z eff decreases so the radius is larger.
Trend for atomic radius for cations
In cations, electrons are removed so it becomes more positive, therefore Zeff increases cause more pull and Atomic radius decreases.
Trend for atomic radius for anions
In anions, electrons are added so it becomes negative, therefore there is less pull so less Zeff and the atomic radius is larger.
comparing atomic radius between isoelectronic species
Isoelectronic species have the same number of electrons. To compare what AR is larger
compare the # of protons (equals to Z the atomic number in the periodic table)
more protons means stronger pull, wich means smaller AR
less protons than electrons means weaker pull and larger AR
Ionization energy trend
Increases up and right
what is ionization energy
How much energy is required to remove the outermost electron from an atom or ion in the gas phase
what electrons are easier to remove?
valence
Electron Affinity
It is the amount of energy involved with adding an electron to an ion or atom
What happens if Ea is negative
energy is released, it goes into a lower state, the atom is more stable and it likes to have an e added
what happens if Ea is positive
energy is absorbed, it goes into a higher energy state, the atom is less stable, it does not like to have an e added
Trend for Ea
Ea increases upwards and to the right
electronegativity trend
upwards and to the right
Most electronegative atoms
F>O>N>Cl>Br>I>S>C>H
electronegativity measures
the amount of e pull
