Studied by 0 peoplemass of 1 proton
1 amu
the number of electrons is equal to the number of
protons
protons + neutrons =
atomic mass / mass number
atomic weight
-constant
-avg of all the diff isotopes
Z
atomic number
A
mass number
hydrogen isotopes
-protium
-deuterium
-tritium
protium
hydrogen isotope with 1 proton
deuterium
hydrogen isotope with 1 proton and 1 neutron
tritium
hydrogen isotope with 1 proton and 2 neutrons
isotopes exhibit similar __ but different _
properties, mass
longer half life = more/less abundant
more
half life corresponds with
stability
avogadro’s number
6.02 × 10²³
energy of a quantum formula
E = hf
h
planks constant
planks constant
6.626 × 10^-34
f (sometimes v)
frequency of radiation
angular momentum of an electron orbiting a hydrogen nucleus formula
L = (nh)/(2π)
n
principal quantum number (any pos integer)
energy of an electron formula
E = - (R_H) / (n²)
R_H
rydberg unit of energy
rydberg unit of energy
2.18 × 10^-18
energy of an electron increases/decreases the farther from the nucleus it is
increases (n increases)
ground state of an atom
n=1
state of lowest energy
room temperature
excited state of atoms
-caused by heat or other energy
-when at least 1 electron moves to higher energy subshell
-brief
electromagnetic energy of photons formula
E = (hc) / λ
c
speed of light in a vacuum
speed of light in a vacuum
3.00 × 10^8 m/s
λ
wavelength of the radiation
line spectrum
each line on the emission spectrum corresponds to a specific electron transition
atomic emission spectrum
a fingerprint for element
(each element can have electrons excited to dif levels)
lyman series
the group of hydrogen emission lines corresponding to transitions from energy levels in n >= 2 to n=1
balmer series
the group of hydrogen emission lines corresponding to transitions from energy levels in n >= 3 to n=2
paschen series
the group of hydrogen emission lines corresponding to transitions from energy levels in n >= 4 to n=3
energy of emitted photon corresponds to dif in energy between __ and _
n_i and n_f
absorption spectrum
exciting the electrons results in energy absorption at specific wavelengths
wavelengths of absorption =
= wavelengths of emission
for electrons to move levels
must absorb exact right amount of energy
energy transition of valence electron formula
E = R_H [ (1/n_i²) - (1/n_f²) ]
energy state
the position and energy of an electron described by its quantum numbers (n, l, m_l, m_s)
values of the quantum numbers give info about the ____ of the orbitals
size, shape, and orientation
larger n =
= higher energy level and higher radius of electron’s shell
maximum number of electrons per shell formula
2n²
l
azimuthal quantum number (angular momentum)
azimuthal quantum number refers to
shape and number of subshells within a given principal energy level
azimuthal quantum number can be __ or _
0 or n-1
spectroscopic notation
l=0=s
l=1=p
l=2=d
l=3=f
l value increase =
= subshell energies increase
maximum number of electrons in a subshell formula
4l+2
M_l
magnetic quantum number
magnetic quantum number
the orbital within a subshell where an electron is found at a given moment
max electrons per M_l orbital
2
M_l can be equal to or between
-l and +l
s subshell shape
spherical
p subshell shape
dumbell
M_s
spin quantum number
the 2 spin orientations of M_s
+1/2 and -1/2
if 2 electrons are in the same orbital
spin opposite directions
if electrons in different orbitals have same M_s value
spin parallel
lower value of n+l
lower energy of subshell
if 2 subshells have same n+l value
lower n = lower energy and will fill w electrons first
s subshell max electrons
2
p subshell max electrons
6
d subshell max electrons
10
f subshell max electrons
14
anions
-negatively charged ions
-have additional electrons
cations
-positively charged ions
-remove electrons from subshells w highest n value and highest l value among these
orbitals per subshell formula
2l+1
hunds rule
within a subshell, orbitals are filled so that there are a max number of half filled orbitals
subshells may be listed in the order they fill or by
grouping same n together
half-filled and fully filled orbitals have
lower energy (more stable)
maximum number of electrons in an orbital formula
2n²
number of orbitals in a shell formula
n²
paramagnetic
-magnetic
-unpaired electrons
diamagnetic
-repels magnetic
-paired electrons
valence electrons
electrons in outermost shell of atom
most easily removed electrons
valence electrons
electrons available for bonding
valence electrons
electrons that dominate chemical behavior of atom
valence electrons
octet rule
atoms tend to have 8 valence electrons
when atoms have less than 8 valence electrons
react to become more stable
all elements in period 3 and below (octet rule)
can hold more than 8 electrons in valence shell
Note 
Flashcard (128)