Chapter 1 – atomic structure Flashcards
Atomic number
Equal to the number of protons in an atom
Mass number
Equal to the total number of protons and neutrons in an atom
Isotope
Atoms with varying numbers of neutrons.
Valence electrons
Electrons on the outer most shell of an atom, and have the strongest interactions with the surrounding environment.
Cat ion
Cat = good, positively charged atom caused by the removal of an electron
An ion
A negatively charged atom Caused by an additional electron.
Hydrogen isotopes
Deuterium
Tritium
Protium
- 1 proton, 1 neutron,
- 1 proton, 2 neutrons
- 1 proton, 0 neutrons
Atomic weight
The weighted average of different isotopes.
Max Planck’s energy equation
E=h(plancks constant) * f (frequency)
Planck’s constant
6.62610^-34js
Bohr’s electron angular momentum model
L= (ring #)(h)/(2pi)
Bohr’s energy equation
E=-(RH)/(n^2)
RH(rydberg’s constant)=2.18*10^-18
Ground state
State at which all electrons are in the lowest energy state
Excited state
When at least one electron has moved to a sub shell of a higher than normal energy
Energy equation based on photon emission
E=hc/wavelength
c is speed of light = 3*10^8
Lyman series
Electron drop from n>=2 to n=1
Balmer series
Energy drop from n>=3 to n=2
Paschen series
Energy drop Fromm>=4 to n=3
Heisenberg uncertainty principle
Momentum and position of an electron cannot be simultaneously found.
Quantum numbers and the pauli exclusion principle
Location of electrons can be given by their quantum number, and the exclusion principle states that new two electrons in a single atom can possess the same set of quantum numbers.
Principal quantum number
n given by the Energy level at the electron is on.
Azimuthal Quantum Number
( lower case L) can be any integer value les than or = to n-1
n=2 L=1 OR 0
n=1 L=0
Spectroscopic notation
Notation of L quantum number L=0=s L=1=p L=2=d L=3=f
Magnetic quantum number
Specifies the specific orbital that an electron is in given in values of negative L to positive L (-L,0,+L) L=2(-2,-1,0,1,2) P has 3 specific orbitals D has 5 specific orbitals Etc.
Spin quantum number
+1/2 or -1/2
Spin of electron within orbital
Paired electrons
Two electrons within the same orbital that have opposite quantum spin numbers(+,-)
Parallel spin electrons
Electrons in different orbitals on the same energy level that have the same spin value(both + or both -)
Equation for the maximum number of electrons within a sub shell
4L+2
Equation for the maximum number of electrons within a shell
2n^2
Electron configuration
Spectroscopic notation used to identify how electrons are configured within an atom.
Aufbau principal
Electrons Phil lower the higher energy subshells 2S before 2P an 2P before 3s
n+L rule
Lower n+L will be filled first
6s = 5+0
4d =4+2
Anion electron configuration
Additional electrons are added to the configuration
2s2 2p5 -> 2s2 2p6
Cat ion electron configuration
Electrons are removed from the highest value for n first, then highest L.
Hund’s rule
Orbitals are filled so that there a maximum number of half filled orbitals with parallel spin
Unpaired electrons cause materials to be paramagnetic
Materials will spin and orient in alignment with a magnetic field
Materials with pair of electrons will be diamagnetic
Have a slight repulsion to a magnetic field
