De broglie
All matter has wave like properties you can calculate
¥=h/mv
Evidence electrons are waves
The diffraction pattern of it passing through aluminum foil is the same as a X-ray
Heisenberg uncertainty principle
You can’t accurately measure Both the position and momentum(or energy or velocity) of a small particle
Schrödinger
-by treatiing electrons as waves derived by mathematical descriptions of the energies and probabilities of electrons
Atomic orbitals
Regions of high probability for finding electrons 90%
Aufbau principle
Electrons occupy lowest level orbitals first
Hunds rule
Electrons occupy orbitals of the same energy singly
Isoelectronic series
Same electron configuration but diff numbers of protons
Ionization energy
Energy required to remove an electron from an atom in the gas phase
Ionization energy on the table
⬇️decreases(electrons are further from nucleus)
➡️increases(slight repulsion when e are paired)
Ionization energies are affected by..
- size of atom/ion
- size of positive charge
- the shell the e is removed from
Chemical reactions
- Involved rearrangements of valence electrons
- element never changes
Nuclear reactions
- involve nucleus
- often result in change of element
- fusion, fission, and radioactive decay
- change in mass
Fusion
- 2 small things makes one large thing
- needs high temperature
- requires a lot of energy to over come electrostatic repulsion
Nuclear fission
The fragmentation of heavy nuclei to form lighter more stable ones+ energy
Ldfs and covalent bond similarities
Causes-electrostatic attraction if the electrons and nuclei of other atoms
Ldfs and covalent bond differences
- magnitude of attraction
- how the electrons are arranged
Frequency
Number of wavefronts per second (hz, 1/s)
Bohr
- electrons move in orbits that have definite energys and distances
- only works for hydrogen
light is a particle bc…
photoelectric effect
photoelectric effect
Light shines on a metal and an electron is emitted depending on frequency and intensity(threshold frequency)
