Chapter 5 Electrons (Rutherford's atomic model couldn't explain…
Chapter 5 Electrons
Rutherford's atomic model couldn't explain the chemical properties of elements.
The Bohr: an electron is found in only specific orbits around the nucleus. (energy levels)
Quantum of energy is the mount of energy needed to move an electron from one level to another.
Quantum Mechanical Model:Erwin Schrodinger, restricts the energy of electrons to certain values, bud does NOT involve an exact path the electron takes around the nucleus
Aufbau: electrons occupy orbits of the lowest energy level first
Pauli:an atomic orbital may at most describe 2 electrons
Hund:electrons occupy orbitals to the same energy in a way that makes the # of electrons with the same spin direction as large as possible
Atomic orbitals: region where you will most likely find electron.
Each energy sub level corresponds to an orbital
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f ,5d, 6p, 5f, 6d
Electron configuration:Carbon:1s2, 2s2, 2p2
Maximum number electrons each sub level:s2, p6, d10, f14
Maximum number of orbitals:s1, p3, d5, f7
Noble gas configuration:Carbon:[He]2s2,2p2
when an electron moves closer to the nucleus the energy gets higher and larger.
Elements burn different colors because the electrons fall back to lower levels
Heisenberg's principle- you cannot know either distance or velocity of a particle
L to R Frequency larger, L to R Wavelength smaller
When an electron makes a jump 3 or less low energy, 5 high energy
an atom is stable when protons and electrons are equal, and it is at its lowest.