KA2- Atoms and the Periodic Table Flashcards
monochromatic
definition
radiation composed of only one wavelength
explain Bohr’s model
A photon of light is absorbed when an electron changes from one energy level to another
Absorbsion spectroscopy
what is happening to the electrons?
they are being promoted to a higher energy level
Emission Spectroscopy
what is happeing to the electrons?
they become excited and drop down from higher energy levels
What would an emission spectroscopy show if it was an atom with less electrons?
there would be less lines as there are less transferrs possible
What are the 4 quantum numbers?
- Principal
- Angular Momentum
- Magnetic
- Spin
1st QN
name, notation, what it determines
- Principal
- n
- size of orbital
2nd QN
name, notation, how to determine the range and what it determines
- angluar momentum
- l (lower case L)
- 0 to n-1
- shape of subshell
3rd QN
name, notation, how to determine an answer and what it determines
- magnetic
- ml
- ml= -l to +l and any whole number in between
- determines location of electron in terms of which subshell the electron is in
4th QN
name, notation, values and what it determines
- spin
- ms
- only 2 values: -1/2 or +1/2
- the direction the electrons are spun either clockwise (+1/2) or anti-clockwise (-1/2)
why are electrons alsways differnt from one another?
no 2 electrons can have the same set of Quantum Numbers in a subshell
What is the Pauli Exclusion Principal?
“No two electrons in any one atom can have the same 4 quantum numbers”
What is Hund’s rule?
“Electrons will occupy degenerate orbitals singly and with parallel spins before pairing”
What is the Aufbau Principle?
“Electrons will fill atomic orbitals in increasing order of energy”
What is the order of in which electrons fill orbitals?
1s, 2s, 2p, 3s, 3p, 4s, 3d
