Atomic Structure , Electron Configuration Flashcards
What are the Properties of photons?
No mass (but has momentum)
Constant Speed (Speed of light , 3 X 10^8 )
What is the formula for the Energy of a Photon
E = Plancs Constant X Speed of Light / Wavelength
Describe Bohr’s model of the Atom
Electrons or Atoms exist in discrete energy levels.
An electron can only have a limited amount of energy
Descirbe the Quantum Mechanics Model of the atom
Considers Electrons as Waves delocalised in space but still of quantized energy (orbitals)
Waves move around the nucleus in a mathematical wave function
What are the four qualities that are used to specify an electrons state in the Quantum Mechanics Model
Energy level
Angular Momentum
Magnetic Moment
Spin
Define Electronegativity
The ability of an atom or molecule to attract its eletron density towards itself within a covalent bond
Ca (atomic number) = 20
Give the electron config for Ca2+
1s2 2s2 2p6 3s2 3p6
(4s2 is emptied first)
Explain the Pauli Exclusion Principle in the context of QMM and Bohr’s model
QMM: No two electrons in an atom can have the same set of four quantum numbers
Bohr: No more then two electrons can occupy the same orbital
Give the Electron Config of palladium - atomic number = 46
1s2 2s2 2p6 3s2 3p6 , 4s2 , 3d10 , 4p6 , 5s2 ,4D8
Explain the Trend of Atomic Radius across a period
Atomic Radius Decreases as you across a period
- More proton rich nucleus as you across a period
- Similar Shielding for all elements in that period
This means that the forces of attraction between the outermost orbital and nucleus increases pulling the orbital in closer
Explain the trend of Atomic Radius Down a group
Atomic radius increases as you go down a group
- More shielding due to extra electron shells
This means the nucleus and the outermost orbital are futher apart
