Chapter 5 Flashcards
(34 cards)
What could Rutherford’s model not explain?
It could not explain the chemical properties of electrons.
Bohr Model
Proposed that an electron is found in specific paths called orbits around the nucleus.
Energy Levels
Fixed energies of electrons.
Like rungs of a ladder, the bigger the number the further it was from the nucleus.
Quantum Mechanical Model
Used a mathematical equation describing the behavior of the electron.
Atomic Orbital
Where the electron possibly is.
- s
Sphere
1 possible shape
2 possible electrons
- p
Dumbell
3 possible shapes
6 possible electrons
- d
Clover
5 possible shapes
10 possible electrons
- f
Quadrants
7 possible shapes
14 possible electrons
How many electrons can each possible shape have?
2 electrons
Where does change proceed?
In the lowest possible energy.
Aufbau Principle
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s
Pauli Exclusion Principle
Electrons have opposite spins.
Hunds Rule
Must count the first electron before the second.
What group does not follow the rule?
Transition Metals
What did the Quantum Mechanical Model grow from?
The study of light.
Amplitude
The height from the origin to the crest.
Wavelength
Distance between crests.
Frequency
Nuber of wave crests that pass a given point.
Crest
The highest point.
What do frequency and wavelength equal?
A constant speed of light.
Constant
C = Frequency x Wavelength C = 2.998x10⁸
When do atoms emit light?
When an electron loses energy.
Atomic Emissions Spectrum
The light emitted by an element separated into discrete lines.
Like a fingerprint, no two are the same.
