Electron arrangement - Ch3 Flashcards
SPECTROMETER
To observe line emission (identify elements).
FLAME TESTS
Soaked wooden splints + blue flame in bunsen burner. (CATION TESTS)
Li FLAME COLOUR
Red
Sr FLAME COLOUR
Red
Na FLAME COLOUR
Yellow / orange
Cu FLAME COLOUR
Blue / green
Ba FLAME COLOUR
Green
K FLAME COLOUR
Lilac
ATOMIC ORBITAL
Region in space where an electron is likely to be found.
S ORBITAL SHAPE
Spherical
P ORBITAL SHAPE
Dumbbell
SUBLEVEL
SUbdivision of a main energy level and consists on one or more orbitals of the same energy.
BOHR’S THEORY
- Electrons occupy the lowest available energy level (ground state) where their energy is fixed
- When provided with energy by heat or electricity, they jump to higher energy levels (excited state)
- They become unstable and fall back down to lower energy levels releasing energy in the form of a photon of light
- Each element has a unique number of electrons, a unique set of transition which gives off a unique spectra
- E2 - E1 = Hf
LYMAN, BALMER AND PASSION
Lyman: UV
Balmer: visible
PASSION: IR
AAS
Atomic absorption spectrometry:
- Used to detect heavy metals in water
DE BROGLIE
Electrons travel in a wave-like motion
HEISENBERG’S UNCERTAINTY PRINCIPLE
You cannot measure both the velocity and position of an electron at the same time.
LIMITATIONS OF BOHR’S
- Didn’t take into account that lectrons travel in a wave-like motion
- Didn’t take into account Heisenberg’s
- Only works perfect with H2 (Hydrogen)
ENERGY LEVEL
Fixed energy value that an electron in an atom may have
