Unit 5/6- Electrons & Trends Flashcards
Frequency
The number of waves that pass per second
Nodes
Where the wave passes through the origin
Longest waves=_____ frequency=______energy
Shorter waves=______frequency=______energy
Longer waves, lowest frequency,lowest energy
Shortest waves, higher frequency, highest energy
S orbitals
Spherical
1 orbital orientation
P orbital
Dumbbell shape
3 orbital orientation
D orbitals
Clover shaped
5 orbital orientations
F orbitals
Different shapes
7 orbital orientations
Absorbtion
A photon gets absorbed
Energy absorbed must be=to this exact difference
Cannot see it
Emission
Photon emitted is = to the difference in energy
Electron moves back down and emits a photon
Seen as a color, limited
Metal properties (9)
-forms a positive ion during a chemical reaction
-low ionization
-lustrous
-solid
-malleable
-high density
-ductile
-good conductor
-high melting/boiling points
Non metal properties (7)
-forms a negative ion during chemical reaction
-high ionization
-no lustrous
-solid and gas
-brittle
-poor conductor
-generally low melting/boiling points
Metalloid properties (4)
-contain intermediate properties
-solid
-semi-conductors
-a mix of properties metals/nonmetals
Group/family
Downwards
Have the same amount of valence electrons
T/F: in reactivity the noble gases are crossed out
TRUE
Arranged elements by atomic mass
Mendeleev
Arranged by atom’s number
Mosley
Pauli’s exclusion principle:
No 2 electrons can have identical quantum numbers
First principal shell= ground state
Aufbau’s rule:
Electrons will always try to occupy the lowest energy orbital position
Hund’s rule
Each orbital of equal energy will be occupied by only 1 electron of parallel spin before pairing up
N
n= principle quantum numbers
Can only increase in positive integers since energy around an electron is quantized
As it increases the orbitals become larger & higher in energy
Electrons existed as ____ around the nucleus in ____
Waves, in orbitals
