FINAL - SECTION 1 Flashcards
zA Z P
A = atomic mass
Z = atomic symbol
P = number of protons
Frequency (v)
Number of cycles per second (s-1)
Wavelength (λ)
Distance wave travels in 1 cycle (nm)
Amplitude
Height of crest of wave
Relationship between frequency and wavelength
Inversely proportional (small freq = big wavelength, big freq = small wavelength)
Rank electromagnetic spectrum from lowest energy (big wavelength) to high energy (small wavelength)
- Radio (10^5-10^-1)
- Microwave (10^-1-10^-3)
- Infrared (10^-3-10^-6)
- Visible light (10^-6-10^-7)
- UV (10^-7-10^-9)
- X ray (10^-9-10^-11)
- Gamma ray (10^-11-10^-15)
Which ER has longest wavelength (small freq)
Radio
Which ER has smallest wavelength (largest freq)
Gamma ray
Rank visible light from low energy (big wavelength) to high energy (small frequency)
- Red
- Orange
- Yellow
- Green
-Blue - Violet
Relationship between visible light and color
Amplitude determines brightness, frequency/wavelength determines color
Important equations (5)
- c = λv
- λ = c/v
- v = c/λ
- E = hc/λ
- λ = hc/Ephoton
Conversion of nm to m
nm x 1m/10^9nm
Conversion of m to nm
m x 10^9nm/1m
KE
Ephoton - Binding energy
Energy of electron
En = -2.179x10^-18 J (z^2/n^2)
Z is atomic number
n is orbital
Excitation
Energy is absorbed and electron gain enough energy to move to higher orbital
Relaxation
Energy emitted (released) and electron moves to lower orbital
Ground state
n=1 (lowest level)
Excited state
n >= 2 (higher level)
Difference in energy level
- Used then question is asking when n=5 goes to n=3
(-2.179x10^-18 J)(z^2/n^2f-z^2/n^2i)
DeBroglie equation
- λ = h/mv (velocity)
- Finds wavelength from mass of electron and velocity, so end unit should be m/nm
Heisenberg uncertainty principle
States that we do not know the speed and position of particles with exact accuracy
3 types of quantum numbers
- Describe orbitals in terms of their property
- Principal quantum number (n)
- Angular momentum quantum number (l)
- Magnetic quantum number (ml)
Principle quantum number (n)
- Size and orbital energy
- n is integer
- Larger n = larger orbital (far from nucleus)
Angular momentum number (l)
- Orbital shape
- Dependant on n, is every shape from 0 to n-1
Relationship of l with orbital subshell
- l = 0: s
- l = 1: p
- l = 2: d
- l = 3: f
- l = 4: d
Magnetic quantum number (ml)
- Orientation of orbital
- Integer from -l to 0 to +1 (DO EVERY l)
- Number of ml = number of orbitals
s orbital
Spherical in shape, as n increases the size of s orbital increase
Spherical node
Round nodes found on 2s orbitals and up
Angular (planar) node
Nodes at nucleus of p orbitals and up
Node
Areas of 0 electron density (n-1)
p orbital
First occur in n=2, there is 3 with different orientations
d orbital
First occur in n=3, there is 5 with different orientations
Draw the orbitals
Ok
Spin orientation quantum number (ms)
If electron configuration has arrow UP = +1/2, if arrow down = -1/2
3 rules for electron configuration
- Aufbau principle
- Pauli exclusion principle
- Hunds rule
Aufbau principle
Electrons occupy lower energy orbitals first before going higher
Pauli exclusion principle
2 electrons in orbitals must have different spins
Hunds rule
Electrons will fill singly before pairing
Periodic table blocks
- s block: alkali earth + alkali metal
- p block: basic metal + metalloid + nonmetal + halogen + noble gas
- d block: transition metal
- f block: lanthanoid + actinide
Diamagnetic atom
All paired electrons
Paramagnetic atom
Unpaired electrons
