-
Proportional or Inversely Proprtional
Frequency/Wave Length
Inversely proportional
-
Proportional or Inversely Proprtional
Wavelength/ Energy
Inversely Proportional
-
Proportional or Inversely Proprtional
Frequency / energy
Proportional
-
Frequency = (symbol and Unit)
u (1/sec; Hz )
-
Wavelength = (symbol and unit)
(m) the upside down y
-
C = (2answers)
- speed of light is wavelength times frequency
- c = 3.00 x 108 m/s
-
High frequency is _____ energy
High
-
Long wavelength is ___ energy
Low
-
Plancks Constant
Energy of Light=
h u(frequency)
-
In Planck's constant:
Energy of Light= h u(frequency)
h=
h = 6.626 x10-34 J s
-
What is Planck’s constant
E = h u
-
 What model is this?
The Bohr Model
-
When electrons move between energy levels they_____ or ____ light.
absorb or give off
-
atomic spectra.
- when Electrons can move between
- energy levels absorbing or
- giving off light
-
Emission spectra “atomic finger prints”
-
A problem with Bohr’s atom
Electrons traveling in an orbit should give off light continuously … they don’t.
-
What did De Broglie say about electrons
They were waves containing specific amounts of energy
-
Wave particle duality
both sets of properties present – wave and particle properties
-
Heisenberg Uncertainty Principle
We can only observe electrons by interaction with photons. Interactions with photons cause electrons to move.
-
What did Heisenberg say about how we can know where and atom is.
- Heisenberg says: we
- can’t know where an electron
- is AND where it is going at the
- same time.
-
Orbital: Definition
A three dimensional space around the nucleus where an electron is likely to be found. 90% probablility.
-
-
Quantum Numbers:
-Tells us.....
-The 4 numbers are...
- Tell us where electrons are LIKELY TO BE based on energy states of electrons
- 1) energy level, 2) the sub level, 3) the orbital and 4) the spin.
-
Energy Level or ______ _____ _______.
What NUmbers
- “principle quantum number”
- n= 1,2,3,4,5,6,7
-
As n increases, the energy and distance from nucleus _____.
Increases
-
2) The Sub Level:
-Describe the ____
- What are they
- Describes the SHAPE
- There are 4 shapes: s, p, d, f
-
3) The Orbital
Each orbital holds _ electrons.
What is it?
- 2
- The orbital is the specific region of the sublevel the electron is in.
- s has 1, p has 3, d has 5, f has 7
-
s orbitals are
are spherical
-
p orbitals are
dumbell shaped
-
d orbitals are
complex
-
f orbitals are
really complex
-
4) The Spin
For each orbital there are two spins: up and down.
-
n^2=
total number of obitals in the Energy Level
-
2n^2=
Number of Electrons in an Energy Level
-
As ____ _____ goes up, orbitals get _____.
Energy Levels, Bigger
-
Electron Configuration:
Arrangement of electrons in an atom.
-
Aufbau principle:
an electron occupies the lowest-energy orbital that it can.
-
Hund’s Rule:
orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron.
-
Pauli exclusion principle:
no two electrons in the same atom can have the same four quantum numbers
-
-
IRREGULARS
24 Cr [Ar] 4s1 3d5 Crunium
29 Cu [Ar] 4s1 3d10 Copper
- IRREGULARS
- 24 Cr [Ar] 4s1 3d5 crunium
- 29 Cu [Ar] 4s1 3d10 copper
-
If an electron moves from a lower energy level to a higher energy level light is________.
Absorbed
-
If an electron moves from a higher energy level to a lower energy level light is _______
Emitted
-
Lyman series:
UV light, goes to n=1 level
-
Balmer series:
visible light, goes to n=2 level
-
Paschen series:
Infrared light, goes to n=3 level
-
Atomic #= # of ______and # of ______.
protons and electrons
-
atomic mass=
(mass #* %)+ (mass #* %)/ 100
-
isotope
same element but different nuetrons and different mass number
-
mass # =
num of protons + Nuetrons
-
Forms of radiation for low to high energy
- Radio - High wavelength low frequency and energy
- Microwaves
- Infared
- Visible- red (low energy) Orange Yellow Green Blue
- Ultraviolet
- Xrays
- Gamma rays- High energy and frequency low wave length
-
Stable electron configurations are likely to contain orbitals that are completely _______ or _________.
full or empty
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