Unit Four Flashcards
Electromagnetic radiation is a kind of —- that acts as —-
Energy
Wave
One type of electromagnetic radiation is
Light
The lowest allowable energy state of an atom is
Ground state
Bohrs model of an atom predicted the — of the lines in hydrogens atomic emission spectrum
Frequency
Smaller electron orbit— energy level
Larger electrons orbit—
Energy level
Lower
Higher
How did bohrs model fail
Failed to explain the atomic emission spectrum for elements other than hydrogen
What makes up for bohrs model
Quantum numbers
Complete atomic symbol
Two numbers on left side, letter symbol, and then charge
Mass number
Proton and neutron
Average atomic mass unit
G/mole
How do we experience the energy released when an electron goes down a level
We see it, colors!
What three principles help us place electrons
Aufbau, Pauli exclusion, hund’s
Cations and anions
Cations positive
Anions negative
Which are for metal and non metals ( C or A)
Metal for C
Nonmetal for A
Energy absorbed by electron
Excited state, jumps
Energy released by electron
Falls down ground state
Where is the higher energy potential
Farther away from the nucleus
In ROY G BIV, where is the highest/ lowest energy
Lowest red, highest violet
In ROY G BIV, where is the highest/ lowest wavelength
Highest red, lowest violet
In ROY G BIV, where is the highest/ lowest frequency
Highest violet, lowest red
Energy and frequency relationship
Directly
Wavelength and frequency relationship
Inversely
Wavelength and energy relationship
Inversely
Line emission spectrum
Finger print lines show what photons are present
Quantum numbers
Energy level= n Sub level (L)= S P D F (orbital type) Spin (Ms, S)
How many quantum numbers
4
Isotopes
Atoms of same element with different mass #’s
Average atomic mass-
(Mass)(%)/100
Weighted average
Of all isotopes of an element on periodic table
Greater amplitude is —– intensity
Greater intensity
What did they Planck do
Observed emission of light from hot objects
Concluded energy is emitted in small specific amounts (quanta)
Quanta represents
Photons
Are electrons evenly spaced
No
Einstein
Concluded light has properties of both waves and particles
Wave particle duality
Schrödinger and wave function
The wave function help describes the location of the electron and it’s probable location
Where is there 90% probability of finding and electron
Orbital electron cloud
N^2
Number of orbitals in the energy level
S orbital
Electrons are found within a sphere around the nucleus
Comes in ones
P orbital
Orbitals that look like dumbells or propellers
Comes in threes
D orbitals
Most appear to be the combination of two p orbitals
Come in fives
F orbitals
Come in sevens
Aufbau principle
Electrons fill the lowest energy orbitals first (lazy tenant rule)
Electrons spin
+1/2,-1/2
Plus up, neg down
Pauli exclusion principle
Each orbital can hold two electrons but have opposite spins
No two electrons in an atom can have the same four quantum mechanics
Hunds rule
Within a sub level, place one electron per orbital before pairing them
Urnal
Orbital diagram
Boxes
Electron longhand configuration
Full thing
Electron shorthand configuration
Noble gases and then rest
Complete symbol
Mass #
Over
Atomic number
Average atomic mass formula
100
