Chapter 4 Flashcards
Scientist…wave-particle duality
Einstein
Scientist… Light as quanta of energy
Mac Planck
Scientist…planetary model of the atom
Bohr
Scientist…wavelike properties of electrons
Broglie
Scientist…the uncertainty principle
Heisenberg
Information scientists obtained for photoelectric effect
- Frequency of light has to be above a certain minimum for the photoelectric effect to occur
- Photons-light exists as a particle and as a wave
Scientist… Wave equation and quantum model of the atom
Schrodinger
Difference between ground and excited state of an atom
The ground state is the lowest energy of an atom and the excited state is when the atom has a higher potential energy
How are the excited states and ground states related to the atom giving off a photon
Electrons release energy and the energy goes back to the ground state and a photon is given off
Why is it that the energy levels of an atom can be determined by measuring the light emitted from the atom?
Specific bands of color=specific energies
Higher frequency=
higher energy
higher frequency=
shorter wavelength
red has a ________ wavelength
long
violet has a ________ wavelength
short
of orientations for s
1
of orientations for p
3
of orientations for d
5
of orientations for f
7
how is bohr’s model of the atom similar to the quantum model
- nucleus with protons
- not surrounded by electrons
- electrons exist in certain energies
how is bohr’s model of the atom different to the quantum model
- bohr had specific circular orbitals
- bohr tried to predict exactly where the electrons were
- quantum- electrons in 3d orbitals, not circular orbitals
Pauli exclusion principle
no electrons can have the same set of quantum numbers
aufbau principle
an electron occupies the lowest energy orbital that can receive it
exceptions to the aufbau principle
- half-full sub levels are more stable
- to make d and f sub levels more stable, electrons will go into orbitals with a higher energy first
- atoms are more stable with a full energy level, full sub level(s,p,d,f) or a half full sub level
electromagnetic radiation
form of energy that exhibits wavelength behavior as it travels through space
wavelength represented by_____(symbol)
lambda
frequency measured in
hertz
photoelectric effect
the emission of electrons from a metal when light shines on the metals
wave-particle duality
light is both a wave and a stream of particles called photons
photon
particle that transmits light
continuous spectrum
emission of a continuous range of frequencies of electromagnetic radiation
what causes the spectrum of an element
energy state of an atom
what happens to extra energy
absorbed by electrons
what determines the color of light
the wavelength of radiation
when electrons absorb more energy, they move _______ from the nucleus
farther
heinsenberg uncertainty principle
it is impossible to determine both the position and velocity of an electron
schrodinger wave equation
tells the probability of finding an electron in a given area(orbital) around the nucleus
4 types of quantum numbers
- principal
- angular momentum
- magnetic
- spin
orbital shapes:
s, p,d,f,g
possible values of spin quantum number
+1/2 or -1/2
aufbau principle
an electron that occupies the lowest energy level can receive it
pauli exclusion principle
no 2 electrons can have the same set of four quantum numbers
hund’s rule
orbitals of = energy are occupied by one electron before an orbital is occupied by a 2nd electrons
octet rule
atoms gain, lose, or share electrons until they have eight valence electrons
