Lecture 1: Unit 1 review of fundamentals and the quantum nature of the atom Flashcards
What is diffraction
An interference of waves
What are the characteristics of a wave
Amplitude
Frequency
Wavelength
Amplitude
Energy intensity of light
What is needed to eject and electron from a metal?
Minimum frequency of light
Above this minimum frequency what does the kinetic energy of and electron increase with?
Light frequency
Above this minimum frequency, how does increase light intensity affect and electron?
Affects the number of removed electrons but not the kinetic energy
Matter
Particulate character
What happens to particles during the double split experiment
Formed two waves
What happened to waves during the double split experiment
They diffracted
What happened to electron during the double split experiment?
They diffracted
What causes atoms to emit light?
Passage of electrons through gas
Wave particle duality
Waves exhibit particle like properties and particles exhibit wave like properties
What characteristics does matter have?
Wave and particle characteristics
What is the wave equation and what is it used for?
H¥=E¥
Mathematical function describing the shape of a wave
What are the quantum numbers of atomic orbitals?
Principle quantum number n
Angular quantum number l
Magnetic quantum number ml
Spin quantum number ms
equation to calculate energy release (rydbergs equation)
dealtaE==-2.178times 10^-18(1/nf^2-1/ni2)Z^2
how do you calculate wavelength given two orbital numbers?
- find the change in energy using rydbergs constant
- use the wavelength equation
what is the wavelength equation? what is the value of h? What is the value of c?
E=hc/lambda
h=6.626times 10^-34
c(speed go light)=3 times 10^8
how can discrete emission lines be explained?
by applying quantum theory to the energy levels
pauli exclussion principle
no two electrons in an atom can have the exact same four quantum numbers
effective nuclear charge
the nuclear charge felt by an electron
two factors that determine an atoms energy?
- electron nucleus attraction
- electron electron repulsion
explain the shielding effect of electrons
electrons further from the nucleus are shielded from the nuclear charge by electrons closer to the nucleus
which state of an electron is most stable
the ground state
Aufbau rule
electrons start filling lower energy levels first
hunds rule
if two or more degenerate orbitals are available, one electron goes into each until they are all half-full. All electrons in half-filled orbitals have the same spin quantum number
what is the trend of atomic size decreasing
left to right
bottom to top
