Chemistry Unit 6: Electromagnetic Spectrum & The Photoelectric Effect + Spectroscopy + Quantum Mechanical Model & Polyelectronic Atoms + Electron Configurations & Orbital Diagrams

electromagnetic radiation

energy that travels in waves at the speed of light in a vacuum

wavelength (lamda)

distance between to peaks or troughs in a wave pattern

frequency (new)

number of waves per second in reciprocal seconds (s^-1)

relationship between wavelength and frequency

inverse; increasing wavelength, decreasing frequency; decreasing wavelength, increasing frequency

speed of light (C)

2.998 × 10⁸ m/s

wavelength and frequency formula

(lamda)(new)=C; lamda must be in meters

plancks formula using frequency

deltaE = h(new)

photon

particle of electromagnetic radiation

frequency formula

(new) = C/(lamda)

plancks formula using wavelength

deltaE = hC/(lamda)

plancks constant

h = 6.626 × 10-34J

photoelectric effect

when light strikes a material, electrons are emitted

ground state

lowest possible energy state

excited state

electrons given energy to jump to higher energy levels

absorption

electron goes to a higher energy level

emission

electron goes to a lower energy level

excited electron configs

electrons will skip the s or p orbital before the d orbital

spectroscopy

how samples interact with light

greater distance jumped by electrons means

there is more energy required

greater energy

shorter wavelength

lesser energy

longer wavelength

isoelectronic

having same # of electrons

electrons are attracted to

the nucleus

electrons are repelled by

other electrons

what elements can be used as shortcuts in electron configurations

nobel gases

aufbau principle

electrons occupy lower energy levels first

pauli exclusion principle

electrons have opposite spins