Quantum Theory test

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visible

ROYGBIV; only particle we can see; wavelength is comparable to hair

exceptions

d-1# less than the period # f block-2# less than the period #

photoelectric effect

einstein; energy is not continuous at all frequencies

Hund's rule

electrons are placed in seperate orbitals of the same energy before pairing up (bus rule)

Aufbau principle

electrons enter the orbitals of the lowest energy first

Schrödinger

electrons move around the nucleus as waves; electrons probably around nucleus; orbitals

general information provided by quantum numbers

energy level, shape, location, and electrons

quantum

finite quantity of energy in discrete units that are gained or lost by an atom

electromagnetic spectrum

forms of radiant energy that show wavelike behavior as it travels through space; forms of waves- both electrial and magnetic properties

gamma rays

harmful; penetrating

microwaves

heating

infared (ir)

heating; red coloring; night vision goggles

amplitude

height of the wave

excited state

higher energy levels than ground state

electron dot notation

how many electrons are in the highest energy level

laser

light amplification by stimulated emission of radiation; scanning playing music

orientations per sublevel

s-1 p-3 d-5 f-7

shapes

s-sphere; p-dumbell; d-4leaf clover and dumbell with donut; f 6leafed flower

orbital quantum number

shape of orbital; s,p,d,f

ground state

state of lowest energy level of an atom

de Broglie

the electron can act like a wave or particle

frequency

the number of waves that pass by a particular point in one second (cycles/second)

x-rays

used to see bones

wavelength

distance between 2 identical points on successive waves

planck

e=hv where h=6.626x10^-34 Jxs

speed of light

c=wavelength (lambda) x frequency (v)

speed of light constant

3.00x10^8 m/s and 3.00x10^10 cm/s

planck constant

6.626x10-34 Js

quantum theory

(physics) a physical theory that certain properties occur only in discrete amounts (quanta)

unit of frequency

("v") 1/s=Hz or s^-1

unit for wavelength

(lambda) cm or m

spin quantum number

+1/2 -1/2; electrons do opposites

possible values for quantum number

1-7

electron configuration pattern

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6

shortcomings of the bohr model

cant work for any atoms except single electron atoms and ions; cant explain chemical bonds

electron configuration

arrangement of electrons of an atom

Octet of electrons

atoms combine so there are eight electrons in valence shells

ultraviolet

black lights; suntan/burn; spf; uva and uvb

radiowaves

music/sound; heihrich hertz

principal quantum number

n; main energy level; periods of the periodic table

Pauli exclusion principle

no 2 electrons in the same atom can have the same set of quantum numbers (opposite spins)

Heisenberg-Uncertainity principle

not possible to measure the velocity and position of the electron exactly; waves are bigger than electron so it gives energy

magnetic quantum number

orientation; x,y,z

photon

particle or packets or particular energy

four quantum numbers

principle quantum number; orbital quantum number; magnetic quantum number; spin quantum number

orbital

probable location of electron

radar

radio detection and ranging; navigation/collision avoidence


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