Electrons In Atoms - Chapter 13

Front 1

Hertz

Back 1

the SI unit of frequency

Front 2

atomic orbital

Back 2

region outside the nucleus where there is a high probability of finding an electron

Front 3

Spectrum

Back 3

a range of colors seen when light passes through a prism

Front 4

atomic emission spectrum

Back 4

lines of colored light obtained by passing the light emitted by an element through a prism

Front 5

quantum of energy

Back 5

the amount of energy required to move an electron from one energy level to the next higher one

Front 6

amplitude

Back 6

the height of a wave from the origin to the crest

Front 7

wavelength

Back 7

the distance between crests of waves

Front 8

energy level

Back 8

the region around an atomic nucleus where an electron is likely to be moving

Front 9

Aufbau principle

Back 9

electrons enter orbitals of lowest energy first

Front 10

frequency

Back 10

the number of wave cycles that pass a given point per unit of time

Front 11

how many orbitals are in each energy level

Back 11

1- 1

2-3

3-5

4-7

Front 12

S^?

p^?

D^?

f^?

Back 12

s2

p6

d10

f14

Front 13

what is the max # of electrons that can occupy the 1,2,3,4 principle energy levels

Back 13

1-2

2-8

3-18

4-32

Front 14

the formula 2n^2 represents what

Back 14

the max number of electrons that can occupy an energy level

Front 15

in order to occupy the same orbital, two electrons must have....

Back 15

opposite spin

Front 16

stable electron configurations are likely to contain

Back 16

filled energy sublevels

Front 17

according to hunds rule, when electrons occupy orbitals of equal energy, one electron enters each orbit until:

Back 17

all the orbitals contain one electron with spins parallel

Front 18

the quantum mechanical model of the atom is...

Back 18

concerned with the probability of finding an electron in a certain position

Front 19

equation to find wavelength or the speed of light

Back 19

c=(wavelength)x(frequency- v)

Front 20

equation to find energy

Back 20

E= (h- planks constaint)x(frequency)

Front 21

What is the max number of electrons that can occupy each of the first five principal energy levels?

Back 21

1-2

2-8

3-18

4-32

5-32

Front 22

why does the 5s sublevel fill before any electrons are added to each of the 4d sublevel

Back 22

5s is less energy

Front 23

ground state

Back 23

lowest energy level for a given electron

Front 24

photoelectric effect

Back 24

a process in which electrons are ejected by metas when certain wavelengths of light shine on them

Front 25

photon

Back 25

quantum of light

Front 26

Heisenberg uncertainty principle

Back 26

It is impossible to know both the velocity and the position of a particle at the same time

Front 27

de Broglie's equation

Back 27

predicts that all matter exhibits wavelike motions

Front 28

what is the highest percent for probability

Back 28

90%

Front 29

Planks constant

Back 29

6.626 x 10^-34

Front 30

2 electron configuration exeptions

Back 30

chromium [ar]4s1 3d5

copper [ar]4s1 3d10