Electromagnetic Spectrum

Front 1

The difference in frequency in visible light accounts for the _______ _______ we see

Back 1

different colors

Front 2

The full range of light at different frequencies and wavelengths is called the

Back 2

electromagnetic spectrum

Front 3

a wave that carries energy through a matter or space

Back 3

light wave

Front 4

The matter through which a light wave travels is called the

Back 4

medium

Front 5

Light and radio waves do not need a medium and are called

Back 5

electromagnetic waves

Front 6

electromagnetic waves are

Back 6

transverse waves

Front 7

All other waves besides electromagnetic waves are

Back 7

compression or longitudinal waves

Front 8

The highest points of a transverse wave are calle

Back 8

crests

Front 9

the lowest parts of a transverse wave are called

Back 9

troughs

Front 10

The greatest distance that particles are displaced fro their normal resting is called the

Back 10

amplitude

Front 11

The distance from one crest of a wave to the next or from one trough to the next, is called teh

Back 11

wavelength

Front 12

The ________ of a wave is the # of full wavelengths that pass a point in a given time interval

Back 12

frequency

Front 13

The symbol for frequency is __ and the units are

Back 13

f (v) hertz (Hz)

Front 14

Hertz units measure the

Back 14

number of vibrations per second

Front 15

All electromagnetic waves in empty space travel at the same speed

Back 15

the speed of light

Front 16

As wavelength increases, frequency ____

Back 16

decreases

Front 17

what is the wavelength symbol

Front 18

Frequency symbol which also equals cycles per second, Hz, or sec

Back 18

v

Front 19

Speed of light symbol

Back 19

c

Front 20

Equation which includes wavelength, frequency, and speed of light

Front 21

Light also has a _______ nature

Back 21

particle-like

Front 22

Light can also be thought of as a stream of tiny particles, or bundles of energy called

Back 22

photons

Front 23

Each photon of light carries a _______ of energy for a certain amount of energy

Back 23

quantum

Front 24

The energy of a photon depends on the

Back 24

frequency of the electromagnetic radiation

Front 25

Electrons surround the nucleus of an atom in ______; every atom has many _______

Back 25

energy levels

Front 26

Electrons are lazy, so they will occupy the lower possible energy, level or __________

Back 26

ground state

Front 27

Electrons become ______ when they absorb or gain energy

Back 27

excited

Front 28

Excited electrons rise in

Back 28

energy levels

Front 29

The # of energy levels an electrons rises is = to

Back 29

amt of energy absorbed or gained

Front 30

Eventually, electrons fall back down to ground state because they are attracted to the ______ charge of the nucleus

Back 30

positive

Front 31

As electrons fall back down to ground state, they _______

Back 31

emit the energy they absorbed

Front 32

Electrons fall from an excited state to the ground state by many different ________, each of these different ______ has different amounts of energy as well as different frequencies and wavelengths

Back 32

pathways

Front 33

If visible light is emitted it can be diffracted (bent) and a ________________ or _________ can be seen

Back 33

bright line spectrum or emission spectrum

Front 34

Every element has a unique bright line _______________

Back 34

spectrum or emission

Front 35

Every element has a

Back 35

element figerprint

Front 36

Since every element has a unique spectrum, every element must have a _____ and _______ arrangement of electrons

Back 36

unique and specific

Front 37

The relationship between light and electrons _____ or _______________

Back 37

flame tests or gas discharge tubes

Front 38

When the electrons within elements are excited, they can emit ______ of ______

Back 38

visible light of certain colors

Front 39

excite electrons by heating a substance in a flame

Back 39

flame test

Front 40

Excite electrons with electricity

Back 40

gas discharge tubes

Front 41

The emission of visible light is due to the ______ of the electrons with in an atom

Back 41

arrangement

Front 42

h=

Back 42

plank's constant

Front 43

why don't we solve for h

Back 43

it is a constant

Front 44

He determined that energy can only be gained or lost in whole number multiples in other words it's quantized

Back 44

Max Plank

Front 45

Once an electron gets enough energy, it can jump to the

Back 45

next energy level

Front 46

c=

Back 46

wavelength x frequency

Front 47

How to get E on the calculator

Back 47

press 2nd, comma button

Front 48

Name of the current model for the atom

Back 48

Quantum mechanical model

Front 49

Quantum mechanics was developed by

Back 49

Erwin Schrodinger

Front 50

Quantum mechanics estimates the probability of finding

Back 50

an e(-) in a certain position

Front 51

Electrons are found in the

Back 51

"electron cloud" or orbital

Front 52

The ________________ states that an electron will occupy the lowest possible energy orbital available

Back 52

Aufbau principle

Front 53

The ______________________ states that each electron in an atom has its own distinct set of four quantum number

Back 53

Pauli exclusion principle

Front 54

No 2 elements in an atom will have the same

Back 54

set

Front 55

symbol for Main or principle energy levels

Back 55

n

Front 56

symbol for: Energy sublevels

Back 56

l

Front 57

space occupied within the atom

Back 57

orbital

Front 58

Symbol : spin

Back 58

m

Front 59

no 2 electrons in the same atom can have the same set of 4 quantum numbers.

That is each electron in an atom has a unique address of quantum numbers. What principle is this???

Back 59

Pauli exclusion principle

Front 60

Contains electrons that are close in energy, similar distance from nucleus. Have values of ___= 1, 2, 3, 4 ,5, 6, 7 which is the same as period # on periodic table

Back 60

Principle energy levels (n)

Front 61

Energy _______ within energy level. Designated s, p, d, f. _________energy s

Back 61

Sublevels (l)

Front 62

Each _____ has a different shape

Back 62

sublevel

Front 63

1 orbital, spherical shaped, and holds up to 2e(-) which means 2 electrons

Back 63

s sublevel

Front 64

3 orbitals, dumbbell shaped, arranged x y z axes, and can hold up to 6e- (6 electrons)

Back 64

p sublevel

Front 65

5 orbitals, clover shaped, and can hold up to 10e- (10 electrons)

Back 65

d sublevel

Front 66

7 orbitals, levels combine to form a spherical shape, this level can hold up to 14e- (14 electrons)

Back 66

f sublevel

Front 67

Another word for "electron cloud"

Back 67

orbital

Front 68

Region in space where there is 90% of probability of finding an electron

Back 68

orbital

Front 69

s sublevel- _ orbital- _ electrons

Back 69

1, 2

Front 70

p sublevel- _ orbital- _ electrons

Back 70

3, 6

Front 71

d sublevel- _ orbital- _ electrons

Back 71

5 orbitals, 10

Front 72

f sublevel-_ orbital- _electrons

Back 72

7 orbitals, 14 electrons

Front 73

What is the order of the wave lengths from low frequency to high frequency on the Electromagnetic Spectrum (7)

Back 73

Radio, Microwave, Infrared, Visible, Ultraviolet (UV), X-Ray, and Gamma Ray

Front 74

each orbital can be assigned no more than ____ electrons

Back 74

2

Front 75

can be proven experimentally that an electron has a

Back 75

spin

Front 76

2 spin directions given by ms

Back 76

1/2 & -1/2

Front 77

2 ways of writing configurations

Back 77

spdf and orbital box notation

Front 78

1s^1 - what is the value of n(energy level)

- # of electrons

Back 78

1; 1

Front 79

Rule? - within a sublevel, place 1 electron per orbital before pairing them; "Empty Bus Seat Rule"

Back 79

Hund's Rule

Front 80

another name for "noble gas configuration/notation" developed for use with larger elements

Back 80

shorthand

Front 81

what are groups on periodic table

Back 81

columns (1-18)

Front 82

what are periods on periodic table

Back 82

rows (1-7)

Front 83

model with electrons in energy clouds around nucleus with specific quantum number

Back 83

Quantum Mechanical Model

Front 84

energy level(n) Ex: 1s^1 4d^10

Back 84

Principal Quantum Number

Front 85

90% probability of finding electron; shape of cloud based on electron density map

Back 85

Orbital

Front 86

type of orbital in energy level 1

Back 86

s

Front 87

type of orbitals in energy level 2

Back 87

s & p

Front 88

type of orbitals in energy level 3

Back 88

s, p, & d

Front 89

type of orbitals in energy level 4

Back 89

s, p,d, & f

Front 90

3 rules for filling electron orbital diagram

Back 90

Hund's Rule (Empty Bus Seat), Aufbaus Principle, Pauli's Exclusion Principle

Front 91

Rule? - fill lowest energy level 1st

Back 91

Aufbaus Principle

Front 92

Rule? - every electron has it's own set of 4 quantum numbers: energy level(n), sublevel(l), orbital, and spin (m)

Back 92

Pauli Exclusion Principle

Front 93

frequency and wavelength are _______ related

Back 93

inversely (higher frequency, smaller wavelength)

Front 94

energy and wavelength are _______ related

Back 94

inversely (higher energy, smaller wavelength)

Front 95

energy and frequency are _______ related

Back 95

directly (higher energy, higher frequency)