Atomic Theory

Question 1

Electromagnetic Waves

Answer 1

Oscillations of an EM field that propagate through space at the speed of light

Question 2

Wavelength Definition

Answer 2

Distance between 2 points of an EM wave (nm)

Question 3

Frequency Definition

Answer 3

Number of oscillation cycles that occur at a fixed point in one second (s)

Question 4

Longer wavelengths imply ____ frequency (lower/higher)

Answer 4

Lower

Question 5

Shorter wavelengths imply ___ frequency (lower/higher)

Answer 5

Higher

Question 6

Amplitude Definition

Answer 6

“height” of a wave from the midpoint

Question 7

Amplitude squared gives the ___

Answer 7

Wave intensity

Question 8

Wavelength and frequency have a ______ relationship

Answer 8

Inverse

Question 9

Balmer Series is for what radiation

Answer 9

Visible color rays

Question 10

Lyman Series is for what radiation

Answer 10

UV rays

Question 11

Paschan Series is for what radiation

Answer 11

Infrared rays

Question 12

Rydberg Series

Answer 12

R0

Question 13

What does the Rydberg Equation do?

Answer 13

Return wavelength regions as energy integers, helping Bohr

Question 14

What is the relationship between wave amplitude and light intensity?

Answer 14

Higher amplitude = higher brightness

Question 15

What is the only characteristic that distinguishes one form of electromagnetic radiation from another?

Answer 15

Wavelength

Question 16

As wavelength increases, energy levels become ______ (lower/higher)

Answer 16

Lower

Question 17

As frequency increases, energy levels become _______ (lower/higher)

Answer 17

Higher

Question 18

Lowest-energy EM radiation?

Answer 18

Radio rays

Question 19

Highest-energy EM radiation

Answer 19

Gamma rays

Question 20

Formula to calculate total energy of a photon? (E=hv or E=hc/lambda)

Answer 20

Plancks constant x frequency or Plancks constant x the speed of light/wavelength

Question 21

Photons from light behave as __________

Answer 21

waves or small particles

Question 22

Energy from a light can be absorbed or emitted only as

Answer 22

individual small photons

Question 23

As the energy level of an orbit increases, how does the energy difference change?

Answer 23

Energy difference between consecutive levels decreases

Question 24

What happens when an excited hydrogen atom returns to a lower energy level orbit?

Answer 24

The atom releases a photon with wavelength that corresponds to the energy difference between the two levels involved

Question 25

What is constructive interference

Answer 25

When two interacting waves are in phase, (max and min are aligned), resulting in a wave that is the sum of both waves

Question 26

What is destructive interference

Answer 26

when two waves are in opposite phases, creating a wave with zero amplitude, cancelling each other out

Question 27

In the two-slit experiment, after diffraction, waves in phase were ___ (dark/bright)

Answer 27

Bright

Question 28

In the two-slit experiement, after diffraction, waves out of phase were ___ (dark/bright)

Answer 28

Dark

Question 29

What was wrong with Bohr's Theory (4 points)

Answer 29

1. Didn't explain why electrons don't fall onto the nucleus 2. Didn't explain why only some wavelengths were allowed 3. Upon inspection, energy levels were split into two lines, unclear why 4. The model doesnt work for other elements aside from hydrogen

Question 30

What was the key difference between Bohr and deBroglie's quantums

Answer 30

Electrons are particles with WAVE properties

Question 31

What equation provides the principal quantum number (n) and what is the purpose of "n"

Answer 31

of nodes + 1 = n, describes wave function type (1-4)

Question 32

More nodes = (more/less) energy

Answer 32

More

Question 33

How does a guitar conceptually demonstrate waves

Answer 33

Guitars have STANDING waves, when amplitude is affected, higher notes are returned

Question 34

Define orbitals

Answer 34

wavefunctions of individual electrons with shapes/sizes that predict the probability of finding an electron within

Question 35

What is the azimuthal (l) quantum number?

Answer 35

l = n-1, describes orbital type and shape (spdf)

Question 36

What is the magnetic (m1) quantum number?

Answer 36

m1= -l to +l, describes orientation: s=0, p= -1 to +1, d=-3 to +3 etc

Question 37

What is the Ms quantum number?

Answer 37

Spin quantum for describing 2 electrons in the same orbital, could be up or down

Question 38

Where is the highest density of electrons most likely to be found near?

Answer 38

The middle of the atom

Question 39

Is there ever a negative possibility of finding an electron

Answer 39

No

Question 40

Pauli's Exclusion Principle

Answer 40

No 2 electrons can have the same 4 quantum numbers

Question 41

Electron in an Excited state

Answer 41

An electron can become excited if it is given extra energy, such as if it absorbs a photon

Question 42

Hund's rule

Answer 42

all orbitals will be singly occupied before any is doubly occupied

Question 43

Aufbau's Rule

Answer 43

electrons fill subshells of the lowest available energy, then they fill subshells of higher energy. For example, the 1s subshell is filled before the 2s subshell is occupied

Question 44

How does the speed of light change for wavelengths in different orbitals

Answer 44

It doesn't, all of c is the same in a vacuum

Question 45

Electron vs standing waves similarities (3)

Answer 45

Both undergo constructive interference, nodes and increase in energy with # of nodes

Question 46

Schrodingers Equation

Answer 46

Gives the wavefunction and associated energy of an electron to describe orbitals

Question 47

Shape of s orbital

Answer 47

spherical, # of colors indicate # of nodes

Question 48

Shape of p orbital

Answer 48

perpendicular axes, xy, xz, yz

Question 49

Shape of d orbital

Answer 49

Four clovers and one inside out cone donut, x^2y^2, xy, xz, zy, z^2

Question 50

Principle number (n) function

Answer 50

of nodes, describes energy and size

Question 51

bohr's model

Answer 51

coorelates each group of spectral lines to a wavelength of EM radtion, and determined that when H+ electrons absorb energy they become excited

Question 52

Node

Answer 52

point where wavelength = 0, no electron probability, changing phases

Question 53

Why do orbital drawings use multiple colors

Answer 53

shows orbitals above and below nodes

Question 54

What does degenerate mean with the magnetic quantum number

Answer 54

determines orientation in xyz but all are the same energy

Question 55

pnictogens

Answer 55

group 15

Question 56

Em-En

Answer 56

Ephoton