Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chemistry 1301a > Atomic Theory > Flashcards

Atomic Theory Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards
1
Q

Electromagnetic Waves

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Wavelength Definition

A

Distance between 2 points of an EM wave (nm)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Frequency Definition

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Longer wavelengths imply ____ frequency (lower/higher)

A

Lower

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Shorter wavelengths imply ___ frequency (lower/higher)

A

Higher

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Amplitude Definition

A

“height” of a wave from the midpoint

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Amplitude squared gives the ___

A

Wave intensity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Wavelength and frequency have a ______ relationship

A

Inverse

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Balmer Series is for what radiation

A

Visible color rays

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Lyman Series is for what radiation

A

UV rays

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Paschan Series is for what radiation

A

Infrared rays

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Rydberg Series

A

R0

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What does the Rydberg Equation do?

A

Return wavelength regions as energy integers, helping Bohr

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is the relationship between wave amplitude and light intensity?

A

Higher amplitude = higher brightness

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

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

A

Wavelength

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

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

A

Lower

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

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

A

Higher

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Lowest-energy EM radiation?

A

Radio rays

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Highest-energy EM radiation

A

Gamma rays

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

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

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Photons from light behave as __________

A

waves or small particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Energy from a light can be absorbed or emitted only as

A

individual small photons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

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

A

Energy difference between consecutive levels decreases

24
Q

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

A

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

25
Q

What is constructive interference

A

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

26
Q

What is destructive interference

A

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

27
Q

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

A

Bright

28
Q

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

A

Dark

29
Q

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

A
  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
30
Q

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

A

Electrons are particles with WAVE properties

31
Q

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

A

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

32
Q

More nodes = (more/less) energy

A

More

33
Q

How does a guitar conceptually demonstrate waves

A

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

34
Q

Define orbitals

A

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

35
Q

What is the azimuthal (l) quantum number?

A

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

36
Q

What is the magnetic (m1) quantum number?

A

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

37
Q

What is the Ms quantum number?

A

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

38
Q

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

A

The middle of the atom

39
Q

Is there ever a negative possibility of finding an electron

A

No

40
Q

Pauli’s Exclusion Principle

A

No 2 electrons can have the same 4 quantum numbers

41
Q

Electron in an Excited state

A

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

42
Q

Hund’s rule

A

all orbitals will be singly occupied before any is doubly occupied

43
Q

Aufbau’s Rule

A

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

44
Q

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

A

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

45
Q

Electron vs standing waves similarities (3)

A

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

46
Q

Schrodingers Equation

A

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

47
Q

Shape of s orbital

A

spherical, # of colors indicate # of nodes

48
Q

Shape of p orbital

A

perpendicular axes, xy, xz, yz

49
Q

Shape of d orbital

A

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

50
Q

Principle number (n) function

A

of nodes, describes energy and size

51
Q

bohr’s model

A

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

52
Q

Node

A

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

53
Q

Why do orbital drawings use multiple colors

A

shows orbitals above and below nodes

54
Q

What does degenerate mean with the magnetic quantum number

A

determines orientation in xyz but all are the same energy

55
Q

pnictogens

A

group 15

56
Q

Em-En

A

Ephoton

chemistry 1301a (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions