Brainscape's Knowledge GenomeTM

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


See full index

Chemistry 10 > Chapter 5 > Flashcards

Chapter 5 Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Rutherford’s Model

A

Positive charge + all of mass is in a concentrated nucleus surrounded by electrons

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

EM radiation

A

Energy that exhibits wavelike behavior as it travels through space

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

Wavelength

A

λ, is the shortest distance between equivalent points on a continuous wave

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

1 nm

A

10-9 m

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

Frequency

A

v, The number of waves that pass a given point per second

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

Hertz

A

One wave per second

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

SI Unit of frequency

A

Hertz

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

____ s-1

A

Used to measure frequency, is equivalent to Hertz. Is used to express “waves per second”

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

Amplitude

A

The length from the origin of a wave to its crest/trough.

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

c

A

Speed of light

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

c=?

A

c=λv c=wavelength*frequency c=3.00*108 m/s

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

Frequency and wavelength are _____ related

A

Inversely

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

White light

A

Contains a continuous range of wavelengths and frequencies. For example, sunlight passing through a prism is separated into a continuous spectrum of colors.

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

Visible spectrum

A

The colors we an see w/ a human eye

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

Why is a spectrum continuous?

A

There is no portion that does not correspond to a unique wavelength and frequency of light.

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

How is a rainbow formed?

A

Drops of water in the air disperse the white light from the sun to it’s component colors to form a rainbow.

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

Electromagnetic Spectrum

A

AKA the EM spectrum, encompasses all forms of EM radiation.

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

The only differences between the types of EM radiation are ______?

A

Frequency and wavelength. Speed (c) remains the same (3.00*108 m/s)

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

What wavelengths bend more as the pass through a prism?

A

Long wavelengths bend more.

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

What color of visible light has the longest wavelength?

A

Red

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

What is the order of colors in visible light from the longest wavelength to the shortest wavelength?

A

Red, Orange, Yellow, Green, Blue, Indigo, Violet

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

Energy is directly proportional to ______

A

Frequency (v)

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

Energy is inversely proportional to _______

A

Wavelength (λ)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What color of visible light has the most energy? Why?

A

Violet; it has the highest frequency.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

List the EM spectrum in terms of longest wavelength to shortest wavelength

A

Radio, Microwaves, Infrared, Visible light, UV, X rays, Gamma

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What type of EM radiation has the most energy?

A

Gamma rays

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What type of EM radiation has the least energy?

A

Radio

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

List the EM spectrum in terms of lowest frequency to highest frequency

A

Radio, Microwaves, Infrared, Visible light, UV, X rays, Gamma

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Max Planck

A

Studied light emitted from heated objects: Matter can gain or lose energy only in small, specific amounts called quanta.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Quantum

A

The minimum amount of energy that can be gained or lost by an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Glowing objects emit light, a form of energy. This emitted light energy is _______.

A

Quantized. (Propsosed by Planck)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Matter, regardless of its form, can gain or lose energy only in small _____ amounts.

A

Quantized.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Equantum=?

A

e=hv; where e is energy, h is Planck’s constant and v is frequency.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Planck’s constant

A

6.626*10-34 Joules seconds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

What is the SI unit of energy?

A

Joules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

What two equations are NOT THE SAME

A

c=λv (Speed of light = wavelength * frequency) e=hv (Energy = Planck’s constant * frequency)

37
Q

Matter can emit or absorb light only in _______

A

Whole number multiples of hv; that is, 1hv, 2hv, 3hv, etc.

38
Q

What is an analogy of the concept of quantized energy?

A

For example a child building a wall of wooden blocks. The child can only take away height from the wall in a whole number of blocks. Fractions of blocks are not possible. In the same way, matter can have only certain amounts of energy. Quantities between these values of energy do not exist.

39
Q

Photoelectric effect

A

Electrons are emitted from a metal’s surface when light of a certain frequency shines on the surface.

40
Q

Photoelectric cells

A

Convert light into electrical energy (for example a solar powered calculator)

41
Q

The wave model predicts what about the photoelectric effect?

A

Given enough time, even low-energy, low-frequency light would accumulate and supply enough energy to eject photoelectrons from a metal.

42
Q

Why is the wave model incorrect?

A

A metal will not eject photoelectrons below a specific frequency of incident light, no matter how intense or how long it shines.

43
Q

Who explained the photoelectric effect?

A

Einstein

44
Q

Einstein said that EM radiation has both _____ and ____ properties

A

Wave and particle.

45
Q

While a beam of light has many wavelike characteristics, it also can be thought of as a tiny stream of particles, or bundles of energy, called ____

A

Photons.

46
Q

Photon

A

A particle of EM radiation with no mass that carries a quantum of energy

47
Q

Einstein’s equation which was similar to Planck’s idea of constant energy was:

A

Ephoton=hv

48
Q

For the photoelectric effect to occur ___________

A

A photon must possess the energy required to free an electron from an atom of the metal.

49
Q

(True/False) Even small numbers of photons with energy above the threshold value will cause the photoelectric effect

A

True

50
Q

Atomic Emission Spectrum

A

The set of frequencies of the EM waves emitted by the atoms of the element.

51
Q

(True/False) Each element’s atomic emssion spectrum is unique and can be used to determine if that element is part of an unknown compound.

A

True

52
Q

What are ways to excite electrons to a higher energy level?

A

Electricity [gas tube], heat [flame tests]

53
Q

Bohr’s model of the atom

A

The hydrogen atom only has certain allowable energy states. The single electron orbits hydrogen in circular orbits. The smaller the orbit, the lower the energy level.

54
Q

Ground state

A

The lowest allowable energy state of an atom

55
Q

Excited state

A

When an atom gains energy

56
Q

(True/False) Because the hydrogen atom contains only a single electron, it is capable of having only one excited state.

A

False. It can have many excited states.

57
Q

ΔE=?

A

Ehigher-energy orbit - Elower-energy orbit = Ephoton = hv

58
Q

The visible series of spectrum lines is called the _____

A

Balmer Series; when electrons drop to the n=2 energy level.

59
Q

Lynman series

A

UV light; when electrons drop to the n=1 energy level.

60
Q

Paschen Series

A

Infrared; when electrons drop to the n=3 energy level.

61
Q

(True/False) An atom’s energy levels are evenly spaced

A

False. The distance between energy levels gets smaller and smaller as the levels get bigger.

62
Q

de Broglie equation

A

λ=h/mv, where λ is wavelength, h is Planck’s constant, and v is velocity

63
Q

(True/False) All moving particles have wave characteristics

A

True

64
Q

Why can’t you see the wavelengths of objects in motion?

A

Because the mass of these objects is so big that the wavelength is far too small to see.

65
Q

Heisenberg Uncertainty Principle

A

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

66
Q

Shrodinger wave equation

A

Treated the H atom’s electron as a wave. It worked for other elements too, unlike Bohr’s model.

67
Q

Quantum Mechanical model of the atom (Wave mechanical model of the atom)

A

Electrons are treated as waves. Like Bohr’s model, an electron’s energy is restricted to certain values. However, it makes no attempt to describe the electron’s path around the nucleus.

68
Q

Wave function predicts _____

A

The electron’s location in an atom

69
Q

Atomic Orbital

A

A 3D location around the nucleus that describes the electron’s probable location.

70
Q

The orbital is where an electron is _____% of the time

A

90%

71
Q

Principal Quantum Numbers

A

(n) Indicates the relative sizes and energies of atomic orbitals.

72
Q

As n increases, the electron ________

A

spends more time further from the nucleus, and the atom’s energy level increases

73
Q

Principal energy levels

A

n specifies the atom’s major energy levels. An atom’s lowest principal energy level is assign a quantum number of 1.

74
Q

How many energy levels have been detected for hydrogen?

A

n=1-7

75
Q

Energy sublevels

A

s, p, d, f orbitals.

76
Q

Principal energy level n contains ____ sublevels

A

n sublevels

77
Q

Each energy sublevel contains how many degenerate orbitals?

A

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

78
Q

Number of orbitals related to principal energy level

A

n2

79
Q

Electron configuration

A

Electron’s arrangement in an atom

80
Q

Aufbau principle

A

Each electron occupies the lowest energy orbital available

81
Q

Pauli exclusion principle

A

Two electrons may occupy a single orbital, but only if they have opposite spins

82
Q

Hund’s Rule

A

Single electrons with the same spin must occupy each degenerate orbital before additional electrons with opposite spins can occupy the same orbital.

83
Q

What is the electron configuration for chromium?

A

[Ar]4s13d5

84
Q

What is the electron configuration for copper?

A

[Ar]4s13d10

85
Q

Valence electrons

A

Electrons in the s and p orbitals

86
Q

Angular quantum number

A

The shape of the orbital (spdf)

Starts at 0 for s, 1 for p, etc.

87
Q

Magnetic quantum number

A

(m), any number from +- l (the anuglar quantum number).

So for example, if l=2, m could be -2,-1,0,1,2

88
Q
A

Chemistry 10 (7 decks)

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