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Chemistry 2016-2017 > Light > Flashcards

Light Flashcards

1
Q

What is light

A

A ray, a wave, and a particle

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2
Q

A ray

A

A straight line moving from one point to another

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3
Q

Pythagoras

A

Believed that vision came from light rays coming from a person’s eye and focusing on an object

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4
Q

Epicurus

A

Believed that object produce light rays, which travel to the eye

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5
Q

Ray-like tendencies

A

Reflection, refraction, and scattering

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6
Q

When a ray strikes a smooth surface

A

Bounces off and reflects - reflecting

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7
Q

When a ray strikes a rough surface

A

Reflects at many different angles because the surface is uneven - scattering

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8
Q

What is it called when a ray strikes a rough surface

A

Scattering

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9
Q

Refraction with a ray

A

When a ray of light passes from one transparent medium to another

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10
Q

What happens when a ray refracts

A

Light changed speed and the light ray bends

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11
Q

How does the angle of a light ray bend

A

Depends on the material

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12
Q

What did James Maxwell discover

A

The EMR (electromagnetic radiation)

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13
Q

What is electromagnetic radiation (EMR)

A

Light is radiation made up of electric and magnetic fields - the fields vibrate at right angles to each other

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14
Q

Properties of waves

A

Wave, wavelength, frequency, amplitude, and node

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15
Q

What is a wave

A

A vibrating disturbance by which energy is transmitted

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16
Q

What is wavelength (in a wave)

A

The distance between identical points in a wave (λ)

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17
Q

What is frequency (in a wave)

A

The number of waves that pass through a point in one second (V)

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18
Q

What is amplitude (in a wave)

A

The height of the wave

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19
Q

What is a node (in a wave)

A

Point of zero amplitude

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20
Q

EMR travels at the speed of…

A

Light (C)

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21
Q

Speed of waves formula

A

C = λV

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22
Q

In the speed of waves formula, what does C stand for

A

Speed of light (2.998 x 10^8 m/s)

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23
Q

In the speed of waves formula, what does λ stand for

A

Wavelength (meters or nanometers)

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24
Q

In the speed of waves formula, what does V stand for

A

Frequency (seconds^-1 or hertz)

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25
What did Max Planck discover
Atoms and molecules emit energy in discrete quantities called quanta - that light is a particle
26
Atoms and molecules emit energy in discrete quantities called...
Quanta
27
Light as a particle formula
E=hv
28
In the light as a particle formula, what does E stand for
Discreet energy units of a vibrating system (jules)
29
In the light as a particle formula, what does h stand for
Planck's constant (6.626 x 10^-34 jules x seconds)
30
In the light as a particle formula, what does v stand for
Frequency (second^-1 or hertz)
31
E=hv, energy, and freequence are ________ related
Directly
32
C = λV, wavelength, and frequency are ________ related
Indirectly
33
What did Albert Einstein study to advance Planck's theory
Photoelectric effect
34
What did Albert Einstein do to advance Planck's theory
Shined UV light on a metal, electrons were ejected from surface of the metal
35
Why when Albert Einstein shined UV light on a metal electrons were ejected from surface of the metal?
Light contains "tiny lumps" of light particles called photons
36
What are photons
"Tiny lumps" of light particles in light
37
Photoelectric effect on low-frequency light
Does not bounce off because the electrons are not excited (not heated up by energy)
38
Photoelectric effect on high-frequency light
Electrons become excited (because they gain energy through high-frequency light)
39
What is the dual nature of light
Light is a collection of particles (photons) moving through space as electromagnetic waves Light moves as waves, and the waves are made up of photons
40
Who used Rutherford's and Planck's work to design a model of the hydrogen atom
Neils Bohr
41
What did Neils Bohr's hydrogen atom model entail
There are electrons circulating around the nucleus like planets around the sun
42
What did Bohr think about electron levels in an atom
An electron could only occupy certain orbits or energy levels in an atom
43
What did Bohr mean when he said energy is quantized
Electrons can occupy only certain orbits
44
What did Bohr's hyrogen model say about colors
Hydrogen atoms emit colors while absorbing energy
45
Formula for calculating the energy of a particular energy level
E= (-Rnc)/(n^2)
46
In the formula for calculating the energy of a particular energy level, what does E stand for
Energy (jules/atom)
47
In the formula for calculating the energy of a particular energy level, what does R stand for
Rydberg's constant (1.097 x 10^7 m^-1)
48
In the formula for calculating the energy of a particular energy level, what does h stand for
Planck's constant (6.626 x 10^-34 jules x seconds)
49
In the formula for calculating the energy of a particular energy level, what does c stand for
Speed of light (2.998 x 10^8 meters/seconds)
50
In the formula for calculating the energy of a particular energy level, what does n stand for
Principal quantam number
51
Basically, what does the numerator of the formula for calculating the energy of a particular energy level always equal
-2.179 x 10^-18 | so formula is (-2.179 x 10^-18)/(n^2)
52
Elements in the gas phase emit light when hooked up to a voltage source, but what happens with the wavelengths
Only certain wavelengths of light are emitted | The wavelength must then be passed through a prism to seperate the lines
53
Does every element has a unique line spectrum
Yes, it represented the fingerprint of an element and thus can be used to identify unknown elements
54
Can two elements ever have the same line spectrum
No, it is different for each element
55
What are spectroscopes
Used to seperate the wavelengths of light given off from the gas tubes
56
What do the lines on spectroscopes mean
Lines show where energy is being absorbed
57
What happens when electrons lose energy from moving to higher energy levels
They emit a photon
58
Can electrons absorb energy and move to a higher energy level?
Yes
59
What is the ground state in an atom
An atom with its electron in the lowest possible energy levels (closest to nucleus)
60
What is the excited state in an atom
Electrons that absorb energy and occupy higher energy levels (further from nucleus)
61
In a hydrogen atom, when an electron jumps from an excited state to a more stable energy state what happens?
Electromagnetic radiation is emitted by the atom
62
If an AM radio station broadcasts at 995 kHz, what is the wavelength of this radiation?
301 m
63
Excited hydrogen atoms emit light in the ultraviolet at 2.47x10^15 Hz. What is the energy of a single photon with this frequency?
1.64x10^-18
64
The ___ of a photon of light is ___ proportional to its frequency and ___ proportional to its wavelength
Energy, directly, inversely
65
Can one simultaneously know the location and energy of an electron in an atom?
No
66
What is the instrument used to measure the emission spectra of different gaseous elements?
Spectroscope

Chemistry 2016-2017 (11 decks)

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