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Chemistry 2016-2017 > Light > Flashcards

Light Flashcards

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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
Q

What did Max Planck discover

A

Atoms and molecules emit energy in discrete quantities called quanta - that light is a particle

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26
Q

Atoms and molecules emit energy in discrete quantities called…

A

Quanta

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27
Q

Light as a particle formula

A

E=hv

28
Q

In the light as a particle formula, what does E stand for

A

Discreet energy units of a vibrating system (jules)

29
Q

In the light as a particle formula, what does h stand for

A

Planck’s constant (6.626 x 10^-34 jules x seconds)

30
Q

In the light as a particle formula, what does v stand for

A

Frequency (second^-1 or hertz)

31
Q

E=hv, energy, and freequence are ________ related

A

Directly

32
Q

C = λV, wavelength, and frequency are ________ related

A

Indirectly

33
Q

What did Albert Einstein study to advance Planck’s theory

A

Photoelectric effect

34
Q

What did Albert Einstein do to advance Planck’s theory

A

Shined UV light on a metal, electrons were ejected from surface of the metal

35
Q

Why when Albert Einstein shined UV light on a metal electrons were ejected from surface of the metal?

A

Light contains “tiny lumps” of light particles called photons

36
Q

What are photons

A

“Tiny lumps” of light particles in light

37
Q

Photoelectric effect on low-frequency light

A

Does not bounce off because the electrons are not excited (not heated up by energy)

38
Q

Photoelectric effect on high-frequency light

A

Electrons become excited (because they gain energy through high-frequency light)

39
Q

What is the dual nature of light

A

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
Q

Who used Rutherford’s and Planck’s work to design a model of the hydrogen atom

A

Neils Bohr

41
Q

What did Neils Bohr’s hydrogen atom model entail

A

There are electrons circulating around the nucleus like planets around the sun

42
Q

What did Bohr think about electron levels in an atom

A

An electron could only occupy certain orbits or energy levels in an atom

43
Q

What did Bohr mean when he said energy is quantized

A

Electrons can occupy only certain orbits

44
Q

What did Bohr’s hyrogen model say about colors

A

Hydrogen atoms emit colors while absorbing energy

45
Q

Formula for calculating the energy of a particular energy level

A

E= (-Rnc)/(n^2)

46
Q

In the formula for calculating the energy of a particular energy level, what does E stand for

A

Energy (jules/atom)

47
Q

In the formula for calculating the energy of a particular energy level, what does R stand for

A

Rydberg’s constant (1.097 x 10^7 m^-1)

48
Q

In the formula for calculating the energy of a particular energy level, what does h stand for

A

Planck’s constant (6.626 x 10^-34 jules x seconds)

49
Q

In the formula for calculating the energy of a particular energy level, what does c stand for

A

Speed of light (2.998 x 10^8 meters/seconds)

50
Q

In the formula for calculating the energy of a particular energy level, what does n stand for

A

Principal quantam number

51
Q

Basically, what does the numerator of the formula for calculating the energy of a particular energy level always equal

A

-2.179 x 10^-18

so formula is (-2.179 x 10^-18)/(n^2)

52
Q

Elements in the gas phase emit light when hooked up to a voltage source, but what happens with the wavelengths

A

Only certain wavelengths of light are emitted

The wavelength must then be passed through a prism to seperate the lines

53
Q

Does every element has a unique line spectrum

A

Yes, it represented the fingerprint of an element and thus can be used to identify unknown elements

54
Q

Can two elements ever have the same line spectrum

A

No, it is different for each element

55
Q

What are spectroscopes

A

Used to seperate the wavelengths of light given off from the gas tubes

56
Q

What do the lines on spectroscopes mean

A

Lines show where energy is being absorbed

57
Q

What happens when electrons lose energy from moving to higher energy levels

A

They emit a photon

58
Q

Can electrons absorb energy and move to a higher energy level?

A

Yes

59
Q

What is the ground state in an atom

A

An atom with its electron in the lowest possible energy levels (closest to nucleus)

60
Q

What is the excited state in an atom

A

Electrons that absorb energy and occupy higher energy levels (further from nucleus)

61
Q

In a hydrogen atom, when an electron jumps from an excited state to a more stable energy state what happens?

A

Electromagnetic radiation is emitted by the atom

62
Q

If an AM radio station broadcasts at 995 kHz, what is the wavelength of this radiation?

A

301 m

63
Q

Excited hydrogen atoms emit light in the ultraviolet at 2.47x10^15 Hz. What is the energy of a single photon with this frequency?

A

1.64x10^-18

64
Q

The ___ of a photon of light is ___ proportional to its frequency and ___ proportional to its wavelength

A

Energy, directly, inversely

65
Q

Can one simultaneously know the location and energy of an electron in an atom?

A

No

66
Q

What is the instrument used to measure the emission spectra of different gaseous elements?

A

Spectroscope

Chemistry 2016-2017 (11 decks)

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