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Chem > Ch 4 Section 1 > Flashcards

Ch 4 Section 1 Flashcards

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1
Q

Visible light is a kind of

A

Electromagnetic radiation

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2
Q

Together all the forms of electromagnetic radiation form the

A

Electromagnetic spectrum

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3
Q

Wavelength is the distance between

A

Corresponding points on adjacent waves

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4
Q

Significant feature of wave motion is its

A

Rewriting nature which can be characterized by wavelength and frequency

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5
Q

Unit for wavelength

A

Distance unit (m, cm, nanometer)

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6
Q

Frequency (v) is defined as the number of

A

Waves that pass a given point in a specific time usually one second

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7
Q

Frequency unit

A

Waves per second (hertz)

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8
Q

Frequency and wavelength are

A

Mathematically related to each other

C = wavelength times frequency

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9
Q

In wavelength frequency equation c is the

A

Speed of light

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10
Q

In wavelength frequency equation wavelength symbol is the

A

Wavelength of the electromagnetic wave in m

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11
Q

In wavelength frequency equation v is the

A

Frequency of the electromagnetic wave in s^-1

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12
Q

In wavelength frequency equation the product is a

A

Constant

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13
Q

Wavelength is

A

Inversely proportional to v

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14
Q

As wavelength decreases

A

Frequency increases

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15
Q

The photoelectric effect refers to the

A

Emission of electrons from a metal when light shines on the metal

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16
Q

Wave theory of light predicted that light of any frequency could supply enough

A

Energy to eject an electron

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17
Q

A quantum of energy is the minimum quantity of

A

Energy that can be lost or gained by an atom

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18
Q

Max Planck proposed the following relationship between a quantum of energy and frequency of radiation:

A

E = hv

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19
Q

In equation E = hv, e is the

A

Energy in joules of a quantum of radiation

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20
Q

In equation E = hv, v is the

A

Frequency in s^-1 of the radiation emitted

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21
Q

In equation E = hv, and h is a fundamental

A

Physical constant known as plancks constant

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22
Q

Plancks constant

A

6.626 x 10^-34 J • s

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23
Q

Einstein introduced idea that electromagnetic radiation has a

A

Dual wave particle nature

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24
Q

Electromagnetic radiation is a form of energy that exhibits

A

Wavelike behavior as it travels through space

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25
Q

A photon is a particle of electromagnetic radiation having

A

Zero mass and carrying a quantum of energy

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26
Q

The energy of a particular photon spends on the

A

Frequency of the radiation

27
Q

Ephoton =

A

Hv

28
Q

Electromagnetic radiation is absorbed by matter only in

A

While numbers of photons

29
Q

Different metals require different

A

Minimum frequencies to exhibit the photoelectric effect

30
Q

When current is passed through gas at low pressure the

A

Potential energy of the gas atoms increases

31
Q

Ground state of an atom

A

Lowest energy state of an atom

32
Q

Excited state of an atom is a state in which an atom has a

A

Higher potential energy than it has in its ground state

33
Q

When an excited atom returns to its ground state or lower energy excited state it gives off

A

Energy it gained in form of electromagnetic radiation

34
Q

When investigators passed electric current through a vacuum tube containing hydrogen gas at low pressure the observed

A

The emission of a characteristic pinkish glow

35
Q

When a narrow beam of the emitted light was shined through a prism it was

A

Separated into four specific colors of the visible spectrum

36
Q

The four bands of emitted light were part of what is known as

A

Hydrogens line emission spectrum

37
Q

Scientists had expected to observe the emission of a

A

Continuous range of frequencies of electromagnetic radiation: continuous spectrum

38
Q

New atomic theory called the

A

Quantum theory

39
Q

Whenever an excited hydrogen atom falls to its ground state or to lower energy excited state it emits a

A

Photon of radiation

40
Q

The fact that hydrogen atoms emit only specific frequencies of light indicated that

A

Energy differences between atoms’ energy stars were fixed

41
Q

Niels Bohr proposed a hydrogen atom model that linked the atoms

A

Electron to photon emission

42
Q

According to the model the electron can

A

Circle the nucleus only in allowed paths (orbits)

43
Q

When the electron is in one of these orbits atom has a

A

Definite fixed energy

44
Q

The electron is in its lowest energy state when it is in the

A

Orbit closest to the nucleus

45
Q

This orbit is separated from the nucleus by a

A

Large empty space where the electron cannot exists

46
Q

The energy of the electron is higher when the electron is in orbits that are

A

Successively farther from the nucleus

47
Q

An electron can be in one orbit or another but not

A

In between

48
Q

While in a given orbit the electron is neither

A

Gaining nor losing energy

49
Q

When an electron falls to a lower energy s photon is emitted and the process is called

A

Emission

50
Q

Energy must be added to an atom in order to

A

Move an electron from a lower energy level to a higher energy level (absorption)

51
Q

Energy of each absorbed or emitted photon corresponds to a

A

Particular frequency of emitted radiation

Ephoton= hv

52
Q

Bohr’s approach did not explain the spectra of atoms with

A

More than one electron

53
Q

Other kinds of electromagnetic radiation

A

X Rays
Ultraviolet and infrared light
Microwaves
Radio waves

54
Q

All forms of electromagnetic radiation move at a constant speed though a vacuum of

A

3.00 x 10^8 meters per second

55
Q

3,00 x 10^8 m/s is also lights

A

Approximate speed through air

C

56
Q

The mystery of the photoelectric effect invoked the

A

Frequency of the light striking the metal

57
Q

Max Planck studied the emission of light by

A

Hot objects

58
Q

Planck proposed that a hot object does not emit

A

Electromagnetic energy continuously

59
Q

Planck suggested that the object emits energy in

A

Small specific packets called quanta

60
Q

The energy of this photon is equal to the difference in

A

Energy between the atoms Initial state and its final state

61
Q

Bohr calculated the allowed

A

Energy levels for the hydrogen atom

62
Q

Bohr related the possible energy level changes to the

A

Lines in the hydrogen emission line spectrum

63
Q

Bohr’s theory didn’t explain the chemical

A

Behavior of atoms

Chem (54 decks)

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