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AP Chemistry > Chapter 6 > Flashcards

Chapter 6 Flashcards

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1
Q

The intensity of a light is a function of the waves______

A

Amplitude

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2
Q

A point of zero amplitude

A

A node

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3
Q

Unit of frequency

A

Cycles per second or hertz

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4
Q

As wavelength increases, frequency and energy ________

A

Decrease

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5
Q

Max Planck proposed that light waves existed as discrete packets of energy known as…

A

Quanta

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6
Q

Ultraviolet catastrophe

A

According to classical physics, the intensity of emitted light approaches infinity as the wavelength approves zero (incorrect)

Predictions failed in the UV region

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7
Q

Light acts as….

A

Waves and particles

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8
Q

An object can gain or lose energy by absorbing or emitting radiant energy in…..

A

Quanta

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9
Q

Quanta of energy

A

Smallest unit of energy that may be emitted as radiation

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10
Q

Electrons can only go up or down_____levels

A

Entire

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11
Q

Quantization is the….

A

Only specific energies that are allowed

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12
Q

Certain metals will____electrons when light strikes the metal surface

(Excited electrons, think of flame test)

A

Release (energy must exceed a threshold energy first)

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13
Q

Blackbody radiation

A

Theory that a body absorbs all of the radiation that falls on it

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14
Q

Packets of energy

A

Photons

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15
Q

There is a 1:1 correspondence between ejected electrons and______

A

Light waves

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16
Q

Credited with the first modern model of the hydrogen atom based on the “line spectra” of atomic emission sources

A

Bohr

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17
Q

Proposed a “planetary” structure for the atom where the electrons circled the nucleus in….

A

Defined orbitals

(Attractive electrostatic forces of the electron and nucleus were balanced by the centripetal forces of the orbiting electron)

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18
Q

When ______light passes through a prism, all of the colors of the rainbow are observed

A

White

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19
Q

When the light from a discharge tube containing a pure element is passed through the same prism….

A

Only certain colors are observed (emission spectrum)

20
Q

Wavelength red presents the distance between one complete______
(Wavelength)

A

Cycle

21
Q

The lines on the line spectrum indicate…

A

Jumps between allowed energy levels

22
Q

Wave duality

A

Electron has the properties of lights and waves

De brogli

23
Q

Heisenberg uncertainty principle

A

Impossible to determine exact position and velocity of electron

24
Q

Schrodinger

A

Determined that matter could be described as a wave, came up with orbitals

25
Q

The behavior of an electron in the atom can be described as….

A

Is standing wave

26
Q

Pauli exclusion principal

A

No 2 electrons have the same quantum numbers

27
Q

The importance of E =mc ^2

A

Energy has mass

28
Q

Electromagnetic radiation can be thought of as..:

A

A stream of particles called photons

29
Q

Diffraction results when…

A

Iight is scattered from a regular array of points or lines

30
Q

T or F

All matter exhibits either particulate or wave properties exclusively

A

F

31
Q

The 4 lines observed in the visible emission spectrum for hydrogen tell us that…

A

Only certain energies are allowed for the electron in a hydrogen atom

32
Q

Criticism of the Bohr model of the atom

A

Does not adequately predict the ionization energy of the valence electrons for elements other than H

33
Q

Bohr’s model correctly describes….

A

Only the H atom

34
Q

Orbital

A

Space where electrons are most likely to be found

35
Q

Can the movement of electrons be determined?

A

No

36
Q

The size of an orbital is_____defined

A

Arbitrarily

37
Q

How to find electrons in n=___

A

n^2 * 2 (electrons)

38
Q

The lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals

A

Hund’s rule

39
Q

n describes the….

Principle quantum number

A

Energy level, row on periodic table, size of orbital

40
Q

n represents the…

A

Subshell

41
Q

l is the_____quantum number

A

Angular momentum

42
Q

l represents the

A

Subshell (shape of orbital)

43
Q

l equals…

A

0 to n-1 values

The # of nodes (space that no electrons occupy)

44
Q

ml represents the _______quantum number

A

Magnetic

45
Q

ml equals

A

-l to +l

46
Q

ms represents the_____quantum number

ms equals…

A

Spin

-1/2 or +1/2

47
Q

The number of orbitals having a given value of l is equal to…

A

2l + 1

AP Chemistry (3 decks)

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