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Junior 2015-2016 > Chemistry Chapter 4 > Flashcards

Chemistry Chapter 4 Flashcards

1
Q

According to the Bohr model of the atom, which particles are allowed to exist in any one of a number of energy levels?

A

electrons

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2
Q

The line emission spectrum is caused by the energies released when electrons…….

A

jump from higher energy level to a lower energy level

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3
Q

Because excited hydrogen atoms always produced the same line-emission spectrum, scientists concluded that hydrogen

A

releases energy of only certain values

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4
Q

Which color of light in the visible spectrum has the longest wavelength?

A

red

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5
Q

A quantum of energy is the …..

A

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

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6
Q

Bohr’s model correctly explains the spectra of atoms with how many electrons?

A

one

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7
Q

A form of energy that exhibits wave behavior as it travels through space is…?

A

microwave radiation
infrared radiation
ultraviolet radiation

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8
Q

In the equations λν = c, c represents ?

A

the speed of light

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9
Q

The process of an atom releasing energy when it moves to a lower energy state is called

A

emission

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10
Q

In the Bohr model of the atom, in which orbit is an electron in its lowest energy state?

A

in the orbit closest to the nucleus

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11
Q

The common characteristics shown by X-rays, visible light, infrared radiation, and radio waves is that they all have the same….

A

speed

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12
Q

A quantum of electromagnetic energy is called a …

A

photon

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13
Q

An optical instrument that separates light entering it into component wavelength is a …

A

spectrascope

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14
Q

The lowest total energy of the electron in a hydrogen atom occurs when the electron is in the state called…

A

ground state

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15
Q

What happens to frequency when wavelength increases

A

decreases

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16
Q

What happens to frequency when energy increases?

A

increases

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17
Q

How does Bohr’s model of the atom differ from Rutherford’s

A

Bohr’s model shows the different levels and is more detailed, which Rutherford’s is a vague outline of what the cell looks like and where the electrons are

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18
Q

Exclusion principle

A

Pauli

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19
Q

wave-particle duality

A

de Broglie

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20
Q

Wave equation

A

Schrodinger

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21
Q

uncertainty principle

A

Heisenberg

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22
Q

Number of energy levels and describes electron cloud size

A

n-energy

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23
Q

Shape of electron cloud

A

l-shape

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24
Q

direction in space of each orbital

A

m-orientation

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25
Q

spin of the electron

A

s-spin

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26
Q

If n=4, there may be… sublevels

A

16 in total

4 in types

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27
Q

The p sublevel may contain… pairs of electrons or orbitals

A

3

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28
Q

Two electrons occupying the same orbital must have opposite…

A

spins

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29
Q

The last electron in an oxygen atom enters the … orbital

A

2p

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30
Q

How many sublevels are possible for each of the following
n=1
n=3
n=6

A

1
3
6/4

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31
Q

How many orbitals are there in the following sublevels.
p
d
f

A

3
5
7

32
Q

The size and shape of an electron cloud are most closely related to the electron’s

A

energy

33
Q

The quantum number that indicates the position of an orbital about the three axes is space is the

A

magnetic quantum number

34
Q

An orbital that would never exist in the quantum description of atom is

A

2d

35
Q

For n=2, the number of possible orbital shapes is

A

4

36
Q

The number of particles found in the nucleus of an atom

A

mass number

37
Q

The method of studying substances that are exposed to continuous exciting radiation is called…

A

spectroscopy

38
Q

a negative electrode

A

anode

39
Q

atoms possessing the same number of protons but different number of neutrons

A

isotopes

40
Q

the number of cycles or peaks of a wave that occur in a unit of time

A

frequency

41
Q

A unique set of wavelengths absorbed by a particular substance

A

spectrum

42
Q

The smallest and least energetic path of an electron around a nucleus

A

ground state

43
Q

A particle found in the nucleus

A

nucleon

44
Q

A negative particle having 1/1836 the mass of a proton

A

ellectron

45
Q

The average mass of an element

A

atomic mass

46
Q

1/12 the mass of the carbon-12 isotope

A

Atomic mass unit

47
Q

a positive electrode

A

cathode

48
Q

a quantum of radiant energy

A

photon

49
Q

the emission of electrons from the surface of a metal when struck by light

A

photoelectric effect

50
Q

the number of protons in an atom

A

atomic number

51
Q

the unit of frequency

A

herts

52
Q

the particles which make up atoms are called

A

subatomic particles

53
Q

the physical distance between the peaks of a wave

A

wavelength

54
Q

energy that exhibits wavelike behavior as it travels through space

A

electromagnetic spectrum

55
Q

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

A

photoelectric effect

56
Q

states that the energy was emittited in small, specific amounts of energy

A

Max Planck

57
Q

Minimum quantity of energy that can be lost or gained by an atom

A

quantum

58
Q

theory for a quantum

A

E=hv

59
Q

particle carrying a quantum energy and having zero mass

A

photon

60
Q

atoms absorb energy from heat or electricity and give off the energy as light

A

bright line spectrum

61
Q

___ explains the bright line spectra

A

Bohr’s model

62
Q

an electron goes to _____ state, then ___ then goes to a ____ level and becomes____ and returns to a _____, ___ is released as photon_spectral lines

A 
ground
excited
higher
unstable
lower
energy
63
Q

electrons have wavelength properties

A

de Broglie

64
Q

it’s impossible to determine simultaneously the position and velocity of an electron

A

uncertainty Principle’

Heinsenberg

65
Q

Dual wave particle properties

A

Schrodinger Wave equation

66
Q

describes mathematically the wave properties of electron

A

quantum theory

67
Q

average region of the most probably electron location

A

orbital

68
Q

energy level(1-7)

A

principle quantum number

69
Q

shape of orbital= s p d f

A

1 3 5 7

70
Q

orientation of the orbital around the nucleus

A

magnetic quantum number

71
Q

indicates the 2 fundamental spin states of an electron in an orbital

A

spin quantum number

72
Q

how many electrons can an orbital carry

and what must they have

A

2

opposite spins

73
Q

no 2 electrons have the same 4 quantum numbers

A

Pauli’s Exclusion Principle

74
Q

an electron occupies the lowest energy orbital that can recieve

A

Aufbau Principle

75
Q

A 2nd electron is not added to an orbital until each orbital in the sublevel contains one

A

Hund’s rule

76
Q

what’s the maximum # of electrons in the outer level of an atom

A

8

Junior 2015-2016 (15 decks)

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