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×Chemistry 1 > Arrangement of Electrons in Atoms > Flashcards

Arrangement of Electrons in Atoms Flashcards

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1
Q

electromagnetic radiation

A

a form of energy that exhibits wavelike behavior as it travels through space

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2
Q

electromagnetic spectrum

A

all the forms of electromagnetic radiation

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3
Q

constant speed of all forms of electromagnetic radiation

A

3.0 × 108 meters per second

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4
Q

speed of light (c)

A

3.0 × 108 meters per second

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5
Q

wavelength (λ)

A

the distance between corresponding points on adjacent waves

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6
Q

units for wavelength

A

meter

centimeter

nanometer

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7
Q

frequency (v)

A

the number of waves that pass a given point in a specific time (usually 1 second)

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8
Q

units for frequency

A

waves per second

hertz (Hz)

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9
Q

Hertz (Hz)

A

unit of measurement for frequency

equal to 1 wave per second

named for Heinrich Hertz

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10
Q

mathematical relationship between frequency and wavelength

A

c = λv

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11
Q

wavelength range of visible light

A

400nm to 700nm

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12
Q

types of electromagnetic radiation (in order of increasing wavelength)

A

gamma rays

X-rays

ultra-violet

visible light

infrared

microwaves

radio waves

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13
Q

types of electromagnetic radiation (in order of increasing frequency)

A

radio waves

microwaves

infrared

visible light

ultra-violet light

X-rays

gamma rays

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14
Q

types of electromagnetic radiation (in order of increasing energy)

A

radio waves

microwaves

infrared

visible light

ultra-violet light

X-rays

gamma rays

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15
Q

quantum

A

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

same thing as a photon

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16
Q

Planck’s constant (h)

A

6.626 × 10-34 joules by seconds

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17
Q

energy (E)

A

power that may be translated into motion, overcoming resistance, or causing a physical change

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18
Q

mathematical relationship between a quantum of energy and the frequency of radiation

A

E = hv

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19
Q

photon

A

a particle of electromagnetic radiation having 0 mass and carrying a quantum of energy

same thing as a quantum

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20
Q

energy of a photon

A

Ephoton = hv

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21
Q

ground state

A

the lowest energy state of an atom

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22
Q

excited state

A

a state in which an atom has a higher potential energy than it has in its ground state

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23
Q

continuous spectrum

A

the emission of a continuous range of frequencies of electromagnetic radiation

24
Q

emission spectrum

A

the spectrum of light released from excited atoms of an element

25
Q

absorbtion spectrum

A

the spectrum of light absorbed from ground-state atoms of an element

26
Q

Bohr’s model of the hydrogen atom

A

structural model in which an electron moves around the nucleus only in circular orbits

linked the atom’s electron with photon emission

explained that energy of electron is higher when in orbits that are successively farther from nucleus

27
Q

quantum theory

A

describes mathematically the wave properties of electrons and other very small particles

28
Q

quantum numbers

A

specify the properties of atomic orbitals and the properties of electrons in orbitals

29
Q

principal quantum number

A

indicates distance from nucleus

30
Q

informal name for principal quantum number

A

energy levels

31
Q

identification of principal quantum number

A

periods on periodic table

32
Q

symbol of principal quantum number

A

n

33
Q

range of principal quantum number

A

1 to 7

34
Q

angular momentum quantum number

A

indicates the shape of the orbital

35
Q

informal name for angular momentum quantum number

A

sublevels

36
Q

symbol of angular momentum quantum number

A

l

37
Q

range of angular momentum quantum number

A

0 to 3

38
Q

magnetic quantum number

A

indicates the orientation of an orbital around the nucleus

39
Q

informal name for magnetic quantum number

A

orbital

40
Q

symbol of magnetic quantum number

A

m

41
Q

range of magnetic quantum number

A

-3 to 0 to 3

42
Q

spin quantum number

A

indicates relation of electrons on axis

43
Q

informal name for spin quantum number

A

spin

44
Q

symbol of spin quantum number

A

s

45
Q

range of spin quantum number

A

ranges from -0.5 to 0.5

46
Q

3 basic rules of electron configuration

A

aufbau principle

Pauli exclusion principle

Hund’s rule

47
Q

aufbau principle

A

states that an electron occupies the lowest-energy orbital that can receive it

derived from the German word meaning “building-up”

discovered by Bohr and Pauli

48
Q

Pauli exclusion principle

A

states that no 2 electrons in the same atom can have the same set of 4 quantum numbers

49
Q

Hund’s rule

A

states that orbitals of equal energy are each occupied by 1 electron before any orbital is occupied by a second electron, and all electrons in singularly occupied orbitals must have the same spin state

50
Q

3 methods of indicating electron configuration

A

orbital notation

electron-configuration notation

noble gas notation

51
Q

orbital notation

A

a diagramic representation that uses dashes and arrows to show the principal energy levels and sublevels for all the electrons in an atom

52
Q

electron-configuration notation

A

method of writing the electron configuration of elements in which coefficients represent the energy level that the electron occupies with the letter of its sublevel and superscripts represent the number of electrons present in an atomic orbital

53
Q

noble gas notation

A

an abbreviated version of electron-configuration notation in which filled inner shells are represented by the symbol of the preceding noble gas in brackets

54
Q

noble gas configuration

A

an outer main energy level fully occupied (in most cases) by 8 electrons

55
Q

highest occupied level

A

electron-containing main energy level with the highest principal quantum number

56
Q

inner-shell electrons

A

electrons that are not in the highest occupied energy level

×Chemistry 1 (20 decks)

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