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CHEM 1201 > CH. 6 > Flashcards

CH. 6 Flashcards

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1
Q

refers to the number of electrons in the atom as well as their distribution around the nucleus and their energies

A

electronic structure

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2
Q

form of energy that has wave characteristics and that propagates through a vacuum at 2.998x10^8 *(the speed of light)

A

electromagnetic radiation (radiant energy)

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3
Q

distance between two adjacent peaks

A

wavelength

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4
Q

number of complete wavelengths (cycles) that pass a given point each second

A

frequency

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5
Q

do all electromagnetic radiation move at different speeds

A

no (they all move at the same speed, the speed of light)

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6
Q

cycles per second

A

hertz

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7
Q

frequency is expressed in ____

A

hertz

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8
Q

what are the three observations that can be made about the wave model of light

A

blackbody radiation, photoelectric effect, emission spectra

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9
Q

the emission of light from hot objects

A

blackbody radiation

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10
Q

the emission of electrons from metal surfaces on which light shines

A

photoelectric effect

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11
Q

the emission of light from electronically excited gas atoms

A

emission spectra

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12
Q

when solids are heated they emit _____

A

radiation

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13
Q

smallest amount of energy that can be emitted or absorbed as electromagnetic radiation

A

quantum

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14
Q

who proposed that energy can be either released or absorbed by atoms only in discrete chunks of some minimum size (won the noble prize for quantum theory)

A

max planck

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15
Q

6.626x10^-34

A

plancks constant

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16
Q

who proposed the photoelectric effect

A

albert einstein

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17
Q

particles of energy

A

photon

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18
Q

each photon must have the energy equal to the ____ ____ times the ____ of the ____

A

plancks constant, frequency, light

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19
Q

who offered a theoretical explanation of line spectra

A

niels bohr

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20
Q

radiation composed of a single wavelength is

A

monochromatic

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21
Q

radiation containing many different wavelengths

A

polychroamtic

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22
Q

produced when radiation from a polychromatic source is separated into its component wavelengths

A

spectrum

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23
Q

rainbow of colors containing light of all wavelengths

A

continuous spectrum

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24
Q

spectrum containing radiation of only specific wavelengths

A

line spectrum

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25
Q

what are the three postulates of bohrs model

A

only orbits of certain radii are permitted for the electron in a hydrogen atom, an electron in a permitted orbit is in an allowed energy state (an electron

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25
Q

what are the three postulates of bohrs model

A

only orbits of certain radii are permitted for the electron in a hydrogen atom, an electron in a permitted orbit is in an allowed energy state (an electron

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25
Q

what are the three postulates of bohrs model

A

only orbits of certain radii are permitted for the electron in a hydrogen atom
an electron in a permitted orbit is in an allowed energy state, an electron in an allowed energy state does not radiate energy and does not spiral into the nucleus
energy is emitted or absorbed by the electron only as the electron changes from one allowed energy state to another

26
Q

the lower (more negative) the energy is, the more ___ the atom is

A

stable

27
Q

the lowest energy state

A

ground state

28
Q

when the electron is in a higher-energy state

A

excited state

29
Q

the energy of the photon must ____ the difference in energy between the two states

A

equal

30
Q

when change of e (delta e) is positive, a photon must be ____ as the electron jumps to a higher energy

A

absorbed

31
Q

when change of e (delta e) is negative, a photon is ___ as the electron falls to a lower energy level

A

emitted

32
Q

what are three limitations of the bohr model

A

cannot explain the spectra of other atoms, does not explain why the negatively charged electron would not just fall into the positively charged nucleus, electron orbiting the nucleus at a fixed distance is not accurate

33
Q

what are two important ideas of the bohr model

A

electrons exist only in certain discrete energy levels (described by quantum numbers), energy is involved in the transition of an electron from one level to another

34
Q

who proposed that an electron moving about the nucleus of an atom behaves like a wave and has a wavelength

A

louis de broglie

35
Q

describes the wave characteristics of material particles

A

matter waves

36
Q

when applied to the electrons in an atom, this principle states that it is impossible for us to know simultaneously both the exact momentum of an electron and its exact location in space

A

uncertainty principle

37
Q

mathematical functions that describe the electron in the atom

A

wave functions

38
Q

photon or particle exists simultaneously in two different quantum states

A

cat state

39
Q

collection of orbitals with the same value of n

A

electron shell

40
Q

set of orbitals that have the same n and l values

A

subshell

41
Q

the shell with principal quantum number n consists of exactly ___ subshells

A

n

42
Q

each subshell consists of a specific number of ____

A

orbitals

43
Q

the total number of orbitals in a shell is ___, where n is the principal quantum number of the shell

A

n2

44
Q

the electron density for the s orbitals are

A

spherically symmetric (electron density at a given distance from the nucleus is the same regardless of the direction in which we proceed from the nucleus)

45
Q

for an ns orbital the number of peaks is equal to __ with the outermost peak being larger than inner ones

A

n

46
Q

for an ns orbital the number of nodes is equal to

A

n-1

47
Q

as n increases, the electron density becomes __ spread out, there is a greater probability of finding the electron further from the nucleus

A

more

48
Q

in a many electron atom, for a given value of n, the energy of an orbital increases with increasing value of

A

1

49
Q

orbitals with the same energy are said to be

A

degenerate

50
Q

intrinsic property that causes each electron to behave as if it were a tiny sphere spinning on its own axis

A

electron spin

51
Q

states that no two electron in an atom can have the same set of four quantum numbers (n, l, m1, ms)

A

pauli exclusion principle

52
Q

an orbital can hold a maximum of ___ electrons and they must have _____ spins

A

two, opposite

53
Q

the way electron are distributed among various orbitals of an atom

A

electron configuration

54
Q

the orbitals are filled in order of ___ energy, with no more than ___ electrons per orbital

A

increasing, 2

55
Q

represents an electron with a positive spin magnetic quantum number

A

half arrow pointing up

56
Q

represents an electron with a negative spin magnetic quantum number

A

half arrow pointing down

57
Q

when filling degenerate orbitals the lowest energy is attained when the number of electrons having the same spin is maximized (electrons occupy orbitals singly to the maximum extent possible and that these single electrons in a given subshell all have the same spin magnetic quantum number)

A

hunds rule

58
Q

the 14 elements corresponding to the filling of the 4f oribtals are known as

A

lanthanide elements (rare earth elements)

59
Q

the s block and the p block elements together are the

A

representative elements (main group elements)

60
Q

elements in which the valence d orbitals are being filled and make up the d block

A

transition metals

61
Q

for representative elements we do not consider the electrons in completely filled d or f subshell to be ___ ___

A

valence electrons

62
Q

for transition elements we do not consider the electrons in a completely filled f subshell to be _____ ____

A

valence electrons

63
Q

there is an ___ relationship between frequency and wavelength

A

inverse

CHEM 1201 (3 decks)

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