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CHM 151 > CHAPTER 3 ELECTRONIC STRUCTURE AND PERIODIC PROPERTIES OF ELEMENTS > Flashcards

CHAPTER 3 ELECTRONIC STRUCTURE AND PERIODIC PROPERTIES OF ELEMENTS Flashcards

1
Q

inner transition metal in the bottom of the bottom two rows of the periodic table

A

actinide

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2
Q

element in group 1

A

alkali metal

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3
Q

element in group 2

A

alkaline earth metal

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4
Q

extent of the displacement caused by a wave

A

amplitude

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5
Q

mathematical function that describes the behavior of an electron in an atom (also called the wavefunction)

A

atomic orbital

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6
Q

procedure in which the electron configuration of the elements is determined by “building” them in order of atomic numbers, adding one proton to the nucleus and one electron to the proper subshell at a time

A

Aufbau principle

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7
Q

idealized perfect absorber of all incident electromagnetic radiation; such bodies emit electromagnetic radiation in characteristic continuous spectra called blackbody radiation

A

blackbody

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8
Q

structural model in which an electron move around the nucleus only in circular orbits, each with a specific allowed radius

A

Bohr’s model of the hydrogen atom

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9
Q

element in group 16

A

chalcogen

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10
Q

electromagnetic radiation given off in a n unbroken series of wavelengths(e.g., white light from the sun)

A

continuous spectrum

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11
Q

electron in a n atom that occupies the orbitals of the inner shells

A

core electron

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12
Q

attractive force between the nuclei of a molecule’s atoms and pairs of electrons between the atoms

A

covalent bond

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13
Q

(also, molecular compound) composed of molecules formed by atoms of two or more different elements

A

covalent compound

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14
Q

one-half the distance between the nuclei of two identical atoms when they are joined by a covalent bond

A

covalent radius

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15
Q

region of space with high electron density that is either four lobed or contains a dumbbell and torus shape; describes orbitals l = 2.

A

d orbital

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16
Q

orbitals that have the same energy

A

degenerate orbitals

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17
Q

charge that leads to the Coulomb force exerted by the nucleus on an electron, calculated as the nuclear charge minus shielding

A

effective nuclear charge

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18
Q

energy transmitted by waves that have an electric-field component and a magnetic-field component

A

electromagnetic radiation

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19
Q

range of energies that electromagnetic radiation can comprise, including radio, microwaves, infrared, visible, ultraviolet, X-rays, and gamma rays

A

electromagnetic spectrum

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20
Q

energy change associated with addition of an electron to a gaseous atom or ion

A

electron affinity

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21
Q

listing that identifies the electron occupancy of an atom’s shells and sub shells

A

electron configuration

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22
Q

a measure of the probability of locating an electron in a particular region of space, it is equal to the squared absolute value of the wave function

A

electron density

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23
Q

processes that increase the energy of an atom and involve the absorption of light

A

endothermic

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24
Q

state having an energy greater than the ground-state energy

A

excited state

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25
Q

processes that decrease the energy of an atom and involve the emission of light

A

exothermic

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26
Q

multilobed region of space with high electron density, describes orbitals with l = 3

A

f orbital

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27
Q

number of wave cycles(peaks or troughs) that pass a specified point in space per unit time

A

frequency (v)

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28
Q

state in which the electrons in an atom, ion , or molecule have the lowest energy possible

A

ground state

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29
Q

vertical column of the periodic table

A

group

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30
Q

element in group 17

A

halogen

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31
Q

rule stating that it is impossible to exactly determine both certain conjugate dynamical properties such as the momentum and the position of a particle at the same time. The uncertainty principle is a consequence of quantum particles exhibiting wave-particle duality

A

Heisenberg uncertainty principle

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32
Q

the unit of frequency, which is the number of cycle per second, s^-1

A

hertz(Hz)

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33
Q

every orbital in a sub shell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin

A

Hund’s rule

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34
Q

(also, noble gas) element in group 18

A

inert gas

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35
Q

(also, lanthanide or actinide) element in the bottom two rows; if in the first row, also called lanthanide, or if in the second row, also called actinide

A

inner transition metal

36
Q

interference pattern

A

pattern typically consisting of alternating bright and dark fringes; it results from constructive and destructive interference of waves

37
Q

property of wave-propagated energy related to the amplitude of the wave, such as brightness of light or loudness of sound

A

intensity

38
Q

electrostatic forces of attraction between the oppositely charged ions of an ionic compound

A

ionic bond

39
Q

compound composed of cations and anions combined in ratios, yielding an electrically neutral substance

A

ionic compound

40
Q

energy required to remove an electron from a gaseous atom or ion

A

ionization energy

41
Q

group of ions or atoms that have identical electron configurations

A

isoelectronic

42
Q

inner transition metal in the top of the bottom two rows of the periodic table

A

lanthanide

43
Q

electromagnetic radiation emitted at discrete wavelengths by a specific atom (or atoms) in an excited state

A

line spectrum

44
Q

quantum number signifying the orientation of an atomic orbital around the nucleus

A

magnetic quantum number (m.l)

45
Q

(also, representative element) element in groups 1, 2, and 13-18

A

main-group element

46
Q

element that is shiny, malleable good conductor of heat and electricity

A

metal

47
Q

element that conducts heat and electricity moderately well, and possesses some properties of metals and some properties of nonmetals

A

metalloid

48
Q

(also, covalent compound) composed of molecules formed by atoms of two or more different elemetns

A

molecular compound

49
Q

ion composed of a single atom

A

monatomic ion

50
Q

(also, inert gas) element in group 18

A

noble gas

51
Q

any point of a standing wave with zero amplitude

A

node

52
Q

element that appears dull, poor conductor of heat and electricity

A

nonmetal

53
Q

pictorial representation of the electron configuration showing each orbital as a box and each electron as an arrow

A

orbital diagram

54
Q

polyatomic anion composed of a central atom bonded to oxygen atoms

A

oxyanion

55
Q

dumbbell-shaped region of space with ihg electron density, describes orbitals with l = 1

A

p orbital

56
Q

specifies that no two electrons in an atom can have the same value for all four quantum numbers

A

Pauli exclusion principle

57
Q

(also, series) horizontal row of the periodic table

A

period

58
Q

properties of the elements are periodic function of their atomic numbers

A

periodic law

59
Q

table of the elements that places elements with similar chemical properties close together

A

periodic table

60
Q

smallest possible packet of electromagnetic radiation, a particle of light

A

photon

61
Q

element in group 15

A

pnictogen

62
Q

ion composed of more than one atom

A

polyatomic ion

63
Q

quantum number specifying the shell an electron occupies in an atom

A

principal quantum number (n)

64
Q

limitation of some property to specific discrete values, not continuous

A

quantization

65
Q

field of study that includes quantization of energy, wave-particle duality, and the Heisenberg uncertainty principle to describe matter

A

quantum mechanics

66
Q

number having only specific allowed values and used to characterize the arrangement of electrons in an atom

A

quantum number

67
Q

(also, main-group element) element in columns 1, 2, and 12-18

A

representative elemtn

68
Q

spherical region of space with high electron density, describes orbitals with l =0

A

s orbital

69
Q

quantum number distinguishing the different shapes of orbitals; it is also a measure of the orbital angular momentum

A

secondary(angular momentum) quantum number (l)

70
Q

(also, period) horizontal row of the period table

A

series

71
Q

atomic orbitals with the same principal qunatum number, n

A

shell

72
Q

number specifying the electron spin direction, either + 1/2 or - 1/2

A

spin quantum number(m.s)

73
Q

(also, stationary wave) localized wave phenomenon characterized by discrete wavelengths determined by the boundary conditions used to generate the waves; standing waves are inherently quantized

A

standing wave

74
Q

atomic orbitals with the same values of n and l

A

subshell

75
Q

element in groups 3-12(more strictly define, 3-11; see chapter on transition metals and coordination chemistry)

A

transition metal

76
Q

electrons in the outermost of valence shell (highest value of n) of a ground-state atom

A

valence electrons

77
Q

outermost shell of electrons in a ground-state atom

A

valence shell

78
Q

oscillation of a property over time or space; can transport energy from one point to another

A

wave

79
Q

observation that elementary particles can exhibit both wave-like and particle-like properties

A

wave-particle duality

80
Q

mathematical description of an atomic orbital that describes the shape of the orbital; it can be used to calculate the probability of finding the electron at any given location in the orbital, as well as dynamical variables such as the energy and the angular momentum

A

wavefunction (w)

81
Q

distance between two consecutive peaks or troughs in a wave

A

wavelength(lambda)

82
Q

c = λν

A

(speed of light) = (wavelength)(velocity)

83
Q

E=hν=hcλ, where h = 6.626 × 10−34 J s

A

(Energy) = (Planck’s constant)(velocity) = (Planck’s constant)(speed of light)(wavelength)

84
Q

1/λ=R∞(1/n21−1/n22)

A

1/(wavelength)=(Rydberg constant)(1/n1^2 - 1/n2^2)

85
Q

En=−kZ2/n2,n=1,2,3,…

A

(Energy)n = -kZ^2/n^2, n = positive integer

86
Q

ΔE=kZ2(1n/21−1n/22)

A

(Change in Energy) = kZ^2(1/n1^2-1/n2^2)

87
Q

r=n2/Za0

A

r = n^2/Z a0

CHM 151 (4 decks)

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