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Chemistry 142 > Chapter 12: Quantum Mechanics and Atomic Theory > Flashcards

Chapter 12: Quantum Mechanics and Atomic Theory Flashcards

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1
Q

electromagnetic radiation

A

radiant energy that exhibits wavelike behavior and travels through space at the speed of light in a vacuum

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2
Q

wavelength

A

the distance between two consecutive peaks or troughs in a wave

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3
Q

frequency

A

the number of waves (cycles) per second that pass a given point in space

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4
Q

continuos spectrum

A

a spectrum that exhibits all the wavelengths of visible light

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5
Q

Planck’s constant

A

the constant relating the change in energy for a system to the frequency of the electromagnetic radiation absorbed or emitted: 6.626x10^-34 Js

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6
Q

quantized

A

the concept that energy can occur only in discrete units called quanta

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7
Q

photon

A

a quantum of electromagnetic radiation

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8
Q

photoelectric effect

A

the emission of electrons when electromagnetic radiation, such as light, hits a material

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9
Q

dual nature of light

A

the statement that light exhibits both wave and particulate properties

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10
Q

diffraction

A

the scattering of light from a regular array of points or lines, producing constructive and destructive interference

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11
Q

line spectrum

A

a spectrum showing only certain discrete wavelengths

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12
Q

ground state

A

the lowest possible energy state of an atom or molecule

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13
Q

wave mechanics (quantum mechanics)

A

the relationship between the motion of a particle that exhibits wavelike properties (such as an electron) and its allowed energies

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14
Q

wave functions

A

a function of the coordinates of an electro’s position in 3-d space that describes the properties of an electron

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15
Q

orbital

A

a specific wave function for an electron in an atom. The square of this function gives the probability distribution for the electron

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16
Q

Heisenberg uncertainty principle

A

a principle stating there is a fundamental limitation to how precisely both the position and momentum of a particle can be known at a given time

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17
Q

probability distribution

A

the square o the wave function indicating the probability of finding an electron at a particular point in space

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18
Q

quantum numbers

A

value that is used when describing the energy levels available to atoms and molecules
an electron or ion has four quantum numbers to describe its state

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19
Q

principle quantum numbers (n)

A

the quantum number relating to the size and energy of an orbital; it can have any positive integer value

20
Q

angular momentum quantum numbers (1)

A

the quantum number relating to the shape of an atomic orbital, which can assume any integral value from 0 to n-1 for each value of n

21
Q

magnetic quantum number (m1)

A

the quantum number relating to the orientation of an orbital in space relative to the other orbital in space relative to the other orbitals with the same quantum number. it can have integer levels between l and -l

22
Q

sub-shell

A

a set of orbitals with a given angular momentum quantum number

23
Q

nodal surfaces (nodes)

A

an area of an orbital having zero electron probability

24
Q

lobe pair

A

an electron pair that is localized on a given atom; an electron pair not involved in bonding

25
Q

degenerate orbital

A

a group of orbitals with the same energy

26
Q

electron spin quantum number

A

a quantum number representing one of the two possible values for the electron spin; either +1/2 or -1/2

27
Q

Pauli exclusion principle

A

in a given atom no two electrons can have the same set of four quantum numbers

28
Q

Polyelectronic tom

A

an ion containing a number of atoms

29
Q

effective nuclear charge

A

the apparent nuclear charge exerted on a particular electron, equal to the actual nuclear charge minus the effect of electron repulsions

30
Q

self-consistent field (SCF) method

A

is an iterative method that involves selecting an approximate Hamiltonian, solving the Schrödinger equation to obtain a more accurate set of orbitals, and then solving the Schrödinger equation again with theses until the results converge

31
Q

triads

A

any of several sets of three chemically similar elements

32
Q

octaves

A

the chemical elements are arranged according to increasing atomic weight, those with similar physical and chemical properties occur after each interval of seven elements

33
Q

Aufbau principle

A

Aufbau Principle states that in ground state of an ion, electrons fill atomic orbitals of lowest available energy levels before occupying higher levels. This means that the orbital with lower energy will be filled first followed by the orbital of higher energy.

34
Q

Hund’s rule

A

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied

35
Q

valance electrons

A

electrons in the outermost shell, or energy level, of an atom. - valance electrons = group number

36
Q

core electrons

A

the electrons in an atom that are not valence electrons and do not participate in chemical bonding

37
Q

transition metals

A

n element that has the ability to form stable cations with an incompletely filled d orbitals

38
Q

lanthanide series

A

rare-earth metals (14)

39
Q

actinide series

A

includes mostly man-made elements

40
Q

shielding

A

the blocking of valence shell electron attraction by the nucleus, due to the presence of inner-shell electrons.

41
Q

ionization energy

A

he amount of energy required to remove an electron from an isolated atom or molecule: increases from left to right

42
Q

first ionizing energy

A

is the energy needed to remove the outermost, or highest energy, electron from a neutral atom in the gas phase

43
Q

second ionizing energy

A

the energy required to remove the outermost, or least bound, electron from a 1+ ion of the element

44
Q

electron affinity

A

an electron is added to a neutral atom to form a negatively charged ion.: same increase pattern as ionization

45
Q

atomic radii

A

The atomic radius of a chemical element is a measure of the size of its atoms

Chemistry 142 (2 decks)

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