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General Chemistry I > Chapter 7 > Flashcards

Chapter 7 Flashcards

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1
Q

absorption spectrum

A

the spectrum produced when atoms absorb specific wavelengths of incoming light and become excited from lower to higher energy levels

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2
Q

amplitude

A

the height of the crest (or depth of the trough) of a wave; related to the intensity of the energy (brightness of the light)

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3
Q

angular momentum quantum number (l)

A

an integer from 0 to n − 1 that is related to the shape of an atomic orbital

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4
Q

atomic orbital

A

the wave function of an electron in an atom. the term is used qualitatively to mean the region of space in which there is a high probability of finding the electron

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5
Q

d orbital

A

an atomic orbital with l = 2

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6
Q

de Broglie wavelength

A

the wavelength of a moving particle obtained from the de Broglie equation: λ = h/mu

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7
Q

diffraction

A

he phenomenon in which a wave striking the edge of an object bends around it. a wave passing through a slit as wide as its wavelength forms a circular wave

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8
Q

electromagnetic radiation

A

oscillating, perpendicular electric and magnetic fields moving simultaneously through space as waves and manifested as visible light, x-rays, microwaves, radio waves, and so on

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9
Q

electromagnetic spectrum

A

the continuum of radiant energy arranged in order of increasing wavelength

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10
Q

electron cloud depiction

A

an imaginary representation of an electron’s rapidly changing position around the nucleus over time

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11
Q

electron density diagram

A

the pictorial representation for a given energy sublevel of the quantity ψ2 (the probability density of the electron lying within a particular tiny volume) as a function of r (distance from the nucleus)

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12
Q

emission spectrum

A

the line spectrum produced when excited atoms return to lower energy levels and emit photons characteristic of the element

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13
Q

excited state

A

any electron configuration of an atom (or ion or molecule) other than the lowest energy (ground) state

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14
Q

f orbital

A

an atomic orbital with l = 3

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15
Q

flame test

A

a procedure for identifying the presence of metal ions in which a granule of a compound or a drop of its solution is placed in a flame to observe a characteristic color

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16
Q

frequency

A

the number of complete waves, or cycles, that pass a given point per second, expressed in units of 1/second, or s−1 [also called hertz (Hz)]; related inversely to wavelength

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17
Q

ground state

A

the electron configuration of an atom (or ion or molecule) that is lowest in energy

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18
Q

infrared (IR)

A

the region of the electromagnetic spectrum between the microwave and visible regions

19
Q

level (shell)

A

a specific energy state of an atom given by the principal quantum number n

20
Q

line spectrum

A

a series of separated lines of different colors representing photons whose wavelengths are characteristic of an element

21
Q

magnetic quantum number

A

an integer from −l through 0 to +l that specifies the orientation of an atomic orbital in the three-dimensional space about the nucleus

22
Q

node

A

a region of an orbital where the probability of finding the electron is zero

23
Q

p orbital

A

an atomic orbital with l = 1

24
Q

photoelectric effect

A

the observation that, when monochromatic light of sufficient frequency shines on a metal, an electric current is produced

25
Q

photon

A

a quantum of electromagnetic radiation

26
Q

Planck’s constant (h)

A

a proportionality constant relating the energy and frequency of a photon, equal to 6.626 × 10−34 J·s

27
Q

principal quantum number (n)

A

a positive integer that specifies the energy and relative size of an atomic orbital; a number that specifies an energy level in an atom

28
Q

probability contour

A

a shape that defines the volume around an atomic nucleus within which an electron spends a given percentage of its time

29
Q

quantum

A

a packet of energy equal to hν. the smallest quantity of energy that can be emitted or absorbed

30
Q

quantum mechanics

A

the branch of physics that examines the wave nature of objects on the atomic scale

31
Q

quantum number

A

a number that specifies a property of an orbital or an electron

32
Q

radial probability distribution plot

A

the graphic depiction of the total probability distribution (sum of ψ2) of an electron in the region near the nucleus

33
Q

refraction

A

a phenomenon in which a wave changes its speed and therefore its direction as it passes through a phase boundary into a different medium

34
Q

s orbital

A

an atomic orbital with l = 0

35
Q

Schrodinger equation

A

an equation that describes how the electron matter-wave changes in space around the nucleus. solutions of the equation provide energy states associated with the atomic orbitals

36
Q

spectrometry

A

any instrumental technique that uses a portion of the electromagnetic spectrum to measure the atomic and molecular energy levels of a substance

37
Q

speed of light (c)

A

a fundamental constant giving the speed at which electromagnetic radiation travels in a vacuum: c = 2.99792458 × 108 m/s

38
Q

stationary state

A

in the Bohr model, one of the allowable energy levels of the atom in which it does not release or absorb energy

39
Q

sublevel (subshell)

A

an energy substate of an atom within a level. given by the n and l values, the sublevel designates the size and shape of the atomic orbitals

40
Q

ultraviolet (UV)

A

radiation in the region of the electromagnetic spectrum between the visible and the x-ray regions

41
Q

uncertainty principle

A

the principle stated by Heisenberg that it is impossible to know simultaneously the exact position and velocity of a particle; the principle becomes important only for particles of very small mass

42
Q

wavelength

A

the distance between any point on a wave and the corresponding point on the next wave, that is, the distance a wave travels during one cycle

43
Q

wave-particle duality

A

the principle stating that both matter and energy have wavelike and particle-like properties

General Chemistry I (12 decks)

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