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Chem 101 > Chapter 5 > Flashcards

Chapter 5 Flashcards

1
Q

Absorption spectrum

A

The spectrum associated with absorption of electromagnetic radiation by atoms (or other species) resulting from transitions from lower to higher electronic energy states

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2
Q

Alpha (⍺) particle

A

A helium ion with a 2+ charge; an assembly of two protons and two neutrons

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3
Q

amu

A

atomic mass unit. An arbitrary mass unity designed to be exactly one twelfth the mass of the carbon-12 isotope

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4
Q

Angular momentum quantum number (𝓁)

A

The quantum mechanical solution to a wave equation that designates the subshell, or set of orpitals (s, p, d, f), within a given main shell in which an electron resides

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5
Q

Anode

A

In a cathode-ray tube, the positive electrode

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6
Q

Atomic mass unit

A

An arbitrary mass unit defined to be exactly one twelfth the mass of the carbon-12 isotope

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7
Q

Atomic number

A

The integral number of protons in the nucleus; defines the identity of an element

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8
Q

Atomic orbital

A

The region or volume in space in which the probability of finding electrons is highest

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9
Q

Aufbau (“building up”) Principle

A

A guide for predicting the order in which electrons fill subshells and shells in atoms

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10
Q

Balmer-Rydberg equation

A

An emperical equation that relates wavelengths in the hydrogen emission spectrum to simple integers.

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11
Q

Canal ray

A

A stream of positivley charged particles (cations) that moves toward the negative electrode in a cathode-ray tube; observed to pass through canals (holes) in the negative electrode

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12
Q

Cathode

A

In a cathode-ray tube, the negative electrode

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13
Q

Cathode ray

A

The beam of electrons going from the negative electrode toward the positive electrode in a cathode-ray tube

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14
Q

Cathode-ray tube

A

A closed glass tube containing a gas under low pressure, with electrodes near the ends and a luminescent screen at the end near the positive electrode; produces cathode rays when high voltage is applied

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15
Q

Continuous spectrum

A

A spectrum that contains all wavelengths in a specified region of the electromagnetic spectrum

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16
Q

d orbitals

A

Beginning in the third shell, a set of five degenerate orbitals per shell, higher in energy than s and p orbitals in the same shell

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17
Q

Degenerate orbitals

A

Two or more orbitals that have the same energy

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18
Q

Diamagnetism

A

Weak repulsion by a magnetic field; associated with all electrons in an atom, molecule, or substance being paired.

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19
Q

Electromagnetic radiation

A

Energy that is propagated by means of electric and magnetic fields that oscillate in directions perpendicular to the direction of travel of the energy

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20
Q

Electron

A

A subatomic particle having a mass of 0.00054858 amu and a charge of 1-.

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21
Q

Elecron configuration

A

The specific distribution of electrons in the atomic orbitals of atoms and ions

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22
Q

Electron transition

A

The transfer of an electron from one energy level to another

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23
Q

Emission spectrum

A

The spectrum associted with emission of electromagnetic radiation by atoms (or other species) resulting from electron transitions from higher to lower energy states

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24
Q

Excited state

A

Any energy state other than the ground state of an atom, ion, or molecule

25
*f* orbitals
Beginning in the fourth shell, a set of seven degenerate orbitals per shell, higher in energy than *s*, *p*, and *d* orbitals in the same shell
26
Ferromagnetism
The property that allows a substance to become permanently magnetized when placed in a magnetic field; exhibited by iron, cobalt, and nicle and some of their alloys
27
Frequency (𝓋)
The number of crests of a wave that pass a given point per unit time
28
Fundamental particles
Subatomic particles of which all matter is composed; protons, electrons, and neutrons are fundamental particles
29
Ground state
The lowest energy state or most stable state of an atom, molecule, or ion
30
Group
A verticle column in the periodic table; also called a family
31
Heisenberg Uncertainty Principle
It is impossible to determine accurately both the momentum and position of an electron simultaneously
32
Hund's Rule
Each orbital of a given subshell is occupied by a single electron before pairing begins.
33
Isotopes
Two or more forms of atoms of the same element with different masses; that is, atoms containing the same number of protons but different numbers of neutrons.
34
Line spectrum
An atomic emission or absorption spectrum
35
Magnetic quantum number (𝓂𝓁)
Quantum mechanical solution to a wave equation that designates the particular orbital within a given subshell (*s*, *p*, *d*, *f*) in which an electron resides. The *px*, *py*, and *pz* orbitals have different magnetic quantum numbers.
36
Mass number
The integral sum of the numbers of protons and neutrons in an atom.
37
Mass spectrometer
An instrument that measures the charge-to-mass ratios of charged particles
38
Natural radioactivity
Spontaneous decomposition of an atom
39
Neutron
A subatomic nuclear particle having a mass of 1.0087 amu and no charge
40
Nucleus
The very small, very dense, positively charged center of an atom containing protons and neutrons, except for 11H
41
Nuclide symbol
The symbol for an atom AZE, in which E is the symbol for an element, Z is its atomic number, and A is its mass number
42
*p* orbitals
Beginning with the second shell, a set of three degenerate mutually perpendicular, equal-arm, dumbbell-shaped atomic orbitals per shell
43
Pairing of electrons
Interaction of two electrons with oposite *ms* values in the same orbital (↑↓)
44
Paramagnetism
Attraction toward a magnetic field, stronger than diamagntism, but still very weak compared with ferromagnetism; due to presence of unpaired electrons
45
Pauli Exclusion Principle
No two electrons in the same atom may have identical sets of four quantum numbers
46
Period
A horizontal row in the periodic table
47
Photoelectric effect
Emission of an electron from the surface of a metal, caused by impinging electromagnetic radiation of certain minimum energy; the resulting current increases with increasing intensity of radiation
48
Photon
A "packet" of light or electromagnetic radiation; also called a quanum of light
49
Principal quantum number (*n*)
The quantum mechanical solution to a wave equation that designates the main shell, or energy level, in wich an electron resides
50
Proton
A subatomic particle having a mass of 1.0073 amu and a charge of 1+, found in the nuclei of atoms
51
Quantum
A "packet" of energy
52
Quantum mechanics
A mathematical method of treating particles on the basis of quantum theory, which assumes that energy (of small particles) is not infinitely divisible.
53
Quantum numbers
Numbers that describe the energies of electrons in atoms; they are derived from quantum mechanical treatment
54
Radiant energy
Energy that is propagated by means of electric and magnetic fields that oscillate in directions perpendicular to the direction of travel of the energy
55
*s* orbital
A spherically symmetrical atomic orbital; one per shell
56
spectral line
Any of a number of lines corresponding to definite wavelengths in an atomic emission or absorption spectrum; these lines represent the energy difference between two energy levels
57
spectrum
Display of component wavelengths of electromagnetic radiation
58
spin quantum number (*m3*)
The quantum mechanical solution to a wave equation that indicates the relative spins of electrons ("spin up" and "spin down")
59
Wavelength (ƛ)
The distance between two identical points of a wave

Chem 101 (13 decks)

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