Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chem 101 > Chapter 5 > Flashcards

Chapter 5 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Physics 101 flashcards Psychology 101 flashcards Chemistry 101 flashcards AP® Chemistry flashcards Biology 101 flashcards Organic Chemistry 101 flashcards Sociology 101 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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Alpha (⍺) particle

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

amu

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Anode

A

In a cathode-ray tube, the positive electrode

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Atomic mass unit

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Atomic number

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Atomic orbital

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Aufbau (“building up”) Principle

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Balmer-Rydberg equation

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Cathode

A

In a cathode-ray tube, the negative electrode

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Cathode ray

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Continuous spectrum

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Degenerate orbitals

A

Two or more orbitals that have the same energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Diamagnetism

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Electron

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Elecron configuration

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Electron transition

A

The transfer of an electron from one energy level to another

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Excited state

A

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

25
Q

f orbitals

A

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
Q

Ferromagnetism

A

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
Q

Frequency (𝓋)

A

The number of crests of a wave that pass a given point per unit time

28
Q

Fundamental particles

A

Subatomic particles of which all matter is composed; protons, electrons, and neutrons are fundamental particles

29
Q

Ground state

A

The lowest energy state or most stable state of an atom, molecule, or ion

30
Q

Group

A

A verticle column in the periodic table; also called a family

31
Q

Heisenberg Uncertainty Principle

A

It is impossible to determine accurately both the momentum and position of an electron simultaneously

32
Q

Hund’s Rule

A

Each orbital of a given subshell is occupied by a single electron before pairing begins.

33
Q

Isotopes

A

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
Q

Line spectrum

A

An atomic emission or absorption spectrum

35
Q

Magnetic quantum number (𝓂𝓁)

A

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
Q

Mass number

A

The integral sum of the numbers of protons and neutrons in an atom.

37
Q

Mass spectrometer

A

An instrument that measures the charge-to-mass ratios of charged particles

38
Q

Natural radioactivity

A

Spontaneous decomposition of an atom

39
Q

Neutron

A

A subatomic nuclear particle having a mass of 1.0087 amu and no charge

40
Q

Nucleus

A

The very small, very dense, positively charged center of an atom containing protons and neutrons, except for 11H

41
Q

Nuclide symbol

A

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
Q

p orbitals

A

Beginning with the second shell, a set of three degenerate mutually perpendicular, equal-arm, dumbbell-shaped atomic orbitals per shell

43
Q

Pairing of electrons

A

Interaction of two electrons with oposite ms values in the same orbital (↑↓)

44
Q

Paramagnetism

A

Attraction toward a magnetic field, stronger than diamagntism, but still very weak compared with ferromagnetism; due to presence of unpaired electrons

45
Q

Pauli Exclusion Principle

A

No two electrons in the same atom may have identical sets of four quantum numbers

46
Q

Period

A

A horizontal row in the periodic table

47
Q

Photoelectric effect

A

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
Q

Photon

A

A “packet” of light or electromagnetic radiation; also called a quanum of light

49
Q

Principal quantum number (n)

A

The quantum mechanical solution to a wave equation that designates the main shell, or energy level, in wich an electron resides

50
Q

Proton

A

A subatomic particle having a mass of 1.0073 amu and a charge of 1+, found in the nuclei of atoms

51
Q

Quantum

A

A “packet” of energy

52
Q

Quantum mechanics

A

A mathematical method of treating particles on the basis of quantum theory, which assumes that energy (of small particles) is not infinitely divisible.

53
Q

Quantum numbers

A

Numbers that describe the energies of electrons in atoms; they are derived from quantum mechanical treatment

54
Q

Radiant energy

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

55
Q

s orbital

A

A spherically symmetrical atomic orbital; one per shell

56
Q

spectral line

A

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
Q

spectrum

A

Display of component wavelengths of electromagnetic radiation

58
Q

spin quantum number (m3)

A

The quantum mechanical solution to a wave equation that indicates the relative spins of electrons (“spin up” and “spin down”)

59
Q

Wavelength (ƛ)

A

The distance between two identical points of a wave

Chem 101 (13 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions