Chapter 3: Atomic Structure

Question 0

Electromagnetic spectrum

Answer 0

A continuous range of radiant energy that includes Gamma Rays, x-rays, ultraviolet radiation, visible light, infrared radiation, and radio waves.

Question 1

Electromagnetic radiation

Answer 1

Any form of radiant energy in the electromagnetic spectrum.

Question 2

Wavelength

Answer 2

The distance from crest to crest or trough to trough on a wave.

Question 3

Frequency (v)

Answer 3

The number of crests of a wave that pass a stationary point of reference per second.

Question 4

Herts (Hz)

Answer 4

The SI unit of frequency with units of reciprocal seconds: 1 Hz = 1s^-1 = 1 cycle per second (cps)

Question 5

Fraunhofer lines

Answer 5

A set of dark lines in the otherwise continuous solar spectrum.

Question 6

Atomic emission spectra

Answer 6

Characteristic patterns of bright lines produced when atoms are vaporized in high-temperature flames or electrical discharges.

Question 7

Atomic absorption spectra

Answer 7

Characteristic patterns of dark lines produced when an external source of radiation passes through free, gaseous atoms.

Question 8

Quantum

Answer 8

The smallest discrete quantity of a particular form of energy.

Question 9

Planck constant (h)

Answer 9

The proportionality constant between the energy and frequency of electromagnetic radiation expressed in E=hv; h=6.626x10^-34 J x s

Question 10

Quantum theory

Answer 10

A model based on the idea that energy is absorbed and emitted in discrete quantities of energy called quanta.

Question 11

Quantized

Answer 11

Having values restricted to whole-number multiples of a specific base value.

Question 12

Photon

Answer 12

A quantum of electromagnetic radiation.

Question 13

Photoelectric effect

Answer 13

The release of electrons from a material as a result of electromagnetic radiation striking it.

Question 14

Threshold frequency

Answer 14

The minimum frequency of light required to produce the photoelectric effect.

Question 15

Work function

Answer 15

The amount of energy needed to dislodge an electron from the surface of a material.

Question 16

Ground state

Answer 16

The most stable, lowest energy state of a particle.

Question 17

Excited state

Answer 17

Any energy state above the ground state.

Question 18

Electron transition

Answer 18

Movement of an electron between energy levels.

Question 19

Matter wave

Answer 19

The wave associated with any moving particle.

Question 20

Standing wave

Answer 20

A wave confined to a given space with a wavelength (lambda) related to the length L of the space by L=(lambda/2), where n is a whole number.

Question 21

Node

Answer 21

A location in a standing wave that experiences no displacement.

Question 22

Heisenberg uncertainty principle

Answer 22

The principle that one cannot simultaneously know the exact position and the exact momentum of an electron.

Question 23

Wave mechanics or quantum mechanics

Answer 23

A mathematical description of the wavelike behavior of electrons and other particles.

Question 24

Schrödinger wave equation

Answer 24

A description of how the electron matter wave varies with location and time around the nucleus of a hydrogen atom.

Question 25

Wave function (phi)

Answer 25

A solution to the Schrödinger wave equation.

Question 26

Orbitals

Answer 26

Defined by the square of the wave function (phi); regions in an atom where the probability of finding an electron is high.

Question 27

Quantum number

Answer 27

One of four related numbers that specify the energy, shape, and orientation of orbitals in an atom and the spin orientation of electrons in the orbitals.

Question 28

Principle quantum number (n)

Answer 28

A positive integer describing the relative size and energy of an atomic orbital or group of orbitals in an atom.

Question 29

Angular momentum quantum number (l)

Answer 29

An integer having any value from 0 to (n-1) that defines the shape of an orbital.

Question 30

Magnetic quantum number (m(base l))

Answer 30

Defines the orientation of an orbital in space; an integer that may have any value from -l to +l, where l is the angular momentum quantum number.

Question 31

Spin quantum number (m(base s))

Answer 31

Either + 1/2 or -1/2, indicating the spin orientation of an electron.

Question 32

Pauli exclusive principle

Answer 32

No two electrons in an atom can have the same set of four quantum numbers.

Question 33

Aufbau principle

Answer 33

The method of building. Electron configurations of atoms by adding one electron at a time as atomic numbers increases across the rows of the periodic table.

Question 34

Electron configuration

Answer 34

The distribution of electrons among the orbitals of an atom or ion.