Chemistry - Ch 6

Question 1

Electronic structure (of atoms)

Answer 1

arrangements of electrons in atoms

Question 2

Electromagnetic radiation

Answer 2

carries energy through space; radiant energy; example = visible light

Question 3

Speed of light

Answer 3

3.00 x 10^8 m/s

Question 4

Wavelength

Answer 4

distance between two adjacent peaks (or two adjacent troughs)

Question 5

Frequency

Answer 5

number of complete wavelengths (or cycles) that pass a given point each second

Question 6

Amplitude

Answer 6

relates to the intensity of the radiation, which is the maximum extent of the oscillation of the wave

Question 7

Electromagnetic spectrum

Answer 7

various types of electromagnetic radiation arranged in order of increasing wavelength

Question 8

Hertz

Answer 8

cycles per second (Hz)

Question 9

Blackbody radiation

Answer 9

the emission of light from hot objects

Question 10

Photoelectric effect

Answer 10

the emission of electrons from metal surfaces on which light shines; explained by Albert Einstein using Planck’s Quantum Theory

Question 11

Emission spectra

Answer 11

the emission of light from electronically excited gas atoms

Question 12

Quantum

Answer 12

“fixed amount”; smallest quantity of energy that can be emitted or absorbed as electromagnetic radiation; named by Max Planck; Energy (E) = h (Planck’s Constant) times nu (v)

Question 13

Planck’s Constant

Answer 13

6.626 x 10^-34 joule-second (j-s)

Question 14

Photon

Answer 14

“energy packet” that behaves like a tiny particle; part of the photoelectric effect; Einstein deduced that each photon must have an energy to Planck’s constant times the frequency of light (E = hv)

Question 15

Work function

Answer 15

certain amount of energy required for an electron to overcome the attractive forces that hold it in the metal

Question 16

Photochemical reactions

Answer 16

radiation breaks chemical bonds

Question 17

Monochromatic

Answer 17

radiation composed of a single wavelength

Question 18

Spectrum

Answer 18

produced from radiation is separated into its different wavelength components

Question 19

Continuous spectrum

Answer 19

rainbow of colors, containing light of all wavelengths

Question 20

Line spectrum

Answer 20

a spectrum containing radiation of only specific wavelengths

Question 21

Rydberg equation

Answer 21

allowed the calculation of the wavelengths of all the spectral lines of hydrogen

Question 22

Ground state

Answer 22

lowest energy state (n=1) of an atom

Question 23

Excited state

Answer 23

electron in a higher, less negative orbit

Question 24

Momentum

Answer 24

product of the mass and velocity of an object

Question 25

Matter waves

Answer 25

wave characteristics of material particles; coined by De Broglie

Question 26

Uncertainty Principle

Answer 26

by Heisenberg; dual nature of matter places a fundamental limitation on how precisely we can know both the location and the momentum of any object; limitation becomes important only when we deal with matter at the subatomic level (with masses as small as that of an electron)

Question 27

Wave functions

Answer 27

series of mathematical functions that describe the electron in an atom

Question 28

Probability density (electron density)

Answer 28

Psi squared; = square of the wave function; represents the probability that the electron will be found at a particular location

Question 29

Orbitals

Answer 29

Set of wave functions and corresponding energies

Question 30

Electron shell

Answer 30

collection of orbitals with the same value of n

Question 31

Subshell

Answer 31

set of orbitals with the same n and l values

Question 32

Radial probability function

Answer 32

probability that the electron will be found a certain distance from the nucleus

Question 33

Node

Answer 33

intermediate point at which a probability function goes to zero

Question 34

Degenerate

Answer 34

Orbitals with the same energy

Question 35

Electron spin

Answer 35

intrinsic property of electrons that causes each electron to behave as if it were a tiny sphere spinning on its own axis

Question 36

Spin Magnetic Quantum Number

Answer 36

quantum number associated with the electron spin; may have values of + 1/2 or -1/2

Question 37

Pauli Exclusion Principle

Answer 37

No two electrons in an atom can have the same set of four quantum numbers (n, l, ml, & ms)

Question 38

Electron configuration

Answer 38

the way in which electrons are distributed among the various orbitals of an atom

Question 39

Hund’s Rule

Answer 39

for degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximized

Question 40

Core electrons

Answer 40

inner shell electrons

Question 41

Outer-shell electrons

Answer 41

electrons given the after the noble-gas core

Question 42

Valence electrons

Answer 42

electrons involved in chemical bonding

Question 43

Transition elements (transition metals)

Answer 43

4th row of the periodic table; 10 elements wider than two previous rows

Question 44

Lanthanide elements (rare earth elements)

Answer 44

14 elements corresponding to the filling of the 4f orbitals

Question 45

Actinide elements

Answer 45

final row of the periodic table; begins by filling the 7s orbitals; most are radioactive, not found in nature

Question 46

Representative elements (main-group elements)

Answer 46

s block and p block of the periodic table together

Question 47

F-block metals

Answer 47

below the main portion of the periodic table, two tan rows with 14 columns; valance f orbitals are being filled