Chem 103 Exam 3

Front 1

The distance between any two adjacent identical points of a wave

Back 1

Wavelength

Front 2

The Greek letter used to express wavelength

Back 2

lambda

Front 3

The Greek letter used to express frequency

Back 3

nu

Front 4

The speed of light is what

Back 4

3.00 X 10e8 m/s

A constant (c)

Front 5

What is the formula relating frequency and wavelength

Back 5

c = νλ

Front 6

How would you rearange the formula for the speed of light to calculate the frequency

Back 6

ν = c
--
λ

Front 7

The range of frequencies (ν) or wavelengths (λ) of electromagnetic radiation

Back 7

Electromagnetic Spectrum

Front 8

The visible spectrum is between ___nm and ___nm

Back 8

350 and 800

Front 9

The ejection of electrons from the surface of a metal or from another material when light shines on it

Back 9

Photoelectric effect

Front 10

A physical constant relating energy and frequency

Back 10

Planck's Constant

6.63 X 10 e-34 J X S

Front 11

A spectrum showing only certain colors or specific wavelengths of light

Back 11

Line Spectrum

Front 12

A spectrum containing light of all wavelengths

Back 12

Continuous Spectrum

Front 13

The branch of physics that mathematically describes the wave properties of submicroscopic particles

Back 13

Quantum or wave mechanics

Front 14

An electron in an atom is described by four different quantum numbers. What are they

Back 14

n, l, mℓ, and ms

Front 15

This quantum number can have any positive value (except 0)and is the one which the energy of an electron in an atom principally depends upon

Back 15

Principal Quantum Number (n)

Front 16

This quantum number can have an integer value of (n - 1) and distinguishes orbitals of a given (n) having different shapes

Back 16

Angular Momentum Quantum Number (l)

Front 17

This quantum number allows values from -l to +l for l = 0 and distinguishes orbitals of given n adn l

Back 17

Magnetic Quantum Number (mℓ)

Front 18

This quantum number has possible values of +1/2 or -1/2 and referes to the 2 possible orientations of the spin axis of an electron

Back 18

Spin Quantum Number (ms)

Front 19

A particular distribution of electrons among available subshells

Back 19

Electron Configuration

Front 20

A diagram to show how the orbitals of a subshell are occupied by electrons

Back 20

Orbital Diagram

Front 21

The observation that no two electrons in an atom can have the same four quantum numbers

Back 21

Pauli exclusion principle

Front 22

An atom can hold at most ___ electrons and then only if the electrons have _______ _____

Back 22

Two, opposite spins

Front 23

The configuration associated with the lowest energy level of the atom

Back 23

Ground State

Front 24

An electron in an atom outside the noble-gas or pseudo-noble-gas core is called...

Back 24

Valence Electron

Front 25

The lowest-energy arrangement of electrons in a subshell is obtained by putting electrons into seperate orbitals of the subshell with the same spin before pairing

Back 25

Hund's Rule

Front 26

A substance that is weakly attracted by a magnetic field, and this attractin is generally the result of unpaired electrons

Back 26

Paramagnetic Substance

Front 27

A substance that is not attracted by a magnetic field or is very slightly repelled by such a field. This property generally means that the substance has only paired electrons

Back 27

Diamagnetic Substance

Front 28

When the elements are arranged by atomic number, their physical and chemical properties vary periodically

Back 28

Periodic Law

Front 29

This tends to decrease with atomic number and increase with period number

Back 29

Atomic Radius

Front 30

The minimum energy needed to remove the highest-energy electron from neutral atom in a gaseous state

Back 30

First Ionization Energy

Front 31

Maximum number of Electrons in the (s) subshell

Back 31

2

Front 32

Maximum number of Electrons in the (p) subshell

Back 32

6

Front 33

Maximum number of Electrons in the (d) subshell

Back 33

10

Front 34

Maximum number of Electrons in the (d) subshell

Back 34

10

Front 35

Maximum number of Electrons in the (f) subshell

Back 35

14

Front 36

Number of orbitals in the (s) subshell

Back 36

1

Front 37

Number of orbitals in the (p) subshell

Back 37

3

Front 38

Number of orbitals in the (d) subshell

Back 38

5

Front 39

Number of orbitals in the (f) subshell

Back 39

7

Front 40

A scheme used to reproduce the electron configurations of the ground states of atoms by successively filling subshells with electrons in specific order

Back 40

Building up principle or (Aufbau Principle)

Front 41

The inner-shell configuration corresponding to one of the noble gases

Back 41

noble-gas core

Front 42

The noble-gas core together with (n - 1)d10th electrons

Back 42

pseudo-noble-gas core

Front 43

An electron in an atom outside the noble-gas or pseudo-noble-gas core

Back 43

valence electron

Front 44

This increases with period number and decreases with atomic number

Back 44

atomic radius

Front 45

This decreases with period number and increases with atomic number

Back 45

Ionization energy

Front 46

The energy change for the process of adding an electron to a neutral atom in a gaseous state to form an negative ion

Back 46

electron affinity

Front 47

An oxide that reacts with acids

Back 47

Basic oxide

Front 48

An oxide that reacts with bases

Back 48

Acidic oxide

Front 49

An oxide that reacts with both basic and acidic properties

Back 49

Amphoteric oxide

Front 50

A chemical bond formed by the electrostatic attraction between positive and negative ions

Back 50

ionic bond

Front 51

A symbol in which the electrons in the valence shell of an atom or ion are represented by dots placed around the letter symbol of the element

Back 51

Lewis electron-dot symbol

Front 52

The change in energy that occurs when an ionic solid is separated into isolated ions in the gas phase

Back 52

lattice energy

Front 53

Particles of electromagnetic energy, with 'E' proportional to the observed frequency of light

Back 53

Photon

Front 54

Albert Einstein postulated that light had both wave and particle properties. He based this postulate off of what?

Back 54

Photoelectric effect

Front 55

The _____ of a wave is the number of wavelengths of that wave that pass a fixed point in one unit of time (usually a second)

Back 55

Frequency

Front 56

E = hv is calcluating what?

Back 56

The energy of a photon

Front 57

When a photon hits metal, its energy (hv) is taken up by the electron. The photon ceases to exist as a particle; it is said to be _____

Back 57

absorbed

Front 58

An electron in an atom can change energy only by going from one energy level to another. What is this called?

Back 58

Transition