Unit 3 Chemisty Test---Vocab

Front 1

Law of Multiple Proportions

Back 1

-if two or more different compounds are composed of the same two elements, the masses of the second element combined with the first element can be expressed as ratios of small whole numbers

Front 2

Three Parts of Dalton's Atomic Theory that still hold true today

Back 2

1.all matter is composed of small particles called atoms
2.atoms of different elements can combine in simple, whole number ratios to form chemical compounds
3.in chemical reactions, atoms are combined, separated, or rearranged.

Front 3

Two Parts of Dalton's Atomic Theory that don't hold true today

Back 3

1.atoms of the same element are identical in size,mass, and other properties
2.atoms cannot be subdivided,createdm or destroyed.

Front 4

Nucleus

Back 4

the postitively charged,dense, central portion of an atom that contains nearly all of its mass but takes up only an insignificant fraction of its volume.

Front 5

Gold-Foil Experiment

Back 5

gold foil was bombarded with positively charged particles(alpha) and the particles that were shot directly back were repulsed by the nucleus that also has a postive charge.

Front 6

Electrons

Back 6

the negatively charged particles that surround the nucleus

Front 7

Electron Cloud

Back 7

comparitively large in volume, contains negatively charged electrons.

Front 8

Cathode

Back 8

Negatively charged end of a cathode ray

Front 9

Anode

Back 9

postively charged end of a cathode ray

Front 10

Atomic Mass Unit (amu)

Back 10

the mass of a carbon 12 atom
1.6605402 x 10(-24) g

Front 11

Relative Atomic Mass

Back 11

the mass of an atom expressed in amu's

Front 12

Average Atomic Mass

Back 12

the weighted average of the atomic masses of the naturally occuring isotopes of an element.

Front 13

Mass Number

Back 13

total number of protons and neutrons in the nucleus of an isotope.

Front 14

Isotope

Back 14

-atom of the same element with different masses
-different masses because they have different numbers of neutrons

Front 15

Nuclide

Back 15

another name for an isotope

Front 16

Atomic Number

Back 16

the number of protons in the nucleus of an atom of an element

Front 17

Nuclear Fusion

Back 17

a less massive nuclei coming together to form a more stable and more massive nuclei with the release of energy

Front 18

Critical Mass

Back 18

the mass and concentration of nuclei that is sufficient enough to sustain a chain reaction

Front 19

Critical Mass

Back 19

the mass and concentration of nuclei that is sufficient enough to sustain a chain reaction

Front 20

Chain Reaction

Back 20

a reaction where the products are able to produce more reactions in a self-sustaining series.

Front 21

Nuclear Fission

Back 21

splitting of a massive nuclei into a more stable, less massive nuclei with the release of energy

Front 22

Binding Energy

Back 22

energy released when a nucleus is formed or energy is absorbed when breaking in nucleus, can be calculated from the mass defect

Front 23

Backround Radiation

Back 23

low amounts of radiation from natural sources

Front 24

Radiation Measurement Instruments

Back 24

Photgraphic film and Geiger Counters

Front 25

Half-Life

Back 25

the time required for 1/2 of the unstable nuclei to decay

Front 26

Radioactive Decay Series

Back 26

a process continuing through a series of decay reactions until a stable nuclei is reached.

Front 27

Nucleons

Back 27

another term for protons and neutrons

Front 28

Radioactive Decay

Back 28

the natural spontaneous disintegration of a nucleus

Front 29

Natural Radioactivity

Back 29

the spontaneous emission of particles or energy form an atomic nucleus as it disintegrates

Front 30

Orbitals

Back 30

a three dimensional region around the nucleus that indicates the probable location of an electron

Front 31

Quantum Theory

Back 31

describes mathmatically the wave properties of electrons and other small particles

Front 32

Spectroscopy

Back 32

a process where a spectroscope which contains a prism, is used to separate the light given off in a substance into the line spectra.

Front 33

The Balmer Series

Back 33

the visible light series

Front 34

Emission Spectrum

Back 34

a spectrum of lines that represents thet emissions of photons with certain energies

Front 35

Photon

Back 35

term used to describe an individual quantum of light

Front 36

Quantum of Light

Back 36

a finite quantity of energy that can be gained or lost by an electron

Front 37

Quanta

Back 37

energy is specific amounts

Front 38

Photoelectric Effect

Back 38

a phenomena where light at particular frequency shines on certain metals and electrons(Called photoelectrons) are emitted.

Front 39

Electromagnetic Spectrum

Back 39

all electromagnetic radiation arranged according to increasing wavelength

Front 40

Electronmagnetic Radiation

Back 40

a form of energy that exhibits wavelike behavior as it travels through space.

Front 41

Spin Quantum Number

Back 41

indicates two possible states of an electron on an orbital
+1/2 or -1/2

Front 42

Magnetic Quantum Number

Back 42

-indicates the orientation of the orbital around the nucleus.

Front 43

Angular Momentum Quantum Number

Back 43

-indicates the shape of the of an or orbital.
-four possible shapes: s,p,d,f

Front 44

Prinicipal Quantum Number

Back 44

indicates the main energy levels surrounding the nucleus

Front 45

Longhand Notation

Back 45

1s2s2p3s3p4s4p is an example of ____________

Front 46

Shorthand Notation

Back 46

[Ne]3s is an example of _______________

Front 47

Orbital Notation

Back 47

the notation that uses arrows is __________________________

Front 48

Aufbau's Principle

Back 48

electron will occupy the lowest energy orbital that it can recieve.

Front 49

Hund's Rule

Back 49

orbitals of equal energy are each occupied by one electron before any one orbital is occupied by a second electron and all electrons in singley occupied orbitals must have same spin(s,p,d,or f)

Front 50

Electron Configurations

Back 50

the arrangement of electrons in atoms; while each element has its own distinct configuration

Front 51

Halogens

Back 51

-most active non-metals
-most commonly combine with a metal to form salts

Front 52

Transition Metals

Back 52

-includes Lanthanide and Actinide Series
-can lose e- below outermost shell
-tendency to share electrons
-similar properties to varying degrees.

Front 53

Alkaline -Earth Metals

Back 53

-rarely found free
-not as explosive as Alkali
-harder, stronger, and higher melting points than those of Alkalis

Front 54

Alkali Metals

Back 54

-most reactive of all metals
-rarely found in nature as free elements
-stored under oil or kerosene
-soft, silvery-white, shiny

Front 55

Actinide Series

Back 55

all elements are reactive and unstable

Front 56

Lanthanide Series

Back 56

-Rare???
-similar properties to one another

Front 57

Noble Gases

Back 57

-normally unreactive(inert)
-except for He all others have 8 valence electrons

Front 58

Periodic Table

Back 58

an arrangement of the elements in order of their atomic numbers so that the elements with similar properties fall in the same columns.

Front 59

Periodic Law

Back 59

the physical and chemical properties of the elements are periodic functions of their atomic numbers .

Front 60

1860's

Back 60

By the _____ already more than 60 elements known

Front 61

Valence Electrons

Back 61

electrons available to be lost, gained or shared in the formation of chemical compounds

Front 62

Electronegativity

Back 62

a measure of the ability of an atom in a chemical compound to attract electrons

Front 63

Formation of an Anion

Back 63

-increase in the radius
-anions are larger than neutral counterparts
-extra electrons will tend to spread out b/c of greater repulsion

Front 64

Formation of a Cation

Back 64

-decrease in the radius
-cations are smaller than neutral counterparts
-smaller cloud and positive charge pulls them in tighter.

Front 65

Anion

Back 65

negatively charged ion

Front 66

Cation

Back 66

positively charged ion

Front 67

Ionic Radii

Back 67

the radii once an ion is formed

Front 68

Electron Affinity

Back 68

the energy change that occurs when an electron is acquired/gains by a neutral atom

Front 69

First Ionization Energy

Back 69

the energy required to move one electron from an atom

Front 70

Ionization

Back 70

the process that results in the formation of an ion.

Front 71

Ion

Back 71

an atom or group of atoms that has a positive or negative charge

Front 72

Ionization Energy

Back 72

the energy that must be supplied when an electron is removed from an atom

Front 73

Atomic Radii

Back 73

-size of the atom;determined by the electron cloud.
-half the distance btwn. the nucleus of identical atoms joined in a molecule.