Honors Chemistry Mid-Term Exam Vocabulary

Front 1

Law of Multiple Proportions

Back 1

Whenever two elements from more than one compound. the different masses of one element that combine with the same mass of the other element are in the ration of small whole numbers.

Front 2

Avogadro's Number

Back 2

The number of representative particles contained in one mole of a substance to 6.022 x10^23 atoms.

Front 3

Molar Mass

Back 3

A general expression used to refer to mass of a mole of any substance unless a more scientific term is needed to avoid confusion.

Front 4

Mole

Back 4

The amount of a substance that contains 6.022x10^23 representative particles of that substance.

Front 5

Endothermic

Back 5

Occurring or formed with the absorption of heat.

Front 6

Exothermic

Back 6

Occurring or formed with the liberation of heat.

Front 7

Atomic Mass Unit

Back 7

Unit of mass for expressing masses of atoms or molecules

Front 8

Atomic Structure

Back 8

The way in which atoms are arranged in a molecule

Front 9

Average Atomic Mass

Back 9

An atomic weight of an element from a specified source is the ratio of the average mass per atom of elements to 1/12 of the mass of C.

Front 10

Electrons

Back 10

Subatomic particle that carries a negative electric charge.

Front 11

Lanthanide Series

Back 11

First row of rare-earth elements in the periodic table.

Front 12

Actinide Series

Back 12

Second row of rare earth elements in the periodic table.

Front 13

Heisenberg's Uncertainty Principle

Back 13

The idea that the exact position and momentum of a particle cannot be precisely determined at the same time.

Front 14

Bohr Model of Atom

Back 14

Depicts atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around nucleus.

Front 15

Biochemistry

Back 15

The study of the composition and behavior of substances in living organisms.

Front 16

Mass

Back 16

The amount of matter that an object contains; the SI base unit is the kilogram

Front 17

Matter

Back 17

Anything that takes up space.

Front 18

Atom

Back 18

The smallest componenent of an element having the chemical properties of the element.

Front 19

Phase

Back 19

Any part of a system with uniform composition and properties.

Front 20

Weight

Back 20

Force that measures the pull of gravity on a given mass.

Front 21

Aufbau Principle

Back 21

Electrons enter orbitals of lowest energy first.

Front 22

Hund's Rule

Back 22

When electrons occupy orbitals of equal energy, one electron enters each orbital until all orbitals contain one electron with their spins parallel.

Front 23

Alkali Metals

Back 23

Any metals in group 1A of the periodic table. Have one electron in the outermost energy level. Tend to form ionic bonds with halogens. Extremely reactive, silver, and softy metals. Not found as elements in nature.

Front 24

Alkaline Earth Metals

Back 24

Group 2A: Have 2 electrons in the outermost energy level. Harder, denser, and stronger than the alkali metals. Extremely reactive. Are not found as elements in nature.

Front 25

Nucleus

Back 25

Dense central portion of atom, composed of protons and neutrons

Front 26

Halogen

Back 26

Group 7A: Most reactive of all the non-metals. React vigorously to form salts. Have 7 electrons in the outermost energy level. Non-conductors of electricity.

Front 27

Atomic Mass

Back 27

The weighted average of the masses of the isotopes of an element.

Front 28

Atomic Number

Back 28

Number of protons and neutrons in the nucleus of an atom

Front 29

Mass Number

Back 29

Total number of protons and neutrons in nucleus of an atom.

Front 30

Isotopes

Back 30

Atoms of the same element that have the same atomic number but different atomic masses due to a different number of neutrons.

Front 31

Transition Metals

Back 31

Gradual filling of the d-orbital, which includes groups 3-12. Good conductors of electricity and have a high luster. Less reactive than groups 1A and 2A

Front 32

Law of Definite Proportions

Back 32

In any sample of a chemical compound, the different elements are always combined in the same proportion by mass.

Front 33

Pauli Exclusion Principle

Back 33

No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers.

Front 34

Precipitate

Back 34

Formation of a solid in a solution during a chemical reaction.

Front 35

Solution

Back 35

A homogeneous mixture of two or more substances

Front 36

Neutrons

Back 36

Subatomic particle with no net electric charge and a mass slightly larger than that of a proton.

Front 37

Analytical Chemistry

Back 37

Science of chemical characterization and measurement

Front 38

Proton

Back 38

Subatomic particle with positive charge equal to negative charge of electron.

Front 39

Fluoride

Back 39

F
-1

Front 40

Potassium

Back 40

K
+1

Front 41

Chlorate

Back 41

ClO(3)
-1

( ) = subscript

Front 42

Calcium

Back 42

Ca
+2

Front 43

Carbonate

Back 43

CO(3)
-2

( ) = subscript

Front 44

Hydroxide

Back 44

OH
-1

Front 45

Lithium

Back 45

Li
+1

Front 46

Oxide

Back 46

O
-2

Front 47

Barium

Back 47

Ba
+2

Front 48

Aluminum

Back 48

Al
+3

Front 49

Thiosulfate

Back 49

S(2)O(3)
-2

( ) = subscript

Front 50

Sulfate

Back 50

SO(4)
-2

( ) = subscript

Front 51

Spatula

Back 51

To transfer solid chemicals in weighing.

Front 52

Pneumatic Trough

Back 52

To hold water, gas collecting bottles, and delivery tube from gas generator.

Front 53

Double Buret Clamp

Back 53

To hold burets when titrating

Front 54

Tongs

Back 54

To pick up and hold apparatus

Front 55

Test Tube

Back 55

Many Uses

Can be heated

Front 56

Erlenmeyer Flask

Back 56

May be heated.

Front 57

Florence Flask

Back 57

Used for heating substances in Organic Chemistry

Front 58

Buret Clamp / Test Tube Clamp

Back 58

To hold apparatus

May be fastened to the ring stand

Front 59

Triangular File

Back 59

To scratch glass

To file

Front 60

Mortar and Pestle

Back 60

To grind chemicals to a powder

Front 61

Ring Stand

Back 61

A support with many uses.

Front 62

Stirring Rod

Back 62

To stir combinations of materials

To use in pouring liquids

Front 63

Gas Measuring Tube

Back 63

Used to collect and measure the volumes of gases

Front 64

10cm Ruler

Back 64

To measure length

Front 65

Test Tube Holder

Back 65

To hold a test tube

Front 66

Graduated Cylinder

Back 66

To measure volume

Front 67

Microtitration Plate

Back 67

Used t hold liquids in micro experiments

Front 68

Crucible and Cover

Back 68

To heat small amounts of solid material at high temperature

Front 69

Plastic Wash Bottle

Back 69

To dispense distilled water

Front 70

Pinch Clamp

Back 70

To clamp a rubber connector

Front 71

Test Tube Brush

Back 71

To scrub glass apparatus

Front 72

Evaporating Dish

Back 72

Used as a container for small amounts of liquid being evaporated.

Front 73

Wire Gauze

Back 73

To spread the heat of a flame

Front 74

Watch Glass

Back 74

May be used as a beaker cover

May be used in evaporating very small amounts of liquid

Front 75

Beaker

Back 75

As a container, like a cup

May be heated

Front 76

Laboratory (Bunsen) Burner

Back 76

To heat chemicals in beakers or test tubes

Front 77

Iron Ring

Back 77

To fasten to the ring stand as a support for apparatus

Front 78

Test Tube Rack

Back 78

To hold test tubes in an upright position

Front 79

Rubber Connector

Back 79

To connect parts of apparatus

Front 80

Volumetric Flask

Back 80

Used in the preparation of solutions

Front 81

Buret

Back 81

Used to withdraw and measure volumes of solutions in titrations

Front 82

Funnel

Back 82

To hold a filter paper

May be used in pouring

Front 83

Medicine Dropper

Back 83

To transfer small amounts of liquid

Front 84

Forceps

Back 84

To pick up or hold small objects

Front 85

Funnel Support

Back 85

To support funnels

Front 86

Thin Stem Pipette

Back 86

Used in micro experiment to transfer small amounts of liquid