Chapter 1–3 Chemistry Key Terms

Vocabulary flashcards containing key terms and their definitions from Chapters 1–3 of the notes.

Chemistry

The study of matter, its composition, properties, and transformations.

Matter

Anything that has mass and takes up volume.

Solid

A state of matter with definite volume and definite shape.

Liquid

A state of matter with definite volume but no definite shape.

Gas

A state of matter with neither definite shape nor definite volume.

Physical property

A characteristic that can be observed or measured without changing the substance's identity.

Common physical properties

Examples include melting point, boiling point, solubility, color, and odor.

Physical change

A change that alters a substance without changing its chemical composition.

Chemical change

A process that transforms one substance into another substance.

Pure substance

A substance composed of a single component with a constant composition.

Mixture

A substance composed of two or more components that retain their identities.

Element

A pure substance that cannot be broken down into simpler substances by a chemical reaction.

Compound

A pure substance formed when two or more elements are chemically bonded.

Mass

A measure of the amount of matter in an object.

Weight

The force that matter feels due to gravity.

Base unit of mass

Gram (g) in the metric system.

Base unit of volume

Liter (L) in the metric system.

Meter

The base unit of length in the metric system (symbol: m).

Gram

The base unit of mass in the metric system (symbol: g).

Liter

The base unit of volume in the metric system (symbol: L).

Second

The base unit of time in the metric system (symbol: s).

Giga

Prefix meaning 10^9; symbol G.

Mega

Prefix meaning 10^6; symbol M.

Kilo

Prefix meaning 10^3; symbol k.

Deci

Prefix meaning 0.1; symbol d.

Centi

Prefix meaning 0.01; symbol c.

Milli

Prefix meaning 0.001; symbol m.

Micro

Prefix meaning 10^-6; symbol μ (listed as uc in notes).

Nano

Prefix meaning 10^-9; symbol n.

Deciliter

Unit of volume; 1 dl = 0.1 L.

Cubic centimeter (cc)

Unit of volume equal to 1 mL; 1 cm^3 = 1 mL.

2.54 cm = 1 in

Conversion factor: 2.54 centimeters equal 1 inch.

1 ft =

12 in.

Inch

English unit of length; 1 in.

1 yd =

3 ft.

1 mile =

5,280 ft.

1 meter =

39.37 in.

1 km =

0.6214 mi.

1 lb =

16 oz.

Ounce

English unit of mass; 1 oz.

1 ton =

2,000 lb.

453.59237 g =

1 lb.

Quart

Unit of volume; 1 qt = 4 cups; 946.3 mL; 1 qt = 32 fl oz; 1 qt = 2 pt.

1 quart =

2 pints.

Cup

Unit of volume used with quarts and pints (4 cups = 1 qt).

Fluid ounce

Unit of volume; 29.57 mL.

Celsius

A temperature scale where 0°C is the freezing point of water.

Fahrenheit

A temperature scale used in the United States; water freezes at 32°F.

Kelvin

The absolute temperature scale; 0 K is absolute zero.

Density

Mass per unit volume; density = mass / volume.

Specific gravity

Density of a substance divided by the density of water.

Element

A pure substance that cannot be broken down into simpler substances by chemical reactions.

Metals

Elements that are good conductors of heat and electricity; typically ductile and malleable.

Nonmetals

Elements that are poor conductors of heat and electricity.

Metalloids

Elements with properties intermediate between metals and nonmetals (e.g., Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium).

Chemical formula

Symbols of elements showing the identity and ratios of atoms in a compound.

Proton

Positively charged subatomic particle located in the nucleus.

Electron

Negatively charged subatomic particle surrounding the nucleus.

Neutron

Neutral subatomic particle in the nucleus.

Nucleus

Dense core containing protons and neutrons.

Electron cloud

Region around the nucleus where electrons move.

Mass number (A)

Total number of protons and neutrons in the nucleus (A = Z + N).

Atomic number (Z)

Number of protons in the nucleus.

Isotope

Variant of an element with the same number of protons but different number of neutrons.

Atomic mass

Weighted average mass of the naturally occurring isotopes of an element (in atomic mass units).

Period

A horizontal row in the periodic table.

Group

A vertical column in the periodic table; elements in a group share properties.

Main Group Elements

Groups on the far left and far right of the periodic table (Groups 1,2,13–18).

Transition Metals

The elements in Groups 3–12 in the middle of the periodic table.

Alkali Metals

Group 1 elements.

Alkaline Earth Metals

Group 2 elements.

Halogens

Group 7 elements.

Noble Gases

Group 8 elements.

Bonding

The joining of two atoms in a stable arrangement.

Ionic bonds

Bonding caused by transfer of electrons; forms cations and anions.

Covalent bonds

Bonding that typically occurs between nonmetals (and also described here as between a metal and a nonmetal in the notes).

Cations

Positively charged ions.

Anions

Negatively charged ions.

Metals form cations

For metals in groups 1A, 2A, and 3A, the group number equals the cation charge.

Nonmetals form anions

For nonmetals in groups 5A, 6A, and 7A, the anion charge equals 8 minus the group number.

Aqueous solution

A solution in which a substance is dissolved in water.

Polyatomic ion

An ion that contains more than one atom.

Carbonate

CO3^2−, a polyatomic anion.

Bicarbonate/hydrogen carbonate

HCO3^−.

Acetate

CH3COO^−.

Cyanide

CN^−.

Nitrate

NO3^−.

Nitrite

NO2^−.

Hydroxide

OH^−.

Phosphate

PO4^3−.

Hydrogen phosphate

HPO4^2−.

Dihydrogen phosphate

H2PO4^−.

Sulfate

SO4^2−.

Hydrogen sulfate (bisulfate)

HSO4^−.

Sulfite

SO3^2−.

Hydrogen sulfite (bisulfite)

HSO3^−.