Physical Science C Final Review

Comprehensive vocabulary and key concepts for the Physical Science C final exam, covering chemistry fundamentals including atoms, bonding, reactions, and solutions.

Malleable

A property of matter that means it is easily shaped or bent.

Polar covalent bond

The type of bond formed when electrons are shared unequally, such as when Sulfur and Oxygen react.

Nonmetals

Elements characterized by a lack of luster and no conductivity.

Carbon

The element that is present in all organic compounds.

Boron Neutrons

A boron atom with a mass number of $11$ and an atomic number of $5$ has $6$ neutrons.

Uranium-238 Protons

An atom of Uranium-238 has $92$ protons.

Uranium-238 Neutrons

An atom of Uranium-238 has $146$ neutrons.

Mass of $NaCl$

A unit of sodium chloride has a mass of $58.5$ atomic mass units ($35.5 + 23.0$).

Solution

Another name for a homogeneous mixture.

Chemical property

A characteristic of matter that allows it to change into something new.

Mixture

The result of combining two or more substances so that each substance can be separated by physical means.

Proton

The part of the atom that carries a positive charge.

Electron

The part of the atom that carries a negative charge.

Element Symbols

Abbreviations for elements such as $Hg$ (Mercury), $Pb$ (Lead), and $Na$ (Sodium).

Dot diagrams

Representations of the outer valence Electrons of an atom.

Cation

A positively charged ion.

Anion

A negatively charged ion.

Covalent bond

A bond formed when electrons are shared between atoms.

Carbon dioxide ($CO_2$)

An example of a correctly written covalent formula.

Lead (IV) nitrate formula

$$Pb(NO_3)_4$$

Lithium Oxide formula

$$Li_2O$$

Calcium Hydroxide formula

$$Ca(OH)_2$$

Double bond

The sharing of four electrons between atoms.

Noble Gases

The group name for Group 18 elements which have stable outer energy levels.

Molecules

The name given to units that make up covalently bonded compounds.

Subscripts

The numbers in a chemical formula that show the exact number of atoms of each element.

Chemical formula

An equation that shows the exact number (#) and types of atoms in a substance.

Oxidation number

The number that shows how many electrons need to be lost, gained, or shared for an atom to become stable.

Reactants

The substances located to the left of the arrow in a chemical equation.

Products

The substances located to the right of the arrow in a chemical equation.

Law of Conservation of Mass

A law stating that matter cannot be created or destroyed in a closed system.

Solute

The substance in a solution that is being dissolved.

Saturated Solution

A solution that contains all the solute it can hold at a given temperature.

Supersaturated solution

A very unstable type of solution.

Synthesis

A type of chemical reaction exemplified by the formation of $H_2O$.

Decomposition

A type of chemical reaction exemplified by the use of baking soda in cooking.

Acids

Substances that produce hydrogen ions in a water solution, taste sour, and are corrosive.

Bases

Substances that produce hydroxide ions in a water solution, taste bitter, and feel slippery.

Indicators

Substances that show pH levels by changing color in the presence of Acids or Bases.

Neutral

A solution that contains equal concentrations of hydrogen and hydroxide ions.

pH scale

The scale used to measure acidic and basic substances.

Buffer

A substance found in blood that allows it to tolerate small amounts of acid and base without damage.