Keiser University CHM2045 General Chemistry Test 1 and Final Study Guide

A comprehensive set of vocabulary flashcards derived from the CHM2045 General Chemistry lecture notes, covering atomic theory, physical states, energy, and chemical nomenclature.

Molecule

Two or more atoms chemically joined together.

Neutron

The largest subatomic particle.

Electron

The smallest subatomic particle; its charge was discovered by Millikan.

Dalton's Atomic Theory

A theory stating that matter is composed of small indestructible particles.

Scientific theory

A framework based on continued observation and experiment.

Liquid

A state of matter characterized by a definite volume and no definite shape.

Element

A substance that cannot be chemically broken down into simpler substances.

Compound

A substance composed of two or more elements in a fixed, definite proportion.

Distillation

A process in which the more volatile liquid is boiled off to separate it from a mixture.

Thermal energy

Energy associated with the temperature of an object.

Kinetic energy

Energy associated with the motion of an object.

Potential energy

Energy associated with the position or composition of an object.

Solid

The physical state of matter that retains both its shape and its volume.

Vinegar

A mixture composed of approximately $5\%$ acetic acid and $95\%$ water.

Nucleons

The collective term for protons and neutrons, which account for essentially all of the mass of an atom.

Absolute zero

A temperature value equal to $-273^{\circ}\text{C}$.

Law of the Conservation of Mass

The principle stating that in a chemical reaction, matter is neither created nor destroyed.

Law of Definite Proportions

The principle stating that all samples of a given compound have the same proportions of their constituent elements.

Cathode ray tube

The equipment utilized by Thomson to conduct his research.

Mass number

The sum of the number of protons and neutrons in an atom.

Isotopes

Atoms of the same element that differ in the number of neutrons they contain.

Ions

Atoms or molecules that differ in the number of electrons, resulting in a net charge.

Metalloids

Elements that act as semiconductors.

Mass spectrometer

An instrument used to determine the mass of a molecule and the percent abundance of isotopes.

Avogadro's number

The constant value $6.022 \times 10^{23}$.

Anion

An atom that has gained an electron to become negatively charged.

Noble gases

The group of elements in the periodic table that are the most unreactive because they do not combine with other elements to form compounds.

Inorganic compound

The general term for a compound that does not contain the element carbon.

Stock system

A nomenclature system where a Roman numeral indicates the ionic charge, such as iron (II) ion for $Fe^{2+}$.

Latin system

A naming system for ions using suffixes, where ferrous oxide refers to $FeO$ and ferric oxide refers to $Fe_2O_3$.

Phosphate ion

The polyatomic ion with the formula $PO_4^{3-}$.

Ammonium ion

The polyatomic ion with the formula $NH_4^+$.

Tetraphosphorus trisulfide

The flammable compound found on match tips with the chemical formula $P_4S_3$.

Hydrochloric acid

An aqueous solution with the chemical formula $HCl_{(aq)}$.

Nitric acid

An aqueous solution with the chemical formula $HNO_{3(aq)}$.

Sulfuric acid

An aqueous solution with the chemical formula $H_2SO_{4(aq)}$.

Perchloric acid

The systematic name for the aqueous solution $HClO_{4(aq)}$.

Phosphorous acid

The systematic name for the aqueous solution $H_3PO_{3(aq)}$.