M1.1 General Chemistry

Anything that occupies space and has mass

Matter

The science that deals with the study of properties, composition and changes that matter undergo

Chemistry

Properties of matter that are independent of the amount of substance present

Intrinsic Properties

Properties of matter that are dependent on the amount of substance present

Extrinsic Properties

The state of matter characterized by a definite volume, definite shape, strong intermolecular forces, and vibrational molecular motion

Solids

The state of matter characterized by a definite volume, indefinite shape, intermediate intermolecular forces, and gliding molecular motion

Liquid

The state of matter characterized by an indefinite volume, indefinite shape, weak intermolecular forces, and constant random molecular motion

Gas

A state of matter consisting of an ionized gas

Plasma

States of matter with intermediate properties between solids and liquids

Liquid Crystals

Pure substances represented by symbols, consisting of 118 known types

Elements

The chemical name for element 110

Darmstadtium

The chemical name for element 111

Roentgenium

The chemical name for element 112

Copernicium

The chemical name for element 114

Flerovium

The chemical name for element 116

Livermorium

Pure substances formed when elements combine in a fixed ratio of whole numbers

Compounds

The law stating that elements combine in a fixed ratio of whole numbers to form compounds

Law of Definite Proportions

The law stating that elements can combine in different ratios of whole numbers to form different compounds

Law of Multiple Proportions

Any part of a system with a uniform set of physical and chemical properties

Phase

A mixture composed of two or more distinct phases, such as oil and water

Heterogenous Mixture

A mixture containing only one phase where a solute is distributed throughout a solvent system

Solutions

A mixture of insoluble substances dispersed in a medium

Colloids

The zigzag movement of colloidal particles due to perfectly elastic collision

Brownian Movement

The scattering of light by particles in a colloid or suspension

Tyndall Effect

A mixture of insoluble substances suspended in a medium using a suspending agent

Suspension

The phase transition from solid directly to gas, with examples like dry ice, mothballs, and iodine crystals

Sublimation

The phase transition from gas directly to solid, such as heavy metal deposition

Deposition

A chemical change involving the formation of complex substances from simpler substances

Direct union

A chemical change involving the breakdown of a complex substance into simpler substances

Decomposition

A chemical reaction based on the activity series where a more active metal displaces a less active metal

Single Replacement

A chemical reaction in which two compounds exchange partners, also known as metathesis

Double Displacement

The chemical model stating that matter is composed of tiny invisible particles called "Atomos"

Democritus Model

The atomic model that depicts the atom as a hard, indestructible sphere

Billiard Ball Model

The atomic model that depicts the atom as a sphere of positive particles embedded with negative particles

Raisin Bread Model

The atomic model stating that an atom consists largely of empty space with a concentrated positive nucleus

Nuclear Model

The atomic model stating that electrons move around the nucleus in circular orbits or energy states

Planetary Model

The atomic model stating that electrons reside in a three-dimensional space called an electron cloud

Quantum mechanical model

The subatomic particle discovered by Thompson using the Cathode Ray Tube experiment

Electrons

The subatomic particle discovered by Goldstein

Protons

The subatomic particle discovered by Chadwick

Neutrons

Atoms of the same element with the same number of protons but different numbers of neutrons

Isotopes

Atoms with the same mass number but different atomic numbers

Isobars

Atoms with the same number of neutrons but different numbers of protons

Isotones

The quantum number used to determine the overall energy and size of the electron cloud

Principal Quantum Number

The quantum number that determines the angular momentum and the shape of the orbital

Azimuthal Quantum Number

The orbital designated by the azimuthal quantum number 0, meaning "Sharp" and having a spherical shape

S orbital

The orbital designated by the azimuthal quantum number 1, meaning "Principal" and having a dumbbell shape

P orbital

The orbital designated by the azimuthal quantum number 2, meaning "Diffused" and having a clover leaf shape

D orbital

The orbital designated by the azimuthal quantum number 3, meaning "Fundamental" and having a complex shape

F orbital

The rule stating that orbitals are filled singly before pairing up

Hund's Rule

The quantum number that determines the orientation of an orbital in space

Magnetic Quantum Number

The quantum number that determines the direction of rotation of electrons

Electron Spin Quantum Number

The principle stating that no two electrons in an atom can have the same set of four quantum numbers

Pauli's Exclusion Principle

The principle stating that the buildup of electrons in an atom results from continually increasing the quantum number

Aufbau's Building Up Principle

The scientist who made an extensive list of 33 elements and distinguished between metals and non-metals

Antoine L. Lavoisier

The scientist who developed a table of atomic weights and introduced letters to symbolize elements

Jons Jakob Berzelius

The scientist who proposed the concept of "Triads" as a forerunner to groups of elements

Johann Dobereiner

The scientist who proposed the Law of Octaves

John Newlands

The scientists who formulated the first periodic law stating that properties vary according to atomic weights

Meyer and Mendeleev

The scientist who modified the periodic law to state that properties of elements vary periodically with their atomic number

Henry Moseley

Columns of elements related to the number of valence electrons

Groups

Horizontal rows of elements related to the highest value of the principal quantum number

Periods

The periodic trend defined as one half the distance between two nuclei in two adjacent atoms

Atomic Radius

The energy required to remove an electron from a neutral atom to convert it to a positively charged ion

Ionization Energy

The amount of energy released when a neutral atom accepts an electron on its outermost shell

Electron Affinity

The tendency of an atom to attract electrons to itself when it is combined with another atom

Electronegativity

Chemical bonds formed by the electrostatic attraction between a metal and a non-metal resulting from electron transfer

Ionic Bonds

A covalent bond formed by a head-on overlap between atomic orbitals along the internuclear axis

Sigma bond

A covalent bond formed by a lateral or sideways overlap between atomic orbitals perpendicular to the internuclear axis

Pi bond

A covalent bond with equal sharing of electrons and no net dipole moment, formed by atoms with similar electronegativity

Non-polar Covalent bond

A covalent bond with unequal sharing of electrons and a net dipole moment, formed by atoms with comparable electronegativity

Polar Covalent Bond

A solution that contains the maximum amount of solute that will dissolve in a given solvent at a specific temperature

Saturated solution

A solution that contains less solute than its capacity to dissolve

Unsaturated solution

A solution that contains more solute than is present in a saturated solution

Supersaturated solution

The principle stating that substances with similar intramolecular forces of attraction interact and dissolve better

Like dissolves like

An acid definition stating that it yields hydrogen ions (H+) in water

Arrhenius Acid

A base definition stating that it is a proton (H+) acceptor

Bronsted-Lowry Base

An acid definition stating that it is an electron pair acceptor

Lewis Acid

Compounds that can both accept and donate protons, such as amino acids

Amphiprotic Compounds

Compounds that can act as either an acid or a base, such as water or tin hydroxide

Amphoteric Compounds

The velocity or rate with which a chemical reaction occurs

Rate of Reaction

The kinetic theory stating that the reaction rate is proportional to the number of effective collisions per time

Collision Theory

The minimum energy required for reactants to undergo an effective collision and react

Activation Energy

The kinetic theory stating that the reaction rate is proportional to the energy required to form a transition state intermediate

Transition State Theory

A reaction order where the rate of reaction is independent of the concentration of the reactants

Zero Order

The time required for the concentration of a drug to decrease by one half

Half Life