Honors Chemistry Final Exam - Vocabulary

Flashcards covering key vocab for Honors Chemistry Final Exam

Stoichiometry

A section of chemistry using relationships between reactants and/or products in a reaction to determine desired quantitative data.

HNRUE Table

A tabular method used in stoichiometry to organize and calculate moles, mass, and volume of reactants and products in a chemical reaction.

Mole Ratio

The ratio of moles of one substance to the moles of another substance in a balanced chemical equation.

Limiting Reactant

The substance in a chemical reaction that is completely consumed first, limiting the amount of product that can be formed.

Excess Reactant

The substance in a chemical reaction that is not completely consumed and remains after the reaction is complete.

Theoretical Yield

The maximum amount of product that can be generated from a given amount of reactants, based on the balanced chemical equation.

Actual Yield

The amount of product actually produced in a chemical reaction.

Percent Yield

The ratio of the actual yield to the theoretical yield, expressed as a percentage. It indicates the efficiency of a reaction.

Kinetic Molecular Theory of Gasses

A theory that explains the behavior of gases in terms of particles in constant motion, emphasizing that gas pressure arises from collisions of these particles with the walls of their container.

Ideal Gas

A hypothetical gas that follows the gas laws at all conditions of temperature and pressure, exhibiting no attractions or repulsions between particles.

1st Postulate of KMT

Gas particles are traveling in straight lines and are in constant motion until they collide with each other or the walls of their container.

2nd Postulate of KMT

Gasses are just empty space since the space they occupy causes the volume to be relatively zero.

3rd Postulate of KMT

Pressure is exerted on the sides of the container when particles make contact.

4th Postulate of KMT

Average kinetic energy of gas particles is proportional to temperature of gas in Kelvin.

5th Postulate of KMT

Gas particles don’t interact w/ each other since they are so small, and presence of Intermolecular Forces are non-existent

Elastic

Ability of something to return to its natural state after deformation or stretching

Absolute Zero

0 Kelvin being no kinetic energy.

Boyle’s Law (Robert Boyle)

Temperature of a given mass of a confined gas is constant, product of pressure & volume is constant. (Inversely proportional)

Charles’ Law (Jacques Charles)

Temperature of a given mass of a confined gas is constant, gasses expand resulting in larger volume. (Directly proportional)

Gay-Lussac’s Law (Joseph Gay-Lussac)

Temperature of a given mass of a confined gas is constant, gasses with have more kinetic energy resulting in more collisions on the container or higher pressure. (Directly proportional)

Standard Temperature and Pressure (STP)

Set of nominal conditions used to predict properties of gasses, its density, etc.

Combined Gas Law

Relates how three properties of a gas: Pressure, Volume, and Temperature, relate to and change with each other

Density

Law when a gas is compressed into a smaller volume, the number and velocity of molecular collisions increase, raising the gas's temperature and pressure

Solution

Any substance classified as a homogeneous mixture of 2 or more substances in a single phase.

Solute

A substance that is being dissolved

Solvent

A substance doing the dissolving

Homogeneous mixtures

A type of mixture where components are evenly distributed and uniform throughout.

Heterogeneous mixtures

A combination of two or more substances where the components are not uniformly distributed and can be visually distinguished

Aqueous

Solution made from water as the solvent

“Universal Solvent”

Water, as it is the most commonly used solvent in Chemistry

Suspension

A type of mixture resulting in a separation of particles

Colloid

Type of mixture not classified as true homogeneous/heterogeneous, but somewhere in between due to particle size being involved

Dispersion Medium

Contains the dispersed substance (if gas: Aerosol)

Dispersed Substance

Thing that spreads throughout dispersion medium (if gas: foam)

Tyndall Effect

A phenomenon in which light is scattered by collided part that are dispersed in a transparent medium

Dissolution

Process in which a solute will dissolve in a solvent to create a solution

Solubility

Maximum amount of solute that can dissolve in a solvent at a particular temperature

Saturated Solution

Solution containing max dissolved solutes

Unsaturated Solution

Solution containing less dissolved solutes than a saturated solution

Supersaturated solution

Solution containing more dissolved solutes than a saturated solution

Miscibility

Property of 2 substances able to mix in all proportions forming homogeneous mixtures

Immiscibility

Property of 2 substances unable to mix in all proportions; not forming homogeneous mixtures

Concentration

Referring to amount of substance within a defined area

Molarity

of moles of solute per liter of the solution

Stock Solution

Solution created in order to conserve materials, save preparation time, and reduce storage space

Diluted Solution

Solutions that are altered w/ a change in amount of solvent

Net Ionic Equation

A chemical equation focusing on compounds and ions undergoing a chemical change in a reaction in an aqueous solution.

Spectator Ions

Ions that are present during a chemical reaction but do not participate in the actual chemical change

Reaction Kinetics

Branch of chemistry w/ understanding of how quickly a reaction occurs.

Reaction Mechanisms

Step by step sequence of reactions by which overall chemical change occurs

Intermediate

Chemical species appearing within a step of a mechanism but not in the net equation

Collision Theory

An idea suggesting in order for a chemical reaction to occur, reactant particles must collide w/ enough energy and proper orientation

Activation Energy

Minimum amount of energy needed to transform reactants into an activated complex

Activation Complex

Transitional states existing momentarily where reactant bonds are broken and reformed to make products

Reaction Rate

Change in reactant concentration per unit time as a reaction proceeds or the speed at which a reaction takes place.

Chemical Kinetics

Area of chemistry concerned w/ reaction rates & mechanisms

Reversible Reaction

Reaction which products can react to reform reactants

Chemical Equilibrium

When rate of forward reaction is equal to rate of the reverse reaction and concentration of reactants & products are constant

Equilibrium Constant

Ratio of mathematical product of the concentrations of substances formed at equilibrium to math product of the concentration of reacting substance formed at equilibrium

Le Chateliers Principle

Idea starting if a system at equilibrium is subjected to a stress, equilibrium is shifted in direction that tends to relieve the stress

Acid

Chemical species having the ability to offer protons and neutralize bases

Base

Chemical species having the ability to accept protons and neutralize acids

Arrhenius Acids

Chemical compound that increase the concentration of Hydrogen ions.

Arrhenius Bases

Chemical compound that increases concentration of Hydroxide ions

Bronsted-Lowry (B/L) Acids

Molecule/ion considered a proton donor

B/L Bases

Molecule/ion considered a proton acceptor

Neutralization

Process in which an acid and a base react together to make salt & water.

Thermochemistry

Study of energy transfer as heat accompanying chemical reactions and physical changes

Heat

Transfer of energy between matter due to temperature differences

Temperature

Measure of average Kinetic Energy of the particles

Entropy

Natural tendency for heat to spread out

Conduction

Heat or electricity is directly transmitted through a substance when there is a difference in temperature or electrical potential between adjoining regions, without movement of the material

Convection

Transfer of heat through a fluid by means of upward movement due to density differences.

Radiation

Energy is emitted as particles or waves