Honors Chemistry Exam Review Flashcards

Vocabulary flashcards for honors chemistry exam review based on lecture notes.

Calorie

The amount of energy needed to raise the temperature of 1 gram of H2O by 1 degree Celsius.

Energy

The capacity to do work or produce heat.

Potential Energy

Stored energy (e.g., water behind a dam).

Kinetic Energy

Energy of motion (e.g., a rolling ball).

Physical Change

A change that does not result in a new chemical substance.

Chemical Change

A change that creates a new substance.

Law of Conservation of Matter

Matter is neither created nor destroyed.

Law of Conservation of Energy

Energy is not created nor destroyed; it can be transformed, though.

Atom

The smallest unit an element can be while still having the same properties of said element.

Isotope

Atoms with the same number of protons but a different number of neutrons.

Ion

An atom or molecule with a net charge from loss or gain of electrons.

Anion

A negatively charged ion (gained electron).

Cation

A positively charged ion.

Single Covalent Bond

A covalent bond using only 2 electrons to bond.

Double Covalent Bond

A covalent bond using 4 electrons to bond.

Triple Covalent Bond

A covalent bond using 6 electrons to bond.

Ionic Bond

The giving and taking of electrons between a metal and a nonmetal.

Covalent Bond

The sharing of electrons between two nonmetals.

Metallic Bond

The sharing of a sea of electrons between two metals.

Polar Covalent Bond

When electrons are shared unequally (e.g., H2O).

Nonpolar Covalent Bond

When electrons are shared equally (e.g., O2).

Formula Mass

The mass of one mole of a compound in amu.

Atomic Mass

The mass of one mole of an element relative to the mass of carbon-12.

Molar Mass

The mass of one mole of an element or one mole of formula units or one mole of molecules.

Empirical Formula

The simplest whole number ratio of elements in a compound.

STP

Standard Temperature and Pressure (273.15 K and 1 atm).

Limiting Reactant

Substance that will be completely used up and will limit the amount of product in a reaction.

Stoichiometry

The quantitative relationships between reactants and products in a balanced equation.

Hess’s Law

The overall enthalpy change in a reaction is equal to the sum of enthalpy changes for the individual steps in the process.

Solute

Substance getting dissolved; the smaller amount.

Solvent

Substance doing the dissolving; the larger amount.

Solution

A homogeneous mixture of 2 or more substances in the same state.

Saturated

When the solvent has the maximum amount of solute that can be dissolved.

Unsaturated

When the solvent can still hold additional solute.

Supersaturated

When the substance contains more solute than the solvent can hold.

Charles’ Law

If pressure and number of moles are constant: V1/T1 = V2/T2

Boyles’ Law

If temperature and moles are constant: P1V1 = P2V2

Combined Gas Law

Combination of Boyle's and Charles' Laws, relating pressure, volume, and temperature for a fixed amount of gas.

Ideal Gas Law

PV = nRT; Real gases behave ideally under conditions of high temperature and low pressure.

Dissociation

When solvent particles separate and so do the solute ones; requires energy.

Solvation

When the solvent and the solute interact; energy released.

Miscible

Two liquids that can dissolve in each other.

Immiscible

Two liquids that cannot dissolve in each other.

Dalton’s Law of Partial Pressures

In a mixture of gases, the total pressure is equal to the sum of the partial pressures of the component gases

Alloy

A mixture of metals (e.g. Pt/Pd/Rh in catalytic converters).

Heat Capacity

The amount of heat required to raise the temperature of a substance by 1 degree Celsius.

Specific Heat

The amount of heat required to raise the temperature by 1 degree Celsius of 1 gram of a substance.

Diffusion

The movement of particles from an area of high concentration to an area of low concentration.

Elastic Collisions

A collision in which kinetic energy is conserved.

Calorimetry

The process of determining the number of calories in a substance.