Chemical Calculations, Gases, Liquids, Solids, and Solutions

These flashcards cover essential vocabulary and concepts related to chemical calculations, states of matter, and solutions, designed for exam preparation.

Formula Mass

The mass of a given formula of a compound, calculated by summing the atomic masses of all atoms in the formula.

Molar Mass

The mass of one mole of a substance, typically measured in grams per mole.

Avogadro’s number

The number of particles (atoms, molecules, etc.) in one mole of a substance, approximately 6.022 x 10^23.

Chemical Formula

A representation of a compound that shows the ratio of atoms of each element present in the compound.

Chemical Equation

A symbolic representation of a chemical reaction showing the reactants and products.

Balanced Chemical Equation

An equation where the number of each type of atom is the same on both sides of the equation.

Theoretical Yield

The maximum amount of product that could be formed from a given amount of reactant in a chemical reaction.

Actual Yield

The amount of product actually produced in a chemical reaction.

Percent Yield

(Actual Yield / Theoretical Yield) x 100, used to measure the efficiency of a reaction.

Kinetic Molecular Theory of Matter

A theory that explains the behavior of gases, stating that particles are in constant motion.

Kinetic Energy

The energy possessed by an object due to its motion.

Potential Energy

The energy possessed by an object due to its position or configuration.

Gas Law

A mathematical relationship between pressure, volume, temperature, and amount of gas.

Boyle’s Law

The gas law stating that at constant temperature, the pressure of a gas is inversely proportional to its volume.

Charles’ Law

The gas law stating that at constant pressure, the volume of a gas is directly proportional to its temperature.

Ideal Gas Law

Principle that describes the behavior of ideal gases, represented by the equation PV=nRT.

Dalton’s Law of Partial Pressures

Law stating that the total pressure of a mixture of gases is equal to the sum of the partial pressures of individual gases.

Boiling Point

The temperature at which a liquid's vapor pressure equals atmospheric pressure.

Vapor Pressure

The pressure exerted by the vapor in equilibrium with its liquid or solid form.

Intramolecular Forces

Forces within molecules that hold atoms together.

Dipole-Dipole Interactions

Attractive forces between polar molecules, due to the positive end of one molecule being attracted to the negative end of another.

Hydrogen Bonds

A type of strong dipole-dipole interaction that occurs when hydrogen is bonded to a highly electronegative atom.

London Forces

Weak intermolecular forces that occur due to temporary dipoles in molecules.

Solvent

The substance in a solution that dissolves the solute, typically present in greater amount.

Solute

The substance that is dissolved in a solution.

Solubility

The ability of a solute to dissolve in a solvent at a given temperature and pressure.

Saturated Solution

A solution that contains the maximum amount of solute that can dissolve at a given temperature.

Supersaturated Solution

A solution that contains more solute than can theoretically dissolve at a given temperature.

Unsaturated Solution

A solution that can still dissolve more solute at a given temperature.

Colligative Properties

Properties of solutions that depend on the number of solute particles but not their identity.

Osmosis

The movement of solvent molecules through a semipermeable membrane from an area of lower solute concentration to an area of higher solute concentration.

Osmotic Pressure

The pressure required to prevent the flow of solvent into a solution by osmosis.

Hypotonic Solution

A solution with a lower concentration of solute compared to another solution.

Hypertonic Solution

A solution with a higher concentration of solute compared to another solution.

Isotonic Solution

A solution with the same concentration of solute as another solution.

Concentration Units

Different ways to express the amount of solute in a solution, including molarity and percent concentration.

Dilution

The process of reducing the concentration of a solute in a solution.

Bubbling

The release of gas from a liquid that occurs when the vapor pressure exceeds atmospheric pressure.

Temperature's Effect on Solubility

As temperature increases, the solubility of solids in liquids usually increases.

Pressure's Effect on Solubility

In gases, increased pressure typically increases solubility in liquids.

Molarity

A concentration unit defined as moles of solute per liter of solution.

Mass-Volume Percent

A concentration expressed as the mass of solute per volume of solution.

Percent by Mass

A concentration unit that expresses the mass of solute as a percentage of the total mass of the solution.

Percent by Volume

A concentration measure defined as the volume of solute divided by the total volume of solution, expressed as a percentage.

Mass Percent Calculation

Calculated by dividing the mass of solute by the total mass of the solution and multiplying by 100.

Boiling-Point Elevation

The raising of a liquid's boiling point due to the presence of a solute.

Freezing-Point Depression

The lowering of a liquid's freezing point due to the addition of a solute.

Ionic Compounds

Compounds formed from the electrostatic attraction between positively and negatively charged ions.

Molecular Compounds

Compounds formed by covalent bonds between atoms.

Endothermic

A process that absorbs heat from the surroundings.

Exothermic

A process that releases heat to the surroundings.

Phase Change

A transition of matter from one state to another, e.g., solid to liquid.

Chemical Stoichiometry

The calculation of reactants and products in chemical reactions based on balanced equations.

Mole Concept

A method to quantify the amount of substance in terms of particles or mass.

Solvent Properties

Characteristics of solvents that influence solubility, such as polarity.

Molecular Polarity

The distribution of electrical charge over the atoms in a molecule affecting solubility.

Chemical Reaction

A process that involves the transformation of one set of chemical substances to another.

Physical States of Matter

The distinct forms that different phases of matter take on: solid, liquid, or gas.

Gas Compression

Reducing the volume of a gas by applying pressure.

Gas Expansion

Increase in volume of a gas when pressure decreases.

Intermolecular Forces

Forces of attraction or repulsion between neighboring particles (atoms, molecules, or ions).