Chem Semester Test

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136 Terms

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Mole
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* SI base unit used to measure the amount of a substance. 
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Avogadro’s Number
6\.02x10^23
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molar mass
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*  **mass in grams of one mole of any pure substance.** 
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percent composition
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* percent by mass of each element in the compound.
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empirical formula
smallest whole-number mole ratio of the elements.
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molecular formula
specifies the actual number of atoms of each element in one molecule or formula unit of the substance.
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hydrate

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* a compound that has a specific number of water molecules bound to its atoms.
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stoichiometry
the study of quantitative relationships between the amounts of reactants used and the amounts of products formed by a chemical reaction.
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mole ratio
a ratio between the numbers of moles of any two of the substances in a balanced chemical equation.
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limiting reactant
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* limits the extent of the reaction and thereby determines the amount of product formed.
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excess reactants
Reactants left over when a reaction stops
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theoretical yield
represents the maximum amount of product that can be produced from a given amount of reactant.
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actual yield
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* the amount of product produced when the chemical reaction is carried out in an experiment.
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percent yield
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* **the ratio of the actual yield to the theoretical yield expressed as a percent.**
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kinetic-molecular theory
describes the behavior of matter in terms of particles in motion.
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elastic collision
one in which no kinetic energy is lost.
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temperature
is a measure of the average kinetic energy of the particles in a sample of matter.
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diffusion
is the movement of one material through another.
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Graham’s Law of Effusion
states that the rate of effusion for a gas is inversely proportional to the square root of its molar mass.
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pressure
defined as force per unit area.
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Barometer
instruments used to measure atmospheric air pressure.
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pascal
is equal to a force of one Newton per square meter or N/m2.
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atmosphere
is equal to 760 mm Hg or 101.3 kilopascals.
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dalton’s law of partial pressures
states that the total pressure of a mixture of gases is equal to the sum of the pressures of all the gases of the mixture.
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dispersion forces
weak forces that result from temporary shifts in the density of electrons in electron clouds.
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dipole-dipole forces
are attractions between oppositely charged regions of polar molecules.
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hydrogen bond
are special dipole-dipole attractions that occur between molecules containing a hydrogen atom bonded to a small, highly electronegative atom with at least one lone electron pair.
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viscosity
measure of the resistance of a liquid to flow and is determined by the type of intermolecular forces, size and shape of particles, and temperature.
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surface tension
the energy required to increase the surface area of a liquid by a given amount.
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surfactant
compounds that lower the surface tension of water.
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crystalline solid
a solid with atoms, ions, or molecules arranged in an orderly, geometric structure.
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unit cell
the smallest arrangement of atoms in a crystal lattice that has the same symmetry as the whole crystal.
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allotrope
an element that exists in different forms at the same state—solid, liquid, or gas.
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amorphous solid
one in which the particles are not arranged in a regular, repeating pattern.
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melting point
the temperature at which the forces holding the crystal lattice together are broken, and the crystalline solid becomes a liquid.
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vaporization
the process by which a liquid changes to a gas or vapor.
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evaporation
vaporization that occurs only at the surface of a liquid.
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vapor pressure
**the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases (solid or liquid) at a given temperature** 
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boiling point
The temperature at which the vapor pressure of a liquid equals the external or atmospheric pressure
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freezing point
the temperature at which
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condensation
The process by which a gas or a vapor becomes a liquid
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deposition
the process by which a substance changes from a gas or vapor to a solid without first becoming a liquid.
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phase diagram
a graph of pressure versus temperature that shows in which phase a substance exists under different conditions of temperature and pressure.
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triple point
the point on a phase diagram that represents the temperature and pressure at which all three phases of a substance can coexist.
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boyles law
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* **states that the volume of a fixed amount of gas held at a constant temperature varies inversely with the pressure.**
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absolute zero
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* **zero on the Kelvin scale.**  
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charle’s law
 states that the volume of a given amount of gas is directly proportional to its Kelvin temperature at constant pressure.
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gay lussac’s law
* **states that the pressure of a fixed amount of gas varies directly with the Kelvin temperature when the volume remains constant.** 

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combined gas law
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* states the relationship among pressure, temperature, and volume of a fixed amount of gas.
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avogadro’s principal
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states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles. 
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molar volume
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* the volume 1 mol occupies at 0.00°C and 1.00 atm of pressure.
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standard temperature and pressure (STP)
.00°C and 1.00 atm
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ideal gas law
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* represented by R and is 0.0821 L•atm/mol•K when pressure is in atmospheres.
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ideal gas constant
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* describes the physical behavior of an ideal gas in terms of the pressure, volume, temperature, and number of moles of gas present.
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suspension
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* **mixtures containing particles that settle out if left undisturbed. Suspensions can also be separated by filtering.** 
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colloids
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*  **heterogeneous mixtures of intermediate-sized particles (1 nm-1000 nm) that do not settle out, nor can they be filtered apart.** 
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brownian motion
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* **the jerky, random movements of particles in a liquid colloid, from the results of particle collisions.**
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tyndall effect
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* the scattering of light by dispersed colloid particles. 
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soluble
A substance that dissolves in a solvent
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miscible
Two liquids that are soluble in each other in any proportion
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insoluble
A substance that does not dissolve in a solvent
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inmiscible
Two liquids that can be mixed but separate shortly after
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concentration
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* a solution is a measure of how much solute is dissolved in a specific amount of solvent or solution.
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molarity
* **the number of moles of solute dissolved per liter of solution.**

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molality
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* **the ratio of moles of solute dissolved in 1 kg of solvent.**
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mole fraction
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* **the process of surrounding solute particles with solvent particles to form a solution.**
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solvation
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* **the process of surrounding solute particles with solvent particles to form a solution.**
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heat of solution
The overall energy change that occurs during solution formation
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unsaturated solution
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* **solutions that contain less dissolved solute for a given temperature and pressure than a saturated solution.**
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saturated solution
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*  **contain the maximum amount of dissolved solute for a given amount of solute at a specific temperature and pressure.**
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supersaturated solution
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* contains more dissolved solute than a saturated solution at the same temperature.
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henrys law
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* **states that at a given temperature, the solubility (S) of a gas in a liquid is directly proportional to the pressure (P).**
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colligative property
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* **are physical properties of solutions that are affected by the number of particles but not by the identity of dissolved solute particles.**
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vapor pressure lowering
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* **depends on the number of solute particles in solution. It is a colligative property of solutions.**
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boiling point elevation
The temperature difference between a solution’s boiling point and a pure solvent's boiling point
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freezing point depression
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* , is the difference in temperature between its freezing point and the freezing point of the pure solvent.
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osmosis
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 the diffusion of a solvent through a semipermeable membrane.
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osmotic pressure
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* **the amount of additional pressure caused by water molecules that move into the concentrated solution.**
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energy
the ability to do work or produce heat.
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law of conservation of energy
states that in any chemical reaction or physical process, energy is neither created nor destroyed.
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chemical potential energy
energy stored in a substance because of its composition.
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heat
energy that is in the process of flowing from a warmer object to a cooler object.
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calorie
defined as the amount of energy required to raise the temperature of one gram of pure water by one degree Celsius (1°C).
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joul
the SI unit of heat and energy.
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specific heat
the amount of heat required to raise the temperature of one gram of that substance by one degree Celsius.
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acidic solution
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*  contains more hydrogen ions than hydroxide ions.
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basic solution
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* contains more hydroxide ions than hydrogen ions.
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Arrhenius model
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* An acid is a substance that contains hydrogen and ionizes to produce hydrogen ions in aqueous solution.
* A base is a substance that contains a hydroxide group and dissociates to produce a hydroxide ion in solution.
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Bronsted-lowery model
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* states that an acid is a hydrogen ion donor, and a base is a hydrogen ion acceptor.
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conjugate acid
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*  the species produced when a base accepts a hydrogen ion.
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conjugate base
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* the species produced when an acid donates a hydrogen ion.
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conjugate acid-base pair
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*  consists of two substances related to each other by donating and accepting a single hydrogen ion.
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amphoteric
can react with acids and bases
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lewis model
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* a Lewis acid is an electron-pair acceptor, and a Lewis base is an electron-pair donor.
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strong acid
Acids that ionize completely
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weak acid
Acids that ionize only partially in dilute aqueous solutions
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acid-ionization constant
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*  is the value of the equilibrium constant expression for the ionization of a weak acid.
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strong base
A base that dissociates completely into metal ions and hydroxide ions
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weak base
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*  ionizes only partially in dilute aqueous solution.
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base ionization constant
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*  is the value of the equilibrium constant expression for the ionization of a base.