chemistry final 2nd Semester

a reactant that:

-is totally consumed in a reaction

-limits the extent of the reaction

-determines the amount of product

A reaction stops when one reactant is used up. That reactant is the limiting reactant.

6.02 x 10^23

6.02 x 10^23 particles

the particle being counted

the mass in grams of one mole of a pure substance

number of moles x molar mass

m=nM

the sum of the masses of the particles

that make up one mole of the compound

the percent by mass of each element in a compound

the formula with subscripts that are the actual number of atoms

the formula with subscripts that are the smallest possible whole-numbers

a compound that has a specific number of water molecules bound to its atoms

“compound” & “prefixhydrate” formula is AX•nH20

Na₂SO₄∙10H₂O is used to store solar energy

the study of quantitative relationships among reactants and products

the ratio between any two substances in a balanced chemical equation

4Fe(s)+3O₂(g)→2Fe₂O₃(s)

ratio of number of moles of Fe2O3 to mo moles of Fe

a reactant that remains after the reaction stops

the maximum amount of product that can be produced from a given amount of reactant

the amount of product produced when the chemical reaction is carried out in an experiment

ratio of actual yield to theoretical yield

describes behavior of matter in terms of particles in motion

1. tiny particles in lots of empty space

2. straight line motion until they collide with each other or with the walls of the container

3. collisions are elastic

4. temperature is a measure of kinetic energy

a collision in which no kinetic energy is lost

a measure of the average kinetic energy of the particles in a sample

the movement of one material through another from an area of high concentration to an area of low concentration

force per unit area

space between gas particles decreases as gas compresses.

space between gas particles increases as gas expands.

equals 14.7 psi, or 760 mmHg

1N/m^2

an instrument used to measure atmospheric pressure

an instrument used to measure vapor pressure of a substance

total pressure of a mixture of gas is the sum of the pressures of all the gasses in the mixture Ptotal=P1+P2+P3+...Pn

attraction between oppositely charged regions of polar molecules=medium

weak force resulting from temporary shifts in the density of electrons in the electron cloud=weak

A strong dipole-dipole attraction between molecules that contain a hydrogen atom bonded to a small, highly electronegative atom formed only by an H atom bonded to N, O, or F atoms

Hold atoms or ions together within a molecule

Hold molecules to each other.

(dipole dipole and london and hydrogen bond)

resistance to flow

the energy required to increase the surface area of a liquid

One of two or more forms of an element with different structures in the same state of matter.

A solid whose atoms, ions, or molecules are not arranged in a regular repeating pattern.

The temperature at which a crystalline solid becomes a liquid

The process by which a liquid changes to a gas or vapor

The temperature at which a liquid becomes a gas

The pressure exerted by a vapor over a liquid

Vaporization occurring only at the surface of a liquid.

Vaporization occurring throughout a liquid

The process by which a solid changes directly to a gas without first becoming a liquid.

shape: definite \n volume: definite \n expansion on heating: small \n compressibility: no

particles flow, vaporization, definite volume, assumes the shape of the container, condensed phase, IMFs present disorder of particles

expand to volume of the container, highly compressible, form homogenous mixtures, IMFs nonexistentfc

The process by which gas becomes a liquid

The temperature at which liquid becomes a crystalline solid

The process by which substance changes from a gas into a solid without first becoming a liquid.

A graph of pressure versus temperature that shows the phases of a substance

The T and P where solid, liquid, and gas can coexist

melting, vaporizing, condensation, freezing, sublimation, deposition

melting, vaporization, sublimation.

freezing, condensation, deposition.

The temperature above which a substance cannot exist at a liquid.

melting point at a pressure of 1 atmosphere

the temperature at which the vapour pressure is equal to the standard sea-level atmospheric pressure

force of attraction between identical molecules

force of attraction between molecules that are different

A compound that lowers the surface tension of water

A solid whose atoms, ions, or molecules are arranged in an orderly, geometric structure

The smallest arrangement of atoms in a crystal lattice that has the same symmetry as the entire pattern of lattice

P₁V₁ = P₂V₂

the lowest possible theoretical temperature

V1/T1 = V2/T2

P₁/T₁=P₂/T₂

P₁V₁/T₁ = P₂V₂/T₂

equal volumes of gases at same T & P have same number of particles

the volume that 1 mole of gas occupies at STP

0˚C and 1 atm, 22.4L

an experimentally determined constant whose value

depends on the units for pressure (should be given on the test)

PV = nRT

a mixture that does not have uniform composition and in which the individual substances remain distinct

a heterogeneous mixture containing particles that settle out if left undisturbed

a heterogeneous mixture that is viscous at rest but flows when agitated

a heterogeneous mixture of intermediate-sized particles that do not settle out

the most abundant substance in a colloid (usually water)

particles that do not settle out of a colloid

erratic, random movement of dispersed particles caused by collisions with the dispersion medium.

the scattering of light by dispersed colloid particles

a mixture that has uniform composition throughout

another word for homogeneous mixture

a substance dissolved in a solution

the substance that dissolves a solute

describes a substance that can be dissolved in a solution

opposite of soluble

describes two liquids that are soluble in each other

opposite of miscible

a combination of two or more pure substances that retain their individual chemical properties

a measure of how much solute is dissolved in a specific amount of solvent or solution

Mass of solute/mass of solution times 100

volume of solute/volume of solution times 100

moles of A/moles of A plus moles of b

moles of solute/liters of solution times 100

to dilute from concentrated solution to less concentrated solution. M1V1=M2V2