chemistry.txt

The volume of a fixed mass of gas varies inversely with pressure at constant temperature

• PV=T
• P₁V₁=P₂V₂

The pressure of a fixed mass of gas at constant volume varies directly with the Kelvin temperature

• P/T=K
• P=KT
• P₁/T₁=P₂/T₂

The relationship between the pressure, volume, and temperature of a fixed amount of gas

• PV/T=K
• P₁V₁/T₁=P₂V₂/T₂

The total pressure of a mixutre of gases is equal to the sum of the partial pressures of the component gases

Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules

At constant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers

e volume occupied by one mole of gas at STP,22.414 10 L

The mathematical relationship of pressure, volume, temperature, and the number of moles of a gas

The constant R,0.082 057 94 L*atm/mol*K

The rates of effusion of gases at the same temperature and pressure are inversely proportional to the square roots of their molar masses

A chemical compound that increases the concentration of hudrogen ions, H⁺, in aqueous solution

A substance that increases the concentration of hydroxide ions, OH^-, in aqueous solution

An acid that contains only two different elements: hydrogen and one of the more electronegative elements

And adic that is a coumpond of hydrogen, oxygen, and a third element, usually non-metal

An acid that ionizes completely in aquesous solution

• Examples:
• Perchloric acid, HCIO₄, hydrochloric acid, HC₁, nitric acid, HNO₃

An acid that is a weak electrolyte

Strong electrolytes

• Examples:
• Potassium hydroxide (KOH), Sr(OH)₂, Ba(OH)₂, NaOH, RbOH, CsOH

Any species that can react as either an acid of a base

A molecule or ion that is a protein donor

• Examples:
• Hydrogen chloride

The transfer of protons from one reactant (the acid) to another (the base)

A molecule or ion that is a proton acceptor

• Examples:
• Ammonia

An atom, ion, or molecule that accepts an electron pair to form a covalent bond

• Examples:
• Boron trifluoride

An atom, ion, or molecule that donates an electron pair to form a covalent bond

• Examples:
• Anion

The formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor

The species that is formed when a Bronsted-Lowry base gains a proton

The species that remains after a Bronsted-Lowry acid has given up a proton

The reaction of hydronium ions and hydroxide ions to form water molecules

An ionic compound composed of a cation and the anion from an acid; an ionic compound composed of a cation from a base and an anion from an acid

The controlled addition and measurement of the amount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentration

• 1) Solutions have a sour taste
• 2) Acids change the color of acid-based indicators
• 3) Some acids react with active materials to release hydrogen gas
• 4) Acids react with bases to produce salts and water
• 5) Some acids conduct electric current

• 1) Aqueous solutions of bases taste bitter
• 2) Bases change the color of acid based indicators
• 3) Dilure aqueous solutions of bases feel slippery
• 4) Bases react with acids to produce salts and water
• 5) Bases conduct electric current

The pH range over which an indicator changes color

The energy transferred between samples of matter because of a difference in their temperature

A measure of the avereage kinetic energy of the particles in a sample of matter

The energy a body has by virtue of its motion

The amount of energy absorbed or lost by a system during a process at constant pressure

The study of the changes in heat energy that accompany chemical reactions and physical changes

The amount of heat energy required to raise the temperature of one gram of substance by one Celsius degree (1 ^oC) or one kelvin (1K)

A measure of the degree of randomness of the particles, such as molecules, in a system

The combined enthalphentropy function of a system

A transitional structire that results from an effective collision and that persists while old bonds are breaking and the new bonds are forming

The minimum energy required to transform the reactants into an activated complex

The set of assumptions explaining how chemical reactions take place and why rates of reaction alter

The step-by-step sequence of reactions by which the overall chemical change occurs

Referring to a chemical reaction that absorbs heat

Referring to a chemical reaction that releases heat

A substance that changes the rate of a chemical reaction without itself being permanently consumed

The change in concentration of reactants per unit time as a reaction proceeds

• 1) Nature of reactants
• 2) Surface area
• 3) Temperature
• 4) Concentration
• 5) Presence of Catalysts

The energy released when a nucleus is formed from nucelons

A proton or neutron

The general term for any isotope of any element, another term for an atom that is identified by the number of protons and neutrons in its nucleus

A change in the identity of a nucleus as a result of a change in the number of its protons

A reaction that affects the nucleus of an atom

Two protons and two neutrons bound together and emitted from the nucleus during some kinds of radioactive decay

An electron emitted from the nucleus during some kinds of radioactive decay

A high-energy electromagnetic wave emitted from a nucleus as it changes from an excited energy state to a ground energy state

The time required for half of the atoms of a radioactive nuclide to decay

The particles or electromagnetic radiation emitted from the nucleus during radioactive decay

A particle that has the same mass as an electron but has a positive charge and is emitted from the nucleus during some kinds of radioactive decay

The spontaneous disintegration of a nucleus into a slightly lighter and more stable nucleus, accompanied by emission of particles and/or electromagnetic radiation

The quantity of ionizing radiation that does as much damage to human tissues as is done by 1 roentgen of high voltage X rays

A unit used to measure nuclear radiation; equal to the amount of radiation that produces 2 x 10⁹ ion pairs when it masses through 1 cm³ of dry air

A radioactive atom that is incorporated into a substance so that movement of the substance can be followed by a radiation detector

The process by which the approximate age of an object is determined based on the amount of certain radioactive nuclides present

A process in which a very heavy nucleus splits into more-stable nuclei of intermediate mass

The combining of light-mass nuclei to form a heavier, more stable nucleus

A material used to slow down the fast neutrons produced by fission

A nuclide produced by the decay of a parent nuclide

The heaviest nuclide of each decay series

The volume of a fixed mass of gas at constant pressure varies directly with the Kelving temperature K=273.15^{+ o}C

• V=KT
• V/T=K
• V₁/T₁=V₂/T₂

The temperature -273.15^o C, given a value of zero in the Kelvin scale

The forces per unit area on a surface

The agreed-upon standard conditions of exactly 1 atm pressure and 0^o C

A theory based on the idea that particles of matter are always in motion

An imaginary gas that perfectly fits all of the assumptions of the kinetic-molecular theory

Spontaneous mixing of the particles of two substances caused by their random motion

A process by which gas particles pass through a tiny opening

The reactant that limits the amounts of the other reactants that can combine - and the amount of product that can form - in a chemical reaction

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

A conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction

The ratio of the actual yield to the theoretical yield, multiplied by 100

Percent Yield = (actual yield/theoretical yield)*100

Calculations involving the mass relationships of elements in compounds

Calculations involving the mass relationships between reactants and products in a chemical reaction