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122 Cards in this Set
- Front
- Back
the capacity for doing work or supplying heat
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energy
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enery that transfers from one object to another because of temperature difference between them
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heat
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defined as the quantity of heat needed to raise the temperature of one gram of pure water one degree Celcius
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calorie
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the SI unit of energy
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joule
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4.18 J
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1 cal
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the quatntity of heat required to change an objects temperature by exactly one degree Celsius
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heat capacity
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amount of heat it take to raise one gram of a substance one degree Celsius
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specific heat capacity
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a heat absorbic process
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endothermic process
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a heat dissipating process
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exothermic process
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the measurement of heat changes for physical and chemical processes
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calorimetry
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the tendency of molecules and ions to move toward areas of lower concentration until the concentration is uniform thoughout the system
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diffusion
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the pressure exerted by each gas in a gaseous mixture
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partial pressure
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factors of gases
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Pressure (kPa, atm, mm Hg)
Temperature (K) Volume (L, mL) |
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pressure and volume are inversely proportional in a gas, if temperature is kept constant
P1 x V1 = P2 x V2 |
Boyle's Law
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temperature and volume are directly proportional, if pressure is kept constant
V1/T1 = V2/T2 |
Charles' Law
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(P1 x V1)/T1 = (P2 x V2)/T2
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Combined Gas Law
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PV = nRT
(pressure x volume = # of moles x constant x temperature) |
Ideal Gas Law
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at a constant temperature and volume, total pressure exerted by a mix of gases is equal to the sum of partial pressures of the component gases
P1 + P2 + P3...= PT |
Dalton's Law of Partial Pressure
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equal volume of gases at the same temperature pressure contain equal numbers of particles
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Avogadro's hypothesis
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rate of effusion of gas is inversely proportional to the square root of its molar mass
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Graham's Law
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STP
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Standard Temperature and Pressure
T= 0 degrees C P= 101.3 kPa, 760 mm Hg, 1 atm V= 22.4 L |
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1 nutritional Calorie
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1000 calories
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the height of a wave
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amplitude
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the pattern of frequencies obtained by passing light emited by atoms of an element in the gaseous state thorough a prism
the emission spectrum of each element is unique to that element |
atomic emission spectrum
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the arrangement of electrons around the nucleous of an atom in its ground state
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electron configuration
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a region around the nucleous of an atom where an electron is likely to be moving
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energy level
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a series of energy waves that travel in a vacuum at 3.0 10^10 cm/s
includes radio waves, microwaves, visible light, infrared and ultraviolet light, x-rays, and gamma rays |
electromagnetic radiation
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the lowest energy level occupied by an electron when an atom is in its most stable energy state
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ground state
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(v) the number of wave cycles that pass a given point per unit of time
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frequency
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the distance between two adjacent crests of a wave
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wavelength
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the SI unit of frequency, equal to one cycle per second
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hertz
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electrons are ejected by certain metals when they absorb light with a frequency above a threshold frequency
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photoelectric effect
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a quantum of light
a discrete bundle of electromagnetic energy that behaves as a particle |
photon
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the amount of energy needed to move an electron
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quantum
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half the distance between the nuclei in a molecule consisting of identical...
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atomic radius
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the tendency for an atom to attract electrons to itself when it is chemically combined with another element
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electronegativity
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the energy required to remove an electron from a gaseous atom
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ionization energy
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a vertical column of elements in the periodic table
the contituent elements of a group have similar chemical and physical properties |
group
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a horizontal row of elements in the periodic table
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period
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electrons enter orbitals of lowest energy first
lowest to highest |
Aufbau principle
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wave mechanics
wave like motions |
de Broglie's equations
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cannot know both velocity and position of particle (electron) at the same time
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Heisenberg uncertainty principle
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each orbital will get one electron before any orbital gets two
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Hund's rule
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two elecrons per orbital
now two electrons will have the same quantum number (NLMS) |
Pauli exclusion principle
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arranged by increasing atomic number
periodic repitition of physical and chemical properties |
Periodic Law
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Group IA
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alkaline metals
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Group IIA
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alkaline earth metals
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Group VIIA
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halogens
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Group VIIIA
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noble gases
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A Group
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representative
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B Group
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transistion metals
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lanthanide and actinide series
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rare earth metals
(inner transition) |
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two different atoms joined by a convalent bond and the bonding electrons are shared unequally
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polar
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atoms in molecules are alike and bonding electrons are shared equally
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nonpolar
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angle at which adjacent atoms in a molecule are attracted
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bond angle
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a notation that depicts valence electrons as dots around the atomic structure of the element
the symbol represents inner electrons and atomic nucleus |
electron dot structure
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a process by which several atomic orbitals (such as s and p)mix to form the same number of equivalent hybrid orbitals
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hybridization
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atoms react by gaining or losing electrons as to acquire the stable electron structure of a noble gas, usually eight valence elctrons
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octet rule
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any atom or group of atoms with a negative charge
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anion
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any atom or group of atoms with a positive charge
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cation
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a molecule in which one or more atoms is slightly negative and one or more is slightly positive, unless molecular geometry causes the polarities to cancel each other out
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polar molecule
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a chemical formula that shows the arrangement of atoms in a molecule or polyatomic ion
each dash between two atoms indicates a pair of shared electrons |
structural formula
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a pair of valence electrons that is not involved in bonding
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unshared pair
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an electron in the highest occupied energy level of an atom
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valence electrons
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valence-shell electron-pair repulsion theory
because electron pairs repel, molecules adjust their shapes so that vealence-electron pairs are as far apart as possible |
VSEPR theory
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a term used to describe the weakest intermolecular attractions
these include dispersion forces and dipole interactions |
van der Waals forces
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the weakest kind of intermolecular attractions
this attraction is thought to be caused by the motion of electrons |
dispersion force
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a relatively strong intermolecular force in which a hydrogen atom that is covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom in the same moleculr or one nearby
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hydrogen bond
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metal (cation) and nonmetal (anion) are bonded together
electrostatic attraction |
ionic
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two nonmetals are bonded together
share electrons |
covalent
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within metals
conducts electricity |
metallic
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an inward force that tends to minimize the surface area of a liquid
it causes the surface to behave as if it were a thin skin |
surface tension
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a suface active reagent
any sustance with molecules that interfere with the hydrogen bonding between water molecules, reducing surface tension i.e. soaps and detergents |
surfactants
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(aq) a solution in which the solvent is water
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aqueous solutions
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the dissolving medium in a solution
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solvent
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dissolved particles in a solution
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solute
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a compound that conducts an electric current in aqueous solution or in the molten state
all ionic compounds are this |
electrolyte
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a compound that does not conduct an electric current in aqueous solution or in the molten state
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nonelectrolyte
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a mixture form which some of the particles settle out slowly upon standing
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suspension
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a mixture whose particles are intermediate in size between those of a susupension and a solute solution
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colloid
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scattering of light by particles in a colloid or suspension, which causes a beam of light to become visible
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Tyndall effect
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the chaotic movement of colloidal paricles caused by collision with particles of the solvent in which they are dispersed
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Brownian motion
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the colloidal dispersion of one liquid in another
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emulsion
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to lose water of hydration
the process occurs when the hydrate has a vapor pressure higher than that of water vapor in in the air |
effloresce
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a term describing salts and other compounds that remove moisture form the air
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hygroscopic
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a hygroscopic substance used as a drying agent
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desiccant
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a term describing a substance that removes sufficient water from the air to form a solution
the solution formed has a lower vapor pressure that that of the water in the air |
deliquescent
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a solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure
an equilibrium exists between undissolved solute and ions in solution |
saturated solution
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a solution that contains less solute than a saturated solution at a given temperature and pressure
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unsaturated solution
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describes liquids that dissolve in each other
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miscible
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describes liquids that are insoluble in one another
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immiscible
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at a given temperature, the solubility of a gas in a liquid is directly porportional to the pressure of the gas above the liquid
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Henry's Law
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a solution that contains more solute that it can theoretically hold and a given temperature
excess solute preciptates if a seed crystal is added |
supersaturated solution
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(M) the concentration of solute in a solution expressed as the number of moles of solute dissolved in one liter of solution
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molarity
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bond angle of water
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105 degrees
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at what temperature is water at maximum density
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4 degrees C
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? = moles of solute/liters of solution
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Molarity
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a compound that produces hydrogen ions in solution, is a hydrogen-ion donor, or an electron-pair acceptor
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acid
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a compound that produces hydroxide ions in solution, is a hydrogen-ion acceptor, or an electron-pair donor
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base
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a solution in which the pH remains relatively constant when small amounts of acid of base are added
can be either a solution of a weak acid and the salt of a weak acid or a solution of a weak base and the salt of a weak base |
buffer
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a number used to denote the hydrogen-ion concentration, or acidity, of a solution
it is the negative logarithm of the hydrogen-ion concentration of a solution |
pH
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(H3O+) the positive ion formed when a woter molecule hains a hydrogen ion
all the hydrogen ion in aqueous solution are present as this |
hydronim ion
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(OH-) the negative ion formed when a water molecule loses a hydrogen ion
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hydroxide ion
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method used to determine the concentration of a solution (often an acid or base)
a solution of known concentration (the standard)is added to a measured amount of the solution of unknown concentration until an indicator signals the end point |
titration
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an organic compound that contains only carbon and hydrogen
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hydrocarbon
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the controlled process by which hydrocarbons are broken down or rearranged into smaller, more useful molecules
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cracking
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a very large molecule formed by the covalent bonding of repeating small molecules, known as monomers
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polymers
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a simple molecule that repeatedly combines to form a polymer
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monomer
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an organic compound having and -OH (hydroxyl)group
the general structure is R-OH |
alocohol
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an organic compound having amino (-NH2) and carboxylic (-COOH) groups in the same molecule
proteins are made from this |
amino acid
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a name originally given to the arenes because many of them have pleasant odors
any compound with bonding like that of benzene |
aromatic compound
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the name given to monomers and polymers of aldehydes and ketones that have numerous hydroxyl groups
i.e.sugars and starches |
carbohydrates
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proteins that act as catalyst
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enzyme
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a member of a large class of relatively water-insoluble organic compounds
i.e. fats, oils, waxes |
lipids
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a polymer of RNA or DNA found primarily in cell nuclei
play an important role in the transmission of hereditary characteristics, protein syntheis, and the control of cell activities |
nucleic acid
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one of the monomers that make up DNA and RNA
it consists of a nitrogen-containing base, a sugar, and a phosphate group |
nucleotide
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any peptide with more than 100 amino acids
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protein
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the process used to make soap
in involves the hydrolysis of fats or oils by a hot aqueous alikli-metal hydroxide |
saponification
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an organic compound in which all carbon atoms are joined by single covalent bonds
it contains the maximum number of hydrogen atoms |
saturated compounds
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an organic compound with one or more double or triple carbon-carbon bonds
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unsaturated compounds
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functional group for organic acids
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COOH
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functional group for alcohols
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OH
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