High School Chemistry Final – Flashcards
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Absolute Zero
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The zero point on the kelvin scale (-273K)
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Accepted Value
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A quantity used by the general scientific community
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Accuracy
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Closeness to the true value of the measurement
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Acid
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Compound that produces hydrogen ions in a solution
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Acid dissociation constant
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An equilibrium expression used to measure weak-acid strength, given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations, with each term raised to the power of its stoichiometric coefficient. K of A
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Acidic Solution
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Any solution in which the hydrogen ion constant is greater than the hydroxide ion constant
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Activated Complex
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An activated complex is an intermediate state that is formed during the conversion of reactants into products. An activated complex is the structure that results at the maximum energy point along the reaction path. The activation energy of a chemical reaction is the difference between the energy of the activated complex and the energy of the reactants.
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Activation energy
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The minimum energy colliding particles need to react
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Active site
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A groove in an enzyme where the reactant of a reaction fits and is converted into products
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Activity series
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A list of elements in order of decreasing activity
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Actual yield
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The amount of product that forms when a reaction is carried out in a lab
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Addition reaction
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A reaction in which a substance is added at the double or triple bond of an alkene or and alkyne
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ATP
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The molecule that transmits the energy of all living things
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Alcohol
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An organic compound that has an OH (hydroxyl)
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Alkali Metal
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Group 1A
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Alkaline earth metal
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Group 2A
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Alkaline Solution
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Basic Solution
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Alkane
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Hydrocarbon with only one covalent bond (saturated)
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Alkyl group
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Hydrocarbon substituent, the methyl group is an alkyl group
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Alkyne
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A hydrocarbon containing triple bonds (unsaturated)
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Allotrope
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One of two or more different molecular forms of an element in the same physical state
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Alloy
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A mixture composed of two or more elements, at least one is a metal
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Alpha particle
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A positively charged particle emitted from a radioactive nuclei, identical to the nucleus of helium
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Amorphous Solid
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Solid that lacks ordered structure, random arrangement of atoms
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Amphoteric
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Could be either and acid or a base
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Amplitude
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Height of a wave's crest
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Analytical chemistry
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The area of chemistry that focuses on composition of matter
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Anion
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Atom with a negative charge
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Applied Chemistry
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Research that is directed towards a practical goal
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Aqueous solution
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Water that contains a dissolved substance
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Aromatic compound
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Contains a benzene ring
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Atmospheric pressure
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Pressure exerted by atoms and molecules in the atmosphere
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Atom
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Smallest particle of an element the retains its identity
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Atomic emission spectrum
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The pattern formed formed when light passes through a prism, separating it into different frequencies of light
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Atomic mass
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The weighted mass of the averages of the isotopes of an element
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Atomic mass unit
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Unit of mass equal to 1/12th of the mass of a carbon-12 atom
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Atomic Number
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The number of protons in the nucleus of an atom
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Atomic radius
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One-half the distance between the nuclei of two of the atoms of the same element when they are joined
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Aufbau Principle
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The rule that electrons occupy the orbitals of the lowest energy first
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Avagadro's Number
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The number of particles in one mole, 6.02*E23
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Balanced equation
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A chemical equation in which mass is conserved on either side
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Band of stability
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The location of stable nuclei on a neutron vs. proton plot
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Barometer
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Used to measure atmospheric pressure
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Base
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Compound that produces hydroxide ions in a solution
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Base dissociation constat
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An equilibrium expression used to measure weak-base strength, given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations, with each term raised to the power of its stoichiometric coefficient. K of B
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Basic Solution
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Any solution in which the hydroxide concentration is higher than the hydrogen concentration
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Beta Particle
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An electron resulting from the breaking apart of neutrons in an atom
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Binary Compound
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Compound composed of two elements
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Boiling Point
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The point at which the vapor pressure of a liquid is just equal to the external pressure on the luquid
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Boiling point elevation
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The difference in temperature between the boiling point of a solution and the point of the solvent
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Bonding orbital
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A molecular orbital that can be occupied by the two electrons of a covalent bond
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Boyle's Law
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For a given mass of a gas at a constant temperature, the volume of the gas varies inversely
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Brownian motion
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The chaotic movement of the colloidal particles, caused by collision with particles of the solvent in which they are dispersed
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Buffer
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A solution in which the pH remains constant when small amounts of an acid/base are added
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Calorie
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The quantity of heat needed to raise 1g of water
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Calorimeter
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An insulated device
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Catalyst
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Speeds up the rate of reaction
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Cation
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Positive charge
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Celsius scale
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0 deg C is freezing point and 100 deg C is boiling point
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Chemical Change
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A change that produces matter with a different composition
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Chemical equation
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Expression representing a chemical reaction
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Chemical equilibrium
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A state of balance in which the rates of the forward and reverse reactions are equal
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Chemical formula
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An expression indicating the number and type of atoms present in the smallest unit of a substance
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Potential Energy
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Energy stored in bonds
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Chemical property
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Ability to undergo specific chemical change
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Chemical reaction
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A change in which one or more of the reactants change into one or more of the products
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Cis configuration
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The configuration in which substituent groups are on the same side of a double bond
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Coefficient
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A small whole number used to preserve the mass of the equation
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Colligative property
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A property of a solution that depends only upon the number of the solute and not on their identities
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Collision theory
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Atoms, ions, and molecules react when they collide, provided they have enough kinetic energy
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Colloid
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Particles are between suspension and solution
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Combination reaction
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A+B-->C
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Combined gas law
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describes a relationship between pressure, temperature and the volume of an enclosed gas
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Combustion reaction
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A chemical change in which an element reacts with oxygen forming heat and light
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Compound
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A substance that contains two or more elements that chemically combine in a fixed proportion
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Concentrated solution
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A solution containing a large amount of solute
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Concentration
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A measurement of the amount of solute that is dissolved in a given quantity of solvent
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Conjugate acid
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The particle formed when a base gets a hydrogen atom
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Dalton's atomic theory
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The first theory to relate a chemical change to events at the atomic level
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Density
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Mass/Volume
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Dipole
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A molecule with two poles with opposite charges
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Dispersion forces
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Attractions between molecules caused by the electron motion one one affecting the motion on the other
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Distillation
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A process used to separate dissolved solids from a liquid which is boiled then condensed
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Double covalent bond
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Bond where two atoms share two pairs of electrons
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Effusion
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Gas escapes through a tiny hole
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Electrolysis
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Electrical energy is used to bring about chemical change
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Electrolyte
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A compound that conducts and electrical current, ionic compounds
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Electromagnetic radiation
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energy that travels through space in the form of waves
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Electron
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negatively charged particle; located outside the atomic nucleus
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Electron dot structure
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diagrams that show valence electrons as dots
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Element
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The simplest form of matter that has unique properties
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Empirical formula
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a chemical formula showing the ratio of elements in a compound rather than the total number of atoms
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Emulsion
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Colloidal dispersion of one liquid in another
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Endothermic
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Absorbs heat from surroundings
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End point
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Point in titration which changes the indicators color
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Energy
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Capacity for doing work
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Energy Level
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The specific energies an electron in an atom can have
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Enthalpy (H)
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The heat content of a system at constant pressure
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Entropy (S)
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Measure of disorder
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Enzyme
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Protein that acts as a catalyst in a reaction
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K eq
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Equilibrium Constant (Eq should be written as subscript) K eq= [C][D]/[A][B] - If the equilibrium constant is greater than 1, then the products (C&D) are in greater concentration than the reactants at equilibrium, meaning that the reaction tends to go to completion as written.
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Equivalence Point
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Point of titration where moles of hydrogen and moles of hydroxide are equal
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Error
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Difference between accepted value and experimental value
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Ether
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Organic compound in which oxygen is bonded to two carbon groups
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Evaporation
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Vaporization that occurs at the surface of a liquid that is not boiling
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Exothermic process
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A process that releases heat to its surroundings
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Experiment
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Repeatable procedure
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Extensive property
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A property that depends on the amount of matter in a sample
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Film badge
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A radiation detector that flashes in the presence of radiation
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Filtration
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Process that separates a solid from the liquid in a heterogenous mixture
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Fission
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The splitting of the nucleus into smaller fragments
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Formula Unit
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The lowest whole-number ratio of ions in an ionic compoud
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Free energy
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The energy available to do work
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Frequency
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The number of wave cycles that pass a point per unit of time
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Fusion
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Combining nuclei
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Gamma ray
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Photon emitted by a radioisotope
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Gas pressure
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Results from the force exerted by a gas per unit surface area of an object
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Gay-Lussac's Law
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P/T
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Gibbs Free Energy Change
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The maximum amount of energy that can be coupled to another process to do useful work
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Grahams Law of Effusion
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The rate of effusion of a gas is inversely proportional to the square root of its molar mass
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Ground state
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Lowest energy of an atom
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Halogen
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Group 7A
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Heat capacity
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Heat needed to increase the temperature of the object by 1 deg C
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Heat of combustion
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The heat of reaction for the complete burning of one mole of a substance
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Heisenburg Uncertainty Principle
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It is impossible to know velocity and position at the same time
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Henry's Law
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At a given temperature the solubility of a gas in a liquid is directly proportional to the pressure of the gas
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Hertz
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The unity of frequency
