Terms : Hide Images
| 6437296146 | PEL 1 | 2 Electrons | 0 | |
| 6437297915 | PEL 2 | 8 Electrons | 1 | |
| 6437297916 | PEL 3 | 18 Electrons | 2 | |
| 6437299707 | PEL 4 | 32 Electrons | 3 | |
| 6437299708 | PEL 5 | 50 Electrons | 4 | |
| 6437308756 | nucleons | protons and neutrons | 5 | |
| 6437310667 | mass number | number of neutrons in nucleus | 6 | |
| 6437312704 | atomic number | number of protons in nucleus | 7 | |
| 6437324153 | isotopes | same number of protons and electrons but different number of neutrons | 8 | |
| 6437347645 | average atomic mass | based on the percentage of isotopes found in nature | 9 | |
| 6437350387 | valence electrons | electrons in the outermost shell (can be easily shared, gained or lost) | 10 | |
| 6437354677 | core electrons | electrons in the inner shell | 11 | |
| 6437368738 | atomic spectra | the electromagnetic emission from atoms and molecules | 12 | |
| 6437418715 | spectroscopy | A technique measuring electromagnetic emissions that is widely used in chemical analysis and in studies of the properties of atoms, molecules, ions, etc. | 13 | |
| 6437437774 | wave mechanical model | Modern model of the atom, atoms have electrons in "orbitals" that are like clouds around the nucleus | 14 | |
| 6437447617 | quantum numbers | specify the properties of atomic orbitals and the properties of electrons in orbitals | 15 | |
| 6437449966 | Pauli Exclusion Principle | An atomic orbital may describe at most two electrons, each with opposite spin direction | 16 | |
| 6437473575 | Hund's Rule | electrons do not pair up until they have to | 17 | |
| 6437475422 | Aufbau Principle | An electron occupies the lowest-energy orbital that can receive it | 18 | |
| 6437487157 | lewis Structures |  | 19 | |
| 6437490119 | Nobel Gas Notation | shortcut→ find the closest noble gas (column 18) with fewer electrons than the element then finish configuration | 20 | |
| 6437503453 | transition elements | What are the elements in groups 3-12 called? | 21 | |
| 6437518993 | transition element properties | elements that have high melting points, often paramagnetic, tend to form salts when reacted w/ halogens ex; iron, copper, gold, silver, and titanium | 22 | |
| 6437575781 | electronegativity | A measure of the ability of an atom in a chemical compound to attract electrons | 23 | |
| 6437578634 | ionization energy | The amount of energy required to remove an electron from an atom | 24 | |
| 6437583074 | alpha decay | A nuclear reaction in which an atom emits a ________ particle consisting of two protons and two neutrons. This increases the atomic number by 2 and the mass number by 4. | 25 | |
| 6437586693 | beta decay | A nuclear reaction in which a neutron changes into a proton and into an electron, and the atoms emits a ______ particle, which is the electron. It increases the atomic number of the atom without changing the mass. | 26 | |
| 6437590735 | gamma radiation | electromagnetic radiation emitted during radioactive decay and having an extremely short wavelength | 27 | |
| 6649993024 | covalent bond | A chemical bond that involves sharing a pair of electrons between atoms in a molecule | 28 | |
| 6649993305 | dipole-dipole attraction | attractive force resulting when polar molecules line up so that the positive and negative ends are close to each other | 29 | |
| 6649993853 | electrostatic repulsion | Describes a force between particles with opposite electrical charges that causes them to push apart from one another | 30 | |
| 6649994166 | hybridization | Several atomic orbitals mix to form the same total number of equivalent hybrid orbitals | 31 | |
| 6649995145 | hydrogen bond | A relatively weak bond formed between any hydrogen atom (which is covalently bound to a nitrogen or oxygen atom) and a nitrogen or oxygen with an unshared electron pair | 32 | |
| 6649995457 | ionic bond | Formed when one or more electrons are transferred from one atom to another | 33 | |
| 6649995861 | London dispersion forces | The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles | 34 | |
| 6649996089 | metallic bond | a bond formed by the attraction between positively charged metal ions and the electrons around them | 35 | |
| 6649996364 | pi bond | when two p orbitals line up in parallel and electron clouds overlap. it exsits over a single bond. | 36 | |
| 6649997810 | resonance structure | a structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion | 37 | |
| 6649998908 | stable octet | the arrangement of eight electrons in the outermost shell of an atom | 38 | |
| 6649999221 | sigma bond | a bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei | 39 | |
| 6649999573 | van der Waals forces | a slight attraction that develops between the oppositely charged regions of nearby molecules | 40 | |
| 6649999929 | VSERP | Valance Electron Pair Repulsion model / Unshared electron pairs around the central atom | 41 | |
| 6650001132 | binary compound | What ionic compounds are called when they are composed of only two different kinds of atoms. | 42 | |
| 6650001133 | coefficient | A number in front of a chemical formula in an equation that indicates how many molecules or atoms of each reactant and product are involved in a reaction. | 43 | |
| 6650001514 | emperical formula | simplest whole # ration of atoms in a compound | 44 | |
| 6650001886 | formula mass | the sum of the average atomic masses of all the atoms represented in the formula of any molecule, formula unit, or ion | 45 | |
| 6650002556 | molecular mass | The sum of the masses of all the atoms in a molecule | 46 | |
| 6650002927 | Law of Definite Composition | Chemical compounds are composed of a fixed ratio of elements as determined by mass. | 47 | |
| 6650003224 | Law of Multiple Proportions | whenever two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers | 48 | |
| 6650003732 | net ionic equation | Includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution | 49 | |
| 6650003932 | percentage composition | the percentage by mass of each element in a compound | 50 | |
| 6650004295 | polyatomic ion | A covalently bonded group of atoms that has a positive or negative charge and acts as a unit | 51 | |
| 6650004466 | products | The elements or compounds produced by a chemical reaction. | 52 | |
| 6650004676 | reactants | a substance that takes part in and undergoes change during a reaction | 53 | |
| 6650005137 | Stock system | A method for naming ions of elements that can form more than one possible positive charge by using a Roman numeral after the ion name to denote the ion's charge. | 54 | |
| 6650005556 | ternary compound | A compound that consists of three or more elements, usually containing | 55 | |
| 6650005557 | true formula | chemical formula that indicates the actual number of atoms of each element in one molecule of a substance | 56 | |
| 6650006770 | atmosphere | Layers of different gases that surround the Earth. | 57 | |
| 6650008025 | atmospheric pressure | the pressure exerted by atoms and molecules in the atmosphere surrounding Earth, resulting from collisions of these particles with objects | 58 | |
| 6650008249 | greenhouse effect | Natural situation in which heat is retained in Earth's atmosphere by carbon dioxide, methane, water vapor, and other gases | 59 | |
| 6650008555 | manometer | A device used to measure the pressure of a sample of gas in a container. | 60 | |
| 6650008880 | Boyle's Law | PV = k | 61 | |
| 6650009301 | Charles's Law | V/T = k | 62 | |
| 6650010778 | Combined Gas Law | P1V1/T1=P2V2/T2 (constant n) | 63 | |
| 6650012519 | Ideal Gas law | PV = n R T | 64 | |
| 6650013191 | Dalton's Law of Partial Pressures | Total pressure of a gas is equal to the sum of the partial pressure of the component gases | 65 | |
| 6650013612 | Graham's Law | Rate of diffusion of a gas is inversely proportional to the square root of its molecular weight. | 66 | |
| 6650013613 | Kinetic-Molecular Theory | a theory that explains that the behavior of physical systems depends on the combined actions of the molecules constituting the system | 67 | |
| 6650015459 | mercury barometer | An instrument that measures changes in air pressure, consisting of a glass tube partially filled with mercury, with its open end resting in a dish of mercury. | 68 | |
| 6650015460 | ozone | A form of oxygen that has three oxygen atoms in each molecule instead of the usual two. | 69 | |
| 6650015633 | pascal | the SI unit of pressure equal to one newton per square meter | 70 | |
| 6650015634 | standard pressure | 1 atm or 101.3 kPa | 71 | |
| 6650017208 | standard temperature | One atmosphere and 273 K. | 72 | |
| 6650017607 | torr | the force per unit area exerted by the gas on its container, usually measured in atmospheres | 73 | |
| 6650021978 | acidic anhydride | a nonmetallic oxide that, when placed in water, reacts to form an acid solution | 74 | |
| 6650021979 | aeration | Air is forced through the water to release unwanted gases, which reduces odor and improves taste | 75 | |
| 6650022257 | alloy | A mixture of two or more metals | 76 | |
| 6650022258 | boiling point | The temperature at which a liquid changes to a gas | 77 | |
| 6650022585 | Brownian movement | kinetic energy spreads small suspended particles throughout the cytoplasm of the cell | 78 | |
| 6650022981 | colligative property | A property of a solution that depends on the number, not the identity, of the solute particles. | 79 | |
| 6650022982 | concentrated | Describes a solution that has a relatively large amount of dissolved solute | 80 | |
| 6650023325 | critical pressure | the lowest pressure at which the substance can exist as a liquid at the critical temperature | 81 | |
| 6650023806 | critical temperature | the temperature above which the substance cannot exist in the liquid state | 82 | |
| 6650024569 | crystal | An orderly, three-dimensional pattern of ions or atoms in a solid | 83 | |
| 6650024845 | deliquescent | compounds that remove sufficient water from the air to dissolve completely and form solutions | 84 | |
| 6650024846 | dilute | to lessen the concentration, force, or purity of by adding something | 85 | |
| 6650025555 | dynamic equilibrium | Result of diffusion where there is continuous movement of particles but no overall change in concentration | 86 | |
| 6650026102 | endothermic | A chemical reaction that absorbs energy (heat) | 87 | |
| 6650026527 | efflorescent | hydrated crystals that lose the water of hydration on exposure to air at ordinary temperatures | 88 | |
| 6650026847 | exothermic | A chemical reaction that releases energy (heat) | 89 | |
| 6650028696 | heat of fusion | Amount of energy required to change a substance from the solid phase to the liquid phase. | 90 | |
| 6650028697 | heat of vaporization | The amount of energy required for the liquid at its boiling point to become a gas | 91 | |
| 6650029172 | "heavy" water | water containing an elevated concentration of molecules with deuterium | 92 | |
| 6650029662 | deuterium | An isotope of hydrogen with one proton and one neutron in the nucleus having an atomic weight of 2.014 | 93 | |
| 6650030344 | hydrate | A compound that has a specific number of water molecules bound to its atoms | 94 | |
| 6650030896 | Le Chatelier's Principle | States that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress. | 95 | |
| 6650030897 | melting point | The temperature at which a solid becomes a liquid | 96 | |
| 6650031287 | miscible | Describes two liquids that are soluble in each other | 97 | |
| 6650031288 | immiscible | Liquid solutes and solvents that are not soluble in each other | 98 | |
| 6650031477 | molality | the concentration of a solution expressed in moles of solute per kilogram of solvent | 99 | |
| 6650031995 | molarity | A common measure of solute concentration, referring to the number of moles of solute per liter of solution. | 100 | |
| 6650031996 | mole fraction | The ratio of the moles of solute in solution to the total number of moles of both solvent and solute | 101 | |
| 6650032383 | normality | Gram equivalent weight of solute per liter of solution, often denoted by N. | 102 | |
| 6650032384 | phase equilibrium | when the rates of evaporation and condensation equalize | 103 | |
| 6650032887 | polarity | A lack of electrical symmetry in a molecule. Charge differences on opposite ends of a structure. | 104 | |
| 6650033121 | saturated | unable to dissolve any more solute | 105 | |
| 6650033434 | solute | A substance that is dissolved in a solution. | 106 | |
| 6650033435 | solvent | A liquid substance capable of dissolving other substances | 107 | |
| 6650033746 | specific gravity | Density of an object realtive to water. No units. | 108 | |
| 6650034165 | sublimation | A change directly from the solid to the gaseous state without becoming liquid | 109 | |
| 6650034446 | surface tension | 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 | 110 | |
| 6650034988 | temporary hardness | Temporary hardness is a type of water hardness caused by the presence of dissolved bicarbonate minerals (calcium bicarbonate and magnesium bicarbonate) | 111 | |
| 6650034989 | viscosity | A liquid's resistance to flowing | 112 | |
| 6650080779 | activation energy | the minimum amount of energy required to start a chemical reaction | 113 | |
| 6650080780 | catalyst | a substance that initiates or accelerates a chemical reaction without itself being affected | 114 | |
| 6650081865 | collision theory | atoms, ions, and molecules can react to form products when they collide, provided that the particles have enough kinetic energy | 115 | |
| 6650082891 | factors affecting reaction rates | temperature, concentration ,particle size, and the use of a catalyst | 116 | |
| 6650084106 | Law of Mass Action | The rate of a chemical reaction is proportional to the product of the concentrations of the reactants | 117 | |
| 6650084249 | reaction mechanism | a series of elementary reactions that take place during the course of a complex reaction | 118 | |
| 6650084804 | acid ionization constant | the value of the equilibrium constant expression for the ionization of a weak acid | 119 | |
| 6650084805 | common ion effect | a decrease in the solubility of an ionic compound caused by the addition of a common ion | 120 | |
| 6650085201 | enthalpy | The heat content of a system at constant pressure | 121 | |
| 6650085702 | entropy | A quantitative measure of disorder or randomness, symbolized by S. | 122 | |
| 6650086167 | equilibrium | A dynamic condition in which two opposing changes occur at equal rates in a closed system | 123 | |
| 6650087617 | equilibrium constant | the ratio of product concentrations to reactant concentrations at equilibrium, with each concentration raised to a power equal to the number of moles of that substance in the balanced chemical equation | 124 | |
| 6650088220 | free energy | Measures the portion of a system's energy that can perform work when temperature and pressure are uniform throughout the system, as in a living cell. | 125 | |
| 6650088758 | Gibbs free-energy equation | ΔG= ΔH(enthalpy)- TΔS(entropy) | 126 | |
| 6650089547 | solubility product constant | an equilibrium constant applied to the solubility of electrolytes; it is equal to the product of the concentrations of the ions each raised to a power equal to the coefficient of the ion in the dissociation equation | 127 | |
| 6650090633 | acid | A substance that increases the hydrogen ion concentration of a solution. | 128 | |
| 6650090642 | amphoteric | a substance that can act as both an acid and a base | 129 | |
| 6650090805 | base | A substance that decreases the hydrogen ion concentration in a solution. | 130 | |
| 6650091025 | buffer solution | A solution made from a weak acid and its conjugate base that neutralizes small amounts of acids or bases added to it | 131 | |
| 6650091352 | conjugate acid | the particle formed when a base gains a hydrogen ion | 132 | |
| 6650092115 | Arrhenius Theory | acids are characterized by their sour taste, low Ph, and the fact that they turn litmus red. Bases are characterized by their bitter taste, slippery feel, high pH, and the fact that they turn litmus paper blue | 133 | |
| 6650092859 | conjugate base | particle that remains when an acid has donated a hydrogen ion | 134 | |
| 6650093074 | end point | the point in a titration at which the indicator changes color | 135 | |
| 6650093415 | equivalence point | the point at which the two solutions used in a titration are present in chemically equivalent amounts | 136 | |
| 6650093416 | indicator | A compound that changes color in the presence of an acid or a base | 137 | |
| 6650094196 | litmus | an indicator paper that turns red in an acid and blue in a base | 138 | |
| 6650094685 | Bronsted-Lowery Theory | Defines acids as proton donors and bases as proton acceptors; recognizes that acids and bases do not need to exist in aqueous (water) solutions; explains how acids and bases react to neutralize each other and produce water and salts when combined | 139 | |
| 6650094808 | neutralization | A reaction of an acid with a base, yielding a solution that is not as acidic or basic as the starting solutions were. | 140 | |
| 6650095326 | pH | a numeric scale used to specify the acidity or basicity of an aqueous solution | 141 | |
| 6650096224 | salt | An ionic compound made from the neutralization of an acid with a base. | 142 | |
| 6650096787 | titration | a measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete | 143 | |
| 6650097094 | volumetric analysis | a technique for determining the amount of a certain substance by doing a titration. | 144 | |
| 6650097629 | Lewis Theory | An acid is defined as an electron pair acceptor (e.g. BF3) and a base is an electron donator (e.g. NH3). | 145 | |
| 6650099243 | anions | Negatively charged ions | 146 | |
| 6650099795 | burning | a type of oxidation reaction | 147 | |
| 6650100758 | cations | Positively charged ions | 148 | |
| 6650101178 | combustion | A rapid reaction between oxygen and fuel that results in fire | 149 | |
| 6650101179 | dissociation | the separation of ions that occurs when an ionic compound dissolves | 150 | |
| 6650101550 | ionization | Process in which electrolytes dissolve in water and separate into charged particles | 151 | |
| 6650101862 | natural gas | A gas with high methane content, found along with various fossil fuels and is used as a fuel. | 152 | |
| 6650102141 | oxidation | A chemical change in which a substance combines with oxygen, as when iron oxidizes, forming rust | 153 | |
| 6650102142 | oxidation states | A concept that provides a way to keep track of electrons in oxidation-reduction reactions according to certain rules | 154 | |
| 6650102677 | oxidizing agent | the substance that oxidizes another substance by accepting its electrons | 155 | |
| 6650103151 | redox | The chemical reasction in which the oxidizing agent is reduced and the reducing agent is oxidized is | 156 | |
| 6650103408 | reducing agent | the substance that reduces another substance by losing electrons | 157 | |
| 6650103757 | reduction | Any process in which electrons are added to an atom or ion (as by removing oxygen or adding hydrogen) | 158 | |
| 6650104544 | acid salt | a salt formed by replacing part of the hydrogen ions of a dibasic or tribasic acid with metallic ions | 159 | |
| 6650104545 | allotropic form | Forms of the same element that differ in their crystalline structures. | 160 | |
| 6650105137 | basic oxygen furnace | Molten pig iron is injected with supersonic oxygen blast | 161 | |
| 6650105895 | blast furnance | How are metals proced | 162 | |
| 6650105896 | brass | An alloy of copper and zinc. | 163 | |
| 6650106267 | bronze | Copper and tin | 164 | |
| 6650106268 | electric arc furnace | enormous amounts of electricity generated through graphite cathodes that are lowered into the molten iron to purify it and produce a high grade of steel | 165 | |
| 6650107648 | metaloid | Demonstrate properties of both metals and nonmetals. Examples are silicon and arsenic. | 166 | |
| 6650108068 | normal salt | A salt in which all the hydrogen of the acid has been displaced by a metal. | 167 | |
| 6650108069 | open-hearth furnace | large oven with a disk-shaped area, alternating blasts of flame are directed across the surface of the melted metal until the proper proportions of additives are established for that "heat" | 168 | |
| 6650108381 | pig iron | iron that had not had its impurities removed | 169 | |
| 6650109386 | rhombic | Crystal structure of sulfur - heated in mineral oil to dissolve | 170 | |
| 6650109387 | monoclinic | Mineral with three planes of cleavage, two are perpendicular, the third is not | 171 | |
| 6650110220 | amorphous | shapeless, without definite form; of no particular type or character; without organization, unity, or cohesion | 172 | |
| 6650110724 | semiconductor | A substance that can conduct electricity under some conditions | 173 | |
| 6650111822 | alcohol | An organic compound with a hydroxyl group attached to one of its carbon atoms. | 174 | |
| 6650112124 | aldehyde | An organic molecule with a carbonyl group located at the end of the carbon skeleton. | 175 | |
| 6650112125 | alkane | a hydrocarbon containing only single covalent bonds | 176 | |
| 6650112529 | alkene | A hydrocarbon that contains a double bond. | 177 | |
| 6650112884 | alkyl groups | Groups of atoms that are formed when one hydrogen atom is removed from an alkane molecule | 178 | |
| 6650112885 | alkyne | a carbon compound with a carbon-carbon triple bond. | 179 | |
| 6650113237 | amine | organic compounds that contain only hydrogen, carbon , and nitrogen | 180 | |
| 6650113481 | amino acid | The building blocks of proteins | 181 | |
| 6650113482 | aromatics | Certain unsaturated cyclic compounds. High stability. Every carbon bond has intermediate single doublr bonds | 182 | |
| 6650114032 | diamond | carbon arranged in a crystal lattice | 183 | |
| 6650114377 | ester | an organic compound made by chemically combining an alcohol and an organic acid | 184 | |
| 6650114378 | ether | n oxygen atom connected to two alkyl or aryl groups | 185 | |
| 6650115619 | fullerene | a form of carbon that consists of atoms arranged in the shape of a hollow sphere | 186 | |
| 6650115796 | functional groups | chemical groups attached to carbon skeletons that give compounds their functionality | 187 | |
| 6650116845 | hydrocarbon | Compounds composed of only carbon and hydrogen | 188 | |
| 6650117168 | hydrogenation | The process of converting unsaturated fats to saturated fats by adding hydrogen | 189 | |
| 6650117876 | isomer | Compounds with the same formula but different structures. | 190 | |
| 6650117877 | ketone | An organic compound with a carbonyl group of which the carbon atom is bonded to two other carbons. | 191 | |
| 6650119752 | photosynthesis | Conversion of light energy from the sun into chemical energy. | 192 | |
| 6650120132 | saturated hydrocarbon | A hydrocarbon in which all the bonds between carbon atoms are single bonds | 193 | |
| 6650120804 | unsaturated hydrocarbon | A hydrocarbon in which one or more of the bonds between carbon atoms is double or triple | 194 | |
| 6650122352 | gravimetric balance | direct readings to thousandths of a gram instead of a triple-beam balance | 195 | |
| 6650122876 | pH meters | Electronic instruments: sensor responds to Hydronium ions by producing a current | 196 | |
| 6650122877 | salt bridge | A tube that allows the slow transfer of ions and maintains the neutrality of the electrolyte solutions. | 197 | |
| 6650123135 | spectrophotometer | An instrument that measures the proportions of light of different wavelengths absorbed and transmitted by a pigment solution. | 198 |
