Chemistry, the Central Science 13th edition chapters 1-8: SUNY CHEMISTRY MIDTERM VOCAB Flashcards
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| 12264367059 | Formula Weight | The sum of the atomic weights of the atoms in the chemical formula of the substance. | 0 | |
| 12264370986 | Molecular weight | What the formula weight is called if the chemical formula is that of a molecule. | 1 | |
| 12264383405 | Percentage composition (elemental composition) | The percentage by mass contributed by each element in the substance. | 2 | |
| 12264385677 | Mole (mol) | The counting unit for numbers of atoms, ions, or molecules in a laboratory-size sample. (6.02 x 10 to the 23 power objects per one mole). | 3 | |
| 12264393857 | Percent yield | (actual yield/theoretical yield) x 100 | 4 | |
| 12264396774 | Actual yield | The amount of product actually obtained (always less than the theoretical yield). | 5 | |
| 12264398018 | Mass spectrometer | The most accurate tool used for determining atomic weight. (CI atoms are introduced at one end of the tube, and are ionized to form CI+ ions. They are then directed through a magnetic field and the paths of the ions of the 2 CI isotopes diverge as they pass through). | 6 | |
| 12264405375 | Periodic table | The arrangement of elements in order of increasing atomic number, with elements having similar properties placed in vertical columns. | 7 | |
| 12264408854 | Periods | The horizontal rows on the periodic table. | 8 | |
| 12264411194 | Groups | The vertical columns on the periodic table (elements in a group have similar properties). | 9 | |
| 12264413318 | Metallic elements (metals) | All the elements (except hydrogen) on the left or in the middle of the periodic table. All of these elements share common characteristics (luster, high electrical and heat conductivity, all except mercury are solid at room temp.). | 10 | |
| 12264420947 | Nonmetallic elements (nonmetals) | Elements that are to the right of the periodic table. Nonmetals have different physical properties than metals, and are separated from them on the periodic table by a stepped line. | 11 | |
| 12264424858 | Metalloids | Elements that lie along the line that separates metals and nonmetals on the periodic table, and have properties that fall between those of metals and nonmetals. | 12 | |
| 12264429225 | Chemical formula | The formula of a molecule. Subscript in a chemical formula tells us how many atoms are in an element or molecule. | 13 | |
| 12264430878 | Molecular compounds | Compounds composed of molecules and contain more than one type of atom. | 14 | |
| 12264434373 | Molecular formula | A chemical formula that indicates the actual number of atoms in a molecule. | 15 | |
| 12264436015 | Empirical formula | Chemical formulas that only give the relative number of atoms of each type of molecule. | 16 | |
| 12264438287 | Structural formula | Shows which atoms are attached to which, with atoms being represented by their chemical symbols and bonds being represented by lines. | 17 | |
| 12264441757 | Ball-and-stick models | A structural formula model that shows atoms as spheres and bonds as sticks. | 18 | |
| 12264442539 | Space filling model | A structural formula model that depicts what a molecule would look like if the atoms were scaled up in size. | 19 | |
| 12264447122 | Ion | A charged particle formed when electrons are added or removed from an atom. | 20 | |
| 12264450131 | Cation | A positively charged ion. | 21 | |
| 12264450132 | Anion | A negatively charged ion | 22 | |
| 12264451531 | Noble gases | Chemically nonreactive elements that form very few compounds. Noble gases have a stable octet. | 23 | |
| 12264453634 | Ionic compound | A compound made up on cations and anions. | 24 | |
| 12264455763 | Chemical nomenclature | The system used in naming substances. | 25 | |
| 12264457386 | Components | The substances that make up a mixture. | 26 | |
| 12264458282 | Physical property | A property that can be observed without changing the identity and composition of a substance. | 27 | |
| 12264460175 | Scientific law | A statement that predicts or summarizes different natural phenomena. | 28 | |
| 12264462016 | Derived unit | A unit that is obtained by multiplying or dividing one or more base units. | 29 | |
| 12264464946 | Conversion factor | A fraction whose numerator and denominator are the same quantity expressed in different units. | 30 | |
| 12264466573 | The Celsius scale | A temperature scale commonly used in science based on 0 degrees Celsius being the freezing point of water and 100 degrees Celsius being the boiling point of water. | 31 | |
| 12264470892 | The Kelvin scale | The SI temperature scale whose unit of temperature is the kelvin. Zero on the kelvin scale is the absolute lowest temperature possible. | 32 | |
| 12264486561 | Atoms | Building blocks of matter. | 33 | |
| 12264488902 | Chemistry | The study of matter and the changes that matter undergoes. | 34 | |
| 12264490734 | Law of Conservation of Mass | The total mass of materials present after a chemical reaction is the same as the total mass before the chemical reaction. | 35 | |
| 12264495086 | Law of Multiple Proportions | If two elements A and B combine to form more than one compound, the masses of B that can combine with a given mass of A are in the ratios of small whole numbers. | 36 | |
| 12264500026 | Subatomic particles | Protons, neutrons, and electrons | 37 | |
| 12264501573 | Aqueous solution | A solution in which water is the dissolving medium. | 38 | |
| 12264504948 | Solvent | The substance present in the greatest quantity of a solution. | 39 | |
| 12264506557 | Electrolyte | A substance whose aqueous solution contains ions. | 40 | |
| 12264507977 | Nonelectrolyte | A substance that does not form ions in solution. | 41 | |
| 12264510425 | Strong electrolytes | Solutes that exist in a solution nearly or completely as ions. | 42 | |
| 12264511805 | Weak electrolytes | Solutes that exist in solution mainly as ions. | 43 | |
| 12264546280 | Chemical equilibrium | A balance of two opposing processes in which the relative numbers of each type of ion or molecule in the reaction are constant over time. | 44 | |
| 12264549320 | Precipitation reactions | Reactions that result in the formation of an insoluble product (precipitate). | 45 | |
| 12264550696 | Precipitate | An insoluble solid formed by a reaction in a solution. | 46 | |
| 12264553095 | Metathesis reactions (exchange reactions) | Reactions in which cations and anions appear to exchange partners. | 47 | |
| 12264556060 | Molecular equation | An equation written in a fashion that shows the complete chemical formulas of reactants and products. | 48 | |
| 12264558609 | Complete ionic equations | Equations written with all soluble strong electrolytes shown as ions. | 49 | |
| 12264560944 | Organic compounds | Compounds that contain carbon and hydrogen. | 50 | |
| 12264563163 | Inorganic compounds | Compounds that do not contain carbon and hydrogen. | 51 | |
| 12264566267 | Transition metals | Elements that occur in the middle of the periodic table, from group 3B to group 2B. - Form cations with different charges. | 52 | |
| 12264568176 | Oxyanions | Polyatomic anions containing oxygen and have names ending in either -ate or -ite. | 53 | |
| 12264571206 | Acid | A substance whose molecules yield hydrogen ions when dissolved in water. | 54 | |
| 12264588241 | Organic chemistry | The study of compounds of carbon and hydrogen. | 55 | |
| 12264590742 | Hydrocarbons | Compounds that contain carbon and hydrogen. | 56 | |
| 12264590802 | Alkanes | The simplest class of hydrocarbons, in which each carbon is bonded to four other atoms. | 57 | |
| 12264594966 | Functional groups | Specific groups of atoms. | 58 | |
| 12264595878 | Alcohol | Obtained by replacing an H atom of an alkane with an -OH group. > Name derived by adding an -ol ending to the name of the alkane. | 59 | |
| 12264597837 | Solid | A substance that has both a definite shape and a definitive volume. | 60 | |
| 12264600046 | Chemical equation | What a chemical reaction is represented by. | 61 | |
| 12264664831 | Reactants | The substances changed during a chemical reaction. | 62 | |
| 12264668330 | Combination reactions | When two or more substances react to form one product. | 63 | |
| 12264670407 | Decomposition reaction | When a single reactant breaks apart to form two or more substances. | 64 | |
| 12264671537 | Isomers | Compounds with the same molecular formula but different structures. | 65 | |
| 12264672761 | Structural isomers | Compounds that have the same molecular formulas but different structural formulas. | 66 | |
| 12264675047 | Stoichiometry | The area of study that examines the quantities of substances consumed and produced in chemical reactions. | 67 | |
| 12264680249 | Extensive property | A property that depends on the amount of sample being examined. | 68 | |
| 12264681191 | Intensive property | A property that does not change with the amount of sample being examined and can be used to identify the substance. | 69 | |
| 12264684887 | Mixture | A combination of two or more substances, in which each substance retains its chemical identity. | 70 | |
| 12264688919 | Gas (vapor) | A substance that has no fixed volume or shape, and perfectly fits its container. > Can be compressed or expanded to fit a certain volume. | 71 | |
| 12264692148 | Elements | A substance consisting of atoms of the same atomic number. > A substance that cannot be chemically separated into simpler substances. | 72 | |
| 12264696463 | Property | A trait, or several traits, of a type of matter that makes it distinguishable from other types of matter. | 73 | |
| 12264700272 | Law of Constant Composition (law of definite proportions) | The observation that the elemental composition of a compound is always the same. | 74 | |
| 12264703209 | Molecule | Two or more atoms joined in a specific shape. | 75 | |
| 12264704628 | Limiting reactant | The reaction that is completely consumed in a chemical reaction and limits the amount of product formed. | 76 | |
| 12264709116 | Excess reactant | The reactant that is left over after the reaction is complete. | 77 | |
| 12264711252 | Theoretical yield | The quantity of product calculated to form when all of a limiting reactant is consumed. | 78 | |
| 12264712826 | Equivalence point | The point at which the two solutions used in a titration are present in chemically equivalent amounts. | 79 | |
| 12265965683 | Combustion reaction | A rapid reaction that produces a flame. > The reaction of a substance with oxygen in which hydrogen and carbon dioxide are produced. | 80 | |
| 12265969016 | Oxidation reaction | A chemical reaction in which a reactant loses one or more electrons such that the reactant becomes more positive in charge | 81 | |
| 12265970612 | Electron | A negatively charged subatomic particle. | 82 | |
| 12265971814 | Dilution | The process by which solutions of lower concentrations are obtained by adding water. | 83 | |
| 12265974886 | Molarity (M) | M= moles solute/volume of solution in liters | 84 | |
| 12265978330 | Concentration | The amount of solute dissolved in a given quantity of solvent or quantity of solution. | 85 | |
| 12265978909 | Monoprotic acids | Acids that yield one H+ per molecule of acid ex) HCl, HNO3 | 86 | |
| 12265980933 | Acids | Substances that ionize in aqueous solution to form hydrogen ions. | 87 | |
| 12265981769 | Net ionic equation | An equation that only includes ions and molecules directly involved in the reaction. | 88 | |
| 12265982692 | Active metals | The metals at the top of an activity series such as alkali metals and alkaline earths that are most easily oxidized. | 89 | |
| 12265985066 | Activity series | A list of metals arranged in order of decreasing ease of oxidation. | 90 | |
| 12265985631 | Displacement reaction | A reaction in which the ion in solution is displaced (or replaced) through the oxidation of an element. | 91 | |
| 12265988754 | Oxidation number (oxidation states) | A system devised to keep track of the gain or loss of electrons by a substance. | 92 | |
| 12265989264 | Reduction | The gain of electrons by a substance. | 93 | |
| 12265989809 | Oxidation | The loss of electrons by a substance. | 94 | |
| 12265990429 | Redox reaction | A reaction in which electrons are transferred from one reactant to another. | 95 | |
| 12265992494 | Weak bases | Bases that are weak electrolytes | 96 | |
| 12265993592 | Weak acids | Acids that are weak electrolytes | 97 | |
| 12265993978 | Strong bases | Bases that are strong electrolytes. | 98 | |
| 12265994684 | Strong acids | Acids that are strong electrolytes. | 99 | |
| 12265995600 | Bases (proton acceptors) | Substances that accept (react with) H+ ions. > Produce hydroxide ions when dissolved in water. | 100 | |
| 12265996788 | Diprotic acids | Acids that yield two H+ ions per molecule of acid. > Ionization occurs in two steps. | 101 | |
| 12265998497 | Noble metals | Metals at the bottom of the activity series that form compounds readily. | 102 | |
| 12266000312 | Spectator ions | Ions that appear in identical forms on both sides of a complete ionic equation. > No direct role in reaction. | 103 | |
| 12266001181 | Cathode rays | The radiation produced between electrodes when high voltage power is applied to electrodes through a glass tube pumped almost empty of air. - Originates at the negative electrode and travels to the positive electrode. - Causes materials to give off light. | 104 | |
| 12266003524 | Hypothesis | A tentative model to explain scientific observations. | 105 | |
| 12266004429 | Theory | A model that predicts what is going to come next and accounts for all available observations. | 106 | |
| 12266005714 | The Metric System | The units used for scientific measurement. | 107 | |
| 12266006198 | Distillation | A process that depends on the different abilities of substances to form gases. | 108 | |
| 12266007671 | Chemical reaction | When a substance is transformed into a chemically different substance. | 109 | |
| 12266008651 | Physical change | A change a substance undergoes that changes its appearance, but not its composition. | 110 | |
| 12266009409 | Liquid | A substance that has a distinct volume and takes the shape of its container. | 111 | |
| 12266010327 | Matter | Anything that has mass and takes up space. | 112 | |
| 12266011858 | Significant figures | All the digits that can be known precisely in a measurement, plus a last estimated digit. | 113 | |
| 12266012385 | Accuracy | How closely individual measurements agree with the correct value. | 114 | |
| 12266014210 | Precision | A measure of how closely individual measurements agree with each other. | 115 | |
| 12266015045 | Absolute zero | The absolute lowest temperature possible. > Zero Kelvin | 116 | |
| 12266016046 | Compounds | Substances composed of two or more elements. | 117 | |
| 12266016643 | Pure substance | Matter that has distinct properties and a composition that does not vary from sample to sample. | 118 | |
| 12266018079 | Homogeneous mixture | A mixture in which substances are evenly distributed throughout the mixture. | 119 | |
| 12266018576 | Heterogeneous mixture | Mixtures that do not have the same composition throughout. | 120 | |
| 12266019460 | Atomic weight | The average atomic mass of an element. Atomic mass = (Σ/mass of element's isotopes) x relative abundance | 121 | |
| 12266025200 | Atomic Mass Unit (amu) | Defined by assigning a mass of exactly 12 amu to a chemically unbound atom of the 12C isotope of carbon. | 122 | |
| 12266026168 | Isotopes | Atoms with identical atomic numbers but different mass numbers (same number of protons but different number of electrons). | 123 | |
| 12266027680 | Mass number | The number of protons + neutrons in an atom. | 124 | |
| 12266028207 | Atomic number | The number of protons in an atom of any particular element. | 125 | |
| 12266029376 | Atomic mass unit | 1 amu = 1.66054 x 10^-24 | 126 | |
| 12266031150 | Angstrom | 10^-10 meters, the most convenient non-SI unit used for atomic dimensions. | 127 | |
| 12266034460 | Electronic charge | Quantity 1.602 x 10^-19 couloumbs | 128 | |
| 12266035416 | Neutron | A neutral subatomic particle that is found in the nucleus of an atom. | 129 | |
| 12266036513 | Proton | A subatomic particle that has a positive charge and that is found in the nucleus of an atom. | 130 | |
| 12266037024 | Nucleus | A very small, extremely dense region in which an atom and all of its positive charge resides. > Center of an atom. | 131 | |
| 12266039665 | Nuclear model | Model of the atom with a nucleus containing protons and neutrons and with electrons in the space outside the nucleus. - Ernest Rutherford created this model in the early 1900's. | 132 | |
| 12266042690 | Radioactivity | The spontaneous emission of radiation. | 133 | |
| 12266045376 | Titration | A process chemists carry out to determine the concentration of a particular solute in a solution. - Combine solution where solute concentration is not known with a standard solution. | 134 | |
| 12266048275 | Standard solution | A reactant of known concentration used in acid-base titration. | 135 | |
| 12266049834 | Avogadro's Number | 6.02 x 10^23 molecules = 1 mole | 136 | |
| 12266051802 | Molar mass | The mass in grams of one mole of a substance. | 137 | |
| 12266055112 | Thermodynamics | The study of energy and its transformations. | 138 | |
| 12266055670 | Thermochemistry | The transformations of energy during chemical reactions. | 139 | |
| 12266057648 | Kinetic energy | The energy due to the motion of an object. | 140 | |
| 12266058736 | Potential energy | The energy an object possesses by virtue of its position relative to other objects. | 141 | |
| 12266062426 | Joule | The SI unit of energy. 1 J = 1kg-m^2/s^2 | 142 | |
| 12266063839 | Calorie (cal) | The quantity of heat needed to raise the temperature of 1 g of pure water 1°C. 1 cal = 4.184 J | 143 | |
| 12266065046 | System | A specific portion of matter in a given region of space that has been selected for study during an experiment or observation. | 144 | |
| 12266066798 | Surroundings | Everything outside the system. | 145 | |
| 12266067328 | Work | The energy expended to move an object against a force. | 146 | |
| 12266070609 | Heat | The energy transferred from a hotter object to a colder one. | 147 | |
| 12266071887 | Energy | The capacity to do work or transfer heat. | 148 | |
| 12266072803 | Internal energy | The sum of all the kinetic and potential energies of its component parts. | 149 | |
| 12266076581 | First law of thermodynamics | ΔE = q+w | 150 | |
| 12266079213 | Endothermic | The system absorbs heat from its surroundings. | 151 | |
| 12266079880 | Exothermic | The system releases heat to the surroundings. | 152 | |
| 12266080873 | State function | A value that depends only on the state or condition of the system and not on the details of how it came to be in that state. | 153 | |
| 12266083408 | Pressure-volume (P-V) work | The work associated with the expansion or compression of a gas. | 154 | |
| 12266084682 | Enthalpy | A state function related to energy. H = E + PV | 155 | |
| 12266087718 | ΔH | The heat gained or lost by the system at constant pressure. ΔH > 0 - Endothermic process ΔH < 0 - Exothermic process | 156 | |
| 12266094006 | Enthalpy of reaction | ΔHrxn = H(products)-H(reactants) | 157 | |
| 12266126643 | Calorimetry | The measurement of the heat transferred between the system and the surroundings. | 158 | |
| 12266128062 | Calorimeter | An insulated device used to measure the absorption or release of heat in chemical or physical processes. | 159 | |
| 12266129380 | Heat capacity | The heat capacity required to raise the temperature of a calorimeter by 1 K. | 160 | |
| 12266132754 | Molar heat capacity | The heat capacity of one mole of a pure substance. | 161 | |
| 12266135514 | Specific heat | The heat capacity of one gram of a pure substance. | 162 | |
| 12266139825 | q (the amount of heat absorbed by a substance) | MCΔT | 163 | |
| 12266143453 | Bomb calorimeter | A vessel of a fixed volume in which constant-volume calorimetry is carried out. | 164 | |
| 12266144871 | Coffee calorimeter | A vessel of a fixed pressure in which constant-pressure calorimetry is carried out. | 165 | |
| 12266149546 | Hess's Law | If a reaction is carried out in a series of steps, ΔH for the reaction will be equal to the sum of the enthalpy changes for the steps. | 166 | |
| 12266152294 | Enthalpy of formation (ΔH°f) | The enthalpy change for the reaction in which the substance is formed from its constituent elements. | 167 | |
| 12266156949 | Standard state | The pure, most stable form of a substance at 1 atm and the temperature of interest. | 168 | |
| 12266163408 | Standard enthalpy change | ΔH°rxn = ΣnΔH°f (products) - ΣmΔH°f (reactants) | 169 | |
| 12269101254 | Electronic structure of an atom | Describes the energies and arrangement of electrons around the atom. | 170 | |
| 12269105537 | Electromagnetic radiation (radiant energy) | Energy waves that travel at the speed of light. | 171 | |
| 12269109328 | Wavelength | Horizontal distance between the crests or between the troughs of two adjacent waves. - Represented by λ (lambda). - Unit is m (or one of its derived units). | 172 | |
| 12269124244 | Frequency | The number of complete wavelengths that pass a point in a given time. - Represented by v - Unit is s^-1 (or hz, s^-1 = hz). | 173 | |
| 12269138928 | Interrelation of wavelength, frequency, and the speed of light | c= λv | 174 | |
| 12269142533 | Quantum of energy | The minimum quantity of energy that can be lost or gained by an atom. | 175 | |
| 12269144830 | E = hv | The minimum amount of radiant energy that an object can gain or lose is related to the frequency of the radiation. | 176 | |
| 12269182468 | Planck's Constant | h = 6.626 x 10^-34 J-s | 177 | |
| 12269186481 | Photoelectric effect | The emission of electrons from metal surfaces when exposed to light. | 178 | |
| 12269191362 | Photons | Packets of quantized energy. - Each photon carries energy, E = hv | 179 | |
| 12269195425 | Spectrum | Something that is created when radiation is dispersed into its component wavelengths. | 180 | |
| 12269199530 | Continuous spectrum | A spectrum that contains all wavelengths. | 181 | |
| 12269201864 | Line spectrum | A spectrum that contains only certain wavelengths. | 182 | |
| 12269207013 | Principal quantum number | Symbolized by n, indicates the main energy level occupied by the electron. - The value of n must be a positive integer. - Energy of the atom increases as n increases. | 183 | |
| 12269214139 | Ground state | The lowest energy state of an atom. > n = 1 | 184 | |
| 12269217814 | Excited states | A higher energy state than the ground state. - Light is emitted when the electron drops from a higher energy state to a lower energy state. | 185 | |
| 12269280735 | Matter waves | Matter, such as electrons, should exhibit wave-like properties. | 186 | |
| 12269284330 | Momentum | The product of an object's mass and velocity. | 187 | |
| 12269287725 | Uncertainty principle | There is an inherent limit to the accuracy with which the position and momentum of a particle can be measured simultaneously. | 188 | |
| 12269294591 | Wave functions | A mathematical description of an allowed energy state (an orbital) for an electron in the quantum mechanical model of the atom. - Denoted using the Greek letter ψ. | 189 | |
| 12269304798 | Probability density | A value that represents the probability that an electron will be found at a given point in space. - ψ^2 | 190 | |
| 12269310552 | Electron density distribution | A map of the probability of finding the electrons at all points in space. | 191 | |
| 12269314982 | Orbital | Described by a combination pf an integer and a letter, corresponding to the values of the three quantum numbers. | 192 | |
| 12269321941 | Angular momentum quantum number (l) | Defines the shape of the orbital. - Indicated by the letters s, p, d , f, etc. - This corresponds to the values of 0, 1, 2, 3, etc. - For a given value of n, l can have integer values ranging from 0 to (n-1). | 193 | |
| 12269334252 | Magnetic quantum number (m sub l) | Relates to the orientation of the orbital in space. - For a given value of l, m sub l can have integral values ranging from -l to l, including 0. - Subscripts can be used to label the orientation of the orbital. | 194 | |
| 12269390745 | Subshell | The set of one or more orbitals with the same n and l values. - Ex, 3s, 3p, 3d. | 195 | |
| 12269396899 | Radial probability function | The probability that the electron will be found a certain distance from the nucleus. | 196 | |
| 12269401917 | Nodes | Regions in which the wave function is 0. | 197 | |
| 12269403857 | Degenerate | Orbitals of the same energy. | 198 | |
| 12269408036 | Spin magnetic quantum number (m sub s) | The directions of an electron spinning about an axis. - Can have only two values; either -1/2 or +1/2 | 199 | |
| 12269415041 | Pauli Exclusion Principle | No two electrons in an atom can have the same values for n, l, m sub l, and m sub s. | 200 | |
| 12269420122 | Electron configuration | Describes how the electrons are distributed among the orbitals of an atom. | 201 | |
| 12269424168 | Orbital diagram | A diagram that shows the distribution of electrons in the orbitals of the energy levels. | 202 | |
| 12269427779 | Hund's Rule | The lowest energy is attained by maximizing the number of electrons with the same electron spin. | 203 | |
| 12269433115 | Valence electrons | The outer-shell electrons that are involved in chemical bonding. | 204 | |
| 12269436787 | Core electrons | The electrons that are not valence electrons. > Not involved in chemical bonding. | 205 | |
| 12269441093 | Representative (main group) elements | Elements in which the outermost subshell is an s or p subshell. | 206 | |
| 12269445777 | Transition elements (transition metals) | Elements in which a d subshell is being filled. | 207 | |
| 12269451549 | Lanthanide (rare earth) elements | Elements in which the 4f subshell is being filled. | 208 | |
| 12269453690 | Actinide elements | Elements in which the 5f subshell is being filled. | 209 | |
| 12269456895 | F-block metals | The lanthanide and actinide elements. | 210 | |
| 12269577427 | Valence orbitals | Orbitals that contain the outer-shell electrons of an atom. - Elements in the same column of the periodic table have the same number of electrons in their valence orbitals. | 211 | |
| 12269584457 | Effective nuclear charge (Zeff) | The charge that an electron experiences from the nucleus = to the nuclear charge, but is reduced from any shielding or screening from any inner shell electrons. - Increases as you go across a period. - Decreases as you go down a group. | 212 | |
| 12269605738 | Bonding atomic radius | One-half of the distance between covalently bonded nuclei. - Increases as you go down a group. - Decreases as you go across a period. | 213 | |
| 12269647681 | Isoelectronic series | A series of ions that have the same number of electrons. | 214 | |
| 12269681033 | Ionization energy | The minimum energy required to remove an electron from the atom in the gas phase, forming a cation. - First, second, third, etc ionization energies. - Increases as you move across a period. - Decreases as you go down a row. | 215 | |
| 12269697234 | Electron affinity | The energy change that occurs when an electron is added to an atom in the gas phase, creating an anion. - Negative electron affinity means that energy is released when the electron is added, so when the electron affinity is negative, the atom is stable. - Noble gases have positive electron affinities. | 216 | |
| 12269713539 | Metallic character | The tendency of metals to exhibit the properties of metals. - Increases as you go down a row. - Decreases as you go across a period. | 217 | |
| 12269736722 | Alkali metals (group 1A) | Soft metals with low densities and low melting points. | 218 | |
| 12269760696 | Alkaline earth metals (group 2A) | Harder, denser, and stronger than alkali metals, less reactive than alkali metals, but still too reactive to be found free in nature. | 219 | |
| 12269764503 | Halogens (group 7A) | Elements that exist as diatomic molecules. - Have the most negative electron affinities. | 220 | |
| 12269767202 | Noble gases (group 8A) | Elements that exist as monatomic gases. - Unreactive because they have completely filled s and p orbitals. | 221 |
