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Chemistry Ch.9-16
| Term | Definition |
|---|---|
| stoichiometry | process of using a balanced chemical equation to determine the relative masses of reactants and products in a reaction |
| limiting reactant | runs out first |
| excess reactant | isn't fully used up |
| theoretical yield | max amount of a product that can be formed when the limiting reactant is completely consumed |
| actual yield | amount of product recovered in a reaction (most often less than theoretical yield) |
| percent yield | percent of theoretical yield recovered in a chemical reaction %yield=actual yield/theoretical yieldX100 |
| wave length | distance between wave crests |
| frequency | number of waves passing per second |
| velocity | all electromagnetic waves travel at the same speed |
| ground state | lowest energy level for electrons |
| excited state | electrons have absorbed energy |
| electron orbital | region of space around a nucleus where there is a 90% chance of finding an electron |
| principal energy level | -each level has different # of sublevels -each sublevel is a different region of space(s,d,p,f) |
| orbital | specific region of space inside a sublevel -up to 2 electrons in each orbital -each electron must have an opposite spin |
| electron configuration | a way to display the location of all electrons in an element (look at electron config. periodic table) (Ex. Li: 1s^2, 2s^1) |
| core electrons | electrons in inner levels |
| valence electrons | electrons in outer sublevel |
| noble gas configuration | shortcut for electron config. (Ex. Li: [He] 2s^1) |
| activeness of atoms | -most chemically active metals=lower left -most chemically active nonmetals=upper right(except noble gasses) -properties of metalloids=between metals+nonmetals |
| size of atoms | big atoms->small atoms, small atoms V big atoms |
| ionization energy | amount of energy required to remove an electron from a gaseous atom or ion |
| bond | force that holds 2+ atoms together and makes them function as a unit |
| bond energy | energy required to break a chemical bond |
| ionic bonding | attraction between oppositely charged ions |
| ionic compound | compound results when a metal reacts with a nonmetal to form cations and anions |
| covalent bonding | atoms share electrons |
| polar covalent bond | electrons are not shared equally because 1 atoms attracts shared electrons more than the other atom |
| electronegativity | tendency of an atom in a molecule to attract shared electrons to itself |
| electronegativity on period table | -increases left to right -decreases when going down a group |
| bonds depended on electronegativity | -very similar=very little polarity bond -very different=very polar bond -difference>2.0=ionic bond |
| dipole moment | property of a molecule in which the charge distribution can be represented by a center of positive charge and a center of negative charge |
| charges on ions | -gr. 1 metals=1+ cations -gr. 2 metals=2+ cations -aluminum in group 3A=3+ cation -gr.7A=1- anions -gr. 6A=2- anions |
| anions and cations | anions are negative and are larger cations are positive and are smaller |
| lewis structure | representation of a molecule or polyatomic ion showing how valence electrons are arranged among the atoms in the molecule or ion (only valance electrons are included) |
| duet rule | H and He both need 2 valance electrons to fill the first level |
| octet rule | most atoms must have 8 valance electrons to be stable |
| bonding pair | pair of electrons that are shared |
| lone pair(unshared pair) | pair of electrons that aren't shared |
| single bond | 1 pair of electrons are shared by 2 atoms |
| double bond | 2 pairs of electrons are shared by 2 atoms |
| triple bond | 3 pairs of electrons are shared by 2 atoms |
| resonance | condition occurring when more than 1 valid lewis structure can be written for a particular molecule |
| molecular structure(geometric structure) | 3-D arrangement of atoms in a molecule |
| bent or V-shape structure | 2 bonds and 2 unshaired pairs on central atom(could also be double bond, single bond, and 1 unshaired pair) |
| linear structure | 2 double bonds on central atom (or only 2 atoms in molecule) |
| trigonal pyramid structure | 3 single bonds and an unshaired pair or central atom |
| tetrahedral structure | 4 single bonds on central atom |
| valence shell electron pair repulsion(VSEPR) model | model used to predict molecular geometry -the structure around a given atom is determined by minimizing repulsions between electron pairs |
| solution | homogeneous solution that doesn't settle |
| alloy | solid mixed with another solid |
| liquid solution | solid, liquid, or gas mixed in with another liquid |
| gaseous solution | solid, liquid, or gas mixed in with a gas |
| aqueous solution | liquid solution in which water is the main component(most common) |
| solvent | component present in largest amount |
| solute | component present in lesser amount |
| ionic | seperates into ions in solution |
| polar | creates hydrogen bonds with other molecules and ions |
| non-polar | no molecular interaction between molecules |
| what dissolves in polar and non-polar | LIKE DISSOLVES LIKE |
| soaps and detergents | huge molecules with both polar and non-polar parts-can dissolve in both polar and non-polar solvents |
| dilute | relatively small amount of solute in mixture |
| concentrated | relatively large amount of solute |
| unsaturated | less than max amount of solute is dissolved in solution |
| saturated | max amount of solute is dissolved in solution |
| supersaturated | more than max amount of solute is dissolved in a solution -made by heating a saturated solution and adding more solute |
| solubility | max number of grams of solute per 100g or 100mL fo water at a given temperature |
| solids in liquids rate of dissolving | -agitation: increases -temperature: usually increases -increasing surface area: increases |
| gases in liquids rate of dissolving | -agitation: decreases -temperature: decreases -increasing in pressure: increases |
| % composition by volume | (Vsolute/Vsolution)X100 |
| % composition by mass | (MASSsolute/MASSsolution)X100 |
| molarity | concentration of solution involving moles -molarity=(MOLESsolute/VOLUMEsolution) |
| standard solution | solution in which the concentration is accurately known |
| dilution | process of adding solvent to a solution to lower the concentration of solute |
| stock solution | beginning concentrated solution -more solvent=lower concentration(but total solute remains constant) |
| dilution equation | M1V1=M2V2 |
| neutralization reaction | acid-base reaction |
| acid | produces H+ ions in a solution |
| base | produces OH- ions in a solution |
| STRONG acid or base | completely dissociates in a solution |
| acid in water | HA->H+ + A- |
| base in water | (A)OH-> A+ + OH- |
| net ionic equation | for neutralization: H+ + OH- = H2O |
| equivalent of an acid | amount of acid that can furnish one mole of hydrogen ions |
| equivalent of a base | amount of base that can furnish one mole of hydroxide ions |
| equivalent weight | mass(g) of one equivalent of an acid or base |
| normality | # of equivalents per 1L solution |
| Equilibrium | NaVa=NbVb |
| colligative property | property that is dependent only on the # of solute particles present in solution |
| freezing point depression | adding more solute to a solution will lower the freezing point of the solution |
| boiling point elevation | adding more solute to a solution will increase the boiling point of the solution |
| arrhenius model | Acid-produce H= ions Base-produce OH- ions (more restrictive model) |
| bronsted-lowry model | Acid-proton donor(H+) Base-proton acceptor(can be hydroxide, but also NH3) |
| hydronium ion | H3O+ ion formed when a acid is added to water |
| conjugate acid | substance formed when a proton is added to a base |
| conjugate base | remaining substance when a proton is lost from an acid |
| conjugate acid-base pairs | 2 substances related to each other by the donating + accepting of a single proton |
| change of charges in conjugates | conjugate base: charge= -1 from original conjugate acid: charge= +1 from original |
| oxyacid | acid in which the acidic hydrogen is attached to an oxygen atom |
| organic acid | acid with a carbon atom backbone(usually weak) |
| amphoteric | substance that can act as both an acid and a base(water) |
| ion-product constant | Kw=[H+][OH-]=1.0 X 10^-14 |
| pH equation | Ph=-log[H+] |
| pOH equation | pOH=-log[OH-] |
| what does pH + pOH equal | 14 |
| indicators | chemicals that change color depending on the pH of a solution in which they are placed |
| titration | technique in which a solution of known concentration is used to determine the concentration of another solution |
| standard solution | concentration is accurately known |
| buret | device used for the accurate measurement of delivery of a given volume of liquid or solution |
| equivalence point(stoichiometric point) | the point in a titration when enough titrant has been added to react exactly with the substance that is being titrated |
| titration curve | plot of pH of solution verses volume of titrant added to a given solution |
| titration equation | NaVa=NbVb |
| buffered solution | solution that resists a change in pH when either an acid or base are added (consist of weak acid and it's conjugate base mixed together) |
Created by:
kaylee.baker
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