Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Vocab Qtr 2
Chemistry Vcoab: 9, 11, 12, 15, 16
| Term | Definition |
|---|---|
| mole ratio | the ratio of moles of one substance to moles of another substance in a balanced chemical equation |
| stoichiometry | the process of using a balanced chemical equation to determine the relative masses of reactants and products involved in a reaction |
| limiting reactant | the reactant that is completely used up when a reaction is run to completion |
| theoretical yield | the maximum amount of a given product that can be formed when the limiting reactant is completely consumed |
| percent yield | the actual yield of a product as the percentage of the theoretical yield |
| electromagnetic radiation | radiant energy that exhibits wavelike behavior and travels through space at the speed of light in a vacuum |
| wavelength | the distance between two consecutive peaks or troughs in a wave |
| frequency | the number of waves (cycles) per second that pass a given point in space |
| photon | a particle of electromagnetic radiation |
| quantized | energy levels of hydrogen are quantized |
| orbital | the three dimensional region in which there is a high probability of finding an electron in an atom |
| principal energy levels | labeled with whole numbers, hydrogen atom |
| sublevels | the levels divided |
| Pauli exclusion principle | in a given atom, no two electrons can occupy the same atomic orbital and have the same spin |
| electron configuration | the arrangement of electrons in an atom |
| box diagram | where orbitals are represented by boxes grouped by sublevels with small arrows indicating the electrons |
| valence electrons | the electron in the outermost principal energy level of an atom |
| core electrons | an inner electron; an electron not in the outermost principal energy level of an atom |
| ionization energy | the amount of energy required to remove an electron from a gaseous atom or ion |
| bond (chemical bond) | the force that holds two or more atoms together and makes them function as a unit |
| bond energy | the energy required to break a given chemical bond |
| ionic bonding | the attraction between oppositely charged ions |
| ionic compound | a compound that results when a metal reacts with a nonmetal to form cations and anions |
| covalent bonding | a type of bonding in which atoms share electrons |
| polar covalent bond | a covalent bond in which the electrons are not shared equally because one atom attracts the shared electrons more than the other atom |
| electronegativity | the tendency of an atom in a molecule to attract shared electrons to itself |
| dipole moment | a property of a molecule in which the charge distribution can be represented by a center of positive charge and a center of a negative charge |
| Lewis structure | a representation of a molecule or polyatomic ion showing how valence electrons are arranged among the atoms in the molecule or ion |
| bonding pair | a pair of electrons that are shared between two atoms forming a covalent or polar-covalent bond |
| lone pair | electron pairs in a Lewis structure that are not involved in bonding |
| single bond | a covalent or polar covalent bond in which one pair of electrons is shared by two atoms |
| double bond | a covalent or polar covalent bond in which two pairs of electrons are shared by two atoms |
| triple bond | a covalent or polar covalent bond in which three pairs of electrons are shared by two atoms |
| resonance | a condition occurring when more than one valid Lewis structure can be written for a particular molecule |
| molecular structure | the three dimensional arrangement of atoms in a molecule |
| VSEPR model (valence shell electron pair repulsion) | a model used to predict molecular geometry, based on the idea that pairs electrons surrounding an atom repel each other and that the atoms in a molecule are positioned to minimize this repulsion |
| solution | a homogenous mixture |
| solvent | the dissolving medium in a solution |
| solute | the substance dissolved in the solvent to make a solution |
| aqueous solution | a solution with water as a solvent |
| saturated | describes a solution that contains as much solute as will dissolve at that temperature |
| unsaturated | describes a solution in which more solute can dissolve than is dissolved already at that temperature |
| supersaturated | describes a solution that contains more solute than a saturated solution will hold at that temperature |
| concentrated | describes a solution in which a relatively large amount of solute is dissolved in a solution |
| dilute | describes a solution in which a relatively small amount of solute is dissolved in a solution |
| standard solution | a solution in which the concentration is accurately known |
| dilution | the process of adding solvent to a solution to lower the concentration of solute |
| neutralization reaction | an acid-base reaction |
| equivalent of an acid | the amount of acid that can furnish one mole of hydrogen ions (H+) |
| equivalent of a base | the amount of base that can furnish one mole of hydroxide ions (OH-) |
| equivalent weight | the mass (in grams) of one equivalent of an acid or base |
| normality | is defined as the number of equivalents of solute per liter of solution |
| colligative property | a property that is dependent only on the number of solute particles present in solution |
| Arrhenius concept of acids and bases | acids produce hydrogen ions and bases produce hydroxide ions |
| conjugate acid | the substance formed when a proton is added to a base |
| conjugate base | the remaining substance when a proton is lost from an acid |
| conjugate acid-base paid | two substances related to each other bu the donating and accepting of a single proton |
| hydronium ion | H 3 O + |
| strong acid | an acid that completely dissociates to produce H+ ions in solution |
| weak acid | an acid that dissociates to a slight extent in aqueous solution |
| diprotic acid | an acid that can furnish two protons |
| oxyacid | an acid in which the acidic proton is attached to an oxygen atom |
| organic acid | an acid with a carbon atom backbone and a carboxyl group |
| amphoteric substance | a substance that can behave either as an acid or as a base |
| indicator (acid-base) | a chemical that changes color depending on the pH of a solution |
| indicator paper | a strip of paper coated with a combination of acid-base indicators |
| pH meter | a device used to measure the pH of a solution |
| neutralization reaction | an acid-base reaction |
| titration | a technique in which a solution of known concentration is used to determine the concentration of another solution |
| standard solution | a solution in which the concentration is accurately known |
| buret | a device used for the accurate measurement of the delivery of a given volume of a liquid or solution |
| equivalence point (stoichiometric point) | the point in a titration when enough titrant has been added to react exactly with the substance in solution that is being titrated |
| titration curve (pH curve) | a plot of pH of solution versus volume of titrant added to a given solution |
| buffered solution | a solution that resists a change in pH when either an acid or a base are added |
Created by:
briannaaa_vik
Popular Chemistry sets