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Chemistry Term II
Chemistry vocabulary
| Term | Definition |
|---|---|
| Mole Ratio | The ratio of moles of a substance to the moles of another substance in a balanced equation using the coefficients |
| Stoichiometry | The relationship between the quantities of substances taking part in a reaction |
| Limiting Reactent | The reactant in a chemical equation that is present in the lesser amount, and is completely used up |
| Excess Reactant | The reactant that is left over |
| Theoretical Yield | The amount of product predicted from the amounts of reactants used |
| Actual Yield | The actual amount of product produced from the amounts of reactants used |
| % Yield | The actual yield of product divided by the theoretical yield multiplied by 100 |
| Photons | Wave packets of energy |
| Electromagnetic Radiation | When energy is transmitted from one place to another by light |
| Wavelength | Distance between wavecrests |
| Frequency | Number of waves passing by a given point per second |
| Ground State | Lowest energy level for electrons |
| Excited State | Electrons have absorbed energy |
| Electron Orbitals | Region of space around the nucleus of an atom within which there is a 90% probability of finding an electron |
| Principal Energy Level | The energy level denoted by n, each containing a different number of sublevels |
| Quantized | Only certain values are allowed in specific energy levels |
| Bohr Model of the Atom | Electrons orbit the nucleus at set distances |
| Wavelength Mechanical Model of the Atom | Electrons exist in atoms and determine the chemical and physical properties of elements |
| Electron Configuration | A way to display the location of all electrons in an element |
| Core Electrons | Electrons in the inner energy levels |
| Valence Electrons | Electrons in outer sublevel |
| Noble Gas Configuration | Shortcut for electron configuration |
| Ionization energy | The amount of energy required to remove an electron from a gaseous atom or ion |
| Atomic Size | Atoms get bigger as you go down a group, and smaller from left to right |
| 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 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 equally |
| 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 |
| 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 charger and a center of negative charge |
| Lewis Structure | A representation of a molecule or polyatomic ion showing how valence electrons are arranged among the atoms in the molecule |
| Resonance | A condition occuring when more than one valid Lewis Structure can be written for a particular molecule |
| Bent or V-Shape Structure | Two bonds and two unshared pairs on central atom |
| Linear Structure | Two double bonds on central atom |
| Trigonal Planar Structure | One double bond and two single bonds on a central atom |
| Trigonal Pyramid Structure | Three single bonds and an unshared pair on a central atom |
| Tetrahedral Structure | Four single bonds on a central atom |
| Valence Shell Electron Pair Repulsion Model | Model used to predict molecular geometry |
| Solution | Homogeneous mixture that doesn't settle |
| Alloy | Solid mixed with another solid |
| Aqueous Solution | Liquid solution in which water is the main component |
| Solvent | Component present in the largest amount |
| Solute | Component present in the lesser amount |
| Soaps and Detergents | Molecules with both polar and non-polar parts that 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 maximum amount of solute |
| Saturated | Maximum amount of solute is dissolved in solution |
| Supersaturated | More than maximum amount of solute is dissolved in solution |
| Solubility | Maximum number of grams of solute per 100 mL of water and a given temperature |
| Molarity | Concentration of solution (# of moles/volume |
| 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 (m1v1=m2v2) |
| Stock Solution | Beginning concentrated solution |
| Arrhenius Acid | Produces H+ in solution |
| Arrhenius Base | Produces OH+ in solution |
| Equivalent of an Acid | The amount of acid that can furnish one mole of hydrogen ions |
| Equivalent Weight | The mass of one equivalent of an acid or base |
| Normality | Number of equivalents per 1 L of solution |
| Colligative Property | Depends only on the number of solute particles present in the 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 |
| Bronsted-Lowery Acid | Proton Donor H+ |
| Bronsted-Lowery Base | Proton Accepter |
| Hydronium Ion | H3O+ ion formed when an 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 Pair | Two substances related to each other by the donating and accepting of a single proton |
| Oxyacid | An acid in which the acidic hydrogen is attached to an oxygen atom |
| Organic Acid | Acid with a carbon atom backbone |
| Amphoteric | A substance that can act as both an acid and a base (water) |
| pH | Scale used to specify the acidity or basicity of an aqueous solution |
| Indicators | Chemicals that change color depending on the pH of a solution in which they are placed |
| 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 known |
| Equivalence Point | The point in a titration when enough titrant has been added to react exactly with the substance in solution that is being titrated |
| Buffered Solution | A solution that resists a change in pH when either an acid or a base is added |
Created by:
emmakolden
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