AP Chemistry Practice

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Across
  1. 3. A solution that resists changes in pH when small amounts of acid or base are added.
  2. 6. Constant: A numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium.
  3. 8. A unit of mass used to express atomic and molecular weights, defined as one-twelfth the mass of a carbon-12 atom.
  4. 9. The point in a titration at which the amount of titrant added is exactly enough to react with the analyte in the solution.
  5. 11. The average distance between the nuclei of two bonded atoms.
  6. 13. Attractive forces between polar molecules with permanent dipoles.
  7. 14. A measure of the disorder or randomness in a system.
  8. 15. The smallest unit of matter that retains the identity of a chemical element.
  9. 16. A chemical reaction in which a single compound breaks down into two or more simpler substances.
  10. 17. A thermodynamic quantity representing the total heat content of a system.
  11. 18. Substances formed from two or more elements chemically bonded together.
  12. 21. The average distance from the center of an atom's nucleus to the outermost electron shell.
  13. 23. Describes a process that absorbs heat from its surroundings.
  14. 24. Negatively charged subatomic particles orbiting the nucleus of an atom.
  15. 26. Individual steps that make up a complex reaction mechanism.
  16. 27. A state in which the forward and reverse reactions occur at the same rate, and the concentrations of reactants and products remain constant.
  17. 32. Chemical bonds formed by the sharing of electron pairs between atoms.
  18. 33. Attractive forces between a polar molecule and a nonpolar molecule that has been temporarily polarized.
  19. 34. A technique for separating mixtures based on differences in the speed at which they move through a stationary phase.
  20. 35. The amount of energy required to break one mole of bonds in gaseous molecules.
Down
  1. 1. A substance that increases the rate of a chemical reaction without being consumed in the process.
  2. 2. Numbers placed before reactants and products in a chemical equation to balance it.
  3. 4. The simplest whole-number ratio of atoms in a compound.
  4. 5. The distribution of electrons in an atom's electron shells and subshells.
  5. 7. A theory stating that chemical reactions occur when reactant molecules collide with sufficient energy and proper orientation.
  6. 10. A measure of an atom's ability to attract and hold onto electrons in a chemical bond.
  7. 12. The science of measuring the heat of chemical reactions or physical changes.
  8. 19. A reaction involving two reactant molecules coming together to form products.
  9. 20. The principle that energy cannot be created or destroyed, only transformed.
  10. 22. A separation of electrical charges within a molecule, resulting in a molecule having a positive end and a negative end.
  11. 25. A process in which substances are transformed into different substances with different properties.
  12. 28. The minimum amount of energy required for a chemical reaction to occur.
  13. 29. The ability of a material to conduct electricity.
  14. 30. The process of reducing the concentration of a solute in a solution, usually by adding more solvent.
  15. 31. The process by which one substance takes in or soaks up another substance.