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CLEP Chemistry 1

Subjects : clep, science, chemistry
  • Answer 50 questions in 15 minutes.
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  • Match each statement with the correct term.
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This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.
1. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.

2. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.

3. The _____ speed up the rate of a chemical reaction but do not change the equilibrium constant - it simply speeds up the rate of approach to equilibrium.

4. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.

5. The change in enthalpy of an endothermic reaction is ________.

6. When an electron moves from an excited state to the ground state - it _______ energy.

7. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.

8. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.

9. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.

10. The heat required to change 1mole of solid completely to vapor.

11. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.

12. Real gases act in a less than ideal way - especially under conditions of increased pressure and/or decreased temperture. Real gas behavior approaches that of ideal gases as the gas pressure becomes very low. The ideal gas is thus considered a _____ _

13. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).

14. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge

15. The freezing point - boiling point - and vapor pressure of a solution differ from those of the pure solvent by amounts which are directly proportional to the molal concentration of the solute.

16. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.

17. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.

18. _______ has very little effect on the solubility of liquids or solids in liquid solvents.

19. A theory of the hydrogen atom stating that the electron can exist in only certain stable energy levels and that when the electronic state of the atom changes - it must absorb or emit exactly that amound of energy equal to the difference betweent he f

20. The solubility of gases in liquid or solid solvents always increases with ________ pressure.

21. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l

22. A solution in which solid solute is in equilibrium with dissolved solute.

23. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.

24. A chemical reaction formed from the union of its elements.

25. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.

26. A process that occurs whent eh system is maintained at constant pressure.

27. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.

28. Electronegativities _______ as you go down a group.

29. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.

30. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.

31. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.

32. When the rate of evaporation equals the rate of condensation - the system is in __________.

33. Electronegativities ________ from left to right in a period.

34. The energy required to remove an electron from an isolated atom in its ground state.

35. A state function in which it is the heat content of a substance.

36. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.

37. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____

38. The average kinetic energy of all the molecules collectively is directly proportional to the absolute temperature of the gas. The average kinetic energy of equal numbers of molecules of any gas is the same at the same temperature.

39. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.

40. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.

41. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.

42. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.

43. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.

44. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.

45. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.

46. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.

47. In titration - this is the point at which a particular indicator changes color.

48. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.

49. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.

50. This process occurs when the system is maintained at the same temperature throughout an experiment.