Test your basic knowledge |

CLEP Chemistry 1

Subjects : clep, science, chemistry
  • Answer 50 questions in 15 minutes.
  • If you are not ready to take this test, you can study here.
  • Match each statement with the correct term.
  • Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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. 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.

2. A hypothetical gas would follow Boyles law under all conditions and is called?

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

4. 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.

5. The law stating that in any spontaneous process there is an increase in the entropy of the universe.

6. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.

7. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.

8. Deviations from Boyles law that occur with real gases represent _______ behavior.

9. Rays made up of electrons in basic electron charges.

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

11. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g

12. The temperature at which a substance's solid and liquid phases are in equilibrium.

13. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.

14. The change in enthalpy of an exothermic reaction is ________.

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

16. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.

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

18. 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

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

20. Liquids with strong attractive forces have ______ boiling points.

21. The pressure exerted by each gas in a mixture is called its _____ pressure.

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

23. *The nature of the reactants and products affect chemical reactions because some elements and compounds have bonds that when broken/formed - react more rapidly with each other than others.

24. _____ bonds are present in molecules containing double or triple bonds.

25. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.

26. The heat change during a process carried out at a constant pressure.

27. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.

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

29. When a system at equilibrium is disturbed by adding or removing one of hte substances - all the concentrations will change until a new equilibrium point is reached with the same value of Keq.

30. The molecules in a gas are in constant - continueous - random - and straight-line motion.

31. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.

32. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.

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

34. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.

35. The action of salts of weak acids or bases with water to form acidic or basic solutions.

36. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.

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

38. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.

39. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.

40. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.

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

42. Metals have electronegativities less than ____

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

44. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.

45. A valence theory that permits the geometric arrangement of atoms - or groups of atoms - about some central atom to be determined solely by considering the repulsions between the electron pairs present in the valence shell of the central atom.

46. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.

47. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.

48. **Proceeding across a period from left to right - the ionization energy _______.

49. In an exothermic process - energy is released and ^E of reaction is ________.

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