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

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

3. The relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).

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

5. 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.

6. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?

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

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

9. The most active metals are found in what corner of the periodic table?

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

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

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

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

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

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

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

17. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.

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

19. Metals have electronegativities less than ____

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

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

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

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

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

25. Rays made up of positive electrodes in basic electron charges.

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

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

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

29. 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.

30. 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.

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

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

33. 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.

34. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.

35. The law stating that change in internal energy is equal to the difference between the energy supplied toi the system as heat and the energy removed from the system as work performed on the surroundings.

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

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

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

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

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

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

42. In an endothermic process - energy is absorbed and ^E is _______.

43. 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

44. 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.

45. 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.

46. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.

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

48. 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

49. 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.

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