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CLEP Chemistry 1

Subjects : clep, science, chemistry
Instructions:
  • 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 enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?






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






3. *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.






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






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






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






7. 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.


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






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






10. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.






11. The vapor pressure increases with increasing _____.






12. *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.






13. 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.






14. 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.






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






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






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






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






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






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






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






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






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






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






27. 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.


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






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






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






31. 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.






32. 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.






33. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.






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






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






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






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






38. This process occurs when the system is thermally isolated so that no heat enters or leaves.






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






40. An increase in temperature causes the position of equilibrium of an exothermic reaction to be shifted to the _____ - while that of and endothermic reactions is shifted to the _______.


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






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






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






44. 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.


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






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






47. 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.






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






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






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