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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 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.






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






3. 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.






4. 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.

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






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






7. The freezing point is always lowered by addition of solute.






8. 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).






9. 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.






10. 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 _____ _






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






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






13. The most active nonmetals are found in what corner of the periodic table?






14. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.






15. 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.






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






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






18. *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.






19. 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.






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






21. 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 _______.

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22. 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.






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






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






25. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.






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






27. Cells that convert electrical energy into chemical energy.






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






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






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






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. **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.






33. 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.






34. 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.






35. 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.






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






37. When the electron moves from the ground state to an excited state - it ______ energy.






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






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






40. 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.

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






42. 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






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






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






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






46. The ______ of the system is some particular set of conditions of pressure - temperature - number of moles of each component - and their physical form (ex: gas - liquid - solid or crystalline form).






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






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






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

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50. 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.

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