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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. *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.






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






3. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?






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






5. 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.






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






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






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






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






10. *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.






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






12. 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






13. 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.






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






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






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






17. **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.






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






19. The vapor pressure increases with increasing _____.






20. 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.






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






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

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






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






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






26. 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.






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






28. 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 _____ _






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






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






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






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






33. 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.






34. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.






35. 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.

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






37. 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.






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






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






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






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






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






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






44. 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.






45. 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.






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






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






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






50. 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).