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






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






3. 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.






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 freezing point is always lowered by addition of solute.






6. *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.






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






8. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.

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






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






11. 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.






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






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






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






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






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






19. 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.






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






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






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






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






24. *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.






25. In titration - this is the point at which a particular indicator changes color.






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






27. 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.






28. 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).






29. 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.






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






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






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






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






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






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






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






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






38. The vapor pressure increases with increasing _____.






39. 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.






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






41. 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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42. 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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43. 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.






44. 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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45. The change in enthalpy of an endothermic reaction is ________.






46. **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.






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






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






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

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