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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. 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.






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






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






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






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






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






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






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






9. 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.






10. *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.






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






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






13. 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.






14. Heat added to a system and work done by a system are considered _________ quantities.






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






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






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






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






19. **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.






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






21. Electronegativities _______ as you go down a group.






22. 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 _____ _






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






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






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






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






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. 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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30. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.






31. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.

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






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






34. Metals have electronegativities less than ____






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






36. 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.






37. 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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38. 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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39. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.






40. 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.






41. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.

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






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






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






46. 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






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






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 _____ 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.






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