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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 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.






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






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






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






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






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






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






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






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






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

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






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






13. 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.






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

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






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






17. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.






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






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






20. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.






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






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






23. In an exothermic process - energy is released and ^E of reaction is ________.






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






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






26. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.






27. 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.






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






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






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






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






33. 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 _____ _






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






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






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. 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.






38. *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.






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






40. The temperature at which a substance's solid and liquid phases are in equilibrium.






41. 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).






42. 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).






43. 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.






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






45. Electronegativities _______ as you go down a group.






46. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.






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






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






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