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






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






3. This process occurs when the system is maintained at the same temperature throughout an experiment.






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






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






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






7. 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.






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






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






11. 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.






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






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






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






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






16. *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.






17. *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.






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






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






20. 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).






21. 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






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






23. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g






24. Metals have electronegativities less than ____






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






26. 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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27. 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






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






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






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






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

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32. Cells that convert electrical energy into chemical energy.






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






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






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






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






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






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






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






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






41. 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.






42. 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.






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






46. *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.






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






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






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






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