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






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






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






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






5. 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 _______.


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






7. The heat change during a process carried out at a constant pressure.






8. 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 _____ _






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






10. 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.






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






12. 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.






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






14. 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.


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






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






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.


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






19. 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.






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






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






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






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


25. 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.


26. 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.






27. Cells that convert electrical energy into chemical energy.






28. Metals have electronegativities less than ____






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






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






31. *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.






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






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






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


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






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






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






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






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






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






41. *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.






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






43. *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






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






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






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






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






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






49. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.






50. *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.