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






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






3. 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.






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






5. 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 _____ _






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






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






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






9. 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.






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






11. Electronegativities _______ as you go down a group.






12. 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.






13. 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.






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






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






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






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






18. 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).






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






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






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






22. 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).






23. 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






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






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






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






27. 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.






28. 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.


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






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






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






32. 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






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






34. *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.






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






36. Cells that convert electrical energy into chemical energy.






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






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






39. *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.






40. 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.


41. The vapor pressure increases with increasing _____.






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






43. **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.






44. 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.


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






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






47. *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.






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






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






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