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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. 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 _____ _






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






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






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






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






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






7. *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






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






9. 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.


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






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






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






13. The solubility of gases in liquid or solid solvents always increases with ________ pressure.






14. 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.






15. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.






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






17. 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.


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






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






20. Liquids with strong attractive forces have ______ boiling points.






21. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






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






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






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






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






26. The vapor pressure increases with increasing _____.






27. 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.


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






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






30. This law states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the gases in mixture.






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






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






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






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






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






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






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






38. **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.






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






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






41. 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.






42. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.






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






44. 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.


45. 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.


46. 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






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 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.






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. 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