Test your basic knowledge |

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 ______ 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).






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






3. Metals have electronegativities less than ____






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






5. 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.






6. *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.






7. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l






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






9. 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.






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






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






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






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






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






15. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






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






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






18. 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).






19. 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.

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


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






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






22. The most active metals are found in what corner of the periodic table?






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






24. 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.






25. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


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






27. 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 _______.

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


28. 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.






29. 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






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






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






32. *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.






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






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






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






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






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






38. 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.






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






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






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






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






43. 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






44. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.






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






46. 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.

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


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






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






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






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