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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 ________ 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.






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






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






4. The vapor pressure increases with increasing _____.






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






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






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






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






9. *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.






10. *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.






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






12. 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).






13. 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.






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






15. 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.






16. 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






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






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






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






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






21. 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 _______.


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






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






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






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






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






27. *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






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






30. *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.






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






32. 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.






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






34. 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.






35. Electronegativities _______ as you go down a group.






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






37. Metals have electronegativities less than ____






38. 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.


39. 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 _____ _






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






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






42. 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.






43. 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.


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






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






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


47. 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






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






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






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