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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. 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.






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






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






4. 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).






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






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






8. 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.


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






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






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






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






13. 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.






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






15. 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.






16. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).






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






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






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






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






21. When an electron moves from an excited state to the ground state - it _______ energy.






22. The vapor pressure increases with increasing _____.






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






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






25. 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.






26. Electronegativities _______ as you go down a group.






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






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






29. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.






30. This process occurs when the system is thermally isolated so that no heat enters or leaves.






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






32. *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






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






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






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






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






37. 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.


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






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






40. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.






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






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






43. 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.






44. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.






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






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






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






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






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






50. 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.