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






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






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


4. 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 _______.


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






6. 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.






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






8. 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.






9. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.






10. This process occurs when the system is maintained at the same temperature throughout an experiment.






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






12. 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.






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






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






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






16. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.






17. 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






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






19. Electronegativities _______ as you go down a group.






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






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






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






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






24. *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.






25. **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.






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






27. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____






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. 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.






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






31. 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.






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






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






34. 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






35. *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






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






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






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






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






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






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






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






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






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






45. 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.


46. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.






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






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






49. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.


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