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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. 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






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






3. 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.






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






5. 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.

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6. 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.






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






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






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






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

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






12. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.






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






14. 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 _____ _






15. 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.

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






17. *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.






18. The vapor pressure increases with increasing _____.






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






20. 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.






21. 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.

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22. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.






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






24. *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






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






26. Cells that convert electrical energy into chemical energy.






27. 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






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






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






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






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






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






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






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






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






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






37. 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.






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






39. Electronegativities _______ as you go down a group.






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






41. 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.






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






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






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






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






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






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






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






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






50. 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.







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