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






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






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






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






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






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






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






8. The freezing point - boiling point - and vapor pressure of a solution differ from those of the pure solvent by amounts which are directly proportional to the molal concentration of the solute.






9. 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.

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






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






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






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






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






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






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






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






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






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






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






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






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






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






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

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






26. 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






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






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






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






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






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






32. 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 _______.

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






34. 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.

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






36. Cells that convert electrical energy into chemical energy.






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






38. 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.






39. 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.






40. 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.






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






42. The vapor pressure increases with increasing _____.






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






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






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






46. 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).






47. 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.






48. *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.






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






50. 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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