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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 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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2. Cells that convert electrical energy into chemical energy.






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






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






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






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






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






8. 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.






9. 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.






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






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






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






14. *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






15. 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).






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






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






18. 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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19. Metals have electronegativities less than ____






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






21. 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






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






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






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






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






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






27. 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.






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






29. *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.






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






31. **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.






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






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






34. 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.






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






36. 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.






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






38. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.






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






40. The vapor pressure increases with increasing _____.






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






42. *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.






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






44. Electronegativities _______ as you go down a group.






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






46. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.






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






48. 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 _____ _






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






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