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






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






4. 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.






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






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 relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).






8. Cells that convert electrical energy into chemical energy.






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






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






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






12. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.






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






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






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






16. Metals have electronegativities less than ____






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






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






19. *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






20. 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.






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






22. *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.






23. 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.






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






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






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






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






28. 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.






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






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






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






32. 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).






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






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






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






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






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






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






41. 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






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






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






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






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






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






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






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






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






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