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






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






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






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






6. 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






7. 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.






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






9. *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.






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






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






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

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






14. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.






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






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






17. 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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18. 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.






19. 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.






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






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






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






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






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






25. The vapor pressure increases with increasing _____.






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






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






28. 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).






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






30. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.






31. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l






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






33. 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.






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






35. The average kinetic energy of all the molecules collectively is directly proportional to the absolute temperature of the gas. The average kinetic energy of equal numbers of molecules of any gas is the same at the same temperature.






36. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.






37. 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.






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






39. Electronegativities _______ as you go down a group.






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






41. *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.






42. *The nature of the reactants and products affect chemical reactions because some elements and compounds have bonds that when broken/formed - react more rapidly with each other than others.






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






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






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

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






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






48. The heat change during a process carried out at a constant pressure.






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






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






Can you answer 50 questions in 15 minutes?



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