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






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






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






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






5. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.






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






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






8. *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.






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






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






11. 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.






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






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






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






15. 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






16. Cells that convert electrical energy into chemical energy.






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






18. *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.






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






20. 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.






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






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

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






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






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






26. 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.






27. 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.






28. 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.






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






30. 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 _____ _






31. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).






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






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






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






36. 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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37. 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).






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






39. 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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40. 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






41. Electronegativities _______ as you go down a group.






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






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

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44. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.






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






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






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






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






50. 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.