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






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






4. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.






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






6. 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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7. Cells that convert electrical energy into chemical energy.






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






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






10. *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.






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






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






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






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






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






16. 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






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






18. 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.






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






20. 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.






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






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






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






24. 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.






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






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






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






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






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






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






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






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






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






35. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.

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36. Electronegativities _______ as you go down a group.






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






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






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






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






42. 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).






43. 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.






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






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






46. 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.






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






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






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






50. *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.







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