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






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






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

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






5. An increase in temperature causes the position of equilibrium of an exothermic reaction to be shifted to the _____ - while that of and endothermic reactions is shifted to the _______.

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6. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.






7. 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.






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






9. 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






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






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






12. 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.






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






14. 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.






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






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






17. Electronegativities _______ as you go down a group.






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






19. 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 _____ _






20. When a system at equilibrium is disturbed by adding or removing one of hte substances - all the concentrations will change until a new equilibrium point is reached with the same value of Keq.

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21. 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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22. Metals have electronegativities less than ____






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






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






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






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






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






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






29. 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.






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






31. 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.






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






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






34. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the 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. Cells that convert electrical energy into chemical energy.






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






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






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






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






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






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






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






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






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






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






47. 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.






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






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






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