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






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






3. In titration - this is the point at which a particular indicator changes color.






4. 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.






5. 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.






6. 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.






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






8. *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.






9. 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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10. The change in enthalpy of an endothermic reaction is ________.






11. 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.






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






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






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






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






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






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






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






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






21. 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.






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






23. 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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24. Rays made up of electrons in basic electron charges.






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






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






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






28. *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.






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






30. 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.






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






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






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






34. 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).






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






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






37. 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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38. Electronegativities _______ as you go down a group.






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






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






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






42. 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






43. 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.






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






45. Metals have electronegativities less than ____






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






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






48. 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.






49. 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.






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