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






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

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3. 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.






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






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






6. 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.






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






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






9. *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.






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






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






12. 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






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






14. 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.






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






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






17. 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






18. Metals have electronegativities less than ____






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






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






21. 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.






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






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






25. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.






26. 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.






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






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






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






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






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






32. 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).






33. 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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34. 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.






35. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.






36. 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.






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






38. 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.






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






40. 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.






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






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






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






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






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






47. 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 _____ _






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






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