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






2. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.






3. 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.






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






5. 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






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






8. Cells that convert electrical energy into chemical energy.






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






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






11. 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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12. Electronegativities ________ from left to right in a period.






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






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






15. 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.






16. 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.






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






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






19. 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.






20. 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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21. *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.






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






23. 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.






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






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






26. 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.






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






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






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






30. Metals have electronegativities less than ____






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






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






33. The vapor pressure increases with increasing _____.






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






35. 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.






36. 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 _____ _






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






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






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






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






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






42. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g






43. 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.






44. 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.






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






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






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






48. 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).






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






50. 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.