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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. Metals have electronegativities less than ____






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






3. 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.






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






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






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






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






8. 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.






9. 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






10. 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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11. 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.






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






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






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






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






16. *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.






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






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






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






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






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






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






24. Rays made up of positive electrodes in basic electron charges.






25. 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.






26. 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.






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






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






29. 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.






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






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






32. 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.






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






34. 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.






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






36. Electronegativities ________ from left to right in a period.






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






38. The vapor pressure increases with increasing _____.






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






41. Electronegativities _______ as you go down a group.






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






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






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






46. 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






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






48. 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.






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






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