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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. 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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2. The vapor pressure increases with increasing _____.






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






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






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






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






8. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






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






10. 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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11. Electronegativities _______ as you go down a group.






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






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






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






15. 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






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






17. *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






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






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






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






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






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






24. *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.






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






26. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.






27. 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.






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






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






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






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






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






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






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






35. 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.






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

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37. 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.






38. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.

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






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






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






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






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

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






45. Cells that convert electrical energy into chemical energy.






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






47. 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.






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






49. 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.






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