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






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






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






4. 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.






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






6. 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.






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

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






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






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






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






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






14. 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.






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






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






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






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






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






20. The vapor pressure increases with increasing _____.






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






22. Electronegativities _______ as you go down a group.






23. 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






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






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






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






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






28. The action of salts of weak acids or bases with water to form acidic or basic solutions.






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






30. *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.






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






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






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






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






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






36. *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.






37. 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.






38. 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.






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






40. 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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41. 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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42. Deviations from Boyles law that occur with real gases represent _______ behavior.






43. Cells that convert electrical energy into chemical energy.






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. *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






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






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






49. **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.






50. 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.