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






2. 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.






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






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






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






6. 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).






7. *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.






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






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






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






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






12. *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.






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






15. 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.






16. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.






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






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






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






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






21. The vapor pressure increases with increasing _____.






22. 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.






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






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






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






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






28. 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.






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






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






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






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






33. 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






34. 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.






35. Electronegativities _______ as you go down a group.






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






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






38. _______ has very little effect on the solubility of liquids or solids in liquid solvents.






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






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






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






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






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






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






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






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






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






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