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






3. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.






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






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






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






8. 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.






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






10. Cells that convert electrical energy into chemical energy.






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






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






14. 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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15. Electronegativities ________ from left to right in a period.






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

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






18. **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.






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






20. Metals have electronegativities less than ____






21. 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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22. Electronegativities _______ as you go down a group.






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






24. Rays made up of electrons in basic electron charges.






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






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






27. 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.






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






29. 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.






30. 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.






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






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






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






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. 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.






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






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






38. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.






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






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






41. 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.






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






43. 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).






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






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






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






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






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






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






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