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






2. The most active nonmetals are found in what corner of the periodic table?






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






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






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






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






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






8. Metals have electronegativities less than ____






9. 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.






10. 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.






11. 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






12. 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.






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






14. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.






15. 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.






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






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






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






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






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






23. 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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24. Liquids with strong attractive forces have ______ boiling points.






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






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






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






28. *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.






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

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






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






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






33. Heat added to a system and work done by a system are considered _________ quantities.






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






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






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






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






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






39. 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.






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






41. 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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42. 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).






43. *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.






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






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






46. Cells that convert electrical energy into chemical energy.






47. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.






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






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






50. 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.