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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. Electronegativities _______ as you go down a group.






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






3. 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.






4. The ______ of the system is some particular set of conditions of pressure - temperature - number of moles of each component - and their physical form (ex: gas - liquid - solid or crystalline form).






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






6. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.






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






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






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






10. Metals have electronegativities less than ____






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






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






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






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






15. *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.






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






17. 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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18. Liquids with strong attractive forces have ______ boiling points.






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. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?






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






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






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






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






25. 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.






26. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.






27. 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.






28. Cells that convert electrical energy into chemical energy.






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






30. 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.






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






32. 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.






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






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






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

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36. *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






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






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






40. 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.






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






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






43. 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 _____ _






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






45. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.






46. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.






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






48. 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).






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






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