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

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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. 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.






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






7. A hypothetical gas would follow Boyles law under all conditions and is called?






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






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






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






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






12. *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.






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






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






16. 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).






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






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






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






20. *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.






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






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






23. **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.






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






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






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






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






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






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






30. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.






31. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.

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32. 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






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






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






35. The vapor pressure increases with increasing _____.






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






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






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






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






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






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






43. Electronegativities _______ as you go down a group.






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






45. 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.






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






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






48. Deviations from Boyles law that occur with real gases represent _______ behavior.






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






50. 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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