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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. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.






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

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3. *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.






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






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






6. 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.






7. The average kinetic energy of all the molecules collectively is directly proportional to the absolute temperature of the gas. The average kinetic energy of equal numbers of molecules of any gas is the same at the same temperature.






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






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






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






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






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






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






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

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






17. *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.






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






19. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.






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






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






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






23. *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






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






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






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






27. 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






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






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






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






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






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






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






34. 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 _____ _






35. 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.






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






37. 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.






38. 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.






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






40. **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.






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






42. *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.






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






44. 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).






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






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






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






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






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






50. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l