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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. 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.






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






3. 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).






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






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






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






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






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






9. Electronegativities _______ as you go down a group.






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






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






12. 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).






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






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






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






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






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






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






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






20. 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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21. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.






22. *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.






23. When a system at equilibrium is disturbed by adding or removing one of hte substances - all the concentrations will change until a new equilibrium point is reached with the same value of Keq.

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24. **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.






25. 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






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






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






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






29. 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.






30. Metals have electronegativities less than ____






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






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






33. 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.






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






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






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






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






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






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






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






41. 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






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

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






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






45. 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 _____ _






46. *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






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






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






49. 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.






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