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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 ______ 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).






2. 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.






3. This law states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the gases in mixture.






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

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






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






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






8. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






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






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






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






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






13. **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.






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






15. Cells that convert electrical energy into chemical energy.






16. *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.






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






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






19. 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.






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






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






22. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.






23. The change in enthalpy of an endothermic reaction is ________.






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






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






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






27. 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.






28. 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






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






30. 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.






31. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.






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






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






34. *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.






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






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






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






38. 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.






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






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






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






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






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






44. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.






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






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






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






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






50. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.