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






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






3. 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.






4. 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.






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






6. 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.






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






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






9. 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).






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






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






12. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.






13. 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 _____ _






14. 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.






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






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






17. Metals have electronegativities less than ____






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






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






20. *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.






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






22. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.






23. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.






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






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






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






27. 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).






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






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






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






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






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






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






34. 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






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






36. 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






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






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






39. 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.


40. 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.


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






42. 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.






43. 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.






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






45. 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.






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






47. *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.






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






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






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