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






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






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






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






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






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






7. 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.


8. 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 _______.


9. 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.






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






11. In titration - this is the point at which a particular indicator changes color.






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






13. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.


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






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






16. 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).






17. 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.






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






19. Cells that convert electrical energy into chemical energy.






20. **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.






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






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






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






24. 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.






25. 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.


26. Electronegativities _______ as you go down a group.






27. 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.






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






29. 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.






30. *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.






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






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






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






34. 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.






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






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






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






38. *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






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






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






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






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






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






44. Heat added to a system and work done by a system are considered _________ quantities.






45. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.


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






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






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






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






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