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






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






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






5. The vapor pressure increases with increasing _____.






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






7. 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.






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






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






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






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






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






13. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.






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






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






16. 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.






17. Metals have electronegativities less than ____






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






19. 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.






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






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

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






23. 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






24. 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).






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






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






27. 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






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






29. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.






30. 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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31. 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






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






33. Cells that convert electrical energy into chemical energy.






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






35. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.






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






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






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






39. 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 _____ _






40. 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.






41. *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






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






43. A chemical reaction formed from the union of its elements.






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






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






46. 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.






47. **Proceeding across a period from left to right - the ionization energy _______.






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






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 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.