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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. 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.






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






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






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






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






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






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






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






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






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






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






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






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






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






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






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






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






18. The law stating that change in internal energy is equal to the difference between the energy supplied toi the system as heat and the energy removed from the system as work performed on the surroundings.






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






20. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.

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






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






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






24. *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.






25. 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.






26. 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.






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






28. 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.






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






30. **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.






31. 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.






32. 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).






33. 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 _______.

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34. *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.






35. 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.






36. 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.






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

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38. 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






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






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






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






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






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






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






45. 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.






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






47. 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






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






49. The vapor pressure increases with increasing _____.






50. Electronegativities _______ as you go down a group.