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






2. 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






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






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






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






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






7. **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.






8. 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).






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






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






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






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






13. *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.






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






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






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






17. Electronegativities _______ as you go down a group.






18. 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.






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






20. 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.






21. 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






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






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






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






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






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






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






28. 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






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






30. 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.

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






32. When the electron moves from the ground state to an excited state - it ______ energy.






33. 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 _____ _






34. 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.






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






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






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






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






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






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






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






42. 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).






43. 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.






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

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






46. 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.






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






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






49. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.






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