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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 required to change 1mole of solid completely to vapor.






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






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






4. Metals have electronegativities less than ____






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






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






7. The vapor pressure increases with increasing _____.






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






9. 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.

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






11. 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.






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






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






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






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






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. *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






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






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






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






21. *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.






22. Electronegativities _______ as you go down a group.






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






24. Cells that convert electrical energy into chemical energy.






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






26. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.






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






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






29. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?






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






31. 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.






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






33. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.






34. 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.






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






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

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37. 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






38. 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.






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






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






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






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






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






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






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






47. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.






48. 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.

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






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