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






4. 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.






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






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






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






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






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






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

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






13. 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






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






15. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.






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






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






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






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






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






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






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






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






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






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

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






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






29. The vapor pressure increases with increasing _____.






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






31. *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.






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






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






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






35. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.






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






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






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






39. 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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40. Liquids with strong attractive forces have ______ boiling points.






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






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






43. 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.

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44. 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.






45. 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.






46. *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






47. 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.






48. Cells that convert electrical energy into chemical energy.






49. 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.






50. Electronegativities _______ as you go down a group.