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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. Metals have electronegativities less than ____






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






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






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






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






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






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






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






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






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






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






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






14. 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).






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






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






17. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.






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






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






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






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






22. 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.






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






24. 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.






25. *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






26. Cells that convert electrical energy into chemical energy.






27. 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.






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






29. 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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30. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.






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






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






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






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






35. 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 _____ _






36. 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.






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






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






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






40. 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.






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






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






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

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






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






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






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






48. 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






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






50. 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.