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






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






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






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






6. 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






7. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.






8. 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.






9. 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.






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






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






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






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






14. 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.






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






16. 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.






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






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

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






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






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






22. Metals have electronegativities less than ____






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






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






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






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






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






28. The vapor pressure increases with increasing _____.






29. **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.






30. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






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






32. 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.






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






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






35. 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.






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






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






38. _____ bonds are present in molecules containing double or triple bonds.






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






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






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






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






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






45. 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.






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






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






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






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






50. 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