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






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






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






4. 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.






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






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






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






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






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






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






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






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






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






15. 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.






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






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






18. 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.






19. 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






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






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






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






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






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






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






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






27. 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.






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






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






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






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






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






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






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






35. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.






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






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






38. Cells that convert electrical energy into chemical energy.






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






40. 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.






41. 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






42. 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.






43. The vapor pressure increases with increasing _____.






44. 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.






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






46. 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.






47. 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.






48. 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.






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






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