Test your basic knowledge |

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






2. The law stating that in any spontaneous process there is an increase in the entropy of the universe.






3. A valence theory that permits the geometric arrangement of atoms - or groups of atoms - about some central atom to be determined solely by considering the repulsions between the electron pairs present in the valence shell of the central atom.






4. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.






5. 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






6. In titration - this is the point at which a particular indicator changes color.






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






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






9. 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 _____ _






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






11. 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






12. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.






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






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






15. 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






16. Cells that convert electrical energy into chemical energy.






17. 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.






18. 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.

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


19. 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.






20. 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.






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






22. 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.






23. The freezing point - boiling point - and vapor pressure of a solution differ from those of the pure solvent by amounts which are directly proportional to the molal concentration of the solute.






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






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






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






27. 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.

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183


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






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






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






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






32. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____






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






34. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.






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






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






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






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






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






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






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






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






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






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






45. Electronegativities _______ as you go down a group.






46. When the rate of evaporation equals the rate of condensation - the system is in __________.






47. 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.






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






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






50. 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.