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






2. The vapor pressure increases with increasing _____.






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






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






5. 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






6. 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.






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






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


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






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






11. 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 _______.


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






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






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






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






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






17. 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.


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






19. 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.






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






21. 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.






22. 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.






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






24. 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.






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






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






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






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






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






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






31. 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.


32. 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






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






34. Electronegativities _______ as you go down a group.






35. 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.


36. *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.






37. 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.






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






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






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






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






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






43. 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.






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






45. 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.






46. 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.






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






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






49. 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).






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