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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. 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.






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






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






4. 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.






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






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






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

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8. Cells that convert electrical energy into chemical energy.






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






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






12. Electronegativities _______ as you go down a group.






13. *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.






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






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






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 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.






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






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






20. 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).






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






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






23. 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.






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






25. The vapor pressure increases with increasing _____.






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






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






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






29. 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.






30. 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.






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






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






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






35. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.

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






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






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






39. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.






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






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






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






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






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






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






46. 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.






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






48. *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






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






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