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






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






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






4. **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.






5. 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.






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






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






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






9. 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






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






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






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






13. 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.


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






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






16. 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.


17. 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.






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






19. 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.






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






21. 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






22. 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






23. Metals have electronegativities less than ____






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






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






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






27. 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.






28. 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.






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






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






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






32. Cells that convert electrical energy into chemical energy.






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






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






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






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






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






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






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






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






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






42. 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).






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






44. 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.


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






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






47. The pressure exerted by each gas in a mixture is called its _____ pressure.






48. 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.






49. *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.






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