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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. Rays made up of electrons in basic electron charges.






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






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






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






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






6. 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.






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






8. 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).






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






10. 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.






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






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






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






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






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






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






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






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






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






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






21. *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.






22. 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.






23. 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 _____ _






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






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






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






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






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






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






31. The vapor pressure increases with increasing _____.






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






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






34. 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.






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






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






37. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.






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






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

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






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






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






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






44. Deviations from Boyles law that occur with real gases represent _______ behavior.






45. 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 _______.

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






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






48. 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.






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






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