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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. 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.






2. 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).






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






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






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






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






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






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






9. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.






10. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.






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






12. 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.






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






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






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






16. 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.






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






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






19. 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.

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20. 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






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






22. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.






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






24. 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 _____ _






25. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.

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






27. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.






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






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






30. 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.






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






32. 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






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






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






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






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






38. 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).






39. 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.






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






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






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

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






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






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






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






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






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






49. *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.






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






Can you answer 50 questions in 15 minutes?



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