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






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






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






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






5. *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






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






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






8. 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.






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






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






11. 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.






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






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






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

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






16. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.

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17. 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






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






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






20. 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.






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






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






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






24. 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.






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






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






27. In an endothermic process - energy is absorbed and ^E is _______.






28. 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.






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






30. 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).






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






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

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






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






35. *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.






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






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






38. When the electron moves from the ground state to an excited state - it ______ energy.






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






40. 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.






41. 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.






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






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






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






45. 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.






46. 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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47. 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 _____ _






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






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






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