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






3. *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.






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






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






6. 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).






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






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






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






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






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






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






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






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






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






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






17. 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).






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






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






21. 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.






22. 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.






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






24. *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.






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






26. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.






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






28. 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.






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






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






31. The molecules in a gas are in constant - continueous - random - and straight-line motion.






32. 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.






33. 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 _____ _






34. 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.






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






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






37. 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.






38. 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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39. 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






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






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






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






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






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






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






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

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47. 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.






48. **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.






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






50. 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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