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






2. 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.






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






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






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






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






7. 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.






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






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






10. 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






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






12. 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.






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






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






16. The vapor pressure increases with increasing _____.






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






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






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






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






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






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






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






25. 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.






26. Electronegativities _______ as you go down a group.






27. 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






28. This process occurs when the system is maintained at the same temperature throughout an experiment.






29. 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 _____ _






30. 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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31. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.






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






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

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






35. 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.






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






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






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






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






40. 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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41. *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






42. 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.






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






44. 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.






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






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

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






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






49. The change in enthalpy of an exothermic reaction is ________.






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