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






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






3. 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.






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

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






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






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






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






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






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






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






12. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.






13. 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.






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






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






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






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






18. Cells that convert electrical energy into chemical energy.






19. 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.






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






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






23. 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.






24. 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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25. 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






26. **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.






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






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






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






31. 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.






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






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






34. 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).






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






36. 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.






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






39. 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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40. Liquids with strong attractive forces have ______ boiling points.






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






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






43. *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






44. 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).






45. 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.






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






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






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

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49. Metals have electronegativities less than ____






50. Rays made up of electrons in basic electron charges.