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






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






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






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






6. 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.






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






8. The freezing point is always lowered by addition of solute.






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






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






11. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.






12. Metals have electronegativities less than ____






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






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






15. 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.






16. 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.






17. 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






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






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






20. 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.






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






22. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?






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






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






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






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






27. Cells that convert electrical energy into chemical energy.






28. 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






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






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






31. *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






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






33. **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.






34. 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.






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






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






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






38. *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.






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






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






41. *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.






42. 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.






43. The law stating that in any spontaneous process there is an increase in the entropy of the universe.






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






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






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






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






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






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






50. 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.