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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 required to change 1mole of solid completely to vapor.






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






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






4. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.






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






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






7. 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.






8. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.






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






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






11. 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






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






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






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






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






18. **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.






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






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






21. 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.






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






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






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






25. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.






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






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






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






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






33. 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.






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






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






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






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






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






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

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






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






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






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






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






46. 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).






47. *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






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






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






50. 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.