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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 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.






2. *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.






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






4. 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.






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






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






7. Cells that convert electrical energy into chemical energy.






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






9. 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.






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






11. Electronegativities _______ as you go down a group.






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






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






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






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.

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16. 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






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






18. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.






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






20. 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.






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






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






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






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






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






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






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






29. The solubility of gases in liquid or solid solvents always increases with ________ pressure.






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






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






32. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.






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






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






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






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






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

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






39. 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.






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






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






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






44. 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.






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






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






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






48. *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






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






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






Can you answer 50 questions in 15 minutes?



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