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Key Concepts in Chemistry: Equilibrium, Reactions, and Properties

This summary encapsulates fundamental concepts in chemistry including equilibrium disturbance, reaction types, properties of elements, and laboratory safety. Key topics covered include Le Chatelier's Principle, endothermic reactions, types of mixtures, and the roles of different solvents and solutes. It highlights the importance of proper lab attire and safety measures when conducting experiments. Furthermore, it discusses atomic structure, isotopes, and changes of state, emphasizing critical chemistry principles crucial for students and professionals alike.

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Key Concepts in Chemistry: Equilibrium, Reactions, and Properties

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  1. Final Review

  2. When a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress. This is known as ________. • Le Chatlier’s Principle

  3. Where is the hottest part of the Bunsen burner flame? • Top of the inner cone

  4. One orbital can hold a MAXIMUM of ______ electrons. • 2

  5. A liquid will boil when equilibrium vapor pressure equals __________. • Atmospheric pressure

  6. If you are using a polar solvent, what type of solute will most likely dissolve? • Polar solute

  7. Suppose that during the reaction a chemistry student touches the beaker and observes that it feels COLD. The student should conclude that the chemical reaction is ______.  • Endothermic

  8. What are 2 examples of appropriate dress in the lab? • Long pants • Closed toe shoes • Hair pulled back • No baggy sleeves • No dangling jewelry

  9. A certain isotope of hydrogen has the following hyphen notation: hydrogen-2. The number 2 represents the ______. • Mass number

  10. Identify: • Erlenmeyer Flask

  11. Given the following equation: 2H2O  2H2 + O2 . What type of reaction does this equation represent? • Decomposition

  12. mL is a unit of ____. • volume

  13. kPa is a unit of _____. • pressure

  14. What type of element is Mg? • Alkaline Earth Metal

  15. Identify: • Florence Flask

  16. Suppose you made a salt water solution. What is the solvent? • Water

  17. What symbol is used in a chemical equation to indicate that a substance is dissolved in water? • (aq)

  18. What type of element is F? • Halogen

  19. A substance made of two or more elements whose atoms are chemically combined is a(n) ______. • Compound

  20. Suppose you made a salt water solution. What is the solute? • Salt

  21. A stable solution in which the maximum amount of solute has been dissolved is _______ • Saturated

  22. Given the following equation: 2Na + 2HCl  2NaCl + H2. What type of reaction does this equation represent? • Single Displacement

  23. What is used as a cover to the evaporating dish? • Watch glass

  24. Isotopes of a given element have a different number of ______. • Neutrons

  25. Food coloring and water is considered a ______ mixture. • Homogeneous

  26. What symbol is used in a chemical equation to indicate that a substance is a solid? • (s)

  27. The process of joining atomic nuclei is called____ • Fusion

  28. A substance that increases the rate of a reaction without itself being changed is a(n) ______. • Catalyst

  29. What is the molecular geometry of the following?: • Trigonal Planar

  30. A homogeneous mixture is also known as a(n) ______. • Solution

  31. Suppose an atom has 6 protons and 8 neutrons. What is the mass number? • 14

  32. Which of the following elements is MOST stable?Na, U, Ba, Cl, Ne • Ne (it’s a noble gas!)

  33. “g” is a unit of _____. • Mass

  34. A bond where there is an UNEQUAL SHARING of electrons is ______. • Polar covalent

  35. According to Arrhenius, bases are defined as substances that ______. • Release OH- ions in water

  36. What is the molecular geometry of the following: • Trigonal pyramidal

  37. Identify: • Watch glass

  38. Soil is considered a ______ mixture. • Heterogeneous

  39. What symbol is used in a chemical equation to indicate that a substance is a gas? • (g)

  40. Suppose a reaction is occurring in a test tube. Further, suppose that a lit splint held over the test tube “pops” and/or “barks”. The gas in the test tube is most likely ______. • Hydrogen

  41. What are 3 ways to increase the rate of dissolving of a solute? • Heating • Stirring • Grinding

  42. Suppose a reaction is occurring in a test tube. Further, suppose that a lit splint held over the test tube and the flame gets brighter. The gas in the test tube is most likely ______. • Oxygen

  43. What type of element is He? • Noble Gas

  44. The change of state from a solid directly to a gas is called ______. • Sublimation

  45. Describe the particle spacing of a gas. Particles are spaced very far apart

  46. A solution that is capable of dissolving more solute is ______. • Unsaturated

  47. The change of state from a solid directly to a liquid is called _____. • melting

  48. Describe the particle spacing of a solid. Particles are spaced very CLOSE together

  49. If the volume of a gas is increased, then the gas pressure will ______. • decrease

  50. What type of element is Mn? • Transition Metal

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