1. Chapter 12 Review- Chemical Periodicity

2. Chapter 12 Review - definitions electronegativity electronegativity periods periods atomic radius atomic radius ionization energy ionization energy periodic table periodic table

3. Chapter 12 Review - definitions alkali metals alkali metals halogens halogens noble gases noble gases alkaline earth metals alkaline earth metals groups groups

4. Chapter 12 Review The modern periodic table is arranged in order of increasing: The modern periodic table is arranged in order of increasing: The elements in Groups 1A through 7A and Group 0 make up the: The elements in Groups 1A through 7A and Group 0 make up the: What are characteristics of the noble gases? What are characteristics of the noble gases? ( atomic number ) ( representative elements ) ( outer s and p sublevels filled, belong to Group 0, called inert gas )

5. Chapter 12 Review What is the number of electrons in the outermost occupied energy level of an element in Group 5A? What is the number of electrons in the outermost occupied energy level of an element in Group 5A? Which have the same number of electrons in their outermost energy levels? a) K, Ca, Rb, Sr b) N, P, As, Sb Which have the same number of electrons in their outermost energy levels? a) K, Ca, Rb, Sr b) N, P, As, Sb ( 5 ) ( b )

6. Chapter 12 Review An element that contains an electron in a d sublevel is: a) Mg b) Fe An element that contains an electron in a d sublevel is: a) Mg b) Fe The elements that contain electrons in the f sublevels are referred to as: The elements that contain electrons in the f sublevels are referred to as: The outermost energy level configuration of the element chlorine is: The outermost energy level configuration of the element chlorine is: ( b ) ( inner transition metals ) ( 3s 2 3p 5 )

7. Chapter 12 Review The element with 8 electrons in its 3d sublevel is: a) Ar b) Ni The element with 8 electrons in its 3d sublevel is: a) Ar b) Ni As you move down a group of the periodic table, atomic size generally: As you move down a group of the periodic table, atomic size generally: The largest atom from among the following is: a) Fr b) Rb The largest atom from among the following is: a) Fr b) Rb ( b ) ( increases ) ( a )

8. Chapter 12 Review The smallest atom from the following is: a) Cl b) Si The smallest atom from the following is: a) Cl b) Si As the number of electrons added to the same principal energy level increases, atomic size generally: As the number of electrons added to the same principal energy level increases, atomic size generally: Removing one electron from a gaseous atom forms a: Removing one electron from a gaseous atom forms a: ( Cl ) ( decreases ) ( 1+ ion )

9. Chapter 12 Review Among the elements listed, which would show the largest increase between the 2nd and 3rd ionization energies? a) Ca b) Zn Among the elements listed, which would show the largest increase between the 2nd and 3rd ionization energies? a) Ca b) Zn Among the following, which element has the lowest IE? a) Cs b) I Among the following, which element has the lowest IE? a) Cs b) I Among the following, which has the highest 2nd IE? a) Na b) Cl Among the following, which has the highest 2nd IE? a) Na b) Cl ( a )

10. Chapter 12 Review Which of the following are always larger than the neutral atoms from which they are formed? a) cations b) anions Which of the following are always larger than the neutral atoms from which they are formed? a) cations b) anions The smallest particle from among the following is: a) Li b) Li 1+ The smallest particle from among the following is: a) Li b) Li 1+ Which is the least electronegative? a) S b) Cs Which is the least electronegative? a) S b) Cs ( b )

11. Fill in requested information from given: 2s 2 3s 2 3p 3 3s 2 3p 6 4s 1 4s 2 3d 1 4s 2 4p 5 ( 2 )( 2A ) ( alkaline earth metal) ( Be ) ( 3 )( 5A ) (representative element) ( P ) ( 3 )( 0 ) ( noble gas ) ( Ar ) ( 4 ) ( 1A ) ( alkali metal ) ( K ) ( 4 )( 3B ) ( transition metal ) ( Sc ) ( 4 ) ( 7A ) ( halogen ) ( Br )

12. Chapter 12 Review Arrange the following: Li, C, K, F, Cs Arrange the following: Li, C, K, F, Cs decreasing atomic size: decreasing atomic size: increasing ioniztion energy: increasing ioniztion energy: decreasing electronegativity: decreasing electronegativity: ( Cs, K, Li, C, F ) ( F, C, Li, K, Cs )

13. Chapter 12 Review ( K )( Li )( K ) ( C )( F )( C ) ( Ca )( Mg ) ( Ca ) ( S ) ( O ) ( S )

14. Chapter 12 Review Explain why atoms with high ionization energies typically also have high electronegativities. Explain why atoms with high ionization energies typically also have high electronegativities. ( A high ionization energy indicates that an atom has a tight hold on it’s electrons. A high electronegativity indicates an ability to attract additional electrons. They both refer to a desire to have electrons. )

15. Chapter 17 Review “Reaction Rates and Equilibrium”

16. Chapter 17 Review Energy that is available to do work is called ____. Energy that is available to do work is called ____. ____ is defined as the number of atoms, ions, or molecules that react in a given time to form products. ____ is defined as the number of atoms, ions, or molecules that react in a given time to form products. What is the name of the minimum energy that colliding particles must have in order to react? What is the name of the minimum energy that colliding particles must have in order to react? Free energy Reaction Rate Activation Energy

17. Chapter 17Review A substance that interferes with a catalyst is a(n) ____. A substance that interferes with a catalyst is a(n) ____. What is the arrangement of atoms at the peak of an energy barrier? What is the arrangement of atoms at the peak of an energy barrier? At equilibrium, what is the rate of production of reactants compared with the rate of production of products? At equilibrium, what is the rate of production of reactants compared with the rate of production of products? inhibitor Activated complex The same

18. Chapter 17 Review What is the equilibrium constant expression for the following reaction: C (s) + O 2(g) ↔ CO 2(g) What is the equilibrium constant expression for the following reaction: C (s) + O 2(g) ↔ CO 2(g) Which of the following is true about the combustion of carbon: a) the reaction is spontaneous, or b) entropy decreases? Which of the following is true about the combustion of carbon: a) the reaction is spontaneous, or b) entropy decreases? The rate of a chemical reaction normally ____ as reactant concentration increases. The rate of a chemical reaction normally ____ as reactant concentration increases. [Carbon Dioxide] [Carbon] [Oxygen] a increases

19. Chapter 17 Review Why does a higher concentration make a reaction faster? Why does a higher concentration make a reaction faster? The amount of disorder in a system is measured by its ____. The amount of disorder in a system is measured by its ____. Entropy measures ____ Entropy measures ____ For a complex reaction, the reaction progress curve has several ____. For a complex reaction, the reaction progress curve has several ____. More collisions /time entropy disorder Elementary steps

20. Chapter 17 Review What happens to a reaction at equilibrium when more reactant is added to the system? What happens to a reaction at equilibrium when more reactant is added to the system? Which reaction results in the greatest increase in entropy: a) A → B, or b) A → 2B Which reaction results in the greatest increase in entropy: a) A → B, or b) A → 2B If a reaction has an equilibrium constant (K eq ) just greater than 1, how do we interpret that information? If a reaction has an equilibrium constant (K eq ) just greater than 1, how do we interpret that information? The Reaction shifts to the right b The Reaction slightly favors Products at equilibrium

21. Chapter 17 Review A catalyst works by ____. A catalyst works by ____. If sulfur dioxide and oxygen can be made into sulfur trioxide, what is the reverse reaction? If sulfur dioxide and oxygen can be made into sulfur trioxide, what is the reverse reaction? Which variable is NOT required to calculate the Gibbs free-energy change for a chemical reaction: a) change in enthalpy, or b) temperature in o C? Which variable is NOT required to calculate the Gibbs free-energy change for a chemical reaction: a) change in enthalpy, or b) temperature in o C? Lowering the activation energy barrier SO 3  S + O 2 b

22. Chapter 17 Review What is the effect of adding more water to the following equilibrium reaction: CO 2 + H 2 O ↔ H 2 CO 3 What is the effect of adding more water to the following equilibrium reaction: CO 2 + H 2 O ↔ H 2 CO 3 In an endothermic reaction at equilibrium, what is the effect of raising the temperature? In an endothermic reaction at equilibrium, what is the effect of raising the temperature? The energy that is available to do work in a reaction is called ____. The energy that is available to do work in a reaction is called ____. Shift right Shift Right Free energy

23. Chapter 17 Review What is the numerical value (+ or -) of Gibbs free-energy change for a spontaneous reaction? What is the numerical value (+ or -) of Gibbs free-energy change for a spontaneous reaction? Which of the following systems has the highest entropy: a) 10 mL of water at 50 o C, or b) 10 mL of water at 100 o C? Which of the following systems has the highest entropy: a) 10 mL of water at 50 o C, or b) 10 mL of water at 100 o C? negative b

24. Chapter 17 Review What happens to a catalyst in a reaction? What happens to a catalyst in a reaction? Write the rate law for the following reaction: A + 2B → C + D Write the rate law for the following reaction: A + 2B → C + D An elementary reaction converts reactants to products in ____. An elementary reaction converts reactants to products in ____. Activation energy is ____. Activation energy is ____. Is the melting of ice at a temperature above 0 o C: a) endothermic, or b) exothermic? Is the melting of ice at a temperature above 0 o C: a) endothermic, or b) exothermic? The catalyst remains nchanged Rate = k[A][B] 2 One step The energy needed to make reactants Become products a

25. Chapter 17 Review Consider the reaction: N 2(g) + 3H 2(g) ↔ 2NH 3(g) What is the effect of decreasing the volume on the contained gases? Consider the reaction: N 2(g) + 3H 2(g) ↔ 2NH 3(g) What is the effect of decreasing the volume on the contained gases? Spontaneous reactions always ____ free energy. Spontaneous reactions always ____ free energy. Why does a higher temperature cause a reaction to go faster? Why does a higher temperature cause a reaction to go faster? Shift right release Increases the likelyhood of a successful collision

26. Chapter 17 Review What 2 factors determine whether or not a reaction is spontaneous? What 2 factors determine whether or not a reaction is spontaneous? What physical state of nitrogen has the highest entropy? What physical state of nitrogen has the highest entropy? What is another name for the catalysts in your body? What is another name for the catalysts in your body? Increasing entropy and decreasing enthalpy gas enzyme

27. Chapter 17 Review What is the order of the following reaction: A + 2B → C + D What is the order of the following reaction: A + 2B → C + D Why does a catalyst cause a reaction to proceed faster? Why does a catalyst cause a reaction to proceed faster? In an equilibrium reaction with a K eq of 1 x 10 8, the ____ are favored. In an equilibrium reaction with a K eq of 1 x 10 8, the ____ are favored. Which of the following explains why melting of ice is spontaneous at room temperature and pressure: a) it is accompanied by an increase in entropy, or b) it is accompanied by an increase in energy? Which of the following explains why melting of ice is spontaneous at room temperature and pressure: a) it is accompanied by an increase in entropy, or b) it is accompanied by an increase in energy? 3 rd order Lower activation energy barrier products a

28. Chapter 17 Review The K eq of a reaction is 4 x 10 -7. At equilibrium, the ____ are favored. The K eq of a reaction is 4 x 10 -7. At equilibrium, the ____ are favored. Another name for the activated complex is ____. Another name for the activated complex is ____. Which change would shift the following reaction to the right: 4HCl (g) + O 2(g) ↔ 2Cl 2(g) + 2H 2 O (g) a) decrease of pressure, or b) increase of pressure? Which change would shift the following reaction to the right: 4HCl (g) + O 2(g) ↔ 2Cl 2(g) + 2H 2 O (g) a) decrease of pressure, or b) increase of pressure? reactants Transition state b

29. Chapter 17Review In which of these systems is the entropy decreasing: a) salt dissolving in water, or b) a liquid cooling? In which of these systems is the entropy decreasing: a) salt dissolving in water, or b) a liquid cooling? Given: 2NClO (g) ↔ 2NO (g) + Cl 2(g) An analysis of the equilibrium mixture in a 1 L flask is: NClO = 1.6 mol; NO = 6.4 mol; Cl 2 = 0.49 mol. Calculate the value of K eq. Given: 2NClO (g) ↔ 2NO (g) + Cl 2(g) An analysis of the equilibrium mixture in a 1 L flask is: NClO = 1.6 mol; NO = 6.4 mol; Cl 2 = 0.49 mol. Calculate the value of K eq. b 7.84

30. Chapter 17 Review In a two-step reaction mechanism, how many elementary reactions occur? In a two-step reaction mechanism, how many elementary reactions occur? The K sp of calcium hydroxide is 6.5 x 10 -6. If the concentration is 0.0010 M Ca(OH) 2, what is the final concentration of the calcium ion? The K sp of calcium hydroxide is 6.5 x 10 -6. If the concentration is 0.0010 M Ca(OH) 2, what is the final concentration of the calcium ion? 2 2.4x10 -3

31. Chapter 17 Review A mixture of hydrogen and iodine are in equilibrium with hydrogen iodide, as shown in the equation: H 2 + I 2 ↔ 2HI Calculate the concentration of HI when the K eq is 1 x 10 5, the equilibrium concentration of H 2 is 0.04 M, and the equilibrium concentration of I 2 is 0.009 M. A mixture of hydrogen and iodine are in equilibrium with hydrogen iodide, as shown in the equation: H 2 + I 2 ↔ 2HI Calculate the concentration of HI when the K eq is 1 x 10 5, the equilibrium concentration of H 2 is 0.04 M, and the equilibrium concentration of I 2 is 0.009 M. 6 x 10 -5

32. Chapter 17 Review

33. Chapter 18 Review Acids and Bases

34. Chapter 18 Review - definitions acidic solution acidic solution conjugate acid-base pair conjugate acid-base pair amphoteric amphoteric alkaline solution alkaline solution K w K w

35. Chapter 18 Review - definitions hydroxide ion hydroxide ion neutral solution neutral solution hydronium ion hydronium ion K a K a triprotic acid triprotic acid

36. Chapter 18 Review A solution in which the hydroxide ion concentration is 1 x 10 -5 M is: A solution in which the hydroxide ion concentration is 1 x 10 -5 M is: In a neutral solution, the [ H 1+ ] is: In a neutral solution, the [ H 1+ ] is: ( basic ) ( equal to [ OH 1- ] )

37. Chapter 18 Review What are the products of the self ionization of water? What are the products of the self ionization of water? Which is most basic: a) [ H + ] = 1 x 10 -11, or b) [ OH - ] = 1 x 10 -4 ? Which is most basic: a) [ H + ] = 1 x 10 -11, or b) [ OH - ] = 1 x 10 -4 ? The formula of the hydrogen ion is often written as: The formula of the hydrogen ion is often written as: ( OH - and H + ) ( a ) ( H + )

38. Chapter 18 Review What is the pH of a solution in which the [ H + ] = 1 x 10 -12 ? What is the pH of a solution in which the [ H + ] = 1 x 10 -12 ? What is the pH of a 0.01 M hydrochloric acid solution? What is the pH of a 0.01 M hydrochloric acid solution? If K a for H 2 CO 3 is 4.3 x 10 -7, it means that H 2 CO 3 is: If K a for H 2 CO 3 is 4.3 x 10 -7, it means that H 2 CO 3 is: ( 12.0 ) ( 2.0 ) ( a poor hydrogen-ion donor )

39. Chapter 18 Review Which of the following pairs consist of a weak acid and a strong base? a) ethanoic acid, sodium hydroxide or b) sulfuric acid, sodium hydroxide Which of the following pairs consist of a weak acid and a strong base? a) ethanoic acid, sodium hydroxide or b) sulfuric acid, sodium hydroxide ( a )

40. Chapter 18 Review In the reaction NH 4 1+ + H 2 O  NH 3 + H 3 O 1+, water is acting as a(n): In the reaction NH 4 1+ + H 2 O  NH 3 + H 3 O 1+, water is acting as a(n): A solution with a pH of 5.0: A solution with a pH of 5.0: ( Bronsted-Lowry base ) ( has a hydroxide ion concentration of 1 x 10 -9 M )

41. Chapter 18 Review With solutions of strong acids and strong bases, the word strong refers to: With solutions of strong acids and strong bases, the word strong refers to: Which of these is an Arrhenius base? a) KOH, or b) NH 3 ? Which of these is an Arrhenius base? a) KOH, or b) NH 3 ? ( the degree of ionization ) ( a )

42. Chapter 18 Review Ethanoic acid ionizes in water as: Ethanoic acid ionizes in water as: CH 3 COOH + H 2 O CH 3 COO 1- + H 3 O 1+ The ethanoate ion (CH 3 COO 1- ) is therefore: 1% --> <-- 99% ( a good hydrogen-ion acceptor )

43. Chapter 18 Review Which acid is monoprotic? Which acid is monoprotic? a) CH 3 COOH, or b) H 2 CO 3 A 12.0 M solution of an acid that is able to ionize completely in solution would be termed: A 12.0 M solution of an acid that is able to ionize completely in solution would be termed: ( a ) ( concentrated and strong )

44. Chapter 20 Review According to the Bronsted-Lowry theory, water will act as a base when it: According to the Bronsted-Lowry theory, water will act as a base when it: ( accepts a hydrogen ion )

45. Chapter 18 Review What are the Bronsted-Lowry acids in this equilibrium reaction? What are the Bronsted-Lowry acids in this equilibrium reaction? CN 1- + H 2 O  HCN + OH 1- CN 1- + H 2 O  HCN + OH 1- ( H 2 O and HCN )

46. Chapter 18 Review Calculate the pH, and state if it is an acid, base, or neutral solution: Calculate the pH, and state if it is an acid, base, or neutral solution: [ H + ] = 1 x 10 -9 [ H + ] = 1 x 10 -9 [ OH - ] = 1 x 10 -10 [ OH - ] = 1 x 10 -10 [ OH - ] = 1 x 10 -1 [ OH - ] = 1 x 10 -1 [ H + ] = 1 x 10 -7 [ H + ] = 1 x 10 -7 ( pH = 9; it is basic ) ( pH = 4; it is acidic ) ( pH = 13; it is basic ) ( pH = 7; it is neutral )

47. Chapter 18 Review Calculate the hydrogen-ion concentration [ H + ] for an aqueous solution in which [ OH - ] is 1 x 10 -12 mol/L. Is this solution acidic, basic, or neutral? Calculate the hydrogen-ion concentration [ H + ] for an aqueous solution in which [ OH - ] is 1 x 10 -12 mol/L. Is this solution acidic, basic, or neutral? ( [ H + ] = 1 x 10 -2 ; it is an acidic solution )

48. Chapter 18 Review Name the following acid, and then write the expression for K a. Assume that only one hydrogen is ionized: H 2 SO 3 Name the following acid, and then write the expression for K a. Assume that only one hydrogen is ionized: H 2 SO 3 [ H + ] x [ HSO 3 - ] [ H 2 SO 3 ] K a = Sulfurous acid

49. Chapter 18 Review Name the following acid, and then write the expression for K a. Assume that only one hydrogen is ionized: HBr Name the following acid, and then write the expression for K a. Assume that only one hydrogen is ionized: HBr [ H + ] x [ Br - ] [ H + ] x [ Br - ] [ HBr ] K a = Hydrobromic acid

50. Chapter 18 Review Name the following acid, and then write the expression for K a. Assume that only one hydrogen is ionized: HNO 3 Name the following acid, and then write the expression for K a. Assume that only one hydrogen is ionized: HNO 3 [ H + ] x [ NO 3 - ] [ H + ] x [ NO 3 - ] [ HNO 3 ] K a = Nitric acid

51. Chapter 18 Review Compare and contrast the properties of acids and bases. Compare and contrast the properties of acids and bases. ( Both acids and bases are electrolytes; they cause indicators to change colors; and they react with each other to form water and a salt. Acids taste sour, bases taste bitter. Bases feel slippery. Acids react with some metals to produce hydrogen gas. )