2. LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity. (Sec )
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied. (Sec )
LO 2.17 The student can predict the type of bonding present between two atoms in a binary compound based on position in the periodic table and the electronegativity of the elements. (Sec 20.1)
LO 5.18 The student can explain why a thermodynamically favored chemical reaction may not produce large amounts of product (based on consideration of both initial conditions and kinetic effects), or why a thermodynamically unfavored chemical reaction can produce large amounts of produce for certain sets of initial conditions. (Sec 20.2)

3. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.
LO 2.17 The student can predict the type of bonding present between two atoms in a binary compound based on position in the periodic table and the electronegativity of the elements.

4. Reviewing the Periodic Table Regions
Representative elements:
Groups 1A – 8A (filling s and p orbitals)
Transition metals:
Center of the table (filling d orbitals)
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5. Reviewing the Periodic Table Regions
Lanthanides and Actinides:
Listed separately, on the bottom of the table (filling 4f and 5f orbitals)
Metalloids:
Separate metals from nonmetals
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6. The Atomic Radii of Some Representative Elements (in Picometers)

7. Which should be the larger atom? Why? Na Cl
CONCEPT CHECK!
Which should be the larger atom? Why?
Na Cl
Na should be the larger atom because the electrons are not bound as tightly due to a smaller effective nuclear charge.
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8. Which should be the larger atom? Why? Li Cs
CONCEPT CHECK!
Which should be the larger atom? Why?
Li Cs
Cs should be the larger atom because of the increase in orbital sizes in successive principal quantum levels (to accommodate more electrons).

9. Distribution of the 18 Most Abundant Elements
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10. Abundance of Elements in the Human Body
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11. AP Learning Objectives, Margin Notes and References
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.
LO 2.17 The student can predict the type of bonding present between two atoms in a binary compound based on position in the periodic table and the electronegativity of the elements.
LO 5.18 The student can explain why a thermodynamically favored chemical reaction may not produce large amounts of product (based on consideration of both initial conditions and kinetic effects), or why a thermodynamically unfavored chemical reaction can produce large amounts of produce for certain sets of initial conditions.
Additional AP References
LO 5.18 (see Appendix 7.11, “Non-Spontaneous Reactions”)

12. Alkali Metals: Sources and Methods of Preparation
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13. Group 1A Oxides
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14. Na2O2(s) + H2O(l) → NaOH(aq) + H2O2(aq) EXERCISE!
Predict the products formed by the following reactants:
Na2O2(s) + H2O(l)
→ NaOH(aq) + H2O2(aq)
NaOH(aq) + H2O2(aq)
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15. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

16. Hydrides Binary compounds containing hydrogen: Ionic hydrides:
hydrogen + the most active metals
(eg; LiH, CaH2)
Covalent hydrides:
hydrogen + other nonmetals
(eg; H2O, CH4, NH3)
Metallic (interstitial) hydrides:
transition metal crystals treated with H2 gas
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17. LiH(s) + H2O(l) → H2(g) + LiOH(aq) EXERCISE!
Predict the products formed by the following reactants:
LiH(s) + H2O(l)
→ H2(g) + LiOH(aq)
H2(g) + LiOH(aq)
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18. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

19. Alkaline Earth Metals Very reactive Great practical importance:
Human life (Ca and Mg)
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20. Selected Reactions of Group 2A Elements
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21. Ion Exchange
Ca2+ and Mg2+ are often removed during ion exchange, releasing Na+ into solution.
Ion exchange resin – large molecules that have many ionic sites.
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22. A Schematic Representation of a Typical Cation Exchange Resin
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23. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

24. Group 3A elements generally show the increase in metallic character in going down the group that is characteristic of the representative elements.
B, Al, Ga, In, Tl
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25. Some Physical Properties, Sources, and Methods of Preparation
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26. Some Important Reactions
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27. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

28. Can form four covalent bonds to nonmetals. CH4, SiF4, GeBr4
Contains two of the most important elements on earth: carbon and silicon.
Can form four covalent bonds to nonmetals.
CH4, SiF4, GeBr4
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29. Some Physical Properties, Sources, and Methods of Preparation
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30. Some Important Reactions
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31. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

32. Exhibits varied chemical properties. N, P, As, Sb, Bi
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33. Some Physical Properties, Sources, and Methods of Preparation
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34. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

35. Nitrogen
The great stability of the NΞN bond means that most binary compounds containing nitrogen decompose exothermically to the elements.
NO2(g) ½N2(g) + O2(g)
ΔH° = –34 kJ
N2H4(g) N2(g) + 2H2(g)
ΔH° = –95 kJ
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36. Nitrogen Fixation
The process of transforming N2 to other nitrogen–containing compounds.
The Haber Process:
N2(g) + 3H2(g) NH3(g)
ΔH° = –92 kJ
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37. The Nitrogen Cycle
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38. Nitrogen Hydrides Ammonia, NH3 Fertilizers Hydrazine, N2H4
Rocket propellant, manufacture of plastics, agricultural pesticides
Monomethylhydrazine, N2H3(CH3)
Rocket fuels
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39. Nitrogen Oxides Compound Oxidation State of N
Nitrogen in its oxides has oxidation states from +1 to +5.
In other compounds, nitrogen could have oxidation states of -1 to -3.
Compound
Oxidation State of N N 2 O +1 NO +2 3 +3 +4
HNO +5

40. Nitrogen Oxyacids Nitric acid, HNO3 Nitrous acid, HNO2
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41. The Ostwald Process
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42. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

43. Allotropes of Phosphorus
White Phosphorus = P4 (tetrahedral) - very reactive
Black Phosphorus = crystalline structure - much less reactive
Red Phosphorus = amorphous with P4 chains
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44. Allotropes of Phosphorus
a) Pwhite b) Pblack c) Pred
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45. Phosphorus Oxyacids Phosphoric acid, H3PO4 Phosphorous acid, H3PO3
Hypophosphorous acid, H3PO2
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46. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

47. Can form covalent bonds with other nonmetals.
O, S, Se, Te, Po
Although in Group 6A there is the usual tendency for metallic properties to increase going down the group, none of the Group 6A elements behaves as a typical metal.
Can form covalent bonds with other nonmetals.
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48. Some Physical Properties, Sources, and Methods of Preparation
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49. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

50. Oxygen O2 makes up 21% of the Earth’s atmosphere.
O3 (ozone) exists naturally in the upper atmosphere of the Earth.
Ozone layer absorbs UV light and acts as a screen to prevent this radiation from penetrating to the Earth’s surface.
Scientists have become concerned that Freons and nitrogen dioxide are promoting the destruction of the ozone layer.
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51. Ozone

52. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

53. Sulfur is found in nature both in large deposits of the free element and in ores such as galena, cinnabar, pyrite, gypsum, epsomite, and glauberite.
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54. Frasch Process
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55. Aggregates of Sulfur
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56. Sulfur Oxide Reactions
2SO2(g) + O2(g) 2SO3(g) SO2(g) + H2O(l) H2SO3(aq) SO3(g) + H2O(l) H2SO4(aq)
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57. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

58. Halogens All nonmetals: F, Cl, Br, I, At
Because of their high reactivities, the halogens are not found as free elements in nature. They are found as halide ions (X–) in various minerals and in seawater.
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59. Trends in Selected Physical Properties
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60. Some Physical Properties, Sources, and Methods of Preparation
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61. Preparation of Hydrogen Halides
H2(g) + X2(g) HX(g)
When dissolved in water, the hydrogen halides behave as acids, and all except hydrogen fluoride are completely dissociated.
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62. Halogen Oxyacids and Oxyanions
All halogens except fluorine combine with various numbers of oxygen atoms to form a series of oxyacids.
The strengths of these acids vary in direct proportion to the number of oxygen atoms attached to the halogen, with the acid strength increasing as more oxygens are added.
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63. The Known Oxyacids of the Halogens
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64. AP Learning Objectives, Margin Notes and References
LO 1.10 Students can justify with evidence the arrangement of the periodic table and can apply periodic properties to chemical reactivity.
LO 1.11 The student can analyze data, based on periodicity and the properties of binary compounds, to identify patterns and generate hypotheses related to the molecular design of compounds for which data are not supplied.

65. Noble Gases Filled s and p valence orbitals
He and Ne form no compounds.
Kr and Xe have been observed to form chemical compounds:
Xe(g) + 2F2(g) XeF4(s) [6 atm, 400°C]
XeF6(s) + 3H2O(l) XeO3(aq) + 6HF(aq)
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66. Selected Properties
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67. Which of the following groups is the most reactive? Group 1A Elements
CONCEPT CHECK!
Which of the following groups is the most reactive?
Group 1A Elements
Group 5A Elements
Group 6A Elements
Group 8A Elements
The correct answer is “a”. The Group 1A elements, alkali metals, are very reactive.
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68. CONCEPT CHECK!
Which of the following groups does not contain at least one element that forms compounds with oxygen?
Group 4A Elements
Group 5A Elements
Group 6A Elements
Group 7A Elements
All of these groups contain at least one element that forms compounds with oxygen.
The correct answer is “e”.
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