Chapter 20. The Main Group Elements 20.1 Lewis Acids and Bases 20.2 Hard and Soft Lewis Acids and Bases 20.3 The Main Group Metals Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.5 Phosphorus 20.4 The Metalloids 20.6 Other Nonmetals 20.1 Lewis Acids and Bases Learning objective: Explaining the chemistry of formation of adducts. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.1 Lewis Acids and Bases Works for solutions that are not aqueous. Focuses on electron pairs, instead of protons. Lewis Acid: any chemical species that acts as an electron-pair acceptor: example B(CH3)3 Lewis Base: any chemical species that acts as an electron-pair donor: example NH3 Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Adduct Formation A + Acid :B → A – B Base Adduct Adduct: what is formed when a Lewis Acid and Base react. SiF4 + :F- → SiF5A B Adduct AlCl3 + :PCl3 → Cl3Al-PCl3 A B Adduct The chemical bond formed is called a coordinate covalent bond. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Ammonia and Trimethylboron Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Recognizing Lewis Acids And Bases Lewis acids can be: 1. 2. 3. A molecule that has vacant valence orbitals. A molecule with delocalized p bonds involving oxygen. A metal cation. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Example 20 – 1 Lewis Acids and Bases Identify the Lewis acids and bases in each of the following reactions and draw structures of the resulting adducts: a. AlCl3 + Cl- → AlCl4b. Co3+ + 6 NH3 → [Co(NH3)6]3+ c. SO2 + OH- → HSO3- Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.2 Hard and Soft Lewis Acids and Bases Learning objective: Applying the concepts of hardness and softness to reactions. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.2 Hard and Soft Lewis Acids and Bases The strength with which an atom holds its valence electrons determines the ability of that atom to act as a Lewis Base. Polarizability – a measure of how tightly electrons are bound to an atom or molecule. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. The Hard-Soft Concept Hard Lewis Base – electron pairs of low polarizability and high electronegativity. (e.g. F-) Soft Lewis Base – large donor atom of high polarizability and low electronegativity. (e.g. I-) Hard Lewis Acid – acceptor atom with low polarizability, most metal atoms and ions. The smaller the ionic radius and the larger the charge, the harder the acid. (e.g. Al3+) Soft Lewis Acid – relatively high polarizability, large atoms with low oxidation state. (e.g. Hg2+) Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Example 20 – 2 Ranking Hardness and Softness Rank the following groups of Lewis acids and bases from softest to hardest: (a) H2S, H2O and H2Se (b) Fe, Fe3+ and Fe2+ (c) BCl3, GaCl3 and AlCl3 Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. HSAB Principle HSAB = Hard – Soft – Acid – Base Hard Lewis acids tend to combine with hard Lewis bases Soft Lewis acids tend to combine with soft Lewis bases. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. HSAB Principle e.g. Soft acids such as gold and platinum have low affinities for oxygen, a hard base. Thus these metals are not easily oxidized. e.g. Soft acids such as Pb, Hg, Ag have high affinities for the soft base sulphur, and exist in nature as PbS, HgS and Ag2S. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Metathesis Reactions Metathesis reaction – an exchange in bonding partners. Lewis acids and bases often undergo this exchange. They proceed in the direction that couples the harder acid with the harder base. Important in organic synthesis because organoboron and organoaluminum species are valuable reagents. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.3 The Main Group Metals Learning objective: Explaining the production, reactions, and uses of the main group metals. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.3 The Main Group Metals Although most metals if important are in the d block, Al, Pb and Sn have considerable technological importance. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Production of Aluminum The only main group element without filled d valence orbitals is a hard Lewis acid Highly reactive, usually found in the +3 oxidation state, difficult to reduce to Al atom. Al metal produced from the oxide by electrolysis. 4.6 % of all electricity in Canada is used to produce Al metal. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Production of Aluminum Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Uses of Aluminum Al alloys – aircraft bodies, trailers, cooking utensils, highway signs, storage tanks, beverage cans, etc. AlCl3 – used as industrial catalysts, forms adduct with itself (Al2Cl6) Catalysis of Friedel – Crafts Reactions. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Sn and Pb +2 and +4 oxidation state common Easy to reduce to free metal Sn – alloys of bronze, solder and pewter, also used as coating because of its resistant to oxidation Pb – most commonly used in automobile industry (battery), being phased out of other process because of the toxicity to organisms. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.4 The Metalloids Learning objective: Explaining the production, reactions, and uses of the metalloids. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.4 The Metalloids B, Si, Ge, As, Sb and Te Si most abundant (27% of Earth’s crust) Si was not discovered until 1824, due mostly to the fact that it was in the form of silica, SiO2. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Boron Has no valence d orbitals to participate in bonding. Boron trihalides are strong Lewis acids that react with a wide collection of Lewis bases. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Silicon Primary ingredient in most semiconductors, mainly in the form of SiO2, silica. In order to make pure Si for semiconductors, silica is first converted to SiCl4, which is then reduced to Si by Mg. Further purification is achieved using zone refining. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Silicones Si is major component of silicone polymers ~ 70,000 tons of silicone polymers are produced each year Used in greases, caulking, gaskets, biomedical devises, cosmetics, surfactants, antifoaming agents, hydraulic fluids and water repellents. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.5 Phosphorous Learning objective: Explaining the production, reactions, and uses of phosphorus. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.5 Phosphorous First extracted from human urine in 1669 Occurs in deposits as apatite, Ca5(PO4)3X where X = F, OH or Cl Elemental phosphorous: as P4 (white) it is highly reactive, but linked it forms Red Phosphorous P4 with cross-linking: the result is black phosphorous which is the most thermodynamically stable. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Example 20 – 3 Melting Points of Phosphorus The melting point of white phosphorous is 44.1°C. In contrast, red phosphorous remains a solid up to 400°C. Account for this large difference in melting point. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Phosphoric Acid Ranks in top 10 of chemicals produced. 345,000 tons produced per year in Canada Apatite is acidified with H2SO4 to form impure phosphoric acid, which is used to make fertilizer. H3PO4 + 2 NH3 → (NH4)2HPO4 Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Phosphate Condensations Play an essential role in metabolism ADP + H3PO4 → ATP + H2O ATP is a major biochemical energy source It releases energy in the reverse (hydrolysis) reaction. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.6 Other Nonmetals Learning objective: Explaining the production, reactions, and uses of the other non-metals. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. 20.6 Other Nonmetals Sulphur – sulphuric acid dominates chemistry of this element. Used in almost every major chemical-related industry H2SO4 – the least expensive strong Brønsted acid. Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Major Uses of Chlorine Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. The Chlor-Alkali Process Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Standard Reduction Potentials for Cl Species Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Production of Fluorine Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Chapter 20 Visual Summary Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Chapter 20 Visual Summary Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Chapter 20 Visual Summary Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Chapter 20 Visual Summary Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Chapter 20 Visual Summary Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd. Chapter 20 Visual Summary Chemistry, 2nd Canadian Edition ©2013 John Wiley & Sons Canada, Ltd.