Compounds and Bonding
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1 Compounds and Bonding Chemical compounds Ionic bonding NaCl as a type example Electron transfer and shell completion Covalent bonding Diamond - pure C example Electron sharing Silicon Tetrahedron Structure (strong sp 3 covalent bonds) Building block of silicate minerals
2 Chemical compound: Two or more elements joined together by a chemical bond. Most minerals are composed of at least two elements. Chemical Formula: NaCl Note Cubic Symmetry and Closest Packing Halite Atomic Structure
3 1s 2 1s 2 2s 2 2p 6 Outer Shell Filling
4 Ionic Bonding and Electron Exchange 11p e - = +1 1s 2 2s 2 2p 6 3s 1 +1e - 1s 2 2s 2 2p 6 3s 2 3p 5 17p e - = -1
5 Ionic Bonding: Electron Transfer The propensity of an element to gain or lose electrons may be parameterized by a value called electronegativity (EN). The scale is arbitrary and was defined by Linus Pauling in Low EN elements tend to lose valence electrons to become cations. High EN elements tend to gain valence electrons to become anions. Cations (+) are always smaller than the neutral atom; Anions (-) are always larger than the neutral atom.
6 Ionic Bonding NaCl example Atoms that become ionized are charged particles - Like charges are repulsive - Unlike charges are attractive - Ionic bonds balance these forces F a (q + ) (q - )/d 2 Coulomb Law F r -n/d 1+n Born Repulsion Where q is charge (+ or -), d is the distance between the atoms, and n is an integer that depends on the number of filled shells F total = F a + F r
7 Covalent Bonding: Electron Sharing Diamond and Graphite - Pure Carbon in complex 3D network
8 Covalent Bonding: Hybrid Orbitals Diamond Example - Pure Carbon in complex 3D network
9 Diamond vs. Graphite - Polymorphs Diamond has a hardness of 10 and is an electrical insulator, while Graphite has a hardness of 2 and is a electrical conductor. Polymorphism is the ability of a chemical compound to crystallize in more than one structure. The different forms are called polymorphs; they may show vastly different physical and chemical behavior. Temperature and pressure are important controls on which polymorph is stable. Diamond stabilization requires very high pressures, which are normally only found deep in the Earth s interior (the mantle).
10 Covalent Bonding: Sigma vs. Pi bonds Note the hexagonal symmetry and that graphite tends to form in layered sheets pi bonds are weaker than sigma bonds Graphite Example - Pure Carbon in layered 3D network
11 Covalent Bonding: Diamond vs. Graphite Diamond Graphite
12 Metallic Bonding Extreme form of covalent bonding in which the electrons become decoupled from the nuclei (low EN) and move through the crystal. Occurs when Valence Band electrons overlap in energy with Conduction Band Effect is enhanced as interatomic spacing is decreased that is with higher pressure (deep interior of Earth and other planets metallic H in Jupiter). Mg Na
13 Partial Ionic Bonding and Electronegativity Electronegativity defined by Linus Pauling (1960) is a relative scale with Li fixed at a value of 1, C at 2.5 and F at 4.0 Low values of EN yield cations (+) High values of EN yield anions (-) Na = 0.9 and Cl = 3.0 -> E = 2.1 ~68% ionic character Si = 1.8 and O = 3.5 -> E = 1.7 ~55% ionic character
14 Silicon Tetrahedron: SiO 4 (net -4 charge) 1.30 Å 1 angstrom = meters 0.34 Å
15 Summary chemical bond types Bonds which involve valence electrons Ionic (transfer of electrons) Covalent (sharing of electrons in hybrid orbitals) Metallic (decoupled electrons) Partial ionic or mixed bonds Non valence electron bonds or molecular bonds Hydrogen (asymmetric charge must have H) van der Waals (short-term charge polarity and doesn t require H)
16 Water, Ice and Snow Most important substance on Earth Essential for biological life as we know it Unique volumetric property Molecular symmetry and its relationship to crystal morphology Crystal growth and its effect on crystal morphology
17 Chemical Formula: H 2 O Water Atomic Structure
18 Hydrogen Bonding in water and ice In the H 2 O molecule, charge is highly polarized. Oxygen pulls electrons from H toward itself and leaves most of the positive charge closer to the center of the H atoms in the form of a H + proton. The 3D network of ice forms bonds because of this charge polarity in the water molecule. This is called hydrogen bonding.
19 Snowflake Morphology Hexagonal Symmetry Oddly, ice is less dense than liquid water, hence it floats and lakes freeze from the top down! 1-5 mm From:
20 Snowflake Growth From:
21 LT-SEM Images of Snow Crystals
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