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There are two main types of compounds: ionic compounds and binary molecular compounds. Ionic compounds form when a metal transfers electrons to a non-metal, creating oppositely charged ions held together by electrostatic attraction. Binary molecular compounds form when two non-metals share electrons in a covalent bond to achieve a full outer shell of 8 electrons. Examples of ionic compounds include LiF, formed when the metal Li loses an electron to the non-metal F. Examples of binary molecular compounds include CH4 and CO2, with covalent bonds between the non-metals.
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1. Organometallic compounds are defined as compounds in which carbon atoms are directly bonded to metal atoms. Organometallic compounds can be classified as ionic, covalent, or electron deficient based on the nature of the metal-carbon bond.
2. Metal carbonyls are compounds where carbon monoxide ligands are bonded directly to metal centers. They can be mononuclear, containing one metal center, or polynuclear, containing multiple metal centers. Common mononuclear metal carbonyls prepared include nickel tetracarbonyl, iron pentacarbonyl, and chromium hexacarbonyl.
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C:\Users\Sam\Documents\Idol Proj Unit531610
- 1. Ionic and Binary Molecular Compounds
- 2. Compounds 2 broad categories: Ionic compounds Binary molecular compounds Both types of compounds: Composed of atoms in fixed ratios Atoms connected by chemical bonds
- 3. Bonds Bonds: Electrostatic attraction Holds atoms together 2 types: Ionic bond Occurs in ionic compounds Complete transfer of electron(s) from metal to non-metal Covalent bond Occurs in binary molecular compounds Sharing of electrons between two non-metals Formed in such a way that the octet rule for all atoms is satisfied Octet rule states that all atoms will have 0 or 8 electrons in their valence(outer) shell after a bond is formed
- 4. Application of Octet Rule Atoms with only 1, 2, or 3 valence electrons: Which groups? Tend to lose electrons Why? Examples(Grp. 1: Li, K, Na and Grp. 2: Be, Mg, Ca) Atoms with close to 8 electrons: Groups 6, and 7 Tend to gain electrons(why?) Examples(Grp. 6: O, S, Se and Grp. 7: F, Cl, Br, I)
- 5. Examples of Ionic Compounds Atom from Group 1 with an atom from Group 7 Li combining with F Li loses 1 electron Why? F gains 1 electron Why? Atom from Group 2 with an atom from Group 6 Mg combining with O Mg loses 2 electrons Why? O gains 2 electrons Why?
- 6. Example of an ionic compound: Li combining with F http://en.wikipedia.org/wiki/Image:Ionic_bonding.png)
- 7. Binary Molecular Compound Formed when 2 non-metals come together Formed via covalent bond Examples: CH4 CO2 SO3 N2O4
- 8. Example of a Binary Molecular Compound: Covalent Bond ({{Information |Description=Covalently bonded hydrogen and carbon in a molecule of methane. |Source=Created with Inkscape |Date=28 January 2006 |Author=DynaBlast |Permission=Creative Commons Attributio)