BIOS 1705 Lecture 3: BIOS 1700 Lecure and Book Notes #2 PDF

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Periodic table: the rows equal the number of shells or orbitals each atom has. Example: hydrogen: row 1, 1 orbital. H: carbon: row 2, 2 orbitals, chlorine: row 3, 3 orbitals. Ch: columns: atoms in the same columns share similar chemical properties. Bonds with shared electrons like covalent and ionic bonds. Bonds without shared electrons like hydrogen bonds and van der waals force: share/bond between charges, covalent bonds (strongest) Make atoms stable by lling their outer orbitals with valence electrons. Number of electrons in outer shell must equal 8 to be stable. The electrons in the outermost orbital are called valence electrons. Covalent bonds are made to satisfy these valence electron needs; all atoms want the outer shell filled. Atoms make single, double, or triple covalent bonds with other atoms to make 8 valence electrons in the outer shell: ionic bonds (2nd strongest) Extreme case of polar covalent bonds (below) Not quiet sharing electrons: example: na + cl bond.

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