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Ionic vs. Covalent Bonding

Ionic vs. Covalent Bonding. 9/11/08. Why bond? Most atoms are not stable by themselves. A chemical bond provides stability for both atoms involved by lowering the potential energy of both atoms.

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Ionic vs. Covalent Bonding

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  1. Ionic vs. Covalent Bonding 9/11/08

  2. Why bond? Most atoms are not stable by themselves. A chemical bond provides stability for both atoms involved by lowering the potential energy of both atoms. • chemical bond = a mutual electrical attraction between the nuclei (positive) and valence electrons(negative) of different atoms that binds the atoms together. • valence electrons = electrons located in the outermost (last) s and psublevels of an atom (max of 8e-). • all atoms want 8 valence electrons for maximum stability (like a noble gas), so they either lose, gain, or share e- from their last s and p sublevels to get 8. • three types of bonds: • ionic bond = bond that results from the electrical attraction of large numbers of cations (positive ions) and anions (negative ions). Electrons transfer from one atom to another in an ionic bond.

  3. three types of bonds: ionic bond = bond that results from the electrical attraction of large numbers of cations (positive ions) and anions (negative ions). Electrons transferfrom 1 atom to another in an ionic bond. polar covalent bond = results from unequalsharing of electrons btwn atoms. non-polar covalent bond = results from equal sharing of electrons btwn atoms.

  4. polar covalent bond = results from unequalsharing of electrons btwn atoms. non-polar covalent bond = results from equal sharing of electrons btwn atoms. to distinguish between each type of bond: determine values for the two elements in the bond (use the electronegativity table) subtract the lower value from the higher value use electronegativityrange to determine the polarity

  5. to distinguish between each type of bond: determine values for the two elements in the bond (use the electronegativity table) subtract the lower value from the higher value use electronegativityrange to determine the polarity Differences between 0 and 0.3 indicate non-polar covalent bonds, from 0.4 to 1.7 indicate polar covalent bonds, and from 1.8 to 3.3 indicate ionic bonds. Ionic bonds mainly form between a metal/metalloid and a nonmetal. Covalent bonds mainly form between two nonmetals (remember, H = nonmetal)

  6. Ionic bonds mainly form between a metal/ metalloid and a nonmetal covalent bonds mainly form between two nonmetals (remember, H = nonmetal) Non-polar covalent bonds exist in diatomic molecules, and a few others practice: are the bonds I, NPC, or PC? sulfur and hydrogen oxygen and cesium sulfur and chlorine calcium and chlorine bromine and chlorine diatomic oxygen magnesium and fluorine carbon and hydrogen aluminum and nitrogen 2.5 – 2.1 = 0.4 = PC 3.5 – 0.7 = 2.8 = I 3.0 – 2.5 = 0.5 = PC 3.0 – 1.0 = 2.0 = I 3.0 – 2.8 = 0.2 = NPC 3.5 – 3.5 = 0 = NPC 4.0 – 1.2 = 2.8 = I 2.5 = 2.1 = 0.4 = PC 3.0 – 1.5 = 1.5 = PC

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