Chemical Bonding.

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Presentation transcript:

Chemical Bonding

Covalent Bonds Formed when 2 atoms share electrons

Polar Covalent Bonds Unequal sharing of electrons Electrons attracted more to atom with the higher electronegativity Electronegativity difference is between 0.4 – 1.7 Polar Covalent Bonds dissolve in water

Polar Covalent Bonds

Non-polar Covalent Bonds Equal sharing of electrons Electronegativity difference is between basically 0. Usually found between diatomic molecules – two of the same atoms Non-polar covalent bonds don’t dissolve in water.

Non-polar Covalent Bonds

Ionic Bonds Electrical attraction between large numbers of cations and anions Ion = a charged particle Cation = + charged particle Loves to give electrons away Low Ionization Energy & Electronegativity Typically are metals

Ionic Bonds (cont.) Anion = - charged particle Loves to accept electrons High Ionization Energy & Electronegativity Typically are nonmetals Electronegativity difference >1.7

Ionic Bonds (cont.)

Ionic Bonds (cont.) If a bond is ionic: The compound will fall apart (dissociate) into its original ions when dissolved in water If a conductivity test is performed, the light bulb will… light!

Metallic Bonds Bond formed between multiple metal atoms. Electrons are free to move within electron clouds of all metal ions = Sea of Electrons Electrons are delocalized – they don’t belong to any one atom anymore.

Metallic Bonds

Hydrogen Bonds Intermolecular – attraction between molecules One molecule is polar and has Hydrogen in a H-F, H-O or H-N bond Other molecule has an unshared pair of electrons, usually F, O, N

Hydrogen Bond Example:

Van der Waals Bonds These bonds are important for Noble Gases Very weak bonds Electrons of Noble Gases get shifted to one side causing it to attract a slightly positive atom that is nearby.

Van der Waals Bond Example: