covalent bonds why do atoms bond? atoms want noble gas configuration (octet) for ionic bonds there...
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Covalent Bonds
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Why do atoms bond?
• Atoms want noble gas configuration (octet)• For ionic bonds there is a transfer of electrons
to get an octet of electrons• For covalent bonds there is a sharing of
electrons to get an octet
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What is a covalent bond?
• Covalent bond - is the chemical bond that results from sharing of valence electrons– Occurs with elements close to each other on the
periodic table– Ex: H2O
– Between a nonmetal and a nonmetal– Molecule is two or more atoms bonded covalently
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Examples of Molecules
• F2
• H2O
• NH3 (ammonia)
• CH4 (methane)
• Notice there are no metals, only non-metals
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Diatomic molecules
• Some atoms do not exist as a single atom• Atoms that exist as two
H2, O2, N2, Cl2, Br2, I2, F2
• HONClBrIF• Magnificent 7-don’t forget H
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3 Types of Covalent Bonds
• Single Covalent Bond• Double Covalent Bond• Triple Covalent Bond
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3 Pencil Demo for Single, Double and Triple Covent bonds
• Make as many observations as you cani.e. facial expressions, body position, muscles
used, noises made, force or energy exerted, etc.
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Single Covalent Bonds
• Each atom shares one pair of electrons• Each atom shares 2 electrons• Longest bond• Weakest bond of the three
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Double Covalent Bonds
• In a double bond, each atom shares two pairs of electrons
• Each atom shares 4 electrons• Medium length bond• Medium strength bond
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Triple Covalent Bond
• In a triple covalent bond, each atom shares three pairs of electrons
• Each atom shares 6 electrons• The shortest bond• The strongest bond• Carbon, nitrogen, oxygen, and sulfur can form
double and triple covalent bonds
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Covalent Molecule Properties• Covalent molecular solids tend to be soft
solids, liquids, or gases at room temperature• Low melting and boiling points• Poor conductors of heat and electricity• Non-electrolytes – do not conduct electricity
in water
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Strength of Covalent Bond
• Several factors control bond strength—Number of shared electrons-the more
electrons shared, greater the bond—Size of the atom—Bond length – the greater the bond length,
the weaker the bond