Transcript Bondingbykyle

Bonding
Ionic Bonding
• Difference in electronegativities > 1.7
• Transfers Electrons from one atom to the
other.
• Opposite charges hold atom together.
Examples
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NaCl
FeO
KCl
Au2O
Covalent Bonds
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Electrons are shared
Can be polar or nonpolar
Polar = .7 < END < 1.7
Nonpolar = 0 < END < .7
Polar = can be “split in half”, on half
positive charge, one negative charge.
Examples
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HCl
NO3
O2
Cl2
Metallic Bonds
• Bond between two metals
• Non-polar
• Electrons move freely (don’t stay attached
to one atom.
– Lattice energy
Polarity
• In Covalent bonds,the bond can be polar or nonpolar
• Polar can be divided into a positive and negative
side.
• Non-polar cannot be evenly divided with all
positive charges on one side, all negative on the
other
• Polar has an END of 0.7 – 1.7
• Non-polar had an END of 0 - 0.7
Lewis Structures
• These “draw” the electron configuration of
an atom
• Can be a maximum of two dots on each of
four sides of the atomic symbol (usually).
• Must have one dot on each side in order to
place more than one dot on a side.
Lewis Dot Structures (Example)
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1 electron
2 Electrons
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A
6 Electrons
A
3 Electrons
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7 electrons
A
4 Electrons
A
5 Electrons
A
A
A
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8 Electrons
A