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Structure, Lewis Formula:
Count the total number of valence electrons
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Structure
Structure 2
Ionic Bonding
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Lattice structure, alternating Cations + Anions, thus Hard+ Brittle
Properties
Conducts electricity in aq. solution - Free ions, soluble in water (Polar dissolves Polar)
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Covalent Bonding
Electrostatic force between shared pair of electrons and positive nuclei usually forming an octet (Incomplete octets are present in small atoms, usually cannot accomodate needed number)
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More Bonds, Shorter bond length leads to stronger bonding
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Resonance Structures
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The bond length is intermediate between a single and a double bond
All the bonds are equal in length and the electron density is spread evenly between the three oxygen atoms
Have the same strength
Hybridization - A half full p-subshell has a slightly lower energy than a partially filled one. The difference in energy
between the 2s and 2p subshells is small, so an electron can fairly easily be promoted from the 2s to the 2p, thus forming hybridized sp subshell
Metallic Bonding
Lattice structures with delocalized electrons, held together by electrostatic force
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Alloys
Alloys contain atoms of varying sizes. The addition of different atoms distorts the regular, uniform lattice of the base metal. This disruption prevents the atomic layers from sliding over each other easily, making the alloy much harder and stronger
Lewis Formula:
- Count the total number of valence electrons
- Draw the skeletal structure to show how many atoms are linked to each other.
- Use a pair of crosses or dot/cross to put an electron pair in each bond between the atoms.
- Add more electron pairs to complete the octets around the atoms ( except H which has 2 electrons)
- If there are not enough electrons to complete the octets, form double/triple bonds.
- Check the total number of electrons in the finished structure is equal to the total number of valence
electrons
Hydrogen Bonding - Special type of Dipole-Dipole, strongest IMF
To find hybridization, calculate steric number by adding the number of sigma bonds and lone pairs attached.