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BondingIonic versus Covalent
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Ionic BondingWhat is it?Bonding between a metal and a non
metalWhat holds the bonds together? Electrostatic attraction between (+) and
(-) “charges” which results from the transfer of the electrons from the least e-neg (metal) to the most e-neg (nonmetal)
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What happens to the electrons?One gets (-) the other gives (+).
Each resulting ion resembles a noble gas. The (-) resembles the noble gas in the same period. The (+) resembles the noble gas from the period above.
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Types of compoundsFormula unit a single piece of the
crystal lattice or ionic compound.
ConductivityConducts electricity when molten or dissolved in solution. (When ions can move around they can conduct the electric charge)
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ElectronegativityLarge electronegativity
differences – greater than 50% or about 1.7 and greater
State of MatterSolids with a very strong bond
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Other characteristicsIons: elements or group of elements
that have a “charge” from an imbalance in + and –
Lewis Dot StructureThe most e- neg element gets all the
electrons show with arrow for e-transfer and ion charge created.
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Covalent Bonding
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What is it?:Nonmetal + nonmetalWhat holds the bonds together?Attraction between nuclei of bonding
atoms and e-Intermolecular forces: affect the bond
polarity and molecular polarityLondon Dispersion-induced dipoleDipole-dipoleHydrogen bondingNonpolar: London disp. OnlyPolar: London disp. And dip-dip with
FON to H, hydrogen bonding
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What happens to the electrons?The atoms share electrons to look like
a noble gas. Nonpolar bonds share electrons evenly. Polar bonds share unevenly depending on electronegativity.
What types of compounds?Molecule is single “piece” of a
molecular compound.
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Conductivity?Does not conduct (no ions – no
conduction)Electronegativity?Little electronegativity difference.
Nonpolar = less than 0.4 difference. Polar = greater than 0.4 but less than 1.7
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States of Matter:All 3 states. Weaker bond: state
depends on size of molecule and intermolecular forces. Stronger than ionic bonds.
Other:Multiple bonds: C.SON group
forms a double, triple bonds.Diatomic molecules: 2 atoms
same element bonded together. BrINClHOF
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Shapes:VSEPR Valence shell electron repulsion theory – shapes based on shared and lone pair electrons and central atom.
Formulas Oxidation State: Find normal charge
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Lewis Dot Structure for Covalent Molecules
Why: Show how the valence electrons are arranged.
Use one dot to represent each valence electron.
A stable compound has all its atoms with a noble gas configuration. (8 v.e.)
Hydrogen follows the duet rule. (2 v.e.)The rest of the elements follow the octet
rule.Bonding pair is the one between the
symbols.
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HowSum the valence electrons.Draw skeletal structure.Central atom is carbon (if present)
or the least electronegative atomUse a pair of electrons to form a
single bond between each pair of atoms.
Arrange the rest to fulfill the octet rule (except for H and the duet).