unit 3: chemical bonding - thunderridge...
TRANSCRIPT
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Unit 3: Chemical BondingSection 1: Bond Types and Properties
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● Chemical Bond – force that holds atoms or ions together to make a molecule or other chemical structure◦ Molecule - two or more atoms bonded together
● When bonding, atoms use their outermost electrons, called valence electrons
Chemical Bonds
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● The goal of bonding is to have a full outer energy level◦ Some atoms GAIN electrons to reach 8 valence electrons◦ Some atoms LOSE electrons to empty their outermost level
(leaving a full one underneath!)
● Three main types of bonds:◦ Ionic Bonds◦ Covalent Bonds◦ Metallic Bonds
Chemical Bonds (cont.)
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● Bonds that form by transferring electrons from one atom to another
● This changes their charges (makes them ions… get it IONic bonds?!) and now they attract one another!!
● Occurs when a positive cation (metal) combines with a negative anion (nonmetal)
● Metal + Nonmetal
Ionic Bonds
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Properties of Ionic Compounds- Ionic Solids
- Solids at room temperature
- Form a rigid crystal lattice structure
- Caused by the attraction between the positive cations and negative anions
- This structure places ions close together = strong attractive force
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Properties of Ionic Compounds- Conduct electricity when they are dissolved in water
(aqueous form) but not as solids. - Many are soluble in water (a polar molecule)- VERY High melting and boiling points
- Caused by the strong ionic bond- Strong Bonds = Strong Molecules = Hard, Brittle on the large
scale (not malleable)
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Why are Ionic Compounds Conductive When Dissolved in Water?
- Electricity conducts because of free-flowing electrons.
- If electrons are not able to move, substances are not conductive (AKA insulators)- Conductive as aqueous and liquids because the ions
dissociate and are removed from crystal lattice structure (allows e- flow)
- NOT conductive as solids because crystal lattice is rigid and does not allow e- flow.
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●Bonds that form by sharing a pair of electrons between atoms
●Forms between two nonmetals
Covalent Bonds
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●Multiple Bonds – occur in covalent compounds when atoms share more than one pair of electronsDouble Bond – atoms share 2 pairs of electrons
Triple Bond – atoms share 3 pairs of electrons
Multiple Covalent Bonds
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●The more bonds between 2 atoms, the stronger the bond●The more bonds between 2 atoms, the shorter the length of the bonds
Bond Strength
Single Bond < Double Bond < Triple Bond
Bond Length
Single Bond > Double Bond > Triple Bond
Bond Strength vs. Bond Length
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Properties of Molecular Compounds (Covalent Bonds)- Solids, liquids, or gases at room temperature- Low melting and boiling points (weaker bond than ionic)- Poor electrical conductors in ALL phases (solid, liquid, gas,
aqueous)- No mobility of electrons to other molecules
- Some molecular compounds are polar, some are nonpolar- Polar molecular compounds dissolve in water- Nonpolar molecular compounds don’t - More info on polarity to come!
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● When metal atoms come together, they can bond!● Metallic bond – bond formed between positive metal
cations and the “sea” of negatively charged delocalized electrons surrounding them◦ Delocalized electrons – electrons that move freely from one
cation to another in a metal structure
Metallic Bonds
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● This free-flowing “sea” of electrons between metal ions helps to explain the ability of metals to conduct electricity and heat
Metallic Properties
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Properties of Metallic Bonds- Solids at room temp (Hg is a liquid)- Malleable: able to be hammered or pressed out of shape without breaking
or cracking- Ductile: Able to be drawn out into a thin wire
- The malleability/ductility of metallic compounds is due to the sea of electrons (Different from ionic bonds because it is not a rigid bond)
- Melting/Boiling Point, Hardness, and Bond strength are variable- Generally weaker than a covalent bond, but not always