guiding question: how does the type of bond relate to the properties of materials?
TRANSCRIPT
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Guiding Question:
How does the type of bond relate to the properties of materials?
Quarter 3-Unit 2Five Types of Bonds!
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Ionic Polar Covalent Non-polar Covalent Metallic Network Covalent
You will need to recognize which is which by looking at the formula.
You will need to know the properties of the five types including:◦ appearance/texture◦ melting point◦ Conductivity◦ solubility.
What are the five types of bonds you will need to know?
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Put “bond types and properties” in the middle
Put the five types of bonds around the outside
Start your popplet!
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You need to look at the formula to see if the compound contains metals or non-metals or both.
Recognizing Bond Type from the formulas!
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Contain at least one metal and one non-metal.
May contain a polyatomic ion.
Examples:
◦ CuO
◦ Na3P
◦ CaCO3
Ionic Compounds (transfer electrons from metal to non-metal)
METAL
NON-METAL
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Ionic compounds are also called SALTS.
Most are white crystals.
They are hard and brittle solids.
Appearance of Ionic Compounds
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Include how to recognize ionic compounds from the formula
Include appearance and textures.
Add to your popplet!
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First let’s remember how to decide if it’s covalent or not.
Then use the Lewis structure to know if it’s polar or non-polar.
Covalent Compounds can be polar or non-polar.
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Contain ONLY non-metals.
Examples:
◦ CH4
◦ H2O
◦ NH3
Covalent Compounds(share electrons)
ALL NON-METALS
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Polar molecules are ASSYMETRICAL – not balanced.
Use Lewis Structure:◦ Unshared pairs make
it assymetrical (pyramid or bent)
◦ Different atoms around the central atom also make it assymetrical.
Polar Covalent Molecules – electrons are unequally shared;one side is slightly positive and one is slightly negative.
H2O is a bent molecule so it is Assymetrical and POLAR
CH3Cl is polar
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Non-Polar molecules are SYMETRICAL – balanced.
Use Lewis Structure:◦ No unshared pairs
◦ Same atoms surround the central atom.
Non-Polar Covalent Molecules – electrons are equally shared;there is no charge difference on each side of molecule
CO2 is a linear molecule so it is Symetrical and NON-POLAR
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Some polar and non-polar covalent molecules
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More examples of polar and non-polar covalent molecules
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Soft solids, liquids, or gases at room temp.
Polar and non-polar covalent molecules are usually…
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Include how to recognize covalent compounds from the formula
Include appearance and textures.
Add to your popplet!
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Formula will contain one metal.
Example:
◦ Cu
◦ Fe
◦ Ag
◦ Al
Metallic Bonds – bonds within metals
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Metallic BondsIn ionic bonding we know metals lose electrons to form positive ions M+ M is any
metalM2+or
This is to achieve a completely full outer electron shell
This also happens in metallic bonding
- but because there are no non-metals to take the electrons, now the electrons have nowhere to go!
e-
e-
e-
e-
The valence electrons get passed from one atom to the next like a “hot potato”!This forms a “sea of negative charge” that flows around the positive metal ions.
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M+M+M+ M+M+M+M+M+M+
M+M+M+ M+M+M+M+M+M+
M+M+M+ M+M+M+M+M+M+
M+M+M+ M+M+M+M+M+M+
M+M+M+ M+M+M+M+M+M+
M+M+M+ M+M+M+M+M+M+
Sea of electrons
How metallic bonding worksValence electrons move around holding the + metal ions in place
How might this structure lead to some of the properties we know about metals?
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Shiny and malleable (bendable)
Metals are usually…
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Include how to recognize metallic compounds from the formula
Include appearance and textures.
Add to your popplet!
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You need to remember:
DIAMOND and SAND are network covalent solids.
Diamond will be written:
C – Diamond
◦ Sand is SiO2
Network Covalent Solids
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Network Covalent Solids
In some substances, millions of atoms join together by covalent bonding. This produces giant covalent structures, not molecules.
Each atom is linked to every other atom in the structure which makes them VERY strong.
This also means that almost all giant covalent structure are hard and NOT brittle (don’t crack easily).
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Diamond- a form of carbonDiamond is a rare form of carbon in which each atom is covalently bonded to four others.
This pattern arrangement is repeated millions of times to create a giant lattice.
C
C
CC
C
This makes diamond VERY hard and strong.
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Diamond coated drill bit!
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Sand – a form of Silicon Dioxide (a network covalent solid)
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Include how to recognize network covalent molecules
Include appearance and textures.
Add to your popplet!