BONDING. Bonds Between Atoms Covalent Ionic Molecules Network Metallic.
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Transcript of BONDING. Bonds Between Atoms Covalent Ionic Molecules Network Metallic.
![Page 1: BONDING. Bonds Between Atoms Covalent Ionic Molecules Network Metallic.](https://reader035.fdocuments.net/reader035/viewer/2022062304/56649ca35503460f94963ba0/html5/thumbnails/1.jpg)
BONDING
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Bonds Between Atoms
Covalent
Ionic
MoleculesNetwork
Metallic
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Metallic Bonding
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Metals lose their outer electrons easily and become cations
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creating a “sea” of electrons to roam freely around the metal cations.
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The strong electrostatic attraction between cations and roaming electrons explains why:
• metals conduct electricity• are extremely strong and
hard to break• Can be bent and stretched• Have high melting points
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Malleable and Ductile
The mobile electrons will shift to adjust to new arrangements around positive ions. They act as the "glue".
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Ionic Bonding
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Ionic Bonds
- results from the TRANSFER of electrons from a metal to a non-metal
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Ions are held strongly by electrostatic forces in a 3D lattice
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Properties
1.Have high melting points because of strong electrostatic attractions between cations and anions
2.Soluble in water
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3. Conducts electricity if dissolved in water (has free ions) but not in solid state
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4. Brittle – similar ions can repel when disturbed
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Covalent Molecules
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Covalent Molecular
- When 2 or more non-metals SHARE electrons; no charged ions are formed
- Does NOT form large lattices
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- forms small, neutral molecules that are weakly attracted to other molecules
Forces
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Properties:
1.Weak forces between molecules means that it has low melting points.
2.Does not conduct electrical current
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Covalent Network
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Covalent Network Solids
•when either carbon or silicon atoms are bonded covalently to form an infinite 3-D lattice
•network solids are extraordinarily strong
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Diamond
•Each Carbon atom bonds to 4 others
•Strong covalent bonds throughout
•High melting points
•does not conduct electricity.
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Silicon Dioxide: Sand & Quartz
• SiO2