CHEMICAL BONDING. Why do bonds form? To complete the valence or outer energy level Octet Rule – 8...
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Transcript of CHEMICAL BONDING. Why do bonds form? To complete the valence or outer energy level Octet Rule – 8...
![Page 1: CHEMICAL BONDING. Why do bonds form? To complete the valence or outer energy level Octet Rule – 8 is great! A bond forms when 2 atoms attract the same.](https://reader035.fdocuments.net/reader035/viewer/2022081513/5697bfd11a28abf838cab169/html5/thumbnails/1.jpg)
CHEMICAL BONDING
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Why do bonds form?
•To complete the valence or outer energy level
•Octet Rule – 8 is great!
•A bond forms when 2 atoms attract the same electron or electron pair
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Bond Characteristics• Attractive Forces pull atoms together:
- (+ ) Nucleus of one atom attracts (–) electrons of another atom
- Opposite charges attract = ELECTROSTATIC ATTRACTION
• Bond Energy- When bonds form Energy is released = Exotherimc- When bonds break Energy is absorbed = Endothermic- When 2 atoms are held together by a chemical bond they
are at a LOWER energy condition than when they are separate!
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Bond Characteristics (cont.)
• Bond Stability- Compounds with LOW energy are STABLE- Compounds with HIGH energy are UNSTABLE- Chemical Change = the rearrangement of atoms to form low
energy and stable compounds
• Bond Strength- Weak Bond – when a small amount of energy is released- Strong Bond – when a large amount of energy is released
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In nature:
• Exothermic reactions are favored (bond formation)
UNSTABLE STABLEREACTIVE UNREACTIVEHIGH ENERGY LOW ENERGYWEAK BOND STRONG BOND
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Electronegativity – Table S
•An atom’s ability to attract electrons•Highest EN value = 4.0 = Fluorine (non-metal)•Lowest EN value = 0.7 = Francium (metal)•The difference in EN values of two bonded atoms can tell you the bond type
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ELECTRONEGATIVITY DIFFERENCE AND BOND TYPE
If the EN Difference is between:
4.0 – 1.7 1.6 – 0.2 0.1 – 0.0Ionic Bond Polar Covalent Non-Polar Covalent
Examples:BaO CH4 Cl2
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BOND TYPES
• Ionic•Covalent:
- Polar Covalent - Non-Polar Covalent- Coordinate Covalent
•Metallic
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Ionic Bonds
• Electrons are TRANSFERRED from one atom to another• Transfer from a metal to a nonmetal• Metals lose electrons to the nonmetals (gain e-)• High EN Diff. – the greater the difference, the stronger the ionic
character• Form ionic solids called Ionic Crystals (crystal lattice)
• Example: Which of the following has the strongest ionic bond?MgO NaCl LiF
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Characteristics of Ionic Compounds
• High Melting Point• High Boiling Point• Conducts electricity when dissolved in solutions• Does not conduct electricity in the solid phase!• Soluble in water• Forms crystals in solid phase
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Metal Hydrides
• Are ALWAYS IONIC• Occurs when Hydrogen bonds with a group 1 or 2 element• Examples: LiH NaH KH• H behaves as a nonmetal and is written second in the formula
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Covalent bonds
• When 2 atoms SHARE electrons in the same orbital• Possible to have single, double, triple bonds (1, 2, or 3 shared e- pairs)• Occurs between 2 nonmetals• Includes the Diatomic Molecules (B O FINCH)• 2 types of Covalent Bonds
1. POLAR Covalent – sharing of e- is uneven2. NONPOLAR Covalent – sharing of e- is even
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Polar Covalent Bonds
• There is an uneven distribution of + and – charges due an uneven sharing of electrons in the bond• EN Difference is between 0.2 – 1.6• Examples: HCl H2O
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Non-Polar Covalent Bonds
• Even distribution of + and – charges due to even sharing of electrons• EN Diff = 0.0 – 0.1• ALL Diatomic molecules have nonpolar covalent bonds
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Coordinate Covalent Bonds
• Occurs when only one atom contributes BOTH electrons in forming a bond• Occurs with the polyatomic ions (see Reference Table E)• Polyatomic Ions – 2 or more atoms that act as a single unit and have
one charge on the entire group• Ex. NH4
+ H3O+ NO3- SO4 -
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Characteristics of Molecular Substances• Can exist as solids, liquids, or gases• SOFT in the solid phase• Poor conductors of heat and electricity *Good
insulators• Low melting and boiling points• Does not dissolve in water• Soluble in Benzene or Ether (organic molecules)
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Network Solids
• In molecular solids, the the covalently bonded atoms are linked into a GIANT NETWORK throughout the entire solid• MACROMOLECULES• EXTENSIVE WEB OF COVALENT BONDS (3-D FISHNET)• Examples: Diamond, Silicon Dioxide, Asbestos• PROPERTIES:
- HIGH melting points- HARD solids- Poor conductors of heat and electricity
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Metallic Bonds
• Bonds between metal atoms• Valence electrons drift from atom to atom• “SEA OF MOBILE ELECTRONS”• Properties:
- Very malleable- Good Conductors of Heat and electricity- Has Luster- Tenacity
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Summary of Bond Types
Ionic Bonds• Metal – Nonmetal• Forms Crystal Compound• Exists as solids• EN Diff = 1.7 – 4.0
• High Melting/Boiling Pt• Conducts electricity when in solution• Soluble in water
Covalent Bonds• Nonmetal – Nonmetal• Forms Molecule• Exists as solids, liquids, gases• EN Diff = 0.2 – 1.6 Polar
0.1 – 0.0 NonPolar• Lo Melting/Boiling pt• Does not conduct electricity in solutions• Not soluble in water (dissolves in Benzene)
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Summary of Bond Types
Metallic Bonds• Metal – Metal
• Sea of Mobile Electrons• Good Conductors of Heat & Elec• Malleable, Luster• High melting/boiling points
Network Solids• Covalently bonded clusters of
atoms• Macromolecule• Poor Conductors of Heat & Elect• Hard Solids• High melting point
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ATTRACTIVE FORCES BETWEEN MOLECULESalso known as IMF’s – Intermolecular Forces• 2 TYPES OF MOLECULES
1. Polar Molecules – molecule has a (+) end and a (-) end- uneven or asymmetrical distributions of + -- Bond angle is less than 180 degrees
- also called DIPOLES Ex. H20, NH3, HCl
2. NonPolar Molecules – symmetrical, bond angle = 180 - All of the DIATOMIC MOLECULES - B O FINCH
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*Important Note*
• All molecules with polar covalent bonds are dipoles EXCEPT:CF4 CCl4 CO2
• A molecule can have polar covalent bonds but be a NONPOLAR molecule
• Example: Draw Lewis Dot Diagram of CCl4 (Carbon Tetrafluoride), CO2, H2O
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Attraction Between POLAR Molecules• Dipole-Dipole Attraction
- When + end of one molecule is attracted to the – end of another molecule- Very strong attraction gives a high boiling point due to energy needed to break the force of + - attraction
• Hydrogen Bond• NOT A BOND • Occurs when H is covalently bonded to an atom which has a
- Small atomic radius- Hi Electronegativity- H is bonded to N, O, F (NH3, H2O, HF)
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Non-Polar Force of Attraction
• WEAK attractive forces• Van der Waals Forces OR London Dispersion Forces• Occurs between: Diatomic Molecules (B O FINCH)
NonPolar MoleculesNoble Gases
*Force increases as they get closed together:Distance btwn molecules decreases ORSize of molecules increases
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Molecule – Ion Attraction
• EXAMPLE: NaCl dissolves in H2O• Hydration of the ions• Draw diagram