Bonding. Types of Bonds Ionic Covalent Metallic Metallic Bonds Electrons are shared by many atoms...
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Transcript of Bonding. Types of Bonds Ionic Covalent Metallic Metallic Bonds Electrons are shared by many atoms...
![Page 1: Bonding. Types of Bonds Ionic Covalent Metallic Metallic Bonds Electrons are shared by many atoms Electrons free to move Two or more metals.](https://reader038.fdocuments.net/reader038/viewer/2022110321/56649f465503460f94c684cc/html5/thumbnails/1.jpg)
Bonding
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Types of Bonds•Ionic
•Covalent
•Metallic
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Metallic Bonds•Electrons are shared by many atoms
•Electrons free to move
•Two or more metals
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Metallic Compounds•Generally high MP
•Hard & lustrous
•Less brittle
•Conductors
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Metallic Bonds•No debate about metallic bonds
•Easy to identify
•Will not be discussed
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Ionic Bonds•Electrons are transferred from one atom to another creating (+) & (-) ions
•Metal & nonmetal
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Ionic Compounds•Held together by electrostatic charge
•Very high MP
•Brittle
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Covalent Bonds•Electrons are shared by two atoms
•Two nonmetals
•Weaker than ionic
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Covalent Compounds•Low MP
•Two nonmetals
•Flexible
•Some exceptions
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Network Covalent or
Macromolecules•VHMP
•Extremely hard
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Molecule•Any compound
that can exist as an entity by itself
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Distinguishing Bonds•Distinguishing ionic & covalent bonds can be difficult, but generally determined by differenceelectronegativity
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Bonds Types•Ionic
•Polar covalent
•Non polar covalent
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Bond Types• Ionic: EN > 2.0
• Covalent: EN < 2.0
• Polar Covalent: 0.5<EN<2.0
• Non polar covalent :EN< 0.5
• Nothing is absolute
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Coordinate Covalent Bonds
•A covalent bond in which the two
electrons are donated by one atom
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Coordinate Covalent Bond
H3N: BF3
H3N-BF3
H3N BF3
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Dipole•Polar bonds
•Polar molecules
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DipoleH F+ -
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Ionic Bonding
-
+
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Covalent Bonding
Occurs when electron orbitals
overlap
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OrbitalsOn the board
Max 2 e- per orbital
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Hybridization•When s, p, and/or d orbitals (electron clouds) mix to make a new type of multi-lobed orbital
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Hybrid Orbitals•sp dsp3
•sp2 d2sp3
•sp3
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Electron Cloud Repulsion
• In molecules each electron cloud repels other clouds enough to spread as far apart as possible
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VSEPR•Valence Shell Electron Pair Repulsion
•Electron pairs repel each other to spread out as much as possible
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Bonding OrbitalsType Hybrid VSEPR• 2 lobes sp AX2
• 3 lobes sp2 AX3
• 4 lobes sp3 AX4
• 5 lobes dsp3 AX5
• 6 lobes d2sp3 AX6
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VSEPR Orbitals
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Bonding Orbital Shape• 2 lobes: Linear 180o
• 3 lobes: Trigonal planar 120o
• 4 lobes: Tetrahedral 109.5o
• 5 lobes: Hexahedral 120&180o
• 6 lobes: Octahedral 90&180o
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Draw the Bonding Electron Dot
Diagrams for Each Element
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Bonding Electron Dot Diagrams
•Electron dot diagrams that go through 4 singles before any electrons are paired up
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1A: 1 single2A: 2 singles3A: 3 singles4A: 4 singles 5A: 1 pair & 3 singles6A: 2 pair & 2 singles7A: 3 pair & 1 single8A: 4 pair
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Drill: Equate each of the following:
sp3 AX2 2 lobes
sp AX3 4 lobes
dsp3 AX4 6 lobes
sp2 AX5 3 lobes
d2sp3 AX6 5 lobes
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Lewis Dot Diagrams
•Representation of valence electrons and bonds in a molecule or polyatomic ion
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Drawing LDDsDraw the bonding electron dot
diagram for each element in the molecule with the element with the most unpaired e- near the center
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Drawing LDDs• If there is more than one carbon, connect the carbons by connecting single dots between one carbon & another
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Drawing LDDs• Connect a single dot on
one atom to a single dot on another (never two on the same atom)(never connect one dot to more than one other dot)
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Drawing LDDs•Repeat connecting the dots until all singled dots are connected making sure to obey the octet rule if possible
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Drawing LDDs• Recognize polyatomic ions
•H2CO3: CO3-2 is a
polyatomic ion; thus, the three Os must connect to the C
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Drawing LDDs•Redraw the molecule neatly making sure to include all dots
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Draw LDDs for:•BeCl2 H2O
•BF3 C2H6
•CH4 C3H6
•NH3 CH2O
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Drawing LDDs• Draw EDDs
• Connect Cs if multiple
• Connect single dots
• Recognize Polyatomic Ions
• Redraw neatly
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Draw LDDs for:
•H2C2O4
•C4H6
![Page 44: Bonding. Types of Bonds Ionic Covalent Metallic Metallic Bonds Electrons are shared by many atoms Electrons free to move Two or more metals.](https://reader038.fdocuments.net/reader038/viewer/2022110321/56649f465503460f94c684cc/html5/thumbnails/44.jpg)
Draw the LDD for:
C4H9NO2
C4H8N2O2
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Coordinate Covalent BondA covalent bond in which both electrons are donated by one
atom
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Draw LDDs for:
SO4-2
SO2
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Resonance Structures
Equally valid Lewis Dot Diagrams for molecules or polyatomic ions that have the same shape.
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OO N O
OO N O
-1 -1
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Draw LDDs:HNO3
C4H5NO
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Draw LDDs for:
•PH3 PO3-3
•KCN C4H8O
![Page 51: Bonding. Types of Bonds Ionic Covalent Metallic Metallic Bonds Electrons are shared by many atoms Electrons free to move Two or more metals.](https://reader038.fdocuments.net/reader038/viewer/2022110321/56649f465503460f94c684cc/html5/thumbnails/51.jpg)
Expanded Octets•Sometimes atoms can be surrounded by more than 8 electrons
• Columns 5A-8A
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If more atoms are bound to the central
atom than its unpaired electrons,
then split some paired electrons
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Example: 5 things bound to P
P P
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HintWhen drawing expanded LDDs for polyatomic ion, adjust the charge of the central atom
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Draw LDDs for:
•PH5
•SCl5-1
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Draw LDDs for:
•PO4-3 P2O7
-4
•K2SO4 C5H8O
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Draw LDDs for:BeH2 AlCl3 SO2
CF4 NH3 H2O
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Hybridizations
•sp 2 lobes
•sp2 3 lobes
•sp3 4 lobes
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Bond Angles
•sp ~180o
•sp2 ~120o
•sp3 ~109.5o
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Sigma Bonds()• End to end orbital overlap
• All single bonds are sigma bonds
• All multiple bonds contain one sigma bond
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Pi Bonds ()•Side by side orbital overlap
•Multiple bonds contain bonds
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Multiple Bonds•Double: 1 & 1
•Triple: 1 & 2
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Intermolecular Forces• Weak temporary
attractions between atoms from one molecule to another or another part of a larger molecule
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Intermolecular Forces
•Sometimes called:
• Van der Waals Forces
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Intermolecular Forces• Hydrogen-bond
• Dipole-dipole
• Dipole-induced dipole
• London dispersion forces
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Hydrogen Bond• Strongest of the
intermolecular forces
• Occurs when H is bound to one highly EN element & connects to another
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Dipole-Dipole•When two polar molecules connect
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Dipole-Induced Dipole
•When a polar molecule gets near a non-polar one, it induces the non-polar one to become polar; thus, they connect
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London Dispersion• Instantaneous attraction
for fractions of seconds in which non-polar molecules connect
• Very weak force
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Draw Lewis Dot Diagram for:
ICl5
Determine: bond s, hybridization, VSEPR, & shape
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Identify as ionic, covalent, or metallic bonds
Na-Cl Fe-CrS-Cl H-Cl
Mg-S C-CN-O Fe-Fe
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Draw LDDs for:
HONO H3PO4
CO2 C3H4O2
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Draw LDDs & Predict All for:
CF4 NH3
BF3 CO2
SeCl4 XeF4
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Draw LLDs & Predict All For:
H3PO4 ICl5
IF3 CO
SeCl4 C4H6O2
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Draw LDDs & predict VSEPR, Hybridization,
bond s, & shape of:
XeF4 SCl4
XeO4
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List & describe the four types of intermolecular
forces
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Draw Lewis Dot Diagrams of:
C4H5NO2