Bonding

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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 DEN gt 2.0
• Covalent DEN lt 2.0
• Polar Covalent 0.5ltDENlt2.0
• Non polar covalent DENlt 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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Dipole
H F d d-
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Ionic Bonding
-

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Covalent Bonding
Occurs when electron orbitals overlap
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Orbitals
On 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 120180o
• 6 lobes Octahedral 90180o

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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 single 2A 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 LDDs
Draw 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

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Draw the LDD for
C4H9NO2 C4H8N2O2
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Coordinate Covalent Bond

• A 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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O O N O
O O N O
-1
-1
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Draw LDDs
HNO3 C4H5NO
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Draw LDDs for

• PH3 PO3-3
• KCN C4H8O

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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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Hint
When 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(s)

• End to end orbital overlap
• All single bonds are sigma bonds
• All multiple bonds contain one sigma bond

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Pi Bonds (p)

• Side by side orbital overlap
• Multiple bonds contain p bonds

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Multiple Bonds

• Double 1 s 1 p
• Triple 1 s 2 p

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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-Cr S-Cl H-Cl Mg-S C-C N-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