Types of chemical bonds Bond: Force that holds groups of two or more atoms together and makes the atoms function as a unit. Example: H-O-H Bond Energy: Energy required to break a bond. Ionic Bond: Attractions between oppositely charged ions. Example: Na+ Cl-

Types of chemical bonds Ionic Compound: A compound resulting from a positive ion (usually a metal) combining with a negative ion (usually a non-metal). Example: M+ + X-  MX Covalent Bond: Electrons are shared by nuclei. Example: H-H Polar Covalent Bond: Unequal sharing of electrons by nuclei. Example: H-F Hydrogen fluoride is an example of a molecule that has bond polarity.

Lewis structures Lewis Structure: Representation of a molecule that shows how the valence electrons are arranged among the atoms in the molecule. Bonding involves the valence electrons of atoms. Example: Na● H-H

Lewis structures of elements Dots around elemental symbol Symbolize valence electrons Thus, one must know valence electron configuration

Lewis Structures of molecules Single Bond: Two atoms sharing one electron pair. Example: H2 Double Bond: Two atoms sharing two pairs of electrons. Example: O2 Triple Bond: Two atoms sharing three pairs of electrons. Example: N2 Resonance Structures: More than one Lewis Structure can be drawn for a molecule. Example: O3

Rules for Lewis structures of molecules Write out valence electrons for each atom Connect lone electrons because lone electrons are destabilizing Become two shared electrons Called a “bond” Check to see if octet rule is satisfied Recall electron configuration resembling noble gas In other words, there must be 8 electrons (bonded or non-bonded) around atom Non-bonded electron-pair Called “lone pair”

Let’s do some examples on the board Duet rule F2 Octet rule O2 N2

Lewis structures Example Write the Lewis Structure for the following molecules: H2O CCl4 Where does the carbon go & why? PH3 H2Se C2H6

Lewis structures continued C2H4 C2H2 SiO2

Polyatomic ions If positive charge on ion If negative charge on ion Take away electron from central species If negative charge on ion Add electron to central species Example: H3O+

Your turn NH4+ ClO- OH-

Resonance structures When structures can be written in more than one way O3 Actual molecule is “in-between” Resonance hybrid Another example HCO3- What would its resonance hybrid look like?

Practice NO2- NO3-

Practice H2O2 H3O+

Aberrant compounds Odd-electron species NO NO2

Aberrant compounds Incomplete octet BH3

Aberrant compounds Expanded octet Some central atoms can exceed an octet Third period and higher elements can do this E.g., Al, Si, P, S, Cl, As, Br, Xe, etc. d-orbitals can accommodate extra electrons

Examples AsI5 XeF2

Practice SCl6 XeF4

Practice SO32- PO33- SO2 SO3 H2SeO4

Electronegativity Electronegativity: The relative ability of an atom in a molecule to attract shared electrons to itself. Example: Fluorine has the highest electronegativity. Similar electronegativities between elements give non-polar covalent bonds (0.0-0.4) Different electronegativities between elements give polar covalent bonds (0.5-1.9) If the difference between the electronegativities of two elements is about 2.0 or greater, the bond is ionic

Electronegativity Example For each of the following pairs of bonds, choose the bond that will be more polar. Al-P vs. Al-N C-O vs. C-S

Dipole moment Dipole Moment A molecule that has a center of positive charge and a center of negative charge Will line up on electric field In Debye units 1 D = 3.34 x 10-30 C  m

Examples F2 CO2 H2O NH3 BF3 CCl4

Molecular polarity Net-dipole moment leads to molecular polarity Thus the following two that have net-dipole moments are polar: H2O NH3

Molecular structure Molecular Structure: or geometric structure refers to the three-dimensional arrangement of the atoms in a molecule. Bond Angle: The angle formed between two bonds in a molecule.

Molecular structure: VSEPR The VSEPR Model: The valence shell electron pair repulsion model is useful for predicting the molecular structures of molecules formed from nonmetals. The structure around a given atom is determined by minimizing repulsions between electron pairs. The bonding and nonbonding electron pairs (lone pairs) around a given atom are positioned as far apart as possible.

Molecular Structure: VSEPR Steps for Predicting Molecular Structure Using the VSEPR Model 1. Draw the Lewis structure for the molecule. 2. Count the electron pairs and arrange them in the way that minimizes repulsion (that is, put the lone pairs as far apart as possible). 3. Determine the positions of the atoms from the way the electron pairs are shared. 4. Determine the name of the molecular structure from the positions of the atoms.

Example Br2 CO2 CF4 PF3

Your turn NH4+ XeF4 AsI5 SF3 + I3 -