CHAPTER 8: BASIC CONCEPTS OF CHEMICAL BONDING Bond-an attractive interaction between two or more atoms. Bonding is the "glue" that holds molecules together. Two extreme types: Ionic (transfer) Covalent (sharing) Polar covalent is in between

LEWIS symbols are a method of using dots to represent VALENCE (those past noble gas core) electrons. #valence electrons=group number

Ionic Bond- the electrostatic attraction between a cation (metal) and anion (non-metal) resulting from transfer of an electron. Covalent Bond-an attractive force resulting from sharing of electron pairs (1-single bond, 2-double bond, or 3-triple bond).

Both try to achieve the Lewis octet (isoelectronic to noble gas) if possible. Illustrate Ionic bond in LiF using Lewis Symbols and equations, do the same for the covalent F2 . Look at Energetics of Ionic cpd formation (Born-Haber, Hess Law) MX(s) → M+(g) + X-(g) ∆Hlattice >0

Lattice E increases as charges on ions increases and as ion radius decreases

Electron Configuration of Ions are predicted by adding electrons (non-metals to give anions) or removing electrons (metals to give cations) from the electron

configuration of the neutral atom. Isoelectronic - Species which have the same electron configuration. Main Group Ions form to achieve an electron configuration isoelectronic to the noble gases. Transition Metals lose ns electrons before (n-1)d electrons

Periodic Properties -Atomic Size -Ion Size -Ionization Energy -Electron Affinity -Electronegativity Ion Size Trends -Cations are ALWAYS smaller than the metals from which they were formed -Anions are ALWAYS larger than the non-metals from which they were

formed

Covalent Bond-an attractive force resulting from sharing of electron pairs (1-single bond, 2-double bond, or 3-triple bond). Draw Lewis Structures of a) CH4, NH3, H2O, and HF b) NH4

+, and OH- c) F2, O2, N2, CO2, and HCN d) BeCl2, BCl3, PF5, SF6

Lewis Structures (p314) 1. Count up valence e-. # valence e- =Group Number Be sure to consider charge. 2. Arrange valence e- in pairs around central atom so that H has 1 pair and C, N, O, and F have 4 pairs (Lewis Octet). You may have to use double or triple bonds or nonbonding (lone pair)(s)- a pair of electrons located

on one atom. 3. Groups II and III (Be and B) cpds. may have less than a Lewis octet. 4. Elements beyond the 2nd period (P, S, Cl) may have more than a Lewis octet. (they have unused "d" orbitals which may participate in bonding) A Lewis structure by itself DOES NOT!!!!! Describe the shape of a molecule. It

simply accounts for the electron distribution. Exceptions to octet rule -odd electron species -less than an octet (Be, B) -more than an octet( 3rd period elements) Free Radicals are paramagnetic odd electron species that are very reactive and cannot satisfy Lewis Octet. Examples are NO, NO2, and Cl.

Draw Lewis structure of NO2

- Resonance structures - possible structures of a species that has more than one acceptable Lewis structure (these differ only in location of double or triple bonds). (horse and donkey) Resonance hybrid- a composite structure based

on the contributing resonance structures that approximates the true structure. (mule) Draw the resonance structures of CO3

2- and its resonance hybrid. Give the formal charge (FC) on each atom. (p316) FC=GN - # lone pair e � ½ # bonding e Exceptions to octet rule -odd electron species

-less than an octet (Be, B) -more than an octet( 3rd period elements) Bond Enthalpy- the energy required to break a bond (endothermic)

A-B →→→→ A + B Bond Length: triple < double < single

Bond Strength: triple > double > single

Single bonds are longer and weaker than double or triple bonds Use the data in Table 8.4 to

calculate the ∆H of the following reaction

H2 + Cl2 →→→→ 2HCl ∆H = sum of bonds broken-sum of bonds formed Charge distribution (even or uneven sharing?) Electronegativity - the ability of an atom in a molecule to attract a pair of electrons to itself. Increases left to right and

bottom to top. (F most electronegative)

Polar Bond - a bond between atoms of different electronegativities that results in unequal charge distribution.

Dipole Moment, µ, is a measure of the polarity of a molecule. A species is polar if: 1) it has polar bonds and 2) the arrangement of the polar bonds does not result in cancellation