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Synthesizing an Ionic Compound. 2Na(s) + Cl 2 (g) 2NaCl (s). Explaining Salt Formation using the Born-Haber Cycle. Explaining Salt Formation using the Born-Haber Cycle. Na(s) + Cl 2 NaCl H° f = -411 kJ/mol. Na(s) Na(g) H° f = 108 kJ/mol. - PowerPoint PPT Presentation
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2Na(s) + Cl2Na(s) + Cl22 (g) (g) 2NaCl (s) 2NaCl (s)
Synthesizing an Synthesizing an IonicIonic Compound Compound
Explaining Salt Formation using the Explaining Salt Formation using the Born-HaberBorn-Haber Cycle Cycle
Na(s) + Cl2 NaCl H°f = -411 kJ/mol
Na(s) Na(g) H°f = 108 kJ/mol
Cl2 Cl(g) H°f = 122 kJ/mol
Na(g) Na+(g) + e- I1 = 496 kJ/mol
Cl(g) + e- Cl-(g) E = -349 kJ/mol
H = [H°f (NaCl)] - [H°f (Na+) + H°f (Cl-) + I1 + E]
H = -788 kJ/mol
Explaining Salt Formation using the Explaining Salt Formation using the Born-HaberBorn-Haber Cycle Cycle
Describing Electrostatic Attraction and Repulsion
E = kQ1Q2
d
E > 0 if the charges Q1 and Q2 have the same sign•Potential energy increases because the particles are repelling
E < 0 if the charges Q1 and Q2 have different signs•Potential energy decreases because the particles are attracting
The lattice energy of NaCl is the result of all the electrostatic repulsions and attractions. Because the attractions outweigh the repulsions, the lattice energy is positive and large
E = kQ1Q2
d
Sizes of Ions•size depends upon nuclear charge
•size depends upon numbers of electrons•size depends upon orbitals in which the outer electrons reside
Within an Isoelectric Series, the higher the atomic numberthe smaller the ion
Covalent Bonds are formed by shared pairs of electrons
H H+ H H H H
Cl Cl+ Cl Cl Cl Cl
Single Bonds
Double Bonds
O O+ C + O OC O OC
Triple Bonds
N N+ N N
Resonance Forms
OO
O OO
O
•Molecules with an odd number of electrons
•Molecules in which an atom has less than an octet
NO contains 5 + 6 = 11 electrons. No octet can be established
Though rare, these are most often encountered in compoundsof Born and Beryllium
B
FF
F
Exceptions to the Octet Rules
Molecules in which an atom has more than an octetThis is observed in compounds constructed from period 3 elements and beyond
PCl
Cl
Cl
Cl
Cl
3s 3p 3d
Exceptions to the Octet Rules
Strengths of Covalent Bonds
Bond dissociation Energy (Bond Energy): is the enthalpy change (H) required to break a particular bond in a mole of gaseous substance
(g) Cl Cl Cl2 (g) H = 242 kJ
Bond Energies and the Enthalpy of Reactions
H = (bond energies of bonds broken) - (bond energies of bonds formed)
H = (bond energies of bonds broken) - (bond energies of bonds formed)Cl2(g) + H-CH3 H-Cl(g) + CH3Cl
H = [(Cl-Cl) + 4(H-C)] - [(Cl-Cl) + 3(H-C) + (Cl-C)] H = [242 kJ+4(413 kJ)]-[431 kJ + 4(413kJ) + (328)] = -104 kJ
Bond Strength and Bond Length
Electronegativity and Bond Polarity
“the ability of an atom in a molecule to attract electrons to itself”
Electronegativity and Bond Polarity
H2 : Ediff = 2.1 -2.1 = 0
HCl: Ediff = 3.0 -2.1 = 0.9
Cl2 : Ediff = 3.0 - 3.0 = 0
note that LiF is ionic : Ediff = 4.0 - 1.0 = 3.0
H Cl
H Cl+ -
BH3 2.1-2.0 = .1
Ionic Character The bigger the electronegativity difference
the more ionic character. 1.4 has more ionic character than 1.2
noble gas configurations
Cl1-
Na1+
Cu1+
Sn2+
Isoelectronic O2-, Cl1-, Ne, Na1+, Mg2+
size trend
energy diagram page 366