Chemistry 1210 Midterm 3:
Octet Rule –
Lattice Energy –
Bond polarity –
Dipole moment –
Formal Charge –
Resonance structures –
What kind of electron transfers occur in the formation of calcium fluoride from elemental calcium and elemental fluorine?
If you were to perform the reaction KCl(s) K+(g) + Cl-(g), would energy be released?
Arrange the ionic compounds NaF, CaI, and CaO in order of increasing lattice energy:
Create the Born-Haber Cycle for the formation of NaCl:
Draw the Lewis Structures for the following compounds:
How does the electronegativity relate to the polarity of a compound? Which molecule has a greater dipole moment: ClF and IF?
Consider the attractions and repulsions associated with the formation of a bond in a diatomic molecule. At some distance the attractive and repulsive forces are equal. What is true about this distance? If you want to learn more check out What kind of expansion diffusion spreads by contact?
a. The distance is less than the bond length
b. The bond enthalpy is zero.
c. The potential energy of the system is at a minimum. We also discuss several other topics like How do officers behave under preventive patrol?
d. The distance is much larger than the bond length. The atoms are far apart. Don't forget about the age old question of What is a superficial mycosis?
Draw the Lewis structures for the NCO- and predict which one would be the rarest according to formal charge:
What are the exceptions to the octet rule?
Two structural isomers are possible for the molecule C2H6O. One of these has an OH bond and the other does not. Sketch each molecule, then use provided bond enthalpy data to determine which molecule is the most stable.
Which of the following pairs will have the most similar electron affinity values?
a. Na and Na+
b. S and S2-
c. Be and Li
d. 39K and 41K
e. F- anion and Na+ cation
Select the molecule that is best described as having 1) very electronegative atoms, 2) zero dipole moment, and 3) a purely covalent bond.
c. None of these molecules
VSEPR Theory –
Bond dipole –
Valence-bond theory –
Fill out the table:
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Draw the orbital diagram for H2CO that is appropriate for carbon:
Molecular theory provides an explanation as to how O2 is paramagnetic. Compare the O22- anion with O2.
a. O22- has a weaker bond and is also paramagnetic.
b. O22- has a stronger bond. It is not paramagnetic.
c. O22- has a stronger bond and is also paramagnetic.
d. O22- has a weaker bond. It is not paramagnetic.
Applying molecular orbital theory, which pair is predicted to have the same bond order?
a. H2 and He2
b. H2 and He2+
c. He2- anion and He22+ cation
d. H2+ cation and He2- anion
How does valence bond theory describe the bonding in N2?
a. Two pi-bonds are formed using unhybridized p-orbitals. b. A sigma-bond is formed using s-orbitals.
c. One pi-bond is formed using an unhybridized s-orbital. d. A sigma-bond is formed using sp3 hyrbridized orbitals. e. Two pi-bonds are formed using sp hybridized orbitals.