Bonds
(EN)ergy
Lewis
surprise me!
VESPR & hybrids
100
Select the strongest bond:
a) N=C
b) N≡N
c) N-O
d) N-S
e) N-F
N≡N
100
Select the element with the highest electronegativity.
(a) Si
(b) P
(c) N
(d) O
(e) S
O
100
Draw the correct Lewis structure for Se
Se (6 v. electrons)
100
Of the bonds listed below, which is the strongest?
a) sigma bond
b) pi bond
c) single bond
d) double bond
e) triple bond
triple bond
100
A triple bond has ___ sigma bonds and ___ pi bonds.
1 sigma, 2 pi
200
Select the most polar bond:
a) C-N
b) B-Cl
c) B-F
d) C-O
e) N-O
B-F
200
Select the element with the lowest electronegativity:
a) Be
b) Ba
c) Al
d) Si
e) S
Ba
200
How many total shared electrons are around boron in BCl3?
(a) 8
(b) 7
(c) 6
(d) 3
(e) 5
3
200
The formal charges on Cl and O in the structure shown for the ClO- ion are...
0 and -1
200
A neutral molecule having the general formula AX4E2 will have what type of hybridization?
(spppdd) sp3d2
300
Which of the following properties is least characteristic of typical ionic compounds?
a) high melting point
b) poor electrical conductor when molten
c) high boiling point
d) brittleness
e) poor electrical conductor when solid
poor electrical conductor when molten
300
Select the compound with the highest lattice energy
(a) BaO
(b) NaI
(c) LiBr
(d) MgO
(e) CaS
MgO
300
Draw the best Lewis Structure for oxygen difluoride
:)
300
The electronic structure of the CO32– molecule is best represented as a resonance hybrid of
___ equivalent structures.
(a) (insert number)
OR
(b) This molecule does not exhibit resonance
3
300
DAILY DOUBLE:
Which of the following species is planar?
(a) NH3
(b) H3O+
(c) SO32–
(d) PF3
(e) NO3–
NO3–
400
List 5 covalent bond properties
1) weak intermolecular forces
2) poor electrical conductor in all states
3) low melting point
4) low boiling point
5) weaker than ionic bonds
400
DAILY DOUBLE:
Estimate the heat of reaction at 298 K for the reaction shown, given the average bond
energies below:
Br2(g) + 3F2(g) → 2BrF3(g)
-516 kJ
400
Which of the following are correct lewis structures?
(a) NO2 and NO
(b) NO2– and NO
(c) NO and N2O
(d) NO2– and N2O
(e) All of the above are correct structures
NO2– and N2O
400
What is the molecular structure and electron pair geometry of KrF2 ?
linear and trigonal bipyramidal
400
In which of the molecules below does the central atom have an sp3d orbital hybridization?
(a) SO42–
(b) H2O
(c) CH4
(d) XeF4
(e) XeF2
XeF2
500
Arrange the following bonds in order of increasing bond strength.
(a) C–I < C–Br < C–Cl < C–F
(b) C–F < C–Cl < C–Br < C–I
(c) C–Br < C–I < C–Cl < C–F
(d) C–I < C–Br < C–F< C–Cl
(e) None of the above orders is correct.
C–I < C–Br < C–Cl < C–F
500
Arrange oxygen, sulfur, calcium, rubidium, and potassium in order of decreasing
electronegativity.
(a) O > S > Ca > Rb > K
(b) O > S > Ca > K > Rb
(c) O > S > Rb > K > Ca
(d) O > S > Rb > Ca > K
(e) None of the above orders is correct.
O > S > Ca > K > Rb
500
Considering all the bonds in a molecule with trigonal bipyramidal geometry, what are the bond angle(s) present?
90, 120, and 180
500
Which of the following BEST describes the bonding found within solid Al2O3?
(a) Strong covalent bonds between atoms with similar electronegativities
(b) Covalently bound atoms arranged in small individual molecules.
(c) Electrostatic attractions between + and - charged ions
(d) Positively charged ions covalently bound with many mobile electrons
(e) None of these
Electrostatic attractions between + and - charged ions
500
Which of the following molecules and ions will have a square planar geometry as predicted by the VESPR theory?
a) PCl3
b) BF4-
c) XeF4
d) BrF5
e) H3O+
XeF4