Valence bond Theory
How are sigma and pi bonds different
sigma bonds are stronger and result from end to end overall and single bonds are sigma bonds
pi bonds between two atoms are weaker because they result from side-by-side overlap, and multiple bonds contain one or more bonds
Give the shape that describes each hybrid orbital set:
sp2, sp3d
trigonal planar, trigonal bipyramidal
What is the total mass of carbon in CH4
12.01amu
what is molarity
unit of concentration, defined as the number of moles of solute dissolved in 1 liter of solution
How many sigma and pi bonds are present in the molecule HCN?
2 sigma, 2 pi
Why is the concept of hybridization required in valence bond theory?
Hybridization is introduced to explain the geometry of bonding orbitals in valance bond theory.
what is the total mass of C in C10H10O6 ?
144.12amu
Determine the molarity of 0.444 mol of CoCl2 in 0.654 L of solution
0.679M
Use valence bond theory to explain the bonding in O2. Sketch the overlap of the atomic orbitals involved in the bonds in O2.
Bonding: One σ bond and one π bond. The s orbitals are filled and do not overlap. The p orbitals overlap along the axis to form a σ bond and side-by-side to form the π bond.
What is the hybridization of the central atom in SF6?
sp3d2
what is the molecular formula for Si2Cl4H2
199.9976amu
What is the molarity of KMnO4 in a solution of 0.0908 g of KMnO4 in 0.500 L of solution?
1.5 x 10-3 M
Draw the Lewis Structures for CO2 and CO. predict # of sigma and pi bonds for each molecule.
CO2: 2 sigma, 2 pi (2 double bonds)
CO: 1 sigma, 2 pi (triple bond)
Explain why a carbon atom cannot form five bonds using sp3d hybrid orbitals.
There are no d orbitals in the valence shell of carbon.
Calculate the molecular formula mass of Ca(NO3)2
164.086amu
Determine the molarity of 20.54 g of Al(NO3)3 in 1575 mL of solution
0.06123 M
A friend tells you N2 has three pi bonds due to overlap of the three p-orbitals on each N atom. Do you agree?
N2 is triple bonded. No, two of the p orbitals will be oriented end-to-end and will form a sigma bond.
Write Lewis structures for NF3 and PF5. Explain the fact that NF3, PF3, and PF5 are stable molecules, but NF5 does not exist.
Phosphorus and nitrogen can form sp3 hybrids to form three bonds and hold one lone pair in PF3 and NF3, respectively. However, nitrogen has no valence d orbitals, so it cannot form a set of sp3d hybrid orbitals to bind five fluorine atoms in NF5. Phosphorus has d orbitals and can bind five fluorine atoms with sp3d hybrid orbitals in PF5.
calculate the molecular formula mass of
C12H22O11
Calculate the number of moles and the mass of the solute in 325 mL of 1.8 x 10-6 M FeSO4
5.9 x 10-7 mol FeSO4, 8.9 x 10-5 g FeSO4