Chapter 3 Flashcards
(26 cards)
Within one principal energy level, which subshell has the least energy?
- s
- p
- d
- f
s
Which of the following compounds possesses at least one sigma bond?
- CH4
- C2H2.
- C2H4.
- All of the above.
All of the above.
A carbon atom participates in one double bond. As such, this carbon contains orbitals with:
- Hybridization between the s-orbital and one p-orbital..
- Hybridization between the s-orbital and two p-orbitals.
- Hybridization between the s-orbital and three p-orbitals.
- Unhybridized s character.
Hybridization between the s-orbital and two p-orbitals.
The hybridization of the carbon and nitrogen in CN- are:
sp and sp.
What hybridization does the Be atom in BeH2 assume?
sp.
Two atomic orbitals may combine to form:
- A bonding molecular orbital.
- An antibonding molecular orbital.
- Hybridized orbitals.
- All of the above.
All of the above.
What is the maximum amount of electrons a single molecular orbital can contain?
two electrons.
Pi bonds are formed by which of the following orbitals?
- Two s-orbitals.
- Two p-orbitals.
- One s and one p orbital.
- Two Sp2-hybridized orbitals.
Two p orbitals overlap side to side.
The four C-H bonds of CH4 point toward the vertices of a tetrahedron. This indicates that the hybridization is:
- sp.
2 sp2. - sp3
- sp3d
sp3.
Why is a single bond stronger than a pi bond?
s-orbitals have more overlap than p-orbitals.
The p character of the carbon atom in HCN is:
50% p 50% s
A resonance structure describes:
a potential arrangement of electrons in a molecule.
An electron is known to be in the n = 4 shell and the l = 2 subshell. How many possible combinations of quantum numbers could this electron have?
10
Which is stronger - single bond or triple bond?
Triple.
Azithumal quantum number (l) :
Describes the subshells. Where 0 = s subshell, 1 = p subshell, 2 = d subshell, and 3 = f subshell.
Principle quantum number (n)
A measure of size. Can be any positive integer. The larger the number, the further away the shell is to the nucleus.
Magnetic quantum number:
Ranges from -l to +l and is used to describe orbitals.
Spin quantum number(ms):
Describes the number of electrons in an orbital, which is always two. So this will always equal + or - 1/2.
If the wave function of two atomic orbitals are of the same charge, what kind of orbital will be produced?
A bonding orbital.
The equation for specific rotation:
Observed rotation/ (Concentration * path length).
The following is constant for a given molecule at any temperature, solvent, and wavelength:
a. Optical activity.
b. Specific rotation.
c. Observed rotation.
d. Concentration.
Specific rotation.
Observed rotation is dependent on:
The concentration of the solution and the distance that light travels through the solution.
If a solution is diluted with water, what will occur to the specific and observed rotation of the molecules in the solution?
The specific rotation remains constant, and the observed rotation will decrease.
Henderson - Hassleback equation:
PH = pKa + log(A/HA)
A = conjugate base
HA = weak acid.
