QUESTIONS RELATE TO: HYDROCODONE
1. A.) Draw the expanded structural formula of HYDROCODONE (showing all atoms
and all covalent bonds).
If it contains atoms other than C or H add lone pairs of electrons to each until the octet rule is satisfied for that atom.
B.) Determine molecular geometry of each central atom.
C.) For each central atom decide if it is polar or non polar.
2. Illustrate all ways that hydrocodone molecule could form hydrogen bonds with water. Do this by drawing bent water molecules as necessary and use dashed RED lines (---) to show H-
bonding between water and the appropriate atom in the molecule. Be very clear which atoms on each molecule are involved in the hydrogen bonds.
Hydrogen bonds from water can only from to the polar parts of your molecule.
If your drug molecule is not capable of forming hydrogen bonds with water, fully explain why
not.
3. Calculate the molar mass hydrocodone (C18H21NO4) to the hundredth’s place
using the molar masses from the periodic table (include units). Clearly show the work for your molar mass calculation below.
4. Calculate how many molecules of hydrocodone are in 200.0mg.
You wish to prepare 50.0 mL of 2.30 x 10^2 M solution of your drug.
5. Calculation. (hint- how many grams will you need of hydrocodone?)
6. Describe how to prepare this solution from the pure drug and deionized water.
Analytical balances and volumetric flasks are available to you. (Assume that your
drug dissolves in water, at least to the extent necessary for this problem.) Use
complete sentences in your description of the solution preparation process.
7. A patient is given 2.0mL of a 3.00% (m/v) solution of hydrocodone, how many milligrams
did they receive?
8. What is the molarity of a 3.00% (m/v) solution of hydrocodone?
7)
3.00% m/v solution contains = (mass / volume of solution)*100
Thus in 2.0mL solution mass of hydrocodone = (3/100)*2.0 = 0.06 g = 60 mg
Thus patient received 60 mg of drug.
8)
The number of moles of hydrocodone = 0.06g / 299.4g/mol = 2.004*10^-4 mol
this is number of moles in every 2.0mL
then for 1000mL the number of moles = (1000*2.004*10^-4)/2 = 0.1002 moles
So the molarity of the solution is = 0.1002 M = 0.100 M 3 sig. fig.
QUESTIONS RELATE TO: HYDROCODONE 1. A.) Draw the expanded structural formula of HYDROCODONE (showing all atoms...
Step 6: Hydrogen Bonding with Water (3) Hydrocodone Directions: Draw the structure of your molecule on a separate page. Illustrate all ways that your molecule could form hydrogen bonds with water. Do this by drawing bent water molecules as necessary and use dashed RED lines (---) to show H-bonding between water and the appropriate atom in the molecule. Be sure that it is very clear which atoms on each molecule are involved in the hydrogen bonds. Keep in mind that...
Step 5: Polarity and Solubility Predictions (4) Hydrocodone Directions: 1) Draw your molecule (or print out the line structure) on a separate page. 2) For each central atom in your molecule, decide if it is polar or nonpolar. 3) For those central atoms that are polar, a. Color the central atom RED if it forms hydrogen bonds b. Color the central atom GREEN if it forms dipole-dipole interactions 4) Make a reasonable prediction stating whether your molecule will be soluble...
The drug is hydrocodone. Step 4: VSEPR Molecular Geometry Predictions (4) Directions: 1) Show the expanded structure (draw all the bonds and lone pairs) of your drug on a separate page. 2) Determine the molecular geometry of each central atom. 3) Color each central atom based on its molecular geometry and include a key for your colors. For example, color tetrahedral C's red, trigonal planar C's, blue, etc.
Name Gdderall Hydrogen Bonding with Water- Your Drug Directions: Show the structure of your molecule below. Ilustrate all ways that your molecule could form hydrogen bonds with water, either as a hydrogen donor or as a target (receiver) of hydrogen bonds from water. Do this by drawing bent water molecules as necessary and representing hydrogen bonds between water and the drug using dashed RED lines are involved in the hydrogen bonds. If your drug molecule is not capable of forming...
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please answer all numbered and lettered questions Chapter 2 & 3 1. Atoms and structure of an atom. For an atom it is the smallest unit of matter, and 2. Valence electrons a. Be able to draw the Lewis dot structure for a given atom or ion 3. Atomic number and atomic mass to determine the number of proton, neutrons and electron a given ator ion, isotope. a. Example: Natl. atomic number 11, 11 p+, 11 n°, 10 e- b....
Name Solution Calculations Directions: Clearly show the setups for your calculations. 1. You wish to prepare 50.0 mL of 2.30x 102 M solution of your drug. Describe how to prepare this solution from the pure drug and deionized water. Analytical balances and volumetric flasks are available to you. (Assume that your drug dissolves in water, at least to the extent necessary for this problem.) Use complete sentences in your description of the solution preparation process. Show any required calculations you...
A covalent bond is a bond in which electrons are shared between atoms of elements. A covalent bond can be polar or nonpolar. In a nonpolar covalent bond, the bond is between two identical atoms and the electrons are evenly shared between the atoms.In contrast, in a polar covalent bond, the bond is between two nonidentical atoms and the electrons are unevenly shared between the atoms. The uneven sharing of electrons takes place because of the difference in the electronegativity...
Solution Calculations for Celecoxib / C17H14F3N3O2S Directions: Clearly show the setups for your calculations. 1. You wish to prepare 50.0 mL of 2.30 x 10–2 M solution of your drug. Describe how to prepare this solution from the pure drug and deionized water. Analytical balances and volumetric flasks are available to you. (Assume that your drug dissolves in water, at least to the extent necessary for this problem.) Show any required calculations you would need to make. 2. Calculate how...