For the two compounds below, use chemical structure and
intermolecular forces to predict which compound would exhibit
greater solubility in water. Use thermodynamics of dissolution in
water to frame your answer.
A molecule can be soluble in water for mainly two reason 1st is if the molecule get stabilised by larger no of hydrogen bonding i.e. intermolecular hydrogen bonding & 2nd is due to polarity in the molecule which gets stability by polar molecule H2O via solvation. Here 1st molecule i.e. Ctechol will exhibit greater solubility in H2O reasons are following-
now from intermolecular forces point of view-Now
from chemical structure Catechol is more polar than O-cresol so
Catechol will be more soluble in polar solvent H2O than O-cresol
.
And also we can see in O-cresol it contains one hydrophobic methyl group which is not soluble in water but in Catechol instead of that methyl group there present hydrophilic OH group that is why also Cresol is more soluble.
For the two compounds below, use chemical structure and intermolecular forces to predict which compound would...
1.5 pts Question 24 Which of the following compounds would have the strongest intermolecular attractive forces ? CH3-NH-CH2-CH3 CH3-CH2-CH2-OH CH3-CH2-O-CH3 CH3-CH2-CO2H CO2 3.5 pts D Question 25 A 0.258-g sample of a pure triprotic acid, H3A, (where A is the generic anion of the acid). was dissolved in water and titrated with 0.150 M barium hydroxide solution. The titration required 13.9 mL of the base to reach the equivalence point. What is the molar mass of the acid? o 227...
Identify the strongest intermolecular force in the compound KHSO4. O lonic forces Dipole-dipole Hydrogen bonding lon-dipole London dispersion forces What intermolecular force or bond is responsible for the density of solid water (ice) being less than that of liquid water? London dispersion forces O lonic bonding Covalent bonding Dipole-dipole forces Hydrogen bonding Which of the following compounds would have the strongest intermolecular attractive forces ? 0 CH3-NH-CH2-CH3 CH3-CH2-CH2-OH O CH3-CH2-O-CH3 O CH3-CH2-CO2H CO2 A 0.258-9 sample of a pure triprotic...
Chemistry 2 help with lab questions! Intermolecular forces are not chemical bonds. Explain the difference. When answering the rest of the essay questions, use language that clearly distinguishes between chemical bonds and intermolecular forces. Why do compounds with higher intermolecular forces have higher boiling points? Show that you understand why a higher temperature is needed to boil a compound that has stronger intermolecular forces. Which has greater dispersion forces, hexane or pentane? How can you use their molecular formulas to...
Question 25 6.67 pts The Lewis structure for a compound is shown below. Which intermolecular forces would you expect it to have? C. HHHH London dispersion, dipole-dipole, and hydrogen bonding forces London dispersion and dipole-dipole forces Dipole-dipole forces only London dispersion forces only
Re-draw the chemical structure of cinnamaldehyde (from the Reaction Scheme) and use it to answer the following solubility-based questions: 1. Circle and label all regions of the molecule that exhibit non-polar behavior. 2. Circle and label the region of the molecule that exhibits polar behavior. 3. Water prefers to interact with solute molecules with what type of intermolecular force (choose one answer): hydrogen bonding, dipole-induced dipole, or induced dipole-induced dipole (London dispersion)? 4. Based on the answers to parts (a)-(c),...
rank the molecules in the table from weakest to strongest
intermolecular forces and briefly justify the ranking.
temperature 310 20 time (s) 40 Fig. 10.1. Sample data for an evaporative cooling process. Before You Come to Lab Based on what you know about the relationship between the structure of a molecule and the strength of its intermolecular forces, rank the molecules in the table below in order from the weakest to the strongest intermolecular forces and briefly justify your ranking...
Discussion Questions The structures of acetanilide and malonic acid are provided below 1. For each structure, draw circles around the polar and nonpolar regions of the molecule, and label each circled regiorn with the type of intermolecular attractive force it can use to interact with other molecules. Acetanilide Malonic Acid но CH2 OH 2. Now-thoroughly explain (on the basis of polarity/nonpolarity and intermolecular attractive forces) how the acetanilide was separated from the malonic acid by recrystallization from water. And explain...
what IR absorption would you use to distinguish
between two compounds?which compound will
GUMUI =C_H | 3300 H 3300-3500 Nitrile C=N 2210-226 Alkyne C=C Amine C- 2100-2260 1030-1230 N Nitro NO 1540 a CH3-C-0-CH2CH3 and b CH3CH2CH2CHCHCH3 What IR absorption would you use to distinguish between the two compounds above? cm-1 Enter a frequency, or range as lower freq-higher freq, from the table above. Which compound will exhibit this absorption? E V 3 item attempts remaining Submit Answer Previous Tayitu...
1. Select the two compounds that are more likely to be a gas at room temperature (as opposed to a liquid). CH4 CH3OH C2H6 H2O 2. The separation of charges within a polar molecule is called a(n) ________. polar bond strong attraction dipole ionic bond dipole-dipole 3. Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C8H18) have only limited solubility in water? dipole-dipole ion-dipole Both dipole-dipole and induced dipole-induced dipole induced dipole-induced dipole dipole-induced dipole...
PART 1 - For the following compounds A. Predict how many signals would be detected in the expected 'H NMR spectrum. B. Label proton groups and determine their multiplicity. c. Predict the chemical shifts of each signal in the expected 'H NMR spectrum of the following compounds from the correlation chart in the last page. <Example> Number of signals O Proton groups Multiplicity Triplet B Multiplet (sextet) c Triplet D Singlet Chemical Shirt (ppm) 0.8-1.0 1.2 - 1.5 3.2 4.0...