The hydrophobic effect is a key driving force for all sorts of biological systems. When a hydrophobic molecule is placed in water, it disrupts the hydrogen bonding of nearby water molecules. Let's consider a simple tetrahedral model of hydrogen bonding to investigate this entropic component of this effect. hydrogen bond oxygen hydrogen a) Depicted above and to the left, is an idealized model of the hydrogen bonding network for a single (central) water molecule. i) For the central water molecule how many possible hydrogen bonding configurations exist? HINT: Above and to the right is one such configuration. The four adjacent water molecules are allowed to adopt any orientation to accommodate the central molecule and are not depicted. ii) Replace one of the four adjacent water molecules with a nonpolar molecule. Now, how many possible hydrogen bonding configurations exist? iii) Calculate the difference in entropy for replacing one of the four adjacent water molecules with a nonpolar molecule. b) If we have a hydrophobic molecule in aqueous solution that makes contact with 25 water molecules, what is the change in molar Gibbs energy for adding this molecule into solution? Assume AH-0 and T- 298 K.

London dispersion forces, or simply dispersion forces are the from surrounding intermolecular force. It is an attractive force that arises dipole moments in molecules or species. These moments arise when there are instantaneous deviations in the electron clouds of the species. Surrounding molecules are dipole influenced by these dipole moments and a chain reaction results in which subsequent weak, dipole-induced dipole interactions are created. These cumulative dipole-induced dipole interactions create the attractive dispersion forces. Dispersion forces are the forces that make substances condense to liquids and freeze into solids as temperatures decrease. Your answer choices are: weakest, temporary and nonpolar. Several of your choices are used more than once.

I need help on part B.

A common error is that student expect the nitrate ion to be non-polar. If thatwere the case which solvent would it be expected to be more soluble in carbon tetrachloride or dicholormethane. Briefly explain your reasoning.

ng and lear X O water treatment systems - Forkly X akeAssignment/takeCovalentActivity.do?locator=assignment-take [Review Topica] [References] Use the References to access important values if needed for this question. The common laboratory solvent diethyl ether (ether) is often used to purify substances dissolved in it. The vapor pressure of diethyl ether , CH3CH,0CH,CH3, is 463.57 mm Hg at 25 °C. In a laboratory experiment, students synthesized a new compound and found that when 5.823 grams of the compound were dissolved in 156.3 grams of diethyl ether, the vapor pressure of the solution was 456.57 mm Hg. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight of this compound? diethyl ether =CH,CH,OCH,CH3= 74.12 g/mol. MW g/mol Submit Answer Retry Entire Group 9 more group attempts remaining ed 8:43 PM 11/17/202 Q