B) permanent dipoles of molecules containing covalent bonds between atoms of very different electronegativities. C) the hydrophobic effect. D) ion pairing between oppositely charged functional groups. Answer: A Page Ref: Section 5 28) The aggregation of nonpolar molecules or groups in water is thermodynamically due to the A) increased entropy of the nonpolar molecules when they associate. B) decreased enthalpy of the system.
3 x (C H5 N) = C3H15N3 Hydrated compounds Solving process: 1st- the difference between the initial mass and that of the dry sample is the mass of water that was driven off. Mass of hydrate minus mass of dry sample equals the mass of water 10.407 – 9.520 = 0.887 g 2nd- The mass of dry BaI2 and the mass of water are converted to MOLES. 9.520 g BaI2 x 1 mol BaI2 ∕ 391 g BaI2 = 0.0243 mol BaI2 anhydrate 0.887 g H2O x 1 mol H2O / 18.0 g H2O = o.o493 mol H2O 3rd: Dividing both results by the amt of 0.0243 mol, we get a ratio of 1 to 2.03, or 1 to 2, since the formula must have full numerical integers of water molecules, in other words no fractions of a water molecule. Thus, for every 1 mole of BaI2, there are two moles of water. The formula for the hydrate is written as BaI2 • 2H2O And it is named barium iodide dihydrate.
Therefore each compound has similar solubility in water. The hydrogen bonds in butanol are stronger that the dipole interactions in diethyl ether. Butanol has a higher boiling point because of the stronger hydrogen bonds. The intermolecular forces holding the butanol molecules together are stronger than those holding the diethyl ether molecules together. 2) Predict which of the following in each set of compounds will have the highest water solubility.
Chemical environment surrounding the carbons are different and therefore affecting the character of the hydrogens attached. This difference in chemical environment finally explains the different interaction between hydrogen and chlorine. Determination of percent yield, and relative reactivity data was processed after the products of the reaction were analyzed using Gas Chromatography. Percent yield was calculated for each isomer and determined to be; 5.94% for 1,1-dichlorobutane, 23.1% for 1,2-dichlorobutane, 47.1% for 1,3-dichlorobutane, and 23.9% for 1,4-dichlorobutane. The relative reactivity of the hydrogens H1, H2, H3 , and H4 were 0.37, 1.4, 2.9, and 1.0 respectively.
With the use of this technique we placed chlorine, bromine, and iodine into solutions containing chloride, bromide, and iodide. In the reaction the free halogen (X2) oxidizes the other halide ion (Y-) and gets reduced by gaining electron(s). In table 3, chlorine was the strongest oxidizing agent and iodine was the weakest oxidizing agent. Since chlorine was the strongest oxidizing agent it will react more and the weak agent will react less. This explanation can be demonstrated in table 3 also because the results of the reactions demonstrates that chloride reacted more by the color of the product compared to the color of chloride in the mineral oil.
This is because hydrogen bonds to the water molecules are formed. Acetaldehyde (ethanal, CH3CHO) and acetone are miscible with water in all proportions. II. Chemical Properties (see Bettelheim, chapter 17.4) Aldehydes are easily oxidized a fact due to the presence of the hydrogen attached to the carbonyl group (this is not present in ketones, which are less easily oxidized). Oxidation of aldehydes yields carboxylic acids.
N F S F F 3.) 4.) O S O S S O S S C C C S The right two structures are equally important and probably more important than the left structure (negative charge on more electronegative atom). 5.) O O O O O O O O I I I O O O O O O I O O O I I O The top three are equally important.
CHE 111 Laboratory 3 Hydrates Introduction Hydrates Water molecules combine with the molecules of certain substances, forming loose chemical combinations called hydrates. An example of a hydrate is MgSO4•7H2O. This formula means 7 water molecules are loosely attached to a magnesium sulfate molecule. Other examples of hydrates are Na2SO4•10H2O and Ba(OH)2•8H2O. When the hydrate is heated, it easily loses water molecules attached and becomes an anhydrous salt.
d. Write the total net ionic equation for the reactions. 3. One industrial method of producing bromine is to react seawater, containing a low concentration of sodium bromide, with chlorine gas. The chlorine gas is bubbled through the seawater in a specially designed vessel. Write the net ionic equation for this reaction.
When pH is high which means more OH⁻, then aluminum ions will react with hydroxide ions to form aluminum hydroxide. Phosphate ions are acting as a natural buffer. If the equipment is not washed with acid, it would cause an error. This is because the phosphorus analyzing is dealing with low concentration of phosphorus and it is easily contaminated by detergent and other chemicals and it has to be washed by using an acid and also it has to be rinsed with distilled water once it is rinsed with acid. Also refer to section 4 (discussion).