Liquid State traditionally red and hydrogen is d.2) Water: Notice the color of t

Question

Liquid State traditionally red and hydrogen is d.2) Water: Notice the color of the atoms: oxygen is atoms traditionally white. Notice also that the water molecules are not linear but the hydrogen are at an angle of greater than 900. The hydrogen of one molecule is pointing toward the oxygen of a neighboring molecule. The ball and spoke model may make this easier to see. Based on your knowledge of water, why are the liquid water molecules aligned in this manner?
d.3) Turn on the simulation. How is he motion of the water molecules different .or similar to the motion of the bromine liquid molecules? Do the liquid water molecules migrate away from their original positions? Solid State ball and spoke model. of on Water: You will need the model and switch to or similar to the mo the simulation, How is the motion of the ice molecules different the solid bromine molecules?
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d.5 Compare the liquid water structure to the solid water(ice) structure. Rotate the"box" so that you see all sides of the water molecule. d 6 Explain why ice floats.
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Part 2: Gas Density Go to the opening page and click on the Molecular stockroom, At the bottom of the page is a section of Mixtures, chose gas phase, and select Air: Remove Text so that the simulation will be enlarged. and choose Properties. On the Properties menu, chose Thermodynamics, then Temperature. Repeat the process but chose volume option. There are now two properties bars open.

Explanation / Answer

Water molecules have molecular formula H2O. These molecules are tiny, electrically neutral and V-shaped. In the liquid state the three atoms do not stay together as the hydrogen atoms are constantly exchanging between water molecules, due to protonation/deprotonation processes. Both acids and bases catalyze this exchange. Even when at its slowest (at pH 7), the average time for the atoms in an H2O molecule to stay together is only about a millisecond. This brief period is, however, much longer than the timescales encountered during investigations of water's hydrogen bonding or hydration properties, and thus, water is usually treated as a permanent structure.

In a water molecule, the oxygen atom attracts electrons much more strongly as it is much more electronegative than the hydrogen atoms. This results in a charge transfer from the hydrogen atoms towards the oxygen atom and, hence, the polarity of the water molecule.

In a water molecule, an oxygen atom alone has six electrons in its outer shell, and each hydrogen atom initially has one. When the hydrogen atoms share their electrons with two of the oxygen atom's outermost shell electrons, two bonds form, one each between a hydrogen atom and the oxygen. Now the oxygen atom has eight electrons, making two bonding pairs and two non-bonding pairs. The four pairs of electrons around oxygen all take up space, and the most stable arrangement is at the corners of a tetrahedron (imagine a pyramid shape with oxygen at the center and the four electron pairs pointing toward the four corners.) The four pairs tetrahedrally arranged sp3-hybridized electron pairs, two of which are associated with hydrogen atoms and the two remaining lone pairs. In a perfect tetrahedral arrangement the bond pair-bond pair, bond pair-lone pair and lone pair-lone pair angles would all be 109.47° and such tetrahedral bonding patterns are found in condensed phases. As a result, the water molecule looks bent, with the hydrogen atoms on one side of the oxygen atom and the unpaired electrons on the other side.

At room temperature and pressure bromine molecules are close together and randomly arranged. The molecules of Br2 can move freely as compare to the molecules of water.

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