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Purdue BCHM 30700 - Water and Organic Chemistry Review
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BCHM 30700 1st Edition Lecture 2Outline of Last Lecture I. SyllabusOutline of Current Lecture I. Basic ChemistryA. Definition of Valence ElectronsII. Water and its PropertiesA. Definition of ElectronegativityIII. Chemical BondsA. Dipole MovementsB. Hydrogen BondsC. Covalent BondsIV. Functional GroupsCurrent LectureValence electrons are electrons in the outermost orbital of the atom. Carbon has 4 valence electrons and can form 4 bonds. Nitrogen has 5 valence electrons and can form 3 bonds. Oxygen has 6 valence electrons and can form 2 bonds. Hydrogen has 1 electron and can form a single bond. Many interactions of these elements take place in an aqueous environment.Water is solvent with unique properties. It can form hydrogen bonds and has hydrophobic interactions. Water forms a dipole, due to a difference in electronegativity between the hydrogen and oxygen atoms that it is made from. Electronegativity refers to how much an atom wants to retain or give up its electrons. Some common electronegativity values are: Fluorine, which has the highest, at 4.0, Oxygen, 3.5, Nitrogen, 3.0, Carbon, 2.5, and Hydrogen, 2.1. Electronegativity trends in the periodic table are as follows: electronegativity increases going upwards and towards the right. The geometry of water, which is a bent shape, also creates the dipole movement. The oxygen atom in the middle of water has a higher electronegativity that the surrounding oxygen. This causes the oxygen to pull electrons forming the bonds more towards itself. The oxygen has a negative dipole movement on it, due to the influx of electrons. The partial loss of electrons creates a positive dipole movement for each hydrogen atom. The These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.electrons are both being pulled the same way, which creates an overall net dipole movement as well. The bonds that form water are covalent bonds. A covalent bond shares the pairs of electrons amongst the atoms. It is the strongest type of biological bond and requires an input ofenergy to break. Water can also form hydrogen bonds with other water molecules, as well as dissolved hydrophilic substances. The hydrogen bonds allow water to have a high boiling point, making it a good solvent for polar molecules. Hydrogen bonds help to stabilize the structure of many three-dimensional molecules in nature. Hydrogen bonds are a weaker type of bond. Covalent bonds have around 400 KJ/mol of energy, while hydrogen bonds only have around 20 KJ/mol. There are certain functional groups that must be memorized for biochemistry. Below is alist of the functional group formulas, their names, and the geometry of the central carbon atom.CH4Methane TetrahedralRCH4Methyl TetrahedralRCH2R’ Methylene TetrahedralRCH=CHR’ Methene PlanarRCHR’-OH Alcohol TetrahedralRCH=O Aldehyde PlanarRCR’=O Ketone PlanarRCX=O Carboxylic Acid


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Purdue BCHM 30700 - Water and Organic Chemistry Review

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