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Wet Chemistry

by: keaffaber.3

Wet Chemistry BIO 1120-01


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About this Document

Hydrogen Bonds
Cells and Genes
Professor Dan E. Krane
Class Notes
25 ?




Popular in Cells and Genes

Popular in Biology

This 3 page Class Notes was uploaded by keaffaber.3 on Monday September 12, 2016. The Class Notes belongs to BIO 1120-01 at Wright State University taught by Professor Dan E. Krane in Fall 2016. Since its upload, it has received 30 views. For similar materials see Cells and Genes in Biology at Wright State University.


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Date Created: 09/12/16
“Wet” Chemistry Professor Krane 09-06-2016 “Wet” Chemistry  All living things are dependent upon water  Cells in our bodies are 70-95% water  Overall body weight is about 75% water Water’s Cohesiveness  Each water molecule can form a hydrogen bond with a total of four other water molecules  Bonds aren’t as strong but are always being broken and remade  Due to extensive hydrogen bonding between water molecules, they basically stick together  It is responsible for the absorbency of paper towels  Responsible for water’s unusual and remarkable surface tension Water Energetics  Has one of the highest heat capacity’s in science  Calorie – the amount of energy that must be added to cause the temperature of one gram of water to increase by one degree centigrade  Temperature – the measure of how fast molecules are moving o The hotter something is, the faster the molecules are moving  Because ice is less dense than liquid water -> ice floats  Since ice floats, water is a better temperature buffer  A “neater” arrangement of molecules results in fewer molecules in a given area and causes ice to be less dense than water  Because of water’s need for a great deal of energy to be invested to get it to evaporate and its tendency to insulate itself with its coldest molecules when it is a solid, water can act as a great reservoir of heat (kinetic energy). Water as a Solvent  Water’s Hydrogen bonding capacity also makes it a wonderful solvent  Solvent – something that dissolves things  Solute – something that IS dissolved  Things that are dissolved in water are said to be part of an aqueous solution o Mechanics  Ions and water molecules have an affinity for each other due to electrical attractions  In a sense water is acting as a solvent for itself and is simply  displaced a bit when another polar molecule is added o Concentration (molarity and pH)  Concentration – the ration of molecules of solute to solvent  A solution that has one mole suspended in one liter is said to be molar (or M)  pH – p stands for the negative of the log of the concentration  solution of pure water where the concentration is 1 x 10^- 7 moles/liter is said to be pH 7 or neutral Acids, Bases, and Buffers  Some solutes effect the concentration of hydrogen ions in an aqueous solution  pH + pOH = 14  Buffers are molecules that minimize changes of pH in aqueous solutions Carbon’s Bonds  Chemistry involving carbon molecules is often referred to as organic chemistry Valences o Carbon has a valence of 4  Makes it capable of being involved in incredibly versatile molecules Isomers o Structural isomers have the same chemical formula but functional groups are arranged in different ways


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