1. The Biological Medium on Earth

2. To get the most out of these notes, you MUST read along with pages 47-57 in the textbook Not everything in these pages are covered in the PowerPoint, only main points. To understand these points, you should read along with the textbook as it elaborates on, and explains the main points presented in this PowerPoint presentation.

3. All living organisms require water more than any other substance Water molecules participate in many chemical reactions needed to sustain life Most cells are surrounded by water, and are composed of 70-95% water themselves ¾ of the Earth’s surface is submerged in water

4. H 2 O: two hydrogen atoms connected to an oxygen atom by single covalent bonds Oxygen is more electronegative than hydrogen (has a stronger attraction for the electrons of a covalent bond), so the electrons of the polar bonds spend more time closer to the oxygen atom In other words, the bonds that hold together the atoms in a water molecule are polar covalent bonds The water molecule is a polar molecule, meaning the ends of the molecule have opposite charges

5. The oxygen end of the molecule has a partial negative charge, and the hydrogens have a partial positive charge

6. Intermolecular forces London-dispersion exist between all atoms and molecules the only intermolecular forces of attraction between noble gas atoms and between nonpolar molecules. formed by the temporary unequal distribution of electrons as they randomly move about the nuclei of atoms. Weak! Form between small nonpolar molecules, such as methane (CH 4 ) and nobel gasses ie helium) That is why these materials are gases at room temperature.

7. Intermolecular forces Dipole-dipole hold polar molecules to one another. the partially positive side of one polar molecule attracts the partially negative side of adjacent polar molecules. These intermolecular forces of attraction are stronger than London forces.

8. the strongest intermolecular forces of attraction. They are just especially strong dipole–dipole forces that only form between an electropositive H of one polar molecule and an electronegative N, O, or F of a neighbouring polar molecule Water molecules hold onto each other by H-bonds. Hydrogen bonds and an angular shape give water its many unique properties London dispersion forces, dipole–dipole attractions, and hydrogen bonds are collectively called van der Waals forces. water molecules would be arranged like this? 

9. 1. Cohesion 2. Moderation of Temperature 3. Insulation of Bodies of Water by Floating Ice 4. The Solvent of Life

10. In liquid form, hydrogen bonds are fragile Collectively, the hydrogen bonds hold the substance together, a phenomenon called cohesion Adhesion: the clinging of one substance to another Surface Tension: a measure of how difficult it is to stretch or break the surface of a liquid Water has a greater surface tension than most other liquids

11. Atoms and molecules have kinetic energy (the energy of motion) because they are always moving Heat is a measure of the total amount of kinetic energy due to molecular motion in a body of matter Temperature measures the intensity of heat due to the average kinetic energy of the molecules

12. When two objects of different temperature come into contact, heat passes from the warmer to the cooler object until they are the same temperature Molecules in the cooler object speed up (at the expense of the kinetic energy of the warmer object) Calorie: a unit of heat. The amount of heat it takes to raise the temp. of 1g of water by 1 o C

13. Specific heat: the amount of heat that must be absorbed or lost for 1g of that substance (in this case, water) to change its temperature by 1 o C The specific heat of water is 1cal/g/ o C Compared to other substances, water has a high specific heat capacity Large bodies of water can absorb and store a huge amount of heat from the sun

14. Heat of vaporization: the amount of heat a liquid must absorb for 1g of it to be converted from the liquid to gaseous state Water has a high heat of vaporization compared to other liquids, caused by hydrogen bonds (which must be broken before the molecules can make their exodus from the liquid) Water’s high heat of vaporization helps moderate Earth’s climate

15. As a liquid evaporates, the surface of the liquid that remains behind cools down This evaporative cooling occurs because the “hottest” molecules (those with the greatest kinetic energy) are the most likely to leave as gas Evaporative cooling contributes to the stability of temperature in lakes and ponds

16. Water is less dense as a solid than as a liquid So, ice floats in water Water expands when it solidifies, again, a result of hydrogen bonding If ice sank, all water bodies would freeze, killing all the life inside them

17. Solution: a liquid that is a completely homogeneous mixture of two substances Solvent: the dissolving agent of a solution Solute: the substance that is dissolved Aqueous solution: water is the solvent Water is the most versatile solvent, due to its polarity Hydrogen shell: the sphere of water molecules around each dissolved ion

18. Hydrophilic: a substance that has an affinity for water (“water-loving”) Some substances are hydrophilic, but do not dissolve. They remain suspended in the aqueous liquid (this is called a “colloid”  a stable suspension of fine particles in a liquid) Hydrophobic: a substance that repels water due to being nonionic and nonpolar (“water- fearing”). An example is vegetable oil.

19. Molecular mass: the sum of the masses of all the atoms in a molecule. For example, in sucrose: C 12 H 22 O 11, the mass of a carbon atom is 12, hydrogen is 1, and oxygen is 16. So, sucrose has a molecular weight of: 12(12) + 1(22) + 11(16) = 342 daltons (atom masses given in daltons rounded to whole numbers) Substances are often measured in units called Moles (mol), which represents and exact number of objects Molarity: the number of moles of solute per litre of solution

20. An acid: a substance increases the hydrogen ion concentration of a solution A base: a substance that reduces the hydrogen ion concentration of a solution pH scale: the pH of a solution is defined as the negative logarithm (base 10) of the hydrogen ion concentration: pH = -log[H + ] Buffers are substances that minimize changes in ion concentration (H + and OH - ) Acid precipitation has a pH lower or more acidic than pH=5.6