Biology Intro…. Chapter 1: Themes in the Study of Life

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Presentation transcript:

Biology Intro…. Chapter 1: Themes in the Study of Life Chapter 2: Chemical Context of Life Chapter 3: Water and the Fitness of the Environment

Unifying Themes in Biology Evolution~ biology’s core theme; differential reproductive success Emergent Properties~ hierarchy of life The Cell~ all organism’s basic structure Heritable Information~ DNA Structure & Function~ form and function Environmental Interaction~ organisms are open systems Regulation~ feedback mechanisms Unity & Diversity~ universal genetic code Scientific Inquiry~ observation; testing; repeatability Science, Technology & Society~ functions of our world

Chemical Context of Life Matter (has volume & mass) Atom: the smallest unit of matter that still retains the physical & chemical properties of its element. Sub-atomic Particles: Neutrons- no charge, in nucleus, 1 amu Protons- (+) charge, in nucleus, 1 amu Electrons- (-) charge, orbit around nucleus negligible mass. Atomic number - # of protons; in a neutral atom, # of protons = # of electrons Mass number - protons + neutrons of an atom Atomic Weight takes into consideration all of the isotopes of that element and averages them…. Isotopes- Atoms of an element that have the same # of protons, but different # of neutrons. same atomic number, different mass number

Structure of an Atom The nucleus of an helium atom contains 2 neutrons, shown in purple and 2 protons, shown in green. 2 electrons move around the nucleus at very extreme speeds. Question: How many neutrons would there be in Carbon 14? a. 6 b. 8 c. 14 d. 28

Reading the Periodic Table Fluorine Chemical Symbol: F # of protons: # of electrons: # of neutrons: 9 2 7 F 9 19 9 19 - 9 = 10

Energy Levels & Orbitals…. Energy Levels- also referred to as “shells” Made up of orbitals Orbital: the 3 dimensional space where the electrons are found No more than 2 electrons per orbital “s” orbital- spherical found in all shells Holds just one pair of electrons The first shell only has the one S orbital “p” orbital- Dumbbell shaped Found in higher energy levels (shells) 3 p orbitals per shell Electron Configuration- the main property which determines chemical behavior. How many electrons are in a shell that has all its s and p orbitals filled? A. 2 B. 4 C. 6 D. 8

Energy Levels & Orbitals…. Valence Electrons- electrons in outer most shell Not to be confused with…. “Valence” – the bonding capacity of an atom; the number of covalent bonds that must be formed to complete the outer shell’s “octet”. Octet Rule: a shell is complete when it contains 8 electrons (or “feels” like it does). H and He exempted Atoms with incomplete valence shells are chemically reactive. Molecule- 2 or more atoms held together by chemical bonds. Bonds- attractions that hold molecules together. Animation

Chemical Bonding Covalent Double covalent Nonpolar covalent Ionic Hydrogen van der Waals

Covalent Bonding Sharing pair of valence electrons Number of electrons required to complete an atom’s valence shell determines how many bonds will form Ex: Hydrogen & oxygen bonding in water; methane Animation

Polar/nonpolar covalent bonds Electronegativity attraction for electrons The difference in electronegativity determines if atoms are: Non-polar covalent (very little to no difference) Polar covalent (somewhere in the middle) Ionic (big difference) Non-polar covalent •electrons shared equally •Ex: diatomic H2 and O2 Polar covalent •one atom more electronegative than the other (charged) •Ex: water Water is a _________ molecule. A. Ionic B. Non-Polar Covalent C. Polar Covalent

Polar/nonpolar bonds

Ionic bonding High electronegativity difference strips valence electrons away from another atom Electron transfer creates ions (charged atoms) Cation (positive ion); anion (negative ion) Ex: Salts (sodium chloride) Animation

Hydrogen bonds Hydrogen atom covalently bonded to one electronegative atom is also attracted to another electronegative atom (oxygen or nitrogen) Hydrogen Bonding occurs: A. Between Polar Molecules. B. Between non-polar molecules. C. Between ionized atoms. D. Between ionic molecules. Animation

van der Waals interactions Weak interactions between molecules or parts of molecules that are brought about by localized change fluctuations Due to the fact that electrons are constantly in motion and at any given instant, ever-changing “hot spots” of negative or positive charge may develop

Water Jesus lizard Polar~ opposite ends, opposite charges Weakly (+) at the Hydrogen; weakly (-) at the Oxygen This causes: HYDROGEN BONDING!!!! Cohesion~ H+ bonds holding molecules together Adhesion~ H+ bonds holding molecules to other substance Surface tension~ measurement of the difficulty to break or stretch the surface of a liquid High Specific heat~ amount of heat absorbed/lost to change temperature by 1oC. Resists Temp changes! (for water, that’s 1 calorie) Heat of vaporization~ quantity of heat required to convert 1g from liquid to gas states. This, too, is high for water which leads to…. Evaporative Cooling~ Molecules with the highest energy escape first, leaving the average energy of the system proportionally MUCH lower. Density………. Jesus lizard

Density & Solvency: Due to hydrogen bonding, water is less dense as solid than liquid Crystalline lattice keeps molecules at a distance Water is the “Solvent of Life” Hydrophilic (water loving) solutes dissolve in it: They include: Ionic Compounds- water surrounds the individual ions, separating and shielding them from each other. Polar Compounds- charged regions have affinity for oppositely charged regions of polar molecules. Don’t forget your molarity! Ionic Animation What is Molarity? A. Moles solvent / Liter Solute B. Moles solute / Liter Solvent C. Grams solvent / Liter Solute D. Grams solute / Liter Solvent

Acid/Base & pH Water Animations Dissociation of water into a hydrogen ion and a hydroxide ion 2H2O  H3O+ + OH- Acid: increases the hydrogen concentration of a solution Considered to be “proton donors” pH between 0 and 7 Base: reduces the hydrogen ion concentration of a solution Considered to be “proton acceptors” pH between 7 and 14 pH = -log[H+] (example on next slide) Buffers: substances that minimize H+ and OH- concentrations (accepts or donates H+ ions) Acidification of the Oceans