Chapter 2 Lecture and Reading Note taking Template Fill in this outline in lecture then use your textbook to add to it Notes from just the lecture are not enough to do well in this class 1 What general announcements and follow ups are there a When where is SI b What assignments are due this week Where are they located c Where are you vs where should you be on your reading 2 How should I be using the Learning Outcomes of the textbook Green box reading helps us learn about the outcome of the chapter 3 What makes something alive Are viruses alive Viruses are not alive they need a host to live 4 Why do we start the semester off with molecules water and chemistry All living things are composed of atoms 5 What is matter Matter 1 has mass and occupies space 2 is composed of atoms 6 What are the three components of an atom Fig 2 3 Where are each found and what is their charge What is the ration of protons to electrons What is ration of protons to electrons protons equals number of electrons 7 Define atomic number element and atomic mass atomic number number of protons Element any substance that can t be broken down to any other substance by ordinary chemical means atomic mass sum of protons and neutrons 8 Why aren t electrons include in the atomic mass 9 Define ion cation and anion 10 What is an isotope What is a radioactive isotope What are some ways radioactive isotopes are used to study science 11 What is the key to the chemical behavior of the atom How important is this principle Key to the chemical behavior of an atom lies in the number and arrangement of its electrons in their orbitals Orbital as area around a nucleus where and electron is most likely to be found Nuclei of atoms don t interact only electrons Electron shell arrangement Carbon has 4 valence electrons in order to help regulate life in all living things 12 Where do electrons have the most energy 13 What is the difference between an energy level and an orbital 14 What is redox short for in organisms chemical energy is stored in high energy electrons that are transferred from one atom to another LEO the lion goes GER OIL RIG Chapter 2 Lecture and Reading Note taking Template 15 What is the difference between an inert and reactive element 16 What is the octet rule and why is it important 17 Look at Figure 2 7 and list the 12 elements found in living things 18 What 4 elements make up 96 of living things 19 What 4 elements do all organic molecules include 20 Define and give examples of molecule compound and chemical bond Molecules are groups of atoms held together in a stable association Compounds molecules containing more than one type of element Chemical Bonds atoms held together in molecules or compunds 21 How do ionic bonds form How stable are they Attraction of oppositely charged ions gain or loss of electrons forms ions water molecules can disrupt ions together weak bonds 22 How do covalent bonds form and how stable are they What is the difference between single and double covalent bonds Covalent Bonds Atoms share 2 or more valence electrons strong bonds Single Covalent Bonds share 2 electrons Double Covalent Bonds share 4 electrons Triple Covalent Bonds share 6 electrons 23 What is electronegativity and why is it important Electronegativity atom s affinity for electrons Dictate how electrons are distributed in covalent bonds 24 What is the difference between polar and nonpolar covalent bonds Nonpolar equals sharing of electrons Polar unequal sharing of electrons 25 How do hydrogen bonds form and how stable are they 26 Be able to identify reactant and products in a chemical reaction Reactants the starting element before a reaction Product What was produced after a reaction 27 What are three things that influence chemical reactions Temperature Concentration of reactants and products Catalysts 28 What are hydrogen bonds and how does the structure of water facilitate hydrogen bonding Single most outstanding chemical property of water is its ability to form hydrogen bonds Weak chemical associations that form between the partially negative O atoms and the partially positive H atoms of two water molecules H and O held together by polar covalent bonds Responsible for many of water s important physical properties 29 What is the difference between adhesion and cohesion Provide examples of each Chapter 2 Lecture and Reading Note taking Template Cohesion polarity of water allows water molecules to be attracted to one another Produces weak and transitory hydrogen bonds Cumulative effects are enormous Water molecules stick to other water molecules by hydrogen bonding Adhesion water molecules stick to other polar molecules by hydrogen bonding 30 In section 2 5 know the 6 properties of water and be able to explain what they mean 1 Water has a high specific heat Measures the extent in which a substance resists changing its temperature when it absorbs or loses heat large amount of energy is required to change the temperature of water 2 Water has a high heat of vaporization evaporation of water from a surface causes 3 Solid water is less dense than liquid water water freezes from the top ice is less cooling of that surface dense than water 4 Water is a good solvent water dissolves polar molecules and ion 5 Water organizes nonpolar molecules hydrophilic water loving hydrophobic water fearing water causes hydrophobic molecules to aggregate or assume specific shapes these interactions are critical for living systems 31 Summarize Table 2 3 in your own words 32 Define pH acid base and buffer pH is the negative logarithm hydrogen ion concentration of solution 0 7 acids 7 14 bases Acids lower pH any substance that dissociates in water to increase the H and lower the pH lowers the H Bases higher pH substances that combine with H dissolved in water and thus Buffers stabilize pH substances that resists change in pH Act by releasing hydrogen ions when a base is added Most biological buffers consist of a pair of molecules one an acid and one a base Carbon framework of biological molecules consists primarily of carbon bonded to other atoms Chapter 3 Can form up to 4 covalent bonds Hydrocarbons