Study Guide Test 1 BSC2010 Spring 2012 Professor Epstein Study Tips sense 1 Learn the terms at the beginning of each study guide first so that the concepts make more 2 Practice each iClicker question so you have a better understanding of the material 3 Review the Quiz Questions throughout the study guide These are directly from the In Class Quizzes The 1st and 3rd quizzes are in this study guide but I didn t have enough time to copy down all the questions to the second quiz 4 Go to the Blackboard site and take the practice exam and review the material that you missed Good Luck Before printing This study guide is 30 pages due to the pictures and practice problems Make sure for the exam you have a thorough understanding of the chemistry and how it relates to biology If you can master polarity valence electrons and bonding it will help with later sections on this test and class BSC 2010 BIOLOGICAL SCIENCE I SPRING 2012 STUDY GUIDE 1 THE CHEMICAL CONTEXT OF LIFE Completed Vocabulary Atom Smallest unit of matter that still retains the properties of an element Made of neutrons protons and electrons Atomic mass of Protons of Neutrons Atomic Mass Atomic number of Protons Atomic Number Chemical reaction reactants and products Compound Substance made of two or more elements in a fixed ratio The characteristics of a compound can be very different from those of the component elements ex Na Cl NaCl Covalent bonds non polar and polar Covalent Sharing of a pair of valence electrons by two atoms Non polar Equal sharing same two electronegativities Polar One atom is more electronegative so the electrons aren t evenly shared Dalton 1 Dalton Mass of 1 Proton or 1 Neutron also called an amu used to describe atomic masses Electron Negative Charge 1 for this class has a negligible mass Form a cloud around the nucleus Responsible for the interactions between atoms during formation of compounds Electron orbital Electron shells are made of electron orbitals subshells that can fill with 2 electrons ex 1s 2s 2p 3s etc The s and p refer to the shape of the orbital s sphere p pi The orbitals are filled from the 1 to 3 energy shells for this class Element Substance that can t be broken down to other substances by chemical reactions Energy shell The electron s state of potential energy is the energy level and this is determined by it s location relative to the nucleus called it s energy shell The larger the electron shell the higher the amount of energy Hydrogen bonds When a polar bonded hydrogen atom is attracted to another electronegative atom generally N or O are the electronegative atoms Inert gasses Nobel Gasses Atom with completely full valence outer shell ex Argon Neon Helium Ionic bonds Unequal sharing of electron causes ions to form cation or anion causing an attraction due to the oppositely charged atoms Attraction not b c of the transfer of e Isotope Different number of neutrons compared to protons for an element Different atomic mass but same atomic number Same chemical properties but different physical properties Matter Anything that takes up space and has mass made of elements Molecular weight Sum of the atomic mass of all the constituent atoms of the compound Moles and molar solutions Measure of the number of molecules of a given type 1 mole 6 x 10 23 molecules Nucleus Composed of the protons and neutrons of an element Neutron No electrical charge but same mass of a proton 1 dalton Periodic table Way of organizing elements by atomic mass and properties Potential energy Stored energy that matter has due to location or structure Electrons have differing amounts of PE the farther the electrons are from the nucleus higher energy shell the higher the PE is of that electron due to the attraction of the positive charge of the protons in the nucleus to the electron s negative charge Proton Positive Charge 1 same mass as a neutron 1 dalton determines the atomic number of an element Radioactive Referring to isotopes meaning unstable and giving off subatomic particles and energy due to spontaneous decay of the nucleus Valence shell electrons and number Valence shell outer shell valence electrons electrons in outer shell that are most important in interactions with other elements bonding valence number of unpaired valence electrons in outer shell ex F 1 O 2 Van der Waals interactions Due to asymmetrically distributed electrons even in nonpolar atoms compounds atoms can create very weak attractions but collectively strong ex Gecko Principles and Concepts Be familiar with the elements that are important to life Table 2 1 Elements Important to Life Know Oxygen Nitrogen Hydrogen and Carbon are most abundant 96 Don t memorize the above list but know that the 2nd group makes up 4 and be aware that trace elements are in small amounts but ARE ABSOLUTELY required in the body Understand the basics of atomic structure and the nature and properties charge and mass of the subatomic particles that atoms are made of Composed of Know the charge mass in comparison to each other Protons 1 1 dalton Neutrons No charge Electrons 1 1 dalton Negligible Mass 0 Formation Neutrons Protons are in the center of the atom nucleus while electrons move around in a cloud or distribution pattern of the nucleus Be able to determine numbers of neutrons protons and electrons in an atom given its charge atomic number and atomic mass Atomic Mass Number of Protons Atomic Size of Protons Neutrons If charge is 0 Protons Electrons If charge is 1 1 less electron than proton If charge is 1 1 more electron than proton Examples from Slides 1 What is the atomic number and atomic mass of an atom that has 6 protons 6 neutrons and 6 electrons respectively a 6 6 b 6 12 c 12 6 d 12 12 e 12 18 2 Fluorine s atomic number is 9 and its atomic mass is 19 How many neutrons and electrons does an uncharged atom of fluorine have respectively a 9 9 b 9 10 c 19 9 d 10 9 e 10 19 Know what isotopes are and that they have similar chemical properties but may have different physical properties such as being magnetic or radioactive Isotopes Different number of neutrons compared to protons for an element Different atomic mass but same atomic number Same chemical properties same of protons and react like normal atoms but different physical properties ex C 14 can be radioactive while C 12 is most common Example from Slides 3 14C and 12C have a different chemical and physical properties b different chemical properties and a different number of neutrons c different chemical
View Full Document
Unlocking...