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Elements are made of atoms = the smallest particle that has all the characteristics of the element How Small is an Atom? • A copper penny contains 2.4 x 1022 atoms • Earth’s population is approx. 7 x 109 • A scanning tunneling microscope makes it possible to see individual atoms • TED Scanning Tunneling Microscope Atom Image Subatomic Particles • Mass of atom is generally protons + neutrons, majority of mass is in nucleus • Mass of proton = 1 • Mass of neutron = 1 • Mass of electron = 1/2000 • (mass of H proton = 1 = is standard) Subatomic Particles Subatomic Particle Proton Neutron Electron Charge Location Why? Distinguishing Between Atoms Atomic Number (Z) • Found on the periodic table • Is equal to the number of protons • Each element has its own atomic # • # protons = # electrons Average Atomic Mass • Also found on the periodic table • Is the average mass of all of the atoms of that element • Mass number = (A) actual mass of one atom • Mass number = protons + neutrons Carbon-12? When written in this format… 12 is the mass # Practice with a Partner Atom Symbol Atomic # Aver Atomic Mass Mass # Lithium 7 Boron 9 Carbon 12 Nitrogen 14 Oxygen 16 Helium 4 Sodium 23 # protons # neutrons # electrons Isotopes • Atoms of the same element that have different masses • Have different masses because they have different numbers of neutrons • # protons always the same Example • Carbon isotopes ▫ Carbon-12 ▫ Carbon-13 ▫ Carbon-14 • Might also be written C-12, C-13, C-14 • Or Nuclear Formulas • Used to write isotopes… Isotopes • How are isotopes similar? • How do they differ? • Isotopes are chemically alike b/c they have identical numbers of protons & electrons Average Atomic Mass • How is it calculated? • Based on the relative abundance of the naturally occurring isotopes of the element • Each isotope has a fixed mass and a natural % abundance Question • With the following information, calculate the average atomic mass of chlorine: ▫ 76% of chlorine isotopes found naturally have a mass of 35 ▫ 24% of chlorine isotopes found naturally have a mass of 37 Warm Up 1/15/2014 • P. 85 2-3 • P. 87 6-9 • Calculate average atomic mass given the following information: ▫ Carbon-12 is found naturally 98.89% of the time ▫ Carbon-13 is found naturally 1.11% of the time Warm Up 1/16/2014 • Write the procedure for determining average atomic mass (paragraph format, complete sentences). • Quiz tomorrow—cumulative • Homework tonight Atomic Theories • • • • • • Democritus John Dalton JJ Thomson Ernest Rutherford Niels Bohr Schrodinger “Atom” & Democritus • 400 BC • Called nature’s basic particle an atom • Atom (Greek) means uncuttable or indivisible • No experimental evidence Dalton’s Atomic Theory (1808) ▫ All matter is composed of tiny indivisible particles called atoms ▫ Atoms of the same element are identical ▫ Atoms of different elements can physically mix together or can chemically combine with one another in simple whole number ratios to form compounds ▫ Chemical reactions occur when atoms (in compounds) are separated, joined, or rearranged Dalton’s Atomic Theory • Much of Dalton’s theory is accepted …except ? • Except that atoms are indivisible AND that all atoms of an element are identical Thomson & Plum Pudding Model • 1897 • Discovered the electron • His model proposed that negatively charged particles were randomly distributed within a pudding of positively charged particles Rutherford & The Gold Foil • 1909 • Discovered the atom’s nucleus • He bombarded a thin, gold foil with fast moving alpha particles (p 72-73) Rutherford & The Gold Foil • A small amount of particles were deflected by the tiny nucleus; most of the particles passed on through • He concluded the volume of the atom was mostly empty space Bohr’s Atomic Model • 1915 • Electrons organized in energy levels or shells around a nucleus of protons and neutrons • A “planetary” model—not entirely correct The Electron Cloud & Schrodinger • Is a probability model • Describes a cloud like region where the electron is likely to be • Based on mathematical equation Project Time A Closer Look…the Bohr Model Video Bohr’s Model of the Atom • Scientists found that when an electric current is passed through a glass tube that contains hydrogen gas, the tube emits light • When this light is passed through a prism, four narrow bands of bright light are observed against a black background • This is hydrogen’s line emission spectrum • Bands are at specific wavelengths, which are unique to each element Niels Bohr • Niels Bohr proposed a model for the hydrogen atom that explained the spectrum of the hydrogen atom. • The Bohr model was based on the following assumptions: Bohr’s Model of the Hydrogen Atom ▫ Electrons are arranged in concentric circular paths or orbits around the nucleus ▫ Electrons in a particular path have a fixed energy ▫ The energy of the electron in an orbit is proportional to its distance from the nucleus. The further the electron is from the nucleus, the more energy it has. ▫ An electron can either gain or lose energy inside this orbit, electrons can move up or down to another orbit Continued… • A quantum of energy = is the amount of energy required to move an electron from its present energy level to the next higher one • Light is absorbed when an electron jumps to a higher energy orbit and emitted when an electron falls into a lower energy orbit Continued… • The energy of the light emitted or absorbed is exactly equal to the difference between the energies of the orbits • The energy given off is electromagnetic radiation • Is given off as photons (particle of light with no mass) Continued… • Lowest energy state of atom = ground state • Higher energy state of atom = excited state • Neon signs—excited neon atoms emit light when falling back to the ground state Project Time Reminder…Quiz tomorrow Warm Up 1/17/2014 • How did Bohr’s model of the atom differ from Schrodinger’s? Modern Atomic Theory Electron Cloud Model • AKA quantum mechanical model • Clouds of probability = where electrons are most likely to be • Electrons are located in orbitals (not orbits) Electron Cloud Model • 4 types of orbitals: s, p, d, f • Each orbital can only hold 2 electrons Warm Up 1/21/2014 • Construct a table to compare subatomic particles. Warm Up 1/24/2014 • Create a Venn diagram to compare the Bohr model to the electron cloud model. • Homework DUE • Quiz today Warm Up 1/27/2014 • Given an isotope for fluorine, fluorine-19… • What is Z? • What is A? Quizzes • Dropped one question • 2nd block 84 • 3rd block 86 What are ions? Why would ions form? Atoms with a charge When they gain, lose, or share electrons But…why would they do this? What is the Octet Rule? Says that atoms tend to gain, lose or share electrons so as to have eight electrons in their outer electron shell… More specifically, the number of electrons needed to fill the s and p sublevels of that energy level Practice Nuclear Chemistry How Atoms Combine Section 3.2 Chemical Properties • Chemical properties = how reactive an atom is • Does it like to combine with other atoms or is it stable alone? • Which groups on the periodic table are reactive? • Which groups are stable? Compounds • A substance that is composed of atoms of 2 or more different elements that are chemically combined • Example = NaCl • Why do these two atoms like to combine? (draw) Types of Bonds • Ionic bonds—when atoms lose or gain electrons • Example = _____________ • Covalent bonds—when atoms share electrons • Example = ______________ (draw) Compounds • Atoms want their outer energy level filled with electrons, in most cases this is 8 electrons • Which groups on the periodic table would you predict would commonly form bonds together? • Class Bonding Activity Warm Up 8/30/12 Complete Section Assessment 3.1 #1-5 on page 59 Group Assignment • Chemical Reactivity worksheet Independent Notebook Assignment • Vocabulary section 3.2 (page 60) Independent Assignment • Create a poster—to display a large drawing of an atom…the element will be assigned to you. • Format: see example • Grading: based on neatness & accuracy. Element Assignment • • • • • • • • • H He Li Be B C N O F • • • • • • • • • Ne Na Mg Al Si P S Cl Ar Warm Up 8/31/12 What group # is chlorine in? What is its symbol? List everything that you can learn about chlorine based its location in the periodic table. Include what other elements it might bond with. Agenda • Quiz • Project Presentations