Ch 3: Atomic Structure
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1 Ch 3: Atomic Structure Name Excited Atoms and the Fourth of July 1. What is light, and how do various colors of light differ? 2. What is going on at the level of atoms and molecules when fireworks produce colored light? 3. How does the instability of copper chloride at high temperatures ineterfere with its ability to emit blue light? 3-1 How are the Elements Organized? Objectives: Describe the organization of the modern periodic table. Use the periodic table to obtain information abour the properties of elements.. Explain how the names and symbols of elements are derived. Identify common metals, nonmetals, and metalloids, and noble gases. PROPERTIES OF ELEMENTS RELATE TO ATOMIC STRUCTURES The periodic table shows all the elements The periodic table is organized by properties Group - a series of elements that form a column in the periodic table. Period - a series of elements that form a horizontal row in the periodic table. REGIONS OF THE PERIODIC TABLE The periodic table contains regions of similar elements Metals - Nonmetals - Metalloids - Noble Gases - Metals for the largest region of the table Nonmetals are the second largest region of the table Metalloids have properties of both metals and nonmetals Noble gases are on the far right of the periodic table Essential Elements - elements needed for health Chapter 3 Atomic Structure Page 2 of 6
2 3-2 What is the Basic Structure of an Atom? Objectives: Infer the existence of atoms from the laws of definite composition, conservation of mass, and multiple proportions. List the five basic principles of Dalton's atomic theory. Describe models of the atom. Compare and contrast the properties of electrons, protons, and neutrons. Explain the particle-wave nature of electrons. Describe the quantum model of the atom. BUILDING THE ATOMIC MODEL Atomos - (Greek word meaning...) Evidence supporting the atomic theory 1. Law of Definite composition 2. Law of Conservation of mass a. combination of atoms b. separation of atoms c. rearrangement of atoms 3. Law of Multiple Proportions Daltons atomic theory includes five principles Chapter 3 Atomic 1. All matter is made of indivisible and indestructable atoms. 2. Atoms of a given element are identical in their physical and chemical properties. 3. Atoms of different elements have different physical and chemical properties. 4. Atoms of different elements combine in simple, whole-number ratios to form chemical compounds. 5. Atoms cannot be subdivided, created, or destroyed when they are combined, separated, or rearranged in chemical reactions. Page 3 of 6 Structure FINDING THE STRUCTURE OF THE ATOM (HISTORICALLY)
3 Electrons are negatively charged particles that have a small mass. Cathode - a negative electrode through which current flows Anode - a positive electrode through which current flows Cathode Ray tube experiment - J.J. Thomson (1897) Each atom has a positively charged inner core Rutheford's Gold Leaf experiment - Ernest Rutheford (Hans Geiger & Marsden - graduate assistants) Nucleus - the central region of an atom made up of protons and neutrons. Electrons occupy energy levels within an atom Energy level or Principal energy level - a specific energy or group of energies that may be possessed by an electron in an atom Quantum Mechanical Model of the Atom - Neils Bohr Orbits - Quantitized - Chapter 3 Atomic Structure Page 4 of 6 Neutrons add mass to the nucleus
4 THE MODERN VIEW OF THE ATOM Electrons can be described as particles or waves Ground State - the lowest energy state of a quantitized system Excited State - the condition of an atom in a state higher than the ground state Electromagnetic Spectrum Red light - LOW frequency LONG wavelength Blue light - HIGH frequency SHORT wavelength Orbital - a region of an atom in which there is a high probability of finding electrons. Quantum theory provides a modern picture of the atom Quantum theory - the field of physics based on the idea that energy is quantitized and that this has significant effects on the atomic level. Present Day - Charge/Cloud Model of the Atom - The atom is a scientific model The model of an atom has changed through time...and will continue to evolve as we learn more. Chapter 3 Atomic Structure Page 5 of How do the Structures of Atoms Differ? Objectives: Decipher an element's atomic number and mass number in terms of its atomic structure. Decipher the information by the four quantum numbers with respect to the location of electrons in atoms. Define the Pauli exclusion principle in terms of the arrangement of electrons.
5 Use the periodic table to write the electron configurations and orbital diagrams for various atoms. ATOMIC NUMBER AND MASS NUMBER Each element has an atomic number Atomic number - the number of protons in the nucleus of an atom Isotope - one or two or more atoms having the same number of protons but different numbers of neutrons. Example: Hydrogen has three isotopes (named protium, deuterium, and tritium) Protium Deuterium Tritium Mass number - the total number of protons and neutrons in the nucleus of an atom The number of neutrons in an element is easy to find LABELING ELECTRONS IN ATOMS Quantum numbers are used to differentiate among electrons Principal Quantum number - (n) describes the energy level that the electron occupies Sublevel - ( ) one orbital or a group of orbitals within an energy level which have the same value of Letter Designations for Values of Letter 0 s 1 p 2 d 3 f Chapter 3 Atomic Structure Page 6 of 6 Orbital diagrams and electron cofigurations are models for electron arrangements 1s
6 1s 2s 2p 2p 2p 1s 2s 2p 2p 2p Hund's Rule - the most stable arrangement of electrons is that with the maximum number of unpaired electrons, all with the same spin direction. Shorthand pneumonic device to remember the filling order of electrons in atoms 7s 7p 6s 6p 6d 5s 5p 5d 5f 4s 4p 4d 4f 3s 3p 3d 2s 2p 1s 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p HOW TO WRITE AN ELECTRON CONFIGURATION 1. Locate the element whose electron configuration you wish to write in the periodic table. 2. Fill orbitals in the proper order with electrons. 3. Check that the total number of electrons in the electron configuration equals the atomic number. Electron configurations can be written in terms of noble gases "s 2 p 6 " AtomicLO
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