Chapter 3 Atomic and Electronic Structure: Images of the Invisible. Atoms. Electricity and the Atom. Atom
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1 Chapter 3 Atomic and Electronic Structure: Images of the Invisible Atom Atoms Too small to see with an ordinary microscope Need scanning tunneling microscope to get an image of an atom Tells nothing about the structure of an atom Chapter 3 2 Electricity and the Atom Electrolyte - Electrodes: Carbon rods of metallic strips that carry electrical current. Anode: positive electrode. Cathode: negative electrode.
2 Ions Ion: Cation: positive ion; moves to cathode Anion: negatively ion; moves to anode Electrons Protons Neutrons Subatomic Particles How are the protons, electrons and neutrons put together to make up the atom? Chapter 3 5 Discovery of Radioactivity Radioactivity Chapter 3 6
3 Types of Radioactivity Three commonly found types Chapter 3 7 Rutherford s Experiment Chapter 3 8 Rutherford Gold Foil Experiment
4 Structure of Atom Rutherford suggested: The center of the atom is nucleus Most of mass All the positive charge Nucleus: protons and neutrons Neutrons have mass but no charge Very small size compared to the rest of the atom The rest of the atom contains the electrons Chapter 3 10 Subatomic Particles Particles smaller than the atom All atoms have the same subatomic particles. Number of protons in element = atomic number Element: all atoms having the same atomic number Chapter 3 11 The Chemists Shorthand: Atomic Symbols Mass number? (nucleon number) Atomic number? A z X?? Element Symbol z = Atomic number = p A = Mass number = n + p Number of neutrons n = Mass Number Atomic Number For a neutral atom p = e Copyright 2000 by Houghton Mifflin Company. All rights reserved. 12
5 The Chemists Shorthand: Atomic Symbols By definition, atomic number = number of protons For a neutral atom, # p = # e Mass number? Atomic number? K?? Element Symbol Copyright 2000 by Houghton Mifflin Company. All rights reserved. 13 Summary: Atomic Structure Atoms made up of protons, electrons and neutrons. Heavier protons and neutrons in the center of nucleus & smaller electrons are outside of the nucleus in shells of specific energy. The atomic number, which is equal to the number of protons, determines the identity of the atom In a NEUTRAL atom the number of electrons and protons are equal. The mass number which is equal to the number of protons plus neutrons determines the weight of the atom in amu. Chapter 3 14 Example: How many protons, electrons & neutrons are in a F atom which has a mass of 19? How many neutrons, protons and electrons are in the atom? Cu Chapter 3 15
6 How many nucleons are in the atom plutonium-238? What is the nuclear charge of a carbon atom? How many electrons are in an argon atom? Chapter 3 16 How many electrons, protons and neutrons are in 238 U? How many electrons, protons and neutrons are in 235 U? Chapter 3 17 Exercise 3.1B A potassium isotope has 21 neutrons in its nucleus. What is the nucleon number and name of the isotope? Exercise 3.2B A Use the X notation to represent the isotope of uranium having Z 148 neutrons.
7 Isotope - Isotopes Isotopes of hydrogen 1 1H 2 1 H 3 1H Chapter 3 19 More Examples: 1. Determine the number of protons, neutron and electrons in the atom 119 Sn ( tin-119) 2. How many neutrons are in the molybdenum-90 atom? Chapter A rubidium atom has 50 neutrons in its nucleus. What is its nucleon number? X Which of the following are isotopes of the same element? X 35 X 37 X 88 38X Note: the atomic weight listed in the periodic table is the average of all the naturally occurring isotopes for the element. Chapter 3 21
8 Electron Structure How do electrons move around the nucleus? Flame Tests Various elements placed in a flame will change the color of the flame The spectrum shows several colors Implies something about the structure of the atom Chapter 3 22 Bohr s Explanation Each color corresponds to a certain value of energy. Electron can have only certain energy values and no others Energy is quantized Chapter 3 23 Energy Levels There are specified energy levels for an electron Shifts to lower energy levels give rise to light Chapter 3 24
9 Ground and Excited States Electrons prefer to be in the lowest energy level levels closest to the nucleus Ground state Excited states higher energy levels Chapter 3 25 Shells Elements may have more than one electron Placed into shells Shells numbered 1, 2, 3, Have 2n 2 electrons/shell Question: How many electrons are in the third shell? Chapter 3 26 Filling Electron Shells Add electrons to the lowest shell until filled, then go to the next shell Nucleus (2 max) (8 max)(usually 8, up to 18)(usually 8, up to 32) Examples: 1. What are the main-shell electron configurations for a) F b) Al Chapter 3 27
10 2. What are the main-shell electron configurations for a) Be b) Mg c) Ca These are in the same group of the periodic table. What do you notice about the electrons in the outermost shell? Chapter 3 28 Orbitals Schrödinger s model: probability of finding electron in a given volume Orbitals Electron clouds Different shapes for different types of orbitals Chapter 3 29 Electron Configurations and the Periodic Table Groups (families): Groups contain elements with similar chemical properties. Periods: Elements in a period demonstrate a range of properties from metallic on the left to nonmetallic on the right.
11 Electron Configurations and the Periodic Table Valence Electrons: These are the electrons that are gained, lost, or shared in a chemical reaction. Elements in a group or family have the of valence electrons. Electron Configurations and the Periodic Table Some groups in the periodic table have special names: Alkali Metals: Alkaline Earth Metals: Halogens: Noble Gases: Metals, Nonmetals, and Metalloids» Horizontal rows - Periods» Vertical Columns - Groups
12 Electron Configurations and the Periodic Table Metals, Nonmetals, and Metalloids Metals : metallic luster, conduct heat and electricity, malleable and ductile. Ex: sodium, copper Nonmetals dull luster, nonconductors, brittle Ex: sulfur, bromine Metalloids Demonstrate properties of both metals and nonmetals. Ex: silicon, arsenic Atomic Structure Electrons are responsible for the chemistry of the atom. Atoms can lose or gain electrons to form negative and positive ions. The total number of electrons and protons determines the charge of the atom. Chapter 3 35 Examples: (use the periodic table) 1. How many electrons does a neutral atom of O have? 2. How many electrons does an O 2- ion have? 3. How many protons does an O 2- ion have? 4. How many protons and how many electrons does a Na + ion have? Chapter 3 36
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Periodic Table Trends in Element Properties Ron Robertson r2 n:\files\courses\1110-20\2010 possible slides for web\ch9trans2.doc The Periodic Table Quick Historical Review Mendeleev in 1850 put together
CHAPTER REVIEW. 3. What category do most of the elements of the periodic table fall under?
CHAPTER REVIEW EVIEW ANSWERS 1. alkaline-earth metals 2. halogens 3. metals. electron affinity 5. actinides 6. answers should involve the transmutation of one element to another by a change in the number
Section 11.3 Atomic Orbitals Objectives
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