10/6/2014. The MACROSCOPIC world we are familiar with is governed by interactions at the atomic & molecular scale. Core Electrons & Valence Electrons:

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1 Today: Summary of Quantum Mechanics: Core vs. Valence Electrons Ionic vs. Covalent Bonding: Electron transfer from one element to another Sharing Electrons Lewis Dot Structures: Following Octet Rule Drawing & Recognizing Correct Lewis Dot Structures Bonding & Lone Pair e - Double & Triple Bonds Problem Set 3 DUE tonight at 11 pm Complete Course Survey by next Wednesday, Oct. 8 th at 11 pm for BONUS POINTS Midterm Exam Answer Key posted to course homepage Where are we going? How are electrons SHARED between elements to form ionic compounds or molecules? What is the SHAPE and POLARITY of a molecule? How does bonding within a molecule influence physical properties like boiling point, melting point, solubility, surface tension, elasticity or viscosity? How can theories of bonding be applied to complex problems in biology, medicine, engineering or the environment? The MACROSCOPIC world we are familiar with is governed by interactions at the atomic & molecular scale Core Electrons & Valence Electrons: fully filled shells of electrons buried deep within the atom. Electrons in the outmost shell on the surface of the atom. These are the electrons involved in bonding and chemical reactions. 1

2 Periodic Properties in the Periodic Table: The chemical properties of elements are largely determined by The Noble gases all have 8 valence electrons FULLY FILLING the outermost shell. This is called an OCTET. Elements will react to lose or gain enough electrons to arrive at a Noble gas electron configuration with a complete OCTET. The Alkali metals all have 1 valence electron in their neutral form Summary of Quantum Mechanics: Electrons exist in orbitals around nuclei as MATTER WAVES: The orbitals are filled in layers or SHELLS with different shapes & energies Electrons PAIR UP in atomic orbitals The INNER SHELLS are composed of CORE ELECTRONS. These do not participate in chemical reactions. The OUTER SHELL is composed of VALENCE ELECTRONS. These are more exposed & participate in chemical reactions. The number of valence electrons corresponds to the group number (i.e. 1A for Na, 2A for Mg, etc.) Summary of Quantum Mechanics: The OUTER SHELL is composed of VALENCE ELECTRONS. These are more exposed & participate in chemical reactions. The number of valence electrons corresponds to the group number (i.e. 1A for Na, 2A for Mg, etc.) 2

3 Major Categories of Compounds: Ionic Compounds: Usually formed through the combination of a metal () and a nonmetal (-) Covalent Compounds: Formed through the combination of multiple nonmetals bonding together The charged particles are connected in a grid; impossible to distinguish one unit from another Individual molecules can be identified and distinguished from one another Ionic vs. Covalent Bonding Ionic Bonds: A transfer of electrons makes one atom negatively charged (an anion) & one atom positively charged (a cation) But why do different combinations of elements produce different types of bonds? Covalent Bonds: Two atoms sharing electrons with a mutual attraction to the negative charge holding the nuclei together Electronegativity: Measuring an element s pull on electrons Ionic Bonds form between elements with a large difference in electronegativities: typically when METALS combine with NON-METALS Covalent Bonds occur between elements with similar electronegativities: when NON-METALS bond with other NON-METALS Table of Electronegativities A table of electronegativities will always be provided on exams if needed 3

4 Chemical Reactions based on Electron Configurations: Elements will react to lose or gain enough electrons to arrive at a Noble gas electron configuration with a complete OCTET. Metals LOSE electrons to reach a complete OCTET with a Noble gas configuration. Nonmetals GAIN electrons to reach a complete OCTET with a Noble gas configuration. Bonding in Ionic Compounds: Metals LOSE electrons to reach a complete OCTET Nonmetals GAIN electrons to reach a complete OCTET Electrons are NOT shared, but atoms are held together through attractive ELECTROSTATIC INTERACTIONS ( ) Lewis Dot Structures of Ionic Compounds: Valence electrons are written as dots around an atom PAIRING UP to reach a complete octet (8 e - total) Write the Lewis Dot Structure for aluminum oxide 4

5 Diatomic Molecules: Covalent Bonding in Nonmetals Co-valent Bonding: atoms sharing valence electrons to reach a fill outer shell. Occurs most often in bonding between NONMETALS Lewis Dot Structures: Valence electrons represented as dots that PAIR UP to reach a complete octet (or duet if Hydrogen) Shared Electron Pairs are written as single lines Diatomic Molecules: Understanding why certain elements pair up OCTECT RULE: Each atom shares enough electrons with its neighboring atoms to arrive at a noble gas configuration with 8 ELECTRONS Write the Lewis Dot Structures for diatomic chlorine gas, oxygen gas, & nitrogen gas Electron orbitals overlap on adjacent atoms to share electrons and reach a STABLE noble gas configuration Bonding vs. NON-Bonding Electron Pairs: Bonding Electrons: 2 electrons SHARED between atoms written as a single line Lone Pair Electrons: reside exclusively on one atom, NOT shared between atoms 5

6 Predicting the Formula of Covalent Molecules with Lewis Theory A. PCl Using only the concepts of Lewis Bonding Theory: Predict the likely covalent molecule that would form between Phosphorus & Chlorine. B. PCl 2 C. PCl 3 D. P 3 Cl E. P 2 Cl 3 Hint: They may combine in any ratio as needed so that each atom arrives at a COMPLETE OCTET (through mutually sharing electrons with neighboring atoms). Lewis Dot Structures for More Complex Molecules: H H C H H Write the Lewis Dot Structure for Carbon Dioxide. Lewis Dot Structures for Neutral Molecules: A Systematic Approach to Predict Bonding Arrangements 6. If needed, move lone pairs from outer atoms to bond with the central atom to form an octet on the central atom. This will make double or triple bonds. 6

7 Examples: CO CH 2 O ClF 3 In an industrial accident, a spill of 900 kg of chlorine trifluoride BURNED through 12 inches of concrete & almost 3 feet of gravel beneath! Writing the Lewis Dot Structure for Polyatomic Ions How many TOTAL electrons would be involved in bonding in the polyatomic anion, NITRATE: NO 3-? A. 11 electrons B. 12 electrons C. 22 electrons D. 23 electrons E. 24 electrons Polyatomic Ions are just CHARGED molecules For each negative (-) charge: add one electron. For each positive () charge: subtract one electron. Lewis Dot Structures for Polyatomic Ions: For each negative (-) charge: add one electron. For each positive () charge: subtract one electron. 6. If needed, move lone pairs from outer atoms to bond with the central atom to form an octet on the central atom. This will make double or triple bonds. 7

8 CO 3 2- Examples: NH 4 NO 2 - BF 4 - Recognizing CORRECT & INCORRECT Lewis Dot Structures Select the Lewis Dot Structures below that are VALID. A. B. C. D. ALL of these Lewis Dot Structures are VALID E. NONE of these Lewis Dot Structures are VALID 8

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