BNG_Bonding Module Overview

Bonding  Module Overview

Introduction

You already know that there are two main types of chemical bonds, ionic and covalent. In this module you will explore the properties of chemicals with these types of bonds. You will learn that there are different types of covalent bonds, polar and nonpolar, and that the type of covalent bond along with the shape of a molecule affects the overall polarity of the molecule.

Module Lessons Preview

• What is a bond?
• How are ionic and covalent bond formed?
• How are ionic and covalent bonds different?
• How are Lewis structures of atoms and ions drawn?
• How are electrons shifted from one atom to another to fill octets?
• How is it determined if a molecule is polar or non-polar?
• What is a dipole moment?
• How are Lewis structures of covalently bonded compounds and ions drawn?
• What is bond resonance?
• How does resonance in bonding increase overall molecular stability?
• How do atoms constitute molecules with linear, planar triangular, tetrahedral, trigonal bipyramidal, and octahedral shapes?
• What are the interior bond angles for linear, planar triangular, tetrahedral, trigonal bipyramidal, and octahedral shapes?
• How is the shape of a molecule predicted from its Lewis Dot Structure?
• How are atomic orbitals hybridized when forming molecular orbitals?
• How is the VSEPR theory used to predict orbital hybridization?
• How many electrons are in double and triple bonds?
• How is the bond order of a molecule computed?

Key Terms

1. Ionic Bond - the attractions between ions that hold them together in an ionic compound
2. Octet Rule - an atom tends to gain or lose electrons until its outer shell has eight electrons
3. Covalent Bond - a chemical bond that results when atoms share electron pairs
4. Lattice Energy - energy released by the imaginary process in which isolated ions come together to form a crystal or ionic compound
5. Partial Charge - charges at opposite ends of a dipole that are fractions of a full 1+ or 1- charges
6. Polar-Covalent Bond - a covalent bond in which more than half of the bond's negative charge is concentrated around one of the two atoms (also known as a polar bond)
7. Electronegativity - the relative ability of an atom to attract electron density toward itself when joined to another atom by a covalent bond
8. Lewis Symbols - the symbol of an element that includes dots to represent the valence elctrons of an atom of the element
9. Lewis Structure - a structural formula drawn with Lewis symbols and that used dots and dashes to show the valence electrons and shared pairs of electrons (also known as a Lewis formula)
10. Lone Pair - a pair of electrons in the valence shell of an atom that is not shared with another atom. An unshared pair of electrons
11. Formal Charge - the apparent charge on an atom in a molecule or polyatomic ion as calculated by a set of rules that generally assign a bonding pair of electrons to the more electronegative of the two atoms held by the bond
12. Resonance Structure - a Lewis structure that contributes to the hybrid structure in resonance-stabilized systems a contributing structure
13. Valence Shell Electron Pair Repulsion Theory (VSEPR) - the geometry of a molecule at any given central atom is determined by the repulsions of both bonding and nonbonding (lone pair) electrons in the valence shell
14. Linear - a molecule consisting of atoms in a straight line
15. Planar Triangular - a molecule in which a central atom holds three other atoms located at the corners of an equilateral triangle and that includes the central atom at its center
16. Dipole - partial positive and partial negative charges separated by distance
17. Polar Molecule - a molecule in which individual bond polarities do not cancel and in which, therefore, the centers of density of negative and positive charges do not coincide
18. Dipole Moment - measurement of the separation of two opposite electrical charges. 
19. Hybrid Atomic Orbitals - orbitals formed by mixing two or more of the basic atomic orbitals of an atom and that make possible more effective overlaps with the orbitals of adjacent atoms than do ordinary atomic orbitals
20. sp Atomic Orbitals - a hybrid orbital formed by mixing one s and one p atomic orbital. The angle between a pair of sp hybrid orbitals is 180°
21. sp2 Atomic Orbitals  -One of a set of hybrid orbitals produced when one s orbital and two p orbitals are combined mathematically to form three new equivalent orbitals oriented toward the corners of a triangle 

eTextbook Reminder

As you read these content pages, also read the corresponding content in your etextbook. Work the example problems in the text as you read to make sure that you understand. The etextbook sections will be listed with the corresponding content pages on your schedule.  

Bonding Practice Problems

Before you begin, print the module practice problems found below.  You should complete a section of problems after covering that particular portion of the content. 

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