CH110-120 Chapter 6 Lecture Notes Powerpoint

CH110-120 Chapter 6 Lecture Notes Powerpoint - Chapter 6...

Info iconThis preview shows pages 1–13. Sign up to view the full content.

View Full Document Right Arrow Icon
Chapter 6 – Fundamentals of Chemical Bonding 6.1 Overview of Bonding 6.2 Lewis Structures 6.3 Molecular Shapes: Tetrahedral Systems 6.4 Other Molecular Shapes 6.5 Properties of Covalent Bonds
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
6.1 Overview of Bonding Electrons and nuclei are continually moving. But, in the motion, they arrange themselves in ways that optimize the net attractive forces among the electrons and the nuclei. The net electrical energy can be calculated.
Background image of page 2
Chemical Bond Formation Electrons and nuclei in a molecule balance all interactions to give the molecule stability. Balance is achieved when the electrons are concentrated between the nuclei. The electrons are shared between the nuclei and this sharing is called a covalent bond .
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
The Hydrogen Molecule Figure 6.2
Background image of page 4
Bond Length and Bond Energy Bond length – the separation distance where the molecule is most stable Bond energy – the amount of stability at this separation distance, also known as the strength of the bond.
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Example 6 -1 The bond length of molecular fluorine is 142 pm, and the bond energy is 155 kJ/mol. Draw a figure similar to Figure 6 – 2 that includes both F 2 and H 2 . Write a caption for the figure that summarizes the comparison of these two diatomic molecules.
Background image of page 6
Lets look at F 2 The fluorine atom has 7 valence electrons 1s 2 2s 2 2p 5 It wants to have 8 valence electrons If two fluorine atoms come together, they can share the 8 th electron. How do they come together? Aka “Noble gas configuration”
Background image of page 7

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Unequal Electron Sharing A pure covalent bond occurs only when two identical atoms are bonded: N 2 When two dissimilar atoms form a covalent bond, the electron pair is unequally shared, the bond is called a polar covalent bond Therefore, the electrons are nearer to one of the atoms, and that atom acquires a partial negative charge . And consequently the other atom has a partial positive charge .
Background image of page 8
Polar Covalent Bonds Bond is referred to as polar and the molecule can be called a dipole (having two poles) The Greek symbol delta “ δ ” is used to indicate partial charge How do you determine which atom has the partial negative charge and which atom has the partial positive charge? Positive end negative end dipole
Background image of page 9

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Electronegativity Electronegativity – the ability to attract bonding electrons. Denoted by the Greek symbol chi, χ When two atoms have different electronegativities, the bond between them is polar. The bigger the difference in electronegativities, the more polar the bond. There are periodic trends in electronegativity – you need to know these general trends!
Background image of page 10
Less electronegativity Most electronegativity
Background image of page 11

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Polar Bonds From graph, you can see that nonmetals are more electronegative than metals. In general:
Background image of page 12
Image of page 13
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

Page1 / 55

CH110-120 Chapter 6 Lecture Notes Powerpoint - Chapter 6...

This preview shows document pages 1 - 13. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online