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Understanding Chemical Bonding and Isomers in Hydrocarbons

This section delves into the essentials of chemical bonding and isomers, focusing on hydrocarbons and their properties. It explains how intermolecular forces vary with the size of hydrocarbon molecules, emphasizing that larger molecules have stronger intermolecular forces and higher boiling points. The concept of valence electrons is addressed, shedding light on ionic bonding through examples of magnesium and fluorine. Additionally, structural formulas and the difference between straight-chain and branched-chain alkanes are explored, along with the implications of isomers on boiling points.

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Understanding Chemical Bonding and Isomers in Hydrocarbons

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  1. Chemical Bonding & Isomers Pages 181 - 191

  2. Recall the petroleum refining….What is this next slide a diagram of?

  3. What are intermolecular forces?

  4. Page 181

  5. The larger the hydrocarbon molecules, the _______________, the intermolecular force. The larger the hydrocarbon molecules, the STRONGERthe intermolecular force.

  6. The larger the hydrocarbon molecules, the _______________, the boiling point. The larger the hydrocarbon molecules, the HIGHERthe boiling point.

  7. Do you remember why atoms are attracted to other atoms? How many valence electrons does a C atom have?

  8. Ions and Ionic bonding • From pages 32 - 34

  9. Find Mg on the Periodic Table…

  10. If an atom of Mg became an ion, • How does its electron structure change? • What would be its charge? • What would it be classified as?

  11. If an atom of F became an ion, • How its electron structure change? • What would be its charge? • What would it be classified as?

  12. Chemical Bonding • Organic chemistry – study of hydrocarbons and their derivatives • Hydrocarbons – composed of carbon chains (backbone) with H atoms attached to remaining bonding sites

  13. Chemical Bonding • Electron-dot formulas • Each dot represents 1 valence e- • Dots placed between chem symbols represent electrons shared by atoms

  14. Single covalent bond – a pair of electrons are shared between two atoms Ex) methane CH4 Carbon has 4 valence e- 4 H each have 1 valence e-

  15. Structural formulas • A line can be used to represent a pair of shared e- • Remember – molecules are not 2-dimensional

  16. Alkanes • Alkanes - Simple hydrocarbon family • Each C forms single covalent bonds w/ 4 other atoms • Because each C atom is bonded to the maximum # of other atoms, it is said to be saturated

  17. Alkanes • Straight-chainalkane – each C is linked to only 1 or 2 other C atoms

  18. Straight-chain Alkanes

  19. Alkanes • Branched-chainalkane – 1 or more C are linked to 3 or 4 other C atoms

  20. Isomers - molecules with identical chemical formulas but different structural formulas Ex) octane C8H18

  21. Page 187

  22. Page 187

  23. Isomers and Boiling Point Q. Which isomer would have the lowest boiling point temperature?

  24. Isomers and Boiling Point • The molecule on the right… branchedshaped decreases surface area which results in weaker intermolecular forces. This makes it easier for the molecules to evaporate.

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