1. Types of Chemical Bonds
Force of attraction
Ionic vs. Covalent Bonds
Ionic Bonds Overview
Covalent Bonds
Single, Double and Triple Bonds
Polar Covalent Bonds
Metallic Bonds

2. Force of Attraction __________ Within molecules
The force that holds atoms of molecules together
Intermolecular Force
Between molecules
The force that holds ________

3. Intramolecular Forces (Bonds)
Ionic Bonds
Covalent (Molecular) Bonds

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5. Ionic Bonds
Occurs when the Electronegativity difference (EN) is ___________
___________
Involves the transfer of electrons from less EN atoms (metals) to an atom of greater EN (non-metal)
Oppositely charged ions are attracted to each other

6. Ionic Bonds
In ionic compounds, the non-metal rips away the electron(s) from the metal because the metals loosely hold their electrons
This creates a positive and negative ion which attract each other making them stick together (opposites attract)

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8. Forming Ionic Bonds
NaCl
MgCl2

9. Properties of Ionic Bonds
A HIGH intramolecular force of attraction results in ionic compounds being _____________
i.e. Table Salt has a melting point of 801 °C
Solid ionic compounds form a crystal lattice, which is repeating pattern of particles.
Remember, NaCl represents a repeating ratio not a specific number of atoms in a molecule

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11. Ionic Compounds in Water
___________
This results in the compounds breaking apart in to form electrolytes (e.g. salt easily dissolves in water).

12. Covalent (Molecular) Bonds
__________
Made up of 2 non-metals
Involves the sharing of 1,2, or 3 pairs of electrons.

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14. Covalent Compounds
Covalent compounds are formed when non-metals share electrons to fill their outer electron orbit (shell).
If we draw the Lewis Structure for Fluorine, we can see that it needs __________
__________
If it bonds with another fluorine atom, we draw the shared pair of electrons between the two atoms. F F F
Shared electron pair  both now have 8 in outer orbit

15. Covalent Compounds

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17. Multiple Covalent BondsH O C O
Water – Single bond because ONE pair of electrons are shared
Carbon Monoxide – Triple Bond because ______ O C
Carbon Dioxide – Double bond because TWO pairs of electrons are shared

18. Multiple Covalent Bonds

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20. Types of Covalent Bonds
Non Polar Covalent Bond: When EN difference is zero. Equal sharing of electrons
Polar Covalent Bond: _________

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22. Polar Covalent Bonds

23. Metallic Bond Occurs between many metal atoms.
Valence electrons are released into a shared pool of electrons.
Electrons move freely through a fixed lattice of atoms.
____________

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25. Polar Molecules Example: H2O
Oxygen is more electronegative than hydrogen
This causes the electrons to spend more time near the oxygen atom and less near the hydrogens
_________

26. Non-polar molecule containing polar bonds
If the molecule contains more than 2 atoms and is symmetrical in shape, the charges cancel out and molecule is NON polar. i.e. CO2