Bonding introduction
Sponsored Links
This presentation is the property of its rightful owner.
1 / 49

Bonding Introduction PowerPoint PPT Presentation

  • Uploaded on
  • Presentation posted in: General

Bonding Introduction. Octet rule Types of bonds Lewis structures Geometry. Video 5.1. Types of Bonds. Octet Rule Review. Atoms bond with other atoms by sharing or transferring electrons in order to achieve a stable octet (8 valence electrons). Bonding creates stability!

Download Presentation

Bonding Introduction

An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.

- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -

Presentation Transcript

Bonding introduction

Bonding Introduction

Octet rule

Types of bonds

Lewis structures


Video 5 1

Video 5.1

Types of Bonds

Octet rule review

Octet Rule Review

Atoms bond with other atoms by sharing or transferring electrons in order to achieve a stableoctet(8 valence electrons). Bonding creates stability!

*When bonds are formed energy is ___________.

*When bonds are broken energy is ___________.



Ionic bonds

Ionic Bonds

  • Transfer of electrons from the cation to the anion (metal to nonmetal).

  • High melting point and boiling point

  • Mostly hardcrystalline solids

  • Conduct as liquid (either melted or dissolved) due to mobile ions.

Ionic bonds1

Ionic Bonds

Sodium Chloride: NaCl (table salt) properties:

  • Hard

  • Solid crystals

  • High melting point, forget boiling!

  • Liquid phase conducts (electrolytes are salts)

Metallic bonds

Metallic Bonds

  • Metals only

  • All metals lose their valence electrons and form a sea of electrons

  • High melting point and boiling point

  • Insoluble in water

  • Always able to conduct heat and electric due to mobile electrons

  • Malleable

  • Ductile

Metallic bonds1

Metallic Bonds

Copper (Cu) properties:

  • Hard solid

  • High melting point, forget boiling!

  • Malleable and ductile

  • Conductor

  • Can’t dissolve

Metallic bonds sea of electrons

Metallic BondsSea of electrons

Copper (I) ions Copper (II) ions

Covalent bonds molecular

Covalent Bonds (Molecular)

  • Nonmetals only

  • Share electrons between atoms

  • Low melting point and boiling point

  • Never conduct heat or electricity

  • Soft solid or gas

Covalent bonds

Covalent Bonds

Dextrose C6H12O6 (Sugar) properties:

  • Soft

  • Melts easily in sauce pans for caramel

  • Doesn’t conduct (nonelectrolyte)

What type of bond is created

What type of bond is created?

M+ NM = Ionic

  • Ca + O

  • K + Br

  • S + Cl

  • I + S

  • Li + Mg

  • Ba + S

M + NM = Ionic

NM + NM = Covalent

NM + NM = Covalent

M + M = Metallic

M + NM = Ionic

Video 5 2

Video 5.2

Ionic Compounds

Review find the ionic formula

Review: Find the ionic formula:




  • K + Br

  • Mg + Cl

  • Na + S

  • Ca + S










Draw lewis structures

Draw Lewis structures:





Which subatomic particle is involved in bonding

Which subatomic particle is involved in bonding?

Electrons only!

Geometry of ionic crystals

Geometry of ionic crystals

Ionic crystal


Video 5 3

Video 5.3

Covalent Compounds

Covalent lewis structures rules ccl4

Covalent Lewis Structures Rules: CCl4

C: 4 + 4Cl: 7 = 32 valence e-

  • Add up all valence e-

  • Draw a skeletal structure with bonds between elements. Least frequent element in the middle.

  • Subtract 2e- from total for each bond drawn.

  • Draw in remaining e- to fill each atom’s octet.

  • Evaluate: each atom should have 8 e- only.







“Valence shell electron pair repulsion” is a model for molecules. Lone electron pairs are repelled by one another and should be placed as far apart as possible.



  • Linear: The molecule is on one plane (flat) such as CO2 or H2.

  • Bent: The molecule is bent at angle like H2O due to unshared electrons and two bonding pairs on the central atom.



  • Pyramidal: The molecule has a triangular shape like NH3 due to a lone pair and three bonding pairs on the central atom.

  • Tetrahedral: The molecule has four

    bonding pairs and no lone pairs on

    the central atom like CH4.



  • Draw the following molecules and identify their geometry:

  • PCl3

  • SiCl2H2

  • Br2

  • H2S





Video 5 4

Video 5.4

Bond Polarity

Bond polarity

Bond Polarity

The earth has two poles; North and South.

A magnet also has two poles.

Bonds may have two poles. This means one element is charged different than the other.

If a bond is polar, the two elements have different electronegativities. The element with a higher electronegativity will be more negative.

Bond polarity1

Bond Polarity

Bond polarity2

Bond Polarity

Nonpolar bond

Nonpolar Bond

Bond polarity3

Bond Polarity

Ionic polar or nonpolar

Ionic, polar or nonpolar?



  • C-Br

  • Na-S

  • C-C

  • H-O

  • K-O

  • Be-B

  • As-O

  • N-O

  • C-O

  • F-F

  • S-C

  • N-H











Covalent bonding


  • If 2 atoms or more form a bond with the same electronegativity the bonds are nonpolar and they share e- equally. ( F-F )

  • If there is an electronegativity difference between bonded atoms, the bonds are polar and e- are pulled toward the more electronegative atom. (H-F)

  • If a bond is polar, the molecule will have a slightly negative and slightly positive side, like 2 poles of a magnet.

Video 5 5

Video 5.5

Molecular Polarity

Molecular polarity

Molecular Polarity

  • A polar molecule will be asymmetrical.

  • A nonpolar molecule will have a symmetrical shape or all nonpolar bonds.

Molecular polarity1

Molecular Polarity

Which are polar molecules? Show charges.





















Molecular polarity2

Molecular Polarity

Water is polar, and like dissolves like, so only polar molecules are soluble in water. Polar molecules are also attracted to an electric field.

Molecular polarity3

Molecular Polarity

  • As you can see, normally polar molecules are unaligned.

  • When a electric source comes by, the molecules quickly align themselves.

Video 5 6

Video 5.6


Bonding introduction


  • Intramolecular forces is another name for bonds, that keep elements together in compounds.

  • Intermolecularforces of attraction are weaker than bonds, but are responsible for holding a substance together (multiple molecules in a confined area).

Bonding introduction


  • The stronger the IMF, the tighter the structure (solid). The melting and boiling points will be high.

  • The weaker the IMF, the looser the structure (gas). The melting and boiling points will be low.

Dipole dipole


  • Dipole-Dipole attractions are strong forces betweenpolarmolecules. It is like static holding the + and – charges together.

Hydrogen bonding

Hydrogen Bonding

A special case: Hydrogen Bonds are the strongestbonds between Hydrogen and very electronegative atoms such as F, O and N. (H bonds are FON!) For example, H2O and HF, due to their polarity, they will attract each other.

London dispersion forces ldf

London Dispersion Forces (LDF)

The weakest attraction betweennonpolarmolecules occur because electrons temporarily shift creating a temporary + and – charge. The more electrons the compound has, the stronger the force is.



  • From weak to strong:

    • Nonpolar LDF

    • Polar Dipole Dipole forces

    • Hydrogen bonds

    • Covalent Bonds

    • Ionic Bonds

    • Metallic Bonds

Class notes

Class Notes

Show the individual and bonded lewis structures

Show the individual and bonded Lewis structures:

  • Li and F

  • Mg and O

  • Be and S

  • What did all the cations do?

  • What did all the anions do?

  • Which of the subatomic particles were changed and how were they changed?

Type of bonding

Type of Bonding?

  • CaCl2

  • CO2

  • H2O

  • BaSO4

  • K2O

  • NaF

  • Na2CO3

  • CH4

  • SO3

  • LiBr

  • MgO

  • NH4Cl

  • HCl

  • KI

  • NaOH

  • NO2

  • AlPO4

  • FeCl3

  • P2O5

  • N2O3

  • Login