Guiding Question:

How does the type of bond relate to the properties of materials?

Quarter 3-Unit 2Five Types of Bonds!

Ionic Polar Covalent Non-polar Covalent Metallic Network Covalent

You will need to recognize which is which by looking at the formula.

You will need to know the properties of the five types including:◦ appearance/texture◦ melting point◦ Conductivity◦ solubility.

What are the five types of bonds you will need to know?

Put “bond types and properties” in the middle

Put the five types of bonds around the outside

Start your popplet!

You need to look at the formula to see if the compound contains metals or non-metals or both.

Recognizing Bond Type from the formulas!

Contain at least one metal and one non-metal.

May contain a polyatomic ion.

Examples:

◦ CuO

◦ Na3P

◦ CaCO3

Ionic Compounds (transfer electrons from metal to non-metal)

METAL

NON-METAL

Ionic compounds are also called SALTS.

Most are white crystals.

They are hard and brittle solids.

Appearance of Ionic Compounds

Include how to recognize ionic compounds from the formula

Include appearance and textures.

Add to your popplet!

First let’s remember how to decide if it’s covalent or not.

Then use the Lewis structure to know if it’s polar or non-polar.

Covalent Compounds can be polar or non-polar.

Contain ONLY non-metals.

Examples:

◦ CH4

◦ H2O

◦ NH3

Covalent Compounds(share electrons)

ALL NON-METALS

Polar molecules are ASSYMETRICAL – not balanced.

Use Lewis Structure:◦ Unshared pairs make

it assymetrical (pyramid or bent)

◦ Different atoms around the central atom also make it assymetrical.

Polar Covalent Molecules – electrons are unequally shared;one side is slightly positive and one is slightly negative.

H2O is a bent molecule so it is Assymetrical and POLAR

CH3Cl is polar

Non-Polar molecules are SYMETRICAL – balanced.

Use Lewis Structure:◦ No unshared pairs

◦ Same atoms surround the central atom.

Non-Polar Covalent Molecules – electrons are equally shared;there is no charge difference on each side of molecule

CO2 is a linear molecule so it is Symetrical and NON-POLAR

Some polar and non-polar covalent molecules

More examples of polar and non-polar covalent molecules

Soft solids, liquids, or gases at room temp.

Polar and non-polar covalent molecules are usually…

Include how to recognize covalent compounds from the formula

Include appearance and textures.

Add to your popplet!

Formula will contain one metal.

Example:

◦ Cu

◦ Fe

◦ Ag

◦ Al

Metallic Bonds – bonds within metals

Metallic BondsIn ionic bonding we know metals lose electrons to form positive ions M+ M is any

metalM2+or

This is to achieve a completely full outer electron shell

This also happens in metallic bonding

- but because there are no non-metals to take the electrons, now the electrons have nowhere to go!

e-

e-

e-

e-

The valence electrons get passed from one atom to the next like a “hot potato”!This forms a “sea of negative charge” that flows around the positive metal ions.

M+M+M+ M+M+M+M+M+M+

M+M+M+ M+M+M+M+M+M+

M+M+M+ M+M+M+M+M+M+

M+M+M+ M+M+M+M+M+M+

M+M+M+ M+M+M+M+M+M+

M+M+M+ M+M+M+M+M+M+

Sea of electrons

How metallic bonding worksValence electrons move around holding the + metal ions in place

How might this structure lead to some of the properties we know about metals?

Shiny and malleable (bendable)

Metals are usually…

Include how to recognize metallic compounds from the formula

Include appearance and textures.

Add to your popplet!

You need to remember:

DIAMOND and SAND are network covalent solids.

Diamond will be written:

C – Diamond

◦ Sand is SiO2

Network Covalent Solids

Network Covalent Solids

In some substances, millions of atoms join together by covalent bonding. This produces giant covalent structures, not molecules.

Each atom is linked to every other atom in the structure which makes them VERY strong.

This also means that almost all giant covalent structure are hard and NOT brittle (don’t crack easily).

Diamond- a form of carbonDiamond is a rare form of carbon in which each atom is covalently bonded to four others.

This pattern arrangement is repeated millions of times to create a giant lattice.

C

C

CC

C

This makes diamond VERY hard and strong.

Diamond coated drill bit!

Sand – a form of Silicon Dioxide (a network covalent solid)

Include how to recognize network covalent molecules

Include appearance and textures.

Add to your popplet!