1. Draw the Lewis dot structure for potassium bonded to chlorine.

2. Ionic bonds most commonly for between _______ and ___________.

3. A cation = ______________.

Day 1 4-8

metals

nonmetalsa positive

ion

1.Lewis dot structure for sodium = _____ How many times can it bond?

2.Lewis dot structure for sulfur = _____ How many times can it bond?

3.Lewis dot structure for the compound formed when sodium and sulfur bond to each other = ______

Electrostatic Force – an interaction between charged particles

Opposites –

Like charges –

Attract

Repel

3 main bond types:• Ionic

• Polar covalent

• Nonpolar covalent

Cation – positive ion

Anion – negative ion

Ions – charged particles

Br

LiBANG

BrLi

But they don’t separate … WHY? + -

Electrostatic Force

Ionic bonds most commonly form between metals and

nonmetals!

Ionic bonds are made up of charged pieces (ions)

Ions can be made up of one element or a combination of elements (polyatomic ions)

Ionic Compounds:

high melting points – strong bonds

Brittle

dissolve in water to produce mobile ions – good conductors

http://www.youtube.com/watch?v=QqjcCvzWwww

http://www.youtube.com/watch?v=bK9nMHTLhmk

http://www.youtube.com/watch?v=BCYrNU-7SfA

Electrostatic force

Anion

Ionic bond

Malleable

Alloy

Cation

What are some properties that are unique to metals?

Metals consist of closely packed closely packed cations and loosely held valence electrons rather than neutral atoms.

The valence electrons of atoms in a pure metal can be modeled as a sea of electrons.

The valence electrons are mobile and can drift freely from one part of the metal to another.

Metallic bonds = the forces of attraction between the free-floating valence electrons and the positively charged metal ions.

Alloys = mixtures of two or more elements, at least one of which is a metal.

Example = Brass is an alloy of copper and zinc.

- Alloys are important because their properties are often superior to those of their component elements (steels).

Alloys•Some of the most important alloys today are steels.

• The principal elements in most steels, in addition to iron and carbon, are boron, chromium, manganese, molybdenum, nickel, tungsten, and vanadium.

• Steels have a wide range of useful properties, such as corrosion resistance, ductility, hardness, and toughness.

Stainless Steel80.6% Fe18.0% Cr0.4% C1.0% Ni

Key Concepts

•The valence electrons of atoms in a pure metal can be modeled as a sea of electrons.

•Alloys are important because their properties are often superior to those of their component elements.

Glossary Terms

• metallic bond: the force of attraction that holds metals together; it consists of the attraction of free-floating valence electrons for positively charged metal ions

• alloy: a mixture composed of two or more elements, at least one of which is a metal

• Metals are made up of closely packed cations surrounded by a sea of electrons.

• The sea-of-electrons model explains why metals are good conductors and why they are ductile and malleable.

Bonding and Interactions