Metals.  Properties of elements determine what we can use them for.  For example, tungsten has the highest melting point of any metal (3410 0 C) but.

Slides:



Advertisements
Similar presentations
Bonding in Metals Section 15.3
Advertisements

This photograph of the tungsten filament from a light bulb was taken with a scanning electron microscope. The filament is magnified more than 100 times.
Ionic Bonding.
Chapter 7 Ionic and Metallic Bonding
Metallic Bonds and Metallic Properties
Metallic Bonds What are the forces that give a metal its structure as a solid? The cations in a metal form a lattice that is held in place by strong metallic.
Metallic Bonds What are the forces that give a ___________ its structure as a solid? The _____________ in a metal form a lattice that is held in place.
Chapter 7 Ionic and Metallic Bonding 7.3 Bonding in Metals 7.1 Ions
6.4 The Structure of Metals. What will we learn? What makes metals different? What properties do metals have and why? What are alloys and how are they.
Chapter 7 Ionic and Metallic Bonding 7.3 Bonding in Metals 7.1 Ions
Chapter 7 Ionic and Metallic Bonding
Metallic Bonding.
Section 7.3. Understanding Metal Atoms The behavior of a metal can be better explained if we understand that it is actually a collection of cations, rather.
I. Metallic Bonds  How atoms are held together in the solid form.  Metals hold onto their valence electrons very weakly.  Think of them as positive.
7.4 Metallic Bonds and the Properties of Metals
Metallic Bonds and Properties of Metals. Metals Metals are made up of closely packed cations surrounded by electrons, rather than neutral atoms or ions.
The Structure of Metals Brittany Braeutigan Ch. 6.4 Dustin Whitehead.
Chapter 8 (p ) Chemistry Mr. Gilbertson.
The Structure of Metals
1. Draw the Lewis dot structure for potassium bonded to chlorine. 2. Ionic bonds most commonly for between _______ and ___________. 3. A cation = ______________.
C HEMICAL B ONDS Chapter 6. I NTRODUCTION There are Three Types of Bonds: 1. Ionic Bonds – bond between a metal and a nonmetal 2. Covalent Bonds – bond.
Chemistry Chapter 8 Notes 3. Review Compounds Can all be represented by chemical formulas Are connected by chemical bonds Ionic Metallic Covalent Compounds.
Section 6.3 – Naming Compounds and Writing Formulas
Example 1: Metals are strong and easily shaped. Example 2: Many substances form brittle crystals which dissolve easily in water.
This photograph of the tungsten filament from a light bulb was taken with a scanning electron microscope. The filament is magnified more than 100 times.
Properties of bonding Mrs. Kay.
Chapter 15. Metallic Bonds Holds metals together by sharing the electrons (sea of electrons) VERY STRONG.
Notes 5-1 Atoms, Bonding and the Periodic Table Key Ideas: How is the reactivity of elements related to valence electrons in atoms? What does the periodic.
Chemical Bonds Review. WHAT DOES THE SYMBOL FOR AN ELEMENT MEAN IN AN ELECTRON DOT DIAGRAM / LEWIS DOT STRUCTURE?
The Structure of Metals
Metallic Bonds Metals can only bond to themselves (same element) Don’t transfer or share electrons (need to lose) Do form lattices in solid state 8-12.
Bonding in Metals. Objectives Be able to model the valence electrons of metal atoms Describe the arrangement of atoms in a metal Explain the importance.
Bonding in Metals Notes 5-4 Key Ideas: 1. How do the properties of metals and alloys compare? 2. How do metal atoms combine? 3. How does metallic bonding.
THE STRUCTURE OF METALS. METALLIC BONDS Bonds that occur only between metals Metals become cations, if there are no nonmetals to receive the electrons.
Section 4 – pg 198 Bonding in Metals
TOPIC 4 CHEMICAL BONDING AND STRUCTURE
Chapter 5 Atoms and Bonding. Valence Electrons and Bonding Valence electrons are those electrons that have the highest energy level and are held most.
WHY DO ATOMS BOND TOGETHER? ATOMS WANT TO ACHIEVE A STABLE ELECTRON CONFIGURATION (OR FULL OUTER SHELL OF VALENCE ELECTRONS).
Metallic Bonds Quartz.
Review Game Unit 5 Element Bonding. When the highest occupied energy level of an atom is filled with electrons, the atom is _______ and not likely to.
4.5 METALLIC BONDING. ESSENTIAL IDEA Metallic bonds involve a lattice of cations with delocalized electrons. NATURE OF SCIENCE (2.2) Use theories to explain.
Bonding. Three Types We will study... Ionic Bonding Covalent Bonding Metallic Bonding occurs between a metal and a nonmetal occurs between two nonmetals.
7.3 Bonding in Metals > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 7 Ionic and Metallic Bonding 7.1 Ions 7.2.
Chemistry Second 9 weeks 3. Review Ionic covalent--and-metallic- bonds?playlist=Chemistry
Metallic Bonds Metal atoms achieve electron configuration by losing electrons In metal, valence electrons are free to move among the atoms The metal atoms.
Metallic Bonds and Properties of Metals
Metallic Bonding.
This photograph of the tungsten filament from a light bulb was taken with a scanning electron microscope. The filament is magnified more than 100 times.
Metallic Bonds and Properties of Metals
Q2: What is the formula & name for a molecule created by a chlorate ion and aluminum. Write the formula for carbon tetrafluoride. 3. Write the name of.
Metallic Bonds are… How metal atoms are held together in the solid.
Metallic Bonding.
IONIC BONDING AND IONIC COMPOUNDS
Chapter 7 Ionic and Metallic Bonding 7.3 Bonding in Metals 7.1 Ions
Bonding In Metals Chapter 5 section 4.
Chapter 7 Ionic and Metallic Bonding 7.3 Bonding in Metals 7.1 Ions
This photograph of the tungsten filament from a light bulb was taken with a scanning electron microscope. The filament is magnified more than 100 times.
Chapter 7 Ionic and Metallic Bonding 7.3 Bonding in Metals 7.1 Ions
This photograph of the tungsten filament from a light bulb was taken with a scanning electron microscope. The filament is magnified more than 100 times.
Chapter 7 Ionic and Metallic Bonding 7.3 Bonding in Metals 7.1 Ions
The Structure of Metals
Section 4: The Structure of Metals
Metallic Bonding.
Chapter 7 Ionic and Metallic Bonding 7.3 Bonding in Metals 7.1 Ions
Chapter 7 Ionic and Metallic Bonding 7.3 Bonding in Metals 7.1 Ions
Sec 6.3 Naming Compounds and Writing Formulas
Metallic Bonding
Metallic Compounds.
Chapter 7 Ionic and Metallic Bonding 7.3 Bonding in Metals 7.1 Ions
Presentation transcript:

Metals

 Properties of elements determine what we can use them for.  For example, tungsten has the highest melting point of any metal ( C) but it is very ductile. For these reasons we use it in light bulbs as the filament.

 Metal atoms lose electrons to become stable.  If there is a nonmetal around to bond with, they will give it their electrons and become part of a stable compound.

 If there is not a nonmetal around, they have another solution.  They become cations with free electrons floating around them.  A metallic bond is the attraction between the cation and the free electrons around it.

 The cations in a metal form a lattice (like the lines on graph paper) that is held in place by strong metallic bonds between the cations and the surrounding valence electrons.  Because the total number of electrons does not change, the total metal is neutral.

 Metallic bonds in some metals are stronger than in other metals.  The more valence electrons in the shared pool, the stronger the metal will be.  Alkali metals can only contribute 1 electron each to the pool so they are weak.  Transition metals contribute more electrons so they are stronger.

 The stronger the metal, the higher its boiling point.

 Metals’ properties are caused by the movement of electrons within the metal lattice.

 Metals conduct electric current.  Electric current is a flow of charged particles.  The pool of shared electrons in metals act like a reservoir for electric current to pass through.

 Malleability is flexibility.  The metal lattice is flexible compared to a rigid ionic compound lattice (remember those shatter when struck).  When a metal lattice (a piece of metal) is struck, the ions shift slightly but do not break their metallic bonds.  For this same reason, metals are ductile.

 Alloys are mixtures of 2 or more elements (at least 1 of the elements must be a metal).  Alloys have the properties of metals.

 Copper alloys  Steel alloys  Others

 Copper alone is a soft metal.  Bronze = copper and tin  Bronze is hard and durable.  Brass = copper and zinc  Brass is softer and shinier than bronze but not as durable.

 Steel = iron + carbon  Carbon atoms fill in spaces in the iron lattice and add strength.  Stainless steel = iron + chromium  The chromium keeps the steel from rusting, but stainless steel is more brittle than steel containing carbon.  Other steels contain sulfur, manganese, phosphorus, and/or silicon.

 Alloys can be made to suit different needs based on what elements are added to them.

 Pure gold (24 karat) is easily worn and bent.  Adding silver, copper, nickel, or zinc to gold (and reducing its karat or purity) makes it stronger and more durable.

 Aluminum is light but weak.  When copper or manganese are added to aluminum it gains strength without gaining excessive weight.  This is used to build airplane bodies.

 Magnesium burns when exposed to air.  An aluminum-magnesium alloy stabilizes magnesium.  This compound is used to make very lightweight airplane parts.

 Bridge cables need to resist stretching and pulling while supporting a great amount of weight.  Special steel alloys are used for this.