Solid Properties on Malleability and Ductility

Metals

Lesson Objectives

• Describe the characteristic properties of metals. Identify the location of metals in the periodic table. Explain how and why the reactivity of metals changes in the periodic table.

Properties of Metals

• Malleable-Can be shaped and does not break easily.

• Ductile-Can be pulled into long sheets of metal or wire.

• Thermal Conductivity-Allows heat to pass easily-Example Pans.

• Electrical Conductivity-Allows the easy flow of electric current.

Multiple Choice

Metallic bonds give metals all of the following properties except for

• malleability

• ductility

• being conductive

• being translucent

Multiple Choice

Which would be the best example of a metal displaying malleability?

Multiple Choice

Select the Vocabulary Word: Ability of a substance to be hammered or shaped into thin sheets

• Ductility

• Resonance

• Hydrogen Bonding

• Malleability

Multiple Choice

Select the Vocabulary Word: Ability of a substance to be drawn into a wire

• Malleability

• Ductility

• Resonance

Multiple Choice

What is the ability of a substance to allow heat, sound, or electricity to flow through it?

• Malleability
• Ductility
• Solubility
• Conductivity

Malleability means it can be bent into different shapes.

Metals are typically malleable, ductile, conductive, and lustrous.

Multiple Choice

What does malleable mean?

• able to be shaped
• will break easily
• can be used for wire
• is shiny

Multiple Choice

Which one of these objects is malleable?

• Antique Ceramic Vase

• Steel Pole Fence Post

• Glass Table Top

• Marbel Sculpture

Physical Properties of Metals

• Lustrous-Shiny to the eye.

• Opaque-Does not allow light to pass through.

• High Melting Points (with some exceptions).

Multiple Choice

Based on the physical appearance of the two crystal samples, which is a metal?

• Sample A

• Sample B

• Sample A and B

How are Metals identified

• Alkali Metals Group 1

• Alkaline Earth Metals Group 2

• Transition Metals Group 3-12

Alkali Metals

• Shiny

• Soft

• Extremley Reactive

• One Valence Electron available to give up to another element.

Alkaline Earth Metals

1.Very Shiny

2.Hard, more Dense, Less Reactive

3.Give up 2 Valence Electrons.

Reactive Trends Periods of the Periodic Table

Electrons are used to bond atoms together. Group one will share with group 2.

Multiple Choice

What type of metal is Lithium (LI) ?

• Alkali Earth Metals

• Alkali Metals

• Transition

Electrical & thermal conductivity

​Electrical conductor

​Electrical insulator

Multiple Choice

TRUE OR FALSE

Thermal conductors allow heat to be transferred through them.

• TRUE

• FALSE

Multiple Choice

The bulbs would light up when--

• the material did not allow electricity to travel through

• the atoms of the material kept electrons inside; electrons could not move

• the material allowed electricity to travel through it

Multiple Choice

Materials which allow electrons to move from atom to atom are called--

• conductors

• non-conductors

Multiple Choice

A material is a non-conductor. What is true of the material?

• It allows electrons to move freely between atoms

• It does not allow electrons to move between atoms

Multiple Select

A conductivity test was done on four objects. Which ones were conductors. Select all that apply.

• Silver earrings

• Plastic ring that looks like a spider

• Bracelet made of wood

• Copper necklace

Multiple Choice

When the light bulbs on the conductivity tester light up, this means that--

• Electrons are leaving the conductivity tester, flowing into the material, and then flowing back into the conductivity tester

• Electrons are not able to move from the conductivity tester into the materail being tested.

Multiple Select

Which two materials can be used to light the bulb up?

Multiple Choice

We use rubber gloves to hold a hot frying pan because the glove .......................

• does not conduct heat

• does not slip

• conducts electricity

• absorbs water

Ionic and Metallic Compounds

​Ionic Compounds

​The electrostatic force that holds oppositely charged particles together in an ionic compound is an ionic bond.

​Compounds that contain ionic bonds are called ionic compounds.

​Properties of Ionic Cmpds

​Strong attractions among the positive ions and negative ions in an ionic compound result in the formation of a crystal lattice.

​A crystal lattice is a 3-D geometric arrangement of particles. Each positive ion is surrounded by negative ions and each negative ion is surrounded by positive ions

​Physical Properties

​High melting & boiling points

​Hard yet brittle

​Does not conduct electricity in the solid state.

​However, ionic compounds are excellent conductors, known as electrolytes, in the liquid or aqueous (dissolved in water) states

​Lattice Energy

​The energy required to separate the ions of an ionic compound is called lattice energy.

​

​Lattice energy is greater when the charge on the ions is greater.

​Lattice energy is greater when the distance between the two ions is smaller.

​Metallic Bonds

​Electron Sea Model proposes that all the metal atoms in a metallic solid contribute their valence electrons to form a "sea" of electrons that surround the metal cations in the lattice.

​Delocalized Electrons

​The electrons are not held by any specific atom and they are free to move.

​A metallic bond is the attraction of a metallic cation for delocalized electrons.

Multiple Choice

What is the structure of metallic compounds?

• Irregular arrangement of metal atoms surrounded by a sea of delocalized electrons

• Random arrangement of metal atoms surrounded by a sea of delocalized electrons

• Regular arrangement of metal atoms surrounded by a sea of delocalized electrons

• Regular arrangement of metal atoms surrounded by a sea of localized electrons

Multiple Choice

What type of bond is illustrated in this image?

• Metallic

• Ionic

• Covalent

• James

• Polar Covalent

Multiple Choice

How does metallic bondbondings contribute to the ductility and malleabilityof metals?

• They allow layers of atoms to slide past each other without breaking the bond.

• They create rigid structures that resist deformation.

• They increase the melting point of metals, making them less ductile.

• They make the metal atoms immobile, reducing ductility.

Multiple Choice

Measure of the tendency of an atom to attract a bonding pair of electrons is known as...

• electronegativity

• bond polarity

• angular momentum

• valence electrons

Multiple Choice

A ________ is located the outermost shell of an atom.

• Proton

• Neuton

• Valence Electron

• Core Electron

Multiple Choice

Metallic bonds are best described as metal cations in a sea of:

• Free Electrons

• Photons

• Anions

• Neutrons

Multiple Choice

_____ bonding takes place between a metal and a nonmetal.

• Covalent

• Metallic

• Ionic

• Hydrogen

Multiple Choice

In covalent bonding, electrons are:

• Dissociated

• Transferred

• Freed

• Shared

Multiple Choice

The diagram shows metallic bonding.

Which labels are correct?

• X: atomic nucleus

  Y: outer electron

• X: metal atom

  Y: mobile electron

• X: metal cation

  Y: mobile electron

• X: positive ion

  Y: negative ion

​Properties of Metals

​In general metals have high melting and boiling points (except Hg is a liquid at room temperature).

Malleability, Ductility, Durability

Thermal & Electrical conductivity

Hardness & Strength (More delocalized electrons means greater strength)

​Alloys

​A homogeneous mixture of metals

​

​Alloys are made to vary properties of metals (increase strength)

​

​Substitutional Alloys - two metals of similar size are mixed.

​Interstitial Alloys - Large and small metals are mixed.

Multiple Choice

A mixture of metals is a/an _.

• polyatomic ion
• alloy
• transition metal
• isotope

Multiple Choice

Name this compound.    BN

• boron mononitride
• beryllium nitride
• monoberyllium mononitride
• monoboron nitride