Metallic Bonds and the Properties of Metals (Chapter 6, Lesson 4)

Question 1

Electron Sea Model

Answer 1

all metal atoms in a metallic contribute their valence electrons to form a “sea” of electrons that surrounds the metal cations in the lattice.

Question 2

The outer energy levels of the metals atoms overlap in…

Answer 2

a metal lattice

Question 3

Delocalized electrons

Answer 3

the electrons in the outer energy levels of bonding metallic atoms

Question 4

What happens when an atom’s outer electrons move throughout the solid?

Answer 4

a metallic cation is formed

Question 5

Metallic Bond

Answer 5

the attraction of a metallic cation for delocalized electrons

Question 6

Physical properties of metals

Answer 6

• melting and boiling points
• thermal and electrical conductivity
• malleability, ductility, and durability
• hardness and strength

Question 7

(+ or o) Metals have moderately high melting points and high boiling points

Answer 7

+

Question 8

Why are melting points of metals less extreme than boiling points?

Answer 8

The cations and electrons are mobile. Doesn’t take much energy to move them.

Question 9

As the number of de localized electrons increases…

Answer 9

so does hardness and strength

Question 10

Alloy

Answer 10

mixtures of elements that have metallic properties

Question 11

(+ or o) alloys are the same as the properties of the elements that they contain

Answer 11

o, they differ

Question 12

What are the two basic types alloy are classified into?

Answer 12

• substitutional alloy
• interstitial alloy

Question 13

Substitutional alloy

Answer 13

some of the atoms in the original metal are replaced by other metals if similar atomic size

Question 14

Interstitial alloy

Answer 14

formed when the small holes in a metallic crystal are formed with smaller atoms