Chem I Unit 7 Metallic Bonds

Last updated about 1 month ago

5 questions

Note from the author:

1

This is a lesson metallic bonds

What are metallic bonds? How do metallic bonds contribute to the characteristics of metals?


The key to the characteristics of metals is the "sea of electrons" that flows around the nuclei of the atoms.
Watch this short animation to see how a metallic bond or sea of electrons is established.
The other videos explain the importance of the sea of electrons and how it behaves.

Which describes a metallic bond and the so-called sea of electrons?

the electrons remain as close to the nuclei as possible

the electrons from inner levels float freely through the piece of metal

the valence electrons move throughout the piece of metal

What does the term "delocalized" mean in reference to electrons in metals?

the electrons act in a crazy and unpredictable manor, the are the "loco" electrons in the atoms

the electrons stay attached to one atom, they are "local" and stay close to "home"

the electrons have some mobility and move among several atoms, they can leave the "home" atom

Why don't metals break when they are hit?
Choose all correct options.

The nuclei of the atoms all repel each other.

The atoms have some mobility and can move around within the cloud of electrons.

They electrons act like "goo" to hold the atoms near each other.

How does the strength of metallic bonds compare to the strengths of other chemical bonds?

Metallic bonds are weak when compared to ionic and covalent bonds.

Metallic bonds are the strongest bonds.

Metallic bond strength is in the middle between the strengths of ionic and covalent bonds.

Why are metals able to conduct heat well?

The electrons have increased mobility as the temperature increases.

The protons have increased mobility as the temperature increases.

All of the atoms within the piece of metal are able to move around as temperature increases.

Which describes a metallic bond and the so-called sea of electrons?

the electrons remain as close to the nuclei as possible

the electrons from inner levels float freely through the piece of metal

the valence electrons move throughout the piece of metal

What does the term "delocalized" mean in reference to electrons in metals?

the electrons act in a crazy and unpredictable manor, the are the "loco" electrons in the atoms

the electrons stay attached to one atom, they are "local" and stay close to "home"

the electrons have some mobility and move among several atoms, they can leave the "home" atom

Why don't metals break when they are hit?
Choose all correct options.

The nuclei of the atoms all repel each other.

The atoms have some mobility and can move around within the cloud of electrons.

They electrons act like "goo" to hold the atoms near each other.

How does the strength of metallic bonds compare to the strengths of other chemical bonds?

Metallic bonds are weak when compared to ionic and covalent bonds.

Metallic bonds are the strongest bonds.

Metallic bond strength is in the middle between the strengths of ionic and covalent bonds.

Why are metals able to conduct heat well?

The electrons have increased mobility as the temperature increases.

The protons have increased mobility as the temperature increases.

All of the atoms within the piece of metal are able to move around as temperature increases.

Chem I Unit 7 Metallic Bonds

Chem I Unit 7 Metallic Bonds

Which describes a metallic bond and the so-called sea of electrons?

What does the term "delocalized" mean in reference to electrons in metals?

Why don't metals break when they are hit?Choose all correct options.

How does the strength of metallic bonds compare to the strengths of other chemical bonds?

Why are metals able to conduct heat well?

Why don't metals break when they are hit?
Choose all correct options.