Metallic Bonding Flashcards

1
Q

What structure do metals consist of?

A

Giant structures.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are the electrons like in metals?

A

The electrons in the outer shell of the metal atoms are delocalised.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What does delocalised mean?

A

Free to move around.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

How strong are the electrostatic forces of attraction in metallic bonding?

A

There are strong forces of electrostatic attraction between positive metal ions and the shared negative electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is metallic bonding?

A

When the forces of attraction hold the atoms together in a regular structure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

How strong is metallic bonding?

A

Metallic bonding is very strong.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are examples of compounds held together by metallic bonding?

A

Metallic elements and alloys.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What produces all of the properties of metals?

A

The delocalised electrons in the metallic bonds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

How much energy do the electrostatic forces in metals need to be broken, and why?

A

Lots of energy is needed to break them.

The electrostatic forces between the metal ions and delocalised electrons are very strong.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What are the melting and boiling points like in compounds with metallic bonds?

A

Most compounds with metallic bonds have high melting and boiling points.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What state are compounds with metallic bonds at room temperature?

A

They’re generally shiny solids at room temperature.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Are compounds with metallic bonds soluble in water?

A

Compounds with metallic bonds are not soluble in water.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Are metals denser than non-metals, and why?

A

Metals are generally denser than non-metals, as the ions in the metallic structure are packed closer together.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Are pure metals malleable?

A

Pure metals are malleable, as the layers of atoms can slide over each other.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What does malleable mean?

A

Something that can be hammered or rolled into flat sheets.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Are metals good conductors of heat and electricity, and why?

A

Yes, because the delocalised electrons carry electrical current and thermal (heat) energy through the material.

17
Q

Why do all metals have similar basic properties?

A

Yes, because all metals have metallic bonding.

18
Q

Why don’t non-metals usually have the same properties as metals?

A

Because non-metals don’t have metallic bonding.

19
Q

Since non-metals form a variety of different structures, what does this tell you about their chemical and physical properties?

A

Because non-metals form a variety of different structures, they also have a wide range of chemical and physical properties.

20
Q

How do non-metals usually look?

A

Non-metals are usually very dull-looking.

21
Q

How do non-metals usually feel?

A

More brittle than metals.

22
Q

What is the boiling point like in non-metals?

A

Non-metals have low boiling points.

23
Q

What state are non-metals at room temperature?

A

Non-metals are usually not solids at room temperature.

24
Q

How dense are non-metals?

A

Non-metals usually have a lower density.

25
Q

Do non-metals generally conduct electricity?

A

Non-metals usually don’t conduct electricity.

26
Q

How are the chemical properties different in non-metals?

A

Non-metals tend to gain electrons to form full outer shells (they are on the top and right-hand side of the periodic table, and their outer shells are generally over half-filled).

27
Q

How are the chemical properties different in metals?

A

Metals lose electrons to gain full outer shells (they are found at the bottom and left-hand side of the periodic table, and their outer shells are generally under half-filled).