The Solid State Flashcards

1
Q

The stronger the intermolecular forces, the ___________ movement of the particles

A

Slower

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

What are the properties of amorphous solids?

A
  • random arrangement of particles
  • particles have no orderly structure
  • macroscopic structures lack well defined faces and shapes
  • many are mixtures of molecules that do not stack up well together
  • glass and rubber are examples
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are the properties of Crystalline Solids?

A
  • atoms, ions, or molecules are arranged in an orderly fashion that follows a pattern of repetition in three dimensions
  • macroscopic structures usually have flat surfaces that make definite angles to one another
  • ionic solids and quarts are examples
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Segments in crystalline solids that repeat in three dimensions

A

Unit cells

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

In liquids particles go thorough ____________ meaning they move around

A

Translation

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

The corners of the cubes

A

Lattice points

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

This unit cell contains:
8 corners x 1/8 of an atom
= 1 atom/unit cell

A

Simple cubic

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

This unit cell contains:
8 corners x 1/8 of an atom + 1 central
=2 atoms/unit cell

A

Body centered cubic

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

This unit cell contains:
8 corners x 1/8 of an atom + 6 faces x 1/2 of an atom
=4 atoms/unit cell

A

Face centered cube

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

What are the properties of molecular solids?

A
  • consists of nonmetals, diatomic elements, or compounds composed of two or more nonmetals
  • normally do not conduct electricity
  • covalently bonded units are held together by weak intermolecular forces
  • soft
  • have low melting points
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Why do molecular solids normally not conduct electricity

A

Electrons are held within the covalent bonds of each molecule

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

What is an example of a molecular solid?

A

I2

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

___________ fats have stronger dispersion forces, and are solid at room temperature

A

Unsaturated

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

Why do unsaturated fats have weaker dispersion forces?

A

A double bond bends the carbon, causing the molecule to be sp2 hybridized, therefore being trigonal planar

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

What is an example of a molecular solid?

A

Wax

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

One or two nonmetals held together by networks of covalent bonds instead of intermolecular forces

A

Covalent network solids

17
Q

What are the properties of a covalent network solid?

A
  • very hard

- very high melting points

18
Q

Why are covalent network solids normally very hard?

A

-atoms are covalently bonded with fixed bond angles

19
Q

In graphite, each carbons forms three _____ hybrid orbitals that bond with three other carbon atoms

20
Q

Graphite and diamond are __________ of each other

A

Allotropes

21
Q

Why can sheets of graphite slide over each other so easily?

A

Weak pi bonds and london dispersion forces

22
Q

Why does graphite have a high melting point?

A

The covalent bonds between carbon in each later are relatively strong

23
Q

In diamond, many carbon atoms bond together with _______ hybrid orbitals

24
Q

What is the molecular geometry of diamond?

A

Tetrahedral

25
In diamonds each carbon makes a single covalent bond with ___ other carbon atoms
4
26
Other common covalent network solids include _________ and __________
SiO2 and Si
27
Si is a ______________
Semiconductor
28
Why is bonding in metallic solids not covalent?
Not enough electrons to fill octets
29
How does bonding in metallic solids work?
Attractions between nuclei and delocalized valence electrons move throughout the structure
30
Bond strength in metallic solids __________ as the number of bonding electrons increases
Increases
31
Why so metals bend, not break when hit with a hammer?
There are no directional bonds
32
Describe the electron sea model in metallic bonding
Nuclei and inner shells are stationary, while valence electrons are free to move throughout the solid
33
What are properties of metallic solids?
- conduct electricity - conduct heat - malleable and ductile - lack directional bonds
34
Why do saturated fats have stronger London dispersion forces?
It's linear shape is good for stacking, meaning there are many points of contact between molecules
35
Why are diamonds so hard?
- Diamonds are one massive molecule held together by covalent bonds - the sp3 hybridization allows for a tetrahedral structure which is very strong