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AP Chemistry > The Solid State > Flashcards

The Solid State Flashcards

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1
Q

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

A

Slower

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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
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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
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4
Q

Segments in crystalline solids that repeat in three dimensions

A

Unit cells

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5
Q

In liquids particles go thorough ____________ meaning they move around

A

Translation

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6
Q

The corners of the cubes

A

Lattice points

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7
Q

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

A

Simple cubic

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8
Q

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

A

Body centered cubic

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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

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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
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11
Q

Why do molecular solids normally not conduct electricity

A

Electrons are held within the covalent bonds of each molecule

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12
Q

What is an example of a molecular solid?

A

I2

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13
Q

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

A

Unsaturated

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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

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15
Q

What is an example of a molecular solid?

A

Wax

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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

A

Sp2

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

A

Sp3

24
Q

What is the molecular geometry of diamond?

A

Tetrahedral

25
Q

In diamonds each carbon makes a single covalent bond with ___ other carbon atoms

A

4

26
Q

Other common covalent network solids include _________ and __________

A

SiO2 and Si

27
Q

Si is a ______________

A

Semiconductor

28
Q

Why is bonding in metallic solids not covalent?

A

Not enough electrons to fill octets

29
Q

How does bonding in metallic solids work?

A

Attractions between nuclei and delocalized valence electrons move throughout the structure

30
Q

Bond strength in metallic solids __________ as the number of bonding electrons increases

A

Increases

31
Q

Why so metals bend, not break when hit with a hammer?

A

There are no directional bonds

32
Q

Describe the electron sea model in metallic bonding

A

Nuclei and inner shells are stationary, while valence electrons are free to move throughout the solid

33
Q

What are properties of metallic solids?

A
  • conduct electricity
  • conduct heat
  • malleable and ductile
  • lack directional bonds
34
Q

Why do saturated fats have stronger London dispersion forces?

A

It’s linear shape is good for stacking, meaning there are many points of contact between molecules

35
Q

Why are diamonds so hard?

A
  • Diamonds are one massive molecule held together by covalent bonds
  • the sp3 hybridization allows for a tetrahedral structure which is very strong

AP Chemistry (18 decks)

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