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CHEMISTRY 2 > IMF of Solids (chapter 3) > Flashcards

IMF of Solids (chapter 3) Flashcards

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1
Q

Solid material whose components, such as atoms, molecules or ions, are arranged in a highly ordered microscopic structure.

A

Crystal/ Crystalline solid

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2
Q

Atom/ group of atoms that has a net positive or negative charge.

A

Ion

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3
Q

Solid that consists of positively and negatively charged ions held together by electrostatic forces.

A

Ionic crystal

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4
Q

Attraction between oppositely charged ions in a chemical compound.

A

Electrostatic bonding

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5
Q

Electrostatic force that holds ions together in an ionic compound.

A

Ionic bond

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6
Q

Solid that may be a chemical compound (or element) in which atoms are bonded by covalent bonds in a continuous network extending throughout the material.

A

Network solid/ Covalent network crystal

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7
Q

Solid composed of molecules held together by Van deer Waals forces.

A

Molecular crystal

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8
Q

Regular repeating structure of a crystalline solid.

A

Crystal lattice

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9
Q

Smallest subunit of a crystal lattice that can be repeated over and over to make the entire crystal.

A

Unit cell

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10
Q

Repetition of structural units of the substance over long atomic distances.

A

Long range order

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11
Q

2 Catergories of Solids

A
  1. Crystalline solids

2. Amorphous solids

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12
Q

There is a presence of long range order.

A

Crystalline solids

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13
Q

There is an absence of long range order.

A

Amorphous solids

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14
Q

2 general ways a component of a solid can be arranged:

A
  1. Regular repeating three dimensional structure called “crystal lattice” (crystalline solid).
  2. Can aggregate with no particular long range order (amorphous solid).
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15
Q

Greek word meaning “shapeless”

A

“amorphos”

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16
Q

fixed geometric patters of lattices

A

crystalline solids

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17
Q

The ordered arrangement of their units maximizes the space they occupy and are essentially incompressible.

A

crystalline solids

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18
Q

Examples of crystalline solids:

A

ice, NaCl, CuSO4, diamond, graphite, sugar (C12H22O11),minerals, sand, clay, limestone, metals, alloys, carbon.

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19
Q

More than __% of ______ and ______ are crystalline.

A

90%; naturally occuring and artificially prepared solids

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20
Q

Random orientation of particles.

A

Amorphous solids

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21
Q

Examples of amorphous solids:

A

glass, plastic, rubber, coal, cotton candy

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22
Q

cause of the difference in the behavior of crystalline solids when heated

A

presence/ absence of long range order

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23
Q

crystals become liquid at a ____ bc?

A

specific temperature bc attractive forces are broken

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24
Q

Change sharply when attractive forces are broken?

A

Physical Properties

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25
Q

When amorphous solids are heated,

A

they soften gradually and melt over wide range of temperature.

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26
Q

Formation of solid crystals from a homogeneous solution.

A

Crystallization

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27
Q

Essentially a solid-liquid separation technique and very important.

A

Crystallization

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28
Q

Technique used to determine the atomic and molecular structure of a crystal wherein atoms cause beams of incident x-rays to diffract into many specific directions.

A

X-ray diffraction

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29
Q

A stream of x-rays directed at a crystal, diffracts and scatters as it encounter atoms

A

X-ray diffraction

30
Q

Interfere with each other and produce a pattern of spots of different intensities that can be recorded on film.

A

Scattered rays

31
Q

4 Types of Crystals

A
  1. Metallic crystals
  2. Ionic crystals
  3. Molecular crystals
  4. Covalent network crystals
32
Q

Can readily lose e- to form cations, but no atoms in the crystal would really gain e-.

A

Metallic crystals

33
Q

Made up of an orderly arrangement of cations surrounded by delocalized e- that move around the crystal.

A

Metallic crystals

34
Q

Metallic bonds also known as?

A

“sea of electrons”

35
Q

Characteristics of metallic crystals (6)

A

high melting points, malleability, thermal and electrical conductivity, ductility, luster, dense

36
Q

Mobile e- simply follows the movement of cations.

A

Malleability and Ductility

37
Q

Large amount of energy in needed for the forces of attraction.

A

High melting points

38
Q

Delocalized e- move throughout the crystal

A

Electrical conductivity

39
Q

Form of emitted light.

A

Luster

40
Q

Atoms are packed closely together.

A

Dense

41
Q

Collisions that kinetic energy is transferred.

A

Thermal conductivity

42
Q

cation and anion

A

Ionic crystals

43
Q

Form strong electrostatic interactions that hold the crystal lattice together.

A

Ionic crystals

44
Q

ions of opposite charge

A

Ionic crystals

45
Q

shatter into pieces when deformed

A

brittle

46
Q

cause repulsion

A

shifting of ions

47
Q

conduct electricity

A

liquid ionic substance

48
Q

nonconducting

A

solid ionic substance

49
Q

holds the crystal together

A

hard

50
Q

Made of atoms, such as noble gases or molecules such as sugar (C12H22O11), Iodine (I2), and napthalene (C10H8).

A

Molecular crystals

51
Q

Atoms/ molecules are held by IMF

A

Molecular crystals

52
Q

Low melting points = ?

A

forces are broken

53
Q

Valence e- is used in?

A

Bonding

54
Q

no charged particles bc of the absence of any mobile paricles

A

nonconducting

55
Q

Why are molecular crystals brittle?

A

bc they are highly directional and shifting would break them

56
Q

Made of atoms in which each atom is covalently bonded to its nearest neighbors

A

Covalent network crystals

57
Q

Used to form covalent bonds

A

valence electrons

58
Q

no delocalized e-

A

nonconducting

59
Q

Only type of attractive force in network solid.

A

Covalent network crystal

60
Q

Requires a large amount of energy

A

Rearranging/ breaking of covalent bond

61
Q

Insoluble in water

A

Covalent network crystal

62
Q

Very structurally complex and has at least 70 crystalline forms

A

Silicon carbide (SiC)

63
Q

Hardest and high melting point

A

diamond

64
Q

2nd hardest

A

Cubic boron nitride (BN)

65
Q

Each silicon atom is bridged to its neighbors by an oxygen atom.

A

Silicon dioxide (SiO2)

66
Q

an allotrope of carbon

A

Graphite

67
Q

Differs in properties with others

A

Graphite

68
Q

Soft

A

Graphite

69
Q

Used as solid lubricant

A

Graphite

70
Q

This indicates the presence of charged particles in graphite.

A

Good conductor of electricity

71
Q

Why is graphite weaker than diamond?

A

bc graphite is only bonded to three and made of layers of rings of Carbon atoms while diamond is bonded to four.

CHEMISTRY 2 (3 decks)

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