IMF of Solids (chapter 3)

Question 1

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

Answer 1

Crystal/ Crystalline solid

Question 2

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

Answer 2

Ion

Question 3

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

Answer 3

Ionic crystal

Question 4

Attraction between oppositely charged ions in a chemical compound.

Answer 4

Electrostatic bonding

Question 5

Electrostatic force that holds ions together in an ionic compound.

Answer 5

Ionic bond

Question 6

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.

Answer 6

Network solid/ Covalent network crystal

Question 7

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

Answer 7

Molecular crystal

Question 8

Regular repeating structure of a crystalline solid.

Answer 8

Crystal lattice

Question 9

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

Answer 9

Unit cell

Question 10

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

Answer 10

Long range order

Question 11

2 Catergories of Solids

Answer 11

1. Crystalline solids

2. Amorphous solids

Question 12

There is a presence of long range order.

Answer 12

Crystalline solids

Question 13

There is an absence of long range order.

Answer 13

Amorphous solids

Question 14

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

Answer 14

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

Question 15

Greek word meaning “shapeless”

Answer 15

“amorphos”

Question 16

fixed geometric patters of lattices

Answer 16

crystalline solids

Question 17

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

Answer 17

crystalline solids

Question 18

Examples of crystalline solids:

Answer 18

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

Question 19

More than __% of ______ and ______ are crystalline.

Answer 19

90%; naturally occuring and artificially prepared solids

Question 20

Random orientation of particles.

Answer 20

Amorphous solids

Question 21

Examples of amorphous solids:

Answer 21

glass, plastic, rubber, coal, cotton candy

Question 22

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

Answer 22

presence/ absence of long range order

Question 23

crystals become liquid at a ____ bc?

Answer 23

specific temperature bc attractive forces are broken

Question 24

Change sharply when attractive forces are broken?

Answer 24

Physical Properties

Question 25

When amorphous solids are heated,

Answer 25

they soften gradually and melt over wide range of temperature.

Question 26

Formation of solid crystals from a homogeneous solution.

Answer 26

Crystallization

Question 27

Essentially a solid-liquid separation technique and very important.

Answer 27

Crystallization

Question 28

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.

Answer 28

X-ray diffraction

Question 29

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

Answer 29

X-ray diffraction

Question 30

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

Answer 30

Scattered rays

Question 31

4 Types of Crystals

Answer 31

1. Metallic crystals 2. Ionic crystals 3. Molecular crystals 4. Covalent network crystals

Question 32

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

Answer 32

Metallic crystals

Question 33

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

Answer 33

Metallic crystals

Question 34

Metallic bonds also known as?

Answer 34

"sea of electrons"

Question 35

Characteristics of metallic crystals (6)

Answer 35

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

Question 36

Mobile e- simply follows the movement of cations.

Answer 36

Malleability and Ductility

Question 37

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

Answer 37

High melting points

Question 38

Delocalized e- move throughout the crystal

Answer 38

Electrical conductivity

Question 39

Form of emitted light.

Answer 39

Luster

Question 40

Atoms are packed closely together.

Answer 40

Dense

Question 41

Collisions that kinetic energy is transferred.

Answer 41

Thermal conductivity

Question 42

cation and anion

Answer 42

Ionic crystals

Question 43

Form strong electrostatic interactions that hold the crystal lattice together.

Answer 43

Ionic crystals

Question 44

ions of opposite charge

Answer 44

Ionic crystals

Question 45

shatter into pieces when deformed

Answer 45

brittle

Question 46

cause repulsion

Answer 46

shifting of ions

Question 47

conduct electricity

Answer 47

liquid ionic substance

Question 48

nonconducting

Answer 48

solid ionic substance

Question 49

holds the crystal together

Answer 49

hard

Question 50

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

Answer 50

Molecular crystals

Question 51

Atoms/ molecules are held by IMF

Answer 51

Molecular crystals

Question 52

Low melting points = ?

Answer 52

forces are broken

Question 53

Valence e- is used in?

Answer 53

Bonding

Question 54

no charged particles bc of the absence of any mobile paricles

Answer 54

nonconducting

Question 55

Why are molecular crystals brittle?

Answer 55

bc they are highly directional and shifting would break them

Question 56

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

Answer 56

Covalent network crystals

Question 57

Used to form covalent bonds

Answer 57

valence electrons

Question 58

no delocalized e-

Answer 58

nonconducting

Question 59

Only type of attractive force in network solid.

Answer 59

Covalent network crystal

Question 60

Requires a large amount of energy

Answer 60

Rearranging/ breaking of covalent bond

Question 61

Insoluble in water

Answer 61

Covalent network crystal

Question 62

Very structurally complex and has at least 70 crystalline forms

Answer 62

Silicon carbide (SiC)

Question 63

Hardest and high melting point

Answer 63

diamond

Question 64

2nd hardest

Answer 64

Cubic boron nitride (BN)

Question 65

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

Answer 65

Silicon dioxide (SiO2)

Question 66

an allotrope of carbon

Answer 66

Graphite

Question 67

Differs in properties with others

Answer 67

Graphite

Question 68

Soft

Answer 68

Graphite

Question 69

Used as solid lubricant

Answer 69

Graphite

Question 70

This indicates the presence of charged particles in graphite.

Answer 70

Good conductor of electricity

Question 71

Why is graphite weaker than diamond?

Answer 71

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