MCHE 3310 Quiz 1

Atomic Mass Unit (amu)

Atomic Mass Unit (amu)

1/12 the mass of a carbon-12 atom

Bohr Model

1. Electrons revolve around the atomic nucleus in discrete orbitals

2. The position of any particular electron is defined by its orbital

3. The electron energies of electrons are quantized - electrons are permitted to have only specific values of energy

Wave-Particle Model

1. Electron exhibits both wave-like and particle-like characteristics

2. Position of an electron is described by a probability distribution or electron cloud

Quantum Numbers

Set of numbers used to completely describe an electron

Principle Quantum Number

1. Symbolized by "n"

2. Designates shell n = 1, 2, 3, 4, 5... Letter = K, L, M, N, O...

Second Quantum Number

1. Symbolized by "l"

2. Designates subshell

3. Electron orbital shapes depend upon this

4. Range from 0 to (n - 1) l = 0, 1, 2, 3... Subshell = s, p, d, f

Third (Magnetic) Quantum Number

1. Symbolized by "ml"

2. Determines number of electron orbitals for each subshell

3. It's an integer between -l and +l, including 0 1 s orbital 3 p orbitals 5 d orbitals 7 f orbitals

Fourth Quantum Number

1. Symbolized by "ms"

2. It's the spin moment and is oriented either up or down (2 electrons per electron orbital)

3. +1/2 for spin up, -1/2 for spin down

Pauli Exclusion Principle

No two electrons in the same atom can have the same set of four quantum numbers

Orbital Filling Sequence

Electrons tend to occupy the lowest available energy states.

Valence Electrons

1. Most available for bonding and tend to control chemical properties

2. Present in the outer-most shell

3. For example, When bonding with iron (Fe), even though the 4s subshell has less energy than the 3d subshell, the iron atom loses the 4s electrons first because they're on the outer-most shell

Electronegativity

1. Ranges from 0.9 to 4.1

2. Smaller values tend to give away electrons while larger values tend to acquire electrons

Primary Bonding Type: Ionic

1. Occurs between metallic and nonmetallic elements

2. Requires electron transfer

3. Large difference in electronegativity required

4. Make for poor conductors and have low chemical reactivity

5. ex. NaCl

Primary Bonding Type: Covalent

1. Similar Electronegativity (sharing electrons)

2. Bonds are determined by valence, where s & p orbitals dominate bonding

3. Directional bonding between nonmetallic elemental molecules

4. Make for poor conductors and have varying mechanical properties

5. ex. H2

Primary Bonding Type: Metallic

1. Mainly found in metals and their alloys

2. Valence electrons are not bound to any particular atom and are free to drift through the entire metal (electrons act as the glue that holds the ion cores together)

3. Non-directional bonding with bonding energy from 62 kJ/mol to 850 kJ/mol

Primary Bonding Combinations

Most materials possess a combination of different bonds, making generalization of bonding difficult

Secondary Bonding: Van der Waals

1. Arise from atomic or molecular dipoles

2. Two types of dipoles: induced and permanent

3. Bonding energy around 4-30 kJ/mol

4. Induced dipole ex. H2, Cl2, etc.

5. Permanents dipole ex. HCl, HF, etc.

Secondary Bonding: Hydrogen Bond

1. Attractive interaction between a hydrogen atom with an electronegative atom (intermolecular bond)

2. Stronger than Van der Waals interaction but far weaker than covalent or ionic bonds

3. ex. bond between lone pair of oxygen and hydrogen in H2O

Energy and Packing

Dense, ordered packed structures tend to have lower energies while non-dense, random structures tend to have higher energies

Crystalline Materials

1. atoms pack in periodic, 3D arrays

2. typical of : metals, many ceramics, some polymers

Noncrystalline Materials

1. atoms have no periodic packing

2. Occurs for complex structures and rapid cooling

FCC Packing

1. ABCABCABC...

2. The atoms in rows A & C aren't aligned

HCP Packing

1. ABABAB...

2. The atoms of the third plane are in exactly the same position as the atoms in the first plane

Hard Sphere Model

Atoms (or ions) are thought of as being solid spheres having well-defined diameters where spheres representing nearest-neighbor atom touch one another

Unit Cell

The smallest component of the crystal that reproduces the whole crystal when stacked together with purely translational repetition

Note: more than one unit cell can be chosen for a given crystal structure, but the one with highest symmetry is chosen

Lattice

1. Infinite, periodic array of mathematical points in which each point has identical surroundings to all others

2. Lattice points are purely mathematical whereas atoms are physical objects

3. Lattice points don't necessarily lie at the center of atoms

Crystal Structure

Periodic arrangement of atoms in the crystal that can be described by a lattice and a basis

Parameters of a Unit cell

(a, b, c) correspond to the length of the 3 adjacent edges of the unit cell

(α, β, γ) correspond to the 3 angles subtended by the lattice cell axes

Crystal Systems and Bravais Lattices

1. 7 possible combinations of (a, b, c) and (α, β, γ) resulting in 7 crystal systems

2. The 7 crystal systems can be described using 14 point lattices

Cubic

a = b = c α = β = γ = 90°

Tetragonal

a = b ≠ c α = β = γ = 90°

Orthorhombic

a ≠ b ≠ c α = β = γ = 90°

Hexagonal

a = b ≠ c α = β = 90° γ = 120°

Trigonal

a = b = c α = β = γ ≠ 90°

Monoclinic

a ≠ b ≠ c α = γ = 90° β ≠ 90°

Triclinic

a ≠ b ≠ c α ≠ β ≠ γ ≠ 90°

Simple Cubic (SC)

Atoms are situated only at the corners of the unit cell (1 atoms per unit cell)

Body Centered Cubic (BCC)

Atoms are situated at the corners in addition to a single atom at the center of the unit cell (2 atoms per unit cell)

Face Centered Cubic (FCC)

Atoms are situated at the corners and on the face of each unit cell (4 atoms per unit cell)

Coordination Number

The number of ions of opposite charge surrounding each ion in a crystal

Atomic Packing Factor (SC)

APF = Volume of atoms in unit cell / Volume of unit cell

APF (SC) = 0.52

Atomic Packing Factor (BCC)

APF = Volume of atoms in unit cell / Volume of unit cell

APF (BCC) = 0.68

Atomic Packing Factor (FCC)

APF = Volume of atoms in unit cell / Volume of unit cell

APF (FCC) = 0.74

Theoretical Density

Mass of Atoms in Unit Cell / Total Volume of Unit Cell

ρ = nA / VcNa n = number of atoms / unit cell A = atomic weight Vc = volume of unit cell Na = Avogadro's number

Point Coordinates of Unit Cell

1. Any point within a unit cell is specified as fractional multiples of the unit cell edge lengths

2. Position "P" specified as "q r s"; convention: coordinates aren't separated by commas or punctuation

Crystallographic Directions

Directional indices highlighting difference between vector head and tail

Algorithm:

1. Determine coordinates of vector tail and vector head

2. Tail point coordinates subtracted from head point coordinates

3. Normalize coordinate differences in terms of lattice parameters "a", "b", and "c"

4. Adjust to smallest integer values

5. Enclose in square brackets with no commas

Nuances:

1. Parallel lines have the same indices

2. No matter the length, one line has just one indices

Family of Directions

Angular bracket < > indicates a family of directions called a form (set of equivalent directions)

HCP Crystallographic Directions

Defined using Miller indices with a non-rectilinear coordinate system

Linear Density (LD)

Number of atoms / unit length of direction vector

Crystallographic Planes

Specified by 3 Miller indices (hkl)

Procedure:

1. If plane passes through origin, translate plane or choose new origin

2. Determine intercepts of planes on each of the axes in terms of unit cell edge lengths, known as lattice parameters (a plane that parallels an axis can be considered to have an infinite intercept)

3. Determine the reciprocal of the three intercepts (reciprocal of infinity is 0)

4. If necessary, multiply or divide to convert to smallest integers

5. The three indices are not separated by commas and are enclosed in parentheses (hkl)

6. If indices are negative, a bar is placed on top of index

Crystallographic Planes (HCP)

In hexagonal unit cells a similar Miller-Bravais approach is used

Family of Crystalline Planes

1. { } indicates family of planes

2. All planes in the same family are crystallographically equivalent

Planar Density (PD)

Number of atoms per 2D repeating unit / Area per 2D repeating unit

Single vs Polycrystals

X-Ray Diffraction

1. The scattering of X-rays by the regularly spaced atoms of a crystal, useful in obtaining information about the structure of the crystal

2. The magnitude of the distance between two adjacent, parallel planes of atoms is a function of the Miller indices as well as the lattice parameters

Crystalline Defect

A lattice irregularity having one or more of its dimensions on the order of an atomic diameter

Point Defects

2 types:

1. Vacancies: vacant atomic sites in a structure

2. Self-Interstitials: "extra" atoms positioned between atomic sites (less likely in metals as it's difficult to get a large metal atom into the small vacancy)

Equilibrium Concentration of Vacancies

Alloy

1. A metal comprised of two or more elements, at least one of which is metallic

2. More abundant element is referred to as the solvent and the less abundant element is the solute

3. Generally, metals do not like to mix, but when they do they form in one of two ways: substitution (element replaces host atom in orderly arrangement) and interstitial (smaller element goes into interstitial voids in an orderly arrangement)

4. The substitutional and interstitial atoms can be thought of as point defects

Hume-Rothery Rules for Alloys

For an alloy to be called substitutional solid, it needs to be:

1. Solute and solvent are soluble

2. Be able to form a homogeneous solution

3. Host structure maintains

4. No new structures (phases) are formed

Empirical Rules:

1. Atomic size factor (size difference between the elements should not be greater than 15%)

2. Crystal structure (the crystal structure for metals must be the same)

3. Electronegativity (must have similar electronegativity values)

4. Valences (a metal will have a greater tendency to dissolve a metal of higher valency than of lower valency; higher in lower alright, lower in higher is a fight)

Edge Dislocation

1. extra half plane of atoms inserted in a crystal structure

2. Burgers vector perpendicular to dislocation line

Screw Dislocations

Result of shear forces on part of the material that caused the displacement of a portion of the crystal

Mixed Dislocations

1. Combination of edge and screw dislocations

2. Relationship between burgers vector and dislocation line is neither perpendicular or a parallel

Planar Defects

Boundaries that have two dimensions and normally separate regions of the materials that have different crystal structure and/or crystallographic orientation

External Surfaces

Surface atoms are not bonded to the maximum number of nearest neighbors, making them have higher energy and high reactivity

Grain Boundaries

1. Regions between grains

2. Transition from lattice of one region to that of the other

3. Small-angle grain boundaries have larger energy than high-angle grain boundaries, but neither have higher energy than external surfaces

Twin Boundary (plane) and Stacking Faults

A reflection of atom positions across the twin plane and an error in the packing sequence

Diffusion

Mass transport by atomic motion

Diffusion is important for the treatment of materials to improve material properties and materials performance in service

The impurity atoms can be provided from an adjacent another solid phase, a liquid, or a gas.

Inter-diffusion

Atoms of one metal diffuse into another.

concentration gradient

Driving force for diffusion from regions of high concentration to regions of low concentration

self-diffusion

In pure metals, atoms also migrate; but all atoms exchanging positions are of the same type.

For an atom to diffuse, two conditions must be met:

•There must have an empty adjacent site

• The atom must have sufficient energy to break bonds with its neighbor atoms and then cause some lattice distortion during the displacement.

vacancy diffusion

atoms exchange with vacancies • applies to substitutional impurities atoms • rate depends on: --number of vacancies --activation energy to exchange

interstitial diffusion

•Smaller atoms, e.g., H, C, N and O, can diffuse into or between interstitial positions.

•Interstitial diffusion occurs much more rapidly than vacancy diffusion

•There are more empty interstitial position than vacancies in a solid.

•Interstitial diffusion is an important method to improve materials' mechanical properties, particularly the surface hardness and strength.

case hardening

Diffuse carbon atoms into the host iron atoms at the surface.

Processing using diffusion

Doping silicon with phosphorus for n-type or p-type semiconductors.

1. Deposit P rich layers on surface.

2. Heat it.

3. Result: Doped semiconductor regions

steady-state diffusion

Rate of diffusion is independent of time • Flux proportional to concentration gradient

Activation energy

the energy required to produce the diffusive motion of one mole of atoms