electronics fundamentals chapter 1: atomic structure and … fu… · a characteristic that hinted...
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Electronics Fundamentals
Chapter 1: Atomic Structure and Semiconductor Materials
Part 1- Atomic Structure
Evidence that scientists had in 1900 to indicate that the atom was not a fundamental unit:
1) There seemed to be too many kinds of atoms, each belonging to a distinct chemical element.
2) Atoms and electromagnetic phenomena were intimately related.
3) The problem of valence. Certain elements combine with some elements but not with others,
a characteristic that hinted at an internal atomic structure.
4) The discoveries of radioactivity, of x rays, and of the electron.
Thomson Model of the Atom:
J. J. Thomson - English physicist. 1897 Made a piece of equipment called a cathode ray tube.
It is a vacuum tube - all the air has been pumped out. Form when high voltage is applied across
electrodes in a partially evacuated tube. Rays originate at the cathode (negative electrode) and
move to the anode (positive electrode). Carry energy and can do work. Travel in straight lines in
the absence of an external field. Using a cathode ray tube, Thomson was able to deflect cathode
rays with an electrical field. The rays bent towards the positive pole, indicating that they are
negatively charged. Thomson used magnetic and electric fields to measure and calculate the ratio
of the cathode ray’s mass to its charge.
Figure 1: Schematic of J.J. Thomson's experiment.
As shown in the figure, the particle that comes off the filament is accelerated by the high voltage
V) and passed between two parallel plates across which an Electric field E exist. This field exerts
a force (FE) on the particle of charge (Q)and deflect it from its path according:
FE= Q*E in Newton’s.
Another force (FB) is exerted on the particle by a magnetic field (B) [FB = Q*B*v], where v is
the particle velocity. Thomson adjusted the directions of the electric and magnetic fields in such
a way that the two forces are opposite and equal. Under these conditions , emitted particle are no
longer deflected. Therefore: FE = FB thus: Q*E = Q*B*v, v= E/B.
The kinetic energy (Ek) received by the particle accelerated by V volt is: Ek = Q*V = 0.5*m*v2,
thus v = (2*Q*V/m)1/2
= E/B and Q/m = E2/ 2*V*B
2
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Knowing the electric field €, the magnetic field intensity (B) and the accelerating voltage (V),
the charge to mass ratio (Q/m) of the electron can be calculated.
He compared the value with the mass/ charge ratio for the lightest charged particle. By
comparison, Thomson estimated that the cathode ray particle weighed 1/1000 as much as
hydrogen, the lightest atom. He concluded that atoms do contain subatomic particles - atoms are
divisible into smaller particles. Since any electrode material produces an identical ray, cathode
ray particles are present in all types of matter - a universal negatively charged subatomic particle
later named the electron
J.J. Thomson discovered the electron and
knew that electrons could be emitted from
matter (1897). William Thomson proposed
that atoms consist of small, negative
electrons embedded in a massive, positive
sphere. The electrons were like currants in a
plum pudding. This is called the ‘plum
pudding’ model of the atom.
Ernest Rutherford (1871-1937) nuclear
physicist, Thomson’s student, New
Zealander teaching in Great Britain :Gold
Leaf Experiment Rutherford’s Experiments
(1910-11) Fired beam of positively-charged
alpha particles at very thin gold foil. Alpha
particles caused flashes of light when they
hit the zinc sulfide screen.
By Thomson’s model, mass and + charge of gold atom are too dispersed to deflect the
positively-charged alpha particles, so particles should shoot straight through the gold atoms.
Most alpha particles went straight through, and some were deflected, BUT a few (1 in 20,000)
reflected straight back to the source.
Expt. Interpretation: gold atom has small,
dense, positively-charged nucleus
surrounded by “mostly empty” space in
which the electrons must exist. Positively
charged particles called “protons” like tiny
solar system.
James Chadwick (1932) Discovered a
neutral (uncharged) particle in the nucleus.
Called it the “neutron”
The order of the elements is determined by their atomic number (= the number of protons). The
atomic mass of the elements is determined by the number of protons and neutrons. A given
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element can have different number of neutrons, and therefore different atomic masses. The
chemical properties of the elements are determined by the number of electrons in their outer
(valence) shells.
Property
Particle Mass in amu (g) Relative Charge(C)
Electron 0.00055 ( 9.110 x 10
-28
)
- 1(1.6*10-19
)
Proton 1.00728 (1.673 x 10
-24
+ 1(1.6*10-19
)
Neutron 1.00866 ( 1.675 x 10
-24
0
The Classical Atomic Model
Let’s consider atoms as a planetary model. The
force of attraction on the electron by the nucleus
and Newton’s 2nd law give
where v is the
tangential velocity of the electron.
atoms planetary mode
The potential energy is: The kinetic energy is:
𝑬𝒑 = ∫ 𝑬𝒆 ∞
𝒓dr=∫
𝒆𝟐
𝟒𝝅ɛ𝒐𝒓𝟐= −
∞
𝟎
𝒆𝟐
𝟒𝝅ɛ𝒐 𝒓
The total energy is
The total energy of electron is negative, so the
system is bound, which is good. Otherwise the
electron will leave the material if it possess
positive energy. From classical E&M theory, an
accelerated electric charge radiates energy
(electromagnetic radiation) which means total
energy must decrease. Radius r must decrease.
Electrons moving through the electrical field
generated by the protons in the nucleus would
radiate away energy and spiral down into the
nucleus. Calculations soon showed that a
“Rutherford atom” would last less than one
minute.
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The Photoelectric Effect:
A photoelectric effect is any effect in which
light energy is converted to electricity. First
explained by Albert Einstein in 1905. It
had long been know that when chemical
elements are heated, they gave off light of a
particular wavelength (or color) Sodium Potassium Lithium
Max Planck found experimental results that suggested light behaved more like a particle when he
was studying black body radiation. A black body is a theoretical object that absorbs all light that
falls on it. It reflects no radiation and appears perfectly black. Black body radiation is the
energy that would be emitted from an ideal black body.
In the year 1900, Planck published a paper on the electromagnetic radiation emitted from a
black object that had been heated. In trying to explain the black body radiation, Planck, in the
same year determined that the experimental results could not be explained with the wave form of
light. Instead, Planck described the radiation emission as discrete bundles of energy, which he
called quanta. A quantum (singular form of quanta) is a small unit into which certain forms of
energy are divided. These “discrete bundles of energy” once again raised the question of whether
light was a wav or a particle. Planck’s work also pointed out that the energy of a quantum of
light was related only to its frequency. Planck’s equation for calculating the energy of a bundle
of light is E= hν, where E is the energy of the photon in joules (J), ν is the frequency in hertz
(s), and h is Planck’s constant, 6:63*10-34
J. s or 4.14*10-15
eV.s.. The word quantum is used for
energy in any form; when the type of energy under discussion is light, the words quantum and
photon become interchangeable.)
In 1905, Einstein proposed that
electromagnetic radiation or light is made up
of photons. Thus the photon is the
elementary element of light or light is made
up of photons. Einstein show that- light
energy is not emitted continuously but it is
emitted by individual amount of energy
called as quantum of energy. Each photon of
a light wave of frequency ν has the energy
E is given by: E= hν
Properties of photon
1. A photon does not have any mass.
2. A photon does not have any charge and are not deflected in electric field or magnetic field.
3. All the quantum numbers are zero for a photon.
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4. In empty space, the photon moves at speed of light.
5. In the interaction of radiation with matter, radiation behaves as if it is made up of particles
called photons.
6. The energy and momentum of a photon are related as follows: E= p*c
where p- magnitude of momentum and c is the speed of light.
7. Photon is called as a virtual particles.
8. The energy of a photon is directly proportional to frequency and inversely proportional to its
wavelength.
Characteristic of photoelectric effect
Photoelectric effect- When light of suitable frequency is incident on metal surface then
electrons are emitted from surface called as Photoelectric effect.
1. Threshold frequency is different for different material.
2. Photoelectric current is directly proportional to intensity of light.
3. The K.E. of photoelectrons is directly proportional to frequency of light.
4. Stopping potential is directly proportional to frequency.
5. The process is instantaneous.
Einstein’s photoelectric function- According to quantum theory, radiation is considered as
shower of particles called photons. Energy of photon absorbed by the atom (hυ) is:
1. Used to detach the electron (W0) and
2. Kinetic energy (Ek) is given to electron.
hυ= W0 + Ek = W0 + 0.5mv2
Where, υ= Frequency of radiation,
W0= Photoelectric work function= hυ0,
m= Mass of electron v= Velocity of electron,
h= Planck’s constant and υ0= Threshold
frequency
0.5mv2 = hυ- W0 = hυ - hυ0 = h (υ- υ0)
Significance
1. If υ < υ0 - Kinetic energy is negative. i.e. No
emission.
2. If υ = υ0 - Kinetic energy is zero. i.e.
Emission just begins.
3. If υ > υ0 - Kinetic energy is positive. i.e.
Emission takes place.
Niels Bohr (1885-1962) Danish physicist: Bohr wondered why hydrogen emitted spectral lines,
and not just a continuous band of light.
The Bohr Model of the Hydrogen Atom (1913): Bohr’s general assumptions:
1. Stationary states, in which orbiting electrons do not radiate energy, exist in atoms and have
well-defined energies, En.
2. Transitions of electrons can occur between the stationary states, yielding light of energy:
E = En1
– En2
= h υ
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The electron will gain energy when it is moved from lower to higher state and loose energy vice
versa. Classical laws of physics do not apply to transitions between stationary states, but they do
apply elsewhere.
3. The angular momentum of the nth
state is: L = nh/2π. (Angular momentum is quantized!).
where n is called the Principal Quantum Number and h is plank constant. The angular
momentum is:
a0 is called the Bohr radius. It’s the radius of the Hydrogen atom (in its lowest-energy, or
“ground,” state). Where the Bohr radius is given by
The smallest diameter of the hydrogen atom is;
n = 1 gives its lowest energy state (called the
“ground” state)
The Hydrogen Atom
The energies of the stationary states where E0
= -13.6 eV.
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The amounts of total energy of the electron is very small. Therefore, instead of Joule we will use
the unit of electron volt (eV), which is the energy a body with a charge of one elementary
charge (e = 1.602 x 10-19
C) gains or losses when it is moved across electric potential difference
of 1 Volt (V).
E (in electron volt) = Q x V,
where Q is the electronic charge (1.602 x 10-19 C) and V is the voltage:
1 electron volt is equal to 1.602 x 10-19
Joule
Example1: Consider Q = -1.6x10-19
Coulomb, me = 9.18x10-31
Kg, εo=8.84x10-12
F/m, h=
6.63x10-34
J. sec or 4.12x10-15
eV.sec and 1 eV = 1.6x10-19
Joules. Calculate the radius and
velocity of the hydrogen electron moved to the second orbit (n=2).
Solution: r = ao*n2 = 0.53*10
-10* 2
2 = 2.12*10
-10 meters
v = [Q/(4π*εo*m*r)1/2
] = [ 1.6*10-19
/(4π*8.84x10-12
*9.18x10-31
*2.12*10-10
)]
v = 1.04*106 m/s
Example: Calculate the radius and velocity of the hydrogen electron having total energy:
(a) -13.6 eV, (b) -10 eV.
Solution:
(a) ra = (1.6*10-19
)2/ (8π*8.84x10-12
*13.6) = 5.3*10-11
m
va = [e/(4π*εo*m*r)1/2
]
= [ 1.6*10-19
/(4π*8.84x10-12
*9.18x10-31
*5.3*10-11
)] 6.9*106 m/s
(b) rb = (1.6*10-19
)2/ (8π*8.84x10-12
*10.4) = 7.19*10-11
m
vb = [e/(4π*εo*m*r)1/2
]
= [ 1.6*10-19
/(4π*8.84x10-12
*9.18x10-31
*7.19*10-11
)] = 5.93*106 m/s
Note: As the radii increase (the electron further away from the nucleus), the velocity of electron
decreases since the centrifugal force required to maintain the stable electron orbit is less.
Emission of light occurs when the atom is in an excited state and decays to a lower energy state
(nu → nℓ).
where υ is the frequency of a photon.
R∞ is the Rydberg constant.
The atom will remain in the excited state for a short time before emitting a photon and returning
to a lower stationary state. All hydrogen atoms exist in n = 1 (invisible). Bohr improved
uh E E
1 h
c hc
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Rutherford’s model by noticing that energy levels in atoms went up and down by specific, “pre-
set” amounts. He suggested that electrons move around the nucleus of an atom like planets
around the sun, and that they move from orbit to orbit as they gain and lose energy.
Louis de Broglie (1927) Particle/Wave Duality of electrons: for matter, just as much as for
radiation, in particular light, we must introduce at one and the same time the corpuscle concept and the
wave concept. In other words, in both cases we must assume the existence of corpuscles accompanied by
waves. All matters big or small behave like a wave. Electrons behave with wave and particle
properties at the same time.
λ= h/m*v, where h is Plank constant, m is the mass of the matter and v its velocity, but the
wavelength for photon is: λ =h/c, where c is the speed of light. Example: Calculate De Broglie wave length (λ) of: (a) A dust particle of mass 1x10
-5Kg
travelling at speed of 0.02m/sec. (b)An electron of mass 9.1x 10-31
Kg moving at 5x105 m/sec.
Compare the results in a and b. Suppose Plank constant h= 6.62x10-34
J.sec.
The Bohr model was a great step of the new quantum theory,
but it had its limitations.
1) Works only to single-electron atoms.
2) Could not account for the intensities or the fine structure of the spectral lines.
3) Could not explain the binding of atoms into molecules.
Quantum theory ; Planck’s work became the basis for quantum theory. Quantum theory is the
theory that energy can only exist in discrete amounts (quanta). The problem involved in
demonstrating this theory is that the scale of a quantum of energy is much smaller than the
objects we normally deal with. The results of the photoelectric effect indicated that if the
experimenter used low frequency light, such as red, no electrons were knocked off the metal. No
matter how many light waves were used and no matter how long the light was shined on the
metal, red light could not knock off any electrons. If a higher frequency light was used, such as
blue light, then many electrons were knocked off the metal. Albert Einstein used Planck’s
quantum theory to provide the explanation for the photoelectric effect. A certain amount of
energy was necessary for electrons to be knocked off a metal surface. If light were quantized,
then only particles of higher frequency light (and therefore higher energy) would have enough
energy to remove an electron. Light particles of lower frequency (and therefore lower energy)
could never remove any electrons, regardless of how many of them were used.
In all previous attempts to describe the electron’s behavior inside an atom, including in the Bohr
model, scientists tried to describe the path the electron would follow around the nucleus. The
theorists wanted to describe where the electron was located and how it would move from that
position to its next position.
In 1927, a German physicist named Werner Heisenberg, a German physicist stated what is now
known as the Heisenberg uncertainty principle. This principle states that it is impossible to
know both the precise location and the precise velocity of an electron at the same time. The
reason that we can’t determine both is because the act of determining the location changes the
velocity. In the process of making a measurement, we have actually changed the measurement.
The Heisenberg uncertainty principle treated the electron as a particle. In effect, the uncertainty
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principle stated that the exact motion of an electron in an atom could never be determined, which
also meant that the exact structure of the atom could not be determined. Consequently, Erwin
Schrodinger, an Austrian physicist, decided to treat the electron as a wave in accordance with de
Broglie’s matter waves. Schrodinger, in considering the electron as a wave, developed an
equation to describe the electron wave behavior in three dimensions. Unfortunately, the equation
is so complex that it is actually impossible to solve exactly for atoms and ions that contain more
than one electron.
Only at certain distances from the nucleus
would the electron complete an integer
number of wavelengths in its movement
around the nucleus.
Figure above is an example of a standing
wave. There are only certain energies
(frequencies) for which the wavelength of
the wave will fit exactly to form a standing
wave. These energies turn out to be the same
as the energy levels predicted by the Bohr
model, but now there is a reason why
electrons may only occupy these energy
levels. The equations of quantum mechanics
tell us about the existence of four quantum
numbers: principal energy levels, the
number of energy levels in any atom, and
more detailed information about the various
energy levels.
Solutions to Schrödinger’s equation involve four special numbers called quantum numbers.
These four numbers completely describe the energy of an electron. Each electron has exactly
four quantum numbers, and no two electrons have the same four numbers. The statement that no
two electrons can have the same four quantum numbers is known as the Pauli exclusion
principle.
Quantum numbers:
1. The principal quantum number (n) is a positive integer (1, 2, 3, . . . n) that indicates the
main energy level of an electron within an atom. According to quantum mechanics, every
principal energy level has one or more sub-levels within it. In any energy level, the maximum
number of electrons possible is Nmax = 2n2. Therefore, the maximum number of electrons that
can occupy the first energy level is 2 (2 * 12). For energy level 2, the maximum number of
electrons is 8 (2*22), and for the 3rd energy level, the maximum number of electrons is 18(2 *
32). The number of sub-levels in a given energy level is equal to the number assigned to that
energy level. That is, principal energy level 1 will have 1 sub-level, principal energy level 2 will
have two sub-levels, principal energy level 3 will have three sub-levels, and so on.
Table 1.1 lists the number of sub-levels and electrons for the first four principal quantum
numbers
Principal
Quantum
Number of
Sub-
Total
Number
Number Levels of Electrons
1 1 2
10
2 2 8
3 3 18
4 4 32
TABLE 1. : Number of Sub-levels and
Electrons by Principal Quantum Number.
Each energy level can have as many sub-
levels as the principal quantum number, as
discussed above, and each sub-level is
identified by a letter. Beginning with the
lowest energy sub-level, the sub-levels are
identified by the letters s, p, d, f, g, h, i, and
so on. The principal energy levels and sub-
levels are shown in the following diagram.
The principal energy levels and sub-levels
that we use to describe electrons are in red.
2. Orbitals: (L)
Quantum mechanics also tells us how many orbitals are in each sub-level, an orbital is defined as
an area in the electron cloud where the probability of finding the electron is high. The number
of orbitals in an energy level is equal to the square of the principal quantum number. Hence,
energy level 1 will have 1 orbital (12), energy level 2 will have 4 orbitals (2
2), energy level 3 will
have 9 orbitals (32), and energy level 4 will have 16 orbitals (4
2). The s sub-level has only one
orbital. Each of the p sub-levels has three orbitals. The d sub-levels have five orbitals, and the f sub-
levels have seven orbitals. If we wished to assign the number of orbitals to the unused sub-levels, g
would have nine orbitals and h would have eleven.
You might note that the number of orbitals in the sub-levels increases by odd numbers (1, 3, 5, 7, 9,
11, . . .). As a result, the single orbital in energy level 1 is the s orbital. The four orbitals in energy
level 2 are a single 2s orbital and three 2p orbitals. The nine orbitals in energy level 3 are a single 3s
orbital, three 3p orbitals, and five 3d orbitals. The sixteen orbitals in energy level 4 are a the single
4s orbital, three 4p orbitals, five 4d orbitals, and seven 4f orbitals. The maximum number of
electrons in each orbital is 2.
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Energy bands Theory
Energy bands consisting of a large number of closely spaced energy levels exist in crystalline
materials. The bands can be thought of as the collection of the individual energy levels of electrons
surrounding each atom. The wave functions of the individual electrons, however, overlap with those
of electrons confined to neighboring atoms. The Pauli exclusion principle does not allow the electron
energy levels to be the same so that one obtains a set of closely spaced energy levels, forming an
energy band. The energy band model is crucial to any detailed treatment of semiconductor devices. It
provides the framework needed to understand the concept of an energy bandgap and that of
conduction in an almost filled band as described by the empty states.
The energy levels are grouped in bands, separated by energy band gaps. The behavior of electrons
at the bottom of such a band is similar to that of a free electron. However, the electrons are
affected by the presence of the periodic potential. The combined effect of the periodic potential is
included by adjusting the value of the electron mass. This mass will be referred to as the effective
mass. The effect of a periodic arrangement on the electron energy levels is illustrated by
Figure shown are the energy levels of electrons in a carbon crystal with the atoms arranged in a
diamond lattice. These energy levels are plotted as a function of the lattice constant, a.
Isolated carbon atoms contain six electrons, which occupy the 1s, 2s and 2p orbital in pairs. The
energy of an electron occupying the 2s and 2p orbital is indicated on the figure. The energy of the 1s
orbital is not shown. As the lattice constant is reduced, there is an overlap of the electron wave
functions occupying adjacent atoms. This leads to a splitting of the energy levels consistent with the
Pauli exclusion principle. The splitting results in an energy band containing 2N states in the 2s band
and 6N states in the 2p band, where N is the number of atoms in the crystal. A further reduction of
the lattice constant causes the 2s and 2p energy bands to merge and split again into two bands
containing 4N states each. At zero Kelvin, the lower band is completely filled with electrons and
labeled as the valence band. The upper band is empty and labeled as the conduction band.
The energy band diagrams shown in the previous section are frequently simplified when analyzing
semiconductor devices. Since the electronic properties of a semiconductor are dominated by the
highest partially empty band and the lowest partially filled band, it is often sufficient to only
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consider those bands. This leads to a simplified energy band diagram for semiconductors as shown
in Figure below
A simplified energy band diagram used to describe semiconductors. Shown are the valence and
conduction band as indicated by the valence band edge, Ev, and the conduction band edge, Ec. The
vacuum level, Evacuum, and the electron affinity, c, are also indicated on the figure.
The diagram identifies the almost-empty conduction band by a set of horizontal lines. The bottom
line indicates the bottom edge of the conduction band and is labeled Ec. Similarly, the top of the
valence band is indicated by a horizontal line labeled Ev. The energy band gap, Eg, is located
between the two bands. The distance between the conduction band edge, Ec, and the energy of a
free electron outside the crystal (called the vacuum level labeled Evacuum) is quantified by the
electron affinity, χ multiplied with the electronic charge q. Evacuum = χ* q
Part 2- Semiconductors
Solid-state electronic materials
Electronic materials generally can be divided into three categories: insulators, conductors, and
semiconductors. The primary parameter used to distinguish among these materials is the resistivity
ρ, with units of Ω· cm. As indicated in Table 1.1, insulators have resistivity greater than 105
Ω·cm,
whereas conductors have resistivity below 10−3
Ω · cm. For example, diamond, one of the highest
quality insulators, has a very large resistivity, 1016
Ω·cm. On the other hand, pure copper, a good
conductor, has a resistivity of only 3 × 10−6
Ω·cm. Semiconductors occupy the full range of
resistivity between the insulator and conductor boundaries; moreover, the resistivity can be
controlled by adding various impurity atoms to the semiconductor crystal.
Elemental semiconductors are formed from
a single type of atom (column IV of the
periodic table of elements; see Table 1.2),
whereas compound semiconductors can be
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formed from combinations of elements from
columns III and V or columns II and VI.
These later materials are often referred to as
III–V (3–5) or II–VI (2–6) compound
semiconductors.
Covalent bond model
Atoms can bond together in amorphous, polycrystalline, or single-crystal forms. Amorphous
materials have a disordered structure, whereas polycrystalline material consists of a large number of
small crystallites.
Most of the useful properties of semiconductors,
however, occur in high-purity, single-crystal
material. Silicon—column IV in the periodic
table—has four electrons in the outershell.
Single-crystal material is formed by the
covalent bonding of each silicon atom with its
four nearest neighbors in a highly regular three-
dimensional array of atoms, as shown in Fig.
1.8.
Figure 1.8: Silicon crystal lattice structure.
Diamond lattice unit cell.
Much of the behavior we discuss can be visualized using the simplified two-dimensional covalent
bond model of Fig. 1.9. a. At temperatures approaching absolute zero, all the electrons reside in the
covalent bonds shared between the atoms in the array, with no electrons free for conduction. The
outer shells of the silicon atoms are full, and the material behaves as an insulator. As the
temperature increases, thermal energy is added to the crystal and some bonds break, freeing a small
number of electrons for conduction, as in Fig. 1.9 b. The density of these free electrons is equal to
the intrinsic carrier density ni (cm−3
), which is determined by material properties and temperature:
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(a) (b)
Figure 1.9 (a) Two-dimensional silicon lattice with shared covalent bonds. At temperatures
approaching absolute zero, 0 K, all bonds are filled, and the outer shells of the silicon atoms are
completely full. (b) An electron–hole pair is generated whenever a covalent bond is broken.
where EG = semiconductor bandgap energy in eV
(electron volts), k =Boltzmann’s constant (8.62* 10-5
eV/K), T =absolute temperature, oK, B =
material parameter, 1.08 × 1031
K−3
cm−6
for Si.
Bandgap energy EG is the minimum energy needed to break a covalent bond in the semiconductor
crystal, thus freeing electrons for conduction. The density of conduction (or free) electrons is
represented by the symbol n (electrons/cm), and for intrinsic material n = ni. The term intrinsic
refers to the generic properties of pure material. Although ni is an intrinsic property of each
semiconductor, it is extremely temperature-dependent for all materials.
Example: Calculate the value of ni in pure silicon at room temperature (300 K). EG = 1.12 eV,
assume T = 300 oK at room temperature.
A second charge carrier is actually formed when the covalent bond in Fig. 1.9 is broken. As an
electron, which has charge −q equal to −1.602 × 10−19 C, moves away from the covalent bond, it
leaves behind a vacancy in the bond structure in the vicinity of its parent silicon atom. The vacancy
is left with an effective charge of +q. An electron from an adjacent bond can fill this vacancy,
creating a new vacancy in another position. This process allows the vacancy to move through the
crystal. The moving vacancy behaves just as a particle with charge +q and is called a hole. Hole
density is represented by the symbol p (holes/cm3). As already described, two charged particles are
created for each bond that is broken: one electron and one hole. For intrinsic silicon, ni = n = p,
and the product of the electron and hole concentrations is:
pn = ni2 . The pn product is given by Eq. whenever a semiconductor is in thermal equilibrium.
15
Drift currents
Electrical resistivity ρ and its reciprocal, conductivity σ, characterize current flow in a material
when an electric field is applied. Charged particles move or drift in response to the electric field,
and the resulting current is called drift current. The drift current density j is defined as:
j = Q*v: (C/cm3)(cm/s) = A/cm
2. where j = current density, Q = charge density, the charge in a
unit volume, the charge in coulombs moving through an area of unit cross section, v =velocity of
charge in an electric field.
Mobility
We know from electromagnetics that charged particles move in response to an applied electric field.
This movement is termed drift, and the resulting current flow is known as drift current. Positive
charges drift in the same direction as the electric field, whereas negative charges drift in a direction
opposed to the electric field. At low fields carrier drift velocity v (cm/s) is proportional to the
electric field E (V/cm); the constant of proportionality is called the mobility μ:
vn=−μn*E : where vn = velocity of electrons (cm/s), vp= velocity of holes (cm/s), μn =electron
mobility, 1350 cm2/V · s in intrinsic Si, μp =hole mobility, 500 cm
2/V · s in intrinsic Si.
Exercise: Calculate the velocity of a hole in an electric field of 10 V/cm. What is the electron
velocity in an electric field of 1000 V/cm? The voltage across a resistor is 1 V, and the length
of the resistor is 2 µm. What is the electric field in the resistor?
Answers: 5.00 × 103cm/s; 1.35 × 10
6cm/s; 5.00 × 10
3V/cm.
Resistivity of intrinsic silicon
We are now in a position to calculate the electron and hole drift current densities jdriftn and jdriftp:
in which Qn = (−qn) and Qp= (+qp) represent the charge densities (C/cm
3) of electrons and
holes, respectively. The total drift current density is then given by:
jdriftT= jn+ jp= q(nμn+ pμp)E = σ E
This equation defines σ, the electrical conductivity: σ = q(nμn + pμp)(Ω· cm) −1
Resistivity ρ is the reciprocal of conductivity: ρ =1/σ(Ω · cm). The resistivity unit, the Ohm.cm,
is therefore:
ρ = E/ jdriftT and V/cm/ A/cm2 = Ω · cm
Example: Find the resistivity of intrinsic silicon at room temperature (300oK) and classify it as an
insulator, semiconductor or conductor. Suppose μn=1350cm2/V·s, μp=500 cm
2/V·s and ni= 10
10/cm
3
in intrinsic Si.
Analysis: : σ = q(nμn + pμp)
σ = (1.60 × 10−19
)[(1010
)(1350) + (1010
)(500)] (C)(cm-3
)(cm2/V·s) = 2.96 × 10
−6 (Ω · cm)
−1
The resistivity ρ is equal to the reciprocal of the conductivity, so for intrinsic silicon
ρ = 1/σ = 3.38 × 105 Ω · cm
we see that intrinsic silicon can be characterized as an insulator, albeit near the
16
low end of the insulator resistivity range.
Exercise: Find the resistivity of intrinsic silicon at 400oK and classify it as an insulator,
semiconductor, or conductor. Use the mobility values μn=1350cm2/V·s, μp=500 cm
2/V·s.
Answer: 1450 Ω· cm, semiconductor
Exercise: Calculate the resistivity of intrinsic silicon at 50oK if the electron mobility is
6500 cm2/V·s and the hole mobility is 2000 cm
2/V· s. Classify the material.
Answer: 1.69 × 1053
Ω·cm, insulator
Example: Calculate the electron concentration a piece of rod of length 3 mm and 1 x 4 µm cross
section area, if a current 5 mA produces 0.1 V drop. Suppose the mobility of electrons is 1000
cm2/V.s. and classify it as an insulator, semiconductor or conductor.
Solution: Jn = σn * E or ( I/A) = σn *( V/L)
Thus: σn = (I*L)/ (V*A) = (5*10-3
*3*10-1
)/( 0.1* 1*10-4
*4*10-4
) = 3.75*105 Ω. cm
σn = qnμn thus n = σn / qμn = 3.75*105/( 1.6*10
-19*10
3) = 2.3 * 10
21 /cm
3
The rode is conductor.
Note: The materials can be classified according to electron concentration number as follow:
Conductor: n > 1021
/ cm3
Semiconductor 10 < n > 1021
/cm3
Insulator: n< 10 /cm3
Impurities in semiconductors
The real advantages of semiconductors emerge when impurities are added to the material in minute
but well-controlled amounts. This process is called impurity doping, or just doping, and the
material that results is termed a doped semiconductor. Impurity doping enables us to change the
resistivity over a very wide range and to determine whether the electron or hole population controls
the resistivity of the material. The following discussion focuses on silicon, although the concepts of
impurity doping apply equally well to other materials. The impurities that we use with silicon are
from columns III and V of the periodic table.
Donor impurities in silicon
Donor impurities in silicon are from column V, having five valence electrons in the outer shell.
The most commonly used elements are phosphorus, arsenic, and antimony. When a donor atom
replaces a silicon atom in the crystal lattice, as shown in Fig. 1.10, four of the five outer shell
electrons fill the covalent bond structure; it then takes very little thermal energy to free the extra
electron for conduction. At room temperature, essentially every donor atom contributes (donates) an
electron for conduction. Each donor atom that becomes ionized by giving up an electron will have a
net charge of +q and represents an immobile fixed charge in the crystal lattice.
Acceptor impurities in silicon
Acceptor impurities in silicon are from column III and have one less electron than silicon in the
outer shell. The primary acceptor impurity is boron, which is shown in place of a silicon atom in the
lattice in Fig. 1.10 (b). Because boron has only three electrons in its outer shell, a vacancy exists in
the bond structure, and it is easy for a nearby electron to move into this vacancy, creating another
vacancy in the bond structure. This mobile vacancy represents a hole that can move through the
lattice, and the hole may simply be visualized as a particle with a charge of +q. Each impurity atom
that becomes ionized by accepting an electron has a net charge of −q and is immobile in the lattice.
17
(a) (b)
Figure 1.10 (a) An extra electron is available from a phosphorus donor atom. (b) A hole is created
after boron atom accepts an electron.
Electron and hole concentrations in doped Semiconductors
We now discover how to calculate the electron and hole concentrations in a semiconductor
containing donor and acceptor impurities. In doped material, the electron and hole concentrations
are no longer equal. If n > p, the material is called n-type, and if p > n, the material is referred to as
p-type. The carrier with the larger population is called the majority carrier, and the carrier with
the smaller population is termed the minority carrier. To make detailed calculations of electron
and hole densities, we need to keep track of the donor and acceptor impurity concentrations:
ND= donor impurity concentration atoms/cm3
NA= acceptor impurity concentration atoms/cm3
Two additional pieces of information are needed. First, the semiconductor material must remain
charge neutral, which requires that the sum of the total positive charge and negative charge be zero.
Ionized donors and holes represent positive charge, whereas ionized acceptors and electrons carry
negative charge. Thus charge neutrality requires: q(ND+ p − NA− n) = 0
Second, the product of the electron and hole concentrations in intrinsic material was given before.
as pn = n2i, the relation is true even for doped semiconductors in thermal equilibrium, and is valid
for a very wide range of doping concentrations.
If the concentration of donor atoms is ND, where ND is usually much greater than ni, the
concentration of free electrons in the n-type silicon will be: nn = ND
where the subscript n denotes n-type silicon. Thus nn is determined by the doping concentration and
not by temperature. This is not the case, however, for the hole concentration. All the holes in the n-
type silicon are those generated by thermal ionization. Their concentration can be found by noting
that the relationship in pn = n2
i applies equally well for doped silicon, provided thermal
equilibrium is achieved. Thus for n-type silicon: pnnn = ni2
Substituting for nn we obtain for Pn = ni2/ND
Finally, we note that in n-type silicon the concentration of free electrons will be much larger than
that of holes. Hence electrons are said to be the majority charge carriers and holes the minority
charge carriers in n-type silicon.
Similarly for p-type material, If the acceptor doping concentration is NA, where the hole
concentration becomes NA>> ni; pp = NA and np =ni2/ NA
18
Example: A silicon bar is 3 mm long and has a rectangular cross section area 0.05 x 0.1 mm and
ni = 1010
/cm3
at room temperature (300 oK). Calculate the voltage applied across the bar to produce
a steady current of 1 µA, if the semiconductor is: (1) intrinsic, (2) if it is doped 5*1014
/ cm3
of donor
atoms (n-type), suppose the electron mobility is 1500 cm2/V.s.
Solution:
(1) When the semiconductor is intrinsic n = ni = 1010
/ cm3
σn = qnμn = 1.6* 10-19
* 1010
* 1500 = 2.4* 10-6
(Ω. cm)
Jn = σn * E or ( I/A) = σn *( V/L)
Thus: σn = (I*L)/ (V*A) = (1*10-6
*3*10-1
)/(V*0.05*0.1*10-2
) = 2.4* 10-6
(Ω. cm)
V = 2500 volt (2) When the semiconductor doped with donor n = ND = 5* 10
14 /cm
3.
σn = qnμn = 1.6* 10-19
*5* 1014
* 1500 = 1.2* 10-1
(Ω. cm)
σn = (I*L)/ (V*A) = (1*10-6
*3*10-1
)/(V*0.05*0.1*10-2
) = 1.2* 10-1
(Ω. cm)
V = 0. 05 volt
Note: the voltage required to produce the current when the semiconductor is doped is much lower
than the voltage required when the semiconductor is intrinsic. In other words the material is
changed from seminsulator to semiconductor
Diffusion currents
As already described, the electron and hole populations in a semiconductor are controlled by the
impurity doping concentrations NA and ND. Up to this point we have tacitly assumed that the doping
is uniform in the semiconductor, but this need not be the case. Changes in doping are encountered
often in semiconductors, and there will be gradients in the electron and hole concentrations.
Gradients in these free carrier densities give
rise to a second current flow mechanism,
called diffusion. The free carriers tend to
move (diffuse) from regions of high
concentration to regions of low concentration
in much the same way as a puff of smoke in
one corner of a room rapidly spreads
throughout the entire room. A simple one-
dimensional gradient in the electron or hole
density is shown in Fig. 1.11.
Figure 1.11 Carrier diffusion in the presence
of a concentration gradient.
The gradient in this figure is positive in the +x
direction, but the carriers diffuse in the −x
direction, from high to low concentration.
Thus the diffusion current densities are
proportional to the negative of the carrier
gradient:
The proportionality constants Dp and Dn are
the hole and electron diffusivities, with units
(cm Diffusivity and mobility are related by
Einstein’s relationship:
19
The quantity (kT/q = VT) is called the thermal voltage VT, and its value is approximately 0.025 Vat
room temperature. Typical values of the diffusivities (also referred to as the diffusion coefficients)
in silicon are in the range 2 to 35 cm2/s for electrons and 1 to 15 cm
2/s for holes at room
temperature.
Exercise: Calculate the value of the thermal voltage VT for T = 50 K, 300 K, and 400 K
Answers: 4.3 mV; 25.8 mV; 34.5 mV
Exercise: What are the maximum values of the room temperature values (300 K) of the diffusion
coefficients for electrons and holes in silicon, let the mobility’s μn=1350cm2/V·s, μp=500 cm
2/V·s.
Answers: Using VT = 25.8 mV; 35.1 cm2/s, 12.8 cm
2/s
Exercise: An electron gradient of +1016
/cm3.µm exists in a semiconductor. What is the diffusion
current density at room temperature if the electron diffusivity = 20 cm2/s? Repeat for a hole gradient
of +1020
cm4 with Dp= 4cm
2/s.
Answer: +320 A/cm2; −64 A/cm
2
Total current
Generally, currents in a semiconductor have both drift and diffusion components. The total electron
and hole current densities jTn and jTp can be found by adding the corresponding drift and diffusion
components:
combined with Gauss’ law: ∇·(ε*E) = Q
where ε = permittivity (F/cm), E = electric field (V/cm), and Q = charge density (C/cm3)
Energy band model
This section discusses the energy band model for a semiconductor, which provides a useful
alternative view of the electron–hole creation process and the control of carrier concentrations by
impurities. Quantum mechanics predicts that the highly regular crystalline structure of a
semiconductor produces periodic quantized ranges of allowed and disallowed energy states for the
electrons surrounding the atoms in the crystal. Figure 1.12 (a) is a conceptual picture of this band
structure in the semiconductor, in which the regions labeled conduction band and valence band
represent allowed energy states for electrons. Energy EV corresponds to the top edge of the valence
and represents the highest permissible energy for a valence electron. Energy EC corresponds to the
bottom edge of the conduction band and represents the lowest available energy level in the
conduction band. Although these bands are shown as continuums in Fig. 1.12 (a), they actually
consist of a very large number of closely spaced, discrete energy levels. Electrons are not permitted
to assume values of energy lying between EC and EV. The difference between EC and EV is called the
bandgap energy EG= EC− EV
Electron–hole pair generation in an intrinsic semiconductor
In silicon at very low temperatures (≈ 0 K), the valence band states are completely filled with
electrons, and the conduction band states are completely empty, as shown in Fig. 1.12 (b). The
semiconductor and in this situation does not conduct current when an electric field is applied. There
are no free electrons in the conduction band, and no holes exist in the completely filled valence
band to support current flow. The band model of Fig. 1.12(b) corresponds directly to the completely
20
filled bond model of Fig. 1.10 (a). As temperature rises above 0 K, thermal energy is added to the
crystal. A few electrons gain the energy required to surmount the energy bandgap and jump from
the valence band into the conduction band, as shown in Fig. 1.12 (c). Each electron that jumps the
bandgap creates an electron– hole pair. This electron–hole pair generation situation corresponds
directly to that presented in Fig. 2.31.10 (b).
(a) (b) (c)
Figure 1.12 (a0 Energy band model for a semiconductor with bandgap EG. (b) Semiconductor at 0
K with filled valence band and empty conduction band. (c) Creation of electron–hole pair by
thermal excitation across the energy bandgap.
Energy band model for a doped semiconductor
Figures 1.13 (a, b, and c) present the band model for extrinsic material containing donor and/or
acceptor atoms. In Fig. 1.13 (a), a concentration N of donor atoms has been added to the
semiconductor. The donor atoms introduce new localized energy levels within the bandgap at a
donor energy level ED near the conduction band edge. The value of (EC− ED) for phosphorus is
approximately 0.045 eV, so it takes very little thermal energy to promote the extra electrons from
the donor sites into the conduction band. The density of conduction-band states is so high that the
probability of finding an electron in a donor state is practically zero, except for heavily doped
material (large ND) or at very low temperature. Thus at room temperature, essentially all the
available donor electrons are free for conduction. In Fig. 1.13 (b), a concentration NA of acceptor
atoms has been added to the semiconductor. The acceptor atoms introduce energy levels within the
bandgap at the acceptor energy level EA near the valence band edge. The value of (EA- EV ) for
boron is approximately 0.044 eV, and it takes very little thermal energy to promote electrons from
the valence band into the acceptor energy levels. At room temperature, essentially all the available
acceptor sites are filled, and each promoted electron creates a hole that is free for conduction.
Compensated semiconductors
The situation for a compensated semiconductor, one containing both acceptor and donor
impurities, is depicted in Fig. 1.13 (c) for the case in which there are more donor atoms than
acceptor atoms. Electrons seek the lowest energy states available, and they fall from donor sites,
filling all the available acceptor sites. The remaining free electron population is given by n = (ND−
NA). The energy band model just discussed represents a conceptual model that is complementary to
the covalent bond model. Together they help us visualize the processes involved in creating holes
and electrons in doped semiconductors.
21
Figure 1.13 (a) Donor level with activation energy (EC− ED). (b) Acceptor level with activation
energy (E A− EV). (c) Compensated semiconductor containing both donor and acceptor atoms with
ND> NA
.