About 20 years before no one use smartphones but nowadays everyone have a smartphone. Apple iPhone 13 Pro, Google Pixel 6 Pro, Oppo Find X3 Pro, OnePlus 9 Pro, Sony Xperia 1 III, Asus ROG Phone 5s Pro and Xiaomi 11T Pro are examples of some popular smartphones. This article is all about chemistry behind smartphones by Chemistry Notes Info.
Different Chemistry Elements in Smartphones
Typically smartphone contains many elements like Silver, Gold, Lithium, Praseodymium, Terbium, Yttrium, Gadolinium, Indium, Tin, Oxygen, Carbon, Copper, Tantalum, Silicon, Oxygen, Antimony, Arsenic, Phosphorus and Gallium.
Generally On Average a Smartphone Contains About
300 mg Silver (Ag having Atomic No. 47, Atomic Mass 107.87)
30 mg Gold (Au having Atomic No. 79, Atomic Mass 196.97)
Battery- Generally smartphones have Li-Ion Battery, this battery have Lithium Cobalt Oxide as a +ve electrode and Carbon or Graphite as a -ve electrode. This -ve electrode release electrons which travel towards +ve electrode as a result provide power to your phone.
Screen- Screen contains following elements which provide color to screen to display visual content.
Praseodymium (Pr having Atomic No. 59, Atomic Mass 140.91)
Terbium (Tb having Atomic No. 65, Atomic Mass 158.93)
Yttrium (Y having Atomic No. 39, Atomic Mass 88.91)
Gadolinium (Gd having Atomic No. 64, Atomic Mass 157.25)
Touch- Touchscreen takes inputs from user and are transparent, all these are possible due to following elements
Indium (In having Atomic No. 49, Atomic Mass 114.82)
Tin (Sn having Atomic No. 50, Atomic Mass 118.71)
Oxygen (O having Atomic No. 8, Atomic Mass 16)
Wiring- Wiring or electrical circuits are made up of copper and capacitors are made up of Tantalum. Capacitor store regulate electricity and loose electrical charge in fraction of seconds.
Copper (Cu having Atomic No. 29, Atomic Mass 63.55)
Tantalum (Ta having Atomic No. 73, Atomic Mass 180.95)
Microchip- Microchip or CPU (Central Processing Unit) also called brain of smartphone is made-up of silicon, oxygen, antimony, arsenic, phosphorus and gallium. All these elements are used to produce highly conductive powerful microchips so you can play games, watch videos, click photos, use your phone camera for taking selfy, audio video recording, calling, chatting, using apps like whats app, facebook, twitter or whatsoever stuff you like to do with your smartphone is possible due to chemistry.
Silicon (Si having Atomic No. 14, Atomic Mass 28.09)
Oxygen (O having Atomic No. 8, Atomic Mass 16)
Antimony (Sb having Atomic No. 51, Atomic Mass 121.76)
Arsenic (As having Atomic No. 33, Atomic Mass 74.92)
Phosphorus (P having Atomic No. 15, Atomic Mass 30.97)
Gallium (Ga having Atomic No. 31, Atomic Mass 69.73)
What's Inside Your Smartphone
Smartphone is made-up of different components which are assembled to make smartphones. Like display (to show visual content), touchscreen (to take inputs from user), cameras (to take photos, selfy and to shoot videos). Microphone (to receive audio or to record sound), case (body of phone), battery (to provide power), sim card slot (for sim), speakers (for sound, to listen music), sensors (for different purpose like ambient light sensor for light intensity means automatically set screen brightness according to surrounding light and ultimately save battery life.
Gyroscope and accelerometer to play video-games as these sensor tracks phone movement, digital compass to detect north direction for maps and navigation, proximity sensor used to prevent unwanted touch commands by locking phone during phone call when you bring phone near your ear).
Motherboard (printed circuit board containing principal components of smartphone with connectors for other circuit boards to be
slotted into), memory (to store data, movies, photos, videos, songs), transceiver (to transmit and receive communications), radio (to transmit data and to receive data).
Cell phone radio (that communicate with cell tower, when you make call) wifi radio (to download big files, movies songs etc and they consume less battery as they travel very less distance) bluetooth radio, NFS rado, GPS radio etc. All these components contain some chemical elements of periodic table and when all components are assembled they give you smartphone which you use daily.
Structure of Atom Class 11 Chemistry Notes Chapter 2
AtomicTheory of matter
:-
According to this theory, atom is the ultimate particle of matter. This atomic theory of matter is also
known as Dalton’sAtomic theory (1808).
Cathode
ray discharge tube experiments: -
Cathode
rays start from cathode and move toward anode.
These
rays are not visible but there behavior can be observed with fluorescent or
phosphorescent material.
In
the absence of magnetic or electric field these rays travels in straight lines.
In
the presence of magnetic or electric field, the behavior of cathode rays is similar to Negatively charged particles. Which suggest that these rays contain negatively charge particles called
electron.
Cathode
rays (or electrons) do not depend on the material
of the electrode andnature of the gas in the tube so electrons are basic constituent of all atoms.
Charge (e) to mass (me)
ratio of electron
Measured
byJ. J. Thomson (1897).
By
using cathode ray tube.
By applying electrical & magnetic field perpendicular
to each other & also perpendicular to path of electrons.
He
proposeddeviation of particles from
their path in presence of magnetic or electrical field depend upon the
following-
1.Magnitude of– vecharge
on particle
i.e.
if magnitude of charge on particles is greater than interaction with magnetic
or electric field is greater so deflection is also grater.
2.Mass of
particles
i.e.
particle is lighter then deflection is greater.
3.Strength of magnetic or electric field.
i.e. if strength of
magneticfield or voltage, at electron is
increases then deflection of e-
also increases.
=>value of e/me =
1.758820× 1011 C kg-1
Charge
of electron
= Determine
byR. A. Millikan
= By
oil drop experiment (1906-1914)
= Charge
on e- =-1.6× 10-19
C
= Present
accepted value , e- = -1.6022× 10-19 C
Mass of electron
From charge on e- & e/me
We get,
Me = 9.1094
´
10-31 kg
Discovery of protons
= Discovered
by E. Goldstein.
= In
modified cathode ray tube gives +ve charge carrying particles known as canal
rays.
= Lithest
& smallest +ve ion obtained from Hydrogen called proton.
Characteristics
1)Depend
upon, nature of gas present in cathode ray tube.
2)Charge
to mass ratio of particles depends on gas from which these originate.
3)Some
of +ve charged particles carry a multiple unit of electrical charge.
4)Behavior
of protons in magnetic or electric field is opposite to that of electron behavior.
Discovery
of neutrons
Discovered
by Chadwick (1932).
By
bombarding a thin sheet of beryllium by alpha particles.
Electrically
neutral particles were emitted known as neutrons.
Thomson
model of atom
Given by J.J Thomson (1898)
According
to J.J. Thomson, atoms posses a spherical shape,
with radius about 10-10 m,
in which + ve charge is uniformly distributed.
Electrons
are embedded in such a manner to give most stable electrostatic arrangement.
Other
names of this model plum pudding, raisin pudding, watermelon model.
Mass
is assumed to be uniformly distributed in atom.
Rutherford’s
nuclear model of atom
= Given
by Rutherford & his students Ernest Marsden and Hans Geiger.
= By
ฮฑ- particles scattering experiment-
Rutherford’s
nuclear model of atom
= When
beam of high energy ฮฑ- particles was directed at gold foil, then tiny flash of
light observed at photographic plate.
Rutherford observed
that-
1)Most
of the ฮฑ-practicalpassedthrough gold foil un-deflected.
2)A
small fraction of ฮฑ- particles was deflected by small angles.
3)A
very few ฮฑ- particles (about 1 in 20,000) bounced back means deflected by nearly
1800
From above observations
he concludes the structure of atom.
1)Most
of space in atom is empty because most of ฮฑ- particles passed un-deflected.
2)Few
+ve charged ฮฑ- particles were deflected.
Because
+ ve charge of the atom present in center in very small volume that repelled
& deflected the +ve charged ฮฑ- particles.
3)Volume
of nucleus is negligible as compared to total volume of atom
i.e.radius of atom = 10-10m (approx)
radius
of nucleus =10-15m(approx)
On the basis of
observation &conclusion Rutherford
proposed model of atom as-
1)+ve
charge & most of mass present in the center of atom known as nucleus.
2)Electrons
moves around nucleus with very high speed in circular paths known as orbits.
3)Electrons
and nucleus (protons) are held together by electrostatic force of attraction .
Atomic
number (Z)
= no of protons in the nucleus of an atom
= no of
electrons in a neutral atom
Mass
number(A) = number
of protons (z) + number of Neutron (n)
Isobars
:-
These are atoms with same mass number
but different atomic number.
Isotopes: -
These are atoms with same atomic number butdifferent atomic mass no.
Wave
nature of electromagnetic radiations: -
First explanation given by James Maxwell (1870).
1)Oscillating
magnetic & electric fields produced by the oscillating charged particles
are perpendicular to each other and also perpendicular to the wave
direction of propagation.
2)These
waves do not require medium i.e. electromagnetic wave can travel in vacuum.
3)Electromagnetic
radiation differs from one another in frequency or wavelength gives
electromagnetic spectrum.
4)Different
units are used to represent electromagnetic radiation.
n
= frequency,
l = wavelength.
Particle
nature of electromagnetic radiation :-
Also known as Planck’sQuantum theory
= Planck suggested that the atoms and molecules
can absorb or emit energy in discrete quantities not in continuous manner.
Planck gives it name as quantum. Energy (E) ofquantum ofradiation is directly
proportional to its frequency(n)
i.e.E=hn
Where,h =
planks constant = 6.626× 10-34 js
Photo
electric effect:-
= given
by H. Hertz (1887)
= When
a beam of light strike a metal surface then electrons were ejected. This phenomena
is known as photo electric effect.
1.Electrons
ejected from metal surface, when beam oflight strike the metal surface.
2.Number
of electron ejected is directly proportional to intensity (or brightness) of
light.
3.There
is characteristic minimum frequency (n0
threshold frequency) below which photoelectric effect is not observed.
4.If
n
> n0
then electrons comes out with kinetic energy which increases with increase in frequency
of light.
Kinetic
energy of ejected electrons is given by-
h
n
= h n0+
½(meV2)
Spectroscopy:-
study ofabsorption or emission spectra
is called spectroscopy .
Bohr’s model for hydrogen
atom:-
= Explain
by Nails Bohr (1913).
= Postulates
for Bohr’s modal are,
1.Electron
in hydrogen atom move around nucleus in circular path of fixed radius and energy.
these paths are called orbits.
2.Energy
of electron does not change with time.
However, when electron move from
lower to higher stationary state. It absorbed some amount of energy and energy
release when it comes back.
3.Frequency
of radiations emitted or absorbed when transition of electron occur is given by
Where, E1 & E2 is lower &
higher energy state.
4.Angular
momentum of n electron in given stationary state is given by-
[Where n =1,2,3.....]
Limitation
of Bohr’s model:-
1.Bohr
model fail to explain fine detail of hydrogen atom spectrum observed by spectroscopic,
techniques.
2.It
fails to explain spectrum of other atom except hydrogen atom.
3.It
fails to explain splitting of the spectral lines in presence of electric field (stark
effect) or magnetic field ( Zeeman effect ).
4.Fail
to explain formation of molecules from atoms by chemical bonding.
Dual behaviour of
matter :-
= Explain
by de-Broglie (1924)
= He
explain that matter also behave like radiation and exhibit dual behavior means
both like particle and wave like properties .
= Relation
Where l =wavelength.
m = mass of particle ,
v = velocity of particle,
p =
momentum
Heisenberg’s
uncertainty principle:-
Given by Werner Heisenberg (1927)
He explain that it is impossible to
determine simultaneously the exact position and exact momentum (or velocity) of
an electron.
Mathematical explanation
Where,Dx= uncertaintyin position
DVx = uncertainty in velocity or momentum
Quantum
mechanical model of atom:-
Branches of science which explain
duel behavior of Metter is called quantum mechanics.
Quantum
mechanics independently developed by Werner Heisenberg and Erwin Schrodinger
(1926).
Fundamental equation developed by Schrodinger. (He won Nobel Prize in 1933).
Equation for a system (atom or molecules
was, energy does not change with time)
Principle
quantum number ‘n’ :-
·It is a positive Integer with value of n
= 1,2,3......
·It determine size and energy of orbital.
·It also identifies the shell with
increase in number of allowed orbital.
And given by n2
N=1,2,3,4........
Shell
= k,l,m,l......
·Size of orbital increase with increase inn.
Azimuthal quantum no.‘l’:-
·It is also known as orbital angular
momentum or subsidiary quantum no.
·It defined 3D shape of orbital.
·For given value of n possible value
of
L= 0,1,2,3,4,5,----------(n-1) ,
Ex :- ifn=1thenl=0
ifn=2thenl=0,1
ifn=5thenl=0,2,3,4
·Each shell consists of one or more
sub-shells.
·No of sub-shells = value ofn
Ifn= 1then1 sub-shell =(l=0)
Ifn= 2then2 sub-shell =(l=0,1)
Ifn= 3then3 sub-shell =(l=0,1,2)
·Value ofl =0,1,2,3,4,5----------
Notation for sub-shell= s, p, d,f,g,
h--------------
·Sub-shell notation
n
l
Sub-shellnotation
1
0
1s
2
0
2s
2
1
2p
3
0
3s
3
1
3p
3
2
3d
4
0
4s
4
1
4p
4
2
4d
4
3
4f
Magnetic orbital quantum no ‘mi’ :-
·This quantum no (mi) gives information
about orientation oftheorbital .
·mi = (2l+1) i.e. if value oflis1 then value ofmi = 2×1+1=3=(-1,0,1)
Value of p
0
1
2
3
4
5
Sub-shell
notation
S
P
D
F
G
H
No of orbital’s
1
3
5
7
9
11
Electron
spin quantum (ms):-
·Proposed by G. Uhlen Beck & S.
Goodsmit (1925).
·Electrons spins around its own axis.
·Ms have two value +1/2 &
-1/2.
·Ms gives information about
orientation of the spin of the
electron.
Aufbau
principle :-
According to this principle, in the ground
state of the atoms the orbital’s are filled in order of their increasing
energies. Means electrons enter higher energy orbital’s,so order in which orbital’s are filled is 1s,
2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p.
Pauli
exclusion principle:-
· Given by W. Pauli (1926).
·Two electrons in an atoms can’t have
same set of 4-quantum no.
·Only two electrons may exist in same orbital
and these electrons must have opposite spin.
Hund’srule of maximum multiplicity
:-.
·According to this rule, pairing ofelectron in the orbital’s belonging to the
same sub-shell (p, d or f) does not take place until each orbital
belonging to that sub-shell has got one electron each i.e. it is singly occupied.
Smartphone is made-up of different components which are assembled to make smartphones. Like display (to show visual content), touchscreen (to take inputs from user), cameras (to take photos, selfy and to shoot videos). Microphone (to receive audio or to record sound), case (body of phone), battery (to provide power), sim card slot (for sim), speakers (for sound, to listen music), sensors (for different purpose like ambient light sensor for light intensity means automatically set screen brightness according to surrounding light and ultimately save battery life. 
