An atomic orbital is defined as the region around the nucleus where an electron is most likely to be found. There are four quantum numbers that describe the orbitals: principal (n), angular momentum (l), magnetic (m), and spin (s). The principal quantum number indicates the electron shell and average distance from the nucleus. The angular momentum number determines the shape of the orbital. The magnetic number indicates the direction of the orbital. The spin number represents the electron's clockwise or counterclockwise spin. Common atomic orbitals include s, p, d, and f orbitals, which have different shapes and orientations determined by their quantum numbers.
Quantum Numbers
Wave nature of electrons
atomic structure
principle Quantum number
Azimuthal quantum number
magnetic quantum number
spic quantum number
shapes of orbitals
Quantum Numbers
Wave nature of electrons
atomic structure
principle Quantum number
Azimuthal quantum number
magnetic quantum number
spic quantum number
shapes of orbitals
A detailed presentation about what is MOT. Explaining its principles, sigma and pi bonds, bond order, and molecular stability. A good and knowledgeable presentation to understand these concepts.
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
An easy guide to one of the most important principles taught in secondary chemistry, The Aufbau Principle. Helpful for students who consider such an amazing topic to be a nightmare. Happy Chemistry!
Modern Periodic Law,Classification of Elements, Periodicity in Atomic Properties,Atomic Radius, Ionisation potential or Ionisation Energy,Electron Affinity
The hydrogen atomic spectrum consists of a sequence of spectral lines arranged in the decreasing order of their wavelengths and the increasing order of their frequencies. These spectral lines are classified into six series. And their names represent scientists who discovered them. The six series of the hydrogen spectrum are;
Lyman series
Balmer series
Paschen series
Brackett series
Pfund series
Humphreys series
Quantum Numbers and Atomic Orbitals By solving t.pdfarasanlethers
Quantum Numbers and Atomic Orbitals By solving the Schrödinger equation (Hy
= Ey), we obtain a set of mathematical equations, called wave functions (y), which describe the
probability of finding electrons at certain energy levels within an atom. A wave function for an
electron in an atom is called an atomic orbital; this atomic orbital describes a region of space in
which there is a high probability of finding the electron. Energy changes within an atom are the
result of an electron changing from a wave pattern with one energy to a wave pattern with a
different energy (usually accompanied by the absorption or emission of a photon of light). Each
electron in an atom is described by four different quantum numbers. The first three (n, l, ml)
specify the particular orbital of interest, and the fourth (ms) specifies how many electrons can
occupy that orbital. Principal Quantum Number (n): n = 1, 2, 3, …, 8 Specifies the energy of
an electron and the size of the orbital (the distance from the nucleus of the peak in a radial
probability distribution plot). All orbitals that have the same value of n are said to be in the same
shell (level). For a hydrogen atom with n=1, the electron is in its ground state; if the electron is in
the n=2 orbital, it is in an excited state. The total number of orbitals for a given n value is n2.
Angular Momentum (Secondary, Azimunthal) Quantum Number (l): l = 0, ..., n-1. Specifies the
shape of an orbital with a particular principal quantum number. The secondary quantum number
divides the shells into smaller groups of orbitals called subshells (sublevels). Usually, a letter
code is used to identify l to avoid confusion with n: l 0 1 2 3 4 5 ... Letter s p d f g h ... The
subshell with n=2 and l=1 is the 2p subshell; if n=3 and l=0, it is the 3s subshell, and so on. The
value of l also has a slight effect on the energy of the subshell; the energy of the subshell
increases with l (s < p < d < f). Magnetic Quantum Number (ml): ml = -l, ..., 0, ..., +l. Specifies
the orientation in space of an orbital of a given energy (n) and shape (l). This number divides the
subshell into individual orbitals which hold the electrons; there are 2l+1 orbitals in each subshell.
Thus the s subshell has only one orbital, the p subshell has three orbitals, and so on. Spin
Quantum Number (ms): ms = +½ or -½. Specifies the orientation of the spin axis of an electron.
An electron can spin in only one of two directions (sometimes called up and down). The Pauli
exclusion principle (Wolfgang Pauli, Nobel Prize 1945) states that no two electrons in the same
atom can have identical values for all four of their quantum numbers. What this means is that no
more than two electrons can occupy the same orbital, and that two electrons in the same orbital
must have opposite spins. Because an electron spins, it creates a magnetic field, which can be
oriented in one of two directions. For two electrons in the same orbital, the spins must be
opposite to each oth.
A detailed presentation about what is MOT. Explaining its principles, sigma and pi bonds, bond order, and molecular stability. A good and knowledgeable presentation to understand these concepts.
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
An easy guide to one of the most important principles taught in secondary chemistry, The Aufbau Principle. Helpful for students who consider such an amazing topic to be a nightmare. Happy Chemistry!
Modern Periodic Law,Classification of Elements, Periodicity in Atomic Properties,Atomic Radius, Ionisation potential or Ionisation Energy,Electron Affinity
The hydrogen atomic spectrum consists of a sequence of spectral lines arranged in the decreasing order of their wavelengths and the increasing order of their frequencies. These spectral lines are classified into six series. And their names represent scientists who discovered them. The six series of the hydrogen spectrum are;
Lyman series
Balmer series
Paschen series
Brackett series
Pfund series
Humphreys series
Quantum Numbers and Atomic Orbitals By solving t.pdfarasanlethers
Quantum Numbers and Atomic Orbitals By solving the Schrödinger equation (Hy
= Ey), we obtain a set of mathematical equations, called wave functions (y), which describe the
probability of finding electrons at certain energy levels within an atom. A wave function for an
electron in an atom is called an atomic orbital; this atomic orbital describes a region of space in
which there is a high probability of finding the electron. Energy changes within an atom are the
result of an electron changing from a wave pattern with one energy to a wave pattern with a
different energy (usually accompanied by the absorption or emission of a photon of light). Each
electron in an atom is described by four different quantum numbers. The first three (n, l, ml)
specify the particular orbital of interest, and the fourth (ms) specifies how many electrons can
occupy that orbital. Principal Quantum Number (n): n = 1, 2, 3, …, 8 Specifies the energy of
an electron and the size of the orbital (the distance from the nucleus of the peak in a radial
probability distribution plot). All orbitals that have the same value of n are said to be in the same
shell (level). For a hydrogen atom with n=1, the electron is in its ground state; if the electron is in
the n=2 orbital, it is in an excited state. The total number of orbitals for a given n value is n2.
Angular Momentum (Secondary, Azimunthal) Quantum Number (l): l = 0, ..., n-1. Specifies the
shape of an orbital with a particular principal quantum number. The secondary quantum number
divides the shells into smaller groups of orbitals called subshells (sublevels). Usually, a letter
code is used to identify l to avoid confusion with n: l 0 1 2 3 4 5 ... Letter s p d f g h ... The
subshell with n=2 and l=1 is the 2p subshell; if n=3 and l=0, it is the 3s subshell, and so on. The
value of l also has a slight effect on the energy of the subshell; the energy of the subshell
increases with l (s < p < d < f). Magnetic Quantum Number (ml): ml = -l, ..., 0, ..., +l. Specifies
the orientation in space of an orbital of a given energy (n) and shape (l). This number divides the
subshell into individual orbitals which hold the electrons; there are 2l+1 orbitals in each subshell.
Thus the s subshell has only one orbital, the p subshell has three orbitals, and so on. Spin
Quantum Number (ms): ms = +½ or -½. Specifies the orientation of the spin axis of an electron.
An electron can spin in only one of two directions (sometimes called up and down). The Pauli
exclusion principle (Wolfgang Pauli, Nobel Prize 1945) states that no two electrons in the same
atom can have identical values for all four of their quantum numbers. What this means is that no
more than two electrons can occupy the same orbital, and that two electrons in the same orbital
must have opposite spins. Because an electron spins, it creates a magnetic field, which can be
oriented in one of two directions. For two electrons in the same orbital, the spins must be
opposite to each oth.
BOHR ATOM MODEL - BOHR SOMERFIELD MODEL - de-BROGLIE DUAL NATURE OF ATOM - SCHRODINGER WAVE EQUATION -MODERN PERIODIC LAW - ELECTRONEGATIVITY SCALES - SLATER RULE - BALANCING OF REDOX EQUATIONS
In this presentation you will be able to, describe how atomic orbitals arise from the Schrodinger's equation, relate orbital shapes to electron density distribution and interpret the information obtained from a four set of quantum numbers.
95electrons in the same orbital have different rus values .docxfredharris32
95
electrons in the same orbital have different rus values (one is +Yz and another -%),they
are said to be paired.
Electron Configuration
The energy of an electron in a hydrogen (H) atom is determined solely by its principal
quantum number n. However for many-electron atoms the orbital energies depend on
both the principal quantum number n andthe angular momenfum quantum number /.
Thus the energy of the orbitals in a many-electron atom increases in the order: ls < 2s <
2p < 3s a 3p < 4s < 3d < 4p < 5s, and so on. This order is also the order of filling
electrons into the orbitals in a many-electron atom. The guiding principle in assigning
electrons to the orbitals in a many-electron atom contains a set of three ru1es called the
Aufbau principle:
1. Lower-energy orbitals f,rll before higher-energy orbitals.
2. An atomic orbital can contain only two electrons, which must have opposite spins.
(Pauli exclusion principle: no two electrons in an atom can have the same four
quantum numbers.)
3 . When electrons are assigne d to p, d, or f orbitals, each successive electron enters a
different orbital of the subshell, each electron having the same spin as the previous
one; this proceeds until the subshell is half-full, after which electrons pair in the
orbitals one by one. (Hund's rule: the most stable arrangement of electrons in the
subshell is that with the maximum number of unpaired electrons, all with the same
spin.)
Flame Test
The resultant lowest-energy electron configuration is called the ground-state
configrnation of the atom. The electrons in the atom's outermost shell are called valance
electrons. When the atom absorbs enough energy, one or more of the valance electrons
move to a higher energy orbital, and the atom is said to be in an excited state. The excited
states are generally short-lived and rapidly decay back to the ground state by releasing
radiant energy in the form of light. The energy and frequency of the light that is released
during the decay transition depend on the difference in energy between the ground state
and the excited state. The energy difference (AQ, the frequency (v), and the wavelength
(2) of the light during emission are related by the equation, LE : hv: hclTwhere h ts
Planck's constant and c is the speed of light. When the wavelengths of the light emitted
fall in the visible region (400-800 nm), colors willbe observed.
Atoms of certain elements emit light
u'hen the elements or their
compounds are heated in a gas flame.
The flame takes on a distinctive
color detemined by the particular
element (flame test). Each atom has
its characteristic emission lines,
therefore flame tests can be used to
detect certain elements in unknown
cornpounds.
b!L
q)
Excited state
LE: hv: hclT
trl
Ground state
L
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t
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t
,
t
t
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the energy of the electron increases, and the electron is farther away from the nucleus. A
coliection of orbitals with the same n is called an electr.
Instructions for Submissions thorugh G- Classroom.pptxJheel Barad
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The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
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The empire's roots lie in the city of Rome, founded, according to legend, by Romulus in 753 BCE. Over centuries, Rome evolved from a small settlement to a formidable republic, characterized by a complex political system with elected officials and checks on power. However, internal strife, class conflicts, and military ambitions paved the way for the end of the Republic. Julius Caesar’s dictatorship and subsequent assassination in 44 BCE created a power vacuum, leading to a civil war. Octavian, later Augustus, emerged victorious, heralding the Roman Empire’s birth.
Under Augustus, the empire experienced the Pax Romana, a 200-year period of relative peace and stability. Augustus reformed the military, established efficient administrative systems, and initiated grand construction projects. The empire's borders expanded, encompassing territories from Britain to Egypt and from Spain to the Euphrates. Roman legions, renowned for their discipline and engineering prowess, secured and maintained these vast territories, building roads, fortifications, and cities that facilitated control and integration.
The Roman Empire’s society was hierarchical, with a rigid class system. At the top were the patricians, wealthy elites who held significant political power. Below them were the plebeians, free citizens with limited political influence, and the vast numbers of slaves who formed the backbone of the economy. The family unit was central, governed by the paterfamilias, the male head who held absolute authority.
Culturally, the Romans were eclectic, absorbing and adapting elements from the civilizations they encountered, particularly the Greeks. Roman art, literature, and philosophy reflected this synthesis, creating a rich cultural tapestry. Latin, the Roman language, became the lingua franca of the Western world, influencing numerous modern languages.
Roman architecture and engineering achievements were monumental. They perfected the arch, vault, and dome, constructing enduring structures like the Colosseum, Pantheon, and aqueducts. These engineering marvels not only showcased Roman ingenuity but also served practical purposes, from public entertainment to water supply.
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TESDA TM1 REVIEWER FOR NATIONAL ASSESSMENT WRITTEN AND ORAL QUESTIONS WITH A...
Orbitals
1.
2. • An atomic orbital is defined as the region in
space around the nucleus in which the
probability of finding the electron is
maximum.
What is orbital?
3. • The number which expresses the size, shapes,
and direction of the orbital from the nucleus
and the spins of the electron of their own
axes, are called quantum number.
Quantum Number
4. • There are four types of quantum number:
1. principal quantum number(n)
2. Subsidiary quantum number(l)
3.Magnetic quantum number (m)
4.Spin quantum number (s)
Types of Quantum Number
5. • Principal quantum number :
This express the orbits or principal energy level to
which the electron belongs and represents the
average distance of the electron from the
nucleus.It is denoted by n(n=1 2 3 etc).For the first
orbit n=1, for the second orbit n=2 and so on.The
energy levels are also called electron shells.
Innermost shell known as K shell and the
succeedings outer shells are denoted by the letter L
M N O P Q etc. Each shell has a definite value of
energy. the energy increase as the value of n
encrease.
6. Subsidiary quantum number
• This express sub-levels and the shapes of the
energy level.It is denoted by l. The vaule of l =o to
(n-1).When n=1 then l=o and so the 1st energy
level has 1 sub-shell.
n=1 then l=o
n=2 then l=0 1
n=3 then l=0 1 2
The value of subsidiary quantum number 0 1 2 3 4
are represented s,p,d,f respectively.
7. Magnetic quantum number
This express the directions of the sub-levels of
the orbital from the nucleus in three –
dimentional spaces. This number is designated
as m.The permitted valus of m are depending on
l. the value for the magnetic quantum numbers
m, are given by +1 to -1 , including 0.
8. Spin Quantum Number
• The spin quantum number represents the
direction of the electron spin.This quantum
number is designed as “s”.This is due to the
spinning of the electron about its own
axis.One spin clockwise and other spin is anti-
clock wise.Their values are s=+12 and s=-12.
9. S orbital
• S orbital is an atomic orbital with an angular
momentum quantum number I which
corresponds to 0. In other words, s
corresponds to l=0. S orbital is the closest
orbital to the nucleus, with other orbitals
lining up further away.).
10.
11. P orbital
• Unlike the spherically symmetric s orbitals, a p orbital is oriented
along a specific axis. All p orbitals have l = 1, and there are three
possible values for m (-1, 0, +1). Whenever m does not equal zero,
the wave function is complex, which makes visualization of the
wave function difficult. For l = 0, the m = 0 wave function is
designated pz. The m = -1 and +1 wave functions are combined to
produce two new wave functions, which are designated px and py.
12.
13. D orbital
• For d orbital l=2.Therefore the angular
momentum of an electron for d orbital is not
zero for l =2 the magnetic quantum number
(m) should have five different values m = -2 -1
0 +1 +2 .Accordingly there are five different
space orientations for d orbitals.
14.
15. F orbital
• A subshell that corresponds to the angular
momentum quantum number l = 3, found in
the fourth and higher principal energy levels.
Each contains seven orbitals.