Hybridization describes the bonding atoms from an atom's point of view. For a tetrahedral coordinated carbon (e.g. methane CH4), the carbon should have 4 orbitals with the correct symmetry to bond to the 4 hydrogen atoms.
Hybridization:
Developed by Linus Pauling, the concept of hybrid orbitals was a theory created to explain the structures of molecules in space. The theory consists of combining atomic orbitals (ex: s,p,d,f) into new hybrid orbitals (ex: sp, sp2, sp3).
Hybridization:
Developed by Linus Pauling, the concept of hybrid orbitals was a theory created to explain the structures of molecules in space. The theory consists of combining atomic orbitals (ex: s,p,d,f) into new hybrid orbitals (ex: sp, sp2, sp3).
The electron configuration is the distribution of electrons of an atom or molecule (or other physical structure) in atomic or molecular orbital . For example, the electron configuration of the neon atom is 1s2 2s2 2p6.
Hybridization is the idea that atomic orbitals fuse to form newly hybridized orbitals, which in turn, influences molecular geometry and bonding properties. Hybridization is also an expansion of the valence bond theory.
CONTENTS
INTRODUCTION
CONCEPTS OF WALSH DIAGRAM
APPLICATION IN TRIATOMIC MOLECULES
[IN AH₂ TYPE OF MOLECULES(BeH₂,BH₂,H₂O)]
INTRODUCTION
Arthur Donald Walsh FRS The introducer of walsh diagram (8 August 1916-23 April 1977) was a British chemist, professor of chemistry at the University of Dundee . He was elected FRS in 1964. He was educated at Loughborough Grammar School.
Walsh diagrams were first introduced in a series of ten papers in one issue of the Journal of the Chemical Society . Here, he aimed to rationalize the shapes adopted by polyatomic molecules in the ground state as well as in excited states, by applying theoretical contributions made by Mulliken .
Electron configuration process and steps. It has the explanation of how quantum numbers are arranged in the periodic table, and how they are used to find the electron configuration of elements. A brief explanation of Aufbau rule, Hund's rule and Pauli's Exclusion principle
A chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between atoms with opposite charges, or through the sharing of electrons as in the covalent bonds.
In chemistry, hybridisation (or hybridization) is.pdfsutharbharat59
In chemistry, hybridisation (or hybridization) is the concept of mixing atomic
orbitals to form new hybrid orbitals suitable for the qualitative description of atomic bonding
properties. Hybridised orbitals are very useful in the explanation of the shape of molecular
orbitals for molecules. It is an integral part of valence bond theory. Although sometimes taught
together with the valence shell electron-pair repulsion (VSEPR) theory, valence bond and
hybridization are in fact not related to the VSEPR model.[1] Contents [hide] 1 Historical
development 2 Types of hybridisation 2.1 sp3 hybrids 2.2 sp2 hybrids 2.3 sp hybrids 3
Hybridisation and molecule shape 3.1 Explanation of the shape of water 3.2 Controversy
regarding d-orbital participation 4 Hybridisation theory vs. MO theory 5 See also 6 External
links 7 References [edit]Historical development Chemist Linus Pauling first developed the
hybridisation theory in order to explain the structure of molecules such as methane (CH4).[2]
This concept was developed for such simple chemical systems, but the approach was later
applied more widely, and today it is considered an effective heuristic for rationalizing the
structures of organic compounds. For quantitative calculations of electronic structure and
molecular properties, hybridisation theory is not as practical as molecular orbital theory.
Problems with hybridisation are especially notable when the d orbitals are involved in bonding,
as in coordination chemistry and organometallic chemistry. Although hybridisation schemes in
transition metal chemistry can be used, they are not generally as accurate. Orbitals are a model
representation of the behaviour of electrons within molecules. In the case of simple
hybridisation, this approximation is based on atomic orbitals, similar to those obtained for the
hydrogen atom, the only atom for which an exact analytic solution to its Schrödinger equation is
known. In heavier atoms, like carbon, nitrogen, and oxygen, the atomic orbitals used are the 2s
and 2p orbitals, similar to excited state orbitals for hydrogen. Hybridised orbitals are assumed to
be mixtures of these atomic orbitals, superimposed on each other in various proportions. The
theory of hybridisation is most applicable under these assumptions. It gives a simple orbital
picture equivalent to Lewis structures. Hybridisation is not required to describe molecules, but
for molecules made up from carbon, nitrogen and oxygen (and to a lesser extent, sulfur and
phosphorus) the hybridisation theory/model makes the description much easier. The
hybridisation theory finds its use mainly in organic chemistry. Its explanation starts with the way
bonding is organized in methane. [edit]Types of hybridisation [edit]sp3 hybrids Hybridisation
describes the bonding atoms from an atom\'s point of view. That is, for a tetrahedrally
coordinated carbon (e.g., methane, CH4), the carbon should have 4 orbitals with the correct
symmetry to bond to the 4 hydrogen atoms. The .
INTRODUCTION:
Hybrid Orbitals
Developed by Linus Pauling, the concept of hybrid orbitals was a theory created to explain the structures of molecules in space. The theory consists of combining atomic orbitals (ex: s,p,d,f) into new hybrid orbitals (ex: sp, sp2, sp3).
The electron configuration is the distribution of electrons of an atom or molecule (or other physical structure) in atomic or molecular orbital . For example, the electron configuration of the neon atom is 1s2 2s2 2p6.
Hybridization is the idea that atomic orbitals fuse to form newly hybridized orbitals, which in turn, influences molecular geometry and bonding properties. Hybridization is also an expansion of the valence bond theory.
CONTENTS
INTRODUCTION
CONCEPTS OF WALSH DIAGRAM
APPLICATION IN TRIATOMIC MOLECULES
[IN AH₂ TYPE OF MOLECULES(BeH₂,BH₂,H₂O)]
INTRODUCTION
Arthur Donald Walsh FRS The introducer of walsh diagram (8 August 1916-23 April 1977) was a British chemist, professor of chemistry at the University of Dundee . He was elected FRS in 1964. He was educated at Loughborough Grammar School.
Walsh diagrams were first introduced in a series of ten papers in one issue of the Journal of the Chemical Society . Here, he aimed to rationalize the shapes adopted by polyatomic molecules in the ground state as well as in excited states, by applying theoretical contributions made by Mulliken .
Electron configuration process and steps. It has the explanation of how quantum numbers are arranged in the periodic table, and how they are used to find the electron configuration of elements. A brief explanation of Aufbau rule, Hund's rule and Pauli's Exclusion principle
A chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between atoms with opposite charges, or through the sharing of electrons as in the covalent bonds.
In chemistry, hybridisation (or hybridization) is.pdfsutharbharat59
In chemistry, hybridisation (or hybridization) is the concept of mixing atomic
orbitals to form new hybrid orbitals suitable for the qualitative description of atomic bonding
properties. Hybridised orbitals are very useful in the explanation of the shape of molecular
orbitals for molecules. It is an integral part of valence bond theory. Although sometimes taught
together with the valence shell electron-pair repulsion (VSEPR) theory, valence bond and
hybridization are in fact not related to the VSEPR model.[1] Contents [hide] 1 Historical
development 2 Types of hybridisation 2.1 sp3 hybrids 2.2 sp2 hybrids 2.3 sp hybrids 3
Hybridisation and molecule shape 3.1 Explanation of the shape of water 3.2 Controversy
regarding d-orbital participation 4 Hybridisation theory vs. MO theory 5 See also 6 External
links 7 References [edit]Historical development Chemist Linus Pauling first developed the
hybridisation theory in order to explain the structure of molecules such as methane (CH4).[2]
This concept was developed for such simple chemical systems, but the approach was later
applied more widely, and today it is considered an effective heuristic for rationalizing the
structures of organic compounds. For quantitative calculations of electronic structure and
molecular properties, hybridisation theory is not as practical as molecular orbital theory.
Problems with hybridisation are especially notable when the d orbitals are involved in bonding,
as in coordination chemistry and organometallic chemistry. Although hybridisation schemes in
transition metal chemistry can be used, they are not generally as accurate. Orbitals are a model
representation of the behaviour of electrons within molecules. In the case of simple
hybridisation, this approximation is based on atomic orbitals, similar to those obtained for the
hydrogen atom, the only atom for which an exact analytic solution to its Schrödinger equation is
known. In heavier atoms, like carbon, nitrogen, and oxygen, the atomic orbitals used are the 2s
and 2p orbitals, similar to excited state orbitals for hydrogen. Hybridised orbitals are assumed to
be mixtures of these atomic orbitals, superimposed on each other in various proportions. The
theory of hybridisation is most applicable under these assumptions. It gives a simple orbital
picture equivalent to Lewis structures. Hybridisation is not required to describe molecules, but
for molecules made up from carbon, nitrogen and oxygen (and to a lesser extent, sulfur and
phosphorus) the hybridisation theory/model makes the description much easier. The
hybridisation theory finds its use mainly in organic chemistry. Its explanation starts with the way
bonding is organized in methane. [edit]Types of hybridisation [edit]sp3 hybrids Hybridisation
describes the bonding atoms from an atom\'s point of view. That is, for a tetrahedrally
coordinated carbon (e.g., methane, CH4), the carbon should have 4 orbitals with the correct
symmetry to bond to the 4 hydrogen atoms. The .
INTRODUCTION:
Hybrid Orbitals
Developed by Linus Pauling, the concept of hybrid orbitals was a theory created to explain the structures of molecules in space. The theory consists of combining atomic orbitals (ex: s,p,d,f) into new hybrid orbitals (ex: sp, sp2, sp3).
A chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between atoms with opposite charges, or through the sharing of electrons as in the covalent bonds
OBJECTIVE:
DESCRIBE THE BONDING OF ETHANE, ETHENE (ETHYLENE) AND ETHYNE(ACETYLENE) AND EXPLAIN THEIR GEOMETRY IN TERMS OF HYBRIDIZATION AND σ AND ¶ CARBON-CARBON BONDS.
Hybridization (or hybridization) is the concept of mixing (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electron to form chemical bond is valence bond theory.
An orbital of one atom can combine with that of another atom to form a sigma (σ) or pi (∏) bond.
A sigma bond is covalent bond resulting from the end-to-end overlap of orbitals.
A pi-bond results from the side-to-side overlap of p orbitals along a plane containing a line connecting the nuclei of the atoms
Incineration is the method of choice for treating large volumes of infectious waste, animal carcasses, and contaminated bedding materials. Because incinerators usually are located some distance from the laboratory, additional precautions for handling and packaging of infectious waste are necessary.
Types of Biomedical Waste Disposal
Autoclaving. The process of autoclaving involves steam sterilization. ...
Incineration. The major benefits of incineration are that it is quick, easy, and simple. ...
Chemicals. When it comes to liquid waste, a common biomedical waste disposal method can be chemical disinfection. ...
Microwaving.
Prokaryotes are always unicellular, while eukaryotes are often multi-celled organisms. Additionally, eukaryotic cells are more than 100 to 10,000 times larger than prokaryotic cells and are much more complex. The DNA in eukaryotes is stored within the nucleus, while DNA is stored in the cytoplasm of prokaryotes
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Eukaryotic cells have several other membrane-bound organelles not found in prokaryotic cells.
These include the mitochondria (convert food energy into adenosine triphosphate, or ATP, to power biochemical reactions); rough and smooth endoplasmic reticulum ,golgi complex and in the case of plant cells, chloroplasts
All of these organelles are located in the eukaryotic cell's cytoplasm.
Mycology is the branch of biology concerned with the study of fungi.
The word 'myco' is derived from the Greek word mýkēs meaning “mushroom, fungus”.
Heinrich Anton de Bary is the father of Mycology.
Fungi are eukaryotic organisms that include such as yeasts, moulds and mushrooms. These organisms are classified under kingdom fungi.
Fungi are diverse and widespread.
Fungi metabolism consists on a series of reactions (biochemical reactions) constantly occurring inside the cells to keep it alive and active and in the results biosynthesis of a huge number of compounds.
These compounds area usually divided into primary and secondary metabolites.
Primary metabolism is common to several species and usually produces compounds with the function of assuring fungi growth and development.
Primary metabolites are involved in the growth, development, and reproduction of organisms.
The primary metabolites consist of vitamins, amino acids, nucleosides and organic acids
Staphylococcus aureus is a bacterium that causes staphylococcal food poisoning, a form of gastroenteritis with rapid onset of symptoms. S. aureus is commonly found in the environment (soil, water and air) and is also found in the nose and on the skin of humans.
Communicable diseases are illnesses that spread from one person to another or from an animal to a person, or from a surface or a food. Diseases can be transmitted during air travel through: direct contact with a sick person. respiratory droplet spread from a sick person sneezing or coughing.
Host-Parasite relationship is the extreme case of animal association, in which both partners influence each others life by affecting each others metabolism and behaviour using different adaptive mechanisms in order to ensure their survival.
Bacteria have their own enzymes for
1. Cell wall formation
2. Protein synthesis
3. DNA replication
4. RNA synthesis
5. Synthesis of essential metabolites
Infections spread from animals to human are called zoonotic infections.
The term zoonos is’ Derived from the Greek
ZOON (animals) and NOSES (diseases)
Pathogens shared with wild or domestic animals cause more than 60% of infectious diseases in man.
Ozone (O3) is a molecule made up of three atoms of oxygen (O), and very reactive gas.
Bluish gas that harmful to breathe.
Is mostly found in the stratosphere, where it protects us from the Sun’s harmful ultraviolet (UV) radiation.
Although it represents only a tiny fraction of the atmosphere, ozone is essential for life on Earth.
Ozone in the stratosphere— a layer of the atmosphere between 15 and 50 kilometers (10 and 31 miles) above us—acts as a shield to protect Earth’s surface from the sun’s harmful ultraviolet radiation.
H: Infects only Human beings
I: Immunodeficiency Virus weakness the Immune system and increases the risk of infections
V: Virus that attacks the body and finally kills the body’s immune system
Tuberculosis is a communicable chronic granulomatous disease caused by Mycobacterium tuberculosis , where the center of the granuloma is Caseous necrosis
It usually involves the lungs but may affect any organ or tissue in the body
Airborne spread of droplet nuclei
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Deep Behavioral Phenotyping in Systems Neuroscience for Functional Atlasing a...Ana Luísa Pinho
Functional Magnetic Resonance Imaging (fMRI) provides means to characterize brain activations in response to behavior. However, cognitive neuroscience has been limited to group-level effects referring to the performance of specific tasks. To obtain the functional profile of elementary cognitive mechanisms, the combination of brain responses to many tasks is required. Yet, to date, both structural atlases and parcellation-based activations do not fully account for cognitive function and still present several limitations. Further, they do not adapt overall to individual characteristics. In this talk, I will give an account of deep-behavioral phenotyping strategies, namely data-driven methods in large task-fMRI datasets, to optimize functional brain-data collection and improve inference of effects-of-interest related to mental processes. Key to this approach is the employment of fast multi-functional paradigms rich on features that can be well parametrized and, consequently, facilitate the creation of psycho-physiological constructs to be modelled with imaging data. Particular emphasis will be given to music stimuli when studying high-order cognitive mechanisms, due to their ecological nature and quality to enable complex behavior compounded by discrete entities. I will also discuss how deep-behavioral phenotyping and individualized models applied to neuroimaging data can better account for the subject-specific organization of domain-general cognitive systems in the human brain. Finally, the accumulation of functional brain signatures brings the possibility to clarify relationships among tasks and create a univocal link between brain systems and mental functions through: (1) the development of ontologies proposing an organization of cognitive processes; and (2) brain-network taxonomies describing functional specialization. To this end, tools to improve commensurability in cognitive science are necessary, such as public repositories, ontology-based platforms and automated meta-analysis tools. I will thus discuss some brain-atlasing resources currently under development, and their applicability in cognitive as well as clinical neuroscience.
What is greenhouse gasses and how many gasses are there to affect the Earth.moosaasad1975
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change, and increasing global population, crop yield and quality need to be improved in a sustainable way over the coming decades. Genetic improvement by breeding is the best way to increase crop productivity. With the rapid progression of functional
genomics, an increasing number of crop genomes have been sequenced and dozens of genes influencing key agronomic traits have been identified. However, current genome sequence information has not been adequately exploited for understanding
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20240520 Planning a Circuit Simulator in JavaScript.pptx
Geometry of hybridization
1. 1
Geometry of Hybridization
sp3
Four sp3 orbitals
Hybridization describes the bonding atoms from an atom's point of view. For a tetrahedral
coordinated carbon (e.g. methane CH4), the carbon should have 4 orbitals with the correct
symmetry to bond to the 4 hydrogen atoms.
Carbon's ground state configuration is 1s2 2s2 2p2 or more easily read:
C
↑↓ ↑↓ ↑ ↑
1s 2s 2p 2p 2p
The carbon atom can use its two singly occupied p-type orbitals, to form two covalent
bonds with two hydrogen atoms, yielding the singlet methylene CH2, the simplest carbene. The
carbon atom can also bond to four hydrogen atoms by an excitation (or promotion) of an electron
from the doubly occupied 2s orbital to the empty 2p orbital, producing four singly occupied
orbitals.
C*
↑↓ ↑ ↑ ↑ ↑
1s 2s 2p 2p 2p
The energy released by the formation of two additional bonds more than compensates for the
excitation energy required, energetically favoring the formation of four C-H bonds.
Quantum mechanically, the lowest energy is obtained if the four bonds are equivalent, which
requires that they are formed from equivalent orbitals on the carbon. A set of four equivalent
orbitals can be obtained that are linear combinations of the valence-shell (core orbitals are almost
never involved in bonding) s and p wave functions, which are the four sp3 hybrids.
2. 2
C*
↑↓ ↑ ↑ ↑ ↑
1s sp3 sp3 sp3 sp3
In CH4, four sp3 hybrid orbitals are overlapped by hydrogen 1s orbitals, yielding four σ (sigma)
bonds (that is, four single covalent bonds) of equal length and strength.
sp2
Three sp2 orbitals
Ethene structure
Other carbon compounds and other molecules may be explained in a similar way. For
example, ethene (C2H4) has a double bond between the carbons.
For this molecule, carbon sp2 hybridizes, because one π (pi) bond is required for the double
bond between the carbons and only three σ bonds are formed per carbon atom. In
sp2 hybridization the 2s orbital is mixed with only two of the three available 2p orbitals,
3. 3
C*
↑↓ ↑ ↑ ↑ ↑
1s sp2 sp2 sp2 2p
forming a total of three sp2 orbitals with one remaining p orbital. In ethylene (ethene) the two
carbon atoms form a σ bond by overlapping one sp2 orbital from each carbon atom. The π bond
between the carbon atoms perpendicular to the molecular plane is formed by 2p–2p overlap all
with 120° bond angles. The hydrogen–carbon bonds are all of equal strength and length, in
agreement with experimental data.
sp
Two sp orbitals
The chemical bonding in compounds such as alkynes with triple bonds is explained by sp
hybridization. In this model, the 2s orbital is mixed with only one of the three p orbitals,
C*
↑↓ ↑ ↑ ↑ ↑
1s sp sp 2p 2p
resulting in two sp orbitals and two remaining p orbitals. The chemical bonding
in acetylene (ethyne) (C2H2) consists of sp–sp overlap between the two carbon atoms forming a
σ bond and two additional π bonds formed by p–p overlap. Each carbon also bonds at 180°
angles.