Lewis Diagram
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Lewis diagrams are a representation of molecules that shows valence electron positions and bonds. They are drawn by determining total valence electrons, writing the skeleton structure and subtracting electrons used in bonds, then distributing remaining electrons so each atom has a full valence shell. The document provides instructions on drawing Lewis diagrams, examples to practice, and explains their importance in showing resonance structures and bond differences between molecules with the same atoms. It also includes additional resources for help.
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2. Elements in the same column are members of the same group and have similar chemical properties.
3. Elements that have many similar properties belong to the same group.
4. As you move from left to right and from top to bottom on the periodic table, the atomic mass of elements generally increases.
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This document provides information about Lewis diagrams and how to draw them. It explains that Lewis diagrams show valence electrons and how atoms bond in molecules. It gives examples of how to draw Lewis diagrams for molecules such as H2, O2, N2, H2O, and SO3. The steps involve counting valence electrons, identifying the central atom, drawing single bonds, adding lone electron pairs, and forming additional bonds to achieve full octets at each atom.
Hello! Please see the correction below! False Hydrogen atoms ar.pdf
Hello! Please see the correction below!
False: Hydrogen atoms are often the central atom of a lewis structure. (This doesn\'t make sense
since hydrogen can only form 1 bond!)
True: For a neutral molecule, the number of electrons in the Lewis structure is the sum of the
valence electrons for the atoms.
FALSE: Each atom of a Lewis structure must have eight electrons. (This is the \"octet rule.)
Typically you would have each atom with eight electrons, but as your hint indicated, Hydrogen
only gets 2 electrons. This exception would make this statement false.
True: Electrons of covalent compounds may be shared between atoms.
Sorry about that - Hope this helps! Please rate if it does : )
Solution
Hello! Please see the correction below!
False: Hydrogen atoms are often the central atom of a lewis structure. (This doesn\'t make sense
since hydrogen can only form 1 bond!)
True: For a neutral molecule, the number of electrons in the Lewis structure is the sum of the
valence electrons for the atoms.
FALSE: Each atom of a Lewis structure must have eight electrons. (This is the \"octet rule.)
Typically you would have each atom with eight electrons, but as your hint indicated, Hydrogen
only gets 2 electrons. This exception would make this statement false.
True: Electrons of covalent compounds may be shared between atoms.
Sorry about that - Hope this helps! Please rate if it does : ).
Lewis Structures
The document discusses Lewis structures and the rules for drawing them. It explains that Lewis structures show how atoms bond via shared electron pairs to achieve stable noble gas configurations. It provides a 4-step process for drawing Lewis structures, covering counting electrons, identifying the central atom, adding lone pairs to complete octets, and checking that all electrons are accounted for. Exceptions to the octet rule and drawing structures for ions are also covered.
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Chapter 6.2 : Covalent Bonding and Molecular Compounds
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1. The document provides an overview of key concepts for Lewis structures and VSEPR theory, including how to draw Lewis structures for covalent compounds and ions.
2. It explains valence shell electron pair repulsion theory (VSEPR) which is used to predict the 3D shape of molecules based on electron pairs around a central atom.
3. A table is included that lists common molecular geometries determined by VSEPR theory based on the number of electron regions around the central atom.
Lesson 8Chemical Bonding & NomenclatureYou should view all.docx
Lesson 8
Chemical Bonding & Nomenclature
You should view all lectures as a slide show. In the toolbar above, click “Slide Show” and “From Beginning” to start. Hit the space bar to forward to next slide or item.
1
*Read: Watch the Lecture as a slideshow, hit the space bar to move forward or just left click.
1
Topics:
Chemical Bonds
Lewis Dot Structures
Molecular Geometry
Polar Bonds
Naming Compounds
Writing Chemical Formulas
Naming Molecular Compounds
Lesson 8: Chemical Bonding and Nomenclature
2
2
Chemical Bonds
Sodium (Na) is a silver-colored metal that reacts so
violently with water that flames are produced when sodium
gets wet.
Chlorine (Cl) is a greenish-colored gas that is so poisonous that it was used as a weapon in World War I.
When the electrons of sodium metal and chlorine gas interact, the compound sodium chloride (NaCl) is formed, which is table salt.
Since the body is over 90% water, ingesting sodium metal would literally set someone on fire!
If we make a compound out of Na, we can make something totally different such as the table salt used to season our food.
3
Chemical Bonds
Atoms can interact with each other to form new substances called
compounds.
Compounds are formed when electrons in an atom’s last energy level interact and form chemical bonds. A chemical bond is an attractive force between atoms that holds them together.
An atom’s outermost energy level of electrons is called the valence shell (or valence level) and the electrons in the valence shell are called valence electrons.
4
Na Atom
Cl Atom
Sodium has 1 valence electron in the valence shell.
Chlorine has 7 valence electron in the valence shell.
Chemical Bonds
In ionic bonds, metals always lose electrons to nonmetals and become positive (or cations).
In ionic bonds, nonmetals always attract electrons from metals and become negative (anions).
Ionic compounds are neutral compounds made up of cations and anions.
Covalent bonds are formed between nonmetals and electrons are shared so no ions are formed.
Cl
nonmetal
Na
metal
O
nonmetal
O
nonmetal
Metal + Nonmetal = Ionic Compound
Nonmetal + Nonmetal = Covalent Compound
Chemical Bonds: Ionic
The octet rule states that atoms will gain, lose, or share
valence electrons in a way that will give each atom eight electrons in their valence shell.
Na has 1 electron in its valence shell and Cl has 7 electrons in its valence shell. Cl needs 1 valence electron to have 8 in its outer shell.
If Na transfers its 1 valence electron to Cl, Na’s second energy level becomes the valence shell, which already has 8 electrons.
Now, Na has a positive 1 charge and Cl has a negative 1 charge. But, the charge on NaCl is zero (the charges cancel each other out).
6
Na Atom
Cl Atom
Ionic Bond
Chemical Bonds: Ionic
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The document provides an overview of chemical bonding principles including ionic bonding, covalent bonding, and molecular geometry. It discusses how atoms interact to achieve stable electronic configurations through ionic bonding by exchanging electrons or covalent bonding by sharing electrons. Lewis structures are introduced as a way to represent valence electrons in molecules and determine molecular geometry and polarity based on electron pair arrangements around central atoms. Key concepts covered include octet rule, electronegativity, bond polarity, and using Lewis structures to systematically determine molecular structure characteristics.
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The document discusses Lewis structures and covalent bonding. It provides steps for writing Lewis structures, including determining the molecular formula and connectivity, counting valence electrons, connecting atoms with bonds, adding electron pairs, checking for octets, and calculating formal charges. Constitutional isomers are described as isomers that differ in the order atoms are connected. Resonance structures are also discussed, where multiple Lewis structures can be written that differ in electron positions but have the same atomic positions.
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Lewis symbols and the octet rule are used to represent valence electrons and chemical bonding. Lewis symbols show valence electrons as dots around the element symbol. The octet rule states that atoms bond to gain, lose, or share electrons to achieve an octet of 8 valence electrons. Exceptions include odd total electron molecules, molecules where atoms have less than an octet, and hypervalent molecules where the central atom has more than 8 electrons.
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chemical bonding
Atoms form bonds to attain a lower potential energy state. They do this through ionic bonds, where oppositely charged ions attract, or covalent bonds, where atoms share valence electrons. Whether a bond is ionic or covalent depends on the electronegativity difference between the atoms. Ionic bonds form between metals and nonmetals, while covalent bonds form between two nonmetals. Lewis structures use dots to represent valence electrons and show how atoms share electrons to achieve stable configurations like noble gases. Valence shell electron pair repulsion theory explains molecular shapes based on electron pair positioning.
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The document discusses Lewis dot structures and how they are used to represent valence electrons in atoms and molecules. It provides examples of writing Lewis dot structures according to the octet rule, which states that atoms are most stable when their valence shells are filled with eight electrons. It also discusses how covalent bonds are formed by the sharing of valence electrons between atoms to achieve stable octet configurations. Key points covered include how to draw Lewis dot structures, count valence electrons, and distribute electrons to atoms following the octet rule.
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This document provides information about Lewis diagrams and how to draw them. It explains that Lewis diagrams show valence electrons and how atoms bond in molecules. It gives examples of how to draw Lewis diagrams for molecules such as H2, O2, N2, H2O, and SO3. The steps involve counting valence electrons, identifying the central atom, drawing single bonds, adding lone electron pairs, and forming additional bonds to achieve full octets at each atom.
Hello! Please see the correction below! False Hydrogen atoms ar.pdf
Hello! Please see the correction below!
False: Hydrogen atoms are often the central atom of a lewis structure. (This doesn\'t make sense
since hydrogen can only form 1 bond!)
True: For a neutral molecule, the number of electrons in the Lewis structure is the sum of the
valence electrons for the atoms.
FALSE: Each atom of a Lewis structure must have eight electrons. (This is the \"octet rule.)
Typically you would have each atom with eight electrons, but as your hint indicated, Hydrogen
only gets 2 electrons. This exception would make this statement false.
True: Electrons of covalent compounds may be shared between atoms.
Sorry about that - Hope this helps! Please rate if it does : )
Solution
Hello! Please see the correction below!
False: Hydrogen atoms are often the central atom of a lewis structure. (This doesn\'t make sense
since hydrogen can only form 1 bond!)
True: For a neutral molecule, the number of electrons in the Lewis structure is the sum of the
valence electrons for the atoms.
FALSE: Each atom of a Lewis structure must have eight electrons. (This is the \"octet rule.)
Typically you would have each atom with eight electrons, but as your hint indicated, Hydrogen
only gets 2 electrons. This exception would make this statement false.
True: Electrons of covalent compounds may be shared between atoms.
Sorry about that - Hope this helps! Please rate if it does : ).
Lewis Structures
The document discusses Lewis structures and the rules for drawing them. It explains that Lewis structures show how atoms bond via shared electron pairs to achieve stable noble gas configurations. It provides a 4-step process for drawing Lewis structures, covering counting electrons, identifying the central atom, adding lone pairs to complete octets, and checking that all electrons are accounted for. Exceptions to the octet rule and drawing structures for ions are also covered.
Lewis dot structures
Lewis dot structures are a way to represent covalent bonding between atoms using dots to represent valence electrons. Atoms form bonds by sharing electrons in order to achieve stable electron configurations like the octet rule. Multiple bonds can form when more than one pair of electrons is shared between two atoms. Sometimes bonds form with both electrons coming from the same atom. Drawing accurate Lewis structures involves counting valence electrons and placing them between atoms to represent shared pairs and complete octets following the rules of covalent bonding. Resonance structures can occur when more than one valid Lewis structure exists for the same molecule.
Chapter 6.2 : Covalent Bonding and Molecular Compounds
Covalent bonding occurs when atoms share valence electrons to achieve stable electron configurations. Molecules are formed when atoms bond covalently, with molecular formulas indicating the types and numbers of atoms. Lewis structures represent molecules by showing bonding pairs and unshared electron pairs. Exceptions to the octet rule include hydrogen and boron. Resonance structures are used to depict molecules that cannot be represented by a single Lewis structure.
Lesson 1 molecular structure for s video.pptx
This document discusses chemical bonding and Lewis dot structures. It begins by listing the objectives of describing chemical bonding, representing atoms with Lewis diagrams, and applying rules to deduce bond formation. It then defines chemical bonds as electrostatic attractions between atoms that share electrons. It discusses valence and core electrons and uses oxygen as an example. It introduces Lewis structures and represents oxygen and sulfur. It explains how covalent bonds form between hydrogen atoms and represents this with an energy diagram. It provides examples of Lewis structures for various elements and molecules such as HCl, H2O, O2, and HCN. It also discusses lone pairs and coordinate covalent bonds. Finally, it provides examples and questions to solidify the concepts.
Lewis structuresvsepr theory cheat sheet
1. The document provides an overview of key concepts for Lewis structures and VSEPR theory, including how to draw Lewis structures for covalent compounds and ions.
2. It explains valence shell electron pair repulsion theory (VSEPR) which is used to predict the 3D shape of molecules based on electron pairs around a central atom.
3. A table is included that lists common molecular geometries determined by VSEPR theory based on the number of electron regions around the central atom.
Lesson 8Chemical Bonding & NomenclatureYou should view all.docx
Lesson 8
Chemical Bonding & Nomenclature
You should view all lectures as a slide show. In the toolbar above, click “Slide Show” and “From Beginning” to start. Hit the space bar to forward to next slide or item.
1
*Read: Watch the Lecture as a slideshow, hit the space bar to move forward or just left click.
1
Topics:
Chemical Bonds
Lewis Dot Structures
Molecular Geometry
Polar Bonds
Naming Compounds
Writing Chemical Formulas
Naming Molecular Compounds
Lesson 8: Chemical Bonding and Nomenclature
2
2
Chemical Bonds
Sodium (Na) is a silver-colored metal that reacts so
violently with water that flames are produced when sodium
gets wet.
Chlorine (Cl) is a greenish-colored gas that is so poisonous that it was used as a weapon in World War I.
When the electrons of sodium metal and chlorine gas interact, the compound sodium chloride (NaCl) is formed, which is table salt.
Since the body is over 90% water, ingesting sodium metal would literally set someone on fire!
If we make a compound out of Na, we can make something totally different such as the table salt used to season our food.
3
Chemical Bonds
Atoms can interact with each other to form new substances called
compounds.
Compounds are formed when electrons in an atom’s last energy level interact and form chemical bonds. A chemical bond is an attractive force between atoms that holds them together.
An atom’s outermost energy level of electrons is called the valence shell (or valence level) and the electrons in the valence shell are called valence electrons.
4
Na Atom
Cl Atom
Sodium has 1 valence electron in the valence shell.
Chlorine has 7 valence electron in the valence shell.
Chemical Bonds
In ionic bonds, metals always lose electrons to nonmetals and become positive (or cations).
In ionic bonds, nonmetals always attract electrons from metals and become negative (anions).
Ionic compounds are neutral compounds made up of cations and anions.
Covalent bonds are formed between nonmetals and electrons are shared so no ions are formed.
Cl
nonmetal
Na
metal
O
nonmetal
O
nonmetal
Metal + Nonmetal = Ionic Compound
Nonmetal + Nonmetal = Covalent Compound
Chemical Bonds: Ionic
The octet rule states that atoms will gain, lose, or share
valence electrons in a way that will give each atom eight electrons in their valence shell.
Na has 1 electron in its valence shell and Cl has 7 electrons in its valence shell. Cl needs 1 valence electron to have 8 in its outer shell.
If Na transfers its 1 valence electron to Cl, Na’s second energy level becomes the valence shell, which already has 8 electrons.
Now, Na has a positive 1 charge and Cl has a negative 1 charge. But, the charge on NaCl is zero (the charges cancel each other out).
6
Na Atom
Cl Atom
Ionic Bond
Chemical Bonds: Ionic
An Ionic bond is formed when there is a transfer of electrons from a metal to a nonmetal. Compounds formed by ionic bonds are ...
Chemical Bonding
The document provides an overview of chemical bonding principles including ionic bonding, covalent bonding, and molecular geometry. It discusses how atoms interact to achieve stable electronic configurations through ionic bonding by exchanging electrons or covalent bonding by sharing electrons. Lewis structures are introduced as a way to represent valence electrons in molecules and determine molecular geometry and polarity based on electron pair arrangements around central atoms. Key concepts covered include octet rule, electronegativity, bond polarity, and using Lewis structures to systematically determine molecular structure characteristics.
Representing Compounds: The Progression in Lewis Structures
Slides pertaining to the progression in thinking for developing Lewis Structures, Ohio Learning Standard C.PM.4: Representing Compounds.
....Ch3_CovalentBonding_Lect5 - Copy.ppt
The document discusses Lewis structures and covalent bonding. It provides steps for writing Lewis structures, including determining the molecular formula and connectivity, counting valence electrons, connecting atoms with bonds, adding electron pairs, checking for octets, and calculating formal charges. Constitutional isomers are described as isomers that differ in the order atoms are connected. Resonance structures are also discussed, where multiple Lewis structures can be written that differ in electron positions but have the same atomic positions.
Chemical bonding sk0023
Lewis symbols and the octet rule are used to represent valence electrons and chemical bonding. Lewis symbols show valence electrons as dots around the element symbol. The octet rule states that atoms bond to gain, lose, or share electrons to achieve an octet of 8 valence electrons. Exceptions include odd total electron molecules, molecules where atoms have less than an octet, and hypervalent molecules where the central atom has more than 8 electrons.
Chemisty structure of atoms.....
The document discusses the structure and bonding of atoms and molecules. It begins by describing the components of an atom, including protons, neutrons, and electrons. It then discusses the periodic table and how elements in the same row or column have similar properties. The document goes on to describe atomic orbitals like s and p orbitals. It also discusses how elements bond, including ionic and covalent bonding. Additional topics covered include Lewis structures, resonance structures, molecular geometry, and organic naming conventions.
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chemical bonding
Atoms form bonds to attain a lower potential energy state. They do this through ionic bonds, where oppositely charged ions attract, or covalent bonds, where atoms share valence electrons. Whether a bond is ionic or covalent depends on the electronegativity difference between the atoms. Ionic bonds form between metals and nonmetals, while covalent bonds form between two nonmetals. Lewis structures use dots to represent valence electrons and show how atoms share electrons to achieve stable configurations like noble gases. Valence shell electron pair repulsion theory explains molecular shapes based on electron pair positioning.
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Recently uploaded
Evidence of Jet Activity from the Secondary Black Hole in the OJ 287 Binary S...
Wereport the study of a huge optical intraday flare on 2021 November 12 at 2 a.m. UT in the blazar OJ287. In the binary black hole model, it is associated with an impact of the secondary black hole on the accretion disk of the primary. Our multifrequency observing campaign was set up to search for such a signature of the impact based on a prediction made 8 yr earlier. The first I-band results of the flare have already been reported by Kishore et al. (2024). Here we combine these data with our monitoring in the R-band. There is a big change in the R–I spectral index by 1.0 ±0.1 between the normal background and the flare, suggesting a new component of radiation. The polarization variation during the rise of the flare suggests the same. The limits on the source size place it most reasonably in the jet of the secondary BH. We then ask why we have not seen this phenomenon before. We show that OJ287 was never before observed with sufficient sensitivity on the night when the flare should have happened according to the binary model. We also study the probability that this flare is just an oversized example of intraday variability using the Krakow data set of intense monitoring between 2015 and 2023. We find that the occurrence of a flare of this size and rapidity is unlikely. In machine-readable Tables 1 and 2, we give the full orbit-linked historical light curve of OJ287 as well as the dense monitoring sample of Krakow.
Alternate Wetting and Drying - Climate Smart Agriculture
Alternate Wetting and Drying - Climate Smart AgricultureInternational Food Policy Research Institute- South Asia Office
PPT on Alternate Wetting and Drying presented at the three-day 'Training and Validation Workshop on Modules of Climate Smart Agriculture (CSA) Technologies in South Asia' workshop on April 22, 2024. Compexometric titration/Chelatorphy titration/chelating titration
Classification
Metal ion ion indicators
Masking and demasking reagents
Estimation of Magnisium sulphate
Calcium gluconate
Complexometric Titration/ chelatometry titration/chelating titration, introduction, Types-
1.Direct Titration
2.Back Titration
3.Replacement Titration
4.Indirect Titration
Masking agent, Demasking agents
formation of complex
comparition between masking and demasking agents,
Indicators/Metal ion indicators/ Metallochromic indicators/pM indicators,
Visual Technique,PM indicators (metallochromic), Indicators of pH, Redox Indicators
Instrumental Techniques-Photometry
Potentiometry
Miscellaneous methods.
Complex titration with EDTA.
Direct Seeded Rice - Climate Smart Agriculture
Direct Seeded Rice - Climate Smart AgricultureInternational Food Policy Research Institute- South Asia Office
PPT on Direct Seeded Rice presented at the three-day 'Training and Validation Workshop on Modules of Climate Smart Agriculture (CSA) Technologies in South Asia' workshop on April 22, 2024.
Applied Science: Thermodynamics, Laws & Methodology.pdf
When I was asked to give a companion lecture in support of ‘The Philosophy of Science’ (https://shorturl.at/4pUXz) I decided not to walk through the detail of the many methodologies in order of use. Instead, I chose to employ a long standing, and ongoing, scientific development as an exemplar. And so, I chose the ever evolving story of Thermodynamics as a scientific investigation at its best.
Conducted over a period of >200 years, Thermodynamics R&D, and application, benefitted from the highest levels of professionalism, collaboration, and technical thoroughness. New layers of application, methodology, and practice were made possible by the progressive advance of technology. In turn, this has seen measurement and modelling accuracy continually improved at a micro and macro level.
Perhaps most importantly, Thermodynamics rapidly became a primary tool in the advance of applied science/engineering/technology, spanning micro-tech, to aerospace and cosmology. I can think of no better a story to illustrate the breadth of scientific methodologies and applications at their best.
The debris of the ‘last major merger’ is dynamically young
The Milky Way’s (MW) inner stellar halo contains an [Fe/H]-rich component with highly eccentric orbits, often referred to as the
‘last major merger.’ Hypotheses for the origin of this component include Gaia-Sausage/Enceladus (GSE), where the progenitor
collided with the MW proto-disc 8–11 Gyr ago, and the Virgo Radial Merger (VRM), where the progenitor collided with the
MW disc within the last 3 Gyr. These two scenarios make different predictions about observable structure in local phase space,
because the morphology of debris depends on how long it has had to phase mix. The recently identified phase-space folds in Gaia
DR3 have positive caustic velocities, making them fundamentally different than the phase-mixed chevrons found in simulations
at late times. Roughly 20 per cent of the stars in the prograde local stellar halo are associated with the observed caustics. Based
on a simple phase-mixing model, the observed number of caustics are consistent with a merger that occurred 1–2 Gyr ago.
We also compare the observed phase-space distribution to FIRE-2 Latte simulations of GSE-like mergers, using a quantitative
measurement of phase mixing (2D causticality). The observed local phase-space distribution best matches the simulated data
1–2 Gyr after collision, and certainly not later than 3 Gyr. This is further evidence that the progenitor of the ‘last major merger’
did not collide with the MW proto-disc at early times, as is thought for the GSE, but instead collided with the MW disc within
the last few Gyr, consistent with the body of work surrounding the VRM.
Methods of grain storage Structures in India.pdf
•Post-harvestlossesaccountforabout10%oftotalfoodgrainsduetounscientificstorage,insects,rodents,micro-organismsetc.,
•Totalfoodgrainproductioninindiais311milliontonnesandstorageis145mt.InIndia,annualstoragelosseshavebeenestimated14mtworthofRs.7,000croreinwhichinsectsaloneaccountfornearlyRs.1,300crores.
•InIndiaoutofthetotalproduction,about30%ismarketablesurplus
•Remaining70%isretainedandstoredbyfarmersforconsumption,seed,feed.Hence,growerneedstoragefacilitytoholdaportionofproducetosellwhenthemarketingpriceisfavourable
•TradersandCo-operativesatmarketcentresneedstoragestructurestoholdgrainswhenthetransportfacilityisinadequate
The binding of cosmological structures by massless topological defects
Assuming spherical symmetry and weak field, it is shown that if one solves the Poisson equation or the Einstein field
equations sourced by a topological defect, i.e. a singularity of a very specific form, the result is a localized gravitational
field capable of driving flat rotation (i.e. Keplerian circular orbits at a constant speed for all radii) of test masses on a thin
spherical shell without any underlying mass. Moreover, a large-scale structure which exploits this solution by assembling
concentrically a number of such topological defects can establish a flat stellar or galactic rotation curve, and can also deflect
light in the same manner as an equipotential (isothermal) sphere. Thus, the need for dark matter or modified gravity theory is
mitigated, at least in part.
Randomised Optimisation Algorithms in DAPHNE
Slides from talk:
Aleš Zamuda: Randomised Optimisation Algorithms in DAPHNE .
Austrian-Slovenian HPC Meeting 2024 – ASHPC24, Seeblickhotel Grundlsee in Austria, 10–13 June 2024
https://ashpc.eu/
Summary Of transcription and Translation.pdf
Hello Everyone Here We are Sharing You with The process of protien Synthesis in very short points you will be Able to understand It Very well
MICROBIAL INTERACTION PPT/ MICROBIAL INTERACTION AND THEIR TYPES // PLANT MIC...
MICROBIAL INTERACTION PPT/ MICROBIAL INTERACTION AND THEIR TYPES // PLANT MIC...ABHISHEK SONI NIMT INSTITUTE OF MEDICAL AND PARAMEDCIAL SCIENCES , GOVT PG COLLEGE NOIDA
Microbial interaction
Microorganisms interacts with each other and can be physically associated with another organisms in a variety of ways.
One organism can be located on the surface of another organism as an ectobiont or located within another organism as endobiont.
Microbial interaction may be positive such as mutualism, proto-cooperation, commensalism or may be negative such as parasitism, predation or competition
Types of microbial interaction
Positive interaction: mutualism, proto-cooperation, commensalism
Negative interaction: Ammensalism (antagonism), parasitism, predation, competition
I. Mutualism:
It is defined as the relationship in which each organism in interaction gets benefits from association. It is an obligatory relationship in which mutualist and host are metabolically dependent on each other.
Mutualistic relationship is very specific where one member of association cannot be replaced by another species.
Mutualism require close physical contact between interacting organisms.
Relationship of mutualism allows organisms to exist in habitat that could not occupied by either species alone.
Mutualistic relationship between organisms allows them to act as a single organism.
Examples of mutualism:
i. Lichens:
Lichens are excellent example of mutualism.
They are the association of specific fungi and certain genus of algae. In lichen, fungal partner is called mycobiont and algal partner is called
II. Syntrophism:
It is an association in which the growth of one organism either depends on or improved by the substrate provided by another organism.
In syntrophism both organism in association gets benefits.
Compound A
Utilized by population 1
Compound B
Utilized by population 2
Compound C
utilized by both Population 1+2
Products
In this theoretical example of syntrophism, population 1 is able to utilize and metabolize compound A, forming compound B but cannot metabolize beyond compound B without co-operation of population 2. Population 2is unable to utilize compound A but it can metabolize compound B forming compound C. Then both population 1 and 2 are able to carry out metabolic reaction which leads to formation of end product that neither population could produce alone.
Examples of syntrophism:
i. Methanogenic ecosystem in sludge digester
Methane produced by methanogenic bacteria depends upon interspecies hydrogen transfer by other fermentative bacteria.
Anaerobic fermentative bacteria generate CO2 and H2 utilizing carbohydrates which is then utilized by methanogenic bacteria (Methanobacter) to produce methane.
ii. Lactobacillus arobinosus and Enterococcus faecalis:
In the minimal media, Lactobacillus arobinosus and Enterococcus faecalis are able to grow together but not alone.
The synergistic relationship between E. faecalis and L. arobinosus occurs in which E. faecalis require folic acid
HUMAN EYE By-R.M Class 10 phy best digital notes.pdf
Class 10 human eye notes physics
Handwritten best quality
Pests of Storage_Identification_Dr.UPR.pdf
InIndia-post-harvestlosses-unscientificstorage,insects,rodents,micro-organismsetc.,accountforabout10percentoftotalfoodgrains
Graininfestation
Directdamage
Indirectly
•theexuviae,skin,deadinsects
•theirexcretawhichmakefoodunfitforhumanconsumption
About600speciesofinsectshavebeenassociatedwithstoredgrainproducts
100speciesofinsectpestsofstoredproductscauseeconomiclosses
CLASS 12th CHEMISTRY SOLID STATE ppt (Animated)
Description:
Dive into the fascinating realm of solid-state physics with our meticulously crafted online PowerPoint presentation. This immersive educational resource offers a comprehensive exploration of the fundamental concepts, theories, and applications within the realm of solid-state physics.
From crystalline structures to semiconductor devices, this presentation delves into the intricate principles governing the behavior of solids, providing clear explanations and illustrative examples to enhance understanding. Whether you're a student delving into the subject for the first time or a seasoned researcher seeking to deepen your knowledge, our presentation offers valuable insights and in-depth analyses to cater to various levels of expertise.
Key topics covered include:
Crystal Structures: Unravel the mysteries of crystalline arrangements and their significance in determining material properties.
Band Theory: Explore the electronic band structure of solids and understand how it influences their conductive properties.
Semiconductor Physics: Delve into the behavior of semiconductors, including doping, carrier transport, and device applications.
Magnetic Properties: Investigate the magnetic behavior of solids, including ferromagnetism, antiferromagnetism, and ferrimagnetism.
Optical Properties: Examine the interaction of light with solids, including absorption, reflection, and transmission phenomena.
With visually engaging slides, informative content, and interactive elements, our online PowerPoint presentation serves as a valuable resource for students, educators, and enthusiasts alike, facilitating a deeper understanding of the captivating world of solid-state physics. Explore the intricacies of solid-state materials and unlock the secrets behind their remarkable properties with our comprehensive presentation.
JAMES WEBB STUDY THE MASSIVE BLACK HOLE SEEDS
The pathway(s) to seeding the massive black holes (MBHs) that exist at the heart of galaxies in the present and distant Universe remains an unsolved problem. Here we categorise, describe and quantitatively discuss the formation pathways of both light and heavy seeds. We emphasise that the most recent computational models suggest that rather than a bimodal-like mass spectrum between light and heavy seeds with light at one end and heavy at the other that instead a continuum exists. Light seeds being more ubiquitous and the heavier seeds becoming less and less abundant due the rarer environmental conditions required for their formation. We therefore examine the different mechanisms that give rise to different seed mass spectrums. We show how and why the mechanisms that produce the heaviest seeds are also among the rarest events in the Universe and are hence extremely unlikely to be the seeds for the vast majority of the MBH population. We quantify, within the limits of the current large uncertainties in the seeding processes, the expected number densities of the seed mass spectrum. We argue that light seeds must be at least 103 to 105 times more numerous than heavy seeds to explain the MBH population as a whole. Based on our current understanding of the seed population this makes heavy seeds (Mseed > 103 M⊙) a significantly more likely pathway given that heavy seeds have an abundance pattern than is close to and likely in excess of 10−4 compared to light seeds. Finally, we examine the current state-of-the-art in numerical calculations and recent observations and plot a path forward for near-future advances in both domains.
Recently uploaded (20)
Evidence of Jet Activity from the Secondary Black Hole in the OJ 287 Binary S...
Evidence of Jet Activity from the Secondary Black Hole in the OJ 287 Binary S...
Alternate Wetting and Drying - Climate Smart Agriculture
Alternate Wetting and Drying - Climate Smart Agriculture
Compexometric titration/Chelatorphy titration/chelating titration
Compexometric titration/Chelatorphy titration/chelating titration
Applied Science: Thermodynamics, Laws & Methodology.pdf
Applied Science: Thermodynamics, Laws & Methodology.pdf
GBSN - Biochemistry (Unit 6) Chemistry of Proteins
GBSN - Biochemistry (Unit 6) Chemistry of Proteins
The debris of the ‘last major merger’ is dynamically young
The debris of the ‘last major merger’ is dynamically young
The binding of cosmological structures by massless topological defects
The binding of cosmological structures by massless topological defects
MICROBIAL INTERACTION PPT/ MICROBIAL INTERACTION AND THEIR TYPES // PLANT MIC...
MICROBIAL INTERACTION PPT/ MICROBIAL INTERACTION AND THEIR TYPES // PLANT MIC...
HUMAN EYE By-R.M Class 10 phy best digital notes.pdf
HUMAN EYE By-R.M Class 10 phy best digital notes.pdf
Microbiology of Central Nervous System INFECTIONS.pdf
Microbiology of Central Nervous System INFECTIONS.pdf
Juaristi, Jon. - El canon espanol. El legado de la cultura española a la civi...
Juaristi, Jon. - El canon espanol. El legado de la cultura española a la civi...
Lewis Diagram
- 1. Lewis Diagrams By: Alex and Etta A3
- 2. Table of Contents What are Lewis Diagrams? Try Some Problems Importance of Lewis Diagrams For more help
- 3. What are Lewis Diagrams? A Lewis diagram is a representation of a molecule where dots are used to show the valance electron* position around the atoms and lines or dot pairs represent covalent bonds between atoms. Our goal is to get to 8 VE surrounding the element because 8VE is stable. Hydrogen is different, it only needs 2VE to be stable. *Valance Electrons? Valence electrons (VE) are the electrons in the outer shell of an atom. The valence electrons are the ones involved in forming bonds to adjacent atoms. Table of Contents
- 4. How to draw them? Solve for H2O, Water. Step 1. Determine the total numbers of valance electrons. Look at the periodic table for help. H has 1 valance electron, and C has 6 valance electrons.
- 5. Step 2. Write the skeleton structure of the molecule and subtract the VE’s you use.
- 6. Step 3. Distribute the remaining valance electrons to the elements as non-bonding electrons so that each have 8 valance electrons, excluding Hydrogen (Hydrogen can only have 2).
- 7. Try Some Problems Try to solve these problems your self: 1. CH4 2. NH3 3. CO2 4. CH4 Click to see Answers Table of Contents
- 8. Answers This is what your answers should look like: 1. 2. 3. 4. 2. Table of Contents Back
- 9. Importance of Lewis Diagrams Resonance Structures These resonance structures demonstrate the importance of Lewis Diagrams. They show the differences in the bonds of molecules with the same atoms. NO3 - --> Table of Contents
- 10. For More Help Links that may help: Wikipedia Chemed Lewisdots Schodor Sources: Video: https://www.youtube.com/watch?v=MWDL5WCZBzE Table of Contents