Intermolecular attractions are attractions between one molecule and a neighbouring
molecule. The forces of attraction which hold an individual molecule together (for example, the
covalent bonds) are known as intramolecular attractions. These two words are so confusingly
similar that it is safer to abandon one of them and never use it. The term \"intramolecular\" won\'t
be used again on this site. All molecules experience intermolecular attractions, although in some
cases those attractions are very weak. Even in a gas like hydrogen, H2, if you slow the molecules
down by cooling the gas, the attractions are large enough for the molecules to stick together
eventually to form a liquid and then a solid. In hydrogen\'s case the attractions are so weak that
the molecules have to be cooled to 21 K (-252°C) before the attractions are enough to condense
the hydrogen as a liquid. Helium\'s intermolecular attractions are even weaker - the molecules
won\'t stick together to form a liquid until the temperature drops to 4 K (-269°C). van der Waals
forces: dispersion forces Dispersion forces (one of the two types of van der Waals force we are
dealing with on this page) are also known as \"London forces\" (named after Fritz London who
first suggested how they might arise). The origin of van der Waals dispersion forces Temporary
fluctuating dipoles Attractions are electrical in nature. In a symmetrical molecule like hydrogen,
however, there doesn\'t seem to be any electrical distortion to produce positive or negative parts.
But that\'s only true on average. The lozenge-shaped diagram represents a small symmetrical
molecule - H2, perhaps, or Br2. The even shading shows that on average there is no electrical
distortion. But the electrons are mobile, and at any one instant they might find themselves
towards one end of the molecule, making that end -. The other end will be temporarily short of
electrons and so becomes +. Note: (read as \"delta\") means \"slightly\" - so + means \"slightly
positive\". An instant later the electrons may well have moved up to the other end, reversing
the polarity of the molecule. This constant \"sloshing around\" of the electrons in the molecule
causes rapidly fluctuating dipoles even in the most symmetrical molecule. It even happens in
monatomic molecules - molecules of noble gases, like helium, which consist of a single atom. If
both the helium electrons happen to be on one side of the atom at the same time, the nucleus is
no longer properly covered by electrons for that instant. How temporary dipoles give rise to
intermolecular attractions I\'m going to use the same lozenge-shaped diagram now to represent
any molecule which could, in fact, be a much more complicated shape. Shape does matter (see
below), but keeping the shape simple makes it a lot easier to both draw the diagrams and
understand what is going on. Imagine a molecule which has a temporary polarity being
approached by one which happens to be entirely non-polar just at .
Introduces the concept of covalent bonding with macro-molecules and simple covalent molecules.
Next, it covers inter-molecular attraction but explaining how temporary dipoles form
Finally, heating and cooling curves together with an explanation for how energy is absorbed or given out during boiling or freezing
Applied science./cosmetic dentistry course by Indian dental academyIndian dental academy
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Introduces the concept of covalent bonding with macro-molecules and simple covalent molecules.
Next, it covers inter-molecular attraction but explaining how temporary dipoles form
Finally, heating and cooling curves together with an explanation for how energy is absorbed or given out during boiling or freezing
Applied science./cosmetic dentistry course by Indian dental academyIndian dental academy
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The presentation "Chemical Bonding" is prepared for class IX. It contains a brief introduction to bonding and a detailed study of types of chemical bonds, basically ionic and covalent, along with the characteristics of compounds formed by these bonds.
All constructive comments are welcome.
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structure_of_matter general classes and principles of adhesion.pptAryaKrishnan59
Structure of Matter:
Matter consists of atoms, which are the fundamental building blocks. Here are some key points:
Atoms: These are indivisible and indestructible particles. Each element has identical atoms in terms of mass and properties.
Compounds: Formed by combining different kinds of atoms.
Chemical Reactions: Involve rearrangements of atoms.
Principles of Adhesion in Dentistry:
Adhesion plays a crucial role in dental treatments. It involves the attachment and binding of one substance to another. Here’s what you need to know:
Bonding System Functions:
Resistance to Separation: Prevents the adherend substrate (e.g., enamel, dentin, metal, composite, ceramic) from separating from restorative or cementing materials.
Stress Distribution: Distributes stress along bonded interfaces.
Interface Sealing: Achieved via adhesive bonding between materials1.
Mechanisms of Adhesion:
Chemical Adhesion: Involves molecular or atomic attraction between contacting surfaces.
Mechanical Adhesion: Results from structural interlocking.
Combination: Adhesion can occur through both chemical and mechanical mechanisms23.
Requirements for Good Adhesion:
Wetting: Sufficient wetting of the adhesive.
Low Viscosity: Allows proper flow and penetration.
Surface Texture: Rough surface texture of the adherend.
High Surface Energy: Promotes effective bonding4.
In summary, understanding the structure of matter and principles of adhesion is essential for successful dental procedures
A chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds or substance . 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........
Structure of matter/certified fixed orthodontic courses by Indian dental acad...Indian dental academy
The Indian Dental Academy is the Leader in continuing dental education , training dentists in all aspects of dentistry and offering a wide range of dental certified courses in different formats.
Indian dental academy provides dental crown & Bridge,rotary endodontics,fixed orthodontics,
Dental implants courses.for details pls visit www.indiandentalacademy.com ,or call
0091-9248678078
Structure of matter /certified fixed orthodontic courses by Indian dental aca...Indian dental academy
The Indian Dental Academy is the Leader in continuing dental education , training dentists in all aspects of dentistry and offering a wide range of dental certified courses in different formats.
Indian dental academy provides dental crown & Bridge,rotary endodontics,fixed orthodontics,
Dental implants courses.for details pls visit www.indiandentalacademy.com ,or call
0091-9248678078
Structure of matter /cosmetic dentistry course by Indian dental academyIndian dental academy
Indian Dental Academy: will be one of the most relevant and exciting training center with best faculty and flexible training programs for dental professionals who wish to advance in their dental practice,Offers certified courses in Dental implants,Orthodontics,Endodontics,Cosmetic Dentistry, Prosthetic Dentistry, Periodontics and General Dentistry.
The presentation "Chemical Bonding" is prepared for class IX. It contains a brief introduction to bonding and a detailed study of types of chemical bonds, basically ionic and covalent, along with the characteristics of compounds formed by these bonds.
All constructive comments are welcome.
Structure of matter/cosmetic dentistry course by Indian dental academyIndian dental academy
Indian Dental Academy: will be one of the most relevant and exciting training center with best faculty and flexible training programs for dental professionals who wish to advance in their dental practice,Offers certified courses in Dental implants,Orthodontics,Endodontics,Cosmetic Dentistry, Prosthetic Dentistry, Periodontics and General Dentistry.
structure_of_matter general classes and principles of adhesion.pptAryaKrishnan59
Structure of Matter:
Matter consists of atoms, which are the fundamental building blocks. Here are some key points:
Atoms: These are indivisible and indestructible particles. Each element has identical atoms in terms of mass and properties.
Compounds: Formed by combining different kinds of atoms.
Chemical Reactions: Involve rearrangements of atoms.
Principles of Adhesion in Dentistry:
Adhesion plays a crucial role in dental treatments. It involves the attachment and binding of one substance to another. Here’s what you need to know:
Bonding System Functions:
Resistance to Separation: Prevents the adherend substrate (e.g., enamel, dentin, metal, composite, ceramic) from separating from restorative or cementing materials.
Stress Distribution: Distributes stress along bonded interfaces.
Interface Sealing: Achieved via adhesive bonding between materials1.
Mechanisms of Adhesion:
Chemical Adhesion: Involves molecular or atomic attraction between contacting surfaces.
Mechanical Adhesion: Results from structural interlocking.
Combination: Adhesion can occur through both chemical and mechanical mechanisms23.
Requirements for Good Adhesion:
Wetting: Sufficient wetting of the adhesive.
Low Viscosity: Allows proper flow and penetration.
Surface Texture: Rough surface texture of the adherend.
High Surface Energy: Promotes effective bonding4.
In summary, understanding the structure of matter and principles of adhesion is essential for successful dental procedures
A chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds or substance . 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........
Structure of matter/certified fixed orthodontic courses by Indian dental acad...Indian dental academy
The Indian Dental Academy is the Leader in continuing dental education , training dentists in all aspects of dentistry and offering a wide range of dental certified courses in different formats.
Indian dental academy provides dental crown & Bridge,rotary endodontics,fixed orthodontics,
Dental implants courses.for details pls visit www.indiandentalacademy.com ,or call
0091-9248678078
Structure of matter /certified fixed orthodontic courses by Indian dental aca...Indian dental academy
The Indian Dental Academy is the Leader in continuing dental education , training dentists in all aspects of dentistry and offering a wide range of dental certified courses in different formats.
Indian dental academy provides dental crown & Bridge,rotary endodontics,fixed orthodontics,
Dental implants courses.for details pls visit www.indiandentalacademy.com ,or call
0091-9248678078
Structure of matter /cosmetic dentistry course by Indian dental academyIndian dental academy
Indian Dental Academy: will be one of the most relevant and exciting training center with best faculty and flexible training programs for dental professionals who wish to advance in their dental practice,Offers certified courses in Dental implants,Orthodontics,Endodontics,Cosmetic Dentistry, Prosthetic Dentistry, Periodontics and General Dentistry.
The term Lewis acid refers to a definition of aci.pdfannaelctronics
The term Lewis acid refers to a definition of acid published by Gilbert N. Lewis in
1923, specifically: An acid substance is one which can employ an electron lone pair from another
molecule in completing the stable group of one of its own atoms.[1] Thus, H+ is a Lewis acid,
since it can accept a lone pair, completing its stable form, which requires two electrons. The
modern-day definition of Lewis acid, as given by IUPAC is a molecular entity (and the
corresponding chemical species) that is an electron-pair acceptor and therefore able to react with
a Lewis base to form a Lewis adduct, by sharing the electron pair furnished by the Lewis
base.[2] This definition is both more general and more specific—the electron pair need not be a
lone pair (it could be the pair of electrons in a p bond, for example), but the reaction should give
an adduct (and not just be a displacement reaction). Crystal field theory (CFT) is a model that
describes the breaking of degeneracies of electronic orbital states, usually d or f orbitals, due to a
static electric field produced by a surrounding charge distribution (anion neighbors). This theory
has been used to describe various spectroscopies of transition metal coordination complexes, in
particular optical spectra (colours). CFT successfully accounts for some magnetic properties,
colours, hydration enthalpies, and spinel structures of transition metal complexes, but it does not
attempt to describe bonding. CFT was developed by physicists Hans Bethe and John Hasbrouck
van Vleck[1] in the 1930s. CFT was subsequently combined with molecular orbital theory to
form the more realistic and complex ligand field theory (LFT), which delivers insight into the
process of chemical bonding in transition metal complexes. In chemistry, valence bond (VB)
theory is one of two basic theories, along with molecular orbital (MO) theory, that were
developed to use the methods of quantum mechanics to explain chemical bonding. It focuses on
how the atomic orbitals of the dissociated atoms combine to give individual chemical bonds
when a molecule is formed. In contrast, molecular orbital theory has orbitals that cover the whole
molecule.
Solution
The term Lewis acid refers to a definition of acid published by Gilbert N. Lewis in
1923, specifically: An acid substance is one which can employ an electron lone pair from another
molecule in completing the stable group of one of its own atoms.[1] Thus, H+ is a Lewis acid,
since it can accept a lone pair, completing its stable form, which requires two electrons. The
modern-day definition of Lewis acid, as given by IUPAC is a molecular entity (and the
corresponding chemical species) that is an electron-pair acceptor and therefore able to react with
a Lewis base to form a Lewis adduct, by sharing the electron pair furnished by the Lewis
base.[2] This definition is both more general and more specific—the electron pair need not be a
lone pair (it could be the pair of electrons in a p bond, for example.
MnO2 may act as a catalyst.in the other reaction .pdfannaelctronics
MnO2 may act as a catalyst.in the other reaction of KBrO3 and Sulfuric acid.
ANSWER
Solution
MnO2 may act as a catalyst.in the other reaction of KBrO3 and Sulfuric acid.
ANSWER.
Xenodiagnosis is the method used to document presesnce of a microorg.pdfannaelctronics
Xenodiagnosis is the method used to document presesnce of a microorganism by exposing the
infected tissue to a vector and than examining the vector for the presence of microorganisms.
Uninfected vectors and detection of pathogen DNA in host cell will be required for
xenodiagnosis.
Solution
Xenodiagnosis is the method used to document presesnce of a microorganism by exposing the
infected tissue to a vector and than examining the vector for the presence of microorganisms.
Uninfected vectors and detection of pathogen DNA in host cell will be required for
xenodiagnosis..
There are many more conditions than just the norms of the culture th.pdfannaelctronics
There are many more conditions than just the norms of the culture that affect and assert the
statement
Solution
There are many more conditions than just the norms of the culture that affect and assert the
statement.
The three layers of smooth muscle that includes mucosa. innermost tu.pdfannaelctronics
The three layers of smooth muscle that includes mucosa. innermost tunic of a ureter; formed by
transitional epithelium that is both stretchable and impermeable to the passage of urine; external
to the transitional epithelium is the lamina propria, composed of dense irregular connective tissue
The correct answer is 2
Solution
The three layers of smooth muscle that includes mucosa. innermost tunic of a ureter; formed by
transitional epithelium that is both stretchable and impermeable to the passage of urine; external
to the transitional epithelium is the lamina propria, composed of dense irregular connective tissue
The correct answer is 2.
The independent variable is the one which changes in each plant. Thi.pdfannaelctronics
The independent variable is the one which changes in each plant. This is the concentration of the
salt solution in each case.Based on the independent variable the changes seen give us the
dependent variable. This is the height of the plants. The heights of the plants[dependent variable]
may be influenced by the salt solutions[independent variable].
Solution
The independent variable is the one which changes in each plant. This is the concentration of the
salt solution in each case.Based on the independent variable the changes seen give us the
dependent variable. This is the height of the plants. The heights of the plants[dependent variable]
may be influenced by the salt solutions[independent variable]..
Species diversity is more in near island as rate of immigration is m.pdfannaelctronics
Species diversity is more in near island as rate of immigration is more.
Also it is more in large islands as more resources are available there and rate kf extinction is low.
Solution
Species diversity is more in near island as rate of immigration is more.
Also it is more in large islands as more resources are available there and rate kf extinction is low..
Solution Flies do not have teeth for chewing food.So,like human f.pdfannaelctronics
Solution
:
Flies do not have teeth for chewing food.So,like human flies have some acid in their stomach for
digestion of food.But digestion of food in flies not occur in the stomach.It is occur outside of the
body.Flies vomit acids present in their stomach on solid food and convert it into liquid form.Flies
can intake food in liquid form only.After converting it into liquid form it is consume by the flies..
Program To change this license header, choose License Heade.pdfannaelctronics
Program:
/*
* To change this license header, choose License Headers in Project Properties.
* To change this template file, choose Tools | Templates
* and open the template in the editor.
*/
package chegg;
// A Java program for Dijkstra\'s single source shortest path algorithm.
// The program is for adjacency matrix representation of the graph
import java.util.*;
import java.lang.*;
import java.io.*;
class DijkstraAlgorithem
{
// A utility function to find the vertex with minimum distance value,
// from the set of vertices not yet included in shortest path tree
static final int V=6;
int minDistance(int dist[], Boolean sptSet[])
{
// Initialize min value
int min = Integer.MAX_VALUE, min_index=-1;
for (int v = 0; v < V; v++)
if (sptSet[v] == false && dist[v] <= min)
{
min = dist[v];
min_index = v;
}
return min_index;
}
// A utility function to print the constructed distance array
void print
Solution
(int dist[], int n,int src)
{
System.out.println( \" Here Infinite=\"+Integer.MAX_VALUE);
System.out.println(\" Source Vertex:\"+(src+1));
System.out.println(\"Vertex Distance from Source\");
for (int i = 0; i < V; i++)
System.out.println((i+1)+\" \\t\\t \"+dist[i]);
}
// Funtion that implements Dijkstra\'s single source shortest path
// algorithm for a graph represented using adjacency matrix
// representation
void dijkstra(int graph[][], int src)
{
int dist[] = new int[V]; // The output array. dist[i] will hold
// the shortest distance from src to i
// sptSet[i] will true if vertex i is included in shortest
// path tree or shortest distance from src to i is finalized
Boolean sptSet[] = new Boolean[V];
// Initialize all distances as INFINITE and stpSet[] as false
for (int i = 0; i < V; i++)
{
dist[i] = Integer.MAX_VALUE;
sptSet[i] = false;
}
// Distance of source vertex from itself is always 0
dist[src] = 0;
// Find shortest path for all vertices
for (int count = 0; count < V-1; count++)
{
// Pick the minimum distance vertex from the set of vertices
// not yet processed. u is always equal to src in first
// iteration.
int u = minDistance(dist, sptSet);
// Mark the picked vertex as processed
sptSet[u] = true;
// Update dist value of the adjacent vertices of the
// picked vertex.
for (int v = 0; v < V; v++)
// Update dist[v] only if is not in sptSet, there is an
// edge from u to v, and total weight of path from src to
// v through u is smaller than current value of dist[v]
if (!sptSet[v] && graph[u][v]!=0 &&
dist[u] != Integer.MAX_VALUE &&
dist[u]+graph[u][v] < dist[v])
dist[v] = dist[u] + graph[u][v];
}
// print the constructed distance array
print.
plexusFormed from anterioe rani o these spinal nervesMajor nerve.pdfannaelctronics
plexus
Formed from anterioe rani o these spinal nerves
Major nerves formed from the plexus
Cervical
The cervical plexus is a plexus of the front rami of the initial four cervical spinal nerves which
are situated from C1 to C4 cervical fragment in the neck.
They are found along the side to the transverse procedures between prevertebral muscles from
the average side and vertebral (m. scalenus, m. levator scapulae, m. splenius cervicis) from
horizontal side. There is anastomosis with extra nerve, hypoglossal nerve and thoughtful trun
The cervical plexus has two sorts of branches: cutaneous and strong.
Cutaneous (4 branches):
Incredible auricular nerve - innervates skin close concha auricle (external ear) and outer acoustic
meatus (ear waterway) (C2&C3)
Transverse cervical nerve - innervates front locale of neck (C2&C3)
Lesser occipital - innervates the skin and the scalp posterosuperior to the auricle (C2)
Supraclavicular nerves - innervate the skin above and underneath the clavicle (C3,C4)
Muscular:
Ansa cervicalis (circle framed from C1-C3), and so forth (geniohyoid (C1 just), thyrohyoid (C1
just), sternothyroid, sternohyoid, omohyoid)
Phrenic (C3-C5 (fundamentally C4))- innervates stomach and the pericardium
Segmental branches (C1-C4)- innervates front and center scalenes
Brachial
The brachial plexus is a system of nerves shaped by the foremost rami of the lower four cervical
nerves and first thoracic nerve (C5, C6, C7, C8, and T1). This plexus stretches out from the
spinal line, through the cervicoaxillary trench in the neck, over the primary rib, and into the
armpit. It supplies afferent and efferent nerve strands to the mid-section, shoulder, arm and hand.
The Brachial Plexus
1 Roots.
2 Trunks.
3 Divisions.
4 Cords.
5 Major Branches. 5.1 Musculocutaneous Nerve. 5.2 Axillary Nerve. 5.3 Median Nerve. 5.4
Radial Nerve. 5.5 Ulnar Nerve. 5.6 Practical Relevance: Dissecting the Brachial Plexus.
6 Minor Branches.
lumbosacral
The anterior divisions of the lumbar nerves, sacral nerves, and coccygeal nerve form the
lumbosacral plexus, the first lumbar nerve being frequently joined by a branch from the twelfth
thoracic. For descriptive purposes this plexus is usually divided into three parts:
lumbar plexus
sacral plexus
pudendal plexus
lumbar plexus
sacral plexus
pudendal plexus
plexus
Formed from anterioe rani o these spinal nerves
Major nerves formed from the plexus
Cervical
The cervical plexus is a plexus of the front rami of the initial four cervical spinal nerves which
are situated from C1 to C4 cervical fragment in the neck.
They are found along the side to the transverse procedures between prevertebral muscles from
the average side and vertebral (m. scalenus, m. levator scapulae, m. splenius cervicis) from
horizontal side. There is anastomosis with extra nerve, hypoglossal nerve and thoughtful trun
The cervical plexus has two sorts of branches: cutaneous and strong.
Cutaneous (4 branches):
Incredible auricular nerve - innervates skin close con.
Ok, so the number of double bond equivalents in the compound is [C4H.pdfannaelctronics
Ok, so the number of double bond equivalents in the compound is [C4H10)-(C4H8)]/2 = 1 DBE
1) IR
so the large trough from 3400cm-1 to 2400cm-1 as well as the peak at ~1700cm-1 indicates an
acid. That accounts for 1 carbon, both oxygens, and one hydrogen. That also accounts for the one
double bond equivalent.
That leaves 3 carbons and 7 hydrogens.
2) NMR
Methyl groups usually give proton peaks around 0.9ppm and shift further downfield when
adding electron withdrawing groups nearby. It\'s a pretty good guess that the triplet at ~1.1ppm is
a methyl group. The fact that it\'s a triplet indicates the carbon next to it has two protons attached
to it.
That gives a CH3-CH2- (as well as the -COOH group)
all that\'s left now is one carbon and two hydrogens (CH2)
Looking at the other two proton peaks in the nmr ... there\'s one triplet and one sextet.
The triplet would be a CH2 group that is next to another CH2 group (and not anything else), so it
must be a CH2 next to the COOH
Now you would have two pieces:
CH3-CH2- and -CH2-COOH
put them together and check the coupling of the protons...
you should end up with two triplets (proton split by two others), one sextet (proton split by 5
others), and a small peak somewhere around 9-13ppm. (that\'s the peak indicated by the offset of
2.0ppm on the spectrum)
So the structure would be:
CH3-CH2-CH2-COOH (C4H8O2)
Solution
Ok, so the number of double bond equivalents in the compound is [C4H10)-(C4H8)]/2 = 1 DBE
1) IR
so the large trough from 3400cm-1 to 2400cm-1 as well as the peak at ~1700cm-1 indicates an
acid. That accounts for 1 carbon, both oxygens, and one hydrogen. That also accounts for the one
double bond equivalent.
That leaves 3 carbons and 7 hydrogens.
2) NMR
Methyl groups usually give proton peaks around 0.9ppm and shift further downfield when
adding electron withdrawing groups nearby. It\'s a pretty good guess that the triplet at ~1.1ppm is
a methyl group. The fact that it\'s a triplet indicates the carbon next to it has two protons attached
to it.
That gives a CH3-CH2- (as well as the -COOH group)
all that\'s left now is one carbon and two hydrogens (CH2)
Looking at the other two proton peaks in the nmr ... there\'s one triplet and one sextet.
The triplet would be a CH2 group that is next to another CH2 group (and not anything else), so it
must be a CH2 next to the COOH
Now you would have two pieces:
CH3-CH2- and -CH2-COOH
put them together and check the coupling of the protons...
you should end up with two triplets (proton split by two others), one sextet (proton split by 5
others), and a small peak somewhere around 9-13ppm. (that\'s the peak indicated by the offset of
2.0ppm on the spectrum)
So the structure would be:
CH3-CH2-CH2-COOH (C4H8O2).
order of overlap of atomic orbitals from highest extent of overlap t.pdfannaelctronics
order of overlap of atomic orbitals from highest extent of overlap to lowest is,
I2 > IBr > ICl > IF
Because,
I2-is homo diatomic molecule and having good overlapping between the atomic orbitals of two
iodine atoms.
IBr-is a hetero di-atomic molecule and having almost good overlapping between the atomic
orbitals of iodine and bromine atoms even though these two atoms belongs to different periods.
ICl-is a hetero di-atomic molecule and having moderate overlapping between the atomic orbitals
of iodine and chlorine atoms.Because, these two atoms belongs to different periods and size
different is more.
IF-is a hetero di-atomic molecule and having poor overlapping between the atomic orbitals of
iodine and fluorine atoms.Because, these two atoms belongs to different periods and size
different is too more.
Solution
order of overlap of atomic orbitals from highest extent of overlap to lowest is,
I2 > IBr > ICl > IF
Because,
I2-is homo diatomic molecule and having good overlapping between the atomic orbitals of two
iodine atoms.
IBr-is a hetero di-atomic molecule and having almost good overlapping between the atomic
orbitals of iodine and bromine atoms even though these two atoms belongs to different periods.
ICl-is a hetero di-atomic molecule and having moderate overlapping between the atomic orbitals
of iodine and chlorine atoms.Because, these two atoms belongs to different periods and size
different is more.
IF-is a hetero di-atomic molecule and having poor overlapping between the atomic orbitals of
iodine and fluorine atoms.Because, these two atoms belongs to different periods and size
different is too more..
Read| The latest issue of The Challenger is here! We are thrilled to announce that our school paper has qualified for the NATIONAL SCHOOLS PRESS CONFERENCE (NSPC) 2024. Thank you for your unwavering support and trust. Dive into the stories that made us stand out!
Welcome to TechSoup New Member Orientation and Q&A (May 2024).pdfTechSoup
In this webinar you will learn how your organization can access TechSoup's wide variety of product discount and donation programs. From hardware to software, we'll give you a tour of the tools available to help your nonprofit with productivity, collaboration, financial management, donor tracking, security, and more.
Synthetic Fiber Construction in lab .pptxPavel ( NSTU)
Synthetic fiber production is a fascinating and complex field that blends chemistry, engineering, and environmental science. By understanding these aspects, students can gain a comprehensive view of synthetic fiber production, its impact on society and the environment, and the potential for future innovations. Synthetic fibers play a crucial role in modern society, impacting various aspects of daily life, industry, and the environment. ynthetic fibers are integral to modern life, offering a range of benefits from cost-effectiveness and versatility to innovative applications and performance characteristics. While they pose environmental challenges, ongoing research and development aim to create more sustainable and eco-friendly alternatives. Understanding the importance of synthetic fibers helps in appreciating their role in the economy, industry, and daily life, while also emphasizing the need for sustainable practices and innovation.
June 3, 2024 Anti-Semitism Letter Sent to MIT President Kornbluth and MIT Cor...Levi Shapiro
Letter from the Congress of the United States regarding Anti-Semitism sent June 3rd to MIT President Sally Kornbluth, MIT Corp Chair, Mark Gorenberg
Dear Dr. Kornbluth and Mr. Gorenberg,
The US House of Representatives is deeply concerned by ongoing and pervasive acts of antisemitic
harassment and intimidation at the Massachusetts Institute of Technology (MIT). Failing to act decisively to ensure a safe learning environment for all students would be a grave dereliction of your responsibilities as President of MIT and Chair of the MIT Corporation.
This Congress will not stand idly by and allow an environment hostile to Jewish students to persist. The House believes that your institution is in violation of Title VI of the Civil Rights Act, and the inability or
unwillingness to rectify this violation through action requires accountability.
Postsecondary education is a unique opportunity for students to learn and have their ideas and beliefs challenged. However, universities receiving hundreds of millions of federal funds annually have denied
students that opportunity and have been hijacked to become venues for the promotion of terrorism, antisemitic harassment and intimidation, unlawful encampments, and in some cases, assaults and riots.
The House of Representatives will not countenance the use of federal funds to indoctrinate students into hateful, antisemitic, anti-American supporters of terrorism. Investigations into campus antisemitism by the Committee on Education and the Workforce and the Committee on Ways and Means have been expanded into a Congress-wide probe across all relevant jurisdictions to address this national crisis. The undersigned Committees will conduct oversight into the use of federal funds at MIT and its learning environment under authorities granted to each Committee.
• The Committee on Education and the Workforce has been investigating your institution since December 7, 2023. The Committee has broad jurisdiction over postsecondary education, including its compliance with Title VI of the Civil Rights Act, campus safety concerns over disruptions to the learning environment, and the awarding of federal student aid under the Higher Education Act.
• The Committee on Oversight and Accountability is investigating the sources of funding and other support flowing to groups espousing pro-Hamas propaganda and engaged in antisemitic harassment and intimidation of students. The Committee on Oversight and Accountability is the principal oversight committee of the US House of Representatives and has broad authority to investigate “any matter” at “any time” under House Rule X.
• The Committee on Ways and Means has been investigating several universities since November 15, 2023, when the Committee held a hearing entitled From Ivory Towers to Dark Corners: Investigating the Nexus Between Antisemitism, Tax-Exempt Universities, and Terror Financing. The Committee followed the hearing with letters to those institutions on January 10, 202
2024.06.01 Introducing a competency framework for languag learning materials ...Sandy Millin
http://sandymillin.wordpress.com/iateflwebinar2024
Published classroom materials form the basis of syllabuses, drive teacher professional development, and have a potentially huge influence on learners, teachers and education systems. All teachers also create their own materials, whether a few sentences on a blackboard, a highly-structured fully-realised online course, or anything in between. Despite this, the knowledge and skills needed to create effective language learning materials are rarely part of teacher training, and are mostly learnt by trial and error.
Knowledge and skills frameworks, generally called competency frameworks, for ELT teachers, trainers and managers have existed for a few years now. However, until I created one for my MA dissertation, there wasn’t one drawing together what we need to know and do to be able to effectively produce language learning materials.
This webinar will introduce you to my framework, highlighting the key competencies I identified from my research. It will also show how anybody involved in language teaching (any language, not just English!), teacher training, managing schools or developing language learning materials can benefit from using the framework.
Biological screening of herbal drugs: Introduction and Need for
Phyto-Pharmacological Screening, New Strategies for evaluating
Natural Products, In vitro evaluation techniques for Antioxidants, Antimicrobial and Anticancer drugs. In vivo evaluation techniques
for Anti-inflammatory, Antiulcer, Anticancer, Wound healing, Antidiabetic, Hepatoprotective, Cardio protective, Diuretics and
Antifertility, Toxicity studies as per OECD guidelines
Introduction to AI for Nonprofits with Tapp NetworkTechSoup
Dive into the world of AI! Experts Jon Hill and Tareq Monaur will guide you through AI's role in enhancing nonprofit websites and basic marketing strategies, making it easy to understand and apply.
TESDA TM1 REVIEWER FOR NATIONAL ASSESSMENT WRITTEN AND ORAL QUESTIONS WITH A...
Intermolecular attractions are attractions betwee.pdf
1. Intermolecular attractions are attractions between one molecule and a neighbouring
molecule. The forces of attraction which hold an individual molecule together (for example, the
covalent bonds) are known as intramolecular attractions. These two words are so confusingly
similar that it is safer to abandon one of them and never use it. The term "intramolecular" won't
be used again on this site. All molecules experience intermolecular attractions, although in some
cases those attractions are very weak. Even in a gas like hydrogen, H2, if you slow the molecules
down by cooling the gas, the attractions are large enough for the molecules to stick together
eventually to form a liquid and then a solid. In hydrogen's case the attractions are so weak that
the molecules have to be cooled to 21 K (-252°C) before the attractions are enough to condense
the hydrogen as a liquid. Helium's intermolecular attractions are even weaker - the molecules
won't stick together to form a liquid until the temperature drops to 4 K (-269°C). van der Waals
forces: dispersion forces Dispersion forces (one of the two types of van der Waals force we are
dealing with on this page) are also known as "London forces" (named after Fritz London who
first suggested how they might arise). The origin of van der Waals dispersion forces Temporary
fluctuating dipoles Attractions are electrical in nature. In a symmetrical molecule like hydrogen,
however, there doesn't seem to be any electrical distortion to produce positive or negative parts.
But that's only true on average. The lozenge-shaped diagram represents a small symmetrical
molecule - H2, perhaps, or Br2. The even shading shows that on average there is no electrical
distortion. But the electrons are mobile, and at any one instant they might find themselves
towards one end of the molecule, making that end -. The other end will be temporarily short of
electrons and so becomes +. Note: (read as "delta") means "slightly" - so + means "slightly
positive". An instant later the electrons may well have moved up to the other end, reversing
the polarity of the molecule. This constant "sloshing around" of the electrons in the molecule
causes rapidly fluctuating dipoles even in the most symmetrical molecule. It even happens in
monatomic molecules - molecules of noble gases, like helium, which consist of a single atom. If
both the helium electrons happen to be on one side of the atom at the same time, the nucleus is
no longer properly covered by electrons for that instant. How temporary dipoles give rise to
intermolecular attractions I'm going to use the same lozenge-shaped diagram now to represent
any molecule which could, in fact, be a much more complicated shape. Shape does matter (see
below), but keeping the shape simple makes it a lot easier to both draw the diagrams and
understand what is going on. Imagine a molecule which has a temporary polarity being
approached by one which happens to be entirely non-polar just at that moment. (A pretty
unlikely event, but it makes the diagrams much easier to draw! In reality, one of the molecules is
likely to have a greater polarity than the other at that time - and so will be the dominant one.)
As the right hand molecule approaches, its electrons will tend to be attracted by the slightly
positive end of the left hand one. This sets up an induced dipole in the approaching molecule,
2. which is orientated in such a way that the + end of one is attracted to the - end of the other. An
instant later the electrons in the left hand molecule may well have moved up the other end. In
doing so, they will repel the electrons in the right hand one. The polarity of both molecules
reverses, but you still have + attracting -. As long as the molecules stay close to each other the
polarities will continue to fluctuate in synchronisation so that the attraction is always maintained.
There is no reason why this has to be restricted to two molecules. As long as the molecules are
close together this synchronised movement of the electrons can occur over huge numbers of
molecules. This diagram shows how a whole lattice of molecules could be held together in a
solid using van der Waals dispersion forces. An instant later, of course, you would have to draw
a quite different arrangement of the distribution of the electrons as they shifted around - but
always in synchronisation. The strength of dispersion forces Dispersion forces between
molecules are much weaker than the covalent bonds within molecules. It isn't possible to give
any exact value, because the size of the attraction varies considerably with the size of the
molecule and its shape. How molecular size affects the strength of the dispersion forces The
boiling points of the noble gases are helium -269°C neon -246°C argon -186°C krypton -152°C
xenon -108°C radon -62°C All of these elements have monatomic molecules. The reason that
the boiling points increase as you go down the group is that the number of electrons increases,
and so also does the radius of the atom. The more electrons you have, and the more distance over
which they can move, the bigger the possible temporary dipoles and therefore the bigger the
dispersion forces. Because of the greater temporary dipoles, xenon molecules are "stickier"
than neon molecules. Neon molecules will break away from each other at much lower
temperatures than xenon molecules - hence neon has the lower boiling point. This is the reason
that (all other things being equal) bigger molecules have higher boiling points than small ones.
Bigger molecules have more electrons and more distance over which temporary dipoles can
develop - and so the bigger molecules are "stickier". How molecular shape affects the strength
of the dispersion forces The shapes of the molecules also matter. Long thin molecules can
develop bigger temporary dipoles due to electron movement than short fat ones containing the
same numbers of electrons. Long thin molecules can also lie closer together - these attractions
are at their most effective if the molecules are really close. For example, the hydrocarbon
molecules butane and 2-methylpropane both have a molecular formula C4H10, but the atoms are
arranged differently. In butane the carbon atoms are arranged in a single chain, but 2-
methylpropane is a shorter chain with a branch. Butane has a higher boiling point because the
dispersion forces are greater. The molecules are longer (and so set up bigger temporary dipoles)
and can lie closer together than the shorter, fatter 2-methylpropane molecules.
Solution
3. Intermolecular attractions are attractions between one molecule and a neighbouring
molecule. The forces of attraction which hold an individual molecule together (for example, the
covalent bonds) are known as intramolecular attractions. These two words are so confusingly
similar that it is safer to abandon one of them and never use it. The term "intramolecular" won't
be used again on this site. All molecules experience intermolecular attractions, although in some
cases those attractions are very weak. Even in a gas like hydrogen, H2, if you slow the molecules
down by cooling the gas, the attractions are large enough for the molecules to stick together
eventually to form a liquid and then a solid. In hydrogen's case the attractions are so weak that
the molecules have to be cooled to 21 K (-252°C) before the attractions are enough to condense
the hydrogen as a liquid. Helium's intermolecular attractions are even weaker - the molecules
won't stick together to form a liquid until the temperature drops to 4 K (-269°C). van der Waals
forces: dispersion forces Dispersion forces (one of the two types of van der Waals force we are
dealing with on this page) are also known as "London forces" (named after Fritz London who
first suggested how they might arise). The origin of van der Waals dispersion forces Temporary
fluctuating dipoles Attractions are electrical in nature. In a symmetrical molecule like hydrogen,
however, there doesn't seem to be any electrical distortion to produce positive or negative parts.
But that's only true on average. The lozenge-shaped diagram represents a small symmetrical
molecule - H2, perhaps, or Br2. The even shading shows that on average there is no electrical
distortion. But the electrons are mobile, and at any one instant they might find themselves
towards one end of the molecule, making that end -. The other end will be temporarily short of
electrons and so becomes +. Note: (read as "delta") means "slightly" - so + means "slightly
positive". An instant later the electrons may well have moved up to the other end, reversing
the polarity of the molecule. This constant "sloshing around" of the electrons in the molecule
causes rapidly fluctuating dipoles even in the most symmetrical molecule. It even happens in
monatomic molecules - molecules of noble gases, like helium, which consist of a single atom. If
both the helium electrons happen to be on one side of the atom at the same time, the nucleus is
no longer properly covered by electrons for that instant. How temporary dipoles give rise to
intermolecular attractions I'm going to use the same lozenge-shaped diagram now to represent
any molecule which could, in fact, be a much more complicated shape. Shape does matter (see
below), but keeping the shape simple makes it a lot easier to both draw the diagrams and
understand what is going on. Imagine a molecule which has a temporary polarity being
approached by one which happens to be entirely non-polar just at that moment. (A pretty
unlikely event, but it makes the diagrams much easier to draw! In reality, one of the molecules is
likely to have a greater polarity than the other at that time - and so will be the dominant one.)
As the right hand molecule approaches, its electrons will tend to be attracted by the slightly
positive end of the left hand one. This sets up an induced dipole in the approaching molecule,
4. which is orientated in such a way that the + end of one is attracted to the - end of the other. An
instant later the electrons in the left hand molecule may well have moved up the other end. In
doing so, they will repel the electrons in the right hand one. The polarity of both molecules
reverses, but you still have + attracting -. As long as the molecules stay close to each other the
polarities will continue to fluctuate in synchronisation so that the attraction is always maintained.
There is no reason why this has to be restricted to two molecules. As long as the molecules are
close together this synchronised movement of the electrons can occur over huge numbers of
molecules. This diagram shows how a whole lattice of molecules could be held together in a
solid using van der Waals dispersion forces. An instant later, of course, you would have to draw
a quite different arrangement of the distribution of the electrons as they shifted around - but
always in synchronisation. The strength of dispersion forces Dispersion forces between
molecules are much weaker than the covalent bonds within molecules. It isn't possible to give
any exact value, because the size of the attraction varies considerably with the size of the
molecule and its shape. How molecular size affects the strength of the dispersion forces The
boiling points of the noble gases are helium -269°C neon -246°C argon -186°C krypton -152°C
xenon -108°C radon -62°C All of these elements have monatomic molecules. The reason that
the boiling points increase as you go down the group is that the number of electrons increases,
and so also does the radius of the atom. The more electrons you have, and the more distance over
which they can move, the bigger the possible temporary dipoles and therefore the bigger the
dispersion forces. Because of the greater temporary dipoles, xenon molecules are "stickier"
than neon molecules. Neon molecules will break away from each other at much lower
temperatures than xenon molecules - hence neon has the lower boiling point. This is the reason
that (all other things being equal) bigger molecules have higher boiling points than small ones.
Bigger molecules have more electrons and more distance over which temporary dipoles can
develop - and so the bigger molecules are "stickier". How molecular shape affects the strength
of the dispersion forces The shapes of the molecules also matter. Long thin molecules can
develop bigger temporary dipoles due to electron movement than short fat ones containing the
same numbers of electrons. Long thin molecules can also lie closer together - these attractions
are at their most effective if the molecules are really close. For example, the hydrocarbon
molecules butane and 2-methylpropane both have a molecular formula C4H10, but the atoms are
arranged differently. In butane the carbon atoms are arranged in a single chain, but 2-
methylpropane is a shorter chain with a branch. Butane has a higher boiling point because the
dispersion forces are greater. The molecules are longer (and so set up bigger temporary dipoles)
and can lie closer together than the shorter, fatter 2-methylpropane molecules.