Dispersion forces (answer)Explanation - Dispersion forces have.pdf
•
0 likes•0 views
Dispersion forces (answer) Explanation - Dispersion forces have many different names: London forces, Van der Waals forces, instantaneous dipoles. Dispersion forces involve the attraction between temporarily induced dipoles in nonpolar molecules (often disappear within an instant). This polarization can be induced either by a polar molecule or by the repulsion of negatively charged electron clouds in nonpolar molecules. As electrons move around their shells, electron density may randomly be distributed unevenly, creating a partially negative (?-) charge. The opposite side of the molecule then becomes partially positive (?+). The result is a temporary dipole. If this process occurs in two molecules that are close to one another, the two molecules will be attracted to each other, and will form a temporary, non-covalent bond. Solution Dispersion forces (answer) Explanation - Dispersion forces have many different names: London forces, Van der Waals forces, instantaneous dipoles. Dispersion forces involve the attraction between temporarily induced dipoles in nonpolar molecules (often disappear within an instant). This polarization can be induced either by a polar molecule or by the repulsion of negatively charged electron clouds in nonpolar molecules. As electrons move around their shells, electron density may randomly be distributed unevenly, creating a partially negative (?-) charge. The opposite side of the molecule then becomes partially positive (?+). The result is a temporary dipole. If this process occurs in two molecules that are close to one another, the two molecules will be attracted to each other, and will form a temporary, non-covalent bond..
Report
Share
Report
Share
Download to read offline
Recommended
INTERMOLECULAR FORCES. Physical Science pptx
This document discusses intermolecular forces (IMFs), which are the forces of attraction or repulsion between molecules. It describes three main types of IMFs: van der Waals forces, ion-dipole interactions, and hydrogen bonding. Van der Waals forces include dipole-dipole interactions, dipole-induced dipole interactions, and dispersion forces. Ion-dipole interactions occur between ions and polar molecules. Hydrogen bonding is a strong type of dipole-dipole interaction between hydrogen and electronegative atoms like nitrogen, oxygen, or fluorine. The document also compares the relative strengths of different IMFs and provides examples of substances that demonstrate each type of interaction.
Lesson 2 Intermolecular Forces.pptx
This document defines and differentiates the main types of intermolecular forces: dipole-dipole forces, London dispersion forces, ion-dipole forces, and hydrogen bonding. It provides examples of polar and nonpolar molecules, and describes the characteristics of each type of intermolecular force, including their relative strengths and the molecules between which they typically occur.
IMK 209 presentation
The document discusses the main forces that affect colloidal systems, including van der Waals attractive forces and electrostatic repulsive forces. It introduces the DLVO theory, which states that the total interaction energy between colloidal particles or surfaces is the sum of attractive van der Waals forces and repulsive double layer interactions. An electrical double layer exists around each particle due to its surface charge, consisting of counterions strongly bound in the Stern layer and less firmly in the diffuse layer. The zeta potential is the potential difference between the dispersion medium and the slipping plane boundary of the electrical double layer. It indicates the stability of a colloid, with higher zeta potentials leading to greater electrostatic repulsion and a more stable dispersion
06 intermolecular forces
The document discusses the different types of intermolecular forces:
1) London dispersion forces involve temporary dipoles induced in molecules by fluctuating electron densities.
2) Induced-dipole forces involve a permanent dipole inducing a temporary dipole in a neighboring non-polar molecule.
3) Dipole-dipole attraction occurs between polar molecules due to the attraction between their partial charges.
4) Hydrogen bonds are very strong dipole-dipole bonds that exist between molecules with oxygen, nitrogen, or fluorine bonded to hydrogen.
Binding forces SB
States of Matter, Intermolecular forces, Van der Waals Forces, Keesom, Diapole-Diapole interaction, Debye forces, London forces, Hydrogen bond
Chem 2 - Intermolecular Forces & Phases of Matter II
1) There are several types of intermolecular forces ranging from strongest to weakest - hydrogen bonding, dipole-dipole interactions, dipole-induced dipole interactions, and dispersion forces.
2) Hydrogen bonding is the strongest and involves the electrostatic attraction between a hydrogen atom covalently bonded to a highly electronegative atom like N, O, or F, and another electronegative atom's lone pair of electrons.
3) Dipole-dipole interactions occur between polar molecules that have partially positive and negative ends that electrostatically attract each other, while dipole-induced dipole interactions involve a polar molecule inducing a dipole in a neighboring nonpolar molecule.
Intermolecular attractions are attractions betwee.pdf
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 .
Stabilization of emulsion via electrostatic
This document discusses the stabilization of emulsions via electrostatic forces. It defines emulsions as dispersions of one liquid in another immiscible liquid, and describes the electrical double layer that forms around dispersed droplets consisting of surface charges and layers of counterions. The document outlines DLVO theory, which states that emulsion stability is determined by a balance between attractive van der Waals forces and repulsive electrostatic forces. It also discusses how zeta potential measurement relates to stability, and how pH and ionic strength can affect zeta potential and thus the stability of emulsions.
Recommended
INTERMOLECULAR FORCES. Physical Science pptx
This document discusses intermolecular forces (IMFs), which are the forces of attraction or repulsion between molecules. It describes three main types of IMFs: van der Waals forces, ion-dipole interactions, and hydrogen bonding. Van der Waals forces include dipole-dipole interactions, dipole-induced dipole interactions, and dispersion forces. Ion-dipole interactions occur between ions and polar molecules. Hydrogen bonding is a strong type of dipole-dipole interaction between hydrogen and electronegative atoms like nitrogen, oxygen, or fluorine. The document also compares the relative strengths of different IMFs and provides examples of substances that demonstrate each type of interaction.
Lesson 2 Intermolecular Forces.pptx
This document defines and differentiates the main types of intermolecular forces: dipole-dipole forces, London dispersion forces, ion-dipole forces, and hydrogen bonding. It provides examples of polar and nonpolar molecules, and describes the characteristics of each type of intermolecular force, including their relative strengths and the molecules between which they typically occur.
IMK 209 presentation
The document discusses the main forces that affect colloidal systems, including van der Waals attractive forces and electrostatic repulsive forces. It introduces the DLVO theory, which states that the total interaction energy between colloidal particles or surfaces is the sum of attractive van der Waals forces and repulsive double layer interactions. An electrical double layer exists around each particle due to its surface charge, consisting of counterions strongly bound in the Stern layer and less firmly in the diffuse layer. The zeta potential is the potential difference between the dispersion medium and the slipping plane boundary of the electrical double layer. It indicates the stability of a colloid, with higher zeta potentials leading to greater electrostatic repulsion and a more stable dispersion
06 intermolecular forces
The document discusses the different types of intermolecular forces:
1) London dispersion forces involve temporary dipoles induced in molecules by fluctuating electron densities.
2) Induced-dipole forces involve a permanent dipole inducing a temporary dipole in a neighboring non-polar molecule.
3) Dipole-dipole attraction occurs between polar molecules due to the attraction between their partial charges.
4) Hydrogen bonds are very strong dipole-dipole bonds that exist between molecules with oxygen, nitrogen, or fluorine bonded to hydrogen.
Binding forces SB
States of Matter, Intermolecular forces, Van der Waals Forces, Keesom, Diapole-Diapole interaction, Debye forces, London forces, Hydrogen bond
Chem 2 - Intermolecular Forces & Phases of Matter II
1) There are several types of intermolecular forces ranging from strongest to weakest - hydrogen bonding, dipole-dipole interactions, dipole-induced dipole interactions, and dispersion forces.
2) Hydrogen bonding is the strongest and involves the electrostatic attraction between a hydrogen atom covalently bonded to a highly electronegative atom like N, O, or F, and another electronegative atom's lone pair of electrons.
3) Dipole-dipole interactions occur between polar molecules that have partially positive and negative ends that electrostatically attract each other, while dipole-induced dipole interactions involve a polar molecule inducing a dipole in a neighboring nonpolar molecule.
Intermolecular attractions are attractions betwee.pdf
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 .
Stabilization of emulsion via electrostatic
This document discusses the stabilization of emulsions via electrostatic forces. It defines emulsions as dispersions of one liquid in another immiscible liquid, and describes the electrical double layer that forms around dispersed droplets consisting of surface charges and layers of counterions. The document outlines DLVO theory, which states that emulsion stability is determined by a balance between attractive van der Waals forces and repulsive electrostatic forces. It also discusses how zeta potential measurement relates to stability, and how pH and ionic strength can affect zeta potential and thus the stability of emulsions.
Stabilization of emulsion via electrostatic
This document discusses the stabilization of emulsions via electrostatic forces. It defines emulsions as dispersions of one liquid in another immiscible liquid, and describes the electrical double layer that forms around dispersed droplets consisting of surface charges and layers of counterions. The document outlines DLVO theory, which states that emulsion stability is determined by a balance of attractive van der Waals forces and repulsive electrostatic forces. It also discusses how zeta potential measurement relates to stability, and how pH and ionic strength can affect zeta potential and thus the stability of emulsions.
Dipole-dipole forces are attractive forces between the positive end .pdf
Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the
negative end of another polar molecule.
London force, or Van der Waals force, are temporary fluctuationg dipoles
Hydrogen bonding is the attractive interaction of a hydrogen atom with an electronegative atom
(usually nitrogen, oxygen or fluorine). Seeing any of those three atoms usually gives away the
fact that it\'s hydrogen bonding and probably makes it the most easily noticeable type of
bonding.
Hope that helps!
Solution
Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the
negative end of another polar molecule.
London force, or Van der Waals force, are temporary fluctuationg dipoles
Hydrogen bonding is the attractive interaction of a hydrogen atom with an electronegative atom
(usually nitrogen, oxygen or fluorine). Seeing any of those three atoms usually gives away the
fact that it\'s hydrogen bonding and probably makes it the most easily noticeable type of
bonding.
Hope that helps!.
Intermolecular Forces of attraction
This document discusses different types of intermolecular forces: dipole-dipole forces between polar molecules, ion-dipole forces between ions and polar molecules, dispersion forces between all molecules due to induced dipoles, and strong hydrogen bonds between partial charges on hydrogen and electronegative atoms like N, O, F. These intermolecular forces are responsible for determining the properties and phase of substances.
The strongest attractive forces between molecules of O_2 are ionic .pdf
The strongest attractive forces between molecules of O_2 are: ionic covalent hydrogen
bonding dipole-dipole attractions dispersion forces
Solution
The attractive forces between molecules of O2 will be dispersion forces. This is because O2 is a
non-polar molecule so there will be no dipole-dipole interactions, also there is no hydrogen atom
so no question of Hydrogen bonding. Dispersion forces are exhibited by non-polar molecules
because of thecorrelated movements of the electrons in interacting molecules. The electrons in
adjacent molecules repel each other and so they run away from their usual place. As a result,
electron density in a molecule becomes redistributed in proximity to another molecule, which is
according to quantum mechanical theory of dispersion forces. This is frequently described as the
formation of instantaneous dipoles that attract each other. These type of Dispersion forces are
present between all chemical groups, and usually represent the main part of the total interaction
force in condensed matter..
INTERMOLECULAR FORCES
The document discusses the four main types of intermolecular forces: ion-ion interaction, dipole-dipole interaction, hydrogen bonding, and dispersion forces. It describes the characteristics of each type of interaction and provides examples. The document also explains how intermolecular forces influence various physical properties of substances, such as surface tension, viscosity, capillary action, and evaporation/vaporization. Stronger intermolecular forces generally result in higher melting and boiling points, as well as increased viscosity.
10intermolecularforcesofattraction2-170909132616 (1).pptx
Intermolecular forces include dipole-dipole forces, ion-dipole forces, dispersion forces, and hydrogen bonding. Dipole-dipole forces exist between polar molecules, ion-dipole forces between ions and polar molecules, and dispersion forces are the weakest attraction between all molecules due to induced dipoles. Hydrogen bonding is a special strong dipole-dipole force between a hydrogen atom and electronegative atoms like N, O, or F. These intermolecular forces determine the properties of substances as solids, liquids or gases.
Intermolecular forces
This document discusses different types of intermolecular forces: permanent dipole-dipole forces, van der Waals forces, and hydrogen bonding. It describes how each type of force arises and provides examples to illustrate the effects of these forces on molecular properties like boiling points. Specifically, it notes that hydrogen bonding results in water having a higher boiling point than other hydrides and ice floating due to its lower density than liquid water.
A dipole-induced dipole attraction is a weak attr.pdf
A dipole-induced dipole attraction is a weak attraction that results when a polar
molecule induces a dipole in an atom or in a nonpolar molecule by disturbing the arrangement of
electrons in the nonpolar species. A temporary dipole moment in a species created as a result of a
dipole in a neighboring species and resulting in an attraction between the species. Dipole-dipole
forces are attractive forces between the positive end of one polar molecule and the negative end
of another polar molecule. + and - together.
Solution
A dipole-induced dipole attraction is a weak attraction that results when a polar
molecule induces a dipole in an atom or in a nonpolar molecule by disturbing the arrangement of
electrons in the nonpolar species. A temporary dipole moment in a species created as a result of a
dipole in a neighboring species and resulting in an attraction between the species. Dipole-dipole
forces are attractive forces between the positive end of one polar molecule and the negative end
of another polar molecule. + and - together..
Key SI #6
Intermolecular forces exist between molecules, while intramolecular forces exist within molecules. Melting points increase as intermolecular forces strengthen. Polar molecules have partial charges and can form ion-dipole attractions. The main intermolecular forces are London dispersion, dipole-dipole, and hydrogen bonding. Ionic and covalent bonds are stronger than any intermolecular force within a molecule. A flow chart determines the dominant intermolecular force based on whether ions or polar molecules are present.
Intermolecular forces of attraction ( IMF)
This is a ppt for the topic IMF this is only a brief lectures that i made for my reporting.
Chemical bonds
This document discusses three types of chemical bonds: metallic bonds, ionic bonds, and covalent bonds. It then describes different types of covalent bonds including nonpolar, polar, and coordinated covalent bonds. Finally, it discusses three types of intermolecular forces: dispersion forces, dipole-dipole forces, and hydrogen bonding. Dispersion forces exist between all molecules due to temporary dipoles, while dipole-dipole forces exist between polar molecules due to attraction of partial charges. Hydrogen bonding is a strong form of dipole-dipole force between a hydrogen atom covalently bonded to an electronegative atom like N, O, or F.
Intermolecular forces
The document discusses the three main types of intermolecular forces: dipole-dipole forces, London dispersion forces, and hydrogen bonding. It describes each type of force, including that dipole-dipole forces exist between polar molecules, London dispersion forces exist between all molecules, and hydrogen bonding specifically refers to the attraction between hydrogen atoms bonded to electronegative atoms like N, O, or F. The document also discusses how these intermolecular forces can explain the physical properties of liquids and some solids.
Lesson 5 Intermolecular Forces of attraction
This document discusses intermolecular forces. It begins by defining adhesion and cohesion. It then discusses the four main types of intermolecular forces - London dispersion forces, dipole-dipole forces, ion-dipole forces, and hydrogen bonding. London dispersion forces are the weakest and exist between all molecules. Dipole-dipole forces are moderate in strength and exist between polar molecules. Ion-dipole forces are strong and result from attraction between ions and polar molecules. Hydrogen bonding is the strongest type and occurs when hydrogen is bonded to fluorine, oxygen, or nitrogen. The strength of intermolecular forces influences various physical properties like boiling point and viscosity.
Intramolecularforces.pdf
1) Intermolecular forces are weak attractions between molecules that depend on factors like temperature, pressure, and molecular polarity. These forces include dipole-dipole interactions, hydrogen bonding, and London dispersion forces.
2) Dipole-dipole interactions occur between polar molecules with partial charges, while hydrogen bonding is a stronger form of dipole-dipole interaction between hydrogen and highly electronegative atoms.
3) London dispersion forces exist in all molecules due to the instantaneous dipoles formed from fluctuations in the electron cloud. They increase with molecular size and polarizability.
Covalent Bonds 2
The document discusses different types of chemical bonds, including covalent, ionic, and intermediate bonds that have characteristics of both. It explains that ionic bonds can take on covalent characteristics when the cation distorts the electron charge of the anion. Polar molecules form when there is a difference in electronegativity between bonded atoms, with larger differences resulting in greater polarity. Molecular shapes are determined by electron pair repulsion theory, where electron pairs repel each other.
Intermolecular_Forces_of_Attraction_pptx.pptx
Intermolecular forces are weaker than intramolecular forces but determine properties like boiling point, melting point, and density. There are several types of intermolecular forces including London dispersion forces, dipole-dipole interactions, hydrogen bonding, and ion-dipole interactions. London dispersion forces result from temporary dipoles between all molecules and increase with atomic mass. Dipole-dipole interactions occur between polar molecules while hydrogen bonding is particularly strong between a hydrogen atom bonded to an electronegative atom like nitrogen, oxygen, or fluorine. Stronger intermolecular forces require more energy to overcome.
intermolecular_forces.pptx
Intermolecular forces
Chemical bonding
Chemical structure
van der Vaal force
electrons, dipole interaction,
Imf intro
This document provides instructions for an experiment on intermolecular forces. Students are asked to draw the structures of water, carbon dioxide, and ammonia including bond angles and lone pairs. They must describe van der Waals, dipole, and hydrogen bonding forces and relate these intermolecular forces to physical properties. The document further explains these different intermolecular forces and provides context for why the experiment is being done to examine solubility based on intermolecular forces. It concludes with a short quiz and assigning homework on bonding.
Intermolecular forces
The document discusses intermolecular forces and their relationship to solubility. It defines intermolecular forces as forces between molecules that are weaker than intramolecular forces. There are three main types of intermolecular forces: London dispersion forces, dipole-dipole interactions, and hydrogen bonding, with hydrogen bonding being the strongest. Compounds with stronger intermolecular forces are harder to separate and therefore have higher melting and boiling points, making them more likely to be liquids or solids, while those with weaker forces are more likely to be gases.
Other Bonding
Metallic bonding occurs in a giant metallic lattice where metal atoms form positive ions that are held in place by a "sea" of delocalized electrons. Intermolecular forces include instantaneous dipole-induced dipole forces, permanent dipole-dipole forces, and especially strong hydrogen bonds between molecules containing hydroxyl or amino groups. The structures of graphite and diamond are explained by their giant molecular structures held together by these different intermolecular forces.
option E .Na2co3 hydrolysyes and gives NaoH which.pdf
option E .Na2co3 hydrolysyes and gives NaoH which is a strong base. disscoation
of weak acid Ch3cooh is increases in a basic medium
Solution
option E .Na2co3 hydrolysyes and gives NaoH which is a strong base. disscoation
of weak acid Ch3cooh is increases in a basic medium.
non polar molecules such as lipids and cholestrol.pdf
non polar molecules such as lipids and cholestrol
Solution
non polar molecules such as lipids and cholestrol.
More Related Content
Similar to Dispersion forces (answer)Explanation - Dispersion forces have.pdf
Stabilization of emulsion via electrostatic
This document discusses the stabilization of emulsions via electrostatic forces. It defines emulsions as dispersions of one liquid in another immiscible liquid, and describes the electrical double layer that forms around dispersed droplets consisting of surface charges and layers of counterions. The document outlines DLVO theory, which states that emulsion stability is determined by a balance of attractive van der Waals forces and repulsive electrostatic forces. It also discusses how zeta potential measurement relates to stability, and how pH and ionic strength can affect zeta potential and thus the stability of emulsions.
Dipole-dipole forces are attractive forces between the positive end .pdf
Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the
negative end of another polar molecule.
London force, or Van der Waals force, are temporary fluctuationg dipoles
Hydrogen bonding is the attractive interaction of a hydrogen atom with an electronegative atom
(usually nitrogen, oxygen or fluorine). Seeing any of those three atoms usually gives away the
fact that it\'s hydrogen bonding and probably makes it the most easily noticeable type of
bonding.
Hope that helps!
Solution
Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the
negative end of another polar molecule.
London force, or Van der Waals force, are temporary fluctuationg dipoles
Hydrogen bonding is the attractive interaction of a hydrogen atom with an electronegative atom
(usually nitrogen, oxygen or fluorine). Seeing any of those three atoms usually gives away the
fact that it\'s hydrogen bonding and probably makes it the most easily noticeable type of
bonding.
Hope that helps!.
Intermolecular Forces of attraction
This document discusses different types of intermolecular forces: dipole-dipole forces between polar molecules, ion-dipole forces between ions and polar molecules, dispersion forces between all molecules due to induced dipoles, and strong hydrogen bonds between partial charges on hydrogen and electronegative atoms like N, O, F. These intermolecular forces are responsible for determining the properties and phase of substances.
The strongest attractive forces between molecules of O_2 are ionic .pdf
The strongest attractive forces between molecules of O_2 are: ionic covalent hydrogen
bonding dipole-dipole attractions dispersion forces
Solution
The attractive forces between molecules of O2 will be dispersion forces. This is because O2 is a
non-polar molecule so there will be no dipole-dipole interactions, also there is no hydrogen atom
so no question of Hydrogen bonding. Dispersion forces are exhibited by non-polar molecules
because of thecorrelated movements of the electrons in interacting molecules. The electrons in
adjacent molecules repel each other and so they run away from their usual place. As a result,
electron density in a molecule becomes redistributed in proximity to another molecule, which is
according to quantum mechanical theory of dispersion forces. This is frequently described as the
formation of instantaneous dipoles that attract each other. These type of Dispersion forces are
present between all chemical groups, and usually represent the main part of the total interaction
force in condensed matter..
INTERMOLECULAR FORCES
The document discusses the four main types of intermolecular forces: ion-ion interaction, dipole-dipole interaction, hydrogen bonding, and dispersion forces. It describes the characteristics of each type of interaction and provides examples. The document also explains how intermolecular forces influence various physical properties of substances, such as surface tension, viscosity, capillary action, and evaporation/vaporization. Stronger intermolecular forces generally result in higher melting and boiling points, as well as increased viscosity.
10intermolecularforcesofattraction2-170909132616 (1).pptx
Intermolecular forces include dipole-dipole forces, ion-dipole forces, dispersion forces, and hydrogen bonding. Dipole-dipole forces exist between polar molecules, ion-dipole forces between ions and polar molecules, and dispersion forces are the weakest attraction between all molecules due to induced dipoles. Hydrogen bonding is a special strong dipole-dipole force between a hydrogen atom and electronegative atoms like N, O, or F. These intermolecular forces determine the properties of substances as solids, liquids or gases.
Intermolecular forces
This document discusses different types of intermolecular forces: permanent dipole-dipole forces, van der Waals forces, and hydrogen bonding. It describes how each type of force arises and provides examples to illustrate the effects of these forces on molecular properties like boiling points. Specifically, it notes that hydrogen bonding results in water having a higher boiling point than other hydrides and ice floating due to its lower density than liquid water.
A dipole-induced dipole attraction is a weak attr.pdf
A dipole-induced dipole attraction is a weak attraction that results when a polar
molecule induces a dipole in an atom or in a nonpolar molecule by disturbing the arrangement of
electrons in the nonpolar species. A temporary dipole moment in a species created as a result of a
dipole in a neighboring species and resulting in an attraction between the species. Dipole-dipole
forces are attractive forces between the positive end of one polar molecule and the negative end
of another polar molecule. + and - together.
Solution
A dipole-induced dipole attraction is a weak attraction that results when a polar
molecule induces a dipole in an atom or in a nonpolar molecule by disturbing the arrangement of
electrons in the nonpolar species. A temporary dipole moment in a species created as a result of a
dipole in a neighboring species and resulting in an attraction between the species. Dipole-dipole
forces are attractive forces between the positive end of one polar molecule and the negative end
of another polar molecule. + and - together..
Key SI #6
Intermolecular forces exist between molecules, while intramolecular forces exist within molecules. Melting points increase as intermolecular forces strengthen. Polar molecules have partial charges and can form ion-dipole attractions. The main intermolecular forces are London dispersion, dipole-dipole, and hydrogen bonding. Ionic and covalent bonds are stronger than any intermolecular force within a molecule. A flow chart determines the dominant intermolecular force based on whether ions or polar molecules are present.
Intermolecular forces of attraction ( IMF)
This is a ppt for the topic IMF this is only a brief lectures that i made for my reporting.
Chemical bonds
This document discusses three types of chemical bonds: metallic bonds, ionic bonds, and covalent bonds. It then describes different types of covalent bonds including nonpolar, polar, and coordinated covalent bonds. Finally, it discusses three types of intermolecular forces: dispersion forces, dipole-dipole forces, and hydrogen bonding. Dispersion forces exist between all molecules due to temporary dipoles, while dipole-dipole forces exist between polar molecules due to attraction of partial charges. Hydrogen bonding is a strong form of dipole-dipole force between a hydrogen atom covalently bonded to an electronegative atom like N, O, or F.
Intermolecular forces
The document discusses the three main types of intermolecular forces: dipole-dipole forces, London dispersion forces, and hydrogen bonding. It describes each type of force, including that dipole-dipole forces exist between polar molecules, London dispersion forces exist between all molecules, and hydrogen bonding specifically refers to the attraction between hydrogen atoms bonded to electronegative atoms like N, O, or F. The document also discusses how these intermolecular forces can explain the physical properties of liquids and some solids.
Lesson 5 Intermolecular Forces of attraction
This document discusses intermolecular forces. It begins by defining adhesion and cohesion. It then discusses the four main types of intermolecular forces - London dispersion forces, dipole-dipole forces, ion-dipole forces, and hydrogen bonding. London dispersion forces are the weakest and exist between all molecules. Dipole-dipole forces are moderate in strength and exist between polar molecules. Ion-dipole forces are strong and result from attraction between ions and polar molecules. Hydrogen bonding is the strongest type and occurs when hydrogen is bonded to fluorine, oxygen, or nitrogen. The strength of intermolecular forces influences various physical properties like boiling point and viscosity.
Intramolecularforces.pdf
1) Intermolecular forces are weak attractions between molecules that depend on factors like temperature, pressure, and molecular polarity. These forces include dipole-dipole interactions, hydrogen bonding, and London dispersion forces.
2) Dipole-dipole interactions occur between polar molecules with partial charges, while hydrogen bonding is a stronger form of dipole-dipole interaction between hydrogen and highly electronegative atoms.
3) London dispersion forces exist in all molecules due to the instantaneous dipoles formed from fluctuations in the electron cloud. They increase with molecular size and polarizability.
Covalent Bonds 2
The document discusses different types of chemical bonds, including covalent, ionic, and intermediate bonds that have characteristics of both. It explains that ionic bonds can take on covalent characteristics when the cation distorts the electron charge of the anion. Polar molecules form when there is a difference in electronegativity between bonded atoms, with larger differences resulting in greater polarity. Molecular shapes are determined by electron pair repulsion theory, where electron pairs repel each other.
Intermolecular_Forces_of_Attraction_pptx.pptx
Intermolecular forces are weaker than intramolecular forces but determine properties like boiling point, melting point, and density. There are several types of intermolecular forces including London dispersion forces, dipole-dipole interactions, hydrogen bonding, and ion-dipole interactions. London dispersion forces result from temporary dipoles between all molecules and increase with atomic mass. Dipole-dipole interactions occur between polar molecules while hydrogen bonding is particularly strong between a hydrogen atom bonded to an electronegative atom like nitrogen, oxygen, or fluorine. Stronger intermolecular forces require more energy to overcome.
intermolecular_forces.pptx
Intermolecular forces
Chemical bonding
Chemical structure
van der Vaal force
electrons, dipole interaction,
Imf intro
This document provides instructions for an experiment on intermolecular forces. Students are asked to draw the structures of water, carbon dioxide, and ammonia including bond angles and lone pairs. They must describe van der Waals, dipole, and hydrogen bonding forces and relate these intermolecular forces to physical properties. The document further explains these different intermolecular forces and provides context for why the experiment is being done to examine solubility based on intermolecular forces. It concludes with a short quiz and assigning homework on bonding.
Intermolecular forces
The document discusses intermolecular forces and their relationship to solubility. It defines intermolecular forces as forces between molecules that are weaker than intramolecular forces. There are three main types of intermolecular forces: London dispersion forces, dipole-dipole interactions, and hydrogen bonding, with hydrogen bonding being the strongest. Compounds with stronger intermolecular forces are harder to separate and therefore have higher melting and boiling points, making them more likely to be liquids or solids, while those with weaker forces are more likely to be gases.
Other Bonding
Metallic bonding occurs in a giant metallic lattice where metal atoms form positive ions that are held in place by a "sea" of delocalized electrons. Intermolecular forces include instantaneous dipole-induced dipole forces, permanent dipole-dipole forces, and especially strong hydrogen bonds between molecules containing hydroxyl or amino groups. The structures of graphite and diamond are explained by their giant molecular structures held together by these different intermolecular forces.
Similar to Dispersion forces (answer)Explanation - Dispersion forces have.pdf (20)
Dipole-dipole forces are attractive forces between the positive end .pdf
Dipole-dipole forces are attractive forces between the positive end .pdf
The strongest attractive forces between molecules of O_2 are ionic .pdf
The strongest attractive forces between molecules of O_2 are ionic .pdf
10intermolecularforcesofattraction2-170909132616 (1).pptx
10intermolecularforcesofattraction2-170909132616 (1).pptx
A dipole-induced dipole attraction is a weak attr.pdf
A dipole-induced dipole attraction is a weak attr.pdf
More from anokhilalmobile
option E .Na2co3 hydrolysyes and gives NaoH which.pdf
option E .Na2co3 hydrolysyes and gives NaoH which is a strong base. disscoation
of weak acid Ch3cooh is increases in a basic medium
Solution
option E .Na2co3 hydrolysyes and gives NaoH which is a strong base. disscoation
of weak acid Ch3cooh is increases in a basic medium.
non polar molecules such as lipids and cholestrol.pdf
non polar molecules such as lipids and cholestrol
Solution
non polar molecules such as lipids and cholestrol.
moles = molarity x volume = 4.25 molL x 2.50 L =.pdf
moles = molarity x volume = 4.25 mol/L x 2.50 L = 10.63 mol
Solution
moles = molarity x volume = 4.25 mol/L x 2.50 L = 10.63 mol.
Londondispersionvan der Waals forces - these ar.pdf
London/dispersion/van der Waals forces - these are weak interactions that occur in
a matter of nanoseconds when one atom in a bond temporarily takes more of the electron density
than the other one, causing a temporary dipole - i.e. this can happen even when you have a C-H
bond that is normally nonpolar.
Solution
London/dispersion/van der Waals forces - these are weak interactions that occur in
a matter of nanoseconds when one atom in a bond temporarily takes more of the electron density
than the other one, causing a temporary dipole - i.e. this can happen even when you have a C-H
bond that is normally nonpolar..
[H2SO4] = 0 because H2SO4 is a strong acid. first consider Ka2.pdf
[H2SO4] = 0 because H2SO4 is a strong acid.
first consider Ka2:
Ka2 = [H+][SO42-]/[HSO4-] = 1.3X10^-2
From the starting condition, let x = [SO42-]. Then, [H+] = 0.14+ x, and [HSO4-] = 0.14 - x.
now the value in Ka2 expression:
1.3X10^-2 = (0.14 +x) (x) / (0.14-x)
1.82 X10^-3 - 1.3X10^-2x = 0.14 x + x^2
x^2 + 0.153 x – 1.82 X10^-3 = 0
solve the above equation we will get;
x = 0.0111
thus;
x = [SO42-]=0.0111
Then, [H+] = 0.14 + 0.0111 = 0.1511
, and [HSO4-] = 0.14 – x = 0.14- 0.0111= 0.1289
Solution
[H2SO4] = 0 because H2SO4 is a strong acid.
first consider Ka2:
Ka2 = [H+][SO42-]/[HSO4-] = 1.3X10^-2
From the starting condition, let x = [SO42-]. Then, [H+] = 0.14+ x, and [HSO4-] = 0.14 - x.
now the value in Ka2 expression:
1.3X10^-2 = (0.14 +x) (x) / (0.14-x)
1.82 X10^-3 - 1.3X10^-2x = 0.14 x + x^2
x^2 + 0.153 x – 1.82 X10^-3 = 0
solve the above equation we will get;
x = 0.0111
thus;
x = [SO42-]=0.0111
Then, [H+] = 0.14 + 0.0111 = 0.1511
, and [HSO4-] = 0.14 – x = 0.14- 0.0111= 0.1289.
You ordered a chest X-ray and saw fluid buildup in her right lung. S.pdf
You ordered a chest X-ray and saw fluid buildup in her right lung. She also has thick whitish
yellow exudates on her tonsils. Finally, her weak pulse made you order an MRI and it revealed
myocarditis. Given all this evidence, you asked the parents if they had given their children
routine vaccinations. When they said no, you knew exactly what it was. Describe the cause of
Ashley’s illness and how you know.
ans: Ashley\'s illness is due to the bacterial infection caused by the bacteria Corynebacterium
diptheriae.This is causing Ashley to suffer.This bacteria causes infection which led to die the
cells of tonsils and throat.Thats why she is having throat infection.And as they have skipped the
vaccination process she got infected as she has less resistance or immunity.
ELEK test is performed for toxin detection and EIA for detecting toxin in isolates.,
immumnochromatographic strip test specific test for detecting toxins in specimens and isolates.
This organism is transmitted by animlas or main cause is transmission for infected person by
coughing or sneezing.
Ashley\'s innate immunity would produce antibodies against the bacteria .
Solution
You ordered a chest X-ray and saw fluid buildup in her right lung. She also has thick whitish
yellow exudates on her tonsils. Finally, her weak pulse made you order an MRI and it revealed
myocarditis. Given all this evidence, you asked the parents if they had given their children
routine vaccinations. When they said no, you knew exactly what it was. Describe the cause of
Ashley’s illness and how you know.
ans: Ashley\'s illness is due to the bacterial infection caused by the bacteria Corynebacterium
diptheriae.This is causing Ashley to suffer.This bacteria causes infection which led to die the
cells of tonsils and throat.Thats why she is having throat infection.And as they have skipped the
vaccination process she got infected as she has less resistance or immunity.
ELEK test is performed for toxin detection and EIA for detecting toxin in isolates.,
immumnochromatographic strip test specific test for detecting toxins in specimens and isolates.
This organism is transmitted by animlas or main cause is transmission for infected person by
coughing or sneezing.
Ashley\'s innate immunity would produce antibodies against the bacteria ..
why would you be the best candidate for the nursing programSTATEM.pdf
why would you be the best candidate for the nursing program?
STATEMENT OF PURPOSE
I am applying for program at xxx University in order to explore the best practices and techniques
in Nursing. From the time of bachelor degree I have gained a lot of experience, knowledge and
skill in technological advancements . I have a passion to learn profoundly the principles and tools
relating to xxx Nursing. I am also exated in learning the finest approaches in Nursing that can be
used to readily and competently build and maintain Nursing and patient applications.
I had successfully completed Masters Degree (M.Sc) with first class from xxx University. I
perceived that I should procure some constructive and functional experience working in a
research environment. I enjoy every minute to my academic work and participation in innovative
projects. I have realized that being part of the research team can direct me to achieve my aim to
become a research scientist in Nursing .This enables me to have access and discuss ideas with
world famous research scientists. I am hopeful that my ambition and vision will be fulfilled since
I have a strong feeling of competitive potential and excellent academic credentials. I have a great
passion for Nursing from my bachelor studies. During my period of study at xxxxxxxxxxx , I
excelled in courses like Biochemistry, Molecular and Cell Biology, Microbiology, Immunology,
Bioprocess Principles and Engineering, Bio and Chemical Thermodynamics, Enzyme
Engineering. This provided a firm foundation and took me a step closer towards the field of
Nursing to fulfill my goal. The fascinations and promises held out by various areas in
Biochemistry, Engineering and Molecular Biology captivated me.
I am well acquainted with Nursing techniques. During my Masters program I have
done project entitled “xxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxxx”. While conducting the above
project , I had gained on hand experience on xxxxxxxxxxxxx. I have real practical and
operational experience during my training at research laboratory at xxxx.. I have the ability to
organize time efficiently and meticulous preparation is my asset. I have experience in medical la
techniques, Immunological Techniques, plant tissue culture and transformation. I am proficient
in three “R” of English, and xxx languages. I also engaged in many social activities and
extracurricular activities in xxx university campus.
I am totally aware of nursing program in Nursing of xxx University which will enable me to
work with the famous research team with contemporary technology. I am much excited and have
the zeal to join in your research program, with my Nursing profile. I strongly believe that I will
definitely contribute and learn in this xxxxxx specialization in xxxxx University. I am confident
that I will attain well defined career goal in this field and hope part of esteemed institution.
Yours truly,
xxxxx
One of the greatest points of interest in picking nursing as a profession is the expan.
when the data value is passed between two different operating system.pdf
when the data value is passed between two different operating system with different machines
they main problem faced by us:
1)one operating system may access the file different way and the other operating in other ways
one operating system may case sensitive file system and other user non case sensitive file
system.
2) each may different transfer protocol and data transfer speed
3)each will hava different hardware architecture
problem to be solved :
userinterface :
both system may have different user interface so we be able support the interface of other
operating system to send data values
interconnection: to send data inter connectionn is very very important.the interconnection should
done between two different operating systems and both should support the data sending and
recieving
security: while sending the data security is important .when data is transfered between two
similar operating system then it is easy to implement connection security between them but
coming to these it much difficult to implement
Solution
when the data value is passed between two different operating system with different machines
they main problem faced by us:
1)one operating system may access the file different way and the other operating in other ways
one operating system may case sensitive file system and other user non case sensitive file
system.
2) each may different transfer protocol and data transfer speed
3)each will hava different hardware architecture
problem to be solved :
userinterface :
both system may have different user interface so we be able support the interface of other
operating system to send data values
interconnection: to send data inter connectionn is very very important.the interconnection should
done between two different operating systems and both should support the data sending and
recieving
security: while sending the data security is important .when data is transfered between two
similar operating system then it is easy to implement connection security between them but
coming to these it much difficult to implement.
Using mathematical induction,STEP 1The base n = 1 is clearl.pdf
Using mathematical induction,
STEP 1:
The base n = 1 is clearly true since12n
Solution
Using mathematical induction,
STEP 1:
The base n = 1 is clearly true since12n.
The process include many steps which could be planning and preparati.pdf
The process include many steps which could be planning and preparation, detection of incident,
initial response, Formulation of response strategy, Foresnsics backups, investigation,
Implementation of security measures , Network monitoring, Recovery, reporting and final is
follow up.
Action or an event never happens on a prescribed or convenient time hence a its always to have a
checklist in place and be prepared like what time the issue happend,who reported etc.
Then to analyse the situation and which might requite forensics software and other environment
support which helps in analysis, gathering and understanding of evidence.
And the most important part is duplication which is accomplised by creating duplicate bit by bit
to a hard drive.And there are basically two approaches of doing so one is software based and
another is hardware based.And in this place hardware based approach has upper hand as it
provides speed and integrity.Also it provided the confidence of less risk of data gettting
corrupted.
Solution
The process include many steps which could be planning and preparation, detection of incident,
initial response, Formulation of response strategy, Foresnsics backups, investigation,
Implementation of security measures , Network monitoring, Recovery, reporting and final is
follow up.
Action or an event never happens on a prescribed or convenient time hence a its always to have a
checklist in place and be prepared like what time the issue happend,who reported etc.
Then to analyse the situation and which might requite forensics software and other environment
support which helps in analysis, gathering and understanding of evidence.
And the most important part is duplication which is accomplised by creating duplicate bit by bit
to a hard drive.And there are basically two approaches of doing so one is software based and
another is hardware based.And in this place hardware based approach has upper hand as it
provides speed and integrity.Also it provided the confidence of less risk of data gettting
corrupted..
The FCPA established criminal and civil penalties for unlawful payme.pdf
The FCPA established criminal and civil penalties for unlawful payments or bribes (or promises
of payments) to foreign officials for the purpose of obtaining or keeping business, either directly
or indirectly or through agents, to influence any act or decision or to secure any improper
advantage in order to obtain or retain business.
The FCPA applies to foreign companies listed on a US exchange or required to file accounts
with the SEC, as well as by US corporations or US nationals. It also applies to foreign nationals
who cause an act in the US (such as a wire transfer or establishment of an e-mail server in the
US) which furthers an FCPA offence.
Accounting requirements apply to companies required to file periodic reports with the SEC.
Requirements cover both systems of internal control and adequate record keeping – non-
compliance can be a criminal offence.
The US federal authorities are pursuing cases aggressively and assessing large penalties for the
violations of FPCA.
Companies which may be subject to the FCPA are strongly advised to conduct suitable due
diligence on intermediaries, agents or local partners. Local U.S. Embassies or Consulates can
provide suitable profiles under the International Company Profile (ICP) service.
Managers and lawyers in most companies want to believe they work for clean, ethical
organizations that hire law-abiding employees. This positive bias often blinds US business
people to the reality of international business, where bribes, kickbacks, and false or unrecorded
transactions are common. Corrupt activity also exists in the US of course, but it is more difficult
to understand what is going on in foreign countries when your US managers have little or no
language ability or cultural context.
Some US business people believe and frequently say \"Everyone knows you can\'t do business in
(Mexico, China, India, Russia - pick a country) without paying bribes. It is part of their culture. It
is crazy to have a US law that makes paying bribes in foreign countries illegal in the USA.\"
Even if that were true, the FCPA is part of the legal environment for international business.
Compliance is not optional because American management has a low opinion of foreign
government officials.
Corruption in international business is common and frequently ignored.
Investigation, prosecution and punishment under the FCPA is common.
Understand your company\'s risk of being involved in international bribery.
Your program requires a Standalone International Anti-corruption Compliance policy, and an
Executive who is Accountable for the “Tone at the Top”.
Train your board, management, employees and third parties who distribute your products
Know all the 3rd parties your company uses in business outside the USA and conduct due
diligence.
Establish a set of internal controls over company expenditures and assets.
Do not permit facilitating payments.
Plan for the likelihood you will have to conduct high quality international internal inves.
The answer is(B.) H- and (C.) NH3Lewis bases are electron pair .pdf
The answer is:
(B.) H- and (C.) NH3
Lewis bases are electron pair donors.
Both H- and NH3 (the N atom) have lone electron pairs for donation and are thus Lewis bases.
Solution
The answer is:
(B.) H- and (C.) NH3
Lewis bases are electron pair donors.
Both H- and NH3 (the N atom) have lone electron pairs for donation and are thus Lewis bases..
Spontaneous mutation rates depend on the rate at which DNA transcrip.pdf
Spontaneous mutation rates depend on the rate at which DNA transcription occurs. All the three
strains given in the question show a higher rate of spontaneous mutation because they have
effects in the mutS or mutL genes, which are involved in mismatch repair system.
In Salmonella A and B, during infectious stage, the DNA mutations occurs faster when
compared to E.coli, because DNA damage does not induce SOS response for DNA repair in
Salmonella.
The E.Coli strain has a better DNA repair system because the SOS response quickly responds to
the DNA damage during infectious phase.
E.coli strain has more permeable membrane compared to Salmonella.
Solution
Spontaneous mutation rates depend on the rate at which DNA transcription occurs. All the three
strains given in the question show a higher rate of spontaneous mutation because they have
effects in the mutS or mutL genes, which are involved in mismatch repair system.
In Salmonella A and B, during infectious stage, the DNA mutations occurs faster when
compared to E.coli, because DNA damage does not induce SOS response for DNA repair in
Salmonella.
The E.Coli strain has a better DNA repair system because the SOS response quickly responds to
the DNA damage during infectious phase.
E.coli strain has more permeable membrane compared to Salmonella..
Sales revenue100000Less- COGS60000Gross profit40000Opera.pdf
Sales revenue
100000
Less- COGS
60000
Gross profit
40000
Operating expenses
Selling expense
Advertising expense
4500
4500
Administrative expense
supplies expense
1500
rent expense
4000
salaries expense
9500
utilities expense
1100
16100
Total operating expenses
20600
Operating income
19400
Non operating income and expenses
loss of sale on land
(3200)
Less- interest expense
6900
Net Other Incomes and Expenses
(10100)
Net income before tax
9300
Less- Income tax
3800
Earnings after tax
5500Income statement
Sales revenue
100000
Less- COGS
60000
Gross profit
40000
Operating expenses
Selling expense
Advertising expense
4500
4500
Administrative expense
supplies expense
1500
rent expense
4000
salaries expense
9500
utilities expense
1100
16100
Total operating expenses
20600
Operating income
19400
Non operating income and expenses
loss of sale on land
(3200)
Less- interest expense
6900
Net Other Incomes and Expenses
(10100)
Net income before tax
9300
Less- Income tax
3800
Earnings after tax
5500
Solution
Sales revenue
100000
Less- COGS
60000
Gross profit
40000
Operating expenses
Selling expense
Advertising expense
4500
4500
Administrative expense
supplies expense
1500
rent expense
4000
salaries expense
9500
utilities expense
1100
16100
Total operating expenses
20600
Operating income
19400
Non operating income and expenses
loss of sale on land
(3200)
Less- interest expense
6900
Net Other Incomes and Expenses
(10100)
Net income before tax
9300
Less- Income tax
3800
Earnings after tax
5500Income statement
Sales revenue
100000
Less- COGS
60000
Gross profit
40000
Operating expenses
Selling expense
Advertising expense
4500
4500
Administrative expense
supplies expense
1500
rent expense
4000
salaries expense
9500
utilities expense
1100
16100
Total operating expenses
20600
Operating income
19400
Non operating income and expenses
loss of sale on land
(3200)
Less- interest expense
6900
Net Other Incomes and Expenses
(10100)
Net income before tax
9300
Less- Income tax
3800
Earnings after tax
5500.
D) Counterclockwise answer .pdf
This document provides a single-word answer of "Counterclockwise" to an unspecified question or problem. No other context or details are given about the question, solution, or meaning of the counterclockwise response.
Please give the differential equation and boundary conditions.So.pdf
Please give the differential equation and boundary conditions.
Solution
Please give the differential equation and boundary conditions..
Point.javapublic class Point { int x,y; double m,n; .pdf
Point.java
public class Point
{
int x,y;
double m,n;
public Point(){}
public double getX() { return x; }
public double getY() { return y; }
public double getRadius() { return Math.sqrt(x * x + y * y); }
public double getAngle() { return Math.atan2(y, x); }
public static Point of(int i,int j)
{
Point p=new Point();
p.x=i;
p.y=j;
return p;
}
public static Point ofPolar(double i,double j)
{
Point p=new Point();
p.m=i;
p.n=j;
return p;
}
}
PointTest.java
import org.junit.*;
import static org.junit.Assert.*;
public class PointTest
{
private static final double TOLERANCE = 1E-12;
@Test public void testOf1()
{
Point p = Point.of(1, -1);
assertEquals(1, p.getX(), TOLERANCE);
assertEquals(-1, p.getY(), TOLERANCE);
assertEquals(Math.sqrt(2), p.getRadius(), TOLERANCE);
assertEquals(-Math.PI / 4, p.getAngle(), TOLERANCE);
}
@Test public void testOf2()
{
Point p = Point.ofPolar(Math.sqrt(2), -Math.PI / 4);
assertEquals(1, p.getX(), TOLERANCE);
assertEquals(-1, p.getY(), TOLERANCE);
assertEquals(Math.sqrt(2), p.getRadius(), TOLERANCE);
assertEquals(-Math.PI / 4, p.getAngle(), TOLERANCE);
}
}
Solution
Point.java
public class Point
{
int x,y;
double m,n;
public Point(){}
public double getX() { return x; }
public double getY() { return y; }
public double getRadius() { return Math.sqrt(x * x + y * y); }
public double getAngle() { return Math.atan2(y, x); }
public static Point of(int i,int j)
{
Point p=new Point();
p.x=i;
p.y=j;
return p;
}
public static Point ofPolar(double i,double j)
{
Point p=new Point();
p.m=i;
p.n=j;
return p;
}
}
PointTest.java
import org.junit.*;
import static org.junit.Assert.*;
public class PointTest
{
private static final double TOLERANCE = 1E-12;
@Test public void testOf1()
{
Point p = Point.of(1, -1);
assertEquals(1, p.getX(), TOLERANCE);
assertEquals(-1, p.getY(), TOLERANCE);
assertEquals(Math.sqrt(2), p.getRadius(), TOLERANCE);
assertEquals(-Math.PI / 4, p.getAngle(), TOLERANCE);
}
@Test public void testOf2()
{
Point p = Point.ofPolar(Math.sqrt(2), -Math.PI / 4);
assertEquals(1, p.getX(), TOLERANCE);
assertEquals(-1, p.getY(), TOLERANCE);
assertEquals(Math.sqrt(2), p.getRadius(), TOLERANCE);
assertEquals(-Math.PI / 4, p.getAngle(), TOLERANCE);
}
}.
pKa of H2PO4- is = 7.21According to Hendersons Equation ,pH = .pdf
pKa of H2PO4- is = 7.21
According to Henderson\'s Equation ,
pH = pKa + log ( [salt] /[acid])
= pKa + log ( [Na2HPO4] / [ KH2PO4 ] )
= 7.21 + log ( 0.135 / 0.185 )
= 7.21 - 0.14
= 7.07
Solution
pKa of H2PO4- is = 7.21
According to Henderson\'s Equation ,
pH = pKa + log ( [salt] /[acid])
= pKa + log ( [Na2HPO4] / [ KH2PO4 ] )
= 7.21 + log ( 0.135 / 0.185 )
= 7.21 - 0.14
= 7.07.
Covalent bonds .pdf
This very short document appears to be about covalent bonds but provides no actual information about the topic in its 1 word title and 2 repeated words. It does not contain enough contextual information to generate a meaningful 3 sentence summary.
naphthalene, dry ice (solid co2),iodine(gentle heating), arsenic (At.pdf
naphthalene, dry ice (solid co2),iodine(gentle heating), arsenic (At high temperature) etc...
Solution
naphthalene, dry ice (solid co2),iodine(gentle heating), arsenic (At high temperature) etc....
More from anokhilalmobile (20)
option E .Na2co3 hydrolysyes and gives NaoH which.pdf
option E .Na2co3 hydrolysyes and gives NaoH which.pdf
non polar molecules such as lipids and cholestrol.pdf
non polar molecules such as lipids and cholestrol.pdf
moles = molarity x volume = 4.25 molL x 2.50 L =.pdf
moles = molarity x volume = 4.25 molL x 2.50 L =.pdf
Londondispersionvan der Waals forces - these ar.pdf
Londondispersionvan der Waals forces - these ar.pdf
[H2SO4] = 0 because H2SO4 is a strong acid. first consider Ka2.pdf
[H2SO4] = 0 because H2SO4 is a strong acid. first consider Ka2.pdf
You ordered a chest X-ray and saw fluid buildup in her right lung. S.pdf
You ordered a chest X-ray and saw fluid buildup in her right lung. S.pdf
why would you be the best candidate for the nursing programSTATEM.pdf
why would you be the best candidate for the nursing programSTATEM.pdf
when the data value is passed between two different operating system.pdf
when the data value is passed between two different operating system.pdf
Using mathematical induction,STEP 1The base n = 1 is clearl.pdf
Using mathematical induction,STEP 1The base n = 1 is clearl.pdf
The process include many steps which could be planning and preparati.pdf
The process include many steps which could be planning and preparati.pdf
The FCPA established criminal and civil penalties for unlawful payme.pdf
The FCPA established criminal and civil penalties for unlawful payme.pdf
The answer is(B.) H- and (C.) NH3Lewis bases are electron pair .pdf
The answer is(B.) H- and (C.) NH3Lewis bases are electron pair .pdf
Spontaneous mutation rates depend on the rate at which DNA transcrip.pdf
Spontaneous mutation rates depend on the rate at which DNA transcrip.pdf
Sales revenue100000Less- COGS60000Gross profit40000Opera.pdf
Sales revenue100000Less- COGS60000Gross profit40000Opera.pdf
Please give the differential equation and boundary conditions.So.pdf
Please give the differential equation and boundary conditions.So.pdf
Point.javapublic class Point { int x,y; double m,n; .pdf
Point.javapublic class Point { int x,y; double m,n; .pdf
pKa of H2PO4- is = 7.21According to Hendersons Equation ,pH = .pdf
pKa of H2PO4- is = 7.21According to Hendersons Equation ,pH = .pdf
naphthalene, dry ice (solid co2),iodine(gentle heating), arsenic (At.pdf
naphthalene, dry ice (solid co2),iodine(gentle heating), arsenic (At.pdf
Recently uploaded
PCOS corelations and management through Ayurveda.
This presentation includes basic of PCOS their pathology and treatment and also Ayurveda correlation of PCOS and Ayurvedic line of treatment mentioned in classics.
Types of Herbal Cosmetics its standardization.
Physiology and chemistry of skin and pigmentation, hairs, scalp, lips and nail, Cleansing cream, Lotions, Face powders, Face packs, Lipsticks, Bath products, soaps and baby product,
Preparation and standardization of the following : Tonic, Bleaches, Dentifrices and Mouth washes & Tooth Pastes, Cosmetics for Nails.
বাংলাদেশ অর্থনৈতিক সমীক্ষা (Economic Review) ২০২৪ UJS App.pdf
বাংলাদেশের অর্থনৈতিক সমীক্ষা ২০২৪ [Bangladesh Economic Review 2024 Bangla.pdf] কম্পিউটার , ট্যাব ও স্মার্ট ফোন ভার্সন সহ সম্পূর্ণ বাংলা ই-বুক বা pdf বই " সুচিপত্র ...বুকমার্ক মেনু 🔖 ও হাইপার লিংক মেনু 📝👆 যুক্ত ..
আমাদের সবার জন্য খুব খুব গুরুত্বপূর্ণ একটি বই ..বিসিএস, ব্যাংক, ইউনিভার্সিটি ভর্তি ও যে কোন প্রতিযোগিতা মূলক পরীক্ষার জন্য এর খুব ইম্পরট্যান্ট একটি বিষয় ...তাছাড়া বাংলাদেশের সাম্প্রতিক যে কোন ডাটা বা তথ্য এই বইতে পাবেন ...
তাই একজন নাগরিক হিসাবে এই তথ্য গুলো আপনার জানা প্রয়োজন ...।
বিসিএস ও ব্যাংক এর লিখিত পরীক্ষা ...+এছাড়া মাধ্যমিক ও উচ্চমাধ্যমিকের স্টুডেন্টদের জন্য অনেক কাজে আসবে ...
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...Nguyen Thanh Tu Collection
https://app.box.com/s/y977uz6bpd3af4qsebv7r9b7s21935vdThe Diamonds of 2023-2024 in the IGRA collection
A review of the growth of the Israel Genealogy Research Association Database Collection for the last 12 months. Our collection is now passed the 3 million mark and still growing. See which archives have contributed the most. See the different types of records we have, and which years have had records added. You can also see what we have for the future.
Advanced Java[Extra Concepts, Not Difficult].docx
This is part 2 of my Java Learning Journey. This contains Hashing, ArrayList, LinkedList, Date and Time Classes, Calendar Class and more.
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...National Information Standards Organization (NISO)
This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.Your Skill Boost Masterclass: Strategies for Effective Upskilling
Your Skill Boost Masterclass: Strategies for Effective UpskillingExcellence Foundation for South Sudan
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.Executive Directors Chat Leveraging AI for Diversity, Equity, and Inclusion
Let’s explore the intersection of technology and equity in the final session of our DEI series. Discover how AI tools, like ChatGPT, can be used to support and enhance your nonprofit's DEI initiatives. Participants will gain insights into practical AI applications and get tips for leveraging technology to advance their DEI goals.
South African Journal of Science: Writing with integrity workshop (2024)
South African Journal of Science: Writing with integrity workshop (2024)Academy of Science of South Africa
A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.DRUGS AND ITS classification slide share
Any substance (other than food) that is used to prevent, diagnose, treat, or relieve symptoms of a
disease or abnormal condition
RPMS TEMPLATE FOR SCHOOL YEAR 2023-2024 FOR TEACHER 1 TO TEACHER 3
RPMS Template 2023-2024 by: Irene S. Rueco
Azure Interview Questions and Answers PDF By ScholarHat
Azure Interview Questions and Answers PDF By ScholarHat
How to Fix the Import Error in the Odoo 17
An import error occurs when a program fails to import a module or library, disrupting its execution. In languages like Python, this issue arises when the specified module cannot be found or accessed, hindering the program's functionality. Resolving import errors is crucial for maintaining smooth software operation and uninterrupted development processes.
Introduction to AI for Nonprofits with Tapp Network
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.
Recently uploaded (20)
বাংলাদেশ অর্থনৈতিক সমীক্ষা (Economic Review) ২০২৪ UJS App.pdf
বাংলাদেশ অর্থনৈতিক সমীক্ষা (Economic Review) ২০২৪ UJS App.pdf
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Your Skill Boost Masterclass: Strategies for Effective Upskilling
Your Skill Boost Masterclass: Strategies for Effective Upskilling
Executive Directors Chat Leveraging AI for Diversity, Equity, and Inclusion
Executive Directors Chat Leveraging AI for Diversity, Equity, and Inclusion
South African Journal of Science: Writing with integrity workshop (2024)
South African Journal of Science: Writing with integrity workshop (2024)
RPMS TEMPLATE FOR SCHOOL YEAR 2023-2024 FOR TEACHER 1 TO TEACHER 3
RPMS TEMPLATE FOR SCHOOL YEAR 2023-2024 FOR TEACHER 1 TO TEACHER 3
Azure Interview Questions and Answers PDF By ScholarHat
Azure Interview Questions and Answers PDF By ScholarHat
Liberal Approach to the Study of Indian Politics.pdf
Liberal Approach to the Study of Indian Politics.pdf
Introduction to AI for Nonprofits with Tapp Network
Introduction to AI for Nonprofits with Tapp Network
Dispersion forces (answer)Explanation - Dispersion forces have.pdf
- 1. Dispersion forces (answer) Explanation - Dispersion forces have many different names: London forces, Van der Waals forces, instantaneous dipoles. Dispersion forces involve the attraction between temporarily induced dipoles in nonpolar molecules (often disappear within an instant). This polarization can be induced either by a polar molecule or by the repulsion of negatively charged electron clouds in nonpolar molecules. As electrons move around their shells, electron density may randomly be distributed unevenly, creating a partially negative (?-) charge. The opposite side of the molecule then becomes partially positive (?+). The result is a temporary dipole. If this process occurs in two molecules that are close to one another, the two molecules will be attracted to each other, and will form a temporary, non-covalent bond. Solution Dispersion forces (answer) Explanation - Dispersion forces have many different names: London forces, Van der Waals forces, instantaneous dipoles. Dispersion forces involve the attraction between temporarily induced dipoles in nonpolar molecules (often disappear within an instant). This polarization can be induced either by a polar molecule or by the repulsion of negatively charged electron clouds in nonpolar molecules. As electrons move around their shells, electron density may randomly be distributed unevenly, creating a partially negative (?-) charge. The opposite side of the molecule then becomes partially positive (?+). The result is a temporary dipole. If this process occurs in two molecules that are close to one another, the two molecules will be attracted to each other, and will form a temporary, non-covalent bond.