Intermolecular Forces and Solubility
•Download as PPTX, PDF•
0 likes•1,576 views
The document discusses intermolecular forces and their effect on solubility. There are three main types of intermolecular forces: London dispersion forces, dipole-dipole interactions, and hydrogen bonding. London dispersion forces are the weakest, while hydrogen bonding is the strongest. Compounds with stronger intermolecular forces have higher melting and boiling points, making them more likely to be liquids or solids rather than gases.
Report
Share
Report
Share
Recommended
Tang 09 intermolecular forces and solubility
This document discusses intermolecular and intramolecular forces. It describes that intramolecular forces are the forces within a molecule that form covalent bonds. Intermolecular forces are the weaker forces between molecules and include London dispersion forces, dipole-dipole forces, and hydrogen bonding. London dispersion forces exist between all molecules and depend on the number of electrons. Dipole-dipole forces exist between polar molecules. Hydrogen bonding is the strongest intermolecular force and occurs when hydrogen is bonded to fluorine, oxygen, or nitrogen. Intermolecular forces influence properties such as melting point, boiling point, solubility, and surface tension.
Intermolecular forces
This document discusses intermolecular forces, which are the forces that act between molecules. There are five main types of intermolecular forces: ion-dipole forces, ion-induced dipole forces, dipole-dipole forces, dipole-induced dipole forces, and induced dipole forces. Intermolecular forces affect the properties of substances, such as their viscosity, density, melting and boiling points, thermal expansion, and thermal conductivity. Water has particularly strong hydrogen bonding intermolecular forces, which give it unique properties like a high heat of vaporization and large liquid range.
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.
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 force
This document discusses intramolecular and intermolecular forces. Intramolecular forces act within molecules and include covalent and ionic bonds. Intermolecular forces act between molecules and include dipole-dipole forces, dipole-induced dipole forces, London dispersion forces, and hydrogen bonding. These intermolecular forces determine physical properties like melting and boiling points, with stronger forces requiring more energy to overcome. Hydrogen bonding is the strongest type of intermolecular force and occurs when a hydrogen atom is bonded to a highly electronegative atom like fluorine, oxygen, or nitrogen.
01 intermolecular forces
This document discusses intermolecular forces (IMFs), the attractive forces between molecules that are weaker than intramolecular chemical bonds. It describes the main types of IMFs - London dispersion forces, dipole-dipole forces, and hydrogen bonding - and how their relative strengths depend on factors like molecular mass and polarity. IMFs determine key properties like a substance's boiling point, with stronger IMFs requiring more energy to overcome, resulting in higher boiling temperatures.
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.
intermolecular forces
This document defines and describes different types of intermolecular forces. It begins by defining intermolecular forces as weak attractive or repulsive forces between molecules due to their polarity. It then contrasts these with intramolecular forces like covalent bonds that hold molecules together. The document goes on to describe four main types of intermolecular forces - permanent dipoles, induced dipoles, dispersed dipoles, and hydrogen bonds. It provides examples to illustrate each type of intermolecular force.
Recommended
Tang 09 intermolecular forces and solubility
This document discusses intermolecular and intramolecular forces. It describes that intramolecular forces are the forces within a molecule that form covalent bonds. Intermolecular forces are the weaker forces between molecules and include London dispersion forces, dipole-dipole forces, and hydrogen bonding. London dispersion forces exist between all molecules and depend on the number of electrons. Dipole-dipole forces exist between polar molecules. Hydrogen bonding is the strongest intermolecular force and occurs when hydrogen is bonded to fluorine, oxygen, or nitrogen. Intermolecular forces influence properties such as melting point, boiling point, solubility, and surface tension.
Intermolecular forces
This document discusses intermolecular forces, which are the forces that act between molecules. There are five main types of intermolecular forces: ion-dipole forces, ion-induced dipole forces, dipole-dipole forces, dipole-induced dipole forces, and induced dipole forces. Intermolecular forces affect the properties of substances, such as their viscosity, density, melting and boiling points, thermal expansion, and thermal conductivity. Water has particularly strong hydrogen bonding intermolecular forces, which give it unique properties like a high heat of vaporization and large liquid range.
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.
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 force
This document discusses intramolecular and intermolecular forces. Intramolecular forces act within molecules and include covalent and ionic bonds. Intermolecular forces act between molecules and include dipole-dipole forces, dipole-induced dipole forces, London dispersion forces, and hydrogen bonding. These intermolecular forces determine physical properties like melting and boiling points, with stronger forces requiring more energy to overcome. Hydrogen bonding is the strongest type of intermolecular force and occurs when a hydrogen atom is bonded to a highly electronegative atom like fluorine, oxygen, or nitrogen.
01 intermolecular forces
This document discusses intermolecular forces (IMFs), the attractive forces between molecules that are weaker than intramolecular chemical bonds. It describes the main types of IMFs - London dispersion forces, dipole-dipole forces, and hydrogen bonding - and how their relative strengths depend on factors like molecular mass and polarity. IMFs determine key properties like a substance's boiling point, with stronger IMFs requiring more energy to overcome, resulting in higher boiling temperatures.
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.
intermolecular forces
This document defines and describes different types of intermolecular forces. It begins by defining intermolecular forces as weak attractive or repulsive forces between molecules due to their polarity. It then contrasts these with intramolecular forces like covalent bonds that hold molecules together. The document goes on to describe four main types of intermolecular forces - permanent dipoles, induced dipoles, dispersed dipoles, and hydrogen bonds. It provides examples to illustrate each type of intermolecular force.
Power Point Solids & Liquids
The document discusses intermolecular forces and phase changes. It defines intermolecular forces as attractive forces between molecules, such as hydrogen bonding, ion-dipole interactions, and dispersion forces. Stronger intermolecular forces result in higher boiling points, melting points, and densities when the substance is in liquid or solid form. The document also describes phase changes such as vaporization, melting, sublimation, and deposition that occur when varying temperature and pressure.
Intermolecular Forces
1. Molecular polarity depends on whether the bonds within a molecule are polar and the overall molecular geometry.
2. CO2 is nonpolar because its linear geometry causes the polar bonds between carbon and oxygen to cancel out. H2O is polar because its bent shape does not allow bond dipoles to cancel out.
3. Forces that hold substances together include ionic bonds, covalent networks, and intermolecular forces such as hydrogen bonding, dipole-dipole interactions, and London forces.
9 general types of intermolecular force
This document discusses different types of intermolecular forces that cause molecules to attract each other and exist in condensed phases as liquids and solids. It describes coulombic interactions between ions and partial charges on neutral molecules. Dipole-dipole attraction occurs between polar substances due to their uneven charge distributions. The strength of intermolecular forces determines a substance's state and increases with molecular polarity and mass. Specifically, it examines dipole-dipole interactions between polar molecules and hydrogen bonding as a special case of dipole attraction between molecules where hydrogen is bonded to highly electronegative atoms like F, N, and O.
Intermolecular Force
The document discusses intermolecular forces, liquids, and solids. It defines intermolecular forces as attractive forces between molecules, and describes different types including dipole-dipole forces, ion-dipole forces, and dispersion forces. Hydrogen bonding is discussed as a special type of dipole-dipole force. Solids are described as possessing rigid, long-range molecular order and defined unit cells, while liquids and amorphous solids lack long-range order.
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.
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.
Atomic combinations
The document discusses chemical bonding and atomic combinations. It explains that atoms form bonds to achieve stable electron configurations, and that there are different bond types including covalent and polar bonds. Valence shell electron pair repulsion theory is used to predict molecular shapes based on electron arrangements around central atoms. Bond properties like length, energy, and strength are also discussed.
Intermolecular forces
The document discusses intermolecular forces, the different types of intermolecular forces (dipole-dipole, ion-dipole, dispersion), and hydrogen bonding. It also covers properties of liquids related to intermolecular forces like surface tension, viscosity, and water's unusual properties. Finally, it discusses phases of matter, phase transitions, vapor pressure, boiling/melting points, and heat effects of phase changes.
Lecture 8.4c- Intermolecular Forces
1) Ammonia (NH3) is a polar molecule that has tetrahedral shape due to hydrogen bonding between nitrogen and hydrogen atoms.
2) Intermolecular forces include dipole-dipole interactions between polar molecules and London dispersion forces between all molecules.
3) Hydrogen bonding is a strong type of dipole-dipole interaction that occurs between molecules containing hydrogen bonded to nitrogen, oxygen, or fluorine.
Intermolecular forces
This document discusses the different types of intermolecular forces that exist between molecules, including permanent dipole-dipole interactions, van der Waals forces, and hydrogen bonding. It explains that van der Waals forces are the weakest intermolecular force and arise from the movement of electrons within molecules creating temporary dipoles that can attract neighboring molecules. The strength of van der Waals forces increases with more electrons in a molecule, which correlates with increasing boiling points among noble gases.
10 general type of intermolecular force
Loudon Despersion Force (LDF), also known as instantaneous dipole induced dipole, is the weakest type of intermolecular force that acts between all atoms and molecules. It results from the electrostatic attraction between ions and polar molecules that have dipoles, and is responsible for the properties of substances. LDF was fundamentally contributed to the understanding of chemical bonding and intermolecular forces by the Jewish physicist and professor Fritz London.
Intermolecular forces
✔Here is an introduction to the Chemistry of Life, where you will learn about Intermolecular forces. This presentation defines not only the term of intermolecular force but also intramolecular force. Three examples of intermolecular forces are presented. Those are dipole-dipole interactions, hydrogen bond, and the London dispersion force. Vivid examples of these three terms are also presented. ✔
Here is a video:
➡➡➡https://www.youtube.com/watch?v=UqIe6FPOWOA
Check out more interesting posts on LabGirl:
➡➡➡ https://www.facebook.com/labgirldzd
Thank you! :)
Chap 1-1 intra and intermolecular forces
Chromatography is a separation technique that exploits differences in how compounds partition between a stationary and mobile phase. Separation occurs based on differences in each compound's distribution constant (KD), which describes how much distributes into each phase. Key intermolecular forces like dipole-dipole interactions, hydrogen bonding, and dispersion forces affect KD values and thus chromatographic separation by influencing compound solubility and interactions. These same intermolecular forces also impact physical properties like boiling point.
Vander waals forces and its significance
The document discusses van der Waals forces, their characteristics, types (Keesom, Debye, London dispersion forces), and significance. Van der Waals forces are weak intermolecular forces between molecules caused by interactions between permanent or induced molecular dipoles. They are important in protein folding, graphite bonding, polymer formation, animal climbing/walking, and modern technologies that aim to mimic gecko adhesion.
Intermolecular Forces of Attraction
The document discusses intermolecular forces of attraction between molecules. It describes three main types of intermolecular forces: London forces, permanent dipoles, and hydrogen bonds. London forces are the weakest and result from instantaneous dipoles formed from electron motion. Permanent dipoles form from molecules with permanent charge separation. Hydrogen bonds are the strongest intermolecular forces and require a hydrogen atom bonded to a nitrogen, oxygen or fluorine. The type of intermolecular forces present influences the phase and properties of substances.
Intermolecular forces
The document discusses intermolecular forces and how they influence the properties of matter. It describes the main types of intermolecular forces - hydrogen bonding, dipole-dipole interactions, and London dispersion forces - and how they affect boiling points, melting points, and phase changes. Stronger intermolecular forces require more energy to overcome during changes of state from solid to liquid to gas.
Intermolecular Forces: London Dispersion Forces and Dipole-Dipole Attractions
Intermolecular Forces: London Dispersion Forces and Dipole-Dipole AttractionsShaina Mavreen Villaroza
Intermolecular Forces
Van der Waals Forces (Johannes van der Waals)
Dipole-Dipole Attractions (Polar)
Dispersion Forces (Nonpolar and Polar, induced dipole)
- Dipole-induced (London Dispersion)
- Ion-inducedForces Of Attraction
Forces of attraction include intramolecular and intermolecular forces. Intramolecular forces like ionic bonds and covalent bonds hold atoms together in molecules through electrostatic attraction or electron sharing. Intermolecular forces between molecules include hydrogen bonding, dipole-dipole interactions, and induced dipole forces from electron motion. These weaker forces influence melting/boiling points and physical states. Polar molecules form stronger intermolecular attractions than nonpolar molecules through orientations of their charge distributions.
2012 topic 4.3 intermolecular forces and physical properties
Intermolecular forces describe the attractions between particles in compounds and depend on the structure. Strong ionic, metallic and covalent bonds in complex structures result in high melting points and conductivity. Weaker van der Waals forces between simple molecules affect properties like boiling points, with polar molecules having higher points due to dipole interactions and hydrogen bonding.
DESCRIBE THE GENERAL TYPES OF INTERMOLECULAR FORCES
This document discusses different types of forces in physics and chemistry. In physics, a force requires an interaction between objects and can result in motion. There are two types of forces: contact and non-contact. In chemistry, forces can be either intramolecular, within elements combined, or intermolecular, between combined elements. Intramolecular forces include ionic bonding, covalent bonding, and metallic bonding. Intermolecular forces include dipole-dipole interactions, hydrogen bonding, and London dispersion forces. These intermolecular forces influence physical properties like melting point and boiling point.
Chemical Structure: Structure of Matter. Elements, Ions & Isotopes
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Tang 08 polarity
This document discusses molecular shape and polarity. It explains that a molecule's polarity depends on the presence of polar bonds and its overall shape. Polar bonds form when there is an unequal sharing of electrons between atoms. To determine a molecule's polarity, one must draw its Lewis structure, use VSEPR theory to predict its shape, determine if bonds are polar, then add bond dipoles. If dipoles cancel out, the molecule is nonpolar. If not, it is polar. Symmetry is also important - symmetrical molecules with identical bond polarities are nonpolar. Examples include the polar NH3 and nonpolar CO2 and symmetrical NF3.
More Related Content
What's hot
Power Point Solids & Liquids
The document discusses intermolecular forces and phase changes. It defines intermolecular forces as attractive forces between molecules, such as hydrogen bonding, ion-dipole interactions, and dispersion forces. Stronger intermolecular forces result in higher boiling points, melting points, and densities when the substance is in liquid or solid form. The document also describes phase changes such as vaporization, melting, sublimation, and deposition that occur when varying temperature and pressure.
Intermolecular Forces
1. Molecular polarity depends on whether the bonds within a molecule are polar and the overall molecular geometry.
2. CO2 is nonpolar because its linear geometry causes the polar bonds between carbon and oxygen to cancel out. H2O is polar because its bent shape does not allow bond dipoles to cancel out.
3. Forces that hold substances together include ionic bonds, covalent networks, and intermolecular forces such as hydrogen bonding, dipole-dipole interactions, and London forces.
9 general types of intermolecular force
This document discusses different types of intermolecular forces that cause molecules to attract each other and exist in condensed phases as liquids and solids. It describes coulombic interactions between ions and partial charges on neutral molecules. Dipole-dipole attraction occurs between polar substances due to their uneven charge distributions. The strength of intermolecular forces determines a substance's state and increases with molecular polarity and mass. Specifically, it examines dipole-dipole interactions between polar molecules and hydrogen bonding as a special case of dipole attraction between molecules where hydrogen is bonded to highly electronegative atoms like F, N, and O.
Intermolecular Force
The document discusses intermolecular forces, liquids, and solids. It defines intermolecular forces as attractive forces between molecules, and describes different types including dipole-dipole forces, ion-dipole forces, and dispersion forces. Hydrogen bonding is discussed as a special type of dipole-dipole force. Solids are described as possessing rigid, long-range molecular order and defined unit cells, while liquids and amorphous solids lack long-range order.
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.
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.
Atomic combinations
The document discusses chemical bonding and atomic combinations. It explains that atoms form bonds to achieve stable electron configurations, and that there are different bond types including covalent and polar bonds. Valence shell electron pair repulsion theory is used to predict molecular shapes based on electron arrangements around central atoms. Bond properties like length, energy, and strength are also discussed.
Intermolecular forces
The document discusses intermolecular forces, the different types of intermolecular forces (dipole-dipole, ion-dipole, dispersion), and hydrogen bonding. It also covers properties of liquids related to intermolecular forces like surface tension, viscosity, and water's unusual properties. Finally, it discusses phases of matter, phase transitions, vapor pressure, boiling/melting points, and heat effects of phase changes.
Lecture 8.4c- Intermolecular Forces
1) Ammonia (NH3) is a polar molecule that has tetrahedral shape due to hydrogen bonding between nitrogen and hydrogen atoms.
2) Intermolecular forces include dipole-dipole interactions between polar molecules and London dispersion forces between all molecules.
3) Hydrogen bonding is a strong type of dipole-dipole interaction that occurs between molecules containing hydrogen bonded to nitrogen, oxygen, or fluorine.
Intermolecular forces
This document discusses the different types of intermolecular forces that exist between molecules, including permanent dipole-dipole interactions, van der Waals forces, and hydrogen bonding. It explains that van der Waals forces are the weakest intermolecular force and arise from the movement of electrons within molecules creating temporary dipoles that can attract neighboring molecules. The strength of van der Waals forces increases with more electrons in a molecule, which correlates with increasing boiling points among noble gases.
10 general type of intermolecular force
Loudon Despersion Force (LDF), also known as instantaneous dipole induced dipole, is the weakest type of intermolecular force that acts between all atoms and molecules. It results from the electrostatic attraction between ions and polar molecules that have dipoles, and is responsible for the properties of substances. LDF was fundamentally contributed to the understanding of chemical bonding and intermolecular forces by the Jewish physicist and professor Fritz London.
Intermolecular forces
✔Here is an introduction to the Chemistry of Life, where you will learn about Intermolecular forces. This presentation defines not only the term of intermolecular force but also intramolecular force. Three examples of intermolecular forces are presented. Those are dipole-dipole interactions, hydrogen bond, and the London dispersion force. Vivid examples of these three terms are also presented. ✔
Here is a video:
➡➡➡https://www.youtube.com/watch?v=UqIe6FPOWOA
Check out more interesting posts on LabGirl:
➡➡➡ https://www.facebook.com/labgirldzd
Thank you! :)
Chap 1-1 intra and intermolecular forces
Chromatography is a separation technique that exploits differences in how compounds partition between a stationary and mobile phase. Separation occurs based on differences in each compound's distribution constant (KD), which describes how much distributes into each phase. Key intermolecular forces like dipole-dipole interactions, hydrogen bonding, and dispersion forces affect KD values and thus chromatographic separation by influencing compound solubility and interactions. These same intermolecular forces also impact physical properties like boiling point.
Vander waals forces and its significance
The document discusses van der Waals forces, their characteristics, types (Keesom, Debye, London dispersion forces), and significance. Van der Waals forces are weak intermolecular forces between molecules caused by interactions between permanent or induced molecular dipoles. They are important in protein folding, graphite bonding, polymer formation, animal climbing/walking, and modern technologies that aim to mimic gecko adhesion.
Intermolecular Forces of Attraction
The document discusses intermolecular forces of attraction between molecules. It describes three main types of intermolecular forces: London forces, permanent dipoles, and hydrogen bonds. London forces are the weakest and result from instantaneous dipoles formed from electron motion. Permanent dipoles form from molecules with permanent charge separation. Hydrogen bonds are the strongest intermolecular forces and require a hydrogen atom bonded to a nitrogen, oxygen or fluorine. The type of intermolecular forces present influences the phase and properties of substances.
Intermolecular forces
The document discusses intermolecular forces and how they influence the properties of matter. It describes the main types of intermolecular forces - hydrogen bonding, dipole-dipole interactions, and London dispersion forces - and how they affect boiling points, melting points, and phase changes. Stronger intermolecular forces require more energy to overcome during changes of state from solid to liquid to gas.
Intermolecular Forces: London Dispersion Forces and Dipole-Dipole Attractions
Intermolecular Forces: London Dispersion Forces and Dipole-Dipole AttractionsShaina Mavreen Villaroza
Intermolecular Forces
Van der Waals Forces (Johannes van der Waals)
Dipole-Dipole Attractions (Polar)
Dispersion Forces (Nonpolar and Polar, induced dipole)
- Dipole-induced (London Dispersion)
- Ion-inducedForces Of Attraction
Forces of attraction include intramolecular and intermolecular forces. Intramolecular forces like ionic bonds and covalent bonds hold atoms together in molecules through electrostatic attraction or electron sharing. Intermolecular forces between molecules include hydrogen bonding, dipole-dipole interactions, and induced dipole forces from electron motion. These weaker forces influence melting/boiling points and physical states. Polar molecules form stronger intermolecular attractions than nonpolar molecules through orientations of their charge distributions.
2012 topic 4.3 intermolecular forces and physical properties
Intermolecular forces describe the attractions between particles in compounds and depend on the structure. Strong ionic, metallic and covalent bonds in complex structures result in high melting points and conductivity. Weaker van der Waals forces between simple molecules affect properties like boiling points, with polar molecules having higher points due to dipole interactions and hydrogen bonding.
DESCRIBE THE GENERAL TYPES OF INTERMOLECULAR FORCES
This document discusses different types of forces in physics and chemistry. In physics, a force requires an interaction between objects and can result in motion. There are two types of forces: contact and non-contact. In chemistry, forces can be either intramolecular, within elements combined, or intermolecular, between combined elements. Intramolecular forces include ionic bonding, covalent bonding, and metallic bonding. Intermolecular forces include dipole-dipole interactions, hydrogen bonding, and London dispersion forces. These intermolecular forces influence physical properties like melting point and boiling point.
What's hot (20)
Intermolecular Forces: London Dispersion Forces and Dipole-Dipole Attractions
Intermolecular Forces: London Dispersion Forces and Dipole-Dipole Attractions
2012 topic 4.3 intermolecular forces and physical properties
2012 topic 4.3 intermolecular forces and physical properties
DESCRIBE THE GENERAL TYPES OF INTERMOLECULAR FORCES
DESCRIBE THE GENERAL TYPES OF INTERMOLECULAR FORCES
Viewers also liked
Chemical Structure: Structure of Matter. Elements, Ions & Isotopes
Lecture materials for the Introductory Chemistry course for Forensic Scientists, University of Lincoln, UK. See http://forensicchemistry.lincoln.ac.uk/ for more details.
Tang 08 polarity
This document discusses molecular shape and polarity. It explains that a molecule's polarity depends on the presence of polar bonds and its overall shape. Polar bonds form when there is an unequal sharing of electrons between atoms. To determine a molecule's polarity, one must draw its Lewis structure, use VSEPR theory to predict its shape, determine if bonds are polar, then add bond dipoles. If dipoles cancel out, the molecule is nonpolar. If not, it is polar. Symmetry is also important - symmetrical molecules with identical bond polarities are nonpolar. Examples include the polar NH3 and nonpolar CO2 and symmetrical NF3.
IB Chemistry on Polarity, Hydrogen Bonding and Van Der Waals forces
- Ionic bonds form when a metal transfers an electron to a nonmetal, forming positive and negative ions.
- Covalent bonds form when atoms share electrons, either equally in nonpolar covalent bonds or unequally in polar covalent bonds.
- The electronegativity difference between bonded atoms determines bond polarity.
The different Biomolecules
This document discusses the key biomolecules found in living things: carbohydrates, lipids, proteins, and nucleic acids. It explains that carbohydrates like sugars, starches, and cellulose are used for energy storage and as structural components. Lipids such as fats and oils store energy and make up cell membranes. Proteins have many functions like structure, movement, defense, and catalysis as enzymes. Nucleic acids DNA and RNA carry genetic information and enable inheritance and protein synthesis. The four main biomolecules all contain the elements carbon, hydrogen, oxygen, and nitrogen arranged into larger structures that allow life.
Formation of Light and Heavy Elements
There were three main processes that led to the formation of elements:
1) Primordial nucleosynthesis formed light elements like hydrogen and helium shortly after the Big Bang due to the extremely high temperatures.
2) Stellar nucleosynthesis fused lighter elements inside stars, producing heavier elements up to iron through processes like the carbon cycle and triple alpha process.
3) Supernovae were needed to form elements heavier than iron via neutron capture reactions, as these require more energy than can be provided by fusion alone.
Media and Information Literacy (MIL) - 1. Introduction to Media and Informati...
Introduction to Media and Information Literacy (Part 1)
The learners will be able to…
1. describe the nature of communication and the concepts related to it (SSHS);
2. describe how communication is affected by media and information (MIL11/12IMIL-IIIa and
3. identify the similarities and differences of media literacy, information literacy, and technology literacy (MIL11/12IMIL-IIIa-2).
Topic Outline
I- Introduction to Media and Information Literacy
A- Communication
1. Definitions
2. Communication Models
3. How Media and Information affect Communication
4. Media Literacy, Information Literacy, Technology (Digital) Literacy
Viewers also liked (6)
Chemical Structure: Structure of Matter. Elements, Ions & Isotopes
Chemical Structure: Structure of Matter. Elements, Ions & Isotopes
IB Chemistry on Polarity, Hydrogen Bonding and Van Der Waals forces
IB Chemistry on Polarity, Hydrogen Bonding and Van Der Waals forces
Media and Information Literacy (MIL) - 1. Introduction to Media and Informati...
Media and Information Literacy (MIL) - 1. Introduction to Media and Informati...
Similar to Intermolecular Forces and Solubility
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.
intermolecular_forces.pptx
Intermolecular forces
Chemical bonding
Chemical structure
van der Vaal force
electrons, dipole interaction,
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.
grade 12 week 2.pptx
The document discusses different types of intermolecular forces including London dispersion forces, dipole-dipole interactions, and hydrogen bonding. It explains that these intermolecular forces determine properties of liquids and solids, such as melting and boiling points, as they must be overcome for phase changes to occur. The forces arise from electrostatic interactions between charged regions in molecules. Hydrogen bonding is a particularly strong form of dipole-dipole interaction.
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.
11.2 intermolecular forces
This document discusses intermolecular forces, which are forces that exist between molecules. It describes the different types of intermolecular forces - dipole-dipole interactions, hydrogen bonding, and London dispersion forces. Stronger intermolecular forces result in higher boiling points and melting points, causing a substance to be a solid at room temperature rather than a gas or liquid. Ionic compounds have even stronger attractions between ions and thus higher melting points than molecular compounds held together by intermolecular forces.
Intermolecular Forces are foces actingwithin a molecule.You should.pdf
Intermolecular Forces are foces actingwithin a molecule.
You should first note whehter the molecule is metallic, ionicor covalent.
There are three different types of Intermolecular Forces thatapplies for covalent molecules:
Dispersion force,Dipole-dipole interactions and hydrogen bonds.
The relative strength of these forces are: dispersion forces< dipole-dipole interactions <
hydrogen bonds
Hence, dispersion forces are the weakest and hydrogen bondsare the strongest.
Dispersion forces (aka. van der Waals Forceor London Force) are for non-polarmolecules.Non-
polar molecules have no dipoles, or the dipoledoesn\'t extend throughout the molecule, and only
dispersion forces.They are generally don\'t mix with water, and are usually anyelement and
carbon compounds.
For example:Cl2,CO2,N2O4,CH4
Dipole-Dipole forces occur between moleculesthat have permanent net dipoles, (hencepolar
molecules)
Polar molecules usually have a dipole and may contain a highlyelectronegative element bonded
to hydrogen, allowing hydrogenbonding. They are also usually soluble in water.
For example: SCl2 , PCl3,CH3Cl
Hydrogen Bonds occur between molecules thathave permanent net dipole resulting from
hydrogen beingcovalently bonded to either fluorine, oxygen ornitrogen.
For example: HF, H2O, H2O2 ,CH3OH, CH3COOH,CH3NH2
These forces operate between covalentmolecules.
As for your answer,
Na+: Dispersion
H3C-CH3: Dispersion
K2O : Ionic Bond
H2O: Hydrogen bonding, the hydrogen has a verylow electronegativety resulting in the oxygen
atoms having greateraffinity to the covalently shared electrons.
NH3 : polar, hence dipole-dipole and hydrogenbonding, since the hydrogen is slightly +ve and
the nitrogenslightly -ve. There more electronegative nitrogen pulls thehydrogen electron towards
it, giving a dipole moment .
Ne: non polar, hence dispersion forces only(randomness of electron clouds instantaneously
causes oppositecharges at the ends of the molecule which induces the same effectin another)
If you want to learn more, this site might help:
http://science.uwaterloo.ca/~cchieh/cact/c123/intermol.html
Solution
Intermolecular Forces are foces actingwithin a molecule.
You should first note whehter the molecule is metallic, ionicor covalent.
There are three different types of Intermolecular Forces thatapplies for covalent molecules:
Dispersion force,Dipole-dipole interactions and hydrogen bonds.
The relative strength of these forces are: dispersion forces< dipole-dipole interactions <
hydrogen bonds
Hence, dispersion forces are the weakest and hydrogen bondsare the strongest.
Dispersion forces (aka. van der Waals Forceor London Force) are for non-polarmolecules.Non-
polar molecules have no dipoles, or the dipoledoesn\'t extend throughout the molecule, and only
dispersion forces.They are generally don\'t mix with water, and are usually anyelement and
carbon compounds.
For example:Cl2,CO2,N2O4,CH4
Dipole-Dipole forces occur between moleculesthat have permanent net dipoles, (hencepolar
molecu.
L4- Intermolecular Forces of Attraction.pptx
There are three main types of intermolecular forces of attraction: London dispersion forces, dipole-dipole forces, and hydrogen bonds. London dispersion forces exist in all molecules and result from fluctuations in electron distribution. Dipole-dipole forces exist in polar molecules with permanent charge distributions. Hydrogen bonds are strong dipole-dipole interactions between a hydrogen and an electronegative atom like nitrogen, oxygen, or fluorine. These intermolecular forces affect phase changes from solid to liquid to gas as the relative strengths decrease.
intermolecular forces.pdf
Intermolecular Forces
Definition
Intermolecular forces are the forces of attraction that exist between molecules. These forces play a crucial role in determining the physical and chemical properties of substances, such as boiling points, melting points, solubility, and viscosity.
Intermolecular Forces
The three main types of intermolecular forces are:
London dispersion forces (also known as Van der Waals forces): These forces are present in all molecules, whether they are polar or nonpolar. They arise due to temporary fluctuations in electron distribution, creating temporary dipoles. These temporary dipoles induce dipoles in neighboring molecules, resulting in attractive forces. London dispersion forces increase with increasing molecular size and shape. Substances with stronger London dispersion forces tend to have higher boiling points and melting points.
London Dispersion force
London dispersion forces are the weakest intermolecular forces.
They occur due to temporary fluctuations in electron distribution within molecules, creating temporary dipoles.
These temporary dipoles induce dipoles in neighboring molecules, resulting in attractive forces.
London dispersion forces increase with increasing molecular size and shape.
Substances with stronger London dispersion forces tend to have higher boiling points and melting points.
Examples of substances with predominant London dispersion forces include noble gases like helium and nonpolar molecules like hydrocarbons.
2 .Dipole-dipole interactions: These forces occur between polar molecules. They arise due to the attraction between the positive end of one polar molecule and the negative end of another polar molecule. Dipole-dipole interactions are stronger than London dispersion forces and contribute significantly to the physical properties of polar substances
.
Dipole dipole interaction
Polar molecules have an uneven distribution of electron density, resulting in a permanent dipole moment.
The positive end of one polar molecule is attracted to the negative end of another polar molecule.
Dipole-dipole interactions are stronger than London dispersion forces.
These forces contribute significantly to the physical properties of polar substances.
Examples of substances with predominant dipole-dipole interactions include hydrogen chloride (HCl) and water (H2O).
3.Hydrogen bonding: This is a special type of dipole-dipole interaction that occurs when a hydrogen atom is bonded to a highly electronegative atom (such as nitrogen, oxygen, or fluorine) and is also attracted to another electronegative atom in a different molecule. Hydrogen bonding is exceptionally strong compared to other intermolecular forces and has a significant impact on the properties of substances. It is responsible for many unique properties of water, such as its high boiling point, surface tension, and the ability to form ice with a lower density than liquid water.
Chapter 11
The document discusses intermolecular forces, which are the attractions between molecules. It describes the different types of intermolecular forces including dipole-dipole interactions, hydrogen bonding, and London dispersion forces. It explains how these intermolecular forces influence various physical properties of substances like boiling point, viscosity, surface tension, and phase changes. The document also discusses how intermolecular forces relate to states of matter and phase diagrams.
Binding forces SB
States of Matter, Intermolecular forces, Van der Waals Forces, Keesom, Diapole-Diapole interaction, Debye forces, London forces, Hydrogen bond
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.
Intermolecular forces- Organic Chemistry
The document discusses different types of intramolecular and intermolecular forces. It describes ionic bonds as the strong electrostatic attraction between oppositely charged ions. Covalent bonds are described as the sharing of electron pairs between atoms. It also discusses hydrogen bonding, dipole-dipole interactions, and van der Waals forces as different types of intermolecular forces that are weaker than ionic or covalent bonds.
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.
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
The document discusses different types of intermolecular forces including London dispersion forces, dipole-dipole forces, dipole-induced dipole forces, ion-dipole interactions, and hydrogen bonding. It provides examples of how these forces influence the properties of substances such as their melting and boiling points. Hydrogen bonding specifically is described as being an important intermolecular force that influences the properties of water, alcohols, and other polar molecules.
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.
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.ppt
This document discusses intramolecular and intermolecular forces. It defines intramolecular forces as those within a molecule that hold atoms together, such as ionic, covalent, and metallic bonds. Intermolecular forces are weaker forces between molecules, including dipole-dipole, ion-dipole, hydrogen bonding, and London dispersion forces. The document explains each type of intramolecular and intermolecular force in more detail and notes that intramolecular bonds are stronger than intermolecular forces.
intermolecular_forces.ppt
This document discusses intramolecular and intermolecular forces. It defines intramolecular forces as those within a molecule that hold atoms together, such as ionic, covalent, and metallic bonds. Intermolecular forces are weaker forces between molecules, including dipole-dipole, ion-dipole, hydrogen bonding, and London dispersion forces. The document explains each type of intramolecular and intermolecular force in more detail and notes that intramolecular bonds are stronger than intermolecular forces.
Similar to Intermolecular Forces and Solubility (20)
10intermolecularforcesofattraction2-170909132616 (1).pptx
10intermolecularforcesofattraction2-170909132616 (1).pptx
Intermolecular Forces are foces actingwithin a molecule.You should.pdf
Intermolecular Forces are foces actingwithin a molecule.You should.pdf
Dipole-dipole forces are attractive forces between the positive end .pdf
Dipole-dipole forces are attractive forces between the positive end .pdf
Recently uploaded
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...Nguyen Thanh Tu Collection
https://app.box.com/s/tacvl9ekroe9hqupdnjruiypvm9rdaneJemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"National Information Standards Organization (NISO)
This presentation was provided by Racquel Jemison, Ph.D., Christina MacLaughlin, Ph.D., and Paulomi Majumder. Ph.D., all of the American Chemical Society, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh - RAYH...
Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh
How to deliver Powerpoint Presentations.pptx
"How to make and deliver dynamic presentations by making it more interactive to captivate your audience attention"
Walmart Business+ and Spark Good for Nonprofits.pdf
"Learn about all the ways Walmart supports nonprofit organizations.
You will hear from Liz Willett, the Head of Nonprofits, and hear about what Walmart is doing to help nonprofits, including Walmart Business and Spark Good. Walmart Business+ is a new offer for nonprofits that offers discounts and also streamlines nonprofits order and expense tracking, saving time and money.
The webinar may also give some examples on how nonprofits can best leverage Walmart Business+.
The event will cover the following::
Walmart Business + (https://business.walmart.com/plus) is a new shopping experience for nonprofits, schools, and local business customers that connects an exclusive online shopping experience to stores. Benefits include free delivery and shipping, a 'Spend Analytics” feature, special discounts, deals and tax-exempt shopping.
Special TechSoup offer for a free 180 days membership, and up to $150 in discounts on eligible orders.
Spark Good (walmart.com/sparkgood) is a charitable platform that enables nonprofits to receive donations directly from customers and associates.
Answers about how you can do more with Walmart!"
How to Make a Field Mandatory in Odoo 17
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
BIOLOGY NATIONAL EXAMINATION COUNCIL (NECO) 2024 PRACTICAL MANUAL.pptx
Practical manual for National Examination Council, Nigeria.
Contains guides on answering questions on the specimens provided
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
The History of NZ 1870-1900.
Making of a Nation.
From the NZ Wars to Liberals,
Richard Seddon, George Grey,
Social Laboratory, New Zealand,
Confiscations, Kotahitanga, Kingitanga, Parliament, Suffrage, Repudiation, Economic Change, Agriculture, Gold Mining, Timber, Flax, Sheep, Dairying,
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UP
This Dissertation explores the particular circumstances of Mirzapur, a region located in the
core of India. Mirzapur, with its varied terrains and abundant biodiversity, offers an optimal
environment for investigating the changes in vegetation cover dynamics. Our study utilizes
advanced technologies such as GIS (Geographic Information Systems) and Remote sensing to
analyze the transformations that have taken place over the course of a decade.
The complex relationship between human activities and the environment has been the focus
of extensive research and worry. As the global community grapples with swift urbanization,
population expansion, and economic progress, the effects on natural ecosystems are becoming
more evident. A crucial element of this impact is the alteration of vegetation cover, which plays a
significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
these activities. As the most crucial natural resource, its utilization by humans results in different
'Land uses,' which are determined by both human activities and the physical characteristics of the
land.
The utilization of land is impacted by human needs and environmental factors. In countries
like India, rapid population growth and the emphasis on extensive resource exploitation can lead
to significant land degradation, adversely affecting the region's land cover.
Therefore, human intervention has significantly influenced land use patterns over many
centuries, evolving its structure over time and space. In the present era, these changes have
accelerated due to factors such as agriculture and urbanization. Information regarding land use and
cover is essential for various planning and management tasks related to the Earth's surface,
providing crucial environmental data for scientific, resource management, policy purposes, and
diverse human activities.
Accurate understanding of land use and cover is imperative for the development planning
of any area. Consequently, a wide range of professionals, including earth system scientists, land
and water managers, and urban planners, are interested in obtaining data on land use and cover
changes, conversion trends, and other related patterns. The spatial dimensions of land use and
cover support policymakers and scientists in making well-informed decisions, as alterations in
these patterns indicate shifts in economic and social conditions. Monitoring such changes with the
help of Advanced technologies like Remote Sensing and Geographic Information Systems is
crucial for coordinated efforts across different administrative levels. Advanced technologies like
Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
structure of plant communities across different temporal and spatial scales. These changes can
occur natural.
How to Setup Warehouse & Location in Odoo 17 Inventory
In this slide, we'll explore how to set up warehouses and locations in Odoo 17 Inventory. This will help us manage our stock effectively, track inventory levels, and streamline warehouse operations.
مصحف القراءات العشر أعد أحرف الخلاف سمير بسيوني.pdf
مصحف أحرف الخلاف للقراء العشرةأعد أحرف الخلاف بالتلوين وصلا سمير بسيوني غفر الله له
The History of Stoke Newington Street Names
Presented at the Stoke Newington Literary Festival on 9th June 2024
www.StokeNewingtonHistory.com
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/y977uz6bpd3af4qsebv7r9b7s21935vdRecently uploaded (20)
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
SWOT analysis in the project Keeping the Memory @live.pptx
SWOT analysis in the project Keeping the Memory @live.pptx
Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh - RAYH...
Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh - RAYH...
Walmart Business+ and Spark Good for Nonprofits.pdf
Walmart Business+ and Spark Good for Nonprofits.pdf
Film vocab for eal 3 students: Australia the movie
Film vocab for eal 3 students: Australia the movie
BIOLOGY NATIONAL EXAMINATION COUNCIL (NECO) 2024 PRACTICAL MANUAL.pptx
BIOLOGY NATIONAL EXAMINATION COUNCIL (NECO) 2024 PRACTICAL MANUAL.pptx
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UP
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UP
How to Setup Warehouse & Location in Odoo 17 Inventory
How to Setup Warehouse & Location in Odoo 17 Inventory
مصحف القراءات العشر أعد أحرف الخلاف سمير بسيوني.pdf
مصحف القراءات العشر أعد أحرف الخلاف سمير بسيوني.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...
Intermolecular Forces and Solubility
- 1. Tuesday review session October 4, 2010 Intermolecular Forces and Solubility
- 2. Intermolecular Forces Definition: Forces between molecules Intermolecular forces are much weaker than intramolecular forces There are three different types London Dispersion Forces/ Van der Waals Dipole-Dipole Interactions Hydrogen Bonds
- 3. London Dispersion Forces Also referred to as Van der Waals forces Occurs because of momentary dipole (uneven distributions of electrons in a molecule causing a partially negative end and a partially positive end) These are the weakest intermolecular forces
- 4. Dipole-Dipole Interactions Occurs when polar molecules align so that their oppositely charged ends are attract each other This bond is stronger than Van der Waals forces
- 5. Hydrogen Bonding A type of dipole-dipole bond that occurs when hydrogen is bonded to a highly electronegative atom (O, F, N) This is the strongest intermolecular force
- 6. Intermolecular Forces Trends Compounds with stronger intermolecular forces will be harder to separate therefore they will have larger melting points and boiling points This means compounds with weak intermolecular forces are more likely to be found in gaseous form, while compounds with stronger molecular forces are more likely to be found as liquids or solids