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Dipole Chemistry

Dipole Chemistry

Up until now, you have probably heard that water has many cool properties such as being polar, having cohesive and adhesive forces, and being a great solvent! But, what you ever heard about water being a dipole and wondered what exactly that means? If your answer is yes, you came to the right place!

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A _____ is a molecule that has a separation of charges.

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True or false: Dipoles occur when electrons are shared unequally between atoms due to a high difference in the electronegativity of the atoms involved.

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The formation of a dipole depends on the polarity of a bond, which is determined by the difference in ______ between the two atoms involved in the bond.

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_____ is the ability of an atom to attract electrons to itself.

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In ______ bonds, the electrons are equally shared between atoms.

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In ______, the electrons are shared unequally between atoms.

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______ do not have dipoles because they cancel out due to symmetry.

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In polar covalent bonds, dipoles are _____ present.

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True or false: Electronegativity decreases from left to right and decreases down a group.

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If the difference in electronegativity is _____ then the molecule will a non-polar covalent bond

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If the difference in electronegativity is ______ then the molecule will have a polar covalent bond

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A _____ is a molecule that has a separation of charges.

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True or false: Dipoles occur when electrons are shared unequally between atoms due to a high difference in the electronegativity of the atoms involved.

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Mo

The formation of a dipole depends on the polarity of a bond, which is determined by the difference in ______ between the two atoms involved in the bond.

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Mo

_____ is the ability of an atom to attract electrons to itself.

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In ______ bonds, the electrons are equally shared between atoms.

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In ______, the electrons are shared unequally between atoms.

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______ do not have dipoles because they cancel out due to symmetry.

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In polar covalent bonds, dipoles are _____ present.

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True or false: Electronegativity decreases from left to right and decreases down a group.

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If the difference in electronegativity is _____ then the molecule will a non-polar covalent bond

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If the difference in electronegativity is ______ then the molecule will have a polar covalent bond

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Last Updated: 12.11.2022
Published at: 26.05.2022
10 min reading time

Chemical Analysis
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Absolute Entropy And Entropy Change
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Acids and Bases
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Amount of Substance
Application of Le Chatelier's Principle
Arrhenius Equation
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Properties of Water
Quantitative Electrolysis
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RICE Tables
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Reacting Masses
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Real Gas
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Reversible Reaction
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Water in Chemical Reactions
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Weak Acids and Bases
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pH Scale
pH and Solubility
pH and pKa
pH and pOH

The Earths Atmosphere

Contents

Chemical Analysis
Chemical Reactions
Chemistry Branches
Inorganic Chemistry
Ionic and Molecular Compounds
Kinetics
Making Measurements
Nuclear Chemistry
Organic Chemistry
Physical Chemistry

Absolute Entropy And Entropy Change
Acid Dissociation Constant
Acid-Base Indicators
Acid-Base Reactions and Buffers
Acids and Bases
Alkali Metals
Allotropes of Carbon
Amorphous Polymer
Amount of Substance
Application of Le Chatelier's Principle
Arrhenius Equation
Arrhenius Theory
Atom Economy
Atomic Structure
Autoionization of Water
Avogadro Constant
Avogadro's Number and the Mole
Beer-Lambert Law
Bond Enthalpy
Bonding
Born Haber Cycles
Born-Haber Cycles Calculations
Boyle's Law
Brønsted-Lowry Acids and Bases
Buffer Capacity
Buffer Solutions
Buffers
Buffers Preparation
Calculating Enthalpy Change
Calculating Equilibrium Constant
Calorimetry
Carbon Structures
Cell Potential
Cell Potential and Free Energy
Chalcogens
Chemical Calculations
Chemical Equations
Chemical Equilibrium
Chemical Thermodynamics
Closed Systems
Colligative Properties
Collision Theory
Common-Ion Effect
Composite Materials
Composition of Mixture
Constant Pressure Calorimetry
Constant Volume Calorimetry
Coordination Compounds
Coupling Reactions
Covalent Bond
Covalent Network Solid
Crystalline Polymer
De Broglie Wavelength
Determining Rate Constant
Deviation From Ideal Gas Law
Diagonal Relationship
Diamond
Dilution
Dipole Chemistry
Dipole Moment
Dissociation Constant
Distillation
Dynamic Equilibrium
Electric Fields Chemistry
Electrochemical Cell
Electrochemical Series
Electrochemistry
Electrode Potential
Electrolysis
Electrolytes
Electromagnetic Spectrum
Electron Affinity
Electron Configuration
Electron Shells
Electronegativity
Electronic Transitions
Elemental Analysis
Elemental Composition of Pure Substances
Empirical and Molecular Formula
Endothermic and Exothermic Processes
Energetics
Energy Diagrams
Enthalpy Changes
Enthalpy For Phase Changes
Enthalpy of Formation
Enthalpy of Reaction
Enthalpy of Solution and Hydration
Entropy
Entropy Change
Equilibrium Concentrations
Equilibrium Constant Kp
Equilibrium Constants
Examples of Covalent Bonding
Factors Affecting Reaction Rates
Finding Ka
Free Energy
Free Energy Of Dissolution
Free Energy and Equilibrium
Free Energy of Formation
Fullerenes
Fundamental Particles
Galvanic and Electrolytic Cells
Gas Constant
Gas Solubility
Gay Lussacs Law
Giant Covalent Structures
Graham's Law
Graphite
Ground State
Group 3A
Group 4A
Group 5A
Half Equations
Heating Curve for Water
Heisenberg Uncertainty Principle
Henderson-Hasselbalch Equation
Hess' Law
Hybrid Orbitals
Hydrogen Bonds
Ideal Gas Law
Ideal and Real Gases
Intermolecular Forces
Introduction to Acids and Bases
Ion And Atom Photoelectron Spectroscopy
Ion dipole Forces
Ionic Bonding
Ionic Product of Water
Ionic Solids
Ionisation Energy
Ions: Anions and Cations
Isotopes
Kinetic Molecular Theory
Lattice Structures
Law of Definite Proportions
Le Chatelier's Principle
Lewis Acid and Bases
London Dispersion Forces
Magnitude Of Equilibrium Constant
Mass Spectrometry
Mass Spectrometry of Elements
Maxwell-Boltzmann Distribution
Measuring EMF
Mechanisms of Chemical Bonding
Melting and Boiling Point
Metallic Bonding
Metallic Solids
Metals Non-Metals and Metalloids
Mixtures and Solutions
Molar Mass Calculations
Molarity
Molecular Orbital Theory
Molecular Solid
Molecular Structures of Acids and Bases
Moles and Molar Mass
Nanoparticles
Neutralisation Reaction
Oxidation Number
Partial Pressure
Particulate Model
Partition Coefficient
Percentage Yield
Periodic Table Organization
Phase Changes
Phase Diagram of Water
Photoelectric Effect
Photoelectron Spectroscopy
Physical Properties
Polarity
Polyatomic Ions
Polyprotic Acid Titration
Prediction of Element Properties Based on Periodic Trends
Pressure and Density
Properties Of Equilibrium Constant
Properties of Buffers
Properties of Solids
Properties of Water
Quantitative Electrolysis
Quantum Energy
Quantum Numbers
RICE Tables
Rate Equations
Rate of Reaction and Temperature
Reacting Masses
Reaction Quotient
Reaction Quotient And Le Chateliers Principle
Real Gas
Redox
Relative Atomic Mass
Representations of Equilibrium
Reversible Reaction
SI units chemistry
Saturated Unsaturated and Supersaturated
Shapes of Molecules
Shielding Effect
Simple Molecules
Solids Liquids and Gases
Solubility
Solubility Curve
Solubility Equilibria
Solubility Product
Solubility Product Calculations
Solutes Solvents and Solutions
Solution Representations
Solutions and Mixtures
Specific Heat
Spectroscopy
Standard Potential
States of Matter
Stoichiometry In Reactions
Strength of Intermolecular Forces
The Laws of Thermodynamics
The Molar Volume of a Gas
Thermodynamically Favored
Trends in Ionic Charge
Trends in Ionisation Energy
Types of Mixtures
VSEPR Theory
Valence Electrons
Van der Waals Forces
Vapor Pressure
Water in Chemical Reactions
Wave Mechanical Model
Weak Acid and Base Equilibria
Weak Acids and Bases
Writing Chemical Formulae
pH
pH Change
pH Curves and Titrations
pH Scale
pH and Solubility
pH and pKa
pH and pOH

The Earths Atmosphere

Contents

Fact Checked Content
Last Updated: 12.11.2022
10 min reading time

Content creation process designed by Lily Hulatt
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Jump to a key chapter

First, we will talk about the definition of a dipole and how dipoles are formed.
Then, we will dive into the different types of dipoles in chemistry and give some examples.

Dipole Definition in Chemistry

Dipoles occur when electrons are shared unequally between atoms in the same molecule due to a high difference in the electronegativity of the atoms involved.

A dipole is a molecule or covalent bond that has a separation of charges.

Determination and Formation of a Dipole

The formation of a dipole depends on the polarity of a bond, which is determined by the difference in electronegativity between the two atoms involved in the bond.

Electronegativity is the ability of an atom to attract electrons to itself.

Types of Bonds

The three types of bonds you should be familiar with are non-polar covalent bonds, polar covalent bonds, and ionic bonds.

In non-polar covalent bonds, the electrons are equally shared between atoms. In polar covalent bonds, the electrons are shared unequally between atoms. In ionic bonds, the electrons are transferred.

In ionic bonds, there are no dipoles.
In polar covalent bonds, dipoles are always present.
Non-polar covalent bonds do have dipoles but they cancel out due to symmetry.

Predicting Bond Polarity

To determine whether a bond is nonpolar covalent, polar covalent, or ionic, we need to look at the electronegativity values of the atoms involved and calculate the difference between them.

If the difference in electronegativity is less than 0.4 → non-polar covalent bond
If the difference in electronegativity falls between 0.4 and 1.7 → polar covalent bond
If the difference in electronegativity is greater than 1.7 → ionic bond

The electronegativity values are given by Pauling's scale of electronegativity. In the periodic table below, we can see the electronegativity values for each element. Notice the trend here: electronegativity increases from left to right and decreases down a group.

Dipoles, Electronegativity Determination and formation of a dipole, StudySmarter

Fig.1-Periodic table showing Pauling's scale of electronegativity

Let's look at an example!

Predict the type of bond polarity between the following atoms:

a) H and Br

H has an EN value of 2.20 and Br has an EN of 2.96. The electronegativity difference between these atoms is 0.76 so it would have a polar covalent bond.

b) Li and F

Li has an EN value of 0.98 and F has an EN of 3.98. The electronegativity difference is 3.00 so it would have an ionic bond.

c) I and I

I has an EN value of 2.66. The electronegativity difference is 0.00 so it would have anon-polar covalent bond.

Dipole Moment in Chemistry

To measure the separation of charges in a molecule we use dipole moment. Dipole moments are present in polar molecules that have asymmetric shapes because, in asymmetric shapes, the dipoles do not cancel out.

Dipole moment is referred to as a measurement of the magnitude of a dipole.

To show the dipole moment, we use arrows pointing toward the more electronegative element. For example, in the figure below we can see an HCl and an SO3 molecule.

In HCl, chlorine has a higher electronegativity value compared to hydrogen. So, the chlorine will have a partial negative charge and the hydrogen will have a partial positive charge. Since chlorine is more electronegative, the dipole arrow will point towards chlorine.
In SO3, the oxygen atom has an electronegativity value higher than that of the sulfur atoms. So, the sulfur atom will have a partial positive charge and the oxygen atoms will have a partial negative charge. In this molecule, the symmetry causes the dipoles to cancel each other out. So, SO3 has no dipole moment.

Dipole moment of a bond can be calculated by using the following equation: μ=Q*r→ where Q is the magnitude of the partial charges δ+ and δ- , and r is the distance vector between the two charges. You can think of the distance vector as an arrow with pointing to the more electron-negative element from the less electron negative one. Dipole moment is measured in Debye units (D). The bigger the dipole moment of the bond, the more polar the bond is.

A dipole moment of a molecule is the sum of the dipole moments of the bonds. This is why it is important that we are using vectors. Vectors have a property called directionality, meaning they point from somewhere to somewhere. You see if two vectors are equally long and point in the opposite direction ( + and -) their sum will be zero. So in theory, if the molecule is perfectly symmetric, meaning all vectors will add up to 0 the dipole moment of the whole molecule will be zero. Okay, let's take a look at an example.

You can learn more about the different molecular shapes by reading "Valence Shell Electron Pair Repulsion (VSEPR) Theory.

Which of the following compounds has a dipole moment? PCl3 or PCl5?

First, we need to take a look at their lewis structures. If the structure is symmetrical, then the dipoles will cancel out and the compound will not have a dipole.

In PCl3, the bond is polar because of the difference in electronegativity between P and Cl atoms, and the presence of a lone pair of electrons gives PCl3 a tetrahedral structure.

On the other hand, PCl5 is considered non-polar because its symmetrical shape, which is trigonal bipyramidal, cancels the dipoles out.

Dipoles, Lewis diagrams of phosphorus trichloride and phosphorus pentachloride, StudySmarter Fig.2-Lewis diagrams of phosphorus trichloride and phosphorus pentachloride

If you need to go back and learn how to draw Lewis structures, check out "Lewis Diagrams".

Types of Dipole in Chemistry

The three types of dipole interactions you might encounter are called ion-dipole, dipole-dipole, and induced-dipole induced-dipole (London dispersion forces).

Ion-Dipole

An ion-dipole interaction occurs between an ion and a polar (dipole) molecule. The higher the ion charge, the stronger the ion-dipole attractive force is. An example of ion-dipole is sodium ion in water.

Dipoles, ion dipole forces holding sodium ion and water, StudySmarter Fig.3-Ion-dipole forces holding sodium ion and water

Another type of interaction involving ions is ion-induced dipole force. This interaction occurs when a charged ion induces a temporary dipole in a non-polar molecule. For example, Fe3+ can induce a temporary dipole in O2, giving rise to an ion-induced dipole interaction!

So what does it mean to induce a dipole? If you put an ion near a non-polar molecule, you can start affecting its electrons. For example, a positive ion will attract these electrons to the side on which the ion is. This will create a larger concentration of ions there and lead to a dipole forming on the originally non-polar molecule.

Dipole-Dipole

When two polar molecules possessing permanent dipoles are near each other, attractive forces called dipole-dipole interactions hold the molecules together. Dipole-dipole interactions are attractive forces that occur between the positive end of a polar molecular and the negative end of another polar molecule. A common example of dipole-dipole forces is seen between HCl molecules. In HCl, the partial positive H atoms get attracted to the partial negative Cl atoms of another molecule.

Dipoles, ion dipole-dipole forces between HCl molecules, StudySmarter Fig.4-Dipole-dipole forces between HCl molecules

Hydrogen Bonding

A special type of dipole-dipole interaction is hydrogen bonding. Hydrogen bonding is an intermolecular force that occurs between the hydrogen atom covalently bonded to an N, O, or F and another molecule containing N, O, or F. For example, in water (H2O), the H atom covalently bonded to oxygen gets attracted to the oxygen of another water molecule, creating hydrogen bonding.

Dipoles, hydrogen bonding between water molecules, StudySmarter Fig.5-Hydrogen bonding between water molecules

Dipole-induced Dipole forces

Dipole-induced dipole forces arise when a polar molecule with a permanent dipole induces a temporary dipole in a non-polar molecule. For example, dipole-induced dipole forces can hold molecules of HCl and He atoms together.

London dispersion forces

Induced-dipole Induced-dipole interactions are also known as London dispersion forces. This type of interaction is present in all molecules, but it is most important when dealing with non-polar molecules. London dispersion forces occur because of the random movement of electrons in the cloud of electrons. This movement produces a weak, temporary dipole moment! For example, London dispersion forces are the only type of attractive force holding F2 molecules together.

Examples of Dipoles in Chemistry

Now that you have a better understanding of what dipoles are, let's look at more examples! If the figure below you can see the structure of acetone. Acetone, C3H6O, is a polar molecular with a bond dipole.

Dipoles, Dipoles in Acetone, StudySmarter Fig.6-Dipoles in Acetone

Another common example of a molecule containing dipoles is carbon tetrachloride, CCl4. Carbon tetrachloride is a non-polar molecule that contains polar bonds, and therefore, has dipoles present. However, the net dipole is zero due to its tetrahedral structure, where the bond dipoles directly oppose each other.

Dipoles, Structure of Carbon Tetrachloride, StudySmarter Fig.7-Structure of Carbon Tetrachloride

Let's look at one last example!

What is the net dipole moment in CO2?

CO2 is a linear molecule that has two C=O bond dipoles equal in magnitude but pointing in opposite directions. Therefore, the net dipole moment is zero.

Dipoles, Dipoles in Carbon Dioxide, StudySmarter Fig.8-Dipoles in Carbon Dioxide

Dipoles can be a little intimidating, but once you get the hang of it you will find it simple!

Dipoles - Key takeaways

Dipoles occur when electrons are shared unequally between atoms due to a high difference in the electronegativity of the atoms involved.
A dipole moment is referred to as a measurement of the magnitude of a dipole.
Dipole moments are present in polar molecules that have asymmetric shapes because, in asymmetric shapes, the dipoles do not cancel out.
Types of dipoles include ion-dipole, dipole-dipole, and induced-dipole induced-dipole (London dispersion forces).

References:

Saunders, N. (2020). Supersimple Chemistry: The Ultimate Bitesize Study Guide. London: Dorling Kindersley.

Timberlake, K. C. (2019). Chemistry: An introduction to general, organic, and Biological Chemistry. New York, NY: Pearson.

Malone, L. J., Dolter, T. O., & Gentemann, S. (2013). Basic concepts of Chemistry (8th ed.). Hoboken, NJ: John Wiley & Sons.

Brown, T. L., LeMay, H. E., Bursten, B. E., Murphy, C. J., Woodward, P. M., Stoltzfus, M., & Lufaso, M. W. (2018). Chemistry: The central science (13th ed.). Harlow, United Kingdom: Pearson.

References

Fig.1-Periodic table showing Pauling's scale of electronegativity (https://upload.wikimedia.org/wikipedia/commons/thumb/4/42/Electronegative.jpg/640px-Electronegative.jpg) by ad blocker on wikimedia commons licensed by CC By-SA 3.0 (https://creativecommons.org/licenses/by-sa/3.0/)

Flashcards in Dipole Chemistry

19 Start learning

A _____ is a molecule that has a separation of charges.

Dipole

True or false: Dipoles occur when electrons are shared unequally between atoms due to a high difference in the electronegativity of the atoms involved.

True

The formation of a dipole depends on the polarity of a bond, which is determined by the difference in ______ between the two atoms involved in the bond.

Electronegativity

_____ is the ability of an atom to attract electrons to itself.

Electronegativity

In ______ bonds, the electrons are equally shared between atoms.

non-polar covalent

In ______, the electrons are shared unequally between atoms.

polar covalent bonds

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Frequently Asked Questions about Dipole Chemistry

How to calculate dipole moment?

Dipole moment can be calculated by using the following equation: = Qr where Q is the magnitude of the partial charges δ+ and δ- , and r is the distance between the two charges.

How do you determine a dipole?

The formation of a dipole depends on the polarity of a bond, which is determined by the difference in electronegativity between the two atoms involved in the bond.

What causes a dipole in chemistry?

Dipoles are caused when electrons are shared unequally between atoms due to a high difference in the electronegativity of the atoms involved.

What is a dipole moment in chemistry?

Dipole moment is referred to as a measurement of the magnitude of a dipole.

What is a dipole in chemistry?

A dipole is a molecule that has a separation of charges.

Save Article Test your knowledge with multiple choice flashcards

A _____ is a molecule that has a separation of charges.

A. Ionic bond B. Dipole moment C. Dipole

True or false: Dipoles occur when electrons are shared unequally between atoms due to a high difference in the electronegativity of the atoms involved.

A. True B. False

The formation of a dipole depends on the polarity of a bond, which is determined by the difference in ______ between the two atoms involved in the bond.

A. Boiling point B. Polarity C. Electronegativity

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Tag » What Is A Dipole Dipole Force

Dipole: Meaning, Examples & Types | StudySmarter

Dipole Definition in Chemistry

Determination and Formation of a Dipole

Types of Bonds

Predicting Bond Polarity

Dipole Moment in Chemistry

Types of Dipole in Chemistry

Ion-Dipole

Dipole-Dipole

Hydrogen Bonding

Dipole-induced Dipole forces

London dispersion forces

Examples of Dipoles in Chemistry

Dipoles - Key takeaways

References

Similar topics in Chemistry

Related topics to Physical Chemistry

Flashcards in Dipole Chemistry

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Frequently Asked Questions about Dipole Chemistry

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