Then what are dipole-induced dipole forces, ion-dipole forces, and ion-induced dipole forces?

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. An ion-dipole force is an attractive force that results from the electrostatic attraction between an ion and a neutral molecule that has a dipole. An ion-induced dipole attraction is a weak attraction that results when the approach of an ion induces a dipole in an atom or in a nonpolar molecule by disturbing the arrangement of electrons in the nonpolar species.

I thought ionic bonds were much weaker than covalent bonds, for example the lattice structure of a carbon diamond is much stronger than a crystal lattice structure of NaCl. Is this table of bond strength wrong?

I initially thought the same thing, but I think there is a difference between bond strengths, and intramolecular forces. The intramolecular force strength is relative to the electronegativity of the 2 atoms in the molecule. The bond strength relates to the stability of the bond in it's energy state.

Why can't we say that H2S also has Hydrogen bond along with London dispersion bond and dipole-dipole attraction ?

Hydrogen bonding is just with H-F, H-O or H-N. I try to remember it by "Hydrogen just wants to have FON"

isnt hydrogen bonding stronger than dipole-dipole ??

Hydrogen bonding is the strongest form of dipole-dipole interaction.

The article said dipole-dipole interactions and hydrogen bonding are equally strong and hydrogen bonding is a type of dipole-dipole interaction, so how come covalent compounds containing hydrogen bonds have higher boiling and melting points than polar covalent compounds?

*Hydrogen bonding is the strongest form of dipole-dipole interaction.* So naturally, compounds that can hydrogen bond have higher bp since the H bonds are harder to overcome than other types of dipole-dipole interactions.

is there hydrogen bonding in HCl??if no why??

I try to remember it by "Hydrogen just wants to have FON"

#3 (C2H6) says that Van Der Waal Forces are found in non polar compounds. OK that i understand. What i'm not so clear on is the reasoning why #2 has Van Der Waal Forces. If Van Der Waal forces are found in any compound irrespective of bond or polarity, can I assume that the compound has van der waal forces if it has dipole or hydrogen bonds?

LDFs exist in everything, regardless of polarity. However nonpolar compounds can only have LDFs. Polar compounds can have LDFs, in addition to dipole-dipoles. Maybe H bonding if O-H F-H N-H bonds exist. Edit: One more thing, LDFs can only happen everywhere, so when drawing molecules, LDFs can be drawn randomly as long as they are connecting the two molecules. And to answer your question, you can say a compound has Van der waal forces if it has dip-dip bonds, H bonding, or LDFs.

In CH3OH (Methanol) Is there really a hydrogen bond between the carbon atom and the top left oxygen atom? Oh by the way wonderful drawings!

You are correct that would be impossible, but that isn't what the figure shows. The red dashed line on the left is labeled as a dipole-dipole bond.

difference between inter and intramolecular bonds?

Intermolecular bonds are the forces between the molecules. Intramolecular are the forces within two atoms in a molecule.

Main content

Intramolecular and intermolecular forces

Google Classroom

There are two kinds of forces, or attractions, that operate in a molecule—intramolecular and intermolecular. Let's try to understand this difference through the following example.

We have six towels—three are purple in color, labeled hydrogen and three are pink in color, labeled chlorine. We are given a sewing needle and black thread to sew one hydrogen towel to one chlorine towel. After sewing, we now have three pairs of towels: hydrogen sewed to chlorine. The next step is to attach these three pairs of towels to each other. For this we use Velcro as shown above.

So, the result of this exercise is that we have six towels attached to each other through thread and Velcro. Now if I ask you to pull this assembly from both ends, what do you think will happen? The Velcro junctions will fall apart while the sewed junctions will stay as is. The attachment created by Velcro is much weaker than the attachment created by the thread that we used to sew the pairs of towels together. A slight force applied to either end of the towels can easily bring apart the Velcro junctions without tearing apart the sewed junctions.

Exactly the same situation exists in molecules. Just imagine the towels to be real atoms, such as hydrogen and chlorine. These two atoms are bound to each other through a polar covalent bond—analogous to the thread. Each hydrogen chloride molecule in turn is bonded to the neighboring hydrogen chloride molecule through a dipole-dipole attraction—analogous to Velcro. We’ll talk about dipole-dipole interactions in detail a bit later. The polar covalent bond is much stronger in strength than the dipole-dipole interaction. The former is termed an intramolecular attraction while the latter is termed an intermolecular attraction.

So now we can define the two forces:

Intramolecular forces are the forces that hold atoms together within a molecule. Intermolecular forces are forces that exist between molecules.

Types of intramolecular forces of attraction

Ionic bond: This bond is formed by the complete transfer of valence electron(s) between atoms. It is a type of chemical bond that generates two oppositely charged ions. In ionic bonds, the metal loses electrons to become a positively charged cation, whereas the nonmetal accepts those electrons to become a negatively charged anion.

Covalent bond: This bond is formed between atoms that have similar electronegativities—the affinity or desire for electrons. Because both atoms have similar affinity for electrons and neither has a tendency to donate them, they share electrons in order to achieve octet configuration and become more stable.
A nonpolar covalent bond is formed between same atoms or atoms with very similar electronegativities—the difference in electronegativity between bonded atoms is less than 0.5.

A polar covalent bond is formed when atoms of slightly different electronegativities share electrons. The difference in electronegativity between bonded atoms is between 0.5 and 1.9. Hydrogen chloride, $HCl$ ‍; the $O - H$ ‍ bonds in water, $H_{2} O$ ‍; and hydrogen fluoride, $HF$ ‍, are all examples of polar covalent bonds.

Metallic bonding: This type of covalent bonding specifically occurs between atoms of metals, in which the valence electrons are free to move through the lattice. This bond is formed via the attraction of the mobile electrons—referred to as sea of electrons—and the fixed positively charged metal ions. Metallic bonds are present in samples of pure elemental metals, such as gold or aluminum, or alloys, like brass or bronze.

The freely moving electrons in metals are responsible for their a reflecting property—freely moving electrons oscillate and give off photons of light—and their ability to effectively conduct heat and electricity.

Relative strength of the intramolecular forces

Intramolecular force	Basis of formation	Relative strength
Metallic bond	Metal cations to delocalized electrons	1, strongest
Ionic bond	Cations to anions	2
Polar covalent bond	Partially charged cation to partially charged anion	3
Nonpolar covalent bond	Nuclei to shared electrons	4, weakest

Intermolecular forces of attraction

Now let’s talk about the intermolecular forces that exist between molecules. Intermolecular forces are much weaker than the intramolecular forces of attraction but are important because they determine the physical properties of molecules like their boiling point, melting point, density, and enthalpies of fusion and vaporization.

Types of intermolecular forces that exist between molecules

Dipole-dipole interactions: These forces occur when the partially positively charged part of a molecule interacts with the partially negatively charged part of the neighboring molecule. The prerequisite for this type of attraction to exist is partially charged ions—for example, the case of polar covalent bonds such as hydrogen chloride, $HCl$ ‍. Dipole-dipole interactions are the strongest intermolecular force of attraction.

Hydrogen bonding: This is a special kind of dipole-dipole interaction that occurs specifically between a hydrogen atom bonded to either an oxygen, nitrogen, or fluorine atom. The partially positive end of hydrogen is attracted to the partially negative end of the oxygen, nitrogen, or fluorine of another molecule. Hydrogen bonding is a relatively strong force of attraction between molecules, and considerable energy is required to break hydrogen bonds. This explains the exceptionally high boiling points and melting points of compounds like water, $H_{2} O$ ‍, and hydrogen fluoride, $HF$ ‍. Hydrogen bonding plays an important role in biology; for example, hydrogen bonds are responsible for holding nucleotide bases together in $DNA$ ‍ and $RNA$ ‍.

London dispersion forces, under the category of van der Waal forces: These are the weakest of the intermolecular forces and exist between all types of molecules, whether ionic or covalent—polar or nonpolar. The more electrons a molecule has, the stronger the London dispersion forces are. For example, bromine, ${Br}_{2}$ ‍, has more electrons than chlorine, ${Cl}_{2}$ ‍, so bromine will have stronger London dispersion forces than chlorine, resulting in a higher boiling point for bromine, 59 $^{o}$ ‍C, compared to chlorine, –35 $^{o}$ ‍C. Also, the breaking of London dispersion forces doesn’t require that much energy, which explains why nonpolar covalent compounds like methane— ${CH}_{4}$ ‍—oxygen, and nitrogen—which only have London dispersion forces of attraction between the molecules—freeze at very low temperatures.

Relative strength of intermolecular forces of attraction

Intermolecular force	Occurs between …	Relative strength
Dipole-dipole attraction	Partially oppositely charged ions	Strong
Hydrogen bonding	$H$ ‍ atom and $O$ ‍, $N$ ‍/ or $F$ ‍ atom	Strongest of the dipole-dipole attractions
London dispersion attraction	Temporary or induced dipoles	Weakest

How forces of attraction affect properties of compounds

Polar covalent compounds—like hydrogen chloride,

HCl

, and hydrogen iodide,

HI

—have dipole-dipole interactions between partially charged ions and London dispersion forces between molecules. Nonpolar covalent compounds—like methane

{CH}_{4}

and nitrogen gas,

N_{2}

)—only have London dispersion forces between molecules. The rule of thumb is that the stronger the intermolecular forces of attraction, the more energy is required to break those forces. This translates into ionic and polar covalent compounds having higher boiling and melting points, higher enthalpy of fusion, and higher enthalpy of vaporization than covalent compounds.

Boiling and melting points of compounds depend on the type and strength of the intermolecular forces present, as tabulated below:

Type of compound	Intermolecular forces present	Relative order of boiling and melting points
Ionic compounds	Ion to ion attraction between ions, London dispersion forces	1, highest)
Covalent compounds containing hydrogen bonds	Hydrogen bonds, London dispersion forces	2
Polar covalent compounds	Dipole-dipole attraction between dipoles created by partially charged ions, London dispersion forces	3
Nonpolar covalent compounds	London dispersion forces	4, lowest

Let’s try to identify the different kinds of intermolecular forces present in some molecules.

$H_{2} S$ ‍—London dispersion force—by default every compound will have this force of attraction between molecules—and dipole-dipole attraction

${CH}_{3} OH$ ‍—London dispersion force, dipole-dipole attraction, and hydrogen bonding

$C_{2} H_{6}$ ‍—London dispersion forces—it’s a nonpolar covalent compound— and no other intermolecular attractions

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sazkhan123
Posted 9 years ago. Direct link to sazkhan123's post “Why can't we say that H2S...”
Why can't we say that H2S also has Hydrogen bond along with London dispersion bond and dipole-dipole attraction ?
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- ms.chantel1221
  Posted 8 years ago. Direct link to ms.chantel1221's post “Hydrogen bonding is just ...”
  Hydrogen bonding is just with H-F, H-O or H-N. I try to remember it by "Hydrogen just wants to have FON"
  Comment on ms.chantel1221's post “Hydrogen bonding is just ...”
  (182 votes)
Muhammad Azeem
Posted 9 years ago. Direct link to Muhammad Azeem's post “is there hydrogen bonding...”
is there hydrogen bonding in HCl??if no why??
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(3 votes)
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- ms.chantel1221
  Posted 8 years ago. Direct link to ms.chantel1221's post “I try to remember it by "...”
  I try to remember it by "Hydrogen just wants to have FON"
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  (43 votes)
Saran V Balachandar
Posted 7 years ago. Direct link to Saran V Balachandar's post “Then what are dipole-indu...”
Then what are dipole-induced dipole forces, ion-dipole forces, and ion-induced dipole forces?
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(16 votes)
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- candy08421
  Posted 5 years ago. Direct link to candy08421's post “A dipole-induced dipole a...”
  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.
  An ion-dipole force is an attractive force that results from the electrostatic attraction between an ion and a neutral molecule that has a dipole.
  An ion-induced dipole attraction is a weak attraction that results when the approach of an ion induces a dipole in an atom or in a nonpolar molecule by disturbing the arrangement of electrons in the nonpolar species.
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  (15 votes)
Mariel Luna
Posted 8 years ago. Direct link to Mariel Luna's post “isnt hydrogen bonding str...”
isnt hydrogen bonding stronger than dipole-dipole ??
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(5 votes)
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- ♪♫ Viola ♫♪
  Posted 8 years ago. Direct link to ♪♫ Viola ♫♪'s post “Hydrogen bonding is the s...”
  Hydrogen bonding is the strongest form of dipole-dipole interaction.
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  (18 votes)
oskargonzalez
Posted 9 years ago. Direct link to oskargonzalez's post “I thought ionic bonds wer...”
I thought ionic bonds were much weaker than covalent bonds, for example the lattice structure of a carbon diamond is much stronger than a crystal lattice structure of NaCl. Is this table of bond strength wrong?
Button navigates to signup pageComment on oskargonzalez's post “I thought ionic bonds wer...”
(10 votes)
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- Brian
  Posted 8 years ago. Direct link to Brian's post “I initially thought the s...”
  I initially thought the same thing, but I think there is a difference between bond strengths, and intramolecular forces. The intramolecular force strength is relative to the electronegativity of the 2 atoms in the molecule. The bond strength relates to the stability of the bond in it's energy state.
  Button navigates to signup page
  (11 votes)
Roy Powell
Posted 5 years ago. Direct link to Roy Powell's post “#3 (C2H6) says that Van ...”
#3 (C2H6) says that Van Der Waal Forces are found in non polar compounds. OK that i understand. What i'm not so clear on is the reasoning why #2 has Van Der Waal Forces.
If Van Der Waal forces are found in any compound irrespective of bond or polarity, can I assume that the compound has van der waal forces if it has dipole or hydrogen bonds?
Button navigates to signup pageButton navigates to signup page
(3 votes)
Answer
- Daniel H.
  Posted 5 years ago. Direct link to Daniel H.'s post “LDFs exist in everything,...”
  LDFs exist in everything, regardless of polarity.
  However nonpolar compounds can only have LDFs.
  Polar compounds can have LDFs, in addition to dipole-dipoles. Maybe H bonding if O-H F-H N-H bonds exist.
  
  Edit: One more thing, LDFs can only happen everywhere, so when drawing molecules, LDFs can be drawn randomly as long as they are connecting the two molecules.
  
  And to answer your question, you can say a compound has Van der waal forces if it has dip-dip bonds, H bonding, or LDFs.
  Button navigates to signup page
  (8 votes)
VAIKALYA PRAJAPATI
Posted 8 years ago. Direct link to VAIKALYA PRAJAPATI's post “difference between inter ...”
difference between inter and intramolecular bonds?
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(0 votes)
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- maressavilla
  Posted 8 years ago. Direct link to maressavilla's post “Intermolecular bonds are ...”
  Intermolecular bonds are the forces between the molecules. Intramolecular are the forces within two atoms in a molecule.
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  (12 votes)
ff142
Posted 8 years ago. Direct link to ff142's post “The article said dipole-d...”
The article said dipole-dipole interactions and hydrogen bonding are equally strong and hydrogen bonding is a type of dipole-dipole interaction, so how come covalent compounds containing hydrogen bonds have higher boiling and melting points than polar covalent compounds?
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(4 votes)
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- ♪♫ Viola ♫♪
  Posted 8 years ago. Direct link to ♪♫ Viola ♫♪'s post “*Hydrogen bonding is the ...”
  *Hydrogen bonding is the strongest form of dipole-dipole interaction.*
  So naturally, compounds that can hydrogen bond have higher bp since the H bonds are harder to overcome than other types of dipole-dipole interactions.
  Button navigates to signup page
  (3 votes)
Benson Kwok
Posted 5 years ago. Direct link to Benson Kwok's post “In CH3OH (Methanol) Is th...”
In CH3OH (Methanol) Is there really a hydrogen bond between the carbon atom and the top left oxygen atom?
Oh by the way wonderful drawings!
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(3 votes)
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- tyersome
  Posted 5 years ago. Direct link to tyersome's post “You are correct that woul...”
  You are correct that would be impossible, but that isn't what the figure shows.
  
  The red dashed line on the left is labeled as a dipole-dipole bond.
  Comment on tyersome's post “You are correct that woul...”
  (3 votes)
Aayman
Posted 5 years ago. Direct link to Aayman's post “Can an ionic bond be clas...”
Can an ionic bond be classified as an intermolecular and an intramolecular bond? If so, how?
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(3 votes)
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Course: MCAT > Unit 10