High school Chemistry help » Elements and Compounds » Compounds and also Bonding » help with Intermolecular forces
Explanation:

Hydrogen bonds are intermolecular forces between hydrogens and nearby molecules. These nearby molecules have to contain one of two people fluorine, oxygen, or nitrogen, the three many electronegative atoms. This electronegative atoms pull electrons away from the bonded hydrogen, providing it a tiny positive charge and giving themselves a slightly an adverse charge. Once the optimistic hydrogen of one molecule come close to a an adverse charge ~ above another, the opposite charges attract and also pull the molecules close together to form a hydrogen bond. The hydrogen should be bonded to oxygen (-OH), fluorine (HF), or nitrogen (-NH) to have actually this charging effect.

You are watching: Which of the following pure compounds will exhibit hydrogen bonding?


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Example concern #2 : assist With Intermolecular forces


Which the the complying with molecules cannot take part in hydrogen bonding?


Possible Answers:


*


*


*


Correct answer:


Explanation:

Hydrogen bonding takes place when a hydrogen atom is attractive to a extremely electronegative atom in another molecule. Hydrogen bonding takes place between hydrogen and also either nitrogen, oxygen, or fluorine. Carbon has an electronegativity comparable to hydrogen"s, and will no hydrogen bond v hydrogens in other molecules.

Only molecules v -OH, -FH, or -NH teams can form hydrogen bonds.


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Example question #11 : Intermolecular pressures


What intermolecular pressures can be found in a molecule of ethene?


Possible Answers:

London dispersion forces and also hydrogen bonding


London dispersion forces only


London dispersion forces and dipole-dipole attraction


Dipole-dipole attraction and ionic bonding


London dispersion forces, hydrogen bonding, and dipole-dipole attraction


Correct answer:

London dispersion pressures only


Explanation:

Ethene is an organic molecule composed of 2 carbon atoms, joined by a dual bond, and also four hydrogen atoms.

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Ethene, favor all molecules, exhibits London dispersion forces. This molecule, however, has no network dipole moment, therefore it will not exhibition dipole-dipole attraction. Also, also though it contains hydrogens, it does no exhibit hydrogen bonding. To exhibition hydrogen bonding, the hydrogen atoms have to be fastened to much more electronegative atoms, specific nitrogen, fluorine, or oxygen. Finally, ionic bonding is only current in ionic compounds, not organic compounds.


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Example question #3 : assist With Intermolecular pressures


Which of the following intermolecular forces is broken once water is boiled?


Possible Answers:

Covalent bonds


Double bonds


Ionic bonds


Hydrogen bonds


None of this answers


Correct answer:

Hydrogen bonds


Explanation:

Intermolecular pressures are transient forces between two different molecules. Water is a polar molecule. The oxygen atom tote a slight positive charge, if the hydrogen atoms bring slight an unfavorable charges. This is the an outcome of the huge difference in electronegativity between oxygen and also hydrogen. Once two water molecule are next to each other, the partially optimistic hydrogen will be attractive to the partially negative oxygen. This attraction is well-known as a hydrogen bond.

Ionic bonds, covalent bonds, and twin bonds are all intramolecular forces. These space stable bonds in between atoms that develop the identification of the molecule. Breaking any of this bonds would transform the identity of the compound.


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Example question #4 : assist With Intermolecular forces


Water has actually a higher boiling suggest than hydrogen sulfide due to which type of bonding?


Possible Answers:

Covalent bonding


Hydrogen bonding


London dispersion forces


Heisenberg bonding


Ionic bonding


Correct answer:

Hydrogen bonding


Explanation:

Hydrogen bonding occurs in between a hydrogen atom on one molecule and a really electronegative atom—namely oxygen, nitrogen, or fluorine—on a surrounding molecule. This electrostatic pressure results in a stronger intermolecular bond than would certainly otherwise be current without the hydrogen bond. A stronger intermolecular bond results in a higher boiling point.

Water (H2O) exhibits hydrogen bonding between the hydrogen of one water molecule and the oxygen of one more water molecule. Due to the fact that sulfur is not as electronegative as oxygen, hydrogen sulfide (H2S) does not exhibit hydrogen bonding. This is the factor why water is a liquid at room temperature, when hydrogen sulfide is a gas.

See more: " Making Peace With The Establishment ", Making Peace With The Establishment

Wrong answers explained: neither water no one hydrogen sulfide has ionic bonds. Both have covalent bonds and also London dispersion force, but this walk not describe why water"s boiling suggest is higher. Heisenberg bonding does no exist and is a misleading prize option.


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Example question #5 : help With Intermolecular forces


Which the the adhering to compounds will exhibit hydrogen bonding?


Possible Answers:

*


Correct answer:

*


Explanation:

When hydrogen is bound to one of two people fluorine, oxygen, or nitrogen, the hydrogen atom carries little of the electron thickness of the covalent bond. This partly positively fee hydrogen atom may interact with the partial an adverse charge located on adjacent electronegative atoms such together F, N, or O on adjacent molecules. Keep in mind that hydrogen bonds are intermolecular forces, no intramolecular. This means that hydrogen bonds form between two separate molecules. Castle plan vital role in the chemistry the water, and other compounds the exhibit hydrogen bonding. 


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