Chemistry, 20.07.2019 08:00, Alienhead6187

Identify the intermolecular forces present in each of these substances nh3 hcl co co2

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answered: reggie36151

The intermolecular forces present in ${\mathbf{N}}{{\mathbf{H}}_{\mathbf{3}}}$ is $\boxed{{\text{hydrogen bonding}}}$

The intermolecular forces present in HCl is $\boxed{{\text{dipole - dipole forces}}}$

The intermolecular forces present in CO is $\boxed{{\text{dipole - dipole forces}}}$

The intermolecular forces present in ${\mathbf{C}}{{\mathbf{O}}_{\mathbf{2}}}$ is $\boxed{{\text{van der Waals forces}}}$

Further Explanation:

The forces that exist between the molecules are known as intermolecular forces (IMF). IMF includes both attractive as well as repulsive forces. They are electrostatic in nature and determine the bulk properties of the substances like melting and boiling points. Molecules are held in any substance due to these forces.

The various types of intermolecular forces are as follows:

1. Hydrogen bonding:

It is an attractive force that exists between hydrogen and more electronegative elements like N, O, F. It can either be intermolecular or intramolecular. Intermolecular hydrogen bonding is the one that occurs between different molecules. For example, the bond between HF and ${{\text{H}}_{\text{2}}}{\text{O}}$ is an intermolecular hydrogen bond. Intramolecular hydrogen bonding occurs between various parts of the same molecule. Ortho-nitro phenol and salicylaldehyde show this type of bonding.

2. Ion-dipole forces:

It is an attractive force that occurs between an ion and a molecule consisting of dipole. The force between ${\text{N}}{{\text{a}}^ + }$ and water molecule is an example of this force.

3. Ion-induced dipole forces:

It is an attractive force that occurs between an ion and a nonpolar molecule. It induces a dipole in the molecule, resulting in ion-induced dipole force. The bond between ${\text{F}}{{\text{e}}^{2 + }}$ and oxygen molecule is an example of such kind of bond.

4. Dispersion forces:

Also known as London dispersion forces, van der Waals forces, instantaneous dipole-induced dipole forces. These forces exist between atoms and molecules. The forces that occur in ${{\text{F}}_2}$ molecule is a dispersion force.

In ${\mathbf{N}}{{\mathbf{H}}_{\mathbf{3}}}$ , nitrogen is more electronegative than hydrogen. The presence of hydrogen and a highly electronegative element result in the formation of hydrogen bonding in this molecule. So hydrogen bonding exists in ${\text{N}}{{\text{H}}_3}$ .

HCl is a polar molecular because of the electronegativity difference between the bonded atoms. Here, chlorine is more electronegative than hydrogen so a dipole is formed with chlorine having a partial negative charge and a partial positive charge exists on hydrogen. So dipole-dipole interaction occurs in HCl.

CO is also a polar molecule. Oxygen is more electronegative than carbon so dipole-dipole forces exist in CO molecule.

${\mathbf{C}}{{\mathbf{O}}_{\mathbf{2}}}$ is a non-polar molecule as the dipole moment of each oxygen gets cancelled by the other one. So van der Waals forces exist in ${\text{C}}{{\text{O}}_2}$ molecule.

Learn more:

1. Which is the oxidation-reduction reaction:

2. Chemical bonds in NaCl:

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Ionic and covalent bonding

Keywords: Intermolecular forces, CO, HCl, CO2, NH3, hydrogen bonding, dispersion forces, polar, nonpolar, dipole moment, electronegativity, chlorine, hydrogen, oxygen, carbon, ion-dipole forces, intermolecular, intramolecular.

answered: Guest

c)red bank

explanation:

red bank is a borough in monmouth county, new jersey, incorporated in 1908 and located on the navesink river, the area's original transportation route to the ocean and other ports.

What city is located at 17° south 36° east answers: a)surfer’ town b)white’s beach c)red bank d)

answered: Guest

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.