Molecular Force Comparison
What is the strongest molecular force that could occur between two molecules of each below?
The strongest molecular force that could occur between two molecules is as follows:
Hydrogen molecule (H2): Dipole-dipole interaction
Oxygen molecule (O2): London Dispersion Forces
Nitrogen molecule (N2): London Dispersion Forces
Carbon dioxide (CO2): Dipole-dipole interaction
Water (H2O): Hydrogen bonding
Note: London Dispersion Forces are the weak attractive forces that occur between all molecules due to the fluctuation of their electron clouds. Dipole-dipole interactions are attractive forces between molecules that have a permanent dipole moment. Hydrogen bonding is a stronger attractive interaction that occurs between a hydrogen atom covalently bonded to a highly electronegative atom and another highly electronegative atom.
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The tibia is the strongest bone below the knee.
Though there are some other applications of the term molecular machine, it is primarily used in the field of nanotechnology. In the world of the ultra small, it is used to mean a handful of molecules (and sometimes a big handful) that perform a function or do work. You can read a bit more by using the link below. It will take you to the Wikipedia post on the molecular machine.
The term average must be used as the molecular motion is not completely uniform. ie. some of the molecules will vibrate at different frequencies and amplitudes, around a fixed average position. This is shown as water can evaporate even if it is below the boiling point, as some molecules have enough energy to escape. the boiling point is when the average energy is 100 degrees centigrade, so the molecules turn to gas.
Atoms bond together by sharing or transferring valence (outer shell) electrons, either in covalent (molecular) bonds or in ionic bonds.See related questions below.
gravity
water molecules can evaporate at the surface but not below the surface
Not at room temperature. But it is a molecular solid at temperatures below -78 degrees Celsius.
The molecular geometry of a molecule can be determined using the VSEPR theory. VSEPR (Valence Shell Electron Pair Repulsion) Theory: The basic premise of this simple theory is that electron pairs (bonding and nonbonding) repel one another; so the electron pairs will adopt a geometry about an atom that minimizes these repulsions. Use the method below to determine the molecular geometry about an atom. Write the Lewis dot structure for the molecule. Count the number of things (atoms, groups of atoms, and lone pairs of electrons) that are directly attached to the central atom (the atom of interest) to determine the overall (electronic) geometry of the molecule. Now ignore the lone pairs of electrons to get the molecular geometry of the molecule. The molecular geometry describes the arrangement of the atoms only and not the lone pairs of electrons. If there are no lone pairs in the molecule, then the overall geometry and the molecular geometry are the same. If the overall geometry is tetrahedral, then there are three possibilities for the molecular geometry; if it is trigonal planar, there are two possibilities; and if it is linear, the molecular geometry must also be linear. The diagram below illustrates the relationship between overall (electronic) and molecular geometries. To view the geometry in greater detail, simply click on that geometry in the graphic below. Although there are many, many different geometries that molecules adopt, we are only concerned with the five shown below.
It is called Hydrogen bonding. It is the strongest intramolecular bond type that can be formed between molecules. It usually occurs between a Hydrogen atom in a molecule and a very electronegative atom (oxygen, nitrogen or fluorine) with a free lone pair of atoms available. Therefore, in water the H and O form hydrogen bonds. The dashed line below represents an example of the Hydrogen bond. H | O ------------- H-O-H | H
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About 68 kDa
There are five carbon atoms in adenine.Its molecular formula is C5H5N5.For structural formulae, see the link below.