Intermolecular Forces Essay

5. The two primary types of chemical bonding is ionic and covalent. Ionic bonding is when atoms give

An ionic bond is a bond that results from the attraction between oppositely charges ions; one atom "gives" another atom an electron. Combinations of metals and nonmetals typically form ionic bonds. A covalent bond is a bond that results from

Of the two alkane liquids studied n-Hexane was determined to have the stronger IMF of attraction by virtue of its experimentally determined lower ?T. Conversely n-Pentane has weaker IMF of attraction due to its larger ?T. As explained at length above, this is because it takes more energy to excite a molecule in liquid to leave (vaporize or become gaseous), when there are stronger IMF of attraction holding the molecules together in liquid form.

As a result of the water molecule bond, each (hydrogen; oxygen) has a slightly negative charge and each (hydrogen; oxygen) has a slightly positive charge.

A greater number of electrons correspond to a great polarizability of a molecule. Greater polarizability leads to greater dispersion forces. Thus, as molar mass increases, the number of electrons increase, which increases the polarizability of the molecule and hence the strength of the dispersion forces of the substance.

A London dispersion force is the name given to intermolecular forces in a non-polar compound. It greatly depends on the amount of electrons in a molecule. The larger/ heavier molecules have more electrons resulting in a greater attractive London force. This is because as the external force causes a temporary shift, the electrons will move to one side and it will become more negative resulting in a greater attraction. Then it will return to its previous state of the dispersion of

There are many types of chemical bonds and forces that bind molecules together. The two most basic types of bonds are characterized as either ionic or covalent. In the lab we separated Citric Acid, Calcium Chloride, Sucrose, Potassium Iodine, Phenyl Salicylate ,and Sodium Chloride into two groups ionic and Covalent bonds .The Chemical Difference between ionic bonding and covalent bonding is, a covalent bond is formed between two nonmetals that have similar electronegativities. Metals are left half and center of the Periodic Table and Nonmetals are upper right of the Periodic Table. The electrical attraction between large numbers of cations and anions which is the transfer of the

An atomic force microscope (AFM) is a type of scanning probe microscope (SPM). An AFM uses a cantilever with a probe to scan over a sample’s surface. The probe is a sharp tip (3 to 6 m pyramid; 15 to 40 nm end radius) such as the one shown in Fig. 1.

Before the atoms are bonded, the single, non-bonded pairs of electrons are called lone pairs of electrons. When the atoms combine by means of covalent bonding they form molecules. Simple covalent compounds consist of many small molecules. The covalent bonds within the molecules are strong but the bondings between them to form the compounds are relatively weak, the force that occurs between them is called the intermolecular force.

False because what keeps them together is Hydrogen bonding.Repellant forces would repel the molecules if the hydrogen bonds weren’t there.

A table of our findings from the five force analysis can be found in Appendix B, our

There are three main types of IMFs: London dispersion forces, dipole-dipole, and hydrogen boding. London dispersion forces are the weakest IMFs due to unequal electrons and consist of a temporary dipole. Dipole-dipole forces are attractions

More recently, distinctions between states have been based on differences in molecular interrelationships. Solid is the state in which intermolecular attractions keep the molecules in fixed spatial relationships. Liquid is the state in which

The Effects of Forces. A force acting on an object may cause the object to change shape, to start moving, to stop moving, to accelerate or decelerate. When two objects interact with each other they exert a force on each other, the forces are equal in size but opposite in direction.

1. Electric charges attract or repel one another with a force inversely proportional to the square of the distance between them: unlike charges attract, like ones repel.