Arrange the different types of forces in order of increasing energy. Covalent, Hydrogen
Bonding, Ion-Dipole, Dipole-Dipole, Induced Dipole-Dipole (induced and London
dispersion), and Ionic Bonding
http://en.wikipedia.org/wiki/Intermolecular_force#Relative_strength_of_forces
Scroll down to relative strengths. Ionic bonding, not discussed in the aboe article, is strongest.
To arrange the different types of forces in order of increasing energy, we need to start by understanding the nature of each type of force. The energy of a force typically depends on the strength of the interaction between the particles involved. Here is a breakdown of each force and an explanation of how to arrange them:
1. Ion-Dipole: This force occurs between an ion (charged atom or molecule) and a polar molecule. It is relatively stronger than other types of intermolecular forces because of the presence of charged particles involved. Therefore, it has the highest energy among the options provided.
2. Ionic Bonding: This force is the electrical attraction between positively and negatively charged ions. It involves the transfer of electrons from one atom to another, resulting in the formation of ions. Ionic bonds are generally stronger than other intermolecular forces, such as hydrogen bonding and dipole-dipole interactions. Hence, it has the second-highest energy.
3. Covalent Bonding: This force is the result of the sharing of electrons between atoms. It occurs in covalent compounds where atoms are bonded together by a shared pair of electrons. Covalent bonding is stronger than intermolecular forces but weaker than ionic bonding. Therefore, it has a moderate energy level.
4. Hydrogen Bonding: This force is a special type of dipole-dipole interaction that occurs between a hydrogen atom bonded to an electronegative atom (such as nitrogen, oxygen, or fluorine) and another electronegative atom in a different molecule. Hydrogen bonding is stronger than other dipole-dipole interactions but weaker than both covalent and ionic bonding. Thus, it has a moderate energy level as well.
5. Dipole-Dipole: This force occurs between two polar molecules and is the attraction between the positive end of one molecule and the negative end of another. It is weaker than both hydrogen bonding and covalent bonding, resulting in lower energy.
6. Induced Dipole-Dipole (induced and London dispersion): This force occurs between nonpolar molecules. It is the weakest of all intermolecular forces and arises from temporary fluctuations of electron distributions. These fluctuations create temporary partial charges in neighboring molecules, leading to the attraction between them. Consequently, it has the lowest energy among the given options.
So, in increasing order of energy, the arrangement of the various forces will be:
Induced Dipole-Dipole (induced and London dispersion) < Dipole-Dipole < Hydrogen Bonding < Covalent Bonding < Ionic Bonding < Ion-Dipole.