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What types of intermolecular forces can exist between molecules of iodine?
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∙ 8y ago
Regardless of the state, the forces which hold an iodine moolecule together are the same for any other covalent bond: the electric force between the two opposite charges (the positive nuclei and the negative electrons).
Wiki User
∙ 15y ago
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∙ 9y agoLondon (dispersion) forces become stronger as the atom or molecule in question becomes larger. This is due to the increased polarizability of molecules with larger, more dispersed electron clouds. This trend is exemplified by the halogens (from smallest to largest: F2, Cl2, Br2, I2). Fluorine and chlorine are gases at room temperature, bromine is a liquid, and iodine is a solid. The London forces also become stronger with larger amounts of surface contact. Greater surface area means closer interaction between different molecules.
Wiki User
∙ 10y agowhat is the major attractive force that exists among different I2 molecoles in the solid
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∙ 9y agoDispersion forces are responsible for iodine being solid at room temperature.
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∙ 6y agoNon-polar bonds, or more specifically, temporary dipole-dipole bonds
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∙ 8y agoLondon dispersion forces are supposed to interact between iodine molecules.
Wiki User
∙ 13y agoyes .because iodine is good
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Which types of intermolecular forces can exist between molecules of iodine (I2)?
yes it is - gentle warming will change it to vapor though.
How does intermolecular forces of a substance determine the phase the substance is in?
The strength of the intermolecular forces will determine what phase the substance is in at any given temperature and pressure. Consider the halogens for example, fluorine and chlorine are gases, while bromine is a liquid and iodine is a solid at room temperature. When considering the intermolecular forces present, each of these substances only has London forces, which increase in magnitude with increasing size of the molecules, and size increases as you go down a group in the periodic table. So, fluorine has the smallest intermolecular forces, and iodine has the largest. This explains why these different substances exist in different phases when at room temperature and pressure. The molecules in fluorine, for example, are only slightly attracted to each other, and therefore the substance exists as a gas. The stronger intermolecular forces in bromine, however, hold the molecules close to each other, but not quite strongly enough to prevent the molecules from sliding past each other; this makes bromine a liquid. Finally, in iodine, the intermolecular forces are actually strong enough that the molecules are held in fixed positions relative to each other, thus making iodine a solid.
Why are covalent bonds typically much stronger than intermolecular forces?
Well, a crystal is solid. If you mean, are ionic bonds stronger than covalent bonds, then the answer would be almost always. With a few exceptions, the ionic bond has a greater intermolecular force than a covalent bond. One exception might be a diamond and a weak ionic compound like RbBr.
What are the intermolecular forces of I2?
Iodine is bound together by van der Waals forces.
On heating sublime substances like iodine and camphor they directly change from solid to gas?
On heating iodine and camphor directly converted into gases and no liquid state is appears in between this process because the intermolecular forces between the molecules in such types of solids is less than ordinary solids, therefore high energy molecules at solid surface over come the attractive forces and directly converted into vapours.
Which types of intermolecular forces can exist between molecules of iodine (I2)?
yes it is - gentle warming will change it to vapor though.
How does intermolecular forces of a substance determine the phase the substance is in?
The strength of the intermolecular forces will determine what phase the substance is in at any given temperature and pressure. Consider the halogens for example, fluorine and chlorine are gases, while bromine is a liquid and iodine is a solid at room temperature. When considering the intermolecular forces present, each of these substances only has London forces, which increase in magnitude with increasing size of the molecules, and size increases as you go down a group in the periodic table. So, fluorine has the smallest intermolecular forces, and iodine has the largest. This explains why these different substances exist in different phases when at room temperature and pressure. The molecules in fluorine, for example, are only slightly attracted to each other, and therefore the substance exists as a gas. The stronger intermolecular forces in bromine, however, hold the molecules close to each other, but not quite strongly enough to prevent the molecules from sliding past each other; this makes bromine a liquid. Finally, in iodine, the intermolecular forces are actually strong enough that the molecules are held in fixed positions relative to each other, thus making iodine a solid.
Why is bromine2 a liquid and Iodine 2 is a solid?
Iodine has stronger intermolecular forces.
Describe the bonding in a crystal of iodine?
iodine is made from diatomic iodine molecules,the two iodine atoms are covalently bonded with each other.the iodine molecules have dispersion forces so,the crystal is made from the dispersion forces between the iodine molecule.
Why are covalent bonds typically much stronger than intermolecular forces?
Well, a crystal is solid. If you mean, are ionic bonds stronger than covalent bonds, then the answer would be almost always. With a few exceptions, the ionic bond has a greater intermolecular force than a covalent bond. One exception might be a diamond and a weak ionic compound like RbBr.
What are the intermolecular forces of I2?
Iodine is bound together by van der Waals forces.
On heating sublime substances like iodine and camphor they directly change from solid to gas?
On heating iodine and camphor directly converted into gases and no liquid state is appears in between this process because the intermolecular forces between the molecules in such types of solids is less than ordinary solids, therefore high energy molecules at solid surface over come the attractive forces and directly converted into vapours.
What type of intermolecular forces is I2?
An iodine molecule is held together by covalent bonds
Why the melting points of sodium chloride and iodine are very different?
It has got to do with the intermolecular (forces in between different atoms) forces. Iodine (I2) has weak intermolecular forces in between molecules, called a dispersion force. This force is very weak, resulting in lower boiling and melting temperatures. This happens for all covalent bonded non-metals. Sodium Chloride, however, has a very strong intermolecular force. This is because they are Ionic (Metal and a Non-Metal). Ionic compounds are like a bar magnet, with the metal (Sodium) as the positive end and the non-metal (Chlorine) as the negative end. These form a 3D lattice Structure (a Cube Structure). The positive ends attract to the negative ends and vice versa. This strong attraction means that when the substance is heated up, the molecules want to stay together. This results in a higher melting and boiling temperatures. Note: Ionic forces are about 1000x stronger than dispersion forces
What is the formula of iodine crystals?
Iodine exists as I2. The crystal of iodine is formed simply by the interaction of iodine molecules as a result of Van de Waals forces, which allows for these molecules to bond together to form a solid.
Does fluorine have weaker or stronger intermolecular forces than iodine?
It depends. If Fluorine is bonded to Hydrogen then it would be greater, having present Hydrogen Bonding-the strongest Intermolecular Force. Iodine,I2, has many more electrons than fluorine, F2,so London dispersion forces are much stronger explaining why fluorine is a gas and iodine is a solid under standard conditions.
How do intermolecular forces affect the properties of chlorine and iodine?
Do your homework yourself C: I had the exact same sheet last week hardy har.
