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Which types of intermolecular forces can exist between molecules of iodine (I2)?
Wiki User
∙ 9y ago
yes it is - gentle warming will change it to vapor though.
Wiki User
∙ 13y ago
Wiki User
∙ 9y agoThese forces are called London dispersion forces, a type of Van der Waals forces.
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Bromine chlorine iodine state intermolecular forces?
Bromine, chlorine, and iodine are all halogens that exist as diatomic molecules (Br2, Cl2, I2) at room temperature. They are held together by weak van der Waals forces, which exist as London dispersion forces due to the temporary dipoles formed by the movement of electrons in the molecules. These intermolecular forces increase in strength as you go down the group from bromine to iodine.
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.
Why are the physical states of chlorine and iodine different at room temperature?
The physical states of chlorine and iodine are different at room temperature due to differences in their intermolecular forces. Chlorine is a diatomic gas because the weak van der Waals forces between chlorine molecules at room temperature are easily overcome. In contrast, iodine is a solid at room temperature because the stronger van der Waals forces hold the iodine molecules together in a solid lattice structure.
What are the intermolecular forces of I2?
Iodine is bound together by van der Waals forces.
Bromine chlorine iodine state intermolecular forces?
Bromine, chlorine, and iodine are all halogens that exist as diatomic molecules (Br2, Cl2, I2) at room temperature. They are held together by weak van der Waals forces, which exist as London dispersion forces due to the temporary dipoles formed by the movement of electrons in the molecules. These intermolecular forces increase in strength as you go down the group from bromine to iodine.
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.
Why are the physical states of chlorine and iodine different at room temperature?
The physical states of chlorine and iodine are different at room temperature due to differences in their intermolecular forces. Chlorine is a diatomic gas because the weak van der Waals forces between chlorine molecules at room temperature are easily overcome. In contrast, iodine is a solid at room temperature because the stronger van der Waals forces hold the iodine molecules together in a solid lattice structure.
What are the intermolecular forces of I2?
Iodine is bound together by van der Waals forces.
What type of intermolecular forces is I2?
An iodine molecule is held together by covalent bonds
What types of intermolecular forces can exist between molecules of iodine?
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).
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.
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
How do intermolecular forces affect the properties of chlorine and iodine?
Intermolecular forces, such as van der Waals forces, affect the physical properties of chlorine and iodine. Iodine, being larger and having more electrons, has stronger van der Waals forces than chlorine, resulting in a higher boiling point and melting point. Consequently, iodine is a solid at room temperature while chlorine is a gas.
