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Ionic Forces

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Camille Carr

on 29 March 2014

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Transcript of Ionic Forces

London Dispersion Forces are the weakest of the intermolecular forces. They usually produce gases.
They exist in Ionic bonds, polar covalent bonds, and non-polar covalent bonds. However, the ionic forces in ionic bonds are so strong that LDF can be ignored. They are most important in non polar molecules.
They primarily affect non-metals.
The charges of the ions are temporary and partial because LDF rely on the constant movement of electrons in order to create a temporary charge.
London Dispersion Forces
Intermolecular Forces
Strong attraction because there are 106 electrons which creates larger temporary poles.
Less attraction than in I2 because there are only 16 electrons involved in this compound, and 106 in I2.
Dipole Dipole Forces
Weaker than F2S because the elements in this compound are closer in electronegativity.
Ionic forces are the strongest of the Intermolecular Forces. Therefore, the substances produced are often solids with high melting points.
They exist in ionic bonds, which are between metals and nonmetals. The charges of the ions are full and permanent.
Ionic Forces
Very strong bond because Na is a small, highly charged element.
Rb has the same charge as Na, but it has a larger atomic size making the attraction less strong.
Attractive forces between two molecules.
Based on the principle of the attraction between positive and negative charges.
Dipole forces are relatively strong Intermolecular Forces. The substances produced can be solids, liquids, or gasses depending on the strength of the bond.
They exist in polar covalent compounds which means that the bond is between a nonmetal and either F,O,N, or Cl.
The charges of the ions are partial and permanent.
Hydrogen bonds are a "special case" of dipole forces. They occur when hydrogen is bonded to a highly electronegative atom it can be attracted to another highly electronegative atom (usually N,O, or F) of another molecule.
They are stronger than dipole forces.
Hydrogen Bonds
Strong attraction because flourine is the most electronegative element.
Weaker than HF because Cl is a weaker element than F
Strong attraction because there is a great difference in the electronegativity
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