What Triggers Ionic Bonding in Atoms?

In summary, the conversation discusses the question of what causes an ionic bond in chemistry. The usual explanation is that one atom releases an electron and another gains it, causing net electric charges on both atoms. However, the conversation delves deeper into the specific scenario of a sodium atom coming near a chlorine atom and what causes the valence electron to leave the sodium atom in the first place. The conversation suggests potential explanations such as a stronger dipole moment on the chlorine atom or a thermodynamic explanation.
  • #1
Pengwuino
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So I never got too far into chemistry and had never had much thought put into this. What exactly causes an ionic bond? And I mean, I know the usual 'one atom releases an electron and another gains it, causing net electric charges on both atoms', but what causes the electron to leave an atom to join another?

For example, a sodium atom coming near a chlorine atom. What causes the valence electron to disassociate with the sodium atom in the first place? A stronger dipole moment on the chlorine? magic? :)
 
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  • #2
This has to be explained thermodynamically. I find this site pretty good.
 

FAQ: What Triggers Ionic Bonding in Atoms?

1. What is ionic bonding?

Ionic bonding is a type of chemical bonding that occurs between a metal and a non-metal. It involves the transfer of electrons from the metal atom to the non-metal atom, resulting in the formation of positively and negatively charged ions.

2. How does ionic bonding occur?

Ionic bonding occurs when there is a large difference in electronegativity between the two atoms involved. The more electronegative atom, usually the non-metal, gains electrons from the less electronegative atom, which is typically the metal. This results in the formation of ions with opposite charges that are attracted to each other.

3. What causes the large difference in electronegativity in ionic bonding?

The large difference in electronegativity is caused by the difference in the number of valence electrons between the metal and non-metal atoms. Metals tend to have fewer valence electrons and a lower electronegativity, while non-metals have more valence electrons and a higher electronegativity. This creates a strong attraction for electrons to be transferred from the metal to the non-metal.

4. What properties does ionic bonding give to compounds?

Ionic bonding results in compounds that have high melting and boiling points, are solid at room temperature, and are electrically conductive when melted or dissolved in water. These properties are due to the strong electrostatic attraction between the positively and negatively charged ions in the compound.

5. What factors affect the strength of ionic bonding?

The strength of ionic bonding is affected by the size of the ions and the distance between them. Smaller ions and closer distances between them result in stronger ionic bonds. It is also influenced by the number of valence electrons involved in the bond, as well as the overall charge of the ions.

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