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LogicalAcid
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Why do some atoms bind with other atoms of their own elements, such as O2 and N2, and why do others not? What property of these atoms enable them to do this?
espen180 said:this does not cover the atoms that no not form covalent dimers, like Be.
DrDu said:No, the nuclei aren't important. The binding in Be_2 etc. is so complicated due to strong correlation of the electrons.
DrDu said:You are probably right Borek, nevertheless then I do not quite understand what the question is. Maybe that not for all elements the diatomic molecules are the most stable ones in comparison with other struktures? I think LocigalAcid could precise that point.
DrDu said:Tell me an element besides the noble gasses which does not form a diatomic molecule.
Diatomic molecules form through a process called bonding, where two atoms share electrons to create a stable molecule. This can happen through either covalent bonding, where the atoms share electrons equally, or ionic bonding, where one atom gives up an electron to the other.
The most common type of diatomic molecules found in nature are homonuclear diatomic molecules, which consist of two atoms of the same element bonded together. Examples include oxygen (O2), nitrogen (N2), and hydrogen (H2).
Diatomic molecules are composed of only two atoms, while polyatomic molecules contain more than two atoms. Diatomic molecules also tend to be more stable and have simpler structures compared to polyatomic molecules.
Yes, many diatomic molecules exist in a gaseous state at room temperature, such as hydrogen (H2), oxygen (O2), and nitrogen (N2). They can also exist in other states of matter, such as liquids (e.g. water) and solids (e.g. iodine).
Diatomic molecules play a crucial role in many chemical reactions because they are often the building blocks of more complex molecules. They can also participate in reactions themselves, either by breaking apart or combining with other atoms to form new molecules.