diatomic elements
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diatomic elements
Hi! Can someone explain to me why diatomic elements form, and how to distinguish between whether an element is existing in its diatomic form or not? For example, if a problem involves a diatomic element like oxygen, do you assume that's in a diatomic form, or does the problem have to state explicitly "oxygen gas"?
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Re: diatomic elements
All the elements in the acronym HOFBrINCl, (hydrogen, oxygen, fluorine, Bromine, Iodine, and chlorine) are included in the diatomic elements. Any time these elements are listed in a chemical equation they must have the subscript of 2 as you always assume they are diatomic.
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Re: diatomic elements
The reason these elements are diatomic is because they don't have enough electrons to fill up their valence shells. Thus, they cannot exist as a single atom.
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Re: diatomic elements
One cheap mnemonic device to remember these is: Never Have Fear Of Ice CoLd Bread
Never: Nitrogen
Have: Hydrogen
Fear: Fluorine
Of: Oxygen
Ice: Iodine
CoLd: Chlorine
Bread: Bromine
Never: Nitrogen
Have: Hydrogen
Fear: Fluorine
Of: Oxygen
Ice: Iodine
CoLd: Chlorine
Bread: Bromine
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Re: diatomic elements
My TA taught us another method to remember the diatomic elements. She refers to them as gens and ines. Ex. HydroGEN and fluorINE
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Re: diatomic elements
For me, it helps when I picture them on the periodic table because, with the exception of Hydrogen, the other six elements (C, N, O, F, Cl, Br, I) border the top right hand corner of the table next to the column of noble gases.
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Re: diatomic elements
In high school, we learned to remember them with a phrase pronounced "Br-inkl-hoff," which is Br(bromine), I(iodine), N (nitrogen), Cl(chlorine), H(hydrogen), O(oxygen), and F(fluorine). Helped me a lot back then and now.
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Re: diatomic elements
Some elements exist as diatomic elements since in their original state, their valence shells are not filled, thus they share electrons between each other and thus fill their shells and achieve a state of lower energy.
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Re: diatomic elements
Diatomics exist to share electrons covalently and achieve a lower energy state.
HOFBrINCl is a metonym to remember the diatomics:
H- Hydrogen
O- Oxygen
F- Fluorine
Br- Bromine
I- Iodine
N- Nitrogen
Cl- Chlorine
HOFBrINCl is a metonym to remember the diatomics:
H- Hydrogen
O- Oxygen
F- Fluorine
Br- Bromine
I- Iodine
N- Nitrogen
Cl- Chlorine
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Re: diatomic elements
Does anyone know what order to put the elements in when writing an empirical formula?
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Re: diatomic elements
Karina Jiayu Xu 4E wrote:Does anyone know what order to put the elements in when writing an empirical formula?
In an empirical formula, it's typically C, H, and then other elements follow in alphabetical order.
Re: diatomic elements
Diatomic elements only need to exist in pairs of atoms when they are standing alone. For instance, in OH-, you wouldn't need two hydrogen atoms because the hydrogen is not free standing. However, if you have hydrogen gas, you would need H2 because it is not attached to a different element.
Re: diatomic elements
Elements are diatomic because their valence shells aren't completely filled by electrons; therefore, electrons are shared a lower energy state is achieved.
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