Lewis dot structure gives information about outermost shell electrons of an atom. This article is discussing about the Rubidium lewis dot structure involving in bonding with different elements.
Rubidium lewis dot structure is written by Atomic symbol of the atom ‘Rb’. The outer orbit electrons are written around ‘Rb’ as dot sign. Rubidium is a ‘group 1’ element with one outer most shell electron. It always tries to donate that electron to an acceptor atom. This gives the Rubidium atom stable electronic structure like nearest Inert gas.
In the article, ” Rubidium lewis dot structure”, here some several elements and Rubidium lewis dot structure are shown-
- Rubidium ion lewis dot structure
- Rubidium sulfide lewis dot structure
- Rubidium fluoride lewis dot structure
- Rubidium iodide lewis dot structure
Rubidium ion lewis dot structure
Rubidium is a ‘Group 1’ element in periodic table with total 37 electrons. It has one electron in outer most orbital 5s.
Octet rule informs that every element covers its last orbit with highest possible number of electrons. This makes the element energetically more stable. So Rubidium transfers the outer shell electron to obtain the stability like nearest Noble gas. Thus it becomes a positive ion.
The symbol of Rubidium ‘Rb’ is written. As it donates the outer shell (5s) electron, there will be no dot sign around the atomic symbol. The atomic symbol is written into a third bracket ([ ]). The positive charge developed on the atom for donating the 5s electron; is written outside the bracket at upper right side.
Rubidium Sulfide lewis dot structure
Rubidium is in group 1 in periodic table. So it has one outer most shell electron in 5s orbital ([Kr] 5s1). Sulfur is a ‘group 16’ element. Its electronic configuration: [Ne] 3s2 3p4.
Rubidium atom donates the outer orbital 5s electron. Hence it becomes a ion, carrying positive charge. For this it develop an energetically stable configuration like nearest inert gas. Sulfur atom takes the electron in vacant 2p orbital and form Sulfide ion.
Sulfur atom requires two electrons to fill up its outer 2p orbital. It adds with two positively charged Rubidium ions and produce Rb2S molecule.
Electrons that form sigma bonds between Rubidium and Sulfur are shown as straight lines in the electron dot structure of Rubidium sulfide.
Rubidium Fluoride lewis dot structure
Fluorine is a ‘group 17’ element. It has seven electrons in last shell which are in 2s and 2p orbital. Rubidium has one outer orbital electron which is in 5s; as a ‘group 1’ element.
Fluorine atom requires one electron to make energetically stable outer orbit structure. Rubidium transfers its one outer shell (5s) electron to electronegative Fluorine atom.
These two oppositely charged Rubidium and fluoride ion produce a molecule with sigma bond formation.
In the electron dot structure of the molecule Rubidium atom has no any unshared electrons in outer orbital. Fluorine atom has six unshared electrons in the outer shell.
Rubidium Iodide lewis dot structure
Iodine is a ‘group 17’ element in periodic table. Electronic configuration of Iodine (outer most shell): [Kr] 4d10 5s2 5p5. Rubidium has only one electron in the last orbital (5s).
According to Octet rule every atom requires full filled up the outer orbit. Rubidium atom gives the last orbital (5s) electron to another atom’s vacant orbital; this results in a positive ion formation. By this the outer shell configuration of Rubidium becomes like nearest noble gas Krypton.
The electron is accepted by Iodine and produces negatively charged Iodide ion. The two opposite charge ion are attracted to each other and produce Rubidium iodide (RbI).
In the molecule Iodide ion contains six unbonding electrons.
Rubidium Hydrogen lewis dot structure
Rubidium is in ‘group 1’ in periodic table with electronic configuration: [Kr] 5s1. So it has one outer shell electron. Hydrogen is also a group 1 element; has one electron in 1s orbital.
Rubidium atom transfers that 5s shell electron to get energetically stable electronic structure. That electron accepted by Hydrogen atom vacant shell. This makes Hydrogen atom having the electronic configuration like Helium atom.
This two oppositely charged ions results in Rubidium hydride (RbH) molecule formation.
The electrons which take part in bonding between Rubidium and Hydride ion are shown as straight lines. Rubidium atom has no non bonding electrons in outer orbit.
Rubidium Nitride lewis dot structure
Rubidium is a ‘group 1’ element in periodic table with 37 electrons. Electronic configuration of Rubidium is [Kr] 5s1. Nitrogen is a ‘group 15’ element. Electronic configuration of Nitrogen: [He] 2s2 2p3.
According to octet rule every atom wants to cover the last orbit with highest possible electrons. To satisfy this Rubidium donates its one outer shell electron which is taken by Nitrogen atom.
Nitrogen atom has three less electrons to get full filled orbital structure. One Nitride ion coordinates with three Rubidium ions and produce Rb3N molecule.
The electrons that participate in bonding formation are written by straight lines between the atomic symbols.
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Hi…I am Triyasha Mondal, pursuing M.Sc in Chemistry. I am an enthusiastic learner. My specialization is in physical chemistry.
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