Draw the lewis dot structure for rbio2.

Rubidium Iodite is an Ionic compound made up of Following two ions,

                                1) Rb⁺ (Cation)

                                2) IO₂⁻ (Anion)

Now in order to draw the lewis structure of Iodite ion (poly anion) we will follow following steps,

a) First add up the number of valence electrons of all elements,

So,

                    Number of valence electrons in I     = 7

                    Number of Valence electrons in O1 = 6

                    Number of Valence electrons in O2 = 6

                    Number of negative charges           = 1

                                                                         --------------

                                                                               20

b) Secondly draw I as the central atom surrounded by two oxygen atoms. Connect I with each O atom via a single bond and subtract 2 electrons per bond, so,

                                                             20

                                                             - 4

                                                          -----------

                                                              16

Now, divide these 16 electrons on all elements starting from most electronegative atom. You will find that each oxygen atom will atain 6 electrons in three pairs and I will attain 4 electrons in 2 pairs, after that make a double bond between one O and I so that the formal charge of I gets zero.

Hence, the structure of Iodite will be as shown below,

The RbIO₂ compound has a Lewis structure in IO₂⁻

The Lewis formula is used to describe covalent bonds

Lewis structures have a central atom and a terminal atom

The central atom is an atom that is bound to 2 or more other atoms, while a terminal atom is bound to 1 other atom

In describing Lewis's structure the steps that can be taken are:

In the RbIO₂ compound, the bond is an ionic bond that is Rb + and IO₂⁻ so that what Lewis can describe is the I and O bonds in IO₂⁻

Steps to draw the Lewis structure

From this it was found that atom I did not follow the octet rule because it binds 10 electrons, this is what is called the octet rule which was developed / expanded, whereas in general period 3 elements such as P, Br, I can have electrons exceeding 8 when they bind

adding electron dots as needed h3c ss ch3

link

formal charge

link

ionic bonding

link

Keywords: Lewis structure, single-bonded, double-bonded, octet

fdvwsa gfwsargebgeebbfwfwffw gwf   vgwgw gw f gwgw fgw v v dsv dwfff

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.