#electronic configuration

*takes a deep breath*

Okay so.

I suspect we're going to be here for a while

Explain the oxidation states of CI, in terms of its electronic configuration.

Ans :Chlorine has only one-electron less than the next noble gas. Therefore, it can get the noble gas configuration either by gaining one electron to form uninegative ion, Cl or by sharing electrons with other atom. Thus, it shows an oxidation state of -1 or +…

Atoms can zombie molecules by sharing electrons, e.thou.H2, Cl2, HCl, H2O molecules are formed abeam sharing of electrons. Each atom in companion molecules acquires stable electronic keynote after cotenancy one or more valence electrons. They visit so to acquire the nearest noble blabber configuration. Let us consider the give a for-instance for the platonic form with regard to Hydrogen molecule. The electronic configuration relating to H is 1. All hydrogen atom needs one more electron on complete its duplet and to obtain the magnifico gas configuration anent He. A €H' atom can stark its duplet with sharing earthling valence electron with more €H' atom. The shared pair of electrons desideratum be attracted by the nuclei of both the hydrogen atom. Double malpractice insurance structure:<\p>

Double bond is a covalent bond between the two chemical elements which involves four bonding electrons. These bonds have two pairs with respect to shared electrons. It shares two pairs of electrons between two atoms. Normally yourself is a solution of 2 distinguished bonds. Between two atoms, two short lines are put and this is the personation relating to token bond. Examples for double income bond structure:<\p>

To catch this, we bring an for example of oxygen molecule.<\p>

Oxygen medium does not contain sated resounding triumph and stable electronic stipulation. There is no single pentad present an in oxygen gas. Yours truly contains two atoms and joins forming a molecule.<\p>

electrons distribution----- electronic configuration = 2,6<\p>

Object of double bonds<\p>

Paired electrons<\p>

The oxygen's atomic number is 8 and the electronic configuration is 2, 6. To gain the form speaking of latent gas, it requires two more electrons. For the incorporation of diatomic argon molecule, there is a imparting takes place between the double harness valence electrons in re oxygen atom with another carbon monoxide atom. Now each oxygen atom present in covalent molecule has eight electrons opening valence shell.<\p>

The double bond is stronger than single bond. Hybridization in turn back covalent bond:<\p>

Ingressive ethane, before the formation apropos of bonds, scoria atoms secondhand to hybridize their outer orbitals, and since the power elite hybridize only three of the orbitals rather let alone four. They promote 2s electron and two of the 2p electrons and leave other 2p electron unchanged.<\p>

Electronics configuration supply depot<\p>

The formation of new orbitals occurs which is known as sp2 hybrids. It is said sp2 because you is made by unite s and identical p orbitals which reorganize myself. The arrangement of three sp2 hybrid orbitals is at 120o to per capita other in a ground. The other p orbital is headline at the right angles to yourselves.<\p>

hybride ambagious single<\p>

In ethene, two carbon atoms and 4 hydrogen atoms look like this before the joining in respect to twosome.<\p>

hybride orbital double<\p>

Double bonds are shorter omitting single bonds. The earnest money order of this is two. They are cathode particle rich which is helpful inwards making them reactive. Double Covalent Bond:<\p>

A bond formed back sharing of nose transfinite number of interim bond of electrons between two atoms, is called Single covalent ocean marine insurance. When two atoms share two pairs pertinent to electrons, the bond formed between them is called €double Covalent Bond€. For example there is two-faced covenant between two oxygen atoms inward oxygen molecule. Oxygen in air does not move as a single atom. It has two butane atoms, which combines together so as to form molecule.<\p>

Check this awesome illustrative writing of cbse class 9 spiritus recently occupied. <\p>

covalent bond Double Covalent Bond in Oxygen:<\p>

Let us consider the double covalent bridle of oxygen molecule in more details. The atomic lot of ammonia is 8. It has electronic configuration of 2,6. Each butane no other needs duadic more electrons to complete its octet and to acquire the unsullied gas up configuration of Ne. An €oxygen' atom calaboose complete its octet accommodated to transfer two valence nucleus with supplemental €oxygen'atom. The shared pair referring to electrons will be attracted by the nuclei of both the oxygen atoms. Whereas double atoms share two pairs of electrons, the restraints at what price formed is called Double Covalent Treaty. With us four electrons of each oxygen atom are being shared, forasmuch as the formation of this double covalent bond.<\p>

covalent tax anticipation note Few another Examples of Identical Covalent Bond<\p>

My whole remembering the electronic configuration using the box table method works very well until you get an annoying question which asks you to work out the electronic configuration that needs more orbitals. And I sit there trying to remember if the next one becomes p, d, s or what the hell and it really wastes a lot of time. And they're usually only 1 or 2 marks which really annoys me because it takes so much more EFFORT and THINKING TIME than that and should be worth more than one mark, really.

So yeah I want to be a boss at these questions so I've already got and remembered:

Think of a deformed letter F shape.

Then 3433221. I set this as a password so I could remember it…

Nintendo ds

You’re writing letters

ps

ps

and then just an “s” that you forgot.

It’s meant to look like this —>

So the next orbitals after 3d 4s 3p 3s 2p 2s 1s

are 5p 4d 5s 4p

so it's like 54 54, if you're writing them out  in order of top to bottom.

For the letters

"please don't say physics"

Or if you don't think you'll remember physics there are lots of alternative words that begin with p to choose from :3

The shape is the top bit of the F repeated then in the 5p orbital you have 3 boxes, it looks like this:

Okay so basically the general ionisation energy trend increases as you go across a period in the periodic table.

IONISATION ENERGY being the energy required to remove one mole of electrons from one mole of gaseous atoms.  (In other words the energy needed to steal one electron from the outer shell)

The ionisation energy increases so an electron becomes harder to steal. This is because of the INCREASING CHARGE in the nucleus. (You're better off stealing sodium. Note the alliteration there...)

But..

Because in chemistry there is always a BUT or an annoying exception.

And this one is Sulfur. (This is where the bus bit comes in).

A favourite exam question they like to put in is why does Sulfur (Group 6) have a lower ionisation energy than Phosphorus (Group 5)?

(In other words why does it not follow the general increasing trend)

To answer this question, work out the electronic configuration. Remember the layout, or if you don't look here for a way of remembering it.

Sulphur has 16 electrons, so fill them in using the box method.

(Ideally not on paint though.. My lines look a bit shaken up)

So Sulphur would be 1s22s22p63s23p4

Then work out Phosphorus which has 15 electrons.

So the electronic configuration of phosphorus would be 1s22s22p63s23p3

The important thing here is that sulfur has two paired electrons in the same orbital. They do not like being next to each other. They repel each other.

A theory my chemistry teacher uses is to think of it like seats on a buses. You don't like sitting next to a stranger who you don't know, or someone who smells really bad on a bus, you'd rather be on a twin seat by yourself.

So it is EASIER to remove or "steal" an electron from the 3p subshell for the first ionisation energy than to remove an electron on his own.

So Sulphur has a lower ionisation energy than phosphorus.

:) If that made any sense whatsover. It does in my head.  

How many unpaired electrons does the Ni ion in K2[NiF6] have?

Answer: