Noble Gas Notation For Chlorine

v.twenty: Noble gas Configuration

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How does it feel to be total after a meal?

Envision that you accept nearly finished a great repast, only cannot put another bite in your oral cavity because there is no place for it to become. The noble gases have the aforementioned problem—at that place is no room for any more electrons in their outer shells. They are completely full and cannot handle any more than.

Element of group 0 Configuration

Sodium, chemical element number 11, is the first element in the tertiary catamenia of the periodic tabular array. Its electron configuration is \(1s^2 2s^2 2p^6 3s^i\). The offset ten electrons of the sodium atom are the inner-beat out electrons and the configuration of just those 10 electrons is exactly the same as the configuration of the element neon \(\left( Z=ten \right)\). This provides the ground for a shorthand notation for electron configurations chosen the noble gas configuration. The elements that are found in the last column of the periodic table are an of import group of elements chosen the noble gases. They are helium, neon, argon, krypton, xenon, and radon. A noble gas configuration of an atom consists of the elemental symbol of the last noble gas prior to that atom, followed by the configuration of the remaining electrons. So for sodium, we brand the exchange of \(\left[ \ce{Ne} \right]\) for the \(1s^2 2s^2 2p^six\) office of the configuration. Sodium's noble gas configuration becomes \(\left[ \ce{Ne} \right] 3s^1\). Table \(\PageIndex{1}\) shows the noble gas configurations of the tertiary menstruum elements.

Table \(\PageIndex{1}\): Electron Configurations of Third-Period Elements
Element Name	Symbol	Atomic Number	Element of group 0 Electron Configuration
Sodium	\(\ce{Na}\)	11	\(\left[ \ce{Ne} \right] 3s^ane\)
Magnesium	\(\ce{Mg}\)	12	\(\left[ \ce{Ne} \right] 3s^2\)
Aluminum	\(\ce{Al}\)	13	\(\left[ \ce{Ne} \right] 3s^2 3p^1\)
Silicon	\(\ce{Si}\)	fourteen	\(\left[ \ce{Ne} \correct] 3s^2 3p^2\)
Phosphorus	\(\ce{P}\)	xv	\(\left[ \ce{Ne} \right] 3s^2 3p^3\)
Sulfur	\(\ce{S}\)	16	\(\left[ \ce{Ne} \right] 3s^2 3p^4\)
Chlorine	\(\ce{Cl}\)	17	\(\left[ \ce{Ne} \right] 3s^2 3p^5\)
Argon	\(\ce{Ar}\)	18	\(\left[ \ce{Ne} \correct] 3s^2 3p^6\)

Again, the number of valence electrons increases from one to eight across the 3rd period.

The fourth and subsequent periods follow the aforementioned design, except for the use of a dissimilar element of group 0. Potassium has xix electrons, one more than than the noble gas argon, then its configuration could be written as \(\left[ \ce{Ar} \right] 4s^1\). In a similar fashion, strontium has two more electrons than the noble gas krypton, which would permit us to write its electron configuration equally \(\left[ \ce{Kr} \right] 5s^2\). All elements tin can be represented in this style.

Summary

The element of group 0 configuration system allows some shortening of the total electron configuration by using the symbol for the element of group 0 of the previous period every bit part of the pattern of electrons.

Review

What is the chemical element represented by \(\left[ \ce{Ne} \correct] 3s^2 3p^two\)?
What element has this electron configuration \(\left[ \ce{Ar} \right] 3d^7 4s^2\)?
What noble gas would be part of the electron configuration notation for Mn?
How would yous write the electron configuration for Ba?