Noble Gas Configuration For Silicon

In chemical science, the noble gas configuration is a shorthand method of writing an atom'southward electron configuration. The reason for using the element of group 0 configuration is considering the full electron configuration becomes very long for atoms with high atomic numbers.

Here is a look at how to write a noble gas configuration and a listing of the electron configurations for all 118 elements.

How to Write a Noble Gas Configuration

The noble gas configuration gives the noble gas core that occurs before the element on the periodic tabular array and then the electron configuration of the atom'south valence electrons. But, you need to understand how to write the total electron configuration to find the number of valence electrons.

Here are the steps for writing a noble gas configuration:

Aufbau Principle — Applying the Aufbau principle makes writing electron configurations much simpler.

Discover the number of electrons for the atom. For a neutral atom, this is the same equally the diminutive number. (For an ion, the number of electrons is not the aforementioned as the number of protons, but otherwise the same steps apply.)
Fill in the electron shells and energy levels with the electrons.
Each s trounce holds up to 2 electrons.
Each p trounce holds up to 6 electrons.
Each d crush holds up to ten electrons.
Each f shell holds up to 14 electrons.
Follow the Aufbau rule and write the full electron configuration. The Aufbau principle states that electrons fill lower energy levels before adding to higher energy levels. While you can apply brute force to write the configuration, information technology'due south easier to describe a diagram and follow the diagonal:
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d
7s 7p
8s

Notice the orbits overlap, so you don't just fill the shells sequentially (1, ii, 3, four, …). Instead, employ Madelung's rule:

1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f < 5d < 6p < 7s < 5f < 6d < 7p

Note: Madelung's rule is not a hard-and-fast rule, especially where some of the heavier transition metals are concerned. Relativistic furnishings come into play and change the gild.
Notice the noble gas preceding the element on the periodic table. Write the element of group 0 configuration by writing the noble gas core, followed by the valence electrons. A element of group 0 core is the noble gas element symbol enclosed in brackets: [He], [Ne], [Ar], [Kr], [Xe], or [Rn]. The valence electrons are "leftover" electrons that don't fill a shell or satisfy the octet rule (except for noble gases) or 18-electron rule (transition metals). There are two easy ways to place them. Valence electrons are the electrons leftover past the noble gas electron configuration. They are also characteristic of an chemical element group. For instance, the alkali metals always have ane valence electron.

Noble gas Configuration Examples

For example, write the noble gas configuration of sodium.

The atomic number of sodium is 11, so you know the neutral cantlet has 11 protons and besides 11 electrons.
Filling in the electron shells using the Aufbau principle gives a configuration of 1s² 2s² sp^six 3s^one. Add up the superscripts and double-check to brand sure you have the correct number of electrons.
Write the noble gas configuration. Looking at a periodic table, notation the noble gas before sodium is neon. The electron configuration of neon is 1s² 2sⁱⁱ 2p⁶. So, the noble gas core symbol [Ne] replaces that portion of the sodium electron configuration. The element of group 0 configuration for sodium is [Ne] 3s^ane.

For example, write the noble gas configuration of neon.

Neon is a noble gas, only you can exercise amend than just write [Ne] and phone call it proficient. First, use the periodic table and run into the number of electrons for a neon atom is ten.
Follow the Aufbau principle and fill electron shells: 1s^two 2s² 2p⁶
Write the noble gas configuration using the element of group 0 core earlier neon on the periodic table, followed past the valence electrons. The noble gas configuration of neon is [He] 2s² 2p^{half dozen}. Observe the valence of neon is viii (2 electrons in the 2s beat and 6 electrons in the 2p beat out), which indicates it has a filled octet.

List of Noble gas Configurations for All 118 Elements

NUMBER	Chemical element	ELECTRON CONFIGURATION
1	Hydrogen	1s¹
ii	Helium	1s²
three	Lithium	[He]2s¹
4	Glucinium	[He]2s^two
5	Boron	[He]2s²2pⁱ
6	Carbon	[He]2s²2p^two
7	Nitrogen	[He]2s²2p³
viii	Oxygen	[He]2s²2p^four
ix	Fluorine	[He]2s²2p⁵
ten	Neon	[He]2sⁱⁱ2p⁶
11	Sodium	[Ne]3s¹
12	Magnesium	[Ne]3s^two
13	Aluminum	[Ne]3s²3p^one
14	Silicon	[Ne]3s²3p²
xv	Phosphorus	[Ne]3s^two3p³
16	Sulfur	[Ne]3s²3p⁴
17	Chlorine	[Ne]3s²3p⁵
18	Argon	[Ne]3s^two3p^half-dozen
19	Potassium	[Ar]4s¹
20	Calcium	[Ar]4s²
21	Scandium	[Ar]3d¹4sⁱⁱ
22	Titanium	[Ar]3d²4s²
23	Vanadium	[Ar]3d³4sⁱⁱ
24	Chromium	[Ar]3d⁵4s¹
25	Manganese	[Ar]3d⁵4s²
26	Iron	[Ar]3d⁶4sⁱⁱ
27	Cobalt	[Ar]3d⁷4sⁱⁱ
28	Nickel	[Ar]3d⁸4sⁱⁱ
29	Copper	[Ar]3d^x4s¹
30	Zinc	[Ar]3d¹⁰4s²
31	Gallium	[Ar]3d¹⁰4s²4p¹
32	Germanium	[Ar]3d^x4s²4p²
33	Arsenic	[Ar]3d¹⁰4s²4pⁱⁱⁱ
34	Selenium	[Ar]3d¹⁰4s²4p⁴
35	Bromine	[Ar]3d¹⁰4s²4p^v
36	Krypton	[Ar]3d^x4s²4p⁶
37	Rubidium	[Kr]5s^ane
38	Strontium	[Kr]5s²
39	Yttrium	[Kr]4d¹5sⁱⁱ
40	Zirconium	[Kr]4dⁱⁱ5s²
41	Niobium	[Kr]4d⁴5s¹
42	Molybdenum	[Kr]4d^v5s¹
43	Technetium	[Kr]4d⁵5s²
44	Ruthenium	[Kr]4d⁷5s¹
45	Rhodium	[Kr]4d⁸5s¹
46	Palladium	[Kr]4d¹⁰
47	Argent	[Kr]4d^x5s^ane
48	Cadmium	[Kr]4d^ten5s²
49	Indium	[Kr]4d^x5s²5p¹
50	Can	[Kr]4d¹⁰5s²5p²
51	Antimony	[Kr]4d^x5s²5p^three
52	Tellurium	[Kr]4d¹⁰5s^two5p⁴
53	Iodine	[Kr]4d¹⁰5s²5p^v
54	Xenon	[Kr]4d¹⁰5s²5p^{half dozen}
55	Cesium	[Xe]6s¹
56	Barium	[Xe]6s²
57	Lanthanum	[Xe]5dⁱ6s²
58	Cerium	[Xe]4f^ane5d¹6s²
59	Praseodymium	[Xe]4f³6s²
lx	Neodymium	[Xe]4f⁴6s²
61	Promethium	[Xe]4f⁵6s²
62	Samarium	[Xe]4f^vi6sⁱⁱ
63	Europium	[Xe]4f⁷6sⁱⁱ
64	Gadolinium	[Xe]4f^vii5d¹6s²
65	Terbium	[Xe]4f⁹6sⁱⁱ
66	Dysprosium	[Xe]4f¹⁰6s²
67	Holmium	[Xe]4f^xi6sⁱⁱ
68	Erbium	[Xe]4f¹²6s^two
69	Thulium	[Xe]4f^thirteen6s²
lxx	Ytterbium	[Xe]4f¹⁴6s²
71	Lutetium	[Xe]4f^xiv5d¹6s^two
72	Hafnium	[Xe]4f¹⁴5d²6s^two
73	Tantalum	[Xe]4f¹⁴5d³6s²
74	Tungsten	[Xe]4f¹⁴5d^iv6s²
75	Rhenium	[Xe]4f^fourteen5d⁵6s²
76	Osmium	[Xe]4f¹⁴5d^half-dozen6s²
77	Iridium	[Xe]4f^xiv5d⁷6s²
78	Platinum	[Xe]4f¹⁴5d⁹6s¹
79	Gilt	[Xe]4f¹⁴5d^x6s¹
80	Mercury	[Xe]4f¹⁴5d¹⁰6sⁱⁱ
81	Thallium	[Xe]4f¹⁴5d^ten6s²6p¹
82	Lead	[Xe]4f^xiv5d¹⁰6s^two6p²
83	Bismuth	[Xe]4f¹⁴5d^ten6s²6p³
84	Polonium	[Xe]4f¹⁴5d^x6s²6p⁴
85	Astatine	[Xe]4f¹⁴5d¹⁰6s²6p⁵
86	Radon	[Xe]4f¹⁴5d¹⁰6sⁱⁱ6p⁶
87	Francium	[Rn]7sⁱ
88	Radium	[Rn]7s²
89	Actinium	[Rn]6d^ane7s²
90	Thorium	[Rn]6d²7s^two
91	Protactinium	[Rn]5f²6d¹7s²
92	Uranium	[Rn]5f³6dⁱ7s²
93	Neptunium	[Rn]5f⁴6d¹7s²
94	Plutonium	[Rn]5f^six7sⁱⁱ
95	Americium	[Rn]5f⁷7s²
96	Curium	[Rn]5f⁷6d^ane7s²
97	Berkelium	[Rn]5f^ix7s²
98	Californium	[Rn]5f¹⁰7s²
99	Einsteinium	[Rn]5f¹¹7s²
100	Fermium	[Rn]5f¹²7s²
101	Mendelevium	[Rn]5f¹³7s²
102	Nobelium	[Rn]5f^xiv7s²
103	Lawrencium	[Rn]5f¹⁴7s²7p¹
104	Rutherfordium	[Rn]5f¹⁴6d²7s²
105	Dubnium	*[Rn]5f¹⁴6d^three7s²
106	Seaborgium	*[Rn]5f^xiv6d⁴7s²
107	Bohrium	*[Rn]5f¹⁴6d^v7s²
108	Hassium	*[Rn]5f¹⁴6d^half-dozen7s²
109	Meitnerium	*[Rn]5f¹⁴6d⁷7s^two
110	Darmstadtium	*[Rn]5f¹⁴6d^ix7s^ane
111	Roentgenium	*[Rn]5f¹⁴6d^ten7s^ane
112	Copernium	*[Rn]5f¹⁴6d¹⁰7s²
113	Nihonium	*[Rn]5f^fourteen6d¹⁰7sⁱⁱ7p¹
114	Flerovium	*[Rn]5f^fourteen6d¹⁰7s²7p²
115	Moscovium	*[Rn]5f^xiv6d¹⁰7s²7pⁱⁱⁱ
116	Livermorium	*[Rn]5f¹⁴6d¹⁰7s^two7p⁴
117	Tennessine	*[Rn]5f¹⁴6d¹⁰7s^two7p^five
118	Oganesson	*[Rn]5f¹⁴6d¹⁰7s²7p⁶

Element of group 0 configurations with * are predicted values.

References

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Langmuir, Irving (June 1919). "The Arrangement of Electrons in Atoms and Molecules". Journal of the American Chemical Society. 41 (6): 868–934. doi:ten.1021/ja02227a002
Rayner-Canham, Geoff; Overton, Tina (2014). Descriptive Inorganic Chemistry (6th ed.). Macmillan Education. ISBN 978-1-319-15411-0.
Stoner, E.C. (1924). "The distribution of electrons amidst diminutive levels". Philosophical Magazine. 6th Series. 48 (286): 719–36. doi:ten.1080/14786442408634535
Wong, D. Pan (1979). "Theoretical justification of Madelung's rule". Journal of Chemical Education. 56 (11): 714–18. doi:10.1021/ed056p714