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This page shows the electron configurations of the neutral gaseous atoms in their ground states. For each atom the subshells are given first in concise form, then with all subshells written out, followed by the number of electrons per shell. For phosphorus (element 15) as an example, the concise form is [Ne] 3s 2 3p 3.
Configurations of elements 109 and above are not available. Predictions from reliable sources have been used for these elements. Grayed out electron numbers indicate subshells filled to their maximum. Bracketed noble gas symbols on the left represent inner configurations that are the same in each period. Written out, these are: He, 2, helium : 1s 2
This is a list of chemical elements and their atomic properties, ordered by atomic number (Z). Since valence electrons are not clearly defined for the d-block and f-block elements, there not being a clear point at which further ionisation becomes unprofitable, a purely formal definition as number of electrons in the outermost shell has been used.
The boron group is notable for trends in the electron configuration, as shown above, and in some of its elements' characteristics. Boron differs from the other group members in its hardness, refractivity and reluctance to participate in metallic bonding. An example of a trend in reactivity is boron's tendency to form reactive compounds with ...
At higher temperatures boron burns to form boron trioxide: [51] 4 B + 3 O 2 → 2 B 2 O 3 Ball-and-stick model of tetraborate anion, [B 4 O 5 (OH) 4 ] 2− , as it occurs in crystalline borax, Na 2 [B 4 O 5 (OH) 4 ]·8H 2 O. Boron atoms are pink, with bridging oxygens in red, and four hydroxyl hydrogens in white.
group 13 (boron group) Period: period 2: Block p-block: Electron configuration 2s 2 2p 1: Electrons per shell: 2, 3: Physical properties; Phase at STP: solid: Melting point: 2349 K (2076 °C, 3769 °F) Boiling point: 4200 K (3927 °C, 7101 °F) Density when liquid (at m.p.) 2.08 g/cm 3 : Heat of fusion: 50.2 kJ/mol : Heat of vaporization: 508 ...
The form of the periodic table is closely related to the atomic electron configuration for each element. For example, all the elements of group 2 (the table's second column) have an electron configuration of [E] n s 2 (where [E] is a noble gas configuration), and have notable similarities in their chemical properties.
Boron forms covalent bonds with other nonmetals and has oxidation states of 1, 2, 3 and 4. [19] [20] [21] Boron does not occur naturally as a free element, but in compounds such as borates. The most common sources of boron are tourmaline, borax, Na 2 B 4 O 5 (OH) 4 ·8H 2 O, and kernite, Na 2 B 4 O 5 (OH) 4 ·2H 2 O. [17] it is difficult to