Group+15Hr7

=Nitrogen group=

From Wikipedia, the free encyclopedia
http://en.wikipedia.org/wiki/Nitrogen_group http://www.britannica.com/EBchecked/topic/416304/nitrogen-group-element http://www.absoluteastronomy.com/topics/Nitrogen_group [|N] || [|P] || [|As] || [|Sb] || [|Bi] ||
 * ~ [|Group] → ||~ 15 ||
 * ~ ↓ [|Period] ||
 * ~ [|2] ||= 7
 * ~ [|3] ||= 15
 * ~ [|4] ||= 33
 * ~ [|5] ||= 51
 * ~ [|6] ||= 83

This group has the defining characteristic that all the component elements have 5 electrons in their outermost shell, that is 2 electrons in the s subshell and 3 unpaired electrons in the p subshell. They are therefore 3 electrons short of filling their outermost electron shell in their non-ionized state. The most important element of this group is **nitrogen** (**N**), which in its diatomic form is the principal component of air.
 * ~ Atomic # ||~ **Element** ||~ No. of Electron/Shells ||
 * 7 || nitrogen || 2, 5 ||
 * 15 || phosphorus || 2, 8, 5 ||
 * 33 || arsenic || 2, 8, 18, 5 ||
 * 51 || antimony || 2, 8, 18, 18, 5 ||
 * 83 || bismuth || 2, 8, 18, 32, 18, 5 ||

__**Nitrogen**__ Electron Configuration- 1s²2s²2p³ Quantum Numbers- n= 2 l= 1 ml= 1 ms= ½ Atomic Number- 7 Atomic Mass- 14 Number of Protons- 7 Number of Neutrons- 7 Number of Electrons- 7 Isotopes- 8

__**Phosphorus**__ Electron Configuration- 1s²2s²2p⁶3s²3p³ Quantum Numbers- n= 3 l= 1 ml= 1 ms= ½ Atomic Number- 15 Atomic Mass- 31 Number of Protons- 15 Number of Neutrons- 16 Number of Electrons- 15 Isotopes- 18

__**Arsenic**__ Electron Configuration- 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p³ Quantum Numbers- n= 4 l= 1 ml= 1 ms= ½ Atomic Number- 33 Atomic Mass- 75 Number of Protons- 33 Number of Neutrons- 42 Number of Electrons- 33 Isotopes- 14

__**Antimony**__ Electron Configuration- 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p³ Quantum Numbers- n= 5 l= 1 ml= 1 ms= ½ Atomic Number- 51 Atomic Mass- 122 Number of Protons- 51 Number of Neutrons- 71 Number of Electrons- 51 Isotopes- 51

__**Bismuth**__ Electron Configuration- 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²4f¹⁴5d¹⁰6p³ Quantum Numbers- n= 6 l= 1 ml= 1 ms= ½ Atomic Number- 83 Atomic Mass- 209 Number of Protons- 83 Number of Neutrons- 126 Number of Electrons- 83 Isotopes- 60

*Nitrogen:
 * Fun Facts**

Discoverer: Daniel Rutherford

Discovered at: Scotland Discovery date: 1772


 * Phosphorus was discovered, by Brandt in 1669
 * Bismuth was discovered by an unknown alchemist

The physical properties of this Group vary widely as nitrogen is a gas, and the other elements are solids of increasingly metallic character. Nitrogen exists as the diatomic molecule N2. It is a colourless, odourless gas, which condenses to a colourless liquid at 77K. The strength of the bond and the short bond length provide evidence for the bond between the N atoms being a triple bond. Phosphorus has at least two allotropes, red and white phosphorus. White phosphorus is a solid composed of covalent tetrahedral P4 molecules, and red phosphorus is an amorphous solid which has an extended covalent structure. The covalent radii of the atoms increase on descending the Group. However, the N atom is anomalously small and so it can multiple-bond to other N, C and O atoms.
 * Physical Properties Differences**

Both nitrogen and phosphorus exist in oxidation states +3 and +5 in their compounds. Nitrogen is very unreactive, mainly because its bond enthalpy is very high (944 kJ mol-1). The only element to react with nitrogen at room temperature is lithium, to form the nitride Li3N. Magnesium also reacts directly, but only when ignited. Some micro-organisms, however, have developed a mechanism for reacting directly with nitrogen gas and building it into protein - this is called nitrogen fixation, and is an important early step in the food chain. Phosphorus is more reactive than nitrogen. It reacts with metals to form phosphides, with sulfur to form sulfides, with halogens to form halides, and ignites in air to form oxides. It also reacts with both alkalis and concentrated nitric acid.
 * Chemical Properties Differences**

They all have the same l, ml, and ms quantum numbers.
 * Periodic Trends**

Google, Wikipedia
 * Sources:**