How many bonds does 5 valence electrons have?

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How many bonds do atoms with 5 valence electrons form?
How many bonds can Group 5 make?
What element has 5 valence electrons?
How many bonds can valence electrons form?

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The distinction between being a "central" atom and "external" atom is quite simple. Any atom bonded to more than one atom is a central atom; when bonded to only one atom it can be thought of as an external atom. For external atoms, the octet rule applies in all cases except for those elements smaller than carbon in the Periodic Table (eg. boron). For central atoms, only carbon, nitrogen and oxygen will always obey the octet rule; for elements below carbon, there are not enough available valence orbitals to accept more than 6 electrons, and for elements above oxygen the d orbitals are often available, thus allowing hybridisation.

Despite these limitations, you can view the octet rule as representing the ideal or default situation.

Although the idea of orbital overlap allows us to understand the formation of covalent bonds, understanding how molecular shapes arise using the simple s, p and d orbitals is not always possible, especially for polyatomic molecules. The approach taken by valence bond theory to rationalise geometries involves mixing together (or hybridising) these simple orbitals, all of which are perpendicular to each other, in order to obtain a different set of orbitals in a different geometrical arrangement (ie. with different angles between them). Hence, by mixing one s orbital with 3 p orbitals (each at 90° to the others) we can make 4 sp3 orbitals, each lying at 109° to the others. In this way, we can in part explain the bond angles observed in polyatomic molecules like H2O.

With regard to Lewis structures, hybridisation is of importance in that elements that have available d orbitals can mix these with the usually considered s and p orbitals to produce either 5 sp3d or 6 sp3d2 hybrid orbitals, thus allowing more than 8 valence electrons (10 and 12 respectively) to surround the central atom.

In drawing Lewis structures, you should follow the simple procedure outlined below.

Sum the valence electrons from all atoms within the molecule you wish to draw.
For an anion, you should add one more electron for each negative charge, and for a cation, you should subtract one electron for each positive charge. [Note: you do not need to worry about keeping track of where each electron comes from as it is only the total number of electrons which is important.]

Write down the symbols of each external atom and connect them to the central atom by a single (s-) bond.
You usually write atoms in the order in which they are connected within the molecule or ion. When one atom is an atom to which other atoms are bonded, you usually write this "central" atom first. For example, carbon is the central atom in carbon dioxide, CO2 . Occasionally, however, you may require further information to determine the order of bonding.
You can achieve the representation of the bond itself either by using a pair of dots or by a single line between the chemical symbols for each atom joined. Each method represents two electrons covalently shared between the atoms in forming the bond.
Complete the octets of the atoms surrounding the central atom
Remember the restrictions on those atoms smaller than carbon. For instance, hydrogen can only ever have two electrons.
Place any remaining electrons as pairs around the central atom even if doing so results in more than the octet.
If there are not enough electrons available to complete step 3, you can then try introducing multiple bonds.
You should introduce the multiple bonds one at a time, between the central atom and one of the other atoms, using one or more of the lone pairs on the external atom.

Hydrogen has one valence electron, carbon has 4 and nitrogen 5, for a total of 10 valence electrons. There are various ways in which you can combine these elements (HCN, HNC, CHN) but hydrogen can only accommodate 2 valence electrons and so can only bond to one other atom. Therefore, the H atom cannot be a central atom. Thus, you really only have two choices, HCN and HNC. Given that the molecule is written as HCN, the best starting point would be for you to assume that the carbon is a central atom, and construct the Lewis structure from there. We begin with a skeletal structure that joins each atom with one pair of electrons. These two "bonds" account for 4 valance electrons.
If we then place the remaining valence electrons as pairs around the nitrogen atom to give it its stable octet, we find that carbon is left with less than the octet.

Therefore, in order to produce a structure where carbon obeys the octet rule, we must introduce multiple bonds (between C and N, remembering that H can only bond once).

A double bond still leaves carbon short of the octet and so we arrive at a situation where the bond between C and N is a triple bond. This gives both C and N the stable octet structure.

A structure drawn with N as the central atom would end up similarly, with a triple bond between N and C. Without any other information, both Lewis structures are viable. However, it is found through experiment that the structure is HCN. In most cases it is always best for you to assume that the way a formula is written gives a clue to the identity of the central atom.

Total valence electrons is 26 (7 from Br, 6 from each O, and 1 for the negative charge). Again assuming that you write the central atom first, and following the steps outlined in the previous example, we get

Note that this ion is drawn within square brackets with the charge indicated at the upper right. This is the correct formulation that must be used for all Lewis structures of ions.

Total valence electrons is 18, six from each O atom. Bonding these atoms together by single bonds results in a structure where the central O atom is deficient in electrons (only 6 instead of 8).

Multiple bonding is therefore required. Bonding one of the external O atoms to the central O atom with a double bond sufficiently shares the electrons such that all 3 O atoms now have the stable octet of electrons.

Note that you can also draw this structure like this.

These two structures are called resonance structures, which simply means that each Lewis structure is equivalent to the other.

How many bonds do atoms with 5 valence electrons form?

Group 5A (15) elements such as nitrogen have five valence electrons in the atomic Lewis symbol: one lone pair and three unpaired electrons. To obtain an octet, these atoms form three covalent bonds, as in NH₃ (ammonia). Oxygen and other atoms in group 6A (16) obtain an octet by forming two covalent bonds.

How many bonds can Group 5 make?

Group 5A elements form 3 bonds.

What element has 5 valence electrons?

Elements having 5 valence electrons are placed in Group 15. The elements of group 15 are nitrogen, phosphorus, arsenic and antimony.

How many bonds can valence electrons form?

Generally speaking, each atom will form as many bonds as are necessary to completely fill its outermost electron shell. For example, oxygen is in group VI, and it has six valence electrons, but there is space for eight electrons in its valence shell.