Charge of po4

Charge of po4 DEFAULT

What is the formal charge on the phosphate ion in #PO_3^-#?

Assigning formal charges assumes covalent character, meaning the electrons in a given chemical bond are assumed to be equally shared.


  • owned electrons are found by cleaving each bond homolytically so that one electron goes to each atom that was bonding.
  • valence electrons are found from the group number of the main group elements.

Of course, this is meaningless for a molecule as a whole. Furthermore, the ion you've quoted does not exist.

Phosphate is actually , and has the following resonance structure ( other permutations):

Assign the labels , . . . , starting from the top oxygen and going clockwise. Then, are identical in formal charge, as they are equivalent oxygens in this representation.

  • would bring in valence electrons, and it owns of them.

Thus, its formal charge is .

  • would each bring in valence electrons, and they each own of them.

Thus, their formal charges are all .

  • And lastly, the in the middle would bring in valence electrons, but own of them, having a formal charge of .

And we indeed still have a total charge of , i.e.


PO43- Lewis Structure (Phosphate ion)

Lewis structure of phosphate ion is drawn clearly in this tutorial step by step. Total valence electrons concept is used to draw the lewis structure of PO43- ion. In lewis structure, there should be charges on atoms.

Phosphate ion | PO43-

Phosphate ion is one of the oxyanion of phosphorous. Phosphorous is at +5 oxidation state in PO43-. Also, phosphate ion has a -3 charge.

Lewis structure of PO43- ion

In the lewis structure of PO43-, three is a double bond between phosphorous atom and one oxygen atom. Between other oxygen atoms, there are only single bonds with phosphorous atom. Also, each oxygen atom has a -1 charge.

PO43- lewis structure

Related lewis structures to H3PO4

H3PO2 lewis structure
H3PO3 lewis structure

Steps of drawing lewis structure of PO43-

Following steps are required to draw the PO43- lewis structure and they are explained in detail in this tutorial.

  1. Find total number of electrons of the valance shells of sulfur and oxygen atoms
  2. Total electrons pairs
  3. Center atom selection
  4. Put lone pairs on atoms
  5. Check the stability and minimize charges on atoms by converting lone pairs to bonds.

Drawing correct lewis structure is important to draw PO43- resonance structures correctly.

Total number of electrons of the valance shells of SO42-

Phosphorous is located at 5th group in the periodic table. Therefore phosphorous has five valence electrons in its last shell. Oxygen atom is located at sixth group in the periodic table and has six valence electrons in its last shell.

  • Total valence electrons given by phosphorous atom = 5

There are four oxygen atoms in PO43- ion, Therefore

  • Total valence electrons given by oxygen atoms = 6 *4 = 24

There are -3 charge on PO43- ion. Therefore there are three more electrons which comes from outside to contribute to the total valence electrons.

  • Total valence electrons = 5 + 24 + 3 = 32

Total valence electrons pairs

Total valance electrons pairs = σ bonds + π bonds + lone pairs at valence shells

Total electron pairs are determined by dividing the number total valence electrons by two. For, PO43- ion, Total pairs of electrons are 16.

Center atom of PO43- ion

To be the center atom, ability of having greater valance is important. Therefore sulfur has the more chance to be the center atom (See the figure) because sulfur can show valance of 6. Maximum valence of oxygen is two. So, now we can build a sketch of PO43- ion.

sketch of PO43- lewis structure

Mark electrons as lone pairs on atoms

  • There are already four P-O bonds around the phosphorous atom in the above sketch. Therefore only twelve (16-4 = 12) valence electrons pairs are remaining to draw the lewis structure.
  • First, mark those twelve valence electrons pairs as lone pairs on outside atoms (on oxygen atoms). One oxygen atom will take three lone pairs following the octal rule (oxygen atom cannot keep more than eight electrons in its valence shell).
  • For four oxygen atoms, twelve electrons pairs are spent. Now all electron pairs are spent. There is no electron pairs to mark on phosphorous atom.
mark valence electrons in lewis structure of phosphate ion

Charges on atoms

After, marking electron pairs on atoms, we should mark charges of each atom. Each oxygen atom will get a -1 charge and phosphorous atom get a +1 charge. The overall charge of ion is ( -1*4 + (+1) ) = -3.

mark charges on atoms in lewis structure of PO43

Check the stability and minimize charges on atoms by converting lone pairs to bonds

When charges exist everywhere (on atoms) in a ion or a molecule, that structure is not stable. We should try to reduce charges on atoms as much as possible. Now, we are going to learn how to reduce charges of atoms in sulfate ion.

  • Oxygen atoms should hold negative charges because electronegativity (3.5) of oxygen is higher than phosphorous (2.1). Otherwise, we can say, ability of holding negative charges is great in oxygen atoms than phosphorous atoms.
  • The drawn structure is not a stable one because all atoms have charges.
  • Now, we should try to minimize charges by converting lone pair or pairs to bonds. So convert one lone pair of one oxygen atom to make a new P-O bond.
  • Now there is a double bond between phosphorous atom and one oxygen atom (one P=O bond). Now, there are three P-O single bonds between phosphorous atom and other three oxygen atoms (three P-O bonds).

reduce charges by transfering lone pair in PO43- lewis structure

You see charges of atoms in PO43- are reduced. Now, there is no charge in one oxygen atom and phosphorous atom. So we have an stable ion than previous one.

Lewis structure of PO43-

lewis structure of PO43-.jpg

Can I reduce charges of atoms furthermore ?

You should know, phosphorous can keep more than eight electrons in its last shell. Therefore we can convert one more lone pair of another oxygen atom to a bond.

But, when you try to do this, phosphorous will get a -1 charge. Earlier in this tutorial, I told you that, most electronegative element should have the negative charges. Therefore, we cannot reduce charges furthermore.

reduce charges of sulfate ion lewis structure


How many oxygen atoms have charges in PO43- lewis structure?

Three oxygen atoms have charges. One oxygen atom holds - 1 charge and overall there is -3 charge.

In phosphate ion lewis structure, there is -3 charge. Are their charge and lone pairs on phosphorous atom?

There are no any charge on phosphorous atom in phosphate ion lewis structure. Also, there is no lone pair or pairs in phosphate ion lewis structure.

How do I get the lewis structure of H3PO4 from PO43- ?

Three hydrogen atoms are linked to oxygen atoms of PO43- in H3PO4 molecule. There were -1 negative charge on each of oxygen atom and they will be lost due to joining with hydrogen atoms.

Why phosphorous atom will not take a hydrogen atom to make a P-H bond?

If a hydrogen atom is joint to the phosphorous atom, phosphours atom will get a minus charge which is not acceptable because phosphorous has a lower electronegativity than oxygen.

Are there lone pairs on phosphorus atom in phosphate Lewis structure?

Around phosphorus atom, three single bonds and one double bond exist. No lone pairs exist on phosphorus atom. Also, no charge exists on phosphorus atom in Lewis structure of PO43-

SO32- lewis structure and resonance structures NO3- lewis structure NO3- resonance structuresNO2- lewis structureN2O lewis structure, resonance structures N2O5 resonance structuresResonance structures examplesH3PO4 lewis structure

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Drawing the Lewis Structure for PO43-

Video: Drawing the Lewis Structure for PO43-

For the PO4 3- Lewis structure use the periodic table to find the total number of valence electrons for the PO4 3- molecule. Once we know how many valence electrons there are in PO4 3- we can distribute them around the central atom with the goal of filling the outer shells of each atom.

In the Lewis structure of PO43- there are a total of 32 valence electrons.

For the Lewis structure for PO4 3- you should take formal charges into account to find the best Lewis structure for the molecule. Remember, PO4 3- has a negative three charge on the molecule. For the Lewis structure you'll need to have a total charge for the molecule of 3-.

It is helpful if you:

  • Try to draw the PO43- Lewis structure before watching the video.
  • Watch the video and see if you missed any steps or information.
  • Try structures similar to PO43- for more practice.

List of Lewis Structures

Lewis Structure: How to draw phosphate (PO4)

Charge? Phosphorus is an element and therefore has a balance of 15 protons and 15 electrons. Therefore has no charge. It can be ionised though, and then it prefers to take up 3 electrons and thereby become phosphide with a -3 charge.

Click to see full answer

Correspondingly, why does phosphate have a negative 3 charge?

Phosphate is PO4. Now, O needs 2 electrons to have 8 electrons in the outer shell and become stable. So the PO4 has an overall 3 electrons more than the protons it has. So it is negatively charged.

Likewise, is Phosphorus a positive or negative ion? Positive at last: A pure phosphorus cation. Summary: The main known forms of the element are white, red, and black phosphorus. In addition, there are hundreds of compounds in which phosphorus is present as an anion, a negatively charged ion.

Also to know, how many electrons are in the ion p3 -?

18 electrons

How do you know the charges of ions?

To find the ionic charge of an element you'll need to consult your Periodic Table. On the Periodic Table metals (found on the left of the table) will be positive. Non-metals (found on the right) will be negative. But you need to know the specific ionic charge elments.


Of po4 charge

What is the charge of po4?

In the Lewis structure of PO43- there are a total of 32 valence electrons. For the Lewis structure for PO4 3- you should take formal charges into account to find the best Lewis structure for the molecule. Remember, PO4 3- has a negative three charge on the molecule.

Besides, what is the charge of bromine?


Which elements are cations?

Positive and Negative Ions: Cations and Anions

  • The alkali metals (the IA elements) lose a single electron to form a cation with a 1+ charge.
  • The alkaline earth metals (IIA elements) lose two electrons to form a 2+ cation.
  • Aluminum, a member of the IIIA family, loses three electrons to form a 3+ cation.
  • The halogens (VIIA elements) all have seven valence electrons.

Is cathode negatively charged?

Both have an anode and a cathode. A battery is a charge-separating device. It stores electric energy by separating cations (positively-charged ions) and anions (negatively-charged ions). One terminal of the battery contains an excess of cations: this is the positive terminal (cathode).

Calculating PO43- Formal Charges: Formal Charges for the Phosphate Ion


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