Formic acid (HCOOH) Lewis structure, molecular geometry or shape, electron geometry, bond angle, hybridization, formal charges, polar or nonpolar
The simple chemical formula HCOOH represents formic acid, also known as methanoic acid. It is the simplest of carboxylic acids. The word ‘formic’ comes from the Latin formica which literally means ants. This name comes from the fact that formic acid was first isolated from ants.
Considering its multifold importance in chemistry, you will learn how to draw the Lewis dot structure of HCOOH, what is its molecular geometry or shape, electron geometry, bond angle, hybridization, formal charges, polarity, etc., all through this article.
So, continue reading!
|Name of Molecule||Formic acid|
|Molecular geometry of HCOOH||Trigonal planar|
|Electron geometry of HCOOH||Trigonal planar|
∠ (H-C-O) = 106° and 111°, ∠ (H-C=O) = 124° and ∠ (O-C=O)= 125°
|Total Valence electron in HCOOH||18|
|Overall Formal charge in HCOOH||Zero|
How to draw lewis structure of HCOOH?
The Lewis structure of formic acid (HCOOH) consists of three different elemental atoms, i.e., a carbon (C) atom, two hydrogens (H) atoms, and two atoms of oxygen (O).
The C-atom is present at the center. It is bonded to a hydrogen (H) atom and a hydroxyl (OH) functional group via single covalent bonds and to an oxygen (O) atom through a double covalent bond, respectively.
In this way, there are a total of 3 electron density regions or electron domains around the central C-atom in the HCOOH Lewis structure. All three electron domains are comprised of bond pairs; consequently, the central C-atom does not possess any lone pairs of electrons.
Steps for drawing the Lewis dot structure of HCOOH
1. Count the total valence electrons in HCOOH
The very first step while drawing the Lewis structure of HCOOH is to calculate the total valence electrons present in its concerned elemental atoms.
As three different elemental atoms are present in HCOOH, so you first need to look for the position of these elements in the Periodic Table.
Carbon (C) belongs to Group IV A (or 14), so it has a total of 4 valence electrons. Oxygen (O) is present in Group VI A (or 16), so it has 6 valence electrons, while hydrogen (H) lies at the top of the Periodic Table containing a single valence electron only.
- Total number of valence electrons in hydrogen = 1
- Total number of valence electrons in carbon = 4
- Total number of valence electrons in oxygen = 6
∴ The HCOOH molecule consists of 1 C-atom, 2 O-atoms, and 2 H-atoms. Therefore, the total valence electrons available for drawing the Lewis dot structure of HCOOH = 1(4) + 2(6) + 2(1) = 18 valence electrons.
2. Choose the central atom
In this second step, usually the least electronegative atom out of all the concerned atoms is chosen as the central atom.
This is because the least electronegative atom is the one that is most likely to share its electrons with the atoms spread around it.
Oxygen (E.N = 3.44) is more electronegative than both carbon and hydrogen. Hydrogen (E.N = 2.20) is less electronegative than carbon (E.N = 2.55). Still, it cannot be chosen as the central atom because a hydrogen (H) atom can accommodate only 2 electrons which denotes it can form a bond with a single adjacent atom only. This means H is always placed as an outer atom in a Lewis structure.
Consequently, the C-atom is placed at the center of the HCOOH Lewis structure while the O-atoms and the H-atoms are spread around it, as shown below.
3. Connect outer atoms with the central atom
In this step, the outer atoms are joined to the central C-atom using single straight lines.
But you must remember that an H-atom present next to the O-atom is only joined to the oxygen atom and not to the C-atom at the center. This is because an H-atom can form a single bond with one adjacent atom only in any Lewis structure. An oxygen atom is highly electronegative, so it readily forms a covalent chemical bond with its adjacent H-atom, not allowing the latter a chance to form a direct C-H bond.
All the other outer atoms, i.e., 1 H-atom and 2 O-atoms, are directly connected to the central C-atom, as shown below.
4. Complete the duplet and/or octet of the outer atoms
As we already identified, the hydrogen and oxygen atoms are the outer atoms in the Lewis dot structure of HCOOH.
Each hydrogen (H) atom requires a total of 2 valence electrons in order to achieve a stable duplet electronic configuration.
A C-H bond and an O-H single bond already represent 2 valence electrons around each H-atom. This means both the H-atoms already have a complete duplet in the Lewis structure drawn till yet. Thus, we do not need to make any changes with regard to the hydrogen atoms in this structure.
In contrast to that, an O-atom needs a total of 8 valence electrons to achieve a stable octet electronic configuration.
So first, see the O-atom marked as oxygen no.1. It is single-bonded to only one carbon atom.
The C-O bond represents 2 valence electrons, which denotes it still needs 6 more electrons to complete its octet. So these 6 electrons are placed as 3 lone pairs on the respective O-atom.
Now, if we see the O-atom marked as oxygen no. 2, it is single-bonded to an O-atom on one side and an H-atom on the other end. The C-H and O-H single bonds represent a total of 4 valence electrons around this O-atom which in turn hints at a deficiency of 4 electrons. So these 4 electrons are placed as 2 lone pairs around the respective O-atom.
In this way, both the outer O-atoms now have a complete octet in addition to a complete duplet of the H-atoms.
5. Complete the octet of the central atom by converting a lone pair into a covalent bond
- Total valence electrons used till step 4 = 4 single bonds + electrons placed around the oxygen shown as dots = 4(2) + 10 = 18 valence electrons.
- Total valence electrons – electrons used till step 4 = 18 – 18 = 0 valence electrons.
As all the valence electrons initially present for drawing the HCOOH Lewis structure are already consumed so there is no lone pair on the central C-atom in this structure.
However, a problem here is that this central C-atom only has a total of 3 single bonds around it which means 6 valence electrons. So it is still short of 2 more electrons to complete its octet.
But don’t worry at all because we have an easy solution to this problem. The solution is to convert a lone pair present on the O-atom containing 3 lone pairs into an extra chemical bond between the central C-atom and that O-atom.
This way, the central C-atom also has a complete octet comprised of 2 single bonds + 1 double bond.
Now that our problem is solved let’s check the stability of the HCOOH Lewis structure obtained above by applying the formal charge concept.
6. Check the stability of Lewis’s structure using the formal charge concept
The fewer formal charges present on the atoms of a molecule, the better the stability of its Lewis structure.
The formal charges can be calculated using the formula given below.
- Formal charge = [ valence electrons – nonbonding electrons- ½ (bonding electrons)]
Now let us use this formula and the Lewis structure obtained in step 5 to determine the formal charges present on HCOOH atoms.
For carbon atom
- Valence electrons of carbon = 4
- Bonding electrons = 1 double bond + 2 single bonds = 4 + 2(2) =8 electrons
- Non-bonding electrons = no lone pairs = 0 electrons
- Formal charge = 4-0-8/2 = 4-0-4 = 4-4 = 0
For hydrogen atoms
- Valence electrons of hydrogen = 1
- Bonding electrons = 1 single bond = 2 electrons
- Non-bonding electrons = no lone pairs = 0 electrons
- Formal charge = 1-0-2/2 = 1-0-1 = 1-1 = 0
For oxygen atom no. 1
- Valence electrons of oxygen = 6
- Bonding electrons = 1 double bond = 4 electrons
- Non-bonding electrons = 2 lone pairs = 2(2) = 4 electrons
- Formal charge = 6-4-4/2 = 6-4-2 = 6-6 = 0
For oxygen atom no. 2
- Valence electrons of oxygen = 6
- Bonding electrons = 2 single bonds = 2(2) = 4 electrons
- Non-bonding electrons = 2 lone pairs = 2(2) = 4 electrons
- Formal charge = 6 – 4 – 4/2 = 6 – 4 – 2 = 6 – 6 = 0
The above calculation shows that zero formal charges are present on the bonded atoms in the HCOOH Lewis structure. Thus it is a stable structure, and the good news is that we have drawn it correctly.
Also check –
What are the electron and molecular geometry of HCOOH?
Formic acid (HCOOH) possesses an identical electron and molecular geometry or shape, i.e., trigonal planar. To a C-atom at the center, one H-atom, one O-atom, and one OH group are attached, which makes a total of 3 electron density regions or electron domains around it.
There is no lone pair of electrons on the central C-atom, so no distortion is witnessed in the shape and geometry of HCOOH.
Molecular geometry of HCOOH
The molecular geometry or shape of formic acid (HCOOH) is trigonal planar.
The absence of any lone pair of electrons on the central C-atom means no lone pair-lone pair and lone pair-bond pair electronic repulsions exist in the molecule.
A bond pair-bond pair repulsive effect is present, which makes the bonded electron pairs occupy the three vertices of an equilateral triangle in a perfectly symmetrical molecular arrangement, as shown in the figure below.
Electron geometry of HCOOH
According to the valence shell electron pair repulsion (VSEPR) theory of chemical bonding, the ideal electron geometry of a molecule containing a total of 3 electron density regions around the central atom is trigonal planar.
In HCOOH, there are 2 single bonds and 1 double bond around the central carbon atom, which makes a total of 3 electron density regions. Thus, its electron geometry is also trigonal planar.
A shortcut to finding the electron and the molecular geometry of a molecule is by using the AXN method.
AXN is a simple formula to represent the number of atoms bonded to the central atom in a molecule and the number of lone pairs present on it.
It is used to predict the shape and geometry of a molecule based on the VSEPR concept.
AXN notation for HCOOH molecule
- A in the AXN formula represents the central atom. In HCOOH, a carbon (C) atom is present at the center, so A = C.
- X denotes the atoms bonded to the central atom. In HCOOH, 1 H-atom, 1 O-atom, and 1 OH group are directly bonded to the central C-atom. The OH group is considered 1 region of electron density. In short, X = 3 for HCOOH.
- N stands for the lone pairs present on the central atom. As per the Lewis structure of HCOOH, there are no lone pairs of electrons on the central carbon; hence N = 0.
As a result, the AXN generic formula for HCOOH is AX3.
Now, you may have a quick look at the VSEPR chart below.
The VSEPR chart confirms that the molecular geometry or shape of a molecule with an AX3 generic formula is identical to its ideal electron pair geometry, i.e., trigonal planar, as we already noted down for formic acid (HCOOH).
Hybridization of HCOOH
The central C-atom is sp2 hybridized in HCOOH.
The electronic configuration of carbon is 1s2 2s2 2p2.
During chemical bonding, the 2s atomic orbital of carbon hybridizes with two of its 2p atomic orbitals to produce three sp2 hybrid orbitals.
Each sp2 hybrid orbital is equivalent and contains a single electron only. It possesses a 33.3 % s-character and a 67.7 % p-character.
The sp2 hybrid orbitals of carbon overlap with the orbitals of adjacent atoms to form the required sigma (σ) bonds.
An unhybridized p-orbital of the central carbon atom overlaps with the p-orbital of the double-bonded O-atom to form the C=O pi (π) bond. Refer to the figure drawn below.
HCOOH hybridization can also be determined from its steric number. The steric number of the central C-atom in HCOOH is 3, so it has sp2 hybridization.
The HCOOH bond angle
The ideal bond angle in a symmetrical trigonal planar molecule is 120°. However, it is due to the different types of bonds present in HCOOH that four different bond angles exist in this molecule. In ascending order, the C-O-H bond angles are 106 ° and 111°, the H-C=O bond angle is 124°, and the O=C-O bond angle is 125° respectively.
Similarly, experimental studies revealed multiple bond lengths present in a formic acid molecule, including the O-H bond length (97 pm), the C-H bond length (110 pm), the C=O bond length (123 pm) and the longest C-O bond length (132 pm), as shown in the figure below.
Also check:- How to find bond angle?
Is HCOOH polar or nonpolar?
Pauling’s electronegativity scale states that a covalent chemical bond is polar if the bonded atoms have an electronegativity difference between 0.5 to 1.6 units.
In HCOOH, four different types of covalent bonds are present, i.e., a C-H bond, a C=O bond, a C-O bond, and an O-H bond.
A small electronegativity difference of 0.35 units exists between the carbon (E.N = 2.55) and hydrogen (E.N = 2.20) atoms. So the C-H bond is only weakly polar. Contrarily, a higher electronegativity difference of 0.89 units exists between a carbon and an oxygen (E.N = 3.44) atom. So both C-O and C=O bonds are strongly polar.
Above all, the O-H bond present in HCOOH is extremely polar as an electronegativity difference of 1.24 units exists between an oxygen and a hydrogen atom.
The highly electronegative oxygen atoms strongly attract the shared electron cloud from each bond of HCOOH.
A partial negative (δ–) charge develops on each O-atom while the C –atom and H-atoms acquire partial positive (δ+) charges.
The individual dipole moments of these polar bonds do not get canceled in the molecule overall. Thus, it is due to this non-uniform electron cloud distribution that HCOOH is a polar molecule (net µ = 1.42 D).
Read in detail–
What is the Lewis structure for HCOOH?
There is no lone pair of electrons on the central C-atom, while the outer O-atoms contain 2 lone pairs each.
How many bond pairs and lone pairs are present in the HCOOH Lewis structure?
The HCOOH Lewis structure consists of a total of 5 bond pairs and 4 lone pairs.
What is the shape or molecular geometry of HCOOH?
The formic acid (HCOOH) molecule possesses a trigonal planar shape or molecular geometry.
How is the shape of HCOOH different from its ideal electron pair geometry?
The formic acid (HCOOH) molecule has an identical electron and molecular geometry or shape, i.e., trigonal planar. Its AXN generic formula is AX3.
To one C-atom at the center, three different atoms are attached, and it has no lone pair of electrons.
Thus, no lone pair-lone pair or lone pair-bond pair repulsive effect exists in the molecule. Consequently, its shape and geometry stay undistorted.
- IF5 lewis structure and its molecular geometry
- CH2Cl2 lewis structure and its molecular geometry
- CH3COOH lewis structure and its molecular geometry
- C2H2Cl2 lewis structure and its molecular geometry
- CHCl3 lewis structure and its molecular geometry
- CH3F lewis structure and its molecular geometry
- CF2Cl2 lewis structure and its molecular geometry
- CH3CN lewis structure and its molecular geometry
- CH2O lewis structure and its molecular geometry
- The total number of valence electrons available for drawing formic acid (HCOOH) Lewis structure is 18.
- HCOOH has an identical electron and molecular geometry or shape, i.e., trigonal planar.
- The HCOOH molecule has sp2 hybridization.
- Multiple bond angles are present in the HCOOH molecule. The bond angles are ∠(H-C-O) = 106° and 111°, ∠(H-C=O) = 124° and ∠(O-C=O)= 125°.
- HCOOH is a polar molecule (net µ = 1.42 D).
- Zero formal charges present on all the bonded atoms account for the extraordinary stability of the HCOOH Lewis structure drawn in this article.
About the author
My name is Vishal Goyal and I am the founder of Topblogtenz. I hold a degree in B.tech (Chemical Engineering) and have a strong passion for the life sciences and chemistry. As a highly qualified and experienced chemistry tutor with 4 years of experience, I possess a deep understanding of the unique challenges that students often encounter when attempting self-study in the field of chemistry. I have created this website as a comprehensive resource for those who are seeking guidance and support in their chemistry studies. I have brought together a team of experts, including experienced researchers, professors, and educators, to provide our readers with accurate and engaging information on a wide range of chemistry and science topics. Our goal is to make complex subjects like chemistry accessible and understandable for all. I hope you find the information and resources on our site helpful in your studies. Let's connect through LinkedIn: https://www.linkedin.com/in/vishal-goyal-2926a122b/