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NH3 Lewis Structure: NH3 (Ammonia) has a trigonal pyramidal structure: central N atom with 5 valence electrons forms 3 N-H single bonds, using 3H atoms (1 electron each), and 1 lone pair on N. Bond angle: 107.8°, due to lone pair repulsion. Valence shell electron pair repulsion (VSEPR) theory explains shape; electron geometry: tetrahedral.
How to draw NH3 Lewis Structure
To draw the NH3 Lewis structure (ammonia) involves a few straightforward steps. This will help you understand the molecule’s electronic structure and bonding. Let’s break it down:
Count the Valence Electrons: Nitrogen (N) is in Group 15 of the periodic table, which means it has 5 valence electrons. Hydrogen (H) is in Group 1, having 1 valence electron. Since NH3 has one nitrogen atom and three hydrogen atoms, the total number of valence electrons is 5 + (3 * 1) = 8.
Sketch the Skeleton Structure: Place the nitrogen atom in the center because hydrogen cannot be a central atom. Draw single bonds between the nitrogen atom and each hydrogen atom. This will use up 3 pairs of electrons (6 electrons total).
Complete Octets for Outer Atoms: In the case of NH3, hydrogen atoms follow the duet rule instead of the octet rule (they only need 2 electrons to be stable). The single bonds you’ve drawn already fulfill this requirement for each hydrogen atom.
Place Remaining Electrons on the Central Atom: After bonding the hydrogens, you have 2 electrons left. These are placed on the nitrogen atom as a lone pair.
Check the Octet Rule: Nitrogen now has three single bonds (each bond consists of 2 electrons) plus one lone pair, making a total of 8 electrons around it, which satisfies the octet rule.
Consider Formal Charges (Optional for NH3 but good practice): To ensure the most stable structure, calculate the formal charge for each atom, which in the case of NH3, will show that all atoms have a formal charge of zero, indicating a stable structure.
The resulting Lewis structure for NH3 shows the nitrogen atom in the center with three hydrogen atoms bonded to it in a trigonal pyramidal geometry, and one lone pair of electrons on the nitrogen. This lone pair contributes to the molecule’s shape and properties, such as its basicity and its polar nature.
NH3 Lewis structure shape
The shape of Ammonia can be determined after drawing the NH3 Lewis structure. It denotes the formation internal geometry of the compound.
NH3 hold Trigonal pyramidal or distorted tetrahedral molecular geometry in terms of its shape. This shape is identified from the Lewis structure as it indicates the presence of one lone pair in the Nitrogen atom, which is centre atom in the compound.
NH3 Lewis structure formal charges
A fundamental formula helps to identify the formal charges held by the atoms in any compound. This is a significant characteristic, which is highly considerable in the case of drawing Lewis structure of the any compound.
The formula of finding formal charges is (valance electrons – nonbonding electrons – ½ bonding electrons).
Therefore, formal charge of Nitrogen atom is (5-2 + (1/2)6) = 0
Formal charge of each of the Hydrogen atoms (1-0+ (1/2)2) = 0
Summing up the individual formal charges of the atoms present in Ammonia the entire charge of the compound is estimated as zero.
NH3 Lewis structure lone pairs
The presence of lone pair is also denoted by Lewis structures of the compounds. As the lone pairs affect the shape of the compounds, it is important to identify the number of lone pairs in those compounds.
Ammonia has two lone pairs held by Nitrogen atom as the hydrogen atoms holds only two electrons, which participate in making bond pairs. Besides, this lone pairs effect on the polarity of the overall compound.
NH3 hybridization
Hybridization of the compounds are also encountered by the Lewis structure, which indicates the internal structure of the compounds, it also influences the shape of the compounds.
NH3 has sp3 hybridisation in the pyramidal or distorted tetrahedral shape. The hybridisation of Nitrogen atom denotes the overall hybridisation of Ammonia. The combination of 2s and 2p orbitals are found in the compound.
NH3 Lewis structure resonance
In the case of posing resonance, the compounds must hold one or more than one π bonds. Only sigma bonds cannot show resonating features in the compounds.
NH3 does not possess any π bonds in the molecular structure, which is lacking resonating characteristics in the Ammonia. Without presence of double bonds there is no chance of transitioning the bonds and structure by keeping the formula same.
NH3 Lewis structure octet rule
Octet rule says that the last energy level of the compounds gives extreme stability to the atoms by driving the atoms to precede electron-sharing process. The elements are likely to adopt the similar electronic configuration like the nearest noble gases by fulfilling their last electron shell of octet state.
In order to maintain this octet rule N and H both the atoms undergoes election-sharing method by sharing their valance electrons with each other. Hydrogen needs one electron for filling octet and Nitrogen needs three electrons for the same.
Each Hydrogen atoms partially adopts one electron from the last electronic shell of Nitrogen. Nitrogen shares its electrons with three hydrogen atoms for adopting three electrons from those hydrogen atoms partially as well.
NH3 polar or nonpolar
The difference between electronegativity of the atoms participate in the formation of any compounds is one of the important factor for finding polarity or amount of dipole moment in the compounds.
NH3 is a polar compound, which is imposed by the existence of dipole moment in the compound. Huge difference in electronegativity of Nitrogen and Hydrogen gives rise to this polar nature. Non-symmetrical pyramidal shape with the lone pairs in the compound is responsible for giving high polarity to the Ammonia.
NH3 Lewis structure bond angle
Bond angle can also be found from the Lewis structure. The bond angle of the compounds is quite dependent on the shape of the compounds and the place of the lone pairs.
The bond angle of NH3 is 107o, which is just a little bit lower than the standard bond angles of the compounds. This bond angle is the result of lone pair-bond pair and lone pair-lone pair repulsion, expressed by the molecular geometry.
NH3 Lewis structure electron geometry
Electron geometry refers to the molecular geometry of the compounds, which is fundamentally obtained from the Lewis structure of the compounds.
The molecular geometry of Ammonia denotes its distorted tetrahedral shape or pyramidal shape with slightly lower bond angle than the standard one. This happens due tie presence of lone pairs. The lone-pair-lone pair repulsion gives slightly bent structure to the electron geometry of Ammonia.
NH3 valence electrons
Valance electrons refer to those electrons, which are present in the last electronic shell of the elements. The number of valance electrum defines the capacity of adopting the dividing electrons of the periodic elements to satisfy octet.
In NH3, the number of valance electrons on Nitrogen is five and each of the three Hydrogen atoms holds one valance electron.
NH3 uses
Ammonia is used in several industrial productions. It has high demand in Agriculture as powerful fertiliser for cultivating crops.
The uses are:
Question 1: What is the difference between NH4+ and Ammonia?
Answer: NH3 possess zero charges in it. It is completely a neutral compound where NH4+ represent Ammonium ion which has one extra Hydrogen atom beyond its capacity.
Question 2: What is Aqueous Ammonia?
Answer: The dissolved state of Ammonia gas in water is called Aqueous Ammonia or Liquid Ammonia.
Question 3: Is ammonia Acidic or basic?
Answer: Ammonia is a basic compound with the pH between 11 and 12.
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Hi……I am Biswarup Chandra Dey, I have completed my Master’s in Chemistry from the Central University of Punjab. My area of specialization is Inorganic Chemistry. Chemistry is not all about reading line by line and memorizing, it is a concept to understand in an easy way and here I am sharing with you the concept about chemistry which I learn because knowledge is worth to share it.
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