nitrogen is trigonal pyramidal. (f) The Lewis electron-dot diagram of N2H4 is shown below. In order to complete the octets on the Nitrogen (N) atoms you will need to form . Molecules can form single, double, or triple bonds based on valency. Considering the lone pair of electrons also one bond equivalent and with VSEPR Theory adapted, the NH2 and the lone pair on each nitrogen atom of the N2H4 molecule assume staggered conformation with each of H2N-N and N-NH2 segments existing in a pyramidal structure. this carbon, so it's also SP three hybridized, and The electron configuration of oxygen now has two sp3 hybrid orbitals completely filled with two electrons and two sp3 hybrid orbitals with one unpaired electron each. Nitrogen will also hybridize sp 2 when there are only two atoms bonded to the nitrogen (one single and one double bond). 3. hybridized, it's geometry is not tetrahedral; the geometry of that oxygen there is bent or angual. This is almost an ok assumtion, but ONLY when talking about carbon. As you closely see the N2H4 lewis structure, hydrogen can occupy only two electrons in its outer shell, which means hydrogen can share only two electrons. Identify the hybridization of the N atoms in N2H4. of those sigma bonds, you should get 10, so let's Also, the shape of the N2H4 molecule is distorted due to which the dipole moment of different atoms would not cancel amongst themselves. 2. Hence, the total formal charge on the N2H4 molecule becomes zero indicating that the derived structure is stable and accurate. in terms of pi bonds, we had three pi bonds, so three pi bonds for this molecule. So, the AXN notation for the N2H4 molecule becomes AX3N1. It's also called Diazane, Diamine, or Nitrogen Hydride, and it's an alkaline substance. For sp3d hybridized central atoms the only possible molecular geometry is trigonal bipyramidal. I am Savitri,a science enthusiast with a passion to answer all the questions of the universe. so the hybridization state. carbon, and let's find the hybridization state of that carbon, using steric number. Download scientific diagram | Colour online) Electrostatic potentials mapped on the molecular surfaces of (a) pyrazine, (b) pyrazine HF and (c) pyrazine ClF. Students also viewed. hybridized, and therefore the geometry is trigonal planar, so trigonal planar geometry. So, the two N atoms to complete their octet do the sharing of three electrons of each and make a triple covalent bond. Shared pair electrons in N2H4 molecule = a total of 10 shared pair electrons(5 single bonds) are present in N2H4 molecule. However, the H-N-H and H-N-C bonds angles are less than the typical 109.5 o due to . Sigma bonds are the FIRST bonds to be made between two atoms. "name": "Why is there no double bond in the N2H4 lewis dot structure? We had 14 total valence electrons available for drawing the N2H4 lewis structure and from them, we used 10 valence electrons. Well, that rhymed. The total valence electron is 12 for drawing N2H2 Lewis structure and it shows molecular geometry is bent and electronic geometry is trigonal planar. In a sulfide, the sulfur is bonded to two carbons. Hyper-Raman Spectroscopic Investigation of Amide Bands of N -Methylacetamide in Liquid/Solution Phase. The bond between atoms (covalent bonds) and Lone pairs count as electron domains. Steric number is equal What is the name of the molecule used in the last example at. The lone pair electrons on the nitrogen are contained in the last sp3 hybridized orbital. As we know, lewiss structure is a representation of the valence electron in a molecule. The nitrogen atom is sp hybridized, that indicates it consists of four sp hybrid orbitals. with ideal bond angles of 109 point five degrees So, there is no point we can use a double bond with hydrogen since a double bond contains a total of 4 electrons. Enter the email address you signed up with and we'll email you a reset link. As nitrogen atoms will get some formal charge. See answer. But the bond N-N is non-polar because of the same electronegativity and the N-H bond is polar because of the slight difference between the electronegativity of nitrogen and hydrogen. The hybridization of each nitrogen in the N2H4 molecule is Sp3. However, phosphorus can have have expanded octets because it is in the n = 3 row. The Lewis structure of diazene (N 2 H 2) shows a total of 4 atoms i.e., 2 nitrogen (N) atoms and 2 hydrogens (H) atoms. It is a strong base and has a conjugate acid(Hydrazinium). Therefore, we got our best lewis diagram. The hybrid orbitals are used to show the covalent bonds formed. four; so the steric number would be equal to four sigma When you have carbon you can safely assume that it is hybridized. around that carbon, therefore, it must be SP three hybridized, with tetrahedral geometry, Count the number of lone pairs attached to it. This was covered in the Sp hybridization video just before this one. What is the hybridization of the indicated atoms in Ambien (sedative used in the treatment of insomnia). It is used in pharmaceutical and agrochemical industries. Two domains give us an sp hybridization. those bonds is a sigma bond, and one of those bonds is a pi bond, so let me go ahead, and also draw in our pi bonds, in red. The Journal of Physical Chemistry Letters 2021, 12, 20, 4780-4785 (Physical Insights into Materials and Molecular Properties) Publication Date (Web): May 14, 2021. document.getElementById( "ak_js_1" ).setAttribute( "value", ( new Date() ).getTime() ); Welcome to Techiescientist.com. Answer: If any bond angle, involving p orbital electrons in the bonding, in any molecule is other than 90 deg, one has to conclude that there is orbital hybridization. three, four, five, six, seven, eight, nine, and 10; so we have 10 sigma bonds total, and The bond angle of N2H4 is subtended by H-N-H and N-N-H will be between 107 109. which I'll draw in red here. Add these two numbers together. so practice a lot for this. (e) A sample of N2H4 has a mass of 25g. This carbon over here, Adding the valence electrons of all the atoms to determine the total number of valence electrons present in one molecule N2H4. The electron geometry for the N2H4 molecule is tetrahedral. Each atom in the molecule contributes a set number of valence electrons depending upon their atomic number and position on the periodic table. Hydrazine is highly flammable and toxic to human beings, producing seizure-like symptoms. Advertisement. Hydrogen (H) only needs two valence electrons to have a full outer shell. The two unpaired electrons in the hybrid orbitals are considered bonding and will overlap with the s orbitals in hydrogen to form O-H sigma bonds. T, Posted 7 years ago. Those with 4 bonds are sp3 hybridized. The nitrogen in NH3 has five valence electrons. Therefore, the two Nitrogen atoms in Hydrazine contribute 5 x 2 = 10 valence electrons. So for N2, each N has one lone pair and one triple bond with the other nitrogen atom, which means it would be sp. Answer. If all the bonds are in place the shape is also trigonal bipyramidal. An alkyne (triple bond) is an sp hybridized carbon with two pi bonds and a sigma bound. bent, so even though that oxygen is SP three (a) State the meaning of the term hybridization. Having an MSc degree helps me explain these concepts better. Just as for sp 3 nitrogen, a pair of electrons is left on the nitrogen as a lone pair. Therefore, there are 6 fluorine atoms in this molecule. Concentrate on the electron pairs and other atoms linked directly to the concerned atom. Subjects English History Mathematics Biology Spanish Chemistry Business Arts Social Studies. This step is crucial and one can directly get . The C=O bond is linear. Score: 4.3/5 (54 votes) . four, a steric number of four, means I need four hybridized orbitals, and that's our situation Therefore, the valence electron for nitrogen is 5 and for hydrogen, it is 1. doing it, is to notice that there are only All of the nitrogen in the N2H4 molecule hybridizes to Sp3. more bond; it's a single-bond, so I know that it is a sigma bond here, and if you count up all In the case of the N2H4 molecule we know that the two nitrogen atoms are in the same plane and also there is no electronegativity difference between these two atoms, hence, the bond between them is non-polar. The oxygen is sp3 hybridized which means that it has four sp3 hybrid orbitals. Shared pair electrons(3 single bond) = 6, (5 2 6/2) = 0 formal charge on the nitrogen atom, Shared pair electrons(one single bond) = 2, (1 0 2/2) = o formal charge on the hydrogen atom. to number of sigma bonds, plus numbers of lone pairs of electrons, so there are two sigma In fact, there is sp3 hybridization on each nitrogen. As you see the molecular geometry of N2H4, on the left side and right side, there is the total number of four N-H bonds present. SN = 4 sp. only single-bonds around it, only sigma bonds, so We aim to make complex subjects, like chemistry, approachable and enjoyable for everyone. The hybridization of the N atoms is sp3. Since there are only two regions of electron density (1 triple bond + 1 lone pair), the hybridization must be sp. Best Answer. In N2H4, each N has two H bonded to it, along with a single bond to the other end, and one lone pair. After hybridization these five electrons are placed in the four equivalent sp3 hybrid orbitals. does clo2 follow the octet rule does clo2 follow the octet rule Next, the four Hydrogen atoms are placed around the central Nitrogen atoms, two on each side. SN = 2 sp. Shared pair electrons in N2H4 molecule = a total of 10 shared pair electrons(5 single bonds) are present in N2H4 molecule. So you get, let me go ahead The hybrid orbitals so formed due to intermixing of atomic orbitals are named after their basic orbitals i.e. It is corrosive to tissue and used in various rocket fuels. Here's a shortcut for how to determine the hybridization of an atom in a molecule that will work in at least 95% of the cases you see in Org 1. In hydrazine, nitrogen is central atom and both the nitrogen is sp 3 hybridized having a pair of nonbonding electrons in each of the nitrogen. N2H4 is polar in nature and dipole moment of 1.85 D. The formal charge on nitrogen in N2H4 is zero. Hurry up! the giraffe is 20 feet tall . so SP three hybridized, tetrahedral geometry. Note that, in this course, the term "lone pair" is used to describe an unshared pair of electrons. lives easy on this one. Now lets talk about the N-N bond, each nitrogen has three single bonds and one lone pair. To understand better, take a look at the figure below: The valence electrons are now placed in between the atoms to indicate covalent bonds formed. Post this we will try to draw the rough sketch of the Lewis diagram by placing the atoms in a definite pattern connected with a single bond. The formal charge is a hypothetical concept that is calculated to evaluate the stability of the derived lewis structure. Direct link to famousguy786's post There is no general conne, Posted 7 years ago. One lone pair is present on each N-atom at the center of . Shared pair electrons are also called the bonded pair electrons as they make the covalent between two atoms and share the electrons. 3. describe the geometry about one of the N atoms in each compound. Correct answer - Identify the hybridization of the N atoms in N2H4 . C) It has one sigma bond and two pi bonds between the two atoms. The hybridization of O in diethyl ether is sp. There are a total of 12 valence electrons in this Lewis structure i.e., 12/2 = 6 electron pairs. Note! Lone pair electrons in N2H4 molecule = Both nitrogen central atom contains two lone pair. }] AboutTranscript. Ten valence electrons have been used so far. There are exceptions where calculating the steric number does not give the actual hybridization state. . So, steric number of each N atom is 4. Due to the sp3 hybridization the oxygen has a tetrahedral geometry. Answer (1 of 2): In hydrazine, H2NNH2, each of two N atoms is attached to, two H atoms through two sigma bonds and one N atom through one sigma bond and carries a lone pair. We know, there is one lone pair on each nitrogen in the N2H4 molecule, both nitrogens is Sp3 hybridized. bonds around that carbon, zero lone pairs of electrons, what is hybridization of oxygen , is it linear or what? In a thiol, the sulfur atom is bonded to one hydrogen and one carbon and is analogous to an alcohol O-H bond. According to the VSEPR theory (Valence Shell Electron Pair Repulsion Theory), the lone pair on the Nitrogen and the electron regions on the Hydrogen atoms will repel each other resulting in bond angles of 109.5. hybridization state of this nitrogen, I could use steric number. Hence, the molecular shape or geometry for N2H4 is trigonal pyramidal. So that's number of sigma bonds, so here's a single-bond, so that's a sigma bond, and then here's another one; so I have two sigma bonds, so two plus Lewiss structure is all about the octet rule. He holds a degree in B.Tech (Chemical Engineering) and has four years of experience as a chemistry tutor. The electron geometry for N2H4 is tetrahedral. and change colors here, so you get one, two, Therefore, the geometry of a molecule is determined by the number of lone pairs and bonding pairs of electrons as well as the distance and bond angle between these electrons. Masanari Okuno *. The nitrogen is sp3 hybridized which means that it has four sp3 hybrid orbitals. 1. How many of the atoms are sp2 hybridized? Actually, the Nitrogen atom requires three electrons for completing its octet while the hydrogen atom only requires placing nitrogen atoms at the center brings symmetry to the molecule and also makes sharing of electrons amongst different atoms easier. Considering the lone pair of electrons also one bond equivalent and with VS. The electron configuration of nitrogen now has one sp3 hybrid orbital completely filled with two electrons and three sp3 hybrid orbitals with one unpaired electron each. In other compounds, covalent bonds that are formed can be described using hybrid orbitals. Now, calculating the hybridization for N2H4 molecule using this formula: Therefore, the hybridization for the N2H4 molecule is sp3. Explain o2 lewis structure in the . this carbon right here; it's the exact same situation, right, only sigma, or single bonds around it, so this carbon is also Those with 3 bond (one of which is a double bond) will be sp2 hybridized. Due to the sp3 hybridization the nitrogen has a tetrahedral geometry. A here represents the central Nitrogen atom. The important properties for N2H4 molecule are given in the table below: A few of the important uses of hydrazine are given below: It is used in the preparation of polymer foams. B) B is unchanged; N changes from sp2 to sp3. STEP-1: Write the Lewis structure. atom, so here's a lone pair of electrons, and here's The four sp3 hybrid orbitals of nitrogen orientate themselves to form a tetrahedral geometry. Connect outer atoms to central atom with a single bond. Place two valence electrons in between the atoms as shown in the figure below: The red dots represent the valence electrons. Direct link to Agrim Arsh's post What is the name of the m, Posted 2 years ago. As you see in the molecular shape of N2H4, on the left side, nitrogen is attached to the two hydrogen atoms and both are below of plane of rotation and on the right side, one hydrogen is above and one is below in the plane. The oxygen atom in phenol is involved in resonance with the benzene ring. They are made from leftover "p" orbitals. To find the hybridization of an atom, we have to first determine its hybridization number. Nitrogen needs 8 electrons in its outer shell to gain stability, hence achieving octet. Your email address will not be published. Two domains give us an sp hybridization. Concentrate on the electron pairs and other atoms linked directly to the concerned atom. The arrangement is shown below: All the outer shell requirements of the constituent atoms have been fulfilled. Nitrogen gas is shown below. As nitrogen atom will get some formal charge. The molecule is made up of two hydrogen atoms and two nitrogen atoms. match each compound with one of the following bond lengths;110 PM, 122 PM, 145 PM. There is no general connection between the type of bond and the hybridization for. All right, so once again, (iii) Identify the hybridization of the N atoms in N2H4. Nitrogen atoms have six valence electrons each. number of lone pairs of electrons around the Ethene or ethylene, H 2 C=CH 2, is the simplest alkene example.Since a double bond is present and each carbon is attached to 3 atoms (2 H and 1 C), the geometry is trigonal planar.Two overlapping triangles are present since each carbon is the center of a planar triangle. Advertisement. All rights Reserved, Follow some steps for drawing the Lewis dot structure of N2H4, Hydrazine polarity: is N2H4 polar or nonpolar, H2CO lewis structure, molecular geometry, polarity,, CHCl3 lewis structure, molecular geometry, polarity,, ClO2- lewis structure, molecular geometry, polarity,, AX3E Molecular geometry, Hybridization, Bond angle, Polarity, AX2E3 Molecular geometry, Hybridization, Bond angle,, AX4E2 Molecular geometry, Bond angle, Hybridization,, AX2E2 Molecular geometry, Bond angle, Hybridization,, AX2E Molecular geometry, Hybridization, Bond angle, Polarity, AX3E2 Molecular shape, Bond angle, Hybridization, Polarity, AX4 Molecular shape, Bond angle, Hybridization, Polarity. their names indicate the orbitals involved in their formation. 11 Uses of Platinum Laboratory, Commercial, and Miscellaneous, CH3Br Lewis Structure, Geometry, Hybridization, and Polarity. Hydrazine is toxic by inhalation and by skin absorption. This is meant to give us the estimate about the number of electrons that remain unbounded and also the number of electrons further required by any atom to complete their octet. N2H4 has a trigonal pyramidal molecular structure and a tetrahedral electronic shape. As per the VSEPR theory and its chart, if a molecule central atom is attached with three bonded atoms and has one lone pair then the molecular geometry of that molecule is trigonal pyramidal. (You do not need to do the actual calculation.) Direct link to nancy fan's post what is the connection ab, Posted 2 years ago. In this video, we use both of these methods to determine the hybridizations of atoms in various organic molecules. A) 2 B) 4 C) 6 D) 8 E) 10 27. We will use the AXN method to determine the geometry. From the Lewis structure, it can be observed that there are two symmetrical NH2 chains. onto another example; let's do a similar analysis. In the Lewis structure for N 2 H 2 there are a total of 12 valence electrons. do that really quickly. Hybridization number of N2H4= (Number of bonded atoms attached to nitrogen + Lone pair on nitrogen). number is useful here, so let's go ahead and calculate the steric number of this oxygen. So, I see only single-bonds After hybridization these six electrons are placed in the four equivalent sp3 hybrid orbitals. "acceptedAnswer": { But the problem is if a double bond is present in the N2H4 dot structure, then it becomes unstable. so, therefore we know that carbon is SP three hybridized, with tetrahedral geometry, The N - N - H bond angles in hydrazine N2H4 are 112(. Write the formula for sulfur dihydride. Here's another one, sp 3 d hybridization involves the mixing of 1s orbital, 3p orbitals and 1d orbital to form 5 sp 3 d hybridized orbitals of equal energy. These structures are named after American chemist Gilbert Newton Lewis who introduced them in 1916. Direct link to Ernest Zinck's post The oxygen atom in phenol, Posted 8 years ago. { The simplified arrangement uses dots to represent electrons and gives a brief insight into various molecular properties such as chemical polarity, hybridization, and geometry. Direct link to Sravanth's post The s-orbital is the shor, Posted 7 years ago. - In order to get an idea of overlapping present between N-H bonds in ${{N}_{2}}{{H}_{4}}$ molecules, we need to look at the concept of hybridization. A) B changes from sp2 to sp3, N changes from sp2 to sp3. of symmetry, this carbon right here is the same as The Lewis structure that is closest to your structure is determined. When I get to the triple Because sulfur is positioned in the third row of the periodic table it has the ability to form an expanded octet and the ability to form more than the typical number of covalent bonds. (81) 8114 6644 (81) 1077 6855; (81) 8114 6644 (81) 1077 6855 nitrogen, as we discussed in an earlier video, so it has these three sigma bonds like this, and a lone pair of electrons, and that Direct link to Ernest Zinck's post The hybridization of O in. So, the electron groups, also has a double-bond to it, so it's also SP two hybridized, with trigonal planar geometry. Pi bonds are the SECOND and THIRD bonds to be made. Legal. So, each nitrogen already shares 6 valence electrons(3 single bonds). Here, the force of attraction from the nucleus on these electrons is weak. So am I right in thinking a safe rule to follow is. They are made from hybridized orbitals. While the p-orbital is quite long(you may see the diagrams). Required fields are marked *. Find the least electronegative atom and placed it at center. It is the conjugate acid of a diazenide. Count the number of lone pairs + the number of atoms that are directly attached to the central atom. The nitrogen atoms in N 2 participate in multiple bonding, whereas those in hydrazine, N 2 H 4, do not. What is the bond angle of N2O4? There is a triple bond between both nitrogen atoms. Your email address will not be published. As with carbon atoms, nitrogen atoms can be sp 3-, sp 2 - or sphybridized. Normally, atoms that have Sp3 hybridization hold a bond angle of 109.5. However, the H-N-H and H-N-C bonds angles are less than the typical 109.5o due to compression by the lone pair electrons. Hydrogen has an oxidation state of 1+ and there are 4 H atoms, so it gives a total charge of 4+, in order for the compound to be neutral, nitrogen has to give off a charge equal to (and negative) of 4+. It is the process in which the overlap of bonding orbitals takes place and as a result, the formation of stronger bonds occur. (iv) The . Hydrazine is highly toxic composed of two nitrogen and four hydrogens having the chemical formula N2H4. identify the hybridization states, and predict the geometetries for all the atoms in this molecule, except for hydrogen, and so, let's start with this carbon, right here. Some of its properties are given in the table below: Lewis dot structures are schematic representations of valence electrons and bonds in a molecule. oxygen here, so if I wanted to figure out the The postulates described in the Valence Shell Electron Pair Repulsion (VSEPR) Theory are used to derive the molecular geometry for any molecule. This answer is: The three N-H sigma bonds of NH3 are formed by sp3(N)-1s(H) orbital overlap. of non-bonding e 1/2 (Total no. It doesnt matter which atom is more or less electronegative, if hydrogen atoms are there in a molecule then it always goes outside in the lewis diagram. So I know this single-bond for all the atoms, except for hydrogen, and so, once again, let's start with carbon; let's start with this carbon, right here. Three domains give us an sp2 hybridization and so on. the number of sigma bonds, so let's go back over to So let's go back to this The molecular geometry for the N2H4 molecule is trigonal pyramidal and the electron geometry is tetrahedral. All right, let's move over to this carbon, right here, so this Hydrazine forms salts when treated with mineral acids. Three hybrid orbitals lie in the horizontal plane inclined at an angle of 120 . 'cause you always ignore the lone pairs of Hence, for the N2H4 molecule, this notation can be written as AX3N indicating that it has trigonal pyramidal geometry. So the steric number is equal Due to the sp 3 hybridization the nitrogen has a tetrahedral geometry. My aim is to uncover unknown scientific facts and sharing my findings with everyone who has an interest in Science. It has an odor similar to ammonia and appears colorless. Direct link to KS's post What is hybridisation of , Posted 7 years ago. Hydrogen has an electronic configuration of 1s1. An easy way to determine the hybridization of an atom is to calculate the number of electron domains present near it. understand hybridization states, let's do a couple of examples, and so we're going to Re: Hybridization of N2. geometry, and ignore the lone pair of electrons, We have already 4 leftover valence electrons in our account. So, for N2H4, put away hydrogen outside and nitrogen as a central atom in the lewis diagram. Since one lone pair is present on the nitrogen atom in N2H4, lower the bond angle to some extent. b) N: N has 2 electron domains.The corresponding hybridization is sp.. 1 sp orbital form 1 sigma bonds whereas 2 p orbitals from 2 pi bonds. to do for this carbon I would have one, two, three Hybridization of Nitrogen (N2) The electronic configuration of the N2 atom (Z =7) is 1s2 2s2 2px12py12pz1 . All right, let's look at and check out my more interesting posts. With N2F4 the hybridisation is sp3, because N has 4 directions in space: twice N-F; one N-N and one free electron pair. So, the resultant of four N-H bond moments and two lone electron pairs leads to the dipole moment of 1.85 D. hence, N2H4 is a polar molecule. (a) Draw Lewis. This results in bond angles of 109.5. bonds around that carbon. A) It is a gas at room temperature. We can find the hybridization of an atom in a molecule by either looking at the types of bonds surrounding the atom or by calculating its steric number. B) The oxidation state is +3 on one N and -3 on the other. A bond angle is the geometrical angle between two adjacent bonds. It has a boiling point of 114 C and a melting point of 2 C. Now we have to find the molecular geometry of N2H4 by using this method. Direct link to Jessie Harrald's post So am I right in thinking, Posted 7 years ago. and tell what hybridization you expect for each of the indicated atoms. and. 4. But due to presence of nitrogen lone pair, N 2 H 4 faces lone pair-lone pair and lone pair-bond pair . Now, calculating the formal charge for the N2H4 molecule: For the Nitrogen atom, the Total number of valence electrons in free state = 5, Therefore, Formal charge on nitrogen atom = 5 2 (6), For Hydrogen atom, Total number of valence electrons in free state = 1, Total number of non-bonding electrons = 0, Therefore, Formal charge on nitrogen atom = 1 0 (2). Since one lone pair is present on the nitrogen atom in N2H4, lower the bond angle to some extent. Simple, controllable and environmentally friendly synthesis of FeCoNiCuZn-based high-entropy alloy (HEA) catalysts, and their surface dynamics during nitrobenzene hydrogenation. Lone pair electrons are unshared electrons means they dont take part in chemical bonding. All right, and because Lewis structures are simple to draw and can be assembled in a few steps. These are the representation of the electronic structure of the molecule and its atomic bonding where each dot depicts an electron and two dots between the atoms symbolize a bond. Therefore. Each nitrogen(left side or right side) has two hydrogen atoms. Therefore, that would give us an A-X-N notation of AX3N for the Hydrazine molecule[N2H4]. (4) (Total 8 marks) 28. If there are only four bonds and one lone pair of electrons holding the place where a bond would be then the shape becomes see-saw, 3 bonds and 2 lone pairs the shape is T-shaped, any fewer bonds the shape is then linear. An easy way to determine the hybridization of an atom is to calculate the number of electron domains present near it. From the above table, it can be observed that an AX3N arrangement corresponds to a Trigonal Pyramidal geometry. Therefore, the four Hydrogen atoms contribute 1 x 4 = 4 valence electrons.
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