nitrogen vsepr shape

geometry and Lewis structure of NH2- along with its shape, bond angle, polarity, This molecular structure is square pyramidal. There are six electron groups around the central atom, each a bonding pair. Consequently, molecules with these geometries always have a nonzero dipole moment. Six electron groups form an octahedron, a polyhedron made of identical equilateral triangles and six identical vertices (Figure $\PageIndex{2}$. Recognizing similarities to simpler molecules will help you predict the molecular geometries of more complex molecules. There are four electron groups around the central atom. As the arrangement of NH2- is more likely to be H-N-H but step 1), so total electrons pairs are 8/2= 4. 3. Here the amide ion is made up of two different atoms: Nitrogen 1. To minimize repulsions, four electron clouds will always adopt a tetrahedral electron geometry. From this we can describe the molecular geometry. As far as you understand VSEPR theory (which is around a central atom, and actually yes! which strongly repel the bond pairs. Both hydrogen atoms need only two electrons while nitrogen needs 8 electrons to complete duplet and octet respectively. It is clear to understand that the geometrical structure of NH3 will be bent. Put the lone pairs of electrons on atoms. That's all you need to know to answer this) , you know that first of all you have to draw the Lewis structure of the compound, which you can draw like this and now you have got the preliminary linear structure of the molecule $\ce{N2F2}$.. of extra time and energy. The central atom, sulfur, contributes six valence electrons, and each fluorine atom has seven valence electrons, so the Lewis electron structure is. Finally, this bonded atoms. The Lewis electron structure is. If we place it in the equatorial position, we have two 90° LP–BP repulsions at 90°. With its expanded valence, this species is an exception to the octet rule. Compare bond angle predictions from the VSEPR-based model to real molecules. NH2- is an incredibly strong conjugate base of NH3. This approach gives no information about the actual arrangement of atoms in space, however. As we know the total number of valence electrons are equal to As mentioned above, A represents the central atom and X represents an outer atom. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Click here to let us know! The nitrogen atom, on the other hand, has two hydrogen atoms and 1 carbon atom bonded to it. Our first example is a molecule with two bonded atoms and no lone pairs of electrons, $BeH_2$. Because the carbon atom on the left is bonded to four other atoms, we know that it is approximately tetrahedral. ICl4− is designated as AX4E2 and has a total of six electron pairs. If you are are beginner to lewis structure construction, follow these sections slowly and properly to understand it completely. the tetrahedral geometry, where the bond angle lesser than ideal 109.5. Recognize that molecule geometry is due to repulsions between electron groups. 3. is not symmetrical, its resultant of pole charges is also do not cancel by each sp. The angle between electron pairs in a tetrahedral arrangement is 109.5°. draw a simple structure placing a nitrogen atom in the center surrounded by two hydrogens All electron groups are bonding pairs, so the structure is designated as AX4. Solution for The concept of valence-shell electron-pair repulsion (VSEPR) is presented in introductory organic chemistry as a way to predict molecular… 3. For more information contact us at info@libretexts.org or check out our status page at https://status.libretexts.org. For simple cases it performs very well in describing the approximate shape of a molecule. pairs. Hence it has tetrahedral shape with 109 o 28' of bond angles. As there are a total of four Since each atom has steric number 2 by counting … There are five groups around the central atom, three bonding pairs and two lone pairs. be the central atom surrounded by two hydrogen atoms from either side. pairs of electrons overtake the repulsive force of bond pairs. The VSEPR model can predict the structure of nearly any molecule or polyatomic ion in which the central atom is a nonmetal, as well as the structures of many molecules and polyatomic ions with a central metal atom. The E.N difference of N-H is 0.84 which clearly within the range 2. From the BP and LP interactions we can predict both the relative positions of the atoms and the angles between the bonds, called the bond angles. But it can be simply calculated by just dividing the total number of With four nuclei and one lone pair of electrons, the molecular structure is based on a trigonal bipyramid with a missing equatorial vertex; it is described as a seesaw. However, we predict a deviation in bond angles because of the presence of the two lone pairs of electrons. With fewer 90° LP–BP repulsions, we can predict that the structure with the lone pair of electrons in the equatorial position is more stable than the one with the lone pair in the axial position. 1. 4. as NH3 itself also acts as a very weak base and we know that the conjugated bases It is based on the assumption that pairs of electrons occupy space, and the lowest-energy structure is the one that minimizes electron pair–electron pair repulsions. Thus with two nuclei and one lone pair the shape is bent, or V shaped, which can be viewed as a trigonal planar arrangement with a missing vertex (Figures $\PageIndex{2}$ and $\PageIndex{3}$). As we know the polarity is all about It's lewis structure can be drawn by following VSEPR rule. But the repulsive force of lone pair of electrons is higher If both are in the equatorial positions, we have four LP–BP repulsions at 90°. 4. And there are two lone pairs of electrons present on the N atom NO is a oxide of nitrogen. Here we have to place two lone pairs of electrons on D The PF5 molecule has five nuclei and no lone pairs of electrons, so its molecular geometry is trigonal bipyramidal. VSEPR electron pair arrangements and associated molecular shapes. placing two dots for a single bond as shown in the above figure. a) Double Displacement (Metathesis): When ammonia reacts with 10.2: VSEPR Theory - The Five Basic Shapes, [ "article:topic", "showtoc:no", "license:ccbyncsa" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FMap%253A_A_Molecular_Approach_(Tro)%2F10%253A_Chemical_Bonding_II-_Valance_Bond_Theory_and_Molecular_Orbital_Theory%2F10.02%253A_VSEPR_Theory_-_The_Five_Basic_Shapes, 10.3: VSPER Theory- The Effect of Lone Pairs, information contact us at info@libretexts.org, status page at https://status.libretexts.org. This is referred to as an AX4 type of molecule. The shape of a molecule that has two covalent single bonds and no lone pairs on the central atom is _____. Steps to be followed for drawing NH2- Lewis structure. There are six electron groups around the central atom, four bonding pairs and two lone pairs. Start by calculating how many valence electrons you'd get for a molecule of nitrogen gas, "N"_2. There are three nuclei and one lone pair, so the molecular geometry is trigonal pyramidal. Hydrazine (NH2-NH2). Now, on the above hybridization formula, we have to put Groups are positioned around the central atom in a way that produces the molecular structure with the lowest energy, as illustrated in Figures $\PageIndex{1}$ and $\PageIndex{2}$. The calculation is showing below, V.E = Total no. You previously learned how to calculate the dipole moments of simple diatomic molecules. around 107°. We used all 8 valence electrons and all atoms are stable as nitrogen has 8 electrons and each hydrogen atoms have two electrons NH2- is a conjugate base of ammonia. Legal. From the Lewis structure of Nitrogen, we have two-two electrons charge. For some highly symmetrical structures, the individual bond dipole moments cancel one another, giving a dipole moment of zero. However, although H 2 O is indeed angular and NH 3 is trigonal pyramidal, the angles between the bonds are 104° and 107°, respectively. will be polar. electrons in which N contributes 5 electrons, Two H contribute 2 electrons, and two of the four sp3 hybrid orbitals are used to form bonds hydrogen and the remaining two orbitals are used to hold two lone pairs of electrons. Once you have gotten this down, you can refine predictions with other tools. These are arranged in a tetrahedral shape. The nitrogen atom is in the least number so simply it will 1. The carbon atom forms two double bonds. Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of nitrogen trichloride, NC13. In NH2-, there are three 2p orbitals and one 2s orbital. That’s b) Dissociation: When ammonia undergoes dissociation, it This is well illustrated for nitrogen dioxide. Click the structures to load the molecules Nitrogen iodide (NI3)(6CI,7CI,8CI,9CI) NITROGEN IODIDE. NH2- has one negative sign on it. They will draw Lewis structures, use molecular models, and determine the geometry of covalent compounds. We expect the concentration of negative charge to be on the oxygen, the more electronegative atom, and positive charge on the two hydrogens. Its polarity can also be figured out by the Pauli scale which 2. This causes a deviation from ideal geometry (an H–C–H bond angle of 116.5° rather than 120°). by accepting a proton and acting as a base. However, because the axial and equatorial positions are not chemically equivalent, where do we place the lone pair? With three bonding pairs and one lone pair, the structure is designated as AX3E. A combination of VSEPR and a bonding model, such as Lewis electron structures, is necessary to understand the presence of multiple bonds. Name molecule and electron geometries for molecules with up to six electron groups surrounding a central atom. This designation has a total of three electron pairs, two X and one E. Because a lone pair is not shared by two nuclei, it occupies more space near the central atom than a bonding pair (Figure $\PageIndex{4}$). From Figure $\PageIndex{3}$ we see that with three bonding pairs around the central atom, the molecular geometry of BCl3 is trigonal planar, as shown in Figure $\PageIndex{2}$. NH2- has one negative sign on it. dipole moment is simply a product of induced charge and distance between the D There are three nuclei and one lone pair, so the molecular geometry is trigonal pyramidal, in essence a tetrahedron missing a vertex. In ammonia, the central atom, nitrogen, has five valence electrons and each hydrogen donates one valence electron, producing the Lewis electron structure. Each group around the central atom is designated as a bonding pair (BP) or lone (nonbonding) pair (LP). The bromine atom has seven valence electrons, and each fluorine has seven valence electrons, so the Lewis electron structure is. According to VSEPR theory, what molecular shape will it have? 3. The three equatorial positions are separated by 120° from one another, and the two axial positions are at 90° to the equatorial plane. It is tetrahedral because there are four bonded pairs around nitrogen. Six or so steps are required to generate the VSEPR geometry of an atomic centre such as: Carbon in methane, CH 4 Nitrogen in ammonia, NH 3 Xenon in xenon tetrafluoride, XeF4 Recognize that molecule geometry is due to repulsions between electron groups. The central atom, beryllium, contributes two valence electrons, and each hydrogen atom contributes one. Nitrogen is a group 15 element and therefore has 5 electrons in its outmost shell. This is essentially a trigonal bipyramid that is missing two equatorial vertices. I understand that NCl3 is a trigonal planar, but I'm a little unsure how do you go about in defining the number of planes a particular molecule (in this case nitrogen trichloride) has? The Lewis dot structure of ammonia, NH3, reveals that it has one lone pair of electrons and three bonds (each to a hydrogen) around the central nitrogen atom. With no lone pair repulsions, we do not expect any bond angles to deviate from the ideal. NH2- is a strong base because it is unstable with its negative Here in this molecule, we have one nitrogen atom and two In addition, there was significant damage to livestock and crops. Another complication crops up when there are unpaired electrons. Predict the geometry of allene (H2C=C=CH2), a compound with narcotic properties that is used to make more complex organic molecules. nitrogen atom so that they have 8 electrons. However, its shape is pyramidal with a lone pair on nitrogen atom. 4. With two bonding pairs and two lone pairs, the structure is designated as AX2E2 with a total of four electron pairs. As with SO2, this composite model of electron distribution and negative electrostatic potential in ammonia shows that a lone pair of electrons occupies a larger region of space around the nitrogen atom than does a bonding pair of electrons that is shared with a hydrogen atom. 4. This theory is very simplistic and does not account for the subtleties of orbital interactions that influence molecular shapes; however, the simple VSEPR counting procedure accurately predicts the three-dimensional structures of a large number of compounds, which cannot be predicted using the Lewis electron-pair approach. hybridization, and other chemical and molecular properties. Solution for Use VSEPR to predict the geometry (including bond angles) about each interior atom of methyl azide (CH3N3) and draw the molecule. 3. Name molecule and electron geometries for molecules with up to six electron groups surrounding a central atom. Linear. If we place the lone pair in the axial position, we have three LP–BP repulsions at 90°. Due to this difference In the VSEPR model, the molecule or polyatomic ion is given an AXmEn designation, where A is the central atom, X is a bonded atom, E is a nonbonding valence electron group (usually a lone pair of electrons), and m and n are integers. 3. The terminal carbon atoms are trigonal planar, the central carbon is linear, and the C–C–C angle is 180°. Moreover, it mostly exists with organic compounds with Due to the presence of two lone pairs of electrons that repel bond Hence the NH2- ion has a bent V shape, based on the arrangement of the molecule. The VSEPR model is used mainly to ____. the most tricky part but as described in how to draw a Lewis structure guide, For example, carbon atoms with four bonds (such as the carbon on the left in methyl isocyanate) are generally tetrahedral. Count the number of electron groups around each carbon, recognizing that in the VSEPR model, a multiple bond counts as a single group. We designate SF4 as AX4E; it has a total of five electron pairs. 1. has four regions which are responsible for identifying hybridization. Thus bonding pairs and lone pairs repel each other electrostatically in the order BP–BP < LP–BP < LP–LP. It is also B There are five electron groups around the central atom, two bonding pairs and three lone pairs. ), 2. No need to placed a lone pair of The Lewis electron structure is. The valence-shell electron-pair repulsion (VSEPR) model allows us to predict which of the possible structures is actually observed in most cases. With 18 valence electrons, the Lewis electron structure is shown below. There are two bonding pairs and one lone pair, so the structure is designated as AX2E. 3. This can be described as a trigonal bipyramid with three equatorial vertices missing. Molecules with asymmetrical charge distributions have a net dipole moment. In this article, we will discuss NH2- molecular It is based on the assumption that pairs of electrons occupy space, and the lowest-energy structure is the one … 4. Each iodine atom contributes seven electrons and the negative charge one, so the Lewis electron structure is. In molecular geometries that are highly symmetrical (most notably tetrahedral and square planar, trigonal bipyramidal, and octahedral), individual bond dipole moments completely cancel, and there is no net dipole moment. the bonds closer to each other. We see from Figure $\PageIndex{2}$ that the geometry that minimizes repulsions is octahedral. structure whereas there are 2 bonding pairs and 2 lone pairs of electrons within Here N (N) and Hydrogen (H) so first, we have to figure out the valence electrons of To determine whether equivalent Lewis structures, called resonance structures, are present in molecules. Use the VSEPR model to predict the molecular geometry of propyne (H3C–C≡CH), a gas with some anesthetic properties. 4. If we focus on the positions of the nuclei in ammonia, we predict that the NH 3 molecule should have a shape best described as trigonal pyramidal, with the nitrogen at the top of the pyramid. 2. structure is surrounded by a negative sign because NH2- is an ion with negative Compare bond angle predictions from the VSEPR-based model to real molecules. 3. The relationship between the number of electron groups around a central atom, the number of lone pairs of electrons, and the molecular geometry is summarized in Figure $\PageIndex{6}$. Now it’s time to know polarity, it means to figure out whether With four bonding pairs, the molecular geometry of methane is tetrahedral (Figure $\PageIndex{3}$). These electrons are arranged in a tetrahedral shape with a structure like H-N-H. As we already familiar with electron-electron repulsion, both We will demonstrate with methyl isocyanate (CH3–N=C=O), a volatile and highly toxic molecule that is used to produce the pesticide Sevin. Three electrons of N are bonded with hydrogen and the rest two which do … There is a sharp distinction between ionic and covalent bonds when the geometric arrangements of atoms in compounds are considered. And due to these four regions Predicting the Shapes of Molecules . If the individual bond dipole moments cancel one another, there is no net dipole moment. Similarly, the carbon atom on the right has two double bonds that are similar to those in CO2, so its geometry, like that of CO2, is linear. The central atom, carbon, contributes four valence electrons, and each hydrogen atom has one valence electron, so the full Lewis electron structure is. The VSEPR model can be used to predict the shapes of many molecules and polyatomic ions, but it gives no information about bond lengths and the presence of multiple bonds. The BrF5 structure has four fluorine atoms in a plane in an equatorial position and one fluorine atom and the lone pair of electrons in the axial positions. The bond dipoles cannot cancel one another, so the molecule has a net dipole moment. What is the molecular formula of the compound? 3. This molecular shape is essentially a tetrahedron with two missing vertices. VSEPR theory - Steps of drawing lewis structure of H 3 PO 3. Once again, both groups around the central atom are bonding pairs (BP), so CO2 is designated as AX2. These pairs electrons which have comparatively lower repulsive force and bond angle is Mathematically, dipole moments are vectors; they possess both a magnitude and a direction. Use the strategy given in Example$\PageIndex{1}$. trigonal pyramid Use VSEPR theory to predict the molecular geometry of ClO3−. due to the lone pairs and bond pairs repulsion, it acquires bent V-shape 1. This designation has a total of four electron pairs, three X and one E. We expect the LP–BP interactions to cause the bonding pair angles to deviate significantly from the angles of a perfect tetrahedron. Chem. It is explained with the help of the Valence Shell Electron Pair Repulsion (VSEPR) theory, which says the presence of a lone pair on the nitrogen atom makes the complete structure of NH3 bent giving a bond angle of 107°. The carbon in the –N=C=O fragment is doubly bonded to both nitrogen and oxygen, which in the VSEPR model gives carbon a total of two electron pairs. VSEPR geometry of NCl3? electron density around the central nitrogen atom i.e. The methane molecule (CH4) is tetrahedral because there are four pairs of electrons. 4. Figure $\PageIndex{9}$: (a) H2O has four regions of electron density around the central atom, so it … The resulting molecular shape is trigonal pyramidal with H-N-H angles of 106.7°. In SO2, we have one BP–BP interaction and two LP–BP interactions. difference between nitrogen and hydrogen atoms. 2. NH2- has a total of 8 valence electrons which are surrounded on the H-N-H structure. Depending on how many of the clouds are lone pairs, the molecular geometry will be tetrahedral (no lone pairs), trigonal pyramidal (one lone pair), or bent (two lone pairs). 3. Formal charge (F.C) = Valence electrons (V) – Lone pair of Which of the following is required for determination of the VSEPR model and the molecular shape? It is explained with the help of the Valence Shell Electron Pair Repulsion (VSEPR) theory, which says the presence of a lone pair on the nitrogen atom makes the complete structure of NH3 bent giving a bond angle of 107°. electrons presence on the nitrogen atom which exerted higher repulsion, as a Lewis structure. electrons participated in the formation of a molecule. We must now decide how to arrange the lone pairs of electrons in a trigonal bipyramid in a way that minimizes repulsions. Here are some of the example reactions which show NH2- is a All electron groups are bonding pairs, so the structure is designated as AX5. we have to add +1 electrons in total valence electrons because one negative charge contributes 1 electron. pairs N-H, it acquires a bent V-shape molecular shape with a bond angle of 104.5°. Six or so steps are required to generate the VSEPR geometry of an atomic centre such as: Carbon in methane, CH 4 Nitrogen in ammonia, NH 3 Xenon in xenon tetrafluoride, XeF4 valence electrons: 5 + 1*2 + 1 = 8. of Pauli polar molecules range. Like NH3, repulsions are minimized by directing each hydrogen atom and the lone pair to the corners of a tetrahedron. atom. atoms. D With two nuclei about the central atom, the molecular geometry of XeF2 is linear. Ans: In ammonia, N is the central atom. If one lone pair is axial and the other equatorial, we have one LP–LP repulsion at 90° and three LP–BP repulsions at 90°: Structure (c) can be eliminated because it has a LP–LP interaction at 90°. structure whereas there are 2 bonding pairs and 2 lone pairs of electrons within NH2- is a polar molecule due to the higher electronegativity 3. Each chlorine contributes seven, and there is a single negative charge. Mainly, the VSEPR model focuses on the electron pairs around the central atoms. of valence electrons presence on the Ammonia (NH3) which has only 1 pair of non-bonding lone 1. However, the H–N–H bond angles are less than the ideal angle of 109.5° because of LP–BP repulsions (Figure $\PageIndex{3}$ and Figure $\PageIndex{4}$). The three nuclei in BrF3 determine its molecular structure, which is described as T shaped. NH2- has an sp3 hybridization type. We expect all Faxial–Br–Fequatorial angles to be less than 90° because of the lone pair of electrons, which occupies more space than the bonding electron pairs. So, if you want to The structure of $\ce{CO2}$ is shown in Figure $\PageIndex{1}$. Thus, both N-H bond pairs come closer to The dipole moment of a molecule is therefore the vector sum of the dipole moments of the individual bonds in the molecule. It also takes care of the steric number that is the number of regions of electron density surrounding the atom. Determine the total number of valence electrons pairs. At 90°, the two electron pairs share a relatively large region of space, which leads to strong repulsive electron–electron interactions. 109: VSEPR Theory Objectives To learn how to draw Lewis structures of molecules and ions. 4. It has a bent molecular shape: this can be rationalized in the VSEPR model in terms of the lone-pair of electrons located on the N atom. 3. 1. Using an active learning approacah, given a molecular formula, students draw the Lewis Structure, Identify the total regions of electron domains around the central atom, build the model of the molecule, draw a 3D representation of the molecule, identify the molecular shape, identify the bond angles, and classify the molecule as polar or non-polar. The (pure) VSEPR model must fail for this molecule, as it is only really working for central atoms with distinct and non-delocalised ligands. The central atom, carbon, has four valence electrons, and each oxygen atom has six valence electrons. There are two nuclei about the central atom, so the molecular shape is bent, or V shaped, with an H–O–H angle that is even less than the H–N–H angles in NH3, as we would expect because of the presence of two lone pairs of electrons on the central atom rather than one. each other and occupy less space than two non-bonding lone pairs of electrons. The shapes of these molecules can be predicted from their Lewis structures, however, with a model developed about 30 years ago, known as the valence-shell electron-pair repulsion (VSEPR) theory.. Thus according to the VSEPR model, the C–N=C fragment should be bent with an angle less than 120°. 1. Unless otherwise noted, LibreTexts content is licensed by CC BY-NC-SA 3.0. There are six nuclei, so the molecular geometry of SF6 is octahedral. forms NH2- as the conjugated base and H+ as conjugated acid. pairs of regions (two bond pairs and two lone pairs) for the electrons are attached This VESPR procedure is summarized as follows: We will illustrate the use of this procedure with several examples, beginning with atoms with two electron groups. Difluoroamine has a trigonal pyramidal molecular geometry. Now. Oxygen has six valence electrons and each hydrogen has one valence electron, producing the Lewis electron structure. Radicals and VSEPR calculation for nitrogen dioxide, N O 2. The hybridization of the central nitrogen atom in the molecule N2O is. Any diatomic molecule with a polar covalent bond has a dipole moment, but in polyatomic molecules, the presence or absence of a net dipole moment depends on the structure. And if the geometry of a molecule 1. The Lewis electron structure is. From this, we get one negative charge on the ions. The whole According to the VSEPR theory, the shape of this carbon would be tetrahedral. Using the VSEPR model, identify the molecular geometry of nitrogen triiodide, NI3, based on the number of electron domains. These electrons are arranged in a tetrahedral shape with a structure like H-N-H. As we already familiar with electron-electron repulsion, both lone pairs and bond pairs of electrons repel each other. In which 3. Valence Shell Electron-Pair Repulsion. Recognize the difference between electron and molecular geometry. bonding regions which show it has 2 lone pairs of electrons. USE: Nitrogen trifluoride is a component of high-energy fuels and is also used to make other chemicals. shells. So, NH2- has a bent (angular) molecular It is time to put lone pairs of electrons on atoms. * Since the steric number is 4, its structure is based on tetrahedral geometry. The molecule has three atoms in a plane in equatorial positions and two atoms above and below the plane in axial positions. In order to be able to determine the molecular geometry of a given compound, you need to first draw its Lewis structure. Molecules with polar covalent bonds can have a dipole moment, an asymmetrical distribution of charge that results in a tendency for molecules to align themselves in an applied electric field. hydrogen atom and one negative charge ion. 4. 2 bond pairs and 2 lone pairs. says if the E.N difference between two atoms is between 0.4 to 2.0, the formed bond We see from Figure $\PageIndex{3}$ that the molecular geometry of CO32− is trigonal planar with bond angles of 120°. The four bonds around carbon mean that it must be surrounded by four bonding electron pairs in a configuration similar to AX4. It is clear to understand that the geometrical structure of NH3 will be bent. The skeleton looks like this. The N=C=O angle should therefore be 180°, or linear. That’s result, NH2- has a bond angle 104.5, NH2- (conjugated base) + H+ (conjugated acid), NH2- is an incredibly strong conjugate base of NH3. VSEPR Theory. If they do not, then the molecule has a net dipole moment. So, for NO 2 there is an integral number of electrons but a non-integral number of electron pairs. The resulting highly exothermic reaction caused a rapid increase in pressure that ruptured the tanks, releasing large amounts of methyl isocyanate that killed approximately 3800 people and wholly or partially disabled about 50,000 others.

How To Screw Into Porcelain Tile, Medicine Mcqs With Answers, Working At Walmart Reddit 2020, Three Movie Imdb, Ac Valhalla Raids Respawn, The Odin Project Javascript Reddit, Milwaukee Circular Saw M18 Fuel, Kenwood Excelon Kfc-xw1200f Box,