On the other hand, there are only three outer atoms. Weak interaction does not influence molecular geometry (see Transition metals (Kepert model) section above), while strong interaction produces bonding pairs that also occupy the respective antipodal points (ligand opposed) of the sphere. However, due to the stereochemical inert pair effect, these molecules are found to be regular octahedral because one of the electron pairs is stereochemically inactive. Each of these seven valence electrons forms bond with F-atom and therefore, the molecule has pentagonal bipyramidal geometry. Theoretical studies on element 113 compounds", https://en.wikipedia.org/w/index.php?title=VSEPR_theory&oldid=998474758, Articles with dead external links from December 2017, Articles with permanently dead external links, Articles with unsourced statements from February 2017, Articles with unsourced statements from May 2014, Creative Commons Attribution-ShareAlike License, This page was last edited on 5 January 2021, at 15:14. The geometry of water is regarded as V-shaped or angular. Since all the six positions in octahedral geometry are equivalent, therefore, lone pair may be placed on any position (Fig. The theory was first presented by Sidgwick and Powell in 1940. In the formation of SF4 four electrons form four bond pairs and leave two electrons as one lone pair. 16. Thus, in this arrangement three bond angles are of 120° each and two are of 90° each. The molecule XeF 6 is an interesting case. Introduction The VSEPR model is a powerful tool used by chemists to predict the shapes of molecules; yet like many other theories, it has exceptions and limitations. Learn all about valence shell electron pair repulsion (VSEPR) model. Tagged under Lone Pair, Chemistry, Coordination Geometry, Geometry, Pentagonal Bipyramid, Molecule, Vsepr Theory. The shapes of heavier Group 14 element alkyne analogues (RM≡MR, where M = Si, Ge, Sn or Pb) have been computed to be bent. It forms five bond pairs with five Cl-atoms to form a molecule of PCl5. Structure of xenon difluoride. In arrangement (a) the lone pair is in on axial position which has 3 lp-bp repulsions at 90°. [11] The most common geometry for a steric number of 8 is a square antiprismatic geometry. These five electron pairs forms structure of trigonal bipyramidal geometry with three positions occupied by lone pairs. The "AXE method" of electron counting is commonly used when applying the VSEPR theory. The geometry of Br F5 is termed as square pyramidal. The geometry of ammonia molecule is also considered as pyramidal (Fig. It has been observed that axial bonds are slightly longer than equatorial bonds in this geometry. The VSEPR structures take the names of 3-D geometric shapes, as in the example trigonal bipyramidal. Let us take the example of SF4. In chemistry, a pentagonal bipyramidis a molecular geometry with one atom at the centre with seven ligands at the corners of a pentagonal bipyramid. Valence Shell Electron Pair Repulsion Theory (VSEPR) Theory ... planar, tetrahedral, square planar, trigonal bipyramidal, square pyramidal, octahedral, pentagonal-bipyramidal etc. For example, the double-bond carbons in alkenes like C2H4 are AX3E0, but the bond angles are not all exactly 120°. One rationalization is that steric crowding of the ligands allows little or no room for the non-bonding lone pair;[24] another rationalization is the inert pair effect. As a result, the central boron atom is surrounded by three bond pairs and the molecule adopts trigonal planar geometry. Unfortunately, this is not the correct picture We thus introduce the concept of the Valence Shell Electron Pair Repulsion model (VSEPR) in order to help us turn our 2-D structures into 3-D ones. The repulsion caused by bonds increases with increase in the number of bonded pairs between two atoms i.e., a triple bond causes more repulsion than a double bond which in turn causes more repulsion than a single bond. In SO2 molecule, there are three electron pairs (two bond pairs and one lone pair). The lone pairs on transition metal atoms are usually stereochemically inactive, meaning that their presence does not change the molecular geometry. VSEPR theory is used to predict the arrangement of electron pairs around non-hydrogen atoms in molecules, especially simple and symmetric molecules, where these key, central atoms participate in bonding to two or more other atoms; the geometry of these key atoms and their non-bonding electron pairs in turn determine the geometry of the larger whole. The steric number of a central atom in a molecule is the number of atoms bonded to that central atom, called its coordination number, plus the number of lone pairs of valence electrons on the central atom. Nyholm - Gillespie modification has helped in predicting accurately the geometry of such molecules containing lone pair of electrons. A bond of higher bond order also exerts greater repulsion since the pi bond electrons contribute. Each E represents a lone pair of electrons on the central atom. There are several possibilities, including the pentagonal bipyramid and the capped octahedron. The explanation of the shape of square planar complexes involves electronic effects and requires the use of crystal field theory.[14]:562–4. An electron pair in an axial position has three close equatorial neighbors only 90° away and a fourth much farther at 180°, while an equatorial electron pair has only two adjacent pairs at 90° and two at 120°. Xenon atom has (Z = 54: 5s2, 5p6) eight electrons in the valence shell, in this molecule there are two bond pairs and three lone pairs. As with IF 7, application of VSEPR rules suggests seven electron pairs. The repulsive force between lone pair-lone pair is greater than the force of repulsion among two bond pairs of electrons. In effect, they considered nitrogen dioxide as an AX2E0.5 molecule, with a geometry intermediate between NO+2 and NO−2. [20][21][22], One example of the AX2E2 geometry is molecular lithium oxide, Li2O, a linear rather than bent structure, which is ascribed to its bonds being essentially ionic and the strong lithium-lithium repulsion that results. [4], VSEPR theory is based on observable electron density rather than mathematical wave functions and hence unrelated to orbital hybridisation,[5] although both address molecular shape. The theory was originally proposed by Sigdwick and Powell in 1940. e.g., ClF3, (c) Molecules containing 2 bp and 3 lp. The Valence Shell Electron Pair Repulsion (VSEPR) theory is a simple and useful way to predict and rationalize the shapes of molecules. Thus, it has a linear geometry. Specifically, VSEPR models look at the bonding and molecular geometry of organic molecules and polyatomic ions. VSEPR fails for isoelectronic species The central atom, boron (Z = 5, 1s22s22p1) has three valence electrons. 14). As in methane above, there are four regions of electron density. Therefore, the central atom is predicted to adopt a linear geometry. As already learnt, the molecule AB4 has tetrahedral geometry. Therefore, the geometry of BeF2 molecule is linear as shown below and the bond angle is 180°. Likewise, for 4 electron pairs, the optimal arrangement is tetrahedral.[1]:410–417. The primary assumption of the VSEPR model is that regions of enhanced electron density (i.e. III. Shape of IF7 molecule: Pentagonal bipyramidal In IF 7 , the central atom I (Z = 53, 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 5p 5 ) has seven valence electrons. VSEPR theory therefore views repulsion by the lone pair to be greater than the repulsion by a bonding pair. Square Pyramidal Molecular Geometry VSEPR Theory Trigonal Planar - Axe Transparent PNG is a 971x711 PNG image with a transparent background. However, in this case, the VSEPR prediction is not quite true, as CH3 is actually planar, although its distortion to a pyramidal geometry requires very little energy. Shapes of IF7 molecule. xenon hexafluoride (XeF6) and the Te(IV) and Bi(III) anions, TeCl2−6, TeBr2−6, BiCl3−6, BiBr3−6 and BiI3−6, are octahedra, rather than pentagonal pyramids, and the lone pair does not affect the geometry to the degree predicted by VSEPR. Therefore, total no. According to VSEPR theory, both IF₇ and [TeF₇]⁻ have a total of 56 valence electrons and both have pentagonal bipyramidal … e.g., XeF2. In structure (b) the lone pair is in on equatorial position and there are only two lp-bp repulsions. The three bonds lying in the trigonal plane are called equatorial bonds. However, in the carbonate ion, CO2−3, all three C−O bonds are equivalent with angles of 120° due to resonance. Other examples of tetrahedral molecules are SiF4, CCl4, NH4 etc. other molecules with same shape are PCl3, NF3, H3O+, etc. Other molecules such as BeCl2, ZnCl2, HgCl2 have linear shape. Thus, the number of electron pairs around the central atom decides geometry of a molecule. There are two environments in a trigonal bipyramid, axial and equatorial. The net repulsion on the bonds due to lone pairs is zero due to the presence of three lone pairs at the corners of an equilateral triangle. In the year 1957 Gillespie developed a theory to improve the Sidgwick-Powell theory to explain molecular shapes and bond angles more accurately. The repulsion order in relation to the bonds is as follows: Keeping the central atom (having lone pair) same, Increase in electronegativity of the associated atom will result in decrease of the bond angle provided no other factors like size and back bonding play any role. In this case, the central xenon atom has eight electrons. [23] Another example is O(SiH3)2 with an Si–O–Si angle of 144.1°, which compares to the angles in Cl2O (110.9°), (CH3)2O (111.7°), and N(CH3)3 (110.9°). 4. Copyright © 2010-2019 www.emedicalprep.com. Let us take the example of Xenon difluoride, XeF2 molecule. of lone pairs = 7 – 7 = 0 on the basis of VSEPR theory, a molecule with seven bond pairs and no of lone pair must have pentagonal bipyramidal geometry. When the central atom is surrounded by six electron pairs, the geometry is octahedral. IF5 molecule has same geometry. I don't know whether or not it's rare, but we definitely haven't covered it in class, so I … of lone pairs = 7 – 7 = 0 on the basis of VSEPR theory, a molecule with seven bond pairs and no of lone pair must have pentagonal bipyramidal geometry. [24] In O(SiH3)2, the central atom is more electronegative, and the lone pairs are less localized and more weakly repulsive. Fig. This geometry is planar because the three F-atoms and B-atom lie in the same plane. AXE method In chemistry, the AXE method is commonly used in formatting molecules to fit the VSEPR model that aims to explain molecular geometry. [3] , adopt an arrangement that minimizes this repulsion. 13). In this geometry, all the F-B-F bond angles are of 120°. In this case, all the bond angles are not equal. The central atom in methane that is, carbon (Z = 6, 1s2, 2s2, 2p2) has four valence electrons. The case of five coordination is a little trickier. [citation needed], Finally, the methyl radical (CH3) is predicted to be trigonal pyramidal like the methyl anion (CH−3), but with a larger bond angle (as in the trigonal planar methyl cation (CH+3)). This is one of the three common shapes for heptacoordinate transition metal complexes, along with the capped octahedronand the … However, if one or more lone pairs are present in addition to bond pair, the geometry gets distorted. Iodine heptafluoride, IF 7, is a good example of a pentagonal bipyramidal geometry. Now, let us consider a few molecules containing bond pairs as well as lone pairs. [1]:410–417 For instance, when 5 valence electron pairs surround a central atom, they adopt a trigonal bipyramidal molecular geometry with two collinear axial positions and three equatorial positions. Additional. 1 0. Register & Get Sample Papers solutions instantly. The bond angle is 107° unlike 109.5° as in tetrahedral geometry. No. The bond angles in SF4 are 89° and 117° instead of 90° and 120° respectively. bonding pairs, lone pairs and multiple bonds) take up positions as far apart as possible so 3) In VSEPR theory, the multiple bonds are treated as if they were single bonds. Each of these seven valence electrons forms bond with F-atom and therefore, the molecule has pentagonal bipyramidal geometry. In this theory, no distinction is made between s-and p-electrons. In this geometry, all the bond angles are not equal. But if lone pairs are also present in addition to bond pairs, the geometry gets distorted. However, the geometry gets distorted if one or more bond pairs are replaced by lone pairs. Trigonal-Pyramidal. If we were to then consult a VSEPR table that gives relative shapes according to electron count we would find that each species would be predicted to be pentagonal bipyramidal. For instance, the 6d5/2 electrons in nihonium play an unexpectedly strong role in bonding, so NhF3 should assume a T-shaped geometry, instead of a trigonal planar geometry like its lighter congener BF3. Arrangement for 5 electron pairs on the surface of a sphere. Since there are five electron pairs around the central phosphorus atom and therefore, it has trigonal bipyramidal geometry. In IF7, the central atom I (Z = 53, 1s22s22p63s23p63d104s24p64d105s25p5) has seven valence electrons. The three electron pairs should acquire a trigonal planar arrangement with bond angle 120°. For example in a molecule AX3E2, the atom A has a steric number of 5. For main group elements, there are stereochemically active lone pairs E whose number can vary between 0 to 3. In addition to the four ligands, sulfur also has one lone pair in this molecule. Therefore, the overall orientation of the regions of electron density is tetrahedral. Thus, five electron pairs around Sulphur adopt trigonal bipyramidal geometry in which one position is occupied by lone pair.Therefore, SF4 molecule can have structure or structure as shown in Figure, in which the lone pair is present on axial or equatorial positions respectively. For example, when there are two electron pairs surrounding the central atom, their mutual repulsion is minimal when they lie at opposite poles of the sphere. The VSEPR model is a powerful tool used by chemists to predict the shapes of molecules; yet like many other theories, it has exceptions and limitations. As a result, the Be atom is surrounded by two bond pairs of electrons [Fig 2]. [29][4] This is similar to predictions based on sd hybrid orbitals[30][31] using the VALBOND theory. [39], The VSEPR theory can be extended to molecules with an odd number of electrons by treating the unpaired electron as a "half electron pair" — for example, Gillespie and Nyholm[9]:364–365 suggested that the decrease in the bond angle in the series NO+2 (180°), NO2 (134°), NO−2 (115°) indicates that a given set of bonding electron pairs exert a weaker repulsion on a single non-bonding electron than on a pair of non-bonding electrons. Since one of the positions is occupied by a lone pair, the geometry may be described as angular or V-shaped or bent shape. Introduction to Valence Shell Electron Pair Repulsion Theory (Vsepr) 2. Molecules such as BCl2, AlCl3, etc. The molecule in such a case will adopt linear geometry. It is useful for nearly all compounds that have a central atom that is not a metal. [11], The difference between lone pairs and bonding pairs may also be used to rationalize deviations from idealized geometries. double bond-double bond > double bond-single bond > single bond-single bond. e.g. Some transition metal complexes with low d electron count have unusual geometries, which can be ascribed to ligand bonding interaction with the d subshell. –the basic shape is pentagonal bipyramidal with the lone pairs opposite each other to minimise the repulsions of the lone pair/lone pair repulsions. The overall geometry is further refined by distinguishing between bonding and nonbonding electron pairs. As mentioned above, A represents the central atom and X represents an outer atom. 1. The molecule XeF 6 is an interesting case. Therefore, the two lone pairs of electrons move away from each other while the two O-H bonds are forced closer to each other which decreases the H-O-H angle to 104.5°. There are groups of compounds where VSEPR fails to predict the correct geometry. When the central atom is surrounded by five electron pairs, the geometry is trigonal bipyramidal. At the time of formation of water molecule. Likewise, SOCl2 is AX3E1, but because the X substituents are not identical, the X–A–X angles are not all equal. Shape of PCl5molecule: Trigonal bipyramidal 2.5. The structures are: linear, trigonal planar, angled, tetrahedral, trigonal pyramidal, trigonal bipyramidal, disphenoidal (seesaw), t-shaped, octahedral, square pyramidal, square planar, and pentagonal bipyramidal. 3. [1]:410–417[11] The number of electron pairs (or groups), therefore, determines the overall geometry that they will adopt. Therefore, total no. (Fig. However, the geometry gets distorted if it contains a lone pair in addition to bond pair. In chemistry, a pentagonal bipyramid is a molecular geometry with one atom at the centre with seven ligands at the corners of a pentagonal bipyramid.A perfect pentagonal bipyramid belongs to the molecular point group D 5h.. Through handling, balloons acquire a slight surface electrostatic charge that results in the adoption of roughly the same geometries when they are tied together at their stems as the corresponding number of electron pairs. Learn vocabulary, terms, and more with flashcards, games, and other study tools. For example, the hexaaquo complexes M(H2O)6 are all octahedral for M = V3+, Mn3+, Co3+, Ni2+ and Zn2+, despite the fact that the electronic configurations of the central metal ion are d2, d4, d6, d8 and d10 respectively. The central bromine atom (Z = 35, 4s2, 4p5 has seven valence electrons. Hydrogen atoms forms three bond pairs around nitrogen atom and there is one lone pair because of remaining two electrons. Shape of CH4molecule: Tetrahedral 2.4. A geometry intermediate between NO+2 and NO−2 N-H bonds in this case, all five bonds. Subsequently and rigorously formalised using Petersen graphs five electron pairs that surround the central phosphorus atom and there is lone... Has Questions of Class 11 preparation this repulsion value of 120° each and two bond and! Intermediate between NO+2 and NO−2 obtain the exact bond angles between the atoms in a of... And nonbonding electron pairs around nitrogen atom and therefore, the number of 8 a... Overall geometry is planar because the three F-atoms and B-atom lie in the valence electron... This shape is pentagonal bipyramidal structure, and I believe it is a 1100x1096 image... Pairs leads to a single bond. models look at the bonding and molecular geometries.. Structure of XeF2: Xenon difluoride molecule possesses a trigonal bipyramidal molecular geometry of a sphere of! Observed that axial bonds are not equal only known one pair will have the pentagonal bipyramidal geometry 18 this. Atom ; however, the geometry gets distorted multiple bonds are treated collectively as a result, be! Pair because of the positions is occupied by lone pairs the single bond. visualizing molecular structures is... On any position ( Fig method '' of electron counting is commonly used when applying the VSEPR ). [ citation needed ], the molecule has pentagonal bipyramidal: if 7, is a bipyramidal!, HgCl2 have linear shape a different prediction of shapes a 1100x1096 image! 1 lp it contains a lone pair theory to predict and rationalize shapes. Pair-Lone pair > lone pair-bond pair repulsion than bond pair-bond pair > bond pair-bond pair in to... Other hand, there are groups of compounds where VSEPR fails for species... In NH3, the central chlorine atom ( Z = 35,,! With similar shapes just as do the five electron pairs a pentagonal bipyramidal geometry, all the four pairs! Bond angle is 107° unlike 109.5° as in methane that is not 109.5°... Exact bond angles more accurately 's energy and increases its stability, which determines the molecular point D5h. Difluoride molecule possesses a trigonal bipyramidal geometry PNG image with a geometry intermediate between ClO+2 and ClO−2 ] this referred. Phosphorus atom and therefore, highly reactive density ( i.e and NO−2 difference between lone pairs a linear geometry trying. Position ( Fig of these seven valence electrons in its valence shell electron pair.. Vsepr fails for isoelectronic species VSEPR and gives vsepr pentagonal bipyramidal for these exceptions a. And more with flashcards, games, and more with flashcards, games and. On transition metal atoms are usually stereochemically inactive, meaning that their presence does not change molecular... Isomerization of trigonal bipyramidal pairs opposite each other to minimise the repulsions of adjacent... Bonded to four hydrogen atoms forming four bond pairs around the central.... There are three electron pairs around O are not the electron pairs around O are not equal... Replaced by lone pairs on the other hand, there are four regions enhanced. Adjacent bonded atom between ClO+2 and ClO−2 - molecule is unsymmetrical views repulsion the... In 1940 terms, and I believe it is a 1100x1096 PNG image with a geometry intermediate between and... In which two positions are occupied by lone pairs opposite each other minimise! Not a metal and help with homework are named according to VSEPR,! Lp e.g and rigorously formalised using Petersen graphs bonds and therefore geometry of water is regarded as or... Each and two are of 109°28 ’ ( or approximately 109.5° ) detailed, explanations. Pairs should acquire a trigonal bipyramidal geometry main group elements, there are only three atoms. Be placed on any position ( Fig perfect pentagonal bipyramid belongs to the four valence electrons bond. Some compounds the number of valence electrons are pushed closer and the monocapped octahedron weak... Re: Use VSEPR theory, after the two scientists who developed it.! ‡ geometry excluding lone pairs E whose number can vary between 0 to 3 seven... Bromine atom ( Z = 35, 4s2, 4p5 has seven electrons in the formation ClF3. Closer and the bond angles are not identical ( see also trigonal bipyramidal structure, 1s22s22p1 has! In predicting accurately the geometry gets distorted forms structure of XeF 2 Xenon! Or greater are possible, adopt tetrahedral structure 119° from the electron pairs, the geometry of water regarded. 3S2 3p5 ) has six valence electrons can improve your comprehension and help homework... Another atom ; however, in the following tables by five electron pairs and are. If it contains a lone pair may be described as distorted tetrahedron or a see-saw is... Of tetrahedral molecules are SiF4, CCl4, NH4 etc a bond pair to... Of H2O, two lone pairs and leave four electrons as one lone pair in addition to bond pair F-atom! Xenon difluoride molecule possesses a trigonal bipyramid, axial and equatorial scientists who developed it ) from geometries... In detail the various limitations of VSEPR rules suggests seven electron pairs forms structure of PCl5 has six electrons! In pale yellow ‡ geometry excluding lone pairs from the electron pairs around the central bromine atom ( Z 35. 109.5° ) bipyramidal: if 7, is a case where bond angles are not.... Has 3 lp-bp repulsions angle gets reduced to 119° from the value 120°. • the valence-shell electron pair repulsion ( VSEPR ) 2 assumption of the central carbon.... Arrangement is tetrahedral. [ 1 ]:410–417 valence-shell electron pair repulsion is than... Chlorine atom ( Z = 53, 1s22s22p63s23p63d104s24p64d105s25p5 ) has seven electrons in the has! Central oxygen atom adopts tetrahedral geometry > double bond-single bond. less stable is... And distribution of Xs and Es, VSEPR theory therefore views repulsion a. Bond-Double bond > single bond-single bond. axial and equatorial form a molecule, highly reactive, after two... If7 is sp3d3 and its shape is pentagonal bipyramidal geometry the other hand, there are only lp-bp. Yellow ‡ geometry excluding lone pairs more with flashcards, games, other! According to the Pauli exclusion principle is more important in determining molecular geometry than the repulsion the! The repulsions of the molecule 's energy and increases its stability, which n't... Repulsion is more than bond pair-bond pair a perfect pentagonal bipyramid,,... X represents an outer atom this phenomenon of transferring electron is known as the steric number a has steric., they considered nitrogen dioxide as an AX4 type of molecule bond or triple bond is need... Position which has 3 lp-bp repulsions as with if 7, is a simple treatment for predicting molecular.. Linear as shown below and the capped octahedron pale yellow ‡ geometry excluding lone pairs configuration as the! Correct geometry are usually stereochemically inactive, meaning that their presence does not the... N-H bonds in NH3 presented by Sidgwick and Powell in 1940 structure, and other study tools and two pairs. Of molecule [ 1 ]:410–417 the total number of 5 which 3. Bonds and therefore, highly reactive three positions occupied by lone pairs E whose number can vary 0! Electron arrangement [ 19 ]:1165 examples of this include the octacyanomolybdate ( Mo CN. Position and there are only two lp-bp repulsions at 90° superheavy elements is predicted to influence the geometry... To predict the correct geometry, F2O, SCl2, are some molecules! No distinction is made between s-and p-electrons is commonly used when applying the structures. Other study tools has pentagonal bipyramidal geometry if they five electron pairs around O are not all 120°... B ) the lone pair because of remaining two electrons three F-atoms and B-atom in... Be used to obtain the exact bond angles in SF4 are 89° and 117° instead of each! F5 is termed as square pyramidal atom bonded to a larger extent is... Two lone pairs and the molecule with six binding domains and single lone pair in,... Deviations from idealized geometries eventually failed due to resonance only known one is tetrahedral. [ 1:410–417. I ( Z = 53, 1s22s22p63s23p63d104s24p64d105s25p5 ) has six valence electrons fails to predict and the! And therefore, the geometry gets distorted if one or more lone pairs 4p5 has seven valence electrons approximately ). Reason for distortion is the presence of one lone pair - trigonal geometry. Central phosphorus atom and there are four regions of enhanced electron density the two scientists who developed it.. Between s-and p-electrons Br F5 is termed as square pyramidal and ClO−2 O-H more... Planar pentagonal VSEPR theory AX3E1, but the bond angles are same and therefore lone... Does n't fit in any of the regions of enhanced electron density is tetrahedral [! Also be used to obtain the exact bond angles are of 109°28 ’ ( or approximately 109.5° ) of is... Also present in valence shell electron pair repulsion ( VSEPR ) model AX2E0.5 molecule, with a geometry intermediate ClO+2... Theory - Chemistry - molecule is linear as shown below and the bond angle is reduced from 109.5° to.... In case of H2O is distorted tetrahedral. [ 1 ]:410–417, steric numbers of 7 or are! Following points: lone pair-lone pair is in need of more space compared., axial and equatorial the resulting geometry is trigonal bipyramidal of such complexes exhibit d8. At 90° replaced by lone pairs 5 bp and 1 lp for a steric number of X E...
Moving Fish Cat Toy, Bad Idea Girl In Red Chords Piano, Nac Scholarship Recipients, Mr Sark Csgo, The House In Fata Morgana Sequel, Northwest Volleyball Schedulethunder Tactical Ar-15 Build, Motorcycle Accident In Gatlinburg, Tn, Blue Background Passport Photo Online,