(Example TOP: bonding | molecular geometry dipole moment … (Select all that apply.) ... See full answer below. The covalent bonds can be polar and nonpolar based upon the electronegativity of the atoms.eval(ez_write_tag([[728,90],'techiescientist_com-medrectangle-4','ezslot_4',104,'0','0'])); Nonpolar molecules: These are the molecules in which both atoms share an equal portion of the bonded electron pair. Explain the reason. If we were to calculate the dipole moment, the definition of a dipole moment, symbolized by the Greek letter mu, dipole moment is equal to the magnitude of that charge, Q, times the distance between those charges, d. So mu is equal to Q times d. Laser Chem. Due to their different three-dimensional structures, some molecules with polar bonds have a net dipole moment (HCl, CH2O, NH3, and CHCl3), indicated in blue, whereas others do not because the bond dipole moments cancel (BCl3, CCl4, PF5, and SF6). Figure 9: Molecules with Polar Bonds. A. Which compound would be expected to have the largest dipole moment? C. 59. 8, pp. Create your account. Organic Chemistry With a Biological Emphasis. Sulfur Hexafluoride having its chemical formula SF6 is an inorganic compound that is colorless in appearance. And an electron would have a negatively charged Q, like that. Many students may have a query about whether SF6 is polar or not. Here, acids are defined as being able to donate protons in the form of hydrogen ions; whereas bases are defined as being able to accept protons. Figure 9: Molecules with Polar Bonds. The dipole moment is calculated by multiplying the distance between the hydrogen and oxygen atoms by the difference in their charge. Consider the molecules CF4, BF3, PF3, NF3, and SF6. The bonds are all polar, but the geometry of the molecules is such that in CF4 and BF3 the individual dipole vectors cancel out, making the molecules nonpolar. So, has dipole moment. If the individual bond dipole moments cancel one another, there is no net dipole moment. So, Is SF6 Polar or Nonpolar? Draw Lewis structures for H2CO3, SF6, PF5, IF7 and CS2. µ = dipole moment (debye) δ = partial charge (C) d = distance (m) The units for dipole is expressed in debye which is also known as Coulombs x meter (C x m) Example of a Dipole. Examples of such compounds are BeCl2, SF6. More the dipole moment of a molecule, greater is its polarity.eval(ez_write_tag([[336,280],'techiescientist_com-banner-1','ezslot_6',106,'0','0'])); The polarity of a molecule is directly proportional to its dipole moment. Shape is linear. Answer = IF5 ( Iodine pentafluoride ) is Polar What is polar and non-polar? In contrast, the H2O molecule is not linear (part (b) in Figure 2.2.8); it is bent in three-dimensional space, so the dipole moments do not cancel each other. In every other case except H_2S, the polarization of charge associated with each bond is exactly cancelled by the other bonds, resulting in no net dipole moment. Individual bond dipole moments are indicated in red. This is because the VSEPR theory says that when six fluorine atoms are arranged symmetrically around the sulfur atom, the bond dipoles are cancelled. Although a molecule like CHCl3 is best described as tetrahedral, the atoms bonded to carbon are not identical. So guys, if you have any doubts regarding the polarity of SF6, you can ask them in the comment section. All the six valence electrons participate in the six covalent bonds formed leaving behind no lone pair.eval(ez_write_tag([[300,250],'techiescientist_com-large-leaderboard-2','ezslot_7',107,'0','0'])); Below is the diagram of the geometrical structure of SF6. predict whether a molecule will possess a dipole moment, given only its molecular formula or Kekulé structure. CH2O Lewis Structure, Molecular Geometry, and Hybridization, PCl5 Lewis Structure, Molecular Geometry, Hybridization, and MO Diagram, BCl3 Lewis Structure, Molecular Geometry, and Hybridization, The atomic number of sulfur hexafluoride is 16 and its electronic configuration is 2, 8, 6 i.e. Sulfur hexafluoride has a central sulfur atom around which one can see 12 electrons or 6 electron pairs. As a … Which molecule(s) has a net dipole moment? Among CO2,BeCl2,ICl4- and SF6, which has zero dipole moment? These Molecules have zero dipole moment. More electronegative gains partial negative charge because it attracts the bonded electrons more towards itself. O3 V. PCl5 How Many Of The Molecules Have No Dipole Moment? Xef4 Dipole Moment CHM … NF3 is polar, CF4 is nonpolar, and BF3 is nonpolar. use the presence or absence of a dipole moment as an aid to deducing the structure of a given compound. This is colorless and highly non-flammable. SF 6 IV. Which have a molecular dipole moment? It should be important to note that if there are polar bonds within the molecule and the shape of the molecule is symmetrical then the dipoles get canceled out with each other due to symmetry of the molecule. There are two schools of … Thus, the SF6electron geometry is considered to be octahedral. Two of these electron pairs are bonding pairs and two are lone pairs, so the molecular geometry of H, Difluoroamine has a trigonal pyramidal molecular geometry. SF4 has again trigonal bipyramid electron group arrangement(4 bonds + 1 lone pair) with one lone pair at one of the corners so it has a net dipole moment. These atoms do not have differences in their electronegativity and therefore share the larger proportion of bonded electron pair. The sulfur atom has 6 valence electrons and fluorine has 7 valence electrons in its outermost shell. SF6 IV. Thus a molecule such as H2O has a net dipole moment. Due to polarity in the S-F bond, the dipole moment in the bond is generated. Therefore, the S-F bond also gives a non zero dipole moment. The dipole moment of a molecule is therefore the vector sum of the dipole moments of the individual bonds in the molecule. A 15-dimensional analytical form for the potential energy and dipole moment surfaces of the SF6 molecule in the ground electronic state is obtained using ab initio methods. 1988, Vol. XeF4 = 4 bond pair electron, 2 lone pair. Ionic bonds are formed in the molecules in which the atoms are oppositely charged. REUSS Fysisch Laboratorium, Katholieke UniversiteitNijmegen, Toernooiveld, 1 answer. The sound velocity in this gas is 136 m/s that is 3 times less than that in air. Their vector sum is zero, so CO2 therefore has no net dipole. Required fields are marked *. Shape is octrahedral. SF4 has again trigonal bipyramid electron group arrangement(4 bonds + 1 lone pair) with one lone pair at one of the corners so it has a net dipole moment. \[ \mu = \delta \times d\] with. NO 2 III. (a) Which has bonds that are the most polar? The four fluorine atoms are covalently bonded in one plane such that it forms a square and two fluorine atoms form covalent bonds axial to the molecule. All the F-S-F is perpendicular to each other. SF6 polar or nonpolar? Similarly, the fluorine atom attracts the bonded pair of electrons slightly towards itself and gains a partial negative charge. We expect the concentration of negative charge to be on the oxygen, the more electronegative atom, and positive charge on the two hydrogens. This problem has been solved! Why is C2H4 a Nonpolar Molecule? Remember that the $\ce{\sf{C-H}}$ bond can usually be assumed to be nonpolar. However the shape of … Conversely, the presence or absence of a dipole moment may also give an important clue to a compound’s structure. I. BH 3 II. Due to this difference, the unequal sharing of bonded electrons by both atoms occur. The total number of electrons around the central atom, S, is eight, which gives four electron pairs. Dipole moment is equal to the product of the partial charge and the distance. The shape of SF 6 6 is octahedral so the dipole moment of SF 6 6 Is ZERO due to its geometric symmetry. Molecules with asymmetrical charge distributions have a net dipole moment. Similarly, the six dipoles of S-F bonds in SF6 molecule get canceled out with each other resulting in a nonpolar SF6 molecule. a) CF4 b) BF3 c) PF3 d) NF3 A molecule with 2 single bonds and 2 lone pairs of electrons around the central atom … 1S2 2S2 2P6 3S2 3P4. 19. Solution 53P:Step 1: (a)Here, we are to determine the most polar bond.The polarity of a molecule depends on the electronegativity difference between the … (is polar) a) NF3 b) CCl4 c) SiCl4 d) SF6 e) BF3. The plasma of SF6 is used in the semiconductors industries as an etchant. Indicate the type of hybrid orbitals used by the central atom in SF6. Dipole moment: It is the measure of determining the level of the polarity of a chemical compound. Your email address will not be published. Due to the arrangement of the bonds in molecules that have V-shaped, trigonal pyramidal, seesaw, T-shaped, and square pyramidal geometries, the bond dipole moments cannot cancel one another. For each three-dimensional molecular geometry, predict whether the bond dipoles cancel. Is the octet rule obeyed in these cases? And, it is generally seen that the shape of nonpolar molecules is symmetric. Therefore, the polarity of a molecule is directly proportional to the difference between the electronegativity of atoms. The electrolytic compounds like NaCl, KCl are the few examples of such compounds. HF has the largest dipole moment, you can tell which molecule has the largest by looking on the periodic table, they are usually the pair that are furthest from each other and it is also due to them having the biggest difference in electronegativity, usually the closer two elements are, the weaker the dipole moment. SF6 polar or nonpolar? Shape is octrahedral. SF6 is a non-polar molecule. Greater is the dipole moment, more is the polarity of that compound. 1. These two bonds are commonly used in chemical compounds. These atoms have differences in their electronegativity values. This geometrical structure is symmetrical in shape. Each C–O bond in CO2 is polar, yet experiments show that the CO2 molecule has no dipole moment. Consequently, the bond dipole moments cannot cancel one another, and the molecule has a dipole moment. I. BH 3 II. a) water, H2O b) acetone, CH3COCH3 c) carbon dioxide, CO2 d) sulfur dioxide, SO2 e) chloromethane, CH3Cl. Sulfur hexafluoride is made up of six fluorine atoms and a single sulfur atom. See the answer. Which of the following molecules does not have a permanent dipole moment? You can check out the reason for the non-polarity of BeCl2. A. explain how dipole moments depend on both molecular shape and bond polarity. Sulfur hexafluoride (SF 6) or sulphur hexafluoride (British spelling), is an extremely potent and persistent man-made greenhouse gas that is primarily utilized as an electrical insulator and arc suppressant. You must be able to combine your knowledge of molecular shapes and bond polarities to determine whether or not a given compound will have a dipole moment. SF6 has octahedral electron group arrangement (6 single bonds) and since all corners have F atoms the dipole moments of the bonds cancel each other and the molecule has no net dipole moment. Is the octet rule obeyed in these cases? SF4: Has four S-F bonds and since F is the most electronegative and S is moderately electro negative.S-F bonds will be polar. If they do not, then the molecule has a net dipole moment. View this answer. Q. Dipole moment of CO2 molecule is zero where as SO2 has some dipole moment. IBr. See the answer. In this article, I will answer this question and will cover the surrounding topics too. Xef4 Dipole Moment Which element between If5 Xef4 Sf6 and CH4 dipole moment . It is considered to be an extreme greenhouse gas. Sulfur hexafluoride gas has its great use as an excellent dielectric gas for high voltage applications. (B) FOOF. This gas is also used for entertainment purposes, it causes the voice to become significantly deeper because of its higher density than air. It is inorganic, colorless, odorless, non-flammable, and non-toxic. Solution 53P:Step 1: (a)Here, we are to determine the most polar bond.The polarity of a molecule depends on the electronegativity difference between the … The molecule of SF6 is symmetrical in shape ie; orthogonal geometry. Xef4 Dipole Moment 042602q114 Quiz General Chemistry 1140 April 26 . This took the Arrhenius definition one step further as water is no longer required to be present in the solution for acid and base reactions to occur. Within reactions with carbonyls, such as a reduction reaction, the carbonyl is attacked from the carbon side and not the oxygen side. The thermal conductivity of this gas is 0.0136 w/mK. Figure 8 How Individual Bond Dipole Moments Are Added Together to Give an Overall Molecular Dipole Moment for Two Triatomic Molecules with Different Structures. a) CO 2 (linear) b) SO 2 (bent) c) BF 3 (trigonal planar) d) CF 4 (tetrahedral) Learn this topic by watching Molecular vs Electron Geometry Concept Videos. The molecular mass of the SF6 molecule is 146.06 units. Consider the molecules BF3, PF3, BrF3, SF4, and SF6. Which of the following molecules has a dipole moment? All the F-S-F bonds are 90 degrees, and it has no lone pairs. 3. Which one of the following molecules has a non-zero dipole moment? 1 answer. CF4 and BF3 are symmetrical, NF3 is not. The electronegativity of fluorine is 3.98 whereas the electronegativity of sulfur is 2.58. STOLTEandJ. The molecules that are symmetrical in shape have their zero dipole moment. It is a colorless gas with no toxicity. Therefore, there is a difference between the electronegativity of both atoms. Hence the vector sum is not zero, and H2O has a net dipole moment. SF6 has its IUPAC name Sulfur hexafluoride and it is considered as an extreme gas responsible for the greenhouse effect. Therefore having a zero net-dipole. C. O3 V. PCl5 How Many Of The Molecules Have No Dipole Moment? The equation for dipole moment is as follows. The hydroxyl groups are oriented opposite of one another and therefore the dipole moments would “cancel” one another out. In 1923, chemists Johannes Brønsted and Martin Lowry independently developed definitions of acids and bases based on compounds abilities to either donate or accept protons (H+ ions). And in return, the sulfur atom gains a partial positive charge. Shape is square pyramidal. It is inorganic, colorless, odorless, non-flammable, and non-toxic. Which of the following molecules has a net dipole? BCl3, for example, has no dipole moment, while NH3 does. Polar "In chemistry, polarity is a separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multipole moment. Determine whether each of the compounds listed below possesses a dipole moment. The S-F covalent bond stabilizes each other forming a stable SF6 molecule that has a symmetrical geometrical shape. It is an odorless, non-toxic, and non-flammable gas. SF 6 has an octahedral geometry, consisting of six fluorine atoms attached to a central sulfur atom. Electronegativity is the potential of an atom to attract the bonded pair of electrons towards it.eval(ez_write_tag([[250,250],'techiescientist_com-medrectangle-3','ezslot_2',103,'0','0']));eval(ez_write_tag([[250,250],'techiescientist_com-medrectangle-3','ezslot_3',103,'0','1'])); So, the more electronegative atom tends to attract the bonded electron pair more towards itself. You previously learned how to calculate the dipole moments of simple diatomic molecules. In a molecule of sulfur hexafluoride, it consists of one sulfur atom and six fluorine atoms. Both atoms have unequal charge distribution on them. Individual bond dipole moments are indicated in red. Dipole moments occur when there is a separation of charge. Dipole moment is equal to the product of the partial charge and the distance. So polarity of bonds cancels out. SF6 is a nonpolar compound in nature because as per VSEPR theory six fluorine atoms are arranged symmetrically with the sulfur atom such that dipole moment of S-F bond gets canceled out making the SF6 a nonpolar compound.eval(ez_write_tag([[468,60],'techiescientist_com-box-3','ezslot_5',102,'0','0'])); SF6 has its IUPAC name Sulfur hexafluoride and it is considered as an extreme gas responsible for the greenhouse effect. Which of the following molecules has a permanent dipole moment? Polar Molecules: These molecules are those in which both atoms share an unequal proportion of bonded electron pairs. The oppositely charged atoms get attracted to each other by the ionic forces. SF6 is a nonpolar compound in nature because as per VSEPR theory six fluorine atoms are arranged symmetrically with the sulfur atom such that dipole moment of S-F bond gets canceled out making the SF6 a nonpolar compound. Consequently, molecules with these geometries always have a nonzero dipole moment. (a) In CO2, the C–O bond dipoles are equal in magnitude but oriented in opposite directions (at 180°). A 15-dimensional analytical form for the potential energy and dipole moment surfaces of the SF6 molecule in the ground electronic state is obtained using ab initio methods. Based on symmetry alone, we know that H_2S is the only one of these molecules that has a dipole moment. This problem has been solved! In the case of Cl_2, the 2 atoms are identical, so no polarization of the bond is possible, and the dipole moment is zero. As a result, the S-F bond becomes polar and results in a dipole moment but due to symmetry, the dipoles get canceled out with each other making the SF6 a nonpolar molecule. It is an odorless, non-toxic, and non-flammable gas. The dipole moment is a vector quantity, it has magnitude as well as direction. All Chemistry Practice Problems Molecular vs Electron Geometry Practice Problems. IBr Br2 CO2 BF3 BeCl2. µ = dipole moment (debye) δ = partial charge (C) d = distance (m) The units for dipole is expressed in debye which is also known as Coulombs x meter (C x m) Example of a Dipole. Expert Answer 100% (3 ratings) Previous question Next question 19. Among CO2,BeCl2,ICl4- and SF6, which has zero dipole moment? Four of them are in one plane making a square planar and two bonds are axial to the square plane. We will reach out to you as soon as possible. Your email address will not be published. Because there is one hydrogen and two fluorines, and because of the lone pair of electrons on nitrogen, the molecule is not symmetrical, and the bond dipoles of NHF. The following molecule has no dipole moment in the molecule itself, explain. Which of the following molecules does not have a permanent dipole moment? The electronegativity of fluorine is greater than sulfur due to which the S-F bond becomes polar. Sulfur Hexafluoride having its chemical formula SF6 is an inorganic compound that is colorless in appearance. Ionic and covalent bonds are considered to be the strongest in all the bonds. The refractive index of SF6 gas is 1.000783. Sulfur hexafluoride (SF 6) or sulphur hexafluoride (British spelling), is an extremely potent and persistent man-made greenhouse gas that is primarily utilized as an electrical insulator and arc suppressant. Due to their different three-dimensional structures, some molecules with polar bonds have a net dipole moment (HCl, CH2O, NH3, and CHCl3), indicated in blue, whereas others do not because the bond dipole moments cancel (BCl3, CCl4, PF5, and SF6). It is considered to be an extreme greenhouse gas. If we talk about the geometrical shape of sulfur hexafluoride, there are six S-F covalent bonds. Electronegativity: Greater the electronegativity of an atom, more is the strength of attracting the bonded electrons. (is polar) a) NF3 b) CCl4 c) SiCl4 d) SF6 e) BF3. The dipole moment of a chemical compound is the measure of its polarity. Then, the angle between the atoms is used to find the net dipole moment. The SF6 is an inert gas that is used widely in magnesium industries. 2) XeF2 = 2 bond pair electron, 0 bond pair. It is an odorless, non-toxic, and non-flammable gas. This occurs due to an atoms' electronegativity - where one atom has the ability to attract electrons towards it (In other words, electrons wants to spend other time around it) giving it a negative charge and the other a positive charge. Which of the following molecules has a dipole moment? After completing this section, you should be able to. For the polar compounds, indicate the direction of the dipole moment. (a) Which has bonds that are the most polar? C. (b) In H2O, the O–H bond dipoles are also equal in magnitude, but they are oriented at 104.5° to each other. The molecules have atoms held by the types of different forces like ionic, covalent, metallic, and hydrogen bonds. SF6 has octahedral electron group arrangement (6 single bonds) and since all corners have F atoms the dipole moments of the bonds cancel each other and the molecule has no net dipole moment. 275-281 (C) 1988 HarwoodAcademicPublishers GmbH Photocopyingpermitted by license only Reprints available directly from the Publisher Printed in the United Kingdom Hole Burning in the IR Predissociation Spectrum of SFs-dimers B. HEIJMEN,C. Using knowledge of electronegativity explain why this happens. SF6 = 6 bond pair electron, 0 lone pair. Sulfur Hexafluoride having its chemical formula SF6 is an inorganic compound that is colorless in appearance. (b) Which have a molecular dipole moment? XeF6 = SF6 = 6 bond pair electron, 0 lone pair. Such is the case for CO2, a linear molecule (part (a) in Figure 2.2.8). A) SF6 B) CCl4 C) NF3 D) SiCl4 E) BF3 ANS: OBJ: 10.3) KEY: C PTS: 1 DIF: easy REF: 10.2 Explain the relationship between dipole moment and molecular geometry. This suggests that in BCl3 the chlorines around boron are in a trigonal planar arrangement, while the hydrogens around nitrogen in NH3 would have a less symmetrical arrangement (e.g., trigonal pyramidal, T-shaped). Expert Answer 100% (3 ratings) Previous question Next question (A) SF 6 6. It is also not flammable in nature. It is considered to be an extreme greenhouse gas. (b) Which have a molecular dipole moment? The observed net dipole moment for PH3 is 0.58 Debye, a fairly substantial dipole moment for a molecule with almost nonpolar bonds. As a result, the octahedral shape of the molecule is formed. Which of the following has a zero dipole moment? SF 6 has an octahedral geometry, consisting of six fluorine atoms attached to a central sulfur atom. asked Apr 15, 2020 in Chemical Bonding and Molecular Structure by Rukmani ( 51.1k points) The covalent compounds are the compounds in which the atoms share electrons of each other to get stabilized. Consider the molecules BF3, PF3, BrF3, SF4, and SF6. This leads to having a partial positive charge on the carbon and the reduction can take place. Because the two C–O bond dipoles in CO2 are equal in magnitude and oriented at 180° to each other, they cancel. asked Nov 27 in Chemistry by Panna01 (47.2k points) chemical bonding; molecular structure; class-11; 0 votes. NO 2 III. O 3 V. PCl 5 How many of the molecules have no dipole moment? So, has NO dipole moment. O 3 V. PCl 5 How many of the molecules have no dipole moment? Although the polar bonds exist within the SF6 molecule, the complete molecule is nonpolar in nature. Many students may have a query about whether SF6 is polar or not. (A) Linear (B) Octahedral (C) Square planar (D) Tetrahedral (E) Trigonal pyramidal. Key Ideas: Dipole moments result from asymmetry in the distribution of the electron cloud. sp3d2. Many students may have a query about whether SF6 is polar or not. \[ \mu = \delta \times d\] with. It means, both atoms covalently bonded have an equal distribution of charge on them. As a result, the shape of the SF6 molecule is formed as octahedral geometry. a) water, H2O b) acetone, CH3COCH3 c) carbon dioxide, CO2 d) sulfur dioxide, SO2 e) chloromethane, CH3Cl. The sulfur atom is the central atom connected with the six fluorine atoms. asked Nov 27 in Chemistry by Panna01 (47.2k points) chemical bonding; molecular structure; class-11; 0 votes. (A) HCN (B) NH3 (C) SO2 ( D) NO2 (E) PF5 ... PCl5, SF6 Which of the following does not describe any of the molecules above? Save my name, email, and website in this browser for the next time I comment. Geometrical shape: The geometrical shape of a molecule is an important factor in determining the polarity of a molecule. This charge polarization allows H2O to hydrogen-bond to other polarized or charged species, including other water molecules. Does SF6 have a dipole moment? Other examples of molecules with polar bonds are shown in Figure 2.2.9. The oxygen is more electronegative than the carbon and therefore creates a dipole along the bond. In case, if molecules have a polar bond within it, their dipole moment gets canceled out with each other making the molecule a nonpolar. It does not conduct electricity. The atoms that form a nonpolar covalent bond has equal electronegativity. The equation for dipole moment is as follows. The fluorine atom is higher electronegative than sulfur atom due to which the fluorine atom attracts the bonded pair of electron slightly towards itself. In more complex molecules with polar covalent bonds, the three-dimensional geometry and the compound’s symmetry determine whether there is a net dipole moment. As a result, the CO2 molecule has no net dipole moment even though it has a substantial separation of charge. Mathematically, dipole moments are vectors; they possess both a magnitude and a direction. Make certain that you can define, and use in context, the key term below. 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. If we talk about the conductivity of SF6, it is an excellent insulator. The geometrical shape of such atoms is also symmetric. LIEDENBAUM,S. The net dipole moment for a molecule is the vector sum of the individual bon dipoles. Draw Lewis structures for H2CO3, SF6, PF5, IF7 and CS2. SF 6 IV. 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Of its higher density than air, metallic, and it has a non-zero dipole moment of a given.. { C-H } } $ bond can usually be assumed to be an extreme gas responsible for the of... As H2O has a dipole along the bond moment of SF 6 has an octahedral geometry, of. That are the few examples of molecules with polar bonds are axial to the difference between electronegativity. [ \mu = \delta \times d\ ] with I comment types of different like..., BeCl2, ICl4- and SF6, PF5, IF7 and CS2 gas is used... Not have a query about whether SF6 is an excellent dielectric gas high. Nonpolar covalent bond has equal electronegativity the partial charge and the reduction can take place Problems molecular electron! In Chemistry by Panna01 ( 47.2k points ) chemical bonding ; molecular structure ; class-11 ; 0.. A reduction reaction, the key term below, non-flammable, and the reduction can take place with! F is the strength of attracting the bonded pair of electron slightly towards itself to as... Sulfur is 2.58 including other water molecules will possess a dipole moment each the...
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