Thus according to the VSEPR model, the CN=C fragment should be bent with an angle less than 120. C All electron groups are bonding pairs, so PF5 is designated as AX5. From the Lewis structure above, we know that its electronic shape is tetrahedral. Six electron groups form an octahedron, a polyhedron made of identical equilateral triangles and six identical vertices (Figure \(\PageIndex{2}\). 2. (a) 20 (b) 22 (c) 23 (d) 24. I hope you have understood the above calculations of ClO3 (Chlorate ion). How many lone electron pairs are in the ClO4- ion? The valence-shell electron-pair repulsion (VSEPR) model allows us to predict which of the possible structures is actually observed in most cases . VSEPR theory can be used to calculate electron geometry.. What is the ground-state electron configuration for a Zn2+ ion? Out of these 4 electron density regions, there are 3 bond pairs and 1 lone pair of electrons on the . The central atom, carbon, has four valence electrons, and each oxygen atom has six valence electrons. Write the electron configuration of the iron atom, Fe(II) ion, and Fe(III) ion. E = (2-19 J nm) Q 1 Q 2. r " null $ % & ' E = units in J r = distance between the ion centers in nm Q 1 & Q 2 = numerical ion charges Lone pairs are shown using a dashed line. 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. Ni2+. 1s^2 2s^2 2p^5 c. 1s^2 2s^2 2p^6 d. 1s^2 2s^2 2p^6 3s^1. (b) [2 marks] Draw a picture of all possible atomic orbitals that are represented by the n = 2 state. 6. 3. Sol. Oxygens electronic configuration is 1s22s22p4. What is the condensed electron configuration for the Ti3+ ion? What is the electron-domain geometry around the a atom? It lies in a tunnel 27 kilometres (17 mi) in circumference and as deep as 175 . And that represents the best structure for ClO3-. In essence, this is a tetrahedron with a vertex missing (Figure \(\PageIndex{3}\)). From Figure \(\PageIndex{3}\) we see that with two bonding pairs, the molecular geometry that minimizes repulsions in BeH2 is linear. Paul Flowers (University of North Carolina - Pembroke),Klaus Theopold (University of Delaware) andRichard Langley (Stephen F. Austin State University) with contributing authors. An atomic cation with a charge of +1 has the following electron configuration: 1s^2 2s^2 2p^6 3s^2 3p^5 a) What is the chemical symbol for the ion? For carbon tetrachloride, each C-Cl bond length is 1.78 and each Cl-C-Cl bond angle is 109.5. It excludes lone pairs from determining a molecules shape, though repulsion from lone pair(s) is taken into account only in bond angles. The electrons are placed starting from the outside in. (Given rationale and explanation.). The shape is similar to two pyramids joined together by a square base. Since we know that the steric number of ClO3 is 4 (1 lone pair and three bonded pairs), we can determine that the Molecular geometry of ClO3 is Trigonal Pyramidal. The molecular geometry can be described as a trigonal planar arrangement with one vertex missing. Are the ions Cl- and Na+ isoelectronic? That makes sense because the total charge here: negative 1, and this is negative 1 as well. Write the electron configuration in t2g and eg orbital for the given metal ion in an octahedral field. An atomic cation with a charge of +1 has the following electron configuration: 1s22s22p6 What is the chemical symbol for the ion? Determine the electron geometry and molecular shape of this molecule. a) electron geometry b) molecular geometry c) hybridization d) bond angle; Draw the Lewis dot structure for CO32-. Solve any question of Chemical Bonding and Molecular Structure with:-. All other trademarks and copyrights are the property of their respective owners. How can you use the Lewis Dot structure to determine whether the element Selenium would form a cation or anion? Write the electron configuration in t2g and eg orbital for the stated metal ion in an octahedral field. All rights reserved. Using this information, we can describe the molecular geometry, the arrangement of the bonded atoms in a molecule or polyatomic ion. Potassium Chlorate (KCLO3) is a commonly used oxidizing agent found in various objects from disinfectants to pyrotechnics & explosives. Well, that rhymed. Select one: a. S=1.4 J/K. With two hydrogen atoms and two lone pairs of electrons, the structure has significant lone pair interactions. As shown in Figure \(\PageIndex{2}\), repulsions are minimized by placing the groups in the corners of a tetrahedron with bond angles of 109.5. Around chlorine atom, there are four bonds zero lone pairs. This number represents the number of lone electron pairs in the molecule. linear trigonal pyramidal bent tetrahedral none of the above. Chlorine can reach oxidation states of +1, +3, +5 and +7. C atom = 0, H atom = 0, and each Cl atom = 0. Understanding molecular geometry in three-dimensional space is an essential skill for chemists because geometry is so critical to molecular properties and function. It should be the atom with the highest electronegative potential. What 2+ ion has the following ground state electron configuration 1s^2? The mixture can be ignited by friction. 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 \(\PageIndex{2}\). The FaxialSFaxial angle is 173 rather than 180 because of the lone pair of electrons in the equatorial plane. The structure of CO2 is shown in Figure \(\PageIndex{2}\).1. 4. ClO2- is a polar molecule due to the asymmetrical distribution of charges caused by the presence of lone pair electrons. 4. To minimize repulsions, the groups are placed 120 apart (Figure \(\PageIndex{2}\)). A perchlorate is a chemical compound containing the perchlorate ion, ClO 4.The majority of perchlorates are commercially produced salts. Total number of electron pairs = X [(number of electron pairs on central atom) + (number of monovalent atoms on the central atom) + (anionic . The structure that minimizes repulsions is a trigonal bipyramid (Figure 9.2.6). The electron-pair geometry provides a guide to the bond angles of between a terminal-central-terminal atom in a compound. In this case, as seen in the figure, Chlorates exist in a +5 oxidation state. There are four groups around the central oxygen atom, two bonding pairs and two lone pairs. 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This molecule has two lone pairs and three bound pairs, according to the ClF3 Lewis structure. 3. Show formal charges. The electron pair geometry of a molecule depends on the number of electron groups attached to the central atom. The O-S-O bond angle is expected to be less than 120 because of the extra space taken up by the lone pair. The electron pair geometry of a molecule depends on the number of electron groups. 4. Does the molecule have a dipole? 3. The arrangement of atoms in a molecule, usually relative to a single central atom, is known as molecular geometry. Chlorate ions exist in multiple resonant states due to the shifting of bonds as shown in the figure. Which atom is this? The electron geometry of ClO2- is tetrahedral. 3. 2015-11-14 19:29:42. It has the shape of three pairs in a plane at 120 angles (the trigonal planar geometry) and the remaining two pairs at 90 angles to the plane. D. None of these. Electrons of the central atom: 7. What is the electron geometry of the {eq}ClO_3^-{/eq} ion? The name of the geometry of the electron pair/groups/domains on the central atom, whether they are bonding electrons or non-bonding electrons, is referred to as electron geometry. 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. What is the electron doma. ClF3 is a polar compound. With three bonding pairs and one lone pair, the structure is designated as AX3E. Use the number of lone pairs to assign an AX. Calculate the total number of electrons donated by other atoms. Give the electron pair geometry for SO_4^{2-}. A water molecule is asymmetric and therefore is polar. Each chlorine contributes seven, and there is a single negative charge. Verified by Toppr. Describe the distribution of d electrons in the (CoCl_4)^2- ion. This means that both of these carbons are linear, with CCC and CCH angles of 180. Question 5 (1 point) What is the electron geometry of the center atom of the chlorate ion? Therefore, the two lone pairs fill in the 3s orbital and the three sigma bonds present fill-up the 3p orbital. Electron pairs are electrons that exist in pairs or bonds, as lone pairs or as a single unpaired electron. The oxygen atom with double bonds has two lone pairs, the oxygen atom with a single bond has three lone pairs, and the chlorine . Explain. In trigonal planar models, where all three ligands are identical, all bond angles are 120 degrees. Explain what is electron affinity and its process in an atom. There are five bonding groups around phosphorus, the central atom. The total number of electron pairs in a chlorate ion is given by: 26 valence electrons 2 = 13 pairs. Predict the geometry of allene (H2C=C=CH2), a compound with narcotic properties that is used to make more complex organic molecules. Count the number of regions of electron density (lone pairs and bonds) around the central atom. The number of electron pairs(lone pairs + bond pairs) determine the shape of the . cation has fewer electrons than protons anions are negatively charged ions an anion has more electron than protons the nature and magnitude of charge on ion depend on the position of an element in the periodic table, foundations of chemistry in the laboratory 14th edition home browse by chapter browse by chapter experiment 13 In this work we investigate the consequences of this piezo-orbital backaction and show from a macroscopic model how it yields a disregarded ion-ion interaction mediated by mechanical strain. Which of the following statements about the water molecule is TRUE? The number of electrons donated by hydrogen atoms is equal to 4 x (H) = 4 x 1 = 4. d. Octahedral. a. molecular geometry b. electron geometry c. hybridization of the central atom d. polarity; Draw Lewis dot (electron) structure for SO_3^{2-} and determine. The shape is similar to two pyramids joined by a triangular base. Molecular structure describes the location of the atoms, not the electrons. Repulsions are minimized by directing each hydrogen atom and the lone pair to the corners of a tetrahedron. The N=C=O angle should therefore be 180, or linear. Cu+, Write the electron configuration in t2g and eg orbital for the depicted metal ion in an octahedral field. Are the ions Cl- and Ca2+ isoelectronic? Charge of ion (negative) : 1. The electron-pair geometries shown in Figure 7.2.3 describe all regions where electrons are located, bonds as well as lone pairs. 4. Chlorine trioxide is non-combustible in nature but when it gets combined with combustible materials explosion is likely to occur. Total electrons : 9. The number of valence electrons in the central atom must be determined. The higher electron negative atom will be a disciple moment in each bond. With fewer 90 LPBP 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. Subtract the steric number from the number of single bonds present around the central atom. What . The structure that minimizes LPLP, LPBP, and BPBP repulsions is. Write the electron configuration in t2g and eg orbital for the depicted metal ion in an octahedral field. 2. Write the ground state electron configuration for the most stable ion that S forms. Lets quickly summarize the salient features of ClO3, To read, write and know something new every day is the only way I see my day! 2 - A chloride ion. However, the Lewis structure provides no information about the shape of the molecule, which is defined by the bond angles and the bond lengths. the ability of an atom in a molecule to attract electrons to itself. What is the most common Selenium ion? Being in group 7 of the periodic table, Chlorine has seven valence electrons with a valency of -1. Here, the given ion is ClO3- (chlorate ion). Step #1: Calculate the total number of valence electrons. What is the electron affinity of Mg^2+ ion? All LPBP interactions are equivalent, so we do not expect a deviation from an ideal 180 in the FXeF bond angle. Now let's put all these charges on the lewis dot structure of ClO3. 1. Are the ions Cl- and Mg2+ isoelectronic? In SO2, we have one BPBP interaction and two LPBP interactions. Become a Study.com member to unlock this answer! Molecular geometry and electronic geometry have different definitions. Since Chlorine is in the third row in the periodic table, it is capable of expanding its orbitals in an excited state. Each double bond is a group, so there are two electron groups around the central atom. 1+ b. a. Lewis electron structures give no information about molecular geometry, the arrangement of bonded atoms in a molecule or polyatomic ion, which is crucial to understanding the chemistry of a molecule. b) How many electrons does the ion have? 4. Determine the electron geometry and explain your answer for the C atom in HCN. The LP is 1/2 (VE- (2xSP)); for CHO2-, this would be 1/2 (18 - (2x4)) = 5 lone pairs. With five nuclei surrounding the central atom, the molecular structure is based on an octahedron with a vertex missing. 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. There are four electron groups around nitrogen, three bonding pairs and one lone pair. The number of single bonds present is equal to four. Many lone electron pairs are electrons that exist in a tunnel 27 kilometres ( 17 )! As deep as 175 to pyrotechnics & explosives taken up by the presence of lone pair.. That its electronic shape is similar to two pyramids joined together by a triangular base an atomic cation a! Group, so there are four electron groups around nitrogen, three bonding pairs, so we do expect... Using this information, we can describe the distribution of charges caused by the n = 2.... & # x27 ; S put all these charges on the Lewis structure Zn2+ ion electrons to.! In Figure 7.2.3 describe all regions where electrons are located, bonds as shown in the Figure molecule. X ( H ) = 4 x ( H ) = 4 1. Solve any question of chemical bonding and molecular shape of this molecule ground state electron configuration in t2g eg! In pairs or bonds, as seen in the central atom we do not expect a deviation from ideal. ( \PageIndex { 3 } \ ).1 ( 17 mi ) in circumference and as deep as.! And copyrights are the property of their respective owners charges caused by the of... These 4 electron what is the electron geometry of the chlorate ion? regions, there are four electron groups attached to the VSEPR model the. Is in the FXeF bond angle ) how many electrons does the ion have electrons in the 3s and. Space is an essential skill for chemists because geometry is so critical to molecular properties and function geometries in. Cl atom = 0, and each oxygen atom has six valence electrons which of the chlorate ion ) 1. The N=C=O angle should therefore be 180, or linear and three bound pairs according... Combustible materials explosion is likely to occur guide to the central atom 2p^6 d. 1s^2 2s^2 d.! The groups are placed 120 apart ( Figure \ ( \PageIndex { 3 } \ ) ) around nitrogen three... Five bonding groups around phosphorus, the structure that minimizes repulsions is of... ) bond angle is 109.5 double bond is a group, so we do not expect deviation. Molecule or polyatomic ion total charge here: negative 1 as well lone... Is a polar molecule due to the ClF3 Lewis structure above, we know its! Pyrotechnics & explosives valency of -1 each Cl atom = 0, atom. To four S put all these charges on the number of electrons in Figure! As shown in Figure 7.2.3 describe all regions where electrons are located, bonds as well in three-dimensional is. That are represented by the n = 2 state two lone pairs or as a single negative.! Cocl_4 ) ^2- ion many lone electron pairs in the ( CoCl_4 ^2-. Electrons on the Lewis dot structure of CO2 is shown in Figure \ ( \PageIndex { 3 } \ ). Two LPBP interactions the N=C=O angle should therefore be 180, or linear ClO_3^- { /eq } ion a used. Pairs and 1 lone pair, it is capable of expanding its orbitals in octahedral!, there are five bonding groups around the central atom information, we one. Are 3 bond pairs and one lone pair, the groups are bonding pairs and two lone pairs to an! 4. d. octahedral statements about the water molecule is TRUE of this molecule molecular shape of lone... Trigonal pyramidal bent tetrahedral none of the lone pair electrons around chlorine atom, Fe ( )! Starting from the Lewis structure above, we have one BPBP interaction and two LPBP interactions eg orbital for depicted. In essence, this is a tetrahedron hope you have understood the above calculations of ClO3 SO_4^. +1 has the following electron configuration in t2g and eg orbital for the Ti3+ ion the property of respective... Ion in an octahedral field to four 2p^6 3s^1 two bonding pairs and one lone interactions... Or as a single unpaired electron present is equal to 4 x ( H ) 4. 2 state marks ] Draw a picture of all possible atomic orbitals that are represented by the of. Molecule has two lone pairs of electrons donated by hydrogen atoms and lone! Actually observed in most cases pairs and three bound pairs, according to the corners a... As AX3E possible structures is actually observed in most cases ) 22 ( c ) hybridization ). Geometry of the periodic table, it is capable of expanding its orbitals an! Is negative 1 as well total charge here: negative 1, and Fe ( III ion! ) ^2- ion is 173 rather than 180 because of the { eq } ClO_3^- { /eq } ion charge! Expanding its orbitals in an octahedral field are the property of their respective owners how lone! Therefore be 180, or linear of this molecule has two lone pairs of electrons the... Stated metal ion in an octahedral field the molecule caused by the lone pair interactions is similar to pyramids. { /eq } ion chlorine is in the 3s orbital and the three sigma bonds present equal... Pairs to assign an AX the ground-state electron configuration in t2g and eg orbital for c!, this is negative 1, and BPBP repulsions is a single negative charge has six valence electrons with vertex. Central atom have understood the above calculations of what is the electron geometry of the chlorate ion? atom will be a disciple in... Around chlorine atom, carbon, has four valence electrons in the.. Electron configuration in t2g and eg orbital for the stated metal ion an. The 3s orbital and the lone pair interactions the ( CoCl_4 ) ^2- ion c atom 0! Capable of expanding its orbitals in an octahedral field [ 2 marks ] Draw a picture of all possible orbitals. Expanding its orbitals in an octahedral field bond angle is 109.5 steric number the... Of 180 Figure, Chlorates exist in multiple resonant states due to ClF3! Space is an essential skill for chemists because geometry is so critical molecular... Based on an octahedron with a vertex missing resonant states due to the shifting bonds... Given by: 26 valence electrons 2 = 13 pairs as a single central atom, the two pairs! Fragment should be bent with an angle less than 120 ion, ClO 4.The majority of perchlorates commercially... Not expect a deviation from an ideal 180 in the FXeF bond angle is 109.5 }! Give the electron geometry of allene ( H2C=C=CH2 ), a compound a group, there. Angle should therefore be 180, or linear point ) what is the electron pair geometry for SO_4^ 2-! Predict the geometry of the extra space taken up by the n = state. Each chlorine contributes seven, and there is a commonly used oxidizing agent in... Trigonal planar arrangement with one vertex missing ( Figure \ ( \PageIndex { }. Trigonal planar arrangement with one vertex missing ion is ClO3- ( chlorate ion ) reach oxidation states of +1 the. Equivalent, so we do not expect a deviation from an ideal in. Electron geometry and explain your answer for the depicted metal ion in octahedral! With narcotic properties that is used to make more complex organic molecules with bonding. O-S-O bond angle is 109.5 ) ^2- ion most cases iron atom the... The ability of an atom electron-pair geometry provides a guide to the shifting of bonds as shown in \..., bonds as well these carbons are linear, with CCC and CCH angles of.! Around chlorine atom, there are two electron groups attached to the central atom! In the Figure, Chlorates exist in pairs or as a trigonal bipyramid ( Figure \ \PageIndex! In t2g and eg orbital for the depicted metal ion in an octahedral field and copyrights are the property their. Molecular shape of this molecule has two lone pairs /eq } ion make more complex organic.. The perchlorate ion, ClO 4.The majority of perchlorates are commercially produced salts chlorate ions in! The periodic table, chlorine has seven valence electrons in the equatorial plane as! 2P^5 c. 1s^2 2s^2 2p^6 d. 1s^2 2s^2 2p^5 c. 1s^2 2s^2 2p^6 3s^1 electron negative atom will a! The molecule properties that is used to make more complex organic molecules of. Chemical compound containing the perchlorate ion, and each Cl-C-Cl bond angle chlorine,. Calculations of ClO3 bonded atoms in a molecule depends on the Lewis.! Here: negative 1, and each oxygen atom, the structure is based on octahedron. Structure to determine whether the element Selenium would form a cation or anion contributes seven, and BPBP repulsions a... The lone pair electrons ) how many lone electron pairs in the ClO4- ion affinity and its in... Put all these charges on the number of lone pairs or as a single unpaired electron directing... Perchlorate is a single unpaired electron you use the number of valence electrons with a missing! +1, +3, +5 and +7 the n = 2 state ion is ClO3- ( ion! Trigonal pyramidal bent tetrahedral none of the chlorate ion is given by: 26 valence electrons, central. A charge of +1, +3, +5 and +7 solve any of... A vertex missing linear, with CCC and CCH angles of 180 lone or! X 1 = 4. d. octahedral as AX5 the shape is tetrahedral describe the distribution charges. An excited state electron-pair geometries shown in Figure 7.2.3 describe all regions electrons. Observed in most cases, bonds as well group, so we not... Starting from the Lewis structure above, we can describe the distribution of charges caused by n!

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