Explain the difference between a nonpolar covalent bond, a polar covalent bond, and an ionic bond. For IF4+SbF6-, the geometry previously reported for IF4+ was reasonably close to that found in this study despite a very large R-factor of 0.15 and a refinement in an incorrect space group. Question. Draw the Lewis structures and predict the shape of each compound or ion: A molecule with the formula AB2, in which A and B represent different atoms, could have one of three different shapes. Thus, the SF6electron geometry is considered to be octahedral. SF4 Molecular Geometry. Use the Molecule Shape simulator to explore real molecules. Is X boron or phosphorus? Explain why a sample of iron(III) sulfate is uncharged. 3 Chemical and Physical Properties Expand this section. NaCl consists of discrete ions arranged in a crystal lattice, not covalently bonded molecules. (c) Removal of the 4s electron in Ca requires more energy than removal of the 4s electron in K because of the stronger attraction of the nucleus and the extra energy required to break the pairing of the electrons. Molecular geometry can be determined by the number of bonds that a particular molecule has. c) Molecular shape is linear, lone pairs go into the horizintal trigonal plane. It has sp3d3 hybridisation. Watch the recordings here on Youtube! The lattice energy of KF is 794 kJ/mol, and the interionic distance is 269 pm. 10 points! Calculate the formal charge of chlorine in the molecules Cl2, BeCl2, and ClF5. If all the 7 are bond pairs then the shape would be pentagonal bypiramidal. (c) Both the electron geometry and the molecular structure are linear. Rotate the molecule to observe the complete geometry. Which of the molecules and ions in Exercise contain polar bonds? Determine the formal charges: Sulfuric acid is the industrial chemical produced in greatest quantity worldwide. P, I, Cl, and O would form anions because they are nonmetals. Is the actual structure consistent with the formal charges? So the molecule is a radical. Structure and Heats of Formation of Iodine Fluorides and the Respective Closed-Shell Ions from CCSD(T) Electronic Structure Calculations and Reliable Prediction of the Steric Activity of the Free-Valence Electron Pair in ClF6−, BrF6−, and IF6−. Starting with the central atom, click on the double bond to add one double bond. SF6 is octahedral, for example, and does have 90 degree angles, as does PF6(-1). There are two molecular structures with lone pairs that are exceptions to this rule. Clearly, IF6+ has six bonds. Is the Cl2BBCl2 molecule polar or nonpolar? Atoms bonded to central atom: 1. All the F-S-F bonds are 90 degrees, and it has no lone pairs. You may need to rotate the molecules in three dimensions to see certain dipoles. Two electrons are shared in a single bond; four electrons are shared in a double bond; and six electrons are shared in a triple bond. The material on this site can not be reproduced, distributed, transmitted, cached or otherwise used, except with prior written permission of Multiply. The molecular geometry of IF5, also known as iodine pentafluoride, is a pyramid with a square base surrounding a central iodine atom. How long will the footprints on the moon last? Thus, all of the valence electrons in PbCl2 are located on the Cl– ions, and all of the valence electrons in a HCl molecule are shared between the H and Cl atoms.”. Identify the electron pair geometry and the molecular structure of each of the following molecules or ions: (a) IF 6 + (b) CF 4 Does whmis to controlled products that are being transported under the transportation of dangerous goodstdg regulations? Inorganic Chemistry 2008, 47 (12) , 5485-5494. The molecular geometry is the geometrical arrangement of the atoms around the central atom. Based on formal charge considerations, which of the following would likely be the correct arrangement of atoms in sulfur dioxide: OSO or SOO? You can view video lessons to learn Molecular vs Electron Geometry. (second structure). 5 Chemical Vendors. Examples: Use the electron dot structure (Lewis structure) and the molecular shape table to determine the molecular shape (molecular geometry). ii. The skeleton structures of these species are shown: Write the Lewis structures for the following, and include resonance structures where appropriate. Sketch the bond dipoles and molecular dipole (if any) for O, (c) Predict whether there should be a molecular dipole for NH. And also, if you can help with this one: What is the number of regions of electron density? In Al, the removed electron is relatively unprotected and unpaired in a p orbital. All Rights Reserved. What is its molecular structure? Which of the following atoms would be expected to form negative ions in binary ionic compounds and which would be expected to form positive ions: P, I, Mg, Cl, In, Cs, O, Pb, Co? This problem has been solved! Explain your choice. When did organ music become associated with baseball? 6.E: Chemical Bonding and Molecular Geometry (Exercises), [ "article:topic", "authorname:openstax", "hypothesis:yes", "showtoc:yes", "license:ccby", "transcluded:yes", "source[1]-chem-77587" ], https://chem.libretexts.org/@app/auth/2/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FSUNY_Oneonta%2FChem_221%253A_Organic_Chemistry_I_(Bennett)%2F3%253AStuff_to_Review_from_General_Chemistry%2F06%253A_Chemical_Bonding_and_Molecular_Geometry%2F6.E%253A_Chemical_Bonding_and_Molecular_Geometry_(Exercises). Why is it incorrect to speak of a molecule of solid NaCl? Count the number of electron pairs around the central atom. Molecular Geometries The VSEPR theory describes five main shapes of simple molecules: linear, trigonal planar, tetrahedral, trigonal bipyramidal, and … A compound with a molar mass of about 42 g/mol contains 85.7% carbon and 14.3% hydrogen by mass. Using the standard enthalpy of formation data in Appendix G, show how the standard enthalpy of formation of HCl(g) can be used to determine the bond energy. Bond angles for IF6+ are 60 . 6. Determining molecular shape (ESBMC) To predict the shape of a covalent molecule, follow these steps: Draw the molecule using a Lewis diagram. When two electrons are removed from the valence shell, the Ca radius loses the outermost energy level and reverts to the lower n = 3 level, which is much smaller in radius. Write the Lewis structure for a molecule of the compound. The Lewis dot structure of "NH"_3 is The central atom, "N", has four groups bonded to it: three hydrogen atoms and a lone pair. There are six I-F bonds. As with IF 7, application of VSEPR rules suggests seven electron pairs. Explain whether the “real” bond angle should be larger or smaller than the ideal model angle. Determine the formal charge on each atom in each of the resonance structures: Based on formal charge considerations, which of the following would likely be the correct arrangement of atoms in nitrosyl chloride: ClNO or ClON? What information can you use to predict whether a bond between two atoms is covalent or ionic? (a) Predict the electron-domain geometry around the centralXe atom in XeF2, XeF4, and XeF6. Lewis dot formulas, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDS), are diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule. 2005-03-27. What is the molecular geometry of "NH"_3? Lewis dot formulas, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDS), are diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule. 2 Names and Identifiers Expand this section. d) Hybridization is sp3d (VSEPR 5 pairs on central atom so need 5 orbitals) e) Nonpolar. Missed the LibreFest? (c) With a small partial negative charge on A, turn on the electric field and describe what happens. Write the Lewis symbols for the monatomic ions formed from the following elements: Write the Lewis symbols of the ions in each of the following ionic compounds and the Lewis symbols of the atom from which they are formed: In the Lewis structures listed here, M and X represent various elements in the third period of the periodic table. Sketch and name the three different shapes that this molecule might have. Chapter 7 Chemical Bonding and Molecular Geometry Figure 7.1 Nicknamed “buckyballs,” buckminsterfullerene molecules (C60) contain only carbon atoms.Here they are shown in a ball-and-stick model (left). Lone pair electrons of central atom: 3 pairs (6 electrons total) Molecular Shape of I 2 (Answer): LINEAR Predict the electron pair geometry and the molecular structure of each of the following ions: Identify the electron pair geometry and the molecular structure of each of the following molecules: electron-pair geometry: trigonal planar, molecular structure: bent (120°); electron-pair geometry: linear, molecular structure: linear; (c) electron-pair geometry: trigonal planar, molecular structure: trigonal planar; electron-pair geometry: tetrahedral, molecular structure: trigonal pyramidal; electron-pair geometry: tetrahedral, molecular structure: tetrahedral; electron-pair geometry: trigonal bipyramidal, molecular structure: seesaw; (g) electron-pair geometry: tetrahedral, molecular structure: trigonal pyramidal. (g) \(\ce{ClOF2+}\) (Cl is the central atom), (c) the oxygen atom in hydrogen peroxide, HOOH, the oxygen atom in the OH group in nitric acid, HNO, the central oxygen atom in the ozone molecule, O, (g) each of the carbon atoms in propyne, CH, (i) each of the carbon atoms in allene, H. Adjust the electronegativity value so the bond dipole is pointing toward B. NaF crystallizes in the same structure as LiF but with a Na–F distance of 231 pm. 2 Names and Identifiers Expand this section. Only the outer electrons move. The 2 ∆EN (F-Xe) vectors in the vertical plane will cancel. Space must be provided for each pair of electrons whether they are in a bond or are present as lone pairs. Define the problem: Write Lewis Structures for a list of formulas and identify their shape. Recognize the difference between electron and molecular geometry. SeS2, CCl2F2, PCl3, and ClNO all have dipole moments. This leads to the smaller angle of 104.5°. Draw the structure of hydroxylamine, H3NO, and assign formal charges; look up the structure. Solution We write the Lewis structure of NH 4 + as: \(\ce{ClO2-}\) b. Which bond in each of the following pairs of bonds is the strongest? Determining molecular shape (ESBMC) To predict the shape of a covalent molecule, follow these steps: Draw the molecule using a Lewis diagram. The placement of the two sets of unpaired electrons in water forces the bonds to assume a tetrahedral arrangement, and the resulting HOH molecule is bent. Write the formula of each compound using the chemical symbols of each element: Write the Lewis structure for the diatomic molecule P2, an unstable form of phosphorus found in high-temperature phosphorus vapor. What did women and children do at San Jose? VSEPR Notation. Do not add any more atoms. Or if you need more Molecular vs Electron Geometry practice, you can also practice Molecular vs Electron Geometry practice problems. Use the Molecule Shape simulator to explore real molecules. Molecular Weight: 81.003 g/mol. Does a cation gain protons to form a positive charge or does it lose electrons? Complete the following Lewis structure by adding bonds (not atoms), and then indicate the longest bond: Use the bond energy to calculate an approximate value of ΔH for the following reaction. How do they differ? Draw them and discuss how measurements of dipole moments could help distinguish among them. Describe the molecular structure around the indicated atom or atoms: tetrahedral; trigonal pyramidal; (c) bent (109°); trigonal planar; bent (109°); bent (109°); (g) CH3CCH tetrahedral, CH3CCH linear; (h) tetrahedral; (i) H2CCCH2 linear; H2CCCH2 trigonal planar. These molecules have single and double carbon-carbon bonds arranged to Draw the Lewis electron dot structures for these molecules, including resonance structures where appropriate: predict the molecular shapes for \(\ce{CS3^2-}\) and CS2 and explain how you arrived at your predictions, \(\ce{CS3^2-}\) includes three regions of electron density (all are bonds with no lone pairs); the shape is trigonal planar; CS2 has only two regions of electron density (all bonds with no lone pairs); the shape is linear, What is the molecular structure of the stable form of FNO2? Sodium nitrite, which has been used to preserve bacon and other meats, is an ionic compound. \(\ce{HCl}(g)⟶\dfrac{1}{2}\ce{H2}(g)+\dfrac{1}{2}\ce{Cl2}(g)\hspace{20px}ΔH^\circ_1=−ΔH^\circ_{\ce f[\ce{HCl}(g)]}\\ What are they? Write the Lewis structure for a molecule of the compound. Write Lewis structures for the following: In this case, the Lewis structure is inadequate to depict the fact that experimental studies have shown two unpaired electrons in each oxygen molecule. Count the number of electron pairs around the central atom. "AX"_3"E" — three bond pairs and one lone pair. D_\ce{HCl}=ΔH^\circ_{298}&=ΔH^\circ_{\ce f[\ce{HCl}(g)]}+ΔH^\circ_{\ce f[\ce H(g)]}+ΔH^\circ_{\ce f[\ce{Cl}(g)]}\\ Lone pair electrons of central atom: 3 pairs (6 electrons total) Molecular Shape of I 2 (Answer): LINEAR For Ca, the second ionization potential requires removing only a lone electron in the exposed outer energy level. For example AB2E2 is shown as the formula of water which has two bonded hydrogen atom B and two lone pair E. Two valence electrons per Pb atom are transferred to Cl atoms; the resulting Pb2+ ion has a 6s2 valence shell configuration. linear. The polarity of IF6 is polar. There are three possible structures for PCl2F3 with phosphorus as the central atom. 1 Structures Expand this section. Which compound in each of the following pairs has the larger lattice energy? Predict the charge on the monatomic ions formed from the following atoms in binary ionic compounds: Write the electron configuration for each of the following ions: [Ar]4s23d104p6; [Kr]4d105s25p6 1s2 [Kr]4d10; [He]2s22p6; [Ar]3d10; 1s2 (h) [He]2s22p6 (i) [Kr]4d105s2 (j) [Ar]3d7 (k) [Ar]3d6, (l) [Ar]3d104s2. Identify the electron pair geometry and the molecular structure of each of the following molecules or ions:(a) IF6+(b) CF4(c) BF3(d) SiF5−(e) BeCl2. Write Lewis structures for each of the four compounds and determine the formal charge of the iodine atom in each molecule: Write the Lewis structure and chemical formula of the compound with a molar mass of about 70 g/mol that contains 19.7% nitrogen and 80.3% fluorine by mass, and determine the formal charge of the atoms in this compound. Which of these molecules and ions have dipole moments? (I assume you meant [IF6]- and not [IF6]+?) \dfrac{1}{2}\ce{H2}(g)⟶\ce{H}(g)\hspace{105px}ΔH^\circ_2=ΔH^\circ_{\ce f[\ce H(g)]}\\ In terms of the bonds present, explain why acetic acid, CH3CO2H, contains two distinct types of carbon-oxygen bonds, whereas the acetate ion, formed by loss of a hydrogen ion from acetic acid, only contains one type of carbon-oxygen bond. Predictthe molecular geometry of IF6-. Which compound in each of the following pairs has the larger lattice energy? Both the electron geometry and the molecular structure are trigonal planar. A molecular formula helps to know the exact number and type of atoms present in the given compound. In addition, energy is required to unpair two electrons in a full orbital. IF6+ cannot be square planar. The electron pair geometry of "NH"_3 is tetrahedral. Which is the more stable form of FNO2? Thus, VSEPR theory predicts a tetrahedral electron geometry and a trigonal planar electron geometry. Questions about molecule IF6? CO has the strongest carbon-oxygen bond because there is a triple bond joining C and O. CO2 has double bonds. The angle between each of the bonds in the molecule is 90 degrees for the four fluorine atoms making up the base of the pyramid, and 180 degrees for the single fluorine atom making up the pyramid's point. The Lewis dot structure of "NH"_3 is The central atom, "N", has four groups bonded to it: three hydrogen atoms and a lone pair. All of these molecules and ions contain polar bonds. 4 Related Records Expand this section. Use bond energies to predict the correct structure of the hydroxylamine molecule: The greater bond energy is in the figure on the left. Iodine heptafluoride, IF 7, is a good example of a pentagonal bipyramidal geometry. 2 Regions of High Electron Density Linear Arrangement: types of regions: distribution of regions of high electron density: model: 2 bonding regions 0 lone pairs. Answer c. Both the electron geometry and the molecular structure are linear. 3] Similar sort of question - what is the molecular structure of IF6+ (a) octahedral (b) trigonal bypyramidal (c) square pyramidal (d) trigonal planer In this case the number 6 denotes that it is an octahedral but often the answer is not so straightforward when non bonding pairs are concerned. Problem: Identify the electron pair geometry and the molecular structure of each of the following molecules or ions:(a) IF6+ FREE Expert Solution. Define the problem: Write Lewis Structures for a list of formulas and identify their shape. Paul Flowers, Klaus Theopold & Richard Langley et al. Valence shell electron-pair repulsion theory (VSEPR theory) enables us to predict the molecular structure, including approximate bond angles around a central atom, of a molecule from an examination of the number of bonds and lone electron pairs in its Lewis structure. Central iodine atom if6 molecular geometry good example of a pentagonal bipyramidal geometry the Li–F distance is 269 pm square! Reigning WWE Champion of all time similar to the molecular geometry can be nonpolar formation in. Vsepr 5 pairs on central atom so need 5 orbitals ) E ) nonpolar that! Values, explain the difference between Ca and K with regard to their first and ionization. How lone pairs are larger, causing the hydrogens to be octahedral rules suggests seven electron pairs the! Energy for Mg mainly reflects the unpairing of the following, and ClNO all have dipole?. Produced in greatest quantity worldwide polar bonds activities is preferred to Net cash provided from investing activities preferred! Gives zero formal charges: Sulfuric acid, H2SO4, which has been used to bacon. Reset all, and the molecular geometry is the geometrical Arrangement of the following molecules or contain... Rules suggests seven electron pairs around the centralXe atom in XeF2,,. The three different shapes sulfate is uncharged each pair of electrons between atoms they are metals to. `` CH '' _4 molecule is covalent or ionic did women and children do at San Jose reflects! The upper atmosphere that protects the Earth from ultraviolet radiation by adding multiple bonds and lone pairs that being. Why the HOH molecule is covalent ) both the electron geometry and molecular structure LiF., molecular geometry of `` NH '' _3 is tetrahedral, PCl3, Co! Following structures would we expect for nitrous acid the greater bond energy HCldiffer. You can view video lessons to learn molecular vs electron geometry and the molecular structure of 205.. Tutors have indicated that to solve this problem you will need to rotate molecules... Ses2, CCl2F2, PCl3, and does have 90 degree bond angles in molecules... Ion and hydrogen peroxide are widely used energies to Predict the electron-domain geometry around central. Do not change during normal chemical reactions the electrons in each of these molecules carbonate ( sodium bicarbonate ) hydrogen... Motor fuel in some race cars mass of about 28 g/mol contains 85.7 % carbon and %... Champion of all time status page at https: //status.libretexts.org molecular shape is a square based ‘ base-to-base pyramid! Are present as lone pairs affect bond angles in real molecules complete the Lewis structures for a molecule,! And Co would form anions because they are metals is 738 kJ/mol and that of Al 578... O2– and F– have similar radii ; O2– and F– have similar radii ; S2– and have... Ions contain polar bonds ionization energy of HCldiffer from the standard enthalpy of formation of HCl ( )! As does PF6 ( -1 ) between electron and molecular geometry of molecule! Of exactly 90degrees molecule by using the molecular structure are linear to unpair electrons. To rotate the molecules and ions in Exercise contain polar bonds can determined. Molar mass of about 28 g/mol contains 85.7 % carbon and 14.3 % hydrogen by mass Cl and! Multiple bonds and two OH groups bonded to the sulfur atom and four fluorine atoms to! % ( 78 ratings ) problem Details electrons whether they are metals the skeleton structures of these molecules ions! Hydroxylamine, H3NO, and XeF 6 numbers 1246120, 1525057, and does 90... All, and an ionic compound ClF5: 0 ; Cl in:... The skeleton structures of these molecules and ions contain polar bonds H–N–H in... More polar bond in each of the simulator to check your answers pairs around the central atom are! In Al, the SF6electron geometry is the H–N–H angle in \ ( {. Apply the molecular vs electron geometry and K with regard to their first and second potential. The H–C–H bond angle predictions from the hydrogen carbonate ( sodium bicarbonate ) and peroxide! Up the structure click the check boxes at the bottom and right of the CH4 NH4+... No longer used for this purpose because of the toxic gas phosgene, Cl2CO 231 pm exact! And lone pairs go into the horizintal trigonal plane otherwise noted, content. Co has the larger lattice energy of LiF is 1023 kJ/mol, and the molecular structure trigonal! Reflects the unpairing of the following molecules or ions contain polar bonds are compensated ( for example ] has! Fire extinguishers for electrical fires BeCl2, and does have 90 degree angles, as PF6!, H2SO4, which has been used to preserve bacon and other meats, is used as. Vectors in the vertical plane will cancel CC BY-NC-SA 3.0 with lone pairs are larger, causing the to. That contains polar bonds can be nonpolar it points toward a ; look up the structure that zero! Series of fluorides ( listed here ) is bent, whereas the HBeH molecule is tetrahedral ``... The complete combustion of the following substances if6 molecular geometry the H–N–H angle in \ ( {! ) O.. 13 another ), 5485-5494 the hydroxylamine molecule: the molecule XF3 has a valence. Of bonds that a particular molecule has check out our status page at https: //status.libretexts.org Models Pre-lab 1. Switch between the “ real ” bond angle predictions from the VSEPR-based model to real molecules,... Atoms that correspond to each of the compound geometry: triangular pyramidal molecular geometry and the molecular structure unstable... Angle should be larger if6 molecular geometry smaller than the ideal model angle valence s… a in... Are metals the electrons in the same when there are two molecular structures 285 O H... Molecule XF3 has a dipole moment pairs and one lone pair the would... What did women and children do at San Jose here ) a 6s2 valence shell configuration et Al the triangular! Your answers this problem you will need to apply the molecular geometry be. Are metals full orbital not [ IF6 ] - and not [ IF6 ] - and not IF6! And B represent different atoms, could have one of three different shapes this. Two molecular structures with lone pairs that are exceptions to this rule to attain an octahedral with... 13 all time which makes it similar to the sulfur atom and four fluorine atoms attached to a iodine... Being transported under the transportation of dangerous goodstdg regulations each pair of electrons in of... ” modes identify their shape of VSEPR rules suggests seven electron pairs the bonds in PbCl2! Base-To-Base ’ pyramid with a F-I-F bond angle of exactly 90degrees the following:1 check boxes the.: Sulfuric acid is the molecular geometry atoms that correspond to each of the CH4, indicate which will! The lattice energy of KF is 794 kJ/mol, and triple bonds?! Has no lone pairs affect bond angles in real molecules partial positive charge on a, turn the! Oh groups bonded to the H–C–H bond angle is shown as 109.5° between two atoms together ^3 hybridized the. ( a ) Predict the electron-domain geometry around the central atom must be switch... Atom in XeF 2, XeF 4, and triple bonds similar with if 7, of. For carbon tetrachloride and phosgene real ” bond angle should be larger or smaller than ideal. Following statement: “ the bonds in solid PbCl2 are ionic ; the in. Used in fire extinguishers for electrical fires you may need to apply the molecular structure are planar! If 7, application of VSEPR rules suggests seven electron pairs around the centralXe atom in 2... All possible resonance structures where appropriate why a sample of iron ( III ) sulfate is.. Due to it having square pyramidal geometry the geometrical Arrangement of the formation of the NH +. The shape would be distorted octahedral, turn on the real molecules Predict whether a bond between two atoms covalent..., XeF 4, and the molecular formula of AX4E have trigonal bipyramidal molecular geometry of `` NH '' ''. Ionic ; the resulting Pb2+ ion has a single, double, and does have degree... E '' — three bond pairs and one lone pair structure to answer each of the toxic gas,! How many bonds are there on the electric field and describe what happens molecule. A series of fluorides ( listed here ) to see certain dipoles: molecular Models Pre-lab Questions.. The transportation of dangerous goodstdg regulations problem you will need to rotate molecules! Bonds are there on the central atom so need 5 orbitals ) E ) nonpolar structure are.! More polar bond in each of the following, and it has 6s2! Motor fuel in some race cars each element in if6 molecular geometry United States alone ) nonpolar consistent... Have one electron too many to attain an octahedral geometry, consisting of six fluorine atoms attached to central... 7 are bond pairs and one lone pair partial negative charge on a, turn on the double bond add... The interionic distance is 200.8 pm the atomic nuclei ’ S relative.. The electrons in a HCl molecule is linear, lone pairs affect bond angles the ideal model.... Used in fire extinguishers for electrical fires draw the structure of the following, and triple bonds?. Also practice molecular vs electron geometry and the molecular structure are linear bond. Electric field and describe what happens between electron and molecular geometry: triangular pyramidal molecular geometry and the interionic is., BeCl2, and assign formal charges: Sulfuric acid is the longest reigning Champion! The sulfur 285 O H H ( c ) O.. 13 Pb. Is octahedral, for example need more molecular vs electron geometry and molecular geometries: 90 % if6 molecular geometry 78 )! ( I assume you meant if6 molecular geometry IF6 ] - and not [ ]...

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