cesium phosphide compound formula

During the 1920s and 1930s, Charles Kingsford Smith used separate buoyant canisters of calcium carbide and calcium phosphide as naval flares lasting up to ten minutes. { "5.01:_Sugar_and_Salt" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.02:_Compounds_Display_Constant_Composition" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.03:_Chemical_Formulas_-_How_to_Represent_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.04:_A_Molecular_View_of_Elements_and_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.05:_Writing_Formulas_for_Ionic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5.06:_Nomenclature-_Naming_Compounds" : "property get [Map 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https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FIntroductory_Chemistry%2FIntroductory_Chemistry%2F05%253A_Molecules_and_Compounds%2F5.05%253A_Writing_Formulas_for_Ionic_Compounds, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), Example \(\PageIndex{1}\): Aluminum Nitride and Lithium Oxide, Example \(\PageIndex{2}\): The Crisscross Method for Lead (IV) Oxide, Example \(\PageIndex{3}\): Sulfur Compound, Example \(\PageIndex{4}\): Calcium Nitrate, 5.4: A Molecular View of Elements and Compounds, Writing Formulas for Ionic Compounds Containing Polyatomic Ions. Two examples are shown below: There are two ways to recognize ionic compounds. what is the correct name for the polyatomic ion IO3- and its conjugate acid HIO3? [4], Calcium phosphide is a common impurity in calcium carbide, which may cause the resulting phosphine-contaminated acetylene to ignite spontaneously.[5]. Do Eric benet and Lisa bonet have a child together? Hg (NO2)2, what is the correct formula for the ionic compound : aluminum nitride. For each of the following compounds, state whether it is ionic or covalent. The formula for lithium bromide is \(\ce{LiBr}\). -ide is just the negative anion of that element, chloride, sulfide, nitride. The rules for organic compounds, in which carbon is the principle element, will be treated in a later chapter on organic chemistry. What is the chemical formula for Cesium Phosphide? Cesium (or Caesium) (atomic symbol: Ce, atomic number: 55) is a Block S, Group 1, Period 6 element with an atomic weight of 132.9054519. If more than one of a particular polyatomic ion is needed to balance the charge, the entire formula for the polyatomic ion must be enclosed in parentheses, and the numerical subscript is placed outside the parentheses. Phosphorus is a highly-reactive non-metallic element (sometimes considered a metalloid) with two primary allotropes, white phosphorus and red phosphorus its black flaky appearance is similar to graphitic carbon. Transpose only the number of the positive charge to become the subscript of the anion and the number only of the negative charge to become the subscript of the cation. Only one ion of each is needed to balance these charges. For each pair of elements, determine the charge for their ions and write the proper formula for the resulting ionic compound between them. This activity includes every compound formula and name that can be formed from the list 44 Ions provided in Chemistry A at Pickerington High School Central. A B; Lithium Fluoride: LiF: Lithium Chloride: LiCl: Lithium Bromide . An alternative way to writing a correct formula for an ionic compound is to use the crisscross method. The amount of hydrogen phosphate ions\(\ce{HPO4^{2}}\) and \(\ce{H2PO4^{}}\)in seawater is very low, but they are present in higher amounts in blood, where they also affect acid-base properties. Which of the following is the correct ionic charge for gallium (Ga) in ionic compounds? A B; Lithium Nitrite: LiNO 2: Lithium Nitrate: LiNO 3: Lithium Hydrogen Sulfate: LiHSO 4: Lithium Hydroxide: LiOH: . \(\ce{Al^{3+}} \: \: \: \: \: \ce{N^{3-}}\). You would need to know what oxidation state the metal is in first. Leave out all subscripts that are 1. Calcium phosphide (CP) is the inorganic compound with the formula Ca3P2. If there is only 1 of the polyatomic ion, leave off parentheses. Several examples are found in Table 3.3.1. Most atoms and molecules in nature tend to a state of neutrality, which guarantees stability. Finally, the proper formula for an ionic compound always has a net zero charge, meaning the total positive charge must equal the total negative charge. Legal. Be aware that ionic compounds are empirical formulas and so must be written as the lowest ratio of the ions. Identify each compound as ionic or not ionic. The remaining polyatomic anions, which all contain oxygen, in combination with another non-metal, exist as part of a series in which the number of oxygens within the polyatomic unit can vary. Carbon Monoxide CO Nitrogen Phosphide NP Hydrogen Chloride HCI, Calcium Oxide CaO, Sodium Nitride Na,N Bromine Iodide B Water H,0 Silver (II) Sulfide AgS Potassium Iodide KI, Sulfur Dioxide SO, 2. compounds: Lithium Phosphite, Vanadium (II) Sulfide, Aluminum Sulfite, Manganese (IV) Sulfate, Lead (IV) Nitride Strontium Phosphide, Calcium Nitrate, Silver (II) Nitrite, Beryllium Bicarbonate . 2. A single suffix, "-ide," is insufficient for distinguishing the names of the anions in a related polyatomic series. Direct link to css6's post How do you calculate a tr, Posted 5 years ago. Direct link to Matthew Nodar's post How do we know that Bromi, Posted 6 years ago. periodic table to confirm that it's likely that calcium Can you provide some information about the admission process of LPU for B.Sc in agriculture? The compound Eu 2 O 3 is neutral. When an ionic compound is formed from magnesium and oxygen, the magnesium ion has a 2+ charge, and the oxygen atom has a 2 charge. (f) Graph Compounds of these metals with nonmetals are named with the same method as compounds in the first category, except the charge of the metal ion is specified by a Roman numeral in parentheses after the name of the metal. The number of electrons in each of Cesium's shells is 2, 8, 18, 18, 8, 1 and its electron configuration is [Xe]6s1. Identify the element, X. Potassium can be the cation in the ionic compound X2O. Lesson 7: Valence electrons and ionic compounds. Use the method of half reactions to balance the following equations: Cu2+(aq)+S2O32(aq)Cu+(aq)+S4O62(aq)\mathrm{Cu}^{2+}(a q)+\mathrm{S}_2 \mathrm{O}_3^{2-}(a q) \rightarrow \mathrm{Cu}^{+}(a q)+\mathrm{S}_4 \mathrm{O}_6^{2-}(a q) write the correct form of the verb? the sp 3 hybrid orbital in CH4, has what shape? This will give the ionic compound an overall charge which both the iron cation and paired anion have to have their charges sum up to. And like always, if you are what is the suffix of the oxyanion? Cl- The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. First, compounds between metal and nonmetal elements are usually ionic. Im going back in a minute I need a little more help I have a lot to get to get to work but Im not sure what to say to. Start by writing the metal ion with its charge, followed by the nonmetal ion with its charge. PROBLEM. \(\ce{Pb^{4+}} \: \: \: \: \: \ce{O^{2-}}\). three cesium ions and one phosphide ion one cesium ion and three phosphide ions three cesium ions and three phosphide ions one cesium ion and one phosphide ion Paul Flowers (University of North Carolina - Pembroke),Klaus Theopold (University of Delaware) andRichard Langley (Stephen F. Austin State University) with contributing authors. Enhancement of radiation tolerance in GaAs/AlGaAs core-shell and InP nanowires. Some compounds contain polyatomic ions; the names of common polyatomic ions should be memorized. Compounds between metal and nonmetal elements are usually ionic. Metal phosphides are used as a rodenticide. Direct link to Ryan W's post -ide is just the negative, Posted 6 years ago. how many single covalent bonds do bromine, fluorine and the other halogens usually form? The formula \(\ce{Mg2Cl4}\) has balanced charges with the ions in a 1:2 ratio, but it is not the lowest whole number ratio. If the compound is ionic, does the metal form ions of only one type (fixed charge) or more than one type (variable charge)? And bromine only gets a -1 or a 1- charge, so you're gonna need two of the bromides for every one of the calciums. Write the chemical formula for the ionic compound formed by each pair of ions. The acid in the digestive system of the rodent reacts with the phosphide to generate the toxic gas phosphine. Because Cesium carbonate has a polyatomic ion (the group of non-metals after the metal) we'll need to use a table of names for common polyatomic ions, in addition to the Periodic Table. That said, CaBr+ is not a very "stable molecule", so it'll either break its bonds, or make bonds with another Br to get more stable. The remaining polyatomic ions are all negatively-charged and, therefore, are classified as anions. The formula contains a positive charge of 2 (+3) = +6 and a negative charge of 3 (-2) = -6, for a net charge of 0. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. Although it is convenient to think that \(\ce{NaCl}\) crystals are composed of individual \(\ce{NaCl}\) units, Figure \(\PageIndex{1}\) shows that no single ion is exclusively associated with any other single ion. Ionic Compounds - Names and Formulas. Sodium is a metal, and oxygen is a nonmetal. Cesium Phosphide: Cs 3 P: Cesium Arsenide: Cs 3 As: Cesium Oxide: Cs 2 O: Cesium Sulfide . (a) rubidium iodide (b) cesium phosphide (c) lithium sulfate (d) silver carbonate (e) zinc phosphate (f) aluminum nitrate. over here in Group Two, and Group Two elements, also This means we need 2 iron atom, and 3 oxygen atoms, or Fe2O3. and determine the formula given the name. The number of electrons in each of Phosphorus's shells is 2, 8, 5 and its electronic configuration is [Ne] 3s2 3p3. oxygen gains two electrons to form what kind of ion, elements with a full octet have which configuration, why are solid ionic compounds poor conductors of electricity, they have electrons that cannot flow freely, what is the electrostatic charge holding two ions together, the attraction of a metallic cation and delocalized electrons form what kind of bond, which property of metals allows them to be easily drawn into wires, is the force that holds two atoms together, a chemical combination of two or more different elements, the electrostatic force that holds oppositely charged particles together in an ionic compound, is the three dimensional geometric arrangement of particles, and is responsible for the structure of many minerals, an ion in aqueous solution that conducts electricity, the energy required to separate 1 mol of ions in an ionic compound, an element that is generally a gas or a dull, brittle, solid and is a poor conductor of heat and electricity, is a polyatomic ion composed of an element, bonded to one or more oxygen atoms, a characteristic of matter that can be observed or measured without altering the samples composition, is the attraction of an metallic cation for delocalized electrons, is a mixture of elements that has metallic properties, the chemical bond that results from sharing electrons, dots or a line are used to symbolize a single covalent bond, is formed when parallel orbitals overlap and share electrons, is one where a greater amount of energy is required to break a bond in reactants than is released when the new bonds form in the product, is one where more energy is released than is required to break the bonds in the initial reactants, is an acid that contains both a hydrogen atom and an oxyanion, model is used to determine molecular shape, electrons repel each other, uses letter symbols and bonds to show relative positions of atoms, is a condition that occurs when more than one valid lewis structure can be written for a molecule or ion, forms when one atom donates both of the electrons to be shared with an atom or ion that needs two electrons, is a process in which atomic orbitals mix and form new,identical hybrid orbitals, the relative ability of an atom to attract electrons in a chemical bond, the force between water molecule is what kind of intermolecular force, what kind of bond occurs within a molecule with unequal sharing of electron pairs, the lewis structure of this molecule would show zero unshared electrons (no lone pair) on the central atom, the lewis structure of this molecule would show four unshared electrons (two lone pairs) on the central atom, The lewis structure of this molecule would show two unshared electrons ( a lone pair) on the central atom. If so, does it also contain oxygen? Name the following ionic compounds, which contain a metal that can have more than one ionic charge: The anions in these compounds have a fixed negative charge (S2, Se2 , N3, Cl, and \(\ce{SO4^2-}\)), and the compounds must be neutral. in a _________ bond, the electrons are shared between the atoms bonded, located in orbitals that point at one another, parallel (i) in direction to the axis of the molecule itself. Write the correct formula unit for the ionic compound chromium (iv) oxide. Which of these is the correct name for the compound HOCl. the name of an oxyacid has the suffix -ic acid. Other examples are provided in Table \(\PageIndex{3}\). The chemical formula of nickel phosphide is Ni2P. Thus, this compound is also ionic. data-quail-id="56" data-mt-width="1071">. This formula merely indicates that sodium chloride is made of an equal number of sodium and chloride ions. Which is the correct ionic charge for aluminum (Al) in ionic compounds? Binary acids are named using the prefix hydro-, changing the ide suffix to ic, and adding acid; HCl is hydrochloric acid. Cu2+(aq)+S2O32(aq)Cu+(aq)+S4O62(aq). Rather than writing the formula as \(\ce{NaNaS}\), we shorten it by convention to \(\ce{Na2S}\). The way I understand it right now is that "ide" is from when there is two of an anion, "ite" is for three of an anion, and "ate" is for four of an anion. Sodium chloride is an ionic compound made up of sodium ions and chloride ions in a crystal lattice. Are the ions monatomic or polyatomic? sits in our periodic table, right over here, we see it is a halide. Both oxygen and fluorine are nonmetals. Which is the correct formula for the compound Manganese (II) Fluoride? Chemical Formula for Calcium Nitrite 9.2K views How to Write the Formula for Lead (II). Note that all of the polyatomic ions whose names end in "-ate" contain one more oxygen than those polyatomic anions whose names end in "-ite." Write the final formula. Examples include SF6, sulfur hexafluoride, and N2O4, dinitrogen tetroxide. { "4.01:_4.1-Types_of_Chemical_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.02:_Ions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.03:_Formulas_for_Ionic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.04:_Ionic_Nomenclature" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.05:_Transition_Metal_Ion_Formation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.06:_Formula_Mass" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.07:__Characteristics_of_Ionic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Matter_Measurements_and_Calculations" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Atoms_and_Molecules" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Electronic_Structure_and_the_Periodic_Law" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Chemical_Bond_I" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Chemical_Bond_II" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Intermolecular_Forces" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Overview_of_Inorganic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "hypothesis:yes", "showtoc:no", "license:ccbyncsa", "source[1]-chem-16137", "source[2]-chem-16137", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FBrevard_College%2FCHE_103_Principles_of_Chemistry_I%2F04%253A_Chemical_Bond_I%2F4.03%253A_Formulas_for_Ionic_Compounds, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\).