下载文档原格式
![[co(nh3)6]br3配合物的名称](https://img.taocdn.com/s1/m/c89ff2ef2dc58bd63186bceb19e8b8f67d1cef70.png)
[co(nh3)6]br3配合物的名称配位化合物的命名配体的种类很多，必须有统一的名称。
最常见的配体列在下面F－氟Cl－氯OH－羟CN－氰O2－氧 O22－过氧根SO42－硫酸根 N3－叠氮NO2－硝基ONO－亚硝酸根-SCN- 硫氰根-NCS－异硫氰根C6H5 －苯基py （）吡啶en 乙二胺Ph3P 三苯基膦NO 亚硝酰CO 羰基H2O 水NH3 氨（O2）双氧1.配位化合物内外界之间的连缀词在配位化合物中，先阴离子，后阳离子。
[ Co（NH3）5 H2O ] Cl3三氯化五氨•水合钴（III）Cu2 [ SiF6 ]六氟合硅（IV）酸亚铜阴阳离子之间加”化” 字或“ 酸”字，配阴离子看成是酸根。
[ Co（NH3）5 H2O ] Cl3三氯化五氨•水合钴（III）Cu2 [ SiF6 ]六氟合硅（IV）酸亚铜1.配位单元在配位单元中，先配体后中心，配体与中心之间加”合”字。
[ Co（NH3）5 H2O ] Cl3三氯化五氨•水合钴（III）Cu2 [ SiF6 ]六氟合硅（IV）酸亚铜配体前面用二、三、四· · ·[ Co（NH3）5 H2O ] Cl3三氯化五氨•水合钴（III）Cu2 [ SiF6 ]六氟合硅（IV）酸亚铜[ Co（NH3）5 H2O ] Cl3三氯化五氨•水合钴（III）Cu2 [ SiF6 ]六氟合硅（IV）酸亚铜几种不同的配体之间加“ • ”隔开。
[ Co（NH3）5 H2O ] Cl3三氯化五氨•水合钴（III）Cu2 [ SiF6 ]六氟合硅（IV）酸亚铜中心后面加（），内写罗马数字表示中心的化合价。
1.配体的先后顺序在配位单元中，可能涉及多种配体，所以要明确规定命名时配体的次序。
下述的每条规定均以其前一条规定为基础。
① 先无机配体后有机配体。
[ PtCl（2 Ph3P）2 ]二氯•二（三苯基膦）合铂（II）② 先阴离子类配体，后阳离子类配体，最后分子类配体。
高中化学奥林匹克竞赛辅导配合物（配位化合物）化学基础【竞赛要求】配位键。
常见的配合物的中心离子（原子）和常见的配体（水、羟离子、卤离子、拟卤离子、氨分子、酸根离子、不饱和烃等）。
螯合物及螯合效应。
常见的络合剂及常见的配合反应。
定性说明配合反应与酸碱反应、沉淀反应、氧化还原反应的联系。
配合物几何构型和异构现象的基本概念。
配合物的杂化轨道理论。
八面体配合物的晶体场理论。
Ti(H2O)6的颜色。
路易斯酸碱的概念。
1.配合物：由中心离子（或原子）和几个配体分子（或离子）以配位键相结合而形成的复杂分子络合物。
如[Co(NH3)6]3+、[Cr(CN)6]3–、Ni(CO)4都是配位单元，分别称作配阳离子、配阴离子、配分子。
判断物质是配合物的关键在于物质是否含有配位单元。
配合物和复盐的区别：前者一定含有配位键，后者没有配位键，如KCl·MgCl2·6H2O是复盐，不是配合物。
2.配合物的组成：为外界，内外界（1）配合物的内界和外界：以[Cu(NH3)4]SO4为例，[Cu(NH3)4]2+为内界，SO-24之间是完全电离的。
内界是配位单元，外界是简单离子。
又如K3[Cr(CN)6]之中，内界是[Cr(CN)6]3–，外界是K+。
配合物可以无外界，但不能没有内界，如Ni(CO)4。
（2）中心离子（原子）和配位体：a.中心离子（原子）：又称配合物的形成体或中心体，多为过渡金属离子，如Fe3+、Fe2+、Co2+、Ni2+、Cu2+，也有电中性的原子为配合物的中心原子，如Ni(CO)4、Fe(CO)5中的Ni和Fe都是电中性的原子。
只要能提供接纳孤对电子的空轨道的离子或原子均可作中心体。
b.配位体：含有孤对电子的阴离子或分子。
如NH3、Cl—、CN—等。
配位体中直接同中心原子配合的原子，叫做配位原子。
如[Cu(NH3)4]2+配阳离子中，NH3是配位体，其中N原于是配位原子。
配位原子经常是含有孤对电子的原子。
配合物eu(no3)3(phen)2的晶体结构和性质
EU(NO3)3(PHEN)2是一种均一的配合物，它是铕（Eu）三氧化物和酚（PHEN）二酸盐的组合。
颜色介于深紫色和棕色之间，熔点为350℃。
它的晶体结构主要是由Eu3+和NO3-组成的网格结构，而这些网格结构内部嵌入了phend伴随物质。
此外，EU(NO3)3(PHEN)2有三个主要的物理性质：板条状，磁性和荧光。
由于PHEN和Eu3+之间存在强烈的依赖性，对于PHEN伴随物质而言，EU(NO3)3(PHEN)2具有板条状的晶体结构，它的晶胞的孔径较大，从而可以将PHEN伴随物质固定住，从而使PHEN伴随物质较小。
此外，EU(NO3)3(PHEN)2具有可以被外部磁场诱导的磁性，它的磁性特征主要由Eu3+元素贡献，但是当较低的外部磁场磁化作用下，PHEN伴随部分也受到磁场的影响而形成磁性结构。
最后， EU(NO3)3(PHEN)2也具有荧光性质，它在紫外线照射下发出微弱的绿色荧光，这是Eu3+元素受到电子跃迁而产生的绿色荧光。
总之，EU(NO3)3(PHEN)2是一种晶体结构稳定且性质多样的配合物，具有板条性，磁性，以及荧光性等卓越的特征，因此，它被广泛用于化学分析，催化，催化剂的研究和应用，荧光成像等领域。
教专题专题 4 分子空间结构与物质性质学单元第二单元配合物的形成和应用课节题第一课时配合物的形成题知识与技能〔1〕了解人类对配合物结构认识的历史〔2〕知道简单配合物的根本组成和形成条件教〔3〕了解配合物的结构与性质及其应用学过程与方法通过配位键作为配离子化学构型，构筑配合物结构平台的方目法逐渐深入地理解配合物的结构与性质之间的关系标情感态度通过学生认识配合物在生产生活和科学研究方面的广泛应与价值观用体会配位化学在现代科学中的重要地位，从而激发学生进一步深入地研究化学。
教学重点配合物结构和性质，配合物形成条件和过程实验解释教学难点配合物结构和性质，配合物形成条件和过程实验解释教学方法探究讲练结合教学准备教师主导活动学生主体活动[复习 ]教 1.以下微粒中同时有离子键和配位键的是4B、NaOH 3+D、MgOA、NH Cl C、H O学3+是H2O和+结合而成的微粒，其化学键属于P692. H O HA、配位键B、离子键C、氢键D、范德华力讨论后口答过[知识回忆 ]1.配位键2.杂化和杂化轨道类型程[导入 ]实验 1：硫酸铜中逐滴参加浓氨水实验 2：氯化铜、硝酸铜中逐滴参加浓氨水实验分析：[知识梳理 ]一、配合物的形成1、配合物： 由提供孤 子 的配体与接受孤 子 的中 察心原子以配位 合形成的化合物称 配位化合物 称 配合物。
理解 教 主 活 学生主体活2、配合物的 成从溶液中析出配合物 ， 配离子 常与 有相反 荷的其他离子合成 ， 称 配 。
配 的 成可以划分 内界和外界。
配离子属于内界， 配离子以外的其他离子属于外界。
内、外界之 以离子 合。
外界离子所 荷 数等于配离子的 荷数。
〔1〕中心原子：通常是 渡金属元素〔离子和原子〕 ，少数是非金属元素，例如： Cu 2+，Ag +，Fe 3+，Fe ，Ni ，B Ⅲ，P Ⅴ⋯⋯〔2〕配位体： 含孤 子 的分子和离子。
如：－ ，OH －， CN －，H 2 ，3 ， CO ⋯⋯ I O NH配位原子： 配位体中具有孤 子 的原子。
A coordination complex is a substance in which a metal atom or ion accepts electrons from (and thus associates with) a group of neutral molecules or anions called ligands.A complex can be an anion, a cation ion, or a neutral molecule. Coordination compounds are neutral substances (i.e. uncharged) in which at least one ion is present as a complex. You will learn more about coordination compounds in the lab lectures for experiment 5 in this course.The coordination compounds are named in the following way.A. When naming coordination compounds, always name the cation before the anion. This rule holds regardless of whether the complex ion is the cation or the anion. (This is just like naming an ionic compound.)B. In naming the complex ion:1. Name the ligands first, in alphabetical order, and then name the central metal. Note: In the chemical formula the central metal is written before the ligands.2. The names of some common ligands are listed in Table 1.·Anionic ligands end in "-o." For anions that end in "-ide"(e.g. chloride, hydroxide), "-ate" (e.g. sulfate, nitrate), and "-ite" (e.g. nirite), change the endings as follows:-ide → -o; e.g., chloride → chloro and hydroxide → hydroxo-ate → -ato; e.g., sulfate → sulfato and nitrate → nitrato-ite → -ito; e.g., nitrite → nitrito·For neutral ligands, the common name of the molecule is used (e.g.H2NCH2CH2NH2 (ethylenediamine)). Important exceptions: water is called ‘aqua’, ammonia is called ‘ammine’, carbon monoxide is called‘carbonyl’, and the N2 and O2 m olecules are called ‘dinitrogen’ and‘dioxygen’.Table 1. Names of Some Common Ligands3. The Greek prefixes di-, tri-, tetra-, etc. are used to designate the number of each type of ligand in the complex ion. If the ligand already contains a Greek prefix (e.g. ethylene di amine) or if it is a polydentate ligand (i.e. it can attach at more than one coordination site), the prefixes bis-, tris-, tetrakis-, and pentakis- are used instead. (See examples 3 and4.) The numerical prefixes are listed in Table 2.Table 2. Numerical Prefixes4. After naming the ligands, name the central metal. If the complex ion isa cation, the metal is named same as the element. For example, Co in a complex cation is called cobalt and Pt is called platinum. (See examples 1-4.) If the complex ion is an anion, the name of the metal ends with the suffix -ate. (See examples 5 and 6.) For example, Co in a complex anion is called cobaltate and Pt is called platinate. For some metals, the Latin names are used in the complex anions (e.g. Fe is called ferrate and not ironate).Table 3: Name of Metals in Anionic Complexes5. Following the name of the metal, the oxidation state of the metal in the complex is given as a Roman numeral in parentheses.C. To name a neutral complex molecule, follow the rules of naming a complex cation. Remember: Name the (possibly complex) cation BEFORE the (possibly complex) anion. See examples 7 and 8.For historic reasons, some coordination compounds are called by their common names. For example: Fe(CN)63- and Fe(CN)64- are named ferricyanide and ferrocyanide respectively, and Fe(CO)5 is called iron carbonyl.Examples:Give the systematic names for the following coordination compounds: 1. [Cr(NH3)3(H2O)3]Cl3Answer: triamminetriaquachromium(III) chlorideSolution:· The complex ion is found inside the parentheses. In this case, the complex ion is a cation.· The ammine ligands are named first because alphabetically, "ammine" comes before "aqua."· The compound is electrically neutral and thus has an overall charge of zero. Since there are three chlorides associated with one complex ion and each chloride has a –1 charge, the charge on the complex ion must be +3.· From the charge on the complex ion and the charge on the ligands, we can calculate the oxidation number of the metal. In this example, all the ligands are neutral molecules. Therefore, the oxidation number of chromium must be the same as the charge of the complex ion, +3.2. [Pt(NH3)5Cl]Br3Answer: pentaamminechloroplatinum(IV) bromideSolution:· The complex ion is a cation, and the counter anions are the 3 bromides.· The charge of the complex ion must be +3 since it is associated with 3 bromides.· The NH3 molecules are neutral while the chloride carries a - 1 charge.· Therefore, the oxidation number of platinum must be +4.3. [Pt(H2NCH2CH2NH2)2Cl2]Cl2Answer: dichlorobis(ethylenediamine)platinum(IV) chloride Solution:· Since Ethylenediamine is a bidentate ligand, the prefix bis- is used instead of the prefix di-.4. [Co(H2NCH2CH2NH2)3]2(SO4)3Answer: tris(ethylenediamine)cobalt(III) sulfateSolution:· The sulfate has a charge of –2 and is the counter anion in this molecule.· Since it takes 3 sulfates to bond with two complex cations, the charge on each complex cation must be +3.· Since ethylenediamine is a neutral molecule, the oxidation number of cobalt in the complex ion must be +3.· Again, remember that you never have to indicate the number of cations and anions in the name of an ionic compound.5. K4[Fe(CN)6]Answer: potassium hexacyanoferrate(II)Solution:· Potassium is the cation, and the complex ion is the anion.· Since there are 4 K+ associated with the complex ion (each K+ having a +1 charge), the charge on the complex ion must be - 4.·Since each ligand carries –1 charge, the oxidation number of Fe must be +2.·The common name of this compound is potassium ferrocyanide.6. Na2[NiCl4]Answer: sodium tetrachloronickelate(II)Solution:· The complex ion is the anion so we have to add the suffix –ate to the name of the metal.7. Pt(NH3)2Cl4Answer: diamminetetrachloroplatinum(IV)Solution:· This is a neutral molecule because the charge on Pt+4 equals the negative charges on the four chloro ligands.· If the compound is [Pt(NH3)2Cl2]Cl2, even though the number of ions and atoms in the molecule are identical to the example, it should be named: diamminedichloroplatinum(IV) chloride because the platinum in the latter compound is only four coordinated instead of six coordinated.8. Fe(CO)5Answer: pentacarbonyliron(0)Solution:· Since it is a neutral complex, it is named in the same way as a complex cation. The common name of this compound, iron carbonyl, is used more often.9. (NH4)2[Ni(C2O4)2(H2O)2]Answer: ammonium diaquabis(oxalato)nickelate(II)Solution: The oxalate ion is a bidentate ligand.10. [Ag(NH3)2][Ag(CN)2]Answer: diamminesilver(I) dicyanoargentate(I)You can have a compound where both the cation and the anion are complex ions. Notice how the name of the metal differs even though they are the same metal ions.Can you give the molecular formulas of the following coordination compounds?1. hexaammineiron(III) nitrate2. ammonium tetrachlorocuprate(II)3. sodium monochloropentacyanoferrate(III)4. potassium hexafluorocobaltate(III)Can you give the name of the following coordination compounds?5. [CoBr(NH3)5]SO46. [Fe(NH3)6][Cr(CN)6]7. [Co(SO4)(NH3)5]+8. [Fe(OH)(H2O)5]2+Answers:1. [Fe(NH3)6](NO3)32. (NH4)2[CuCl4]3. Na3[FeCl(CN)5]4. K3[CoF6]5. pentaamminebromocobalt(III) sulfate6. hexaammineiron(III) hexacyanochromate (III)7. pentaamminesulfatocobalt(III) ion8. pentaaquahydroxoiron(III) ion。
