四川大学无机化学答案 第1章 物质的聚集状态
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第1章 原子结构与元素周期律1-1在自然界中氢有三种同位素,氧也有三种同位素,问:总共有多少种含有不同核素的水分子?由于3H 太少,可忽略不计,问:不计3H 时天然水中共有多少种同位素异构水分子?解: 共有18种不同核素的水分子 共有9种不同核素的水分子1-2.答:出现两个峰1-3用质谱仪测得溴的两种天然同位素的相对原子质量和同位素丰度分别为 79Br 78。
9183 占 50。
54%,81Br 80。
9163 占 49。
46%,求溴的相对原子质量。
解:1-4铊的天然同位素203Tl 和205Tl 的核素质量分别为202.97u 和204。
97u ,已知铊的相对原子质量为204。
39,求铊的同位素丰度。
解: 设203Tl 的丰度为X ,205Tl 的丰度为1-X204。
39 = 202。
97X + 204.97(1-X) X= 29.00%1-5等质量的银制成氯化银和碘化银,测得质量比m (AgCl ):m(AgI )= 1:1。
63810,又测得银和氯的相对原子质量分别为107.868和35。
453,求碘的原子量.解: X= 126.911-8为什么有的元素原子量的有效数字的位数多达9位,而有的元素的原子量的有效数字的位数却少至3~4位?答:单核素元素只有一种同位素,因而它们的原子量十分准确。
而多核素元素原子量的准确性与它们同位素丰度的测量准确性有关(样品的来源、性质以及取样方式方法等)。
若同位素丰度涨落很大的元素,原子量就不可能取得很准确的数据.1—13.解:(1)r=c /λ=(3×108)/(633×10-9) = 4。
74×1014Hz 氦—氖激发是红光(2)r=c/λ=(3.0×108)/(435。
8×10-9) = 6。
88×1014Hz 汞灯发蓝光 (3)r=c/λ=(3.0×108)/(670.8×10—9) = 4.47×1014Hz 锂是紫红18)33(313131323=+⨯=⋅+⋅c c c c 9)21(313121322=+⨯=⋅+⋅c c c c 91.79%46.499163.80%54.509183.78)Br (=⨯+⨯=Ar X 107.86835.453107.86863810.11)AgI ()AgCl (++==m m1—14 Br 2分子分解为Br 原子需要的最低解离能为190kJ 。
无机化学基础习题参考答案《无机化学基础》习题解答第一章物质的量1、计算下列物质的摩尔质量。
(1)Fe (2)H2(3)HCl (4)HNO3(5)H2SO4(6)Al(OH)3(7)KOH (8)Ba(OH)2 (9)K2HPO4(10)NH4Cl (11)Cl—(12)PO43—解:物质的摩尔质量是以g/mol为单位,在数值上等于该物质的式量(分子量或原子量)。
所以以上物质的摩尔质量分别为:(1)mol (2)2 g/mol (3) g/mol (4)63 g/mol (5)98 g/mol (6)84 g/mol (7)56 g/mol (8)171 g/mol (9)174 g/mol (10) g/mol (11) g/mol (12)95 g/mol。
2、计算下列物质的物质的质量。
(1)90g H2O (2)22g CO2(3)Fe3O4(4)200gCaCO3解:H2O、CO2、Fe3O4、CaCO3的摩尔质量M分别为:18 g/mol、44 g/mol、232 g/mol、100 g/mol。
根据公式:n = m / M,计算得出以上物质的量分别为:(1)5 mol (2)mol (3)mol (4)2 mol。
3、计算下列物质的质量。
(1)2molNaHCO3(2)(3)3molCaCl2 (4)解:NaHCO3、AgNO3、CaCl2、Na2SO4的摩尔质量M分别为:84 g/mol、170 g/mol、111 g/mol、142 g/mol。
根据公式:m = n*M ,计算得出以上物质的质量分别为:(1)168 g (2)255g (3)333 g (4)71 g4、请写出下列反应中各物质的“物质的量”之比。
(1)2Na + 2H2O = 2NaOH + H2↑(2)Fe + H2SO4 = FeSO4 + H2↑(3)Cl2 + 2KBr = 2KCl + Br2(4)Fe2O3 + 6HCl = 2FeCl3 + 3H2O(5)Acl3 + 3NaOH = Al(OH)3↓+ 3NaCl(6)Na2CO3 + 2HCl = 2NaCl + H2O + CO2↑解:根据反应中各物质的“物质的量”之比等于反应中各物质前的系数之比。
大学无机化学试题及答案Document serial number【NL89WT-NY98YT-NC8CB-NNUUT-NUT108】第一章 一些基本概念和定律本章总目标:1:学习物质的聚集状态分气态、固态、液态三种,以及用来表示这三种聚集态的相关概念。
2;重点掌握理想气体状态方程、道尔顿分压定律以及拉乌尔定律。
各小节目标 第一节:气体1:了解理想气体的概念,学习理想气体的状态方程推导实际气体状态方程的方法。
2:掌握理想气体状态方程的各个物理量的单位及相关的计算。
理想气体:忽略气体分子的自身体积,将分子看成是有质量的几何点;假设分子间没有相互吸引,分子之间及分子与器璧之间发生的碰撞时完全弹性的,不造成动能损失。
3:掌握Dalton 分压定律的内容及计算。
第二节:液体和溶液1:掌握溶液浓度的四种表示方法及计算 ○1物质的量浓度(符号:Bc 单位1mol L -•):溶液中所含溶质B 的物质的量除以溶液的体积。
○2质量摩尔浓度(BB An b m =,单位:1mol kg -•):溶液中溶质B 的物质的量除以溶剂的质量。
○3质量分数(BB m m ω=):B 的质量与混合物的质量之比。
○4摩尔分数(B B nn χ=):溶液中溶质的物质的量与溶液的总物质的量之比。
2:了解非电解质稀溶液的依数性及其应用。
第三节:固体1:了解常见的四种晶体类型2:掌握四类晶体的结构特征及对物质性质的影响,比较其熔沸点差异。
Ⅱ习题一选择题:1.如果某水合盐的蒸汽压低于相同温度下的蒸汽压,则这种盐可能发生的现象是() (《无机化学例题与习题》吉大版)A.气泡B.分化C.潮解D.不受大气组成影响2.严格的讲,只有在一定的条件下,气体状态方程式才是正确的,这时的气体称为理想气体。
这条件是()A.气体为分子见的化学反应忽略不计B.各气体的分压和气体分子本身的体积忽略不计C.各气体分子的“物质的量”和气体分子间的引力忽略不计D.各气体分子间的引力,气体分子的体积忽略不计3.在300K,把电解水得到的并经干燥的H2和O2的混合气体40.0克,通入60.0L的真空容器中,H2和O2的分压比为():1 :1 C.1:1 :14.在下述条件中,能使实际气体接近理想的是()A.低温、高压B.高温、低压C.低温、低压D.高温、高压5.某未知气体样品为5.0克,在温度为1000C时,压力为291KPa时体积是0.86L,该气体的摩尔质量是()A.42g/molB.52g/molC.62g/molD.72g/mol6.处于室温一密闭容器内有水及与水相平衡的水蒸气。
第一章物质的聚集状态§1~1基本概念一、物质的聚集状态1.定义:指物质在一定条件下存在的物理状态。
2.分类:气态(g)、液态(l)、固态(s)、等离子态。
等离子态:气体在高温或电磁场的作用下,其组成的原子就会电离成带电的离子和自由电子,因其所带电荷符号相反,而电荷数相等,故称为等离子态,(也称物质第四态)特点:①气态:无一定形状、无一定体积,具有无限膨胀性、无限渗混性和压缩性。
②液态:无一定形状,但有一定体积,具有流动性、扩散性,可压缩性不大。
③固态:有一定形状和体积,基本无扩散性,可压缩性很小。
二、体系与环境1.定义:①体系:我们所研究的对象(物质和空间)叫体系。
②环境:体系以外的其他物质和空间叫环境。
2.分类:从体系与环境的关系来看,体系可分为①敞开体系:体系与环境之间,既有物质交换,又有能量交换时称敞开体系。
②封闭体系:体系与环境之间,没有物质交换,只有能量交换时称封闭体系。
③孤立体系:体系与环境之间,既无物质交换,又无能量交换时称孤立体系。
三、相体系中物理性质和化学性质相同,并且完全均匀的部分叫相。
1.单相:由一个相组成的体系叫单相。
多相:由两个或两个以上相组成的体系叫多相。
单相不一定是一种物质,多相不一定是多种物质。
在一定条件下,相之间可相互转变。
单相反应:在单相体系中发生的化学反应叫单相反应。
多相反应:在多相体系中发生的化学反应叫多相反应。
2.多相体系的特征:相与相之间有界面,越过界面性质就会突变。
需明确的是:①气体:只有一相,不管有多少种气体都能混成均匀一体。
②液体:有一相,也有两相,甚至三相。
只要互不相溶,就会独立成相。
③固相:纯物质和合金类的金属固熔体作为一相,其他类的相数等于物质种数。
§1~2 气体定律一、理想气体状态方程PV=nRT国际单位制:R=1.0133*105Pa*22.4*10-3 m 3/1mol*273.15K=8.314(Pa.m3.K-1.mol-1)1. (理想)气体状态方程式的使用条件温度不太低、压力不太大。
大学化学教材1、大学化学/普通高等教育“十一五”国家级规划教材2、大学化学教程——高等学校教材3、新大学化学(第二版)4、大学化学——面向21世纪课程教材5、化学功能材料概论——高等学校教材6、新编普通化学/21世纪高等院校教材7、大学基础化学/高等学校教材8、大学化学9、大学化学10、大学普通化学(第六版)11、大学化学教程——21世纪高等院校教材12、大学化学13、化学实验教程——高等学校教材14、大学化学(高等学校教学用书)15、大学化学原理及应用(上下)/高等学校教材16、大学化学教程/高等学校教材17、大学基础化学/新世纪高职高专教材18、新大学化学19、大学化学原理及应用·上下册20、普通化学(英文版)21、近代高分子科学22、绿色化学与环境23、普通化学简明教程24、大学化学(第二版)——高等学校教材1、大学化学/普通高等教育“十一五”国家级规划教材•作者:金继红主编•丛书名:•出版社:化学工业出版社•ISBN:9787502597221•出版时间:2007-1-1•版次:1•印次:1•页数:403•字数:679000•纸张:胶版纸•包装:平装•开本:16开•定价:39 元当当价:30.6 元折扣:78折节省:8.40元钻石vip价:30.60 元••共有顾客评论0条内容提要本书为普通高等教育“十一五”国家级规划教材。
本书在编写过程中注意与中学化学的衔接,力求理论联系实际,概念阐述准确,深入浅出,循序渐进,便于教师教学和学生自学。
本书包括物质的聚集状态、热力学第一定律、热力学第二定律、相平衡、化学平衡、水溶液中的离子平衡(含酸碱滴定、重量分析)、氧化还原和电化学基础(含氧化—还原滴定)、原子结构、分子结构、晶体结构、配位化合物(含配位滴定)、单质和无机化合物、表面与胶体、环境化学及材料化学等内容。
本书可供高等学校非化学化工类专业对化学要求较多的材料、地质、能源、环境、冶金、海洋等专业的基础化学教学使用。
无机化学(第四版)答案第一章物质的结构1-1 在自然界中氢有三种同位素,氧也有三种同位素,问:总共有种含不同核素的水分子?由于3H太少,可以忽略不计,问:不计3H时天然水中共有多少种同位素异构水分子?1-2 天然氟是单核素(19F)元素,而天然碳有两种稳定同位素(12C和13C),在质谱仪中,每一质量数的微粒出现一个峰,氢预言在质谱仪中能出现几个相应于CF4+的峰?1-3 用质谱仪测得溴得两种天然同位素的相对原子质量和同位素丰度分别为79Br 789183占50。
54%,81Br 80。
9163占49。
46%,求溴的相对原子质量(原子量)。
1-4 铊的天然同位素203Tl和205Tl的核素质量分别为202。
97u和204。
97u,已知铊的相对原子质量(原子量)为204。
39,求铊的同位素丰度。
1-5 等质量的银制成氯化银和碘化银,测得质量比m(AgCl):m(AgBr)=1。
63810:1,又测得银和氯得相对原子质量(原子量)分别为107。
868和35。
453,求碘得相对原子质量(原子量)。
1-6 表1-1中贝采里乌斯1826年测得的铂原子量与现代测定的铂的相对原子质量(原子量)相比,有多大差别?1-7 设全球有50亿人,设每人每秒数2个金原子,需要多少年全球的人才能数完1mol金原子(1年按365天计)?1-8 试讨论,为什么有的元素的相对质量(原子量)的有效数字的位数多达9位,而有的元素的相对原子质量(原子量)的有效数字却少至3~4位?1-9 太阳系,例如地球,存在周期表所有稳定元素,而太阳却只开始发生氢燃烧,该核反应的产物只有氢,应怎样理解这个事实?1-10 中国古代哲学家认为,宇宙万物起源于一种叫“元气”的物质,“元气生阴阳,阴阳生万物”,请对比元素诞生说与这种古代哲学。
1-11 “金木水火土”是中国古代的元素论,至今仍有许多人对它们的“相生相克”深信不疑。
与化学元素论相比,它出发点最致命的错误是什么?1-12 请用计算机编一个小程序,按1.3式计算氢光谱各谱系的谱线的波长(本练习为开放式习题,并不需要所有学生都会做)。
第1章 化学反应中的质量关系和能量关系 习题参考答案1.解:1.00吨氨气可制取2.47吨硝酸。
2.解:氯气质量为2.9×103g 。
3.解:一瓶氧气可用天数33111-1222()(13.210-1.0110)kPa 32L9.6d 101.325kPa 400L d n p p V n p V -⨯⨯⨯===⨯⨯4.解:pV MpVT nR mR== = 318 K 44.9=℃ 5.解:根据道尔顿分压定律ii n p p n=p (N 2) = 7.6⨯104 Pap (O 2) = 2.0⨯104 Pa p (Ar) =1⨯103 Pa6.解:(1)2(CO )n = 0.114mol; 2(CO )p = 42.87 10 Pa ⨯(2)222(N )(O )(CO )p p p p =--43.7910Pa =⨯ (3)4224(O )(CO ) 2.6710Pa 0.2869.3310Pan p n p ⨯===⨯7.解:(1)p (H 2) =95.43 kPa (2)m (H 2) =pVMRT= 0.194 g 8.解:(1)ξ = 5.0 mol(2)ξ = 2.5 mol结论: 反应进度(ξ)的值与选用反应式中的哪个物质的量的变化来进行计算无关,但与反应式的写法有关。
9.解:∆U = Q p - p ∆V = 0.771 kJ 10.解: (1)V 1 = 38.3⨯10-3 m 3= 38.3L(2) T 2 =nRpV 2= 320 K (3)-W = - (-p ∆V ) = -502 J (4) ∆U = Q + W = -758 J (5) ∆H = Q p = -1260 J11.解:NH 3(g) +45O 2(g) 298.15K−−−−→标准态NO(g) + 23H 2O(g) m r H ∆= - 226.2 kJ·mol -1 12.解:m r H ∆= Q p = -89.5 kJ m r U ∆= m r H ∆- ∆nRT= -96.9 kJ13.解:(1)C (s) + O 2 (g) → CO 2 (g)m r H ∆ =m f H ∆(CO 2, g) = -393.509 kJ·mol -121CO 2(g) + 21C(s) → CO(g) m r H ∆ = 86.229 kJ·mol -1CO(g) +31Fe 2O 3(s) → 32Fe(s) + CO 2(g)m r H ∆ = -8.3 kJ·mol -1各反应m r H ∆之和m r H ∆= -315.6 kJ·mol -1。
1、教材《无机化学》北京师范大学、华中师范大学、南京师范大学无机化学教研室编,高等教育出版社,2002年8月第4版。
2、参考书《无机化学》北京师范大学、华中师范大学、南京师范大学无机化学教研室编,高等教育出版社,1992年5月第3版。
《无机化学》邵学俊等编,武汉大学出版社,2003年4月第2版。
《无机化学》武汉大学、吉林大学等校编,高等教育出版社,1994年4月第3版。
《无机化学例题与习题》徐家宁等编,高等教育出版社,2000年7月第1版。
《无机化学习题精解》竺际舜主编,科学出版社,2001年9月第1版《无机化学》电子教案绪论(2学时)第一章原子结构和元素周期系(8学时)第二章分子结构(8学时)第三章晶体结构(4学时)第四章配合物(4学时)第五章化学热力学基础(8学时)第六章化学平衡常数(4学时)第七章化学动力学基础(6学时)第八章水溶液(4学时)第九章酸碱平衡(6学时)第十章沉淀溶解平衡(4学时)第十一章电化学基础(8学时)第十二章配位平衡(4学时)第十三章氢和稀有气体(2学时)第十四章卤素(6学时)第十五章氧族元素(5学时)第十六章氮、磷、砷(5学时)第十七章碳、硅、硼(6学时)第十八章非金属元素小结(4学时)第十九章金属通论(2学时)第二十章s区元素(4学时)第二十一章p区金属(4学时)第二十二章ds区元素(6学时)第二十三章d区元素(一)第四周期d区元素(6学时)第二十四章d区元素(二)第五、六周期d区金属(4学时)第二十五章核化学(2学时)1 .化学的研究对象什么是化学?●化学是研究物质的组成、结构、性质与变化的一门自然科学。
(太宽泛)●化学研究的是化学物质(chemicals) 。
●化学研究分子的组成、结构、性质与变化。
●化学是研究分子层次以及以超分子为代表的分子以上层次的化学物质的组成、结构、性质和变化的科学。
●化学是一门研究分子和超分子层次的化学物种的组成、结构、性质和变化的自然科学。
大一无机化学课本答案Chapter one problem solvingSolution: because the pressure of the gas is not too high and the temperature is not too low, it can be regarded as an ideal gas.Because, PM = rho-r-t, the same gas, mass M doesn,t change.2.Solution:So the molecular mass is 163.Solution: (1)2.So the relative mass is 30The molecular formula is C2H6.4.Solution:5.Solution: in 35 °C, and reason: So, in the same condition, you compress it to 250mLThe answer is: In 313 k. So,;So there,s air in composition, T, n, so V is equal to P1V1 / P empty = 7. 79 L, V is equal to 7. 79 LBecause in the process of air flow, each bubble is alwayssaturated with CHC13 steam, so it's always 49. 3 kPa. Its volumeis 7. 79 L. So the ideal gas equation for CHC13 is:.7.theThe quality score of the impurity is zeroIt is.Solution: suppose that a mixture of IL H20 and 560L NH3 is soluble in water..Its mass is 1, 000 grams of water, so the volume of this ammonia solution is,It is.9. Solution:In this case, the simplest form is:.(2),So,・This is the molecular formula11. Answer: because CaC12 and NaCl electrolyte, CH3C00H for weak electrolytes, C6H1206 as the electrolyte, the solution of the concentration of the solute (particle) size in the order: CaC12 > NaCl > CH3COOH > C6H1206, so high and low order to freezing point C6H12O6 > CH3COOH > NaCl > CaC12.Answer: so,Let's say I take this solution, 1,000 grams, and I have oneAnswer: 14.In the sum of the formula,No, because it's too small to be accurateA: because of the Ag + overdose, the preparation of the Agl aerosol tape is positive, so it is the anion that makes up the glue. So the ability to get together is the order of magnitude K3 [Fe (CN).B: because of the I - excess, the prepared Agl sol tape is negatively charged. Therefore, it is the cation that makes the coagulation of the glue. So the ability to get together is in the order of A1C13 > MgS04.Chapter ii problem solvingAnswer: (1)2.2. Answer:(1), so there is.(2)the initial pressure is,The volume of the intermediate state is zero(3)answer: because, therefore,(constant pressure is)Answer: because the reaction is available⑷(1)-215-296.8 + (-1) (-100)二-411.8Material - 412.-219-296.8 + (-1) (-100)二-416.8Material - 417.(2)(3) (4)... So you can look it up in the same wayAnswer: the reaction equation is:It is.8.Answer:Answer: 1, 2, 3, 5, 4, 6Answer: (because of the reduced gas component)(because of the increase in the gas component)(because the gas component increases)(because of the reduced gas component)(because the gas component increases)11. Answer:(1)because the melting is an isothermal constant pressure reversible process, so there is,(2)because gasification is a reversible process such as isothermal pressure, so there isIt is.Solution: because melting and boiling are both isothermal and isostatic equilibrium processes, so there areAnswer: because boiling is an isothermal constant pressurereversible process, so there is,The equilibrium state of freedom is equal to zeroIt is possible to make a mistake by mistake, mistake, mistake, mistake.Answer: the high temperature spontaneously.The lower temperature is spontaneous.At any temperature, it's spontaneous.18. Answer:So, the reaction is never going to happen spontaneously.Answer: reaction20.Answer:So it's higher than 111221.Answer: (1),so, not spontaneous at 25 °C reaction.(2), so, in 360 °C can occur spontaneously.3.Chapter iii problem solving(2)(3)⑷2.Solution:A fG - 394.4-16.5-228.6-228. 6A rG = 1 x (394. 4) + (2) x (16. 5), (228. 6) and (197. 15) = 1.65 KJ, mol, 1A rG = - RTln3,Equilibrium time n over moles 0.021 0.004 0. 0040. 025 * 0. 16 二0. 164HBr (g) + 02 (g)= 2H20 (g) + 2 Br2 (g)(1)the rate equation for the reaction is zeroFrom the experimental data analysis:So the rate equation for this reaction is zero(1)the rate equation for the experimental data is: (3)Because the reaction is slow (v is small) and the time is short,it can be assumed that the reaction is approximately constant within the interval, so 12 is produced7.According toIn the case of milk, the rate at which the acid reacts is directly proportional to the rate constant of different temperatures, namelyReaction 2 so2 (g) + 02 (g) = 2 S03 (g) heat effectAccording to theThere areThe watch can calculate the reactionSo, balance moves to the left.Or:18.(1)decrease; (2); (3) increase; (4) : (5) : (6):(7); (8); (9); (10); (12) remains the same.(1)PC15 (g)二PC13 (g) + C12 (g)The initial mole number is 2, 0, 0Balance the number of moles 0. 5, 1. 5, 1. 5The concentration of each component in equilibrium is: (2)when set to balance, the decomposition PC15 is x moles. PC15 (g)二PC13 (g) + C12 (g)The initial number of moles is 2, 0, 1. 0Balance the number of moles 2. 0 minus x, x, x, and x22.The initial Mohr is 0. 2 0. 2 0The initial Mohr is 0. 2 minus x 0. 2 minus x 2x12 pyrolysis rate for25. Solution:Chapter 5. Problem setsA. 2A. 3A. 4A. 5A. 6A. 7"EightA. 1 3.A. 2A. 3A. 4The change in the number of 1, 1, 2, 1, 3, 4, 1, 3, 4, 1, 3, 4, 1, 3, 4, 1, 3, 4(1)battery reaction:(2)battery reaction: AgCl (S) + e = + Cl -(3)electrode response:(4)negative poles:The positive:Electromotive force:Original battery reaction:8. 1 negative:The positive:Electromotive forceCell response:2 negative:The positive:Electromotive force:Battery reaction: Ce4 + Fe2 + + + Ce3 +Negative 3:2H + + 2e 二H2The positive pole: Cr2072 - + + 6e = 2Cr3 + + 7H20 Electromotive force VThe battery reaction is: Cr2072 - + + + + 3112Question 15: (1)(2)positive pole: negative pole:(3)battery reaction:⑷(5)in a solution, it decreases, causing the electromotive force to rise. If you add ammonia to the solution, it's going to go down,It's causing the electric force to go down.Problem 22: positive and negativeCell response:So there areBecause it can be thought of as the anode and composition of the battery:Chapter 6 answers the atomic structure2. (1)By calculation, the volatility of the macro object is so small that it can be ignored.6. (1) reasonable(2)unreasonable. Because L can,t be equal to n, L < n and > 二o integer.(3).⑷.(5)unreasonable. Because L = 0(6)it's not reasonable because L can,t be greater than nThe seven electrons of the atom are arranged in ones22s22pxl2pyxl2pyxl2pzlTherefore, its quantum combination is 1S2 (1, 0, 0, 1/2) (1, 0, 0, -1/2).2S2 (2, 0, 0, 1/2) (2, 0, 0, -1/2)2P3 (2, 0, 1/2) (2, 1, 1, 1/2) (2, 1, 1, 1/2) (1, 1, 1, 1/2) (1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1, 1,Or 2, 1, 0, minus 1/2, 2, 1, minus 1/2, 2, 1, minus 1, minus 1/2. 9.Na: 1 s22s22p63slThe IS electron valid nuclear charge = 11 -= 11-0. 30 1 = 10. 702S electrons = 11 - = 11 -= 11-2 0. 85-7 0. 35 二6. 85 (2S2P is thesame group)3 3S electrons 二11 - 二11 -二11-8 0. 85-2 1 二2. 2 (2S2P is the same group)For multi-electron atoms, when the main quantum number n = 4, there are four energy levels, namely 4S, 4P, 4D and 4f. They correspond to the number of orbitals, 1, 3, 5, 7. The maximum number of electrons you can hold is 2n2 二242 - 32 - 2 (1 + 3 + 5 + 7)For hydrogen, the E4s, >, E3d because it's a single electron system, energy levels are only related to the number of quantum Numbers.In the case of K, because of the drilling effect and shielding effect, there is an energy level crossing, its E3d > E4s2S [Ar] 3d54S2[Xe] 4fl45dlO6Sl, 4f145dl06S26P613. (1) errors Because of the Angle of the atomic orbital part of the graphical representation is the electron distribution outside the nucleus different spatial orientation of risk, not represent the actual movement of the electrons.(2)the error in the N shell (principle quantum number 二4) thereare 4 s, 4 p, 4 d, 4 f, a total of four energy level, the corresponding 1 hc-positie atomic orbital is a total of 16, of the principal quantum number N = 1, only Ils, can accommodate two opposite spin electronics.(3)correct because the hydrogen atom is a single electronic system, there is no interleaving phenomenon.(4)error because hydrogen is a single electronic system withoutthe shielding of electrons.Cu2 + [Ar] 3dl + [Ar] 3d5Pb2 + [Xe] 4fl45dlO6S2 - [Ne] 3S23P6(1) 24 (2) [Ar] 3d54sl (3) 3d54sl(4)the fourth period; VI. B; Cr03When n > 4, it's the Ens < E (n - 1) dSo when you complete the ns and np orbitals, the rest of the electrons are going to have to fill in the E (n + 1) s orbital.So you can,t fill the outer layer with d electrons, so you can only have up to eight electrons in the outer layer of the atomic orbital. Similarly, due to the Ens < E f (n - 2), while the electrons tofill after the (n - 1) d orbitals, will give priority to fill inthe E (n + 1) s not enter E (n + 1) f orbit, so the time could notfill f electrons in the outer, therefore, the atomic orbital can more than 18 times on the outer electrons.(1) A B C is A metalIt is possible to infer their valence structure from the set up conditions:A: 4S1, Z = 19 potassium; B: 4S2. Z = 20C: 3dl04s2, Z = 30 zinc; D: 4S24P5, Z = 35 bromo(2) D A +, Br - and K +(3)AOH is the strongest(4)BD2 is the ionic compound of CaBr221.The eighth cycle element is the most available number of electrons in the eighth level group, which is8S25gl86f147dl08p6, 50 electrons, so there are 50 elements in the eighth cycle.The electronic structure of the element is [118] 8S25gl (the atomic number of the seventh cycle of a rare gas), so the atomic number of the element is 121. (note: E5g > E8s cannot be determined by n + 0.7 L)The atomic electron layer of element 100 is [Rn] 7S25f 146dl07p2So this element is the fourth period of the seventh cycleSc > Ca: The Sr < Ba; K > AgFe2 + > Fe3 +; Pb > Pb2 +; S < S2 -0 < N. Al < Ag; The Sr > RbCu < Zn: Cs < Au; Br < KrBecause the valence electron configuration of a rare gas is ns2np6, which is an 8 electron stable structure, it is very difficult to lose electrons, so it has very high ionization energy.Because the valence electron configuration of P is 3S23P3, and S is 3S23P4, the former 3P orbital is semi-filled and stable, so it is not easy to lose electrons, so the ionization energy is high.Because of the electronegativity of 0, the repulsive force of the electron is so large that it is not easy to gain electrons, so it emits energy, so the electron affinity can be S > 0Because N is more electronegative than C, and the valence electron configuration of N is 2S22P3 electrons in half full structure, not easily gaining electrons, so the affinity energy is N < C.The largest element of the atomic radius is Fr, and the smallestis ILThe largest of the ionization energy is He; The minimum is FrThe biggest negative is F; The smallest is FrThe maximum of the electron affinity is ClChapter 7 problem solving the molecular structure3.(the octahedron)3.P150In the BF3 molecule, the valence electron of B is 2S22P1 2S22P12Pyl to form the triangle SP2 hybridized orbital (plane triangle) BF3 plane triangular molecule.NF3: the valence electron of N is 2S22P3. 3 NF3 molecules of the SP3 hybridized cone.5.BBr3 central atom B: SP2 isotropism; The molecular configuration is a plane triangle.SiH4 center atom Si: SP3 hybridized orbital, tetrahedronPH3 center atom P: SP3 hybridized orbital, triconeSeF6 center atom Se: d2sp3 hybridization, positive octahedron.The nucleus of CS2. Valence electron configuration: linearThe geometry of the molecule is linear.Central atom N: electron log;Valence electron configuration: the geometric configuration of a plane triangle ion is the Angle.The central atom Cl, the valence electron log;Valence electron configuration: regular tetrahedron; The configuration is linear.Central ions; The valence electrons;Valence electron configuration: trig double cone; The geometric configuration is linear.Central atom N; The valence electrons;Valence electron pair configurations: flat triangles; The geometric configuration is a plane triangleCenter atom Br; The valence electrons:Valence electron configuration: trig double cone: The geometric configuration of the molecule is 〃T〃.Center atom P; The valence electrons;Valence electron configuration: regular tetrahedron; Ion geometry: the tetrahedronCenter atom Br; The valence electrons;Valence shell electron pair configuration: positive octahedron; The geometry of the ions is the plane squareCenter atom P; Valence shell electron log;Valence shell electron pair configuration: delta double cone; Geometry of the molecules: trig and double conesCentral atom Br; The valence electrons;Valence shell electron pair configuration: positive octahedron; Molecular geometry: quadrilateral conesCentral atom: The valence electrons;Valence shell electron pair configuration: positive octahedron;The geometric configuration of ions: the octahedronNonpolar molecules; Although the c~h bond is polar, the polarity of the bond is just offset by the fact that the space is tetrahedral.Polar molecules. Because the c~h and c-cl are different, though the molecules are symmetric and tetrahedral, the polarity of the bond cannot cancel out.Non-polar molecules; The molecule is a flat triangle, symmetric structure, and the polarity of the b-cl bond cancels out.Polar molecules. The molecules are triangular and asymmetrical, and the polarity of the n-cl bond cannot be offset.Polar molecules. The molecules are 〃V〃, asymmetrical, and the polarity of the h-s bond cannot be canceled out.Non-polar molecules; The molecules are linear, symmetric, and thepolar offset of c-s bonds.01 (for non-polar molecules, u = 0, for polar molecules)Both of them are non-polar molecules, u 二0.(both of these are polar molecules, but because of the electronegativity of N, the positive and negative charge on the n~h in the numerator is more open.)BF3 is a non-polar molecule, u 二0, and NF3 is a polar molecule.(both of these are polar molecules, but because of the electronegativity of 0, the electrons on the h-o in the moleculeare larger, and the center of the negative charge is more open.)13. NaF > NaCl > NaBr > Nal. SiI4 > SiBr4 > SiC14 > SiF414. A. because Ge4 + 1 charge is very big, has strong ability of polarization and combined with its large volume, strong deformation, thus has a strong covalent compounds from the molecular, and K + polarization force is very good, so for the ionic crystals; The melting point is higher for the covalent molecular crystal.A. 2Since the Zn2 + has a 18e configuration, it is better than the 8e configurational Ca2 + polarization, which makes the covalent bond in the crystal more numerous, so the melting point is lower than that.Because Fe3 + is more polarizing than Fe2 +, it makes the crystal communist party more valuable, so the melting point is lower.A. 1 error 15. For polyatomic molecule, the key of the polarity and molecular polarity is not consistent, although bonds have polarity, but molecules for the symmetric structure, the polarity can be offset each other, the possibility of non-polar molecules, such as, etc.A. 2 error Because of Mn (VII) polarization is far greater than Mn (II), which makes for covalent compound, and MnO for ionic compounds, so the melting point is lower than MnO.A. 3 error Because the dispersion force is caused is the instantaneous dipole, it exists between all molecules, and the most molecules of the main molecular inter-atomic forces.A. 4 error Because one of the three electronic key electronic is single, so the key is smaller than 2 electronic key bond energy, (note only for and comparison, if it's big keys will not necessarily)Benzene and both are non-polar molecules, so they only have a dispersion force between them.Methanol and water: there is dispersion force, orientation force, induction force and hydrogen bonding.The dispersion force and the inductive force are present.Because both are polar molecules, there is a force of orientation,inducement, and dispersion.You can form hydrogen bonds on your own.18. Melting point is greater than, because the former, and intermolecular hydrogen bond between form associated molecules, leading to higher melting point, while the latter is only formed intramolecular hydrogen bonding (according to the hydrogen bonding of saturated, after forming intramolecular hydrogen bond, no longer form intermolecular hydrogen bond), won,t form associated molecules, the boiling point will not rise significantly. So the melting point of the former is greater than the latter.There is a hydrogen bond between the three NH3 and the > PH3 The molecular weight of PH3 < SbH3 is smaller than SbH3 and small in dispersionAlthough the molecular weight is similar, the dispersive force is similar, but because it is a polar molecule, there is theorientation force and the inductive force.Both of them are ionic crystals, but because of the high charge,the ionic bond is strong.Because it's an atomic crystal, it's a molecular crystal.Because of the polarization force, only the covalent bonds are large.。
第1章 物质的聚集状态
1-1
答:理想气体状态方程适合于高温低压的条件,只有在高温低压条件下,气体分子间距离大,气体所占的体积远大于分子本身体积,使得分子间作用力和分子本身的体积可以忽略不计时,实际气体的存在状态才接近理想气体。
实际气体的Van der Waals 方程是考虑了实际气体分子自身体积和分子间作用力,对压强和体积进行了修正。
1-2
答:当压强接近0Pa 时,气体接近理想气体状态,故可用m 01=lim(p P R V T
→)或0lim()P M RT P
ρ→=来计算R 和M ,如果压强不趋近于0,则要用实际气体的状态方程式。
1-3
答:某组分B 的分体积定义为混合气体中某组分B 单独存在并且同混合气体的温度和压强相同时所具有的体积V B 。
分体积定律:当温度压力相同时,混合气体的总体积等于各组分分体积之和。
组分B 的体积分数与其摩尔分数是数值上相等的关系。
1-4答:
(1). 错,在压强一定时才成立。
(2). 错,在标准状态下,一摩尔气体的体积才是22.4L 。
(3). 对。
(4). 错,根据理想气体的状态方程式,组分的压强温度体积中两者确定时它的状
态才确定,所以一者发生变化另一者不一定发生变化。
1-5
答:饱和蒸气压是指蒸发出的分子数和进入液体的分子数相等时达到平衡状态时蒸气的压强。
压强反应的是单位面积处的气体的压力,所以蒸气压液体上方的空间大小无关,由于温度越高,逸出的分子越高速度越快,所以温度会影响蒸气压的大小。
实际上饱和蒸气压是液体的重要性质,它仅与液体的本质和温度有关。
1-6
答:晶体与非晶体的基本区别是组成晶体的质点排列是否有规律,质点排列有规律为晶体,无规律为非晶体。
晶体可以分为金属晶体、离子晶体、分子晶体和原子晶体几种类型。
物理特性:由于不同晶体质点间的作用力强度不同,共价键>离子键>分子间作用力(金属键的强度不确定,但一般都比分子间作用力强),所以晶体的熔点沸点硬度一般是原子晶体>离子晶体>金属晶体>分子晶体,导电性主要是金属晶体,但离子晶体在一定条件下也可以导电。
1-7说明:理想气体状态方程的基本应用。
解:273.15K 、p θ
下,pV nRT = 33110V m -=⨯,32.8610m kg -=⨯,
64.1r mRT M pV
==;35704.4/r pM g m RT ρ== 1-8
解:(1)已知1202p kPa =,10.500V L =,1273T K =。
在标准状况下,2273T K =,2101p kPa =。
N 一定,T 不变时,1122pV p V =,则11222020.500 1.00101p V kPa L V L p kPa ⨯=
== 该气体的密度ρ14.107 4.111.00m g g L V L
-===⋅ (2)该气体的摩尔质量121 4.1078.31427392.32020.500
mRT M g mol p V -⨯⨯===⋅⨯ 该气体化合物的相对分子质量92.0r M =。
也可以先根据pV nRT =求n ,再根据n=m/M 求M 。
在该化合物分子中92.030.5%(N) 2.0014.0N ⨯==,92.0(130.5%)(O) 4.0016.0
N ⨯-==所以该氮氧化物的分子式为24N O
1-9
解:混合气体状态改变时,物质的量没有改变,因而:
111222//PV T PV T =()(),
2202/3001014V V T ⨯=⨯()() 则 T 2=600(K )
(2)由于225.0/2.0/75/20.2 3.37H Ne n n ==:()()
则222/ 3.37202/3.371156H H H Ne P Pn n n KPa =+=⨯+=()()()()()
1-10
解:解:(1) 降低压力,水蒸气分压相应减小,小于蒸气压,不会液化,适用Boyle 定律
1122pV p V =,故2112/ 2.00 L V pV p ==
(2)升高温度,水的蒸气压增大,分压小于蒸气压,全部为气体,适用Gay-Lussac 定律2121/ 1.13 L V VT T ==
1-11
解:此种气体的摩尔质量为46g/mol
通空气前后,其气体体积变化看忽略不记,故
pV nRT =则330.03358.314273 1.65101046
p Pa -⨯⨯==⨯⨯ 1-12
解:根据分压定律,同温同压下,气体所占体积正比于物质的量,22222H O H O +=,完全反应的氢气与氧气之比为2:1,所以(1)11:4(2)8:7
1-13
解:(1)无液体出现。
反应生成200mlH 2O (g ),余100mlH 2(g ),故根据分压
定律,反应后各组分2222::H O H H O H p p V V =,所以267.53H O p kPa =,233.77H p kPa =
(2)
1-14
解:2322(s)2(s)3O (g)MnO KClO KCl −−−→+
100g 3KClO 完全分解生成2O ,323360249
KClO o KClO m n mol M =⨯= 295.0 2.33392.667O p kPa kPa kPa =-=
由pV nRT =得
22232.2o O O n RT V L p ==,2222
0.81H O
H O O O p V V L p ==
2233.01H O O V V V L =+=
(2)干燥氧气222
32.2o O O n RT
V L p ==
1-15
解: 根据分压定律,当T,p一定时,气体的体积与物质的量成正比, 即∝Vn,由已知可知气体的体积相同,故O2An=n,即
0.480.06
32/A
g g mol M =
解得4/mol A M g =,所以A 气体的相对分子质量为4。
根据气体扩散定律,气体的扩散速度与其相对分子质量的平方根成反比,即
2A o u u =
2 2.83A
o u u ==
即A 气体的扩散速度是氧气的2.83倍,由已知可得A 气体扩散用的时间为100352.83s
s =。