Complex coMPOUNDS

Содержание

1. Complex coMPOUNDS
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4. compounds, which include complex ions, existing in
5. Structure of complex compounds In
6. Oppositely charged ions or neutral molecules called ligands are coordinated around the central ion.
7. The complexing agent and ligands form inner
8. The total number of coordinate bonds formed
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10. Nomenclature of complex compoundsNames of complex compounds
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12. [Cu(NH3)4]Cl2 – tetraammine copper(II) chloride; K2 [Cu(OH)4] – potassium tetrahydroxocupprate(II); [Cr(NH3)3Cl3] – trichloro triammine chromium(III).
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14. Classification of complex compoundsThere are several types of classification of complex compounds.
15. Classification of complex compounds1. Depending upon a charge
16. 22) Depending upon the type of the ligand:(i) Aqua-complexes
17. б)Гидроксокомплексы – это комплексные анионы, в которых лигандами
18. Depending upon the nature of a central ion: complexes of copper, silver, iron, chrome etc.
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21. Isomerism
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30. Electronic structure of
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34. Возможны октаэдрические комплексы:внутриорбитальные (d2sp3);внешнеорбитальные (sp3d2);
35. Электронное строения атома кобальта:
36. Entering of lone electronic pairs
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38. 2. Если лиганды
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compounds, which include complex ions, existing in the crystal, and in solution, called the complex or coordination compounds

Слайды и текст этой презентации

Слайд 1Complex coMPOUNDS

Слайд 4compounds, which include complex ions, existing in the crystal, and

in solution, called the complex or coordination compounds

compounds, which include complex ions, existing in the crystal, and in solution, called the complex or coordination

Слайд 5 Structure of complex compounds
In a molecule of a

complex compound, one of the atoms, generally positively charged, occupies

the central site (central ion or complexing agent).

Structure of complex compounds In a molecule of a complex compound, one of the atoms,

Слайд 6Oppositely charged ions or neutral molecules called ligands are coordinated

around the central ion.

Слайд 7The complexing agent and ligands form inner sphere of a

complex compound. It is characterized by coordinate bonds which are

formed while overlapping of empty p- and d-orbitals of a central ion and orbitals containing lone electron pairs of ligands. The ions in the outer sphere are mainly bonded to the complex ions by forces of electrostatic interaction (ionic bonds).

The complexing agent and ligands form inner sphere of a complex compound. It is characterized by coordinate

Слайд 8The total number of coordinate bonds formed by the complexing

agent is known as coordination number of the central ion.

It mainly depends upon the charge of the complexing agent (for monocharged ions it usually equals 1, for discharged ions – 4 or 6, for tricharged – 6 and above), and the size of an ion (the larger the central ion, the greater its coordination number is, for lanthanides and actinides it can reach to 12).

The total number of coordinate bonds formed by the complexing agent is known as coordination number of

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Слайд 10Nomenclature of complex compounds
Names of complex compounds are similar to

the names of simple salts. The order of naiming particles

in a complex ion is the following: anionic ligands – neutral ligands – central ion. Number of ligands is designated with the help of greek numerals

Nomenclature of complex compoundsNames of complex compounds are similar to the names of simple salts. The order

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Слайд 12[Cu(NH3)4]Cl2 – tetraammine copper(II) chloride;
K2 [Cu(OH)4] – potassium tetrahydroxocupprate(II);

[Cr(NH3)3Cl3] – trichloro triammine chromium(III).

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Слайд 14Classification of complex compounds
There are several types of classification of

complex compounds.

Слайд 15Classification of complex compounds
1. Depending upon a charge of the inner

sphere:
(i) Cationic complexes (the inner sphere is positively charged – complex

cations). Examples: [Cr(H2O)6]Cl3, [Co(NH3)6]Cl3.
(ii) Anionic complexes (the inner sphere is negatively charged – complex anions). Examples: K2[HgI4], Na[Sb(OH)6].
(iii) Neutral complexes (the inner sphere is not charged). Examples: [Pt(NH3)2Cl2], [Fe(CO)5].

Classification of complex compounds1. Depending upon a charge of the inner sphere:(i) Cationic complexes (the inner sphere is positively

Слайд 1622) Depending upon the type of the ligand:
(i) Aqua-complexes (ligands are water

molecules – [Cu(H2O)5]SO4).
(ii) Ammino-complexes (ligands are molecules of ammonia or organic

ammines – [Ag(NH3)2]Cl).
(iii) Hydroxy-complexes (ligands are OH– anions – Na2[Sn(OH)4]).
(iv) Carbonyl-complexes (ligands are molecules of carbon monoxide – [Fe(CO)5]).
(v) Acido-complexes (ligands are anions of inorganic acids). Examples: chlorocomplexes K2[HgCl4], fluorocomplexes K3[FeF6], cyanocomplexes KFe[Fe(CN)6], thiocyanocomplexes K3[Fe(SCN)6], sulphitocomplexes K[Ag(SO3)], etc.

22) Depending upon the type of the ligand:(i) Aqua-complexes (ligands are water molecules – [Cu(H2O)5]SO4).(ii) Ammino-complexes (ligands are molecules of

Слайд 17б)Гидроксокомплексы – это комплексные анионы, в которых лигандами являются гидроксид-ионы OH–.

Комплексообразователями являются металлы, склонные к проявлению амфотерных свойств – Be, Zn,

Al, Cr.
Например: Na[Al(OH)4], Ba[Zn(OH)4].
в) Аммиакаты – это комплексные катионы, в которых лигандами являются молекулы NH3. Комплексообразователями являются d-элементы.
Например: [Cu(NH3)4]SO4, [Ag(NH3)2]Cl.

б)Гидроксокомплексы – это комплексные анионы, в которых лигандами являются гидроксид-ионы OH–. Комплексообразователями являются металлы, склонные к проявлению амфотерных

Слайд 18Depending upon the nature of a central ion: complexes of

copper, silver, iron, chrome etc.

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Слайд 21Isomerism

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Слайд 30 Electronic structure of complex ions Interaction of

lone electronic pairs of ligands with empty valence orbitals of

the central ion of different types leads to their hybridization. For example, the electronic structure of a complex ion [Cu(NH3)4]2+ can be reflected as following:

Electronic structure of complex ions Interaction of lone electronic pairs of ligands with

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Слайд 34Возможны октаэдрические комплексы:
внутриорбитальные (d2sp3);
внешнеорбитальные (sp3d2);

Слайд 35Электронное строения атома кобальта:

При образовании

иона Со3+ освобождается 4s-орбиталь, а на 3d-орбитали остается 6 валентных

электронов:
Со3+

Лиганды – 6 молекул NH3 предоставляют на связь с комплексообразователем 6 неподеленных электронных пар (НЭП).

Электронное строения атома кобальта: При образовании иона Со3+ освобождается 4s-орбиталь, а на 3d-орбитали

Слайд 36 Entering of lone electronic pairs of ligands into

valence orbitals of the central ion leads to their interaction

with the electrons of 3d-orbitals. This interaction is defined by degree of penetration of electrons of ligands on empty orbitals of metallic cations. In connection of force of interaction, ligands may be arranged in a spectrochemical series and are devided into ligands of weak and strong field:

Entering of lone electronic pairs of ligands into valence orbitals of the central ion leads

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Все валентные

электроны спарены. Комплекс [Co(NH3)6]3+ - диамагнитный, что согласуется с экспериментом.

Все валентные электроны спарены. Комплекс [Co(NH3)6]3+ - диамагнитный, что

Слайд 38 2. Если лиганды недостаточно активны и

спаривания электронов на внутренних d-орбиталях не происходит, то в гибридизации

участвуют внешние d-орбитали (sp3d2):
F– - создает слабое поле

Четыре электрона иона кобальта неспарены, комплекс - парамагнитен.

2. Если лиганды недостаточно активны и спаривания электронов на внутренних d-орбиталях не происходит,

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