9 topics with a brief review: definitions, key facts, and classroom questions.
Chapter 13 is dedicated to the chemistry of metals, which play a key role in physiological processes and pharmaceutical analysis. In this section, we examine how their position in the periodic table determines the chemical behavior of s-, p-, and d-elements.
The material covers the chemical properties of alkali metals, magnesium, aluminum, and copper. Special attention is given to vital iron and the general characteristics of d-block metals. An applied medical topic—water hardness and chemical methods for its removal—is also discussed in detail.
Colloquia and exams most frequently test the redox properties of manganese and chromium compounds (especially their color changes depending on the pH of the medium), as well as reactions demonstrating the specific properties of iron. A solid understanding of these processes is the foundation for comprehending enzyme biochemistry, metabolism, and toxicology.
Why are alkali metals stored under a layer of kerosene?
To completely prevent their contact with moisture and atmospheric oxygen. Without a protective layer, they oxidize within seconds or may ignite.
Is magnesium classified as an alkaline earth metal?
No, it occupies an intermediate position between beryllium and the alkaline earth metals (calcium, strontium, barium, radium). Its hydroxide is a weak electrolyte.
Why cannot permanent hardness be eliminated by simple boiling?
Permanent hardness is caused by the presence of magnesium and calcium sulfates and chlorides. These compounds are thermally stable and do not decompose upon heating, so chemical precipitants such as sodium carbonate must be used to remove them.
Why does aluminum not react with pure water despite being located before hydrogen in the reactivity series?
The reason lies in the presence of an extremely thin, dense, and very durable aluminum oxide film on the metal's surface. It mechanically isolates the metal from water; if the film is removed with alkali, the reaction proceeds violently.
Why is copper often compared to alkali metals?
Copper subgroup atoms have one electron in their outer shell (ns¹ configuration), which superficially resembles alkali metals. The main difference lies in the structure of the ions: the copper cation has a fully filled 3d sublevel beneath its outer layer, which alkali metal ions lack.
Why do concentrated acids fail to dissolve iron under normal conditions?
Passivation occurs: a dense oxide film rapidly forms on the metal surface, protecting it from further oxidation. The reaction starts only upon heating.
Master the entire topic in the "Chemistry" course
This is a summary. The course covers everything tested in classes and exams.
3,009 pages of study guides for all topics
Assignments and quizzes after every topic — just like in a colloquium