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  2. Reactivity (chemistry) - Wikipedia

    en.wikipedia.org/wiki/Reactivity_(chemistry)

    Both factors are actually distinct, and both commonly depend on temperature. For example, it is commonly asserted that the reactivity of alkali metals (Na, K, etc.) increases down the group in the periodic table, or that hydrogen's reactivity is evidenced by its reaction with oxygen. In fact, the rate of reaction of alkali metals (as evidenced ...

  3. Reactivity series - Wikipedia

    en.wikipedia.org/wiki/Reactivity_series

    The most reactive metals, such as sodium, will react with cold water to produce hydrogen and the metal hydroxide: 2 Na (s) + 2 H 2 O (l) →2 NaOH (aq) + H 2 (g) Metals in the middle of the reactivity series, such as iron , will react with acids such as sulfuric acid (but not water at normal temperatures) to give hydrogen and a metal salt ...

  4. Alkali metal - Wikipedia

    en.wikipedia.org/wiki/Alkali_metal

    When an alkali metal is dropped into water, it produces an explosion, of which there are two separate stages. The metal reacts with the water first, breaking the hydrogen bonds in the water and producing hydrogen gas; this takes place faster for the more reactive heavier alkali metals. Second, the heat generated by the first part of the ...

  5. Salt (chemistry) - Wikipedia

    en.wikipedia.org/wiki/Salt_(chemistry)

    In some reactions between highly reactive metals (usually from Group 1 or Group 2) and highly electronegative halogen gases, or water, the atoms can be ionized by electron transfer, [16] a process thermodynamically understood using the Born–Haber cycle. [17] Salts are formed by salt-forming reactions. A base and an acid, e.g., NH 3 + HCl → ...

  6. Pyrophoricity - Wikipedia

    en.wikipedia.org/wiki/Pyrophoricity

    The creation of sparks from metals is based on the pyrophoricity of small metal particles, and pyrophoric alloys are made for this purpose. [2] Practical applications include the sparking mechanisms in lighters and various toys, using ferrocerium; starting fires without matches, using a firesteel; the flintlock mechanism in firearms; and spark testing ferrous metals.

  7. Zinc - Wikipedia

    en.wikipedia.org/wiki/Zinc

    It is a moderately reactive metal and strong reducing agent; [48] in the reactivity series it is comparable to manganese. [49] The surface of the pure metal tarnishes quickly, eventually forming a protective passivating layer of the basic zinc carbonate, Zn 5 (OH) 6 (CO 3) 2, by reaction with atmospheric carbon dioxide. [50]

  8. Titanium - Wikipedia

    en.wikipedia.org/wiki/Titanium

    Titanium is a very reactive metal that burns in normal air at lower temperatures than the melting point. Melting is possible only in an inert atmosphere or vacuum. At 550 °C (1,022 °F), it combines with chlorine. [12] It also reacts with the other halogens and absorbs hydrogen. [13]

  9. Actinide - Wikipedia

    en.wikipedia.org/wiki/Actinide

    Neptunium metal is very reactive. Ions of neptunium are prone to hydrolysis and formation of coordination compounds. [38] Plutonium also exhibits valence states between 3 and 7 inclusive, and thus is chemically similar to neptunium and uranium. It is highly reactive, and quickly forms an oxide film in air.