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Reactivity with oxygen, halogens and water

Atomic structure and the periodic table • Properties of transition metals

Key concepts

What you'll likely be quizzed about

  • Transition elements occupy the d-block of the periodic table and form ions with partly filled d-subshells.
  • Multiple stable oxidation states arise because electrons from both s- and d-subshells can participate in bonding.
  • This variability creates diverse compound types, often yielding colored ions and complex formation.

Flashcards

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How do oxidation states influence transition metal reactions?

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Variable oxidation states lead to different reaction products and slower, condition-dependent reactivity.

Key notes

Important points to keep in mind

Transition elements are d-block metals with variable oxidation states and often slower reaction rates.

Group 1 metals have one outer electron, forming +1 ions, and react rapidly with oxygen, halogens, and water.

Group 1 oxides may be oxides, peroxides, or superoxides based on the metal and conditions.

Transition metal oxides can form protective layers that reduce further oxidation.

Group 1 reactions with water yield hydroxides and hydrogen; reactivity increases down the group.

Transition metals may react with steam or acids instead of cold water; oxidation states determine products.

Surface area, temperature, and oxidation state are key limiting factors for observed reactivity.

Halide products differ: Group 1 yields simple ionic halides, while transition metals yield multiple halides with varying stoichiometry.

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