What is a transition element
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1) Transition elements are found in the d-block of the Periodic Table between Groups 2 and 13, but not all d-block elements are transition elements. 2) The chapter will focus on transition elements in the first row of the d-block, specifically titanium through copper, excluding scandium and zinc. 3) Transition metal atoms have their 4s subshell filled first and then electrons occupy the 3d subshell, though chromium and copper are exceptions with only one electron in the 4s subshell.
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![Scandium/Electron configuration
[Ar] 3d¹ 4s² --- minus 3 for Sc+3 ion ------- empty d
Zinc/Electron configuration
[Ar] 3d10 4s² --- minus 2 for Zn+2 ion----not incomplete d](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
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Chapter 8 the d and f block elements
The document provides the electronic configurations of various ions of transition metals and lanthanides. It also provides answers to questions related to oxidation states, stability, and properties of transition metal ions and compounds. The key points are:
1) Electronic configurations of ions such as Cr3+, Cu+, Co2+, Mn2+, Pm3+, Ce4+, Lu2+, and Th4+ are given.
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The document discusses the d-block and f-block elements of the periodic table. It provides details about their electronic configurations, properties, and reactions. The d-block contains the transition metals whose d orbitals are filled from groups 3 to 12. The f-block contains the inner transition metals whose 4f and 5f orbitals are filled. Elements in these blocks can exhibit a variety of oxidation states and form complexes due to their electronic structure.
D f-block chemistry-12
Transition elements have several key characteristics:
(1) They exhibit variable oxidation states unlike s-block and p-block elements.
(2) Many of their compounds are colored due to electron transitions between d-orbital energy levels.
(3) They have a great tendency to form complex compounds due to their small, highly charged ions and vacant low energy d-orbitals.
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What is a transition element
- 1. What is a transition element? The transition elements are found in the d block of the Periodic Table, between Groups 2 and 13. However, not all d-block elements are classified as transition elements.
- 2. Scandium/Electron configuration [Ar] 3d¹ 4s² --- minus 3 for Sc+3 ion ------- empty d Zinc/Electron configuration [Ar] 3d10 4s² --- minus 2 for Zn+2 ion----not incomplete d
- 3. In this chapter we will be looking at the transition elements in the first row of the d block. These are the metals titanium (Ti) through to copper (Cu), according to the definition below which excludes Sc and Zn
- 11. The electronic configurations of the atoms in the first row of the transition elements. In atoms of the transition elements, the 4s subshell is normally filled and the rest of the electrons occupy orbitals in the 3d subshell. However, chromium and copper atoms are the exceptions. Chromium atoms have just one electron in the 4s subshell. The remaining five electrons are arranged in the 3d subshell so that each orbital is occupied by one electron. Copper atoms also have just one electron in the 4s subshell. The remaining ten electrons are arranged in the 3d subshell so that each orbital is filled by two electrons.
- 25. Ions of Transition elements The transition elements are all metals. In common with all metals, their atoms tend to lose electrons so they form positively charged ions. However, each transition metal can form more than one ion. For example, the common ions of copper are Cu+ and Cu2+. We say that the transition metals have variable oxidation states. The resulting ions are often different colours
- 26. The most common oxidation states of the first row of the transition elements. The existence of variable oxidation states means that the names of compounds containing transition elements must have their oxidation number included, e.g. manganese(IV) oxide, cobalt(II) chloride.
- 27. When transition elements form ions, their atoms lose electrons from the 4s subshell first, followed by 3d electrons.
- 28. From previous work looking at periodic properties we would expect the 1st ionization energy, atomic radius and ionic radius of positively charged ions to vary across a period. In general, the 1st ionization energy would increase as the increasing nuclear charge has a tighter hold on electrons filling the same main energy level or shell, and the shielding effect stays roughly the same. For similar reasons the atomic radius and ionic radius of a positively charged ion would be expected to decrease