A106 Lesson 3 Team 3 Mindmap by Raamly Productions https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj en-us 2024-10-29 02:34:36 UTC 2024-10-29 05:15:58 UTC hello@padlet.com Transition metals parashuraam2006 https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191628566 2024-10-29 02:35:13 UTC https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191628566 What are transition metals? (Sof) parashuraam2006 https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191630317 Transition metals are found in Group 3 to 12 of the periodic table

  • Forms colored compounds

  • Has multiple O.S (Oxidation State)

  • Good catalyst

  • Based on the IUPAC definition, a transition metal is an element whose atom has an incomplete d sub-shell, or which can give rise to cations with an incomplete d sub-shell


    Physical properties

    •Higher melting point & densities than Group I and II metals

    •Harder and stronger than Group I and II metals

    •Good conductors of heat & electricity


    Chemical properties

    • Less reactive than Group I and II metals.

    • Variable oxidation states

    • Forms coloured compounds

    • Forms complex ions

    • Shows catalytic activity

]]> 2024-10-29 02:36:10 UTC https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191630317 Electron configuration of First Row Transition metals (raam) parashuraam2006 https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191630943

  • 1 orbital —> 2 electrons spinning in opposite directions

  • The subshells are s,p,d and f

    • Subshell S —> 1 orbital (2 electrons)

    • Subshell P —> 3 orbitals (6 electrons)

    • Subshell D —> 5 orbitals (10 electrons)

    • Subshell F —> 7 orbitals (14 electrons)

  • Aufbau Principle

    • This states that lower energy atomic orbitals are filled by electrons before higher energy ones are filled

    • The energy of orbitals increase from S to F

    • There are certain discrepancies such as 4s orbitals being filled first before 3d orbitals

      • This is mainly due to the fact that 4s orbitals have lower energy levels than 3d orbitals

    • Forming ions:

      • When ions are formed, electrons are removed first from 4s orbitals and then from the 3d orbitals.

  • Hund’s rule

    • Hund’s rule states that every orbital in a subshell is singly occupied with one electron before any orbital is occupied

    • All of the electrons in singly occupied orbitals have the same spin (points in the same direction).

  • Pauli’s exclusion principle

    • This principle states that an orbital can have a maximum of only 2 electrons and the 2 electrons must have opposing spins

  • Exceptions to the principles mentioned:

    1. Chromium

    2. Copper


    • ]]>     2024-10-29 02:36:29 UTC https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191630943     Variable oxidation states [Zahra] parashuraam2006 https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191631390

    Transition metals will form positive ions that have a positive oxidation state (O.S.) by losing electrons. When they form ions, electrons are removed from the 4s subshell before they are removed from the 3d subshell. Transition metals have multiple O.S. meaning they form ions with variable charges. Transition metals are good catalysts due to this property.


    The variable O.S. is possible due to the 4s and 3d having very close energy levels. This allows electrons to be removed from either orbital without a huge difference in energy occurring.


    Most transition metals have +2 and +3 oxidation states.


    ]]>     2024-10-29 02:36:43 UTC https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191631390     Complex ions [ Li Ying] parashuraam2006 https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191631727 Complex ion

    • has a metal ion at its centre with a number of other molecules / ions known as ligands

    • ligands are attached to the central ion by coordinate(dative) bonds


    Ligands

    • neutral molecules / anions that have at least one atom with a lone pair of electrons

    • Examples: chloro (CI-), cyano (CN-), hydroxo (OH-), aqua (H2O), ammine (NH3)


    Coordination number

    • total number of bonds the metal atom forms with ligands


    Ligand exchange

    Hexaaquacopper (II) ions [Cu(H2O)6]2+

    • Acid

      • adding concentrated hydrochloric acid

      • blue colour --> green

      • [Cu(H2O)6]2+ (aq) + 4Cl- (aq) --> [CuCl4]2- (aq) + 6H2O (l)


    • Base

      • adding excess amounts of ammonia solution

      • blue --> deep blue

      • [Cu(H2O)6]2+ (aq) + 4NH3 (aq) --> [Cu(NH3)4(H2O)2]2+ (aq) + 4H2O (l)


    ]]>     2024-10-29 02:36:53 UTC https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191631727     Coloured compounds [umai] parashuraam2006 https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191632267

  • In transition metal, the d orbital split into two different energy level [Lower and higher energy level]

  • Absorption of Energy:

    • When light hits these complexes, electrons can absorb energy to jump from the lower energy level to the higher energy level.

  • Color Formation:

    • The specific wavelength (color) of light that is absorbed corresponds to the energy difference between these two levels.

    • The color we see is the result of the light that is not absorbed; it is the complementary color of the absorbed light.

  • Energy Difference and Wavelength:

    • The greater the energy difference between the lower and higher energy levels, the more energy (shorter wavelength) is needed for an electron to make the jump.

    • Higher energy transitions correspond to shorter wavelengths, while lower energy transitions correspond to longer wavelengths.


    • ]]>     2024-10-29 02:37:08 UTC https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191632267     Catalysts(Chinmay) parashuraam2006 https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191632627 Catalysts are chemical substances that increase the rate of reaction without itself undergoing any permanent physical change.

    Transition metals and their compounds function as catalysts either because of their ability to change oxidation state or, in the case of the metals, to adsorb other substances on to their surface and activate them in the process.

    Types of catalytic reactions:

    Heterogenous and Homogeneous.

    In a heterogeneous reaction, the catalyst is in a different phase from the reactants.

    In a homogeneous reaction, the catalyst is in the same phase as the reactants.

    ]]>     2024-10-29 02:37:19 UTC https://padlet.com/parashuraam2006/oc9u2hdvtjfwxoaj/wish/3191632627