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- https://chem.libretexts.org/Courses/Tennessee_State_University/CHEM_4210%3A_Inorganic_Chem_II_(Siddiquee)/04%3A_d-Block_Metal_Chemistry/4.01%3A_Properties_of_Transition_Metals/4.1.03%3A_General_Trends_among_the_Transition_MetalsTransition metals are characterized by the existence of multiple oxidation states separated by a single electron. Most transition-metal compounds are paramagnetic, whereas virtually all compounds of t...Transition metals are characterized by the existence of multiple oxidation states separated by a single electron. Most transition-metal compounds are paramagnetic, whereas virtually all compounds of the p-block elements are diamagnetic.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Coordination_Chemistry/Complex_Ion_Chemistry/Origin_of_Color_in_Complex_IonsThis page is going to take a simple look at the origin of color in complex ions - in particular, why so many transition metal ions are colored.
- https://chem.libretexts.org/Courses/Northern_Michigan_University/CH_215%3A_Chemistry_of_the_Elements_Fall_2023/01%3A_Atoms_and_Electronic_Structure/1.09%3A_Electron_Configurations_for_Transition_Metal_ElementsWriting an electron configuration for a transition metal element follows the same basic steps as for writing an electron configuration for an element in the s-block or p-block. List each subshell, and...Writing an electron configuration for a transition metal element follows the same basic steps as for writing an electron configuration for an element in the s-block or p-block. List each subshell, and then fill each subshell with an appropriate number of electrons until all electrons in the element are accounted for. Transition elements have electrons in the d orbital, which introduces some additional nuance in the electron configurations.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/07%3A_Chemical_Nomenclature/7.06%3A_The_Stock_System_of_NomenclatureThis page discusses mp3 players' design and specifications, along with the naming of compounds with transition metals using the Stock system to indicate ionic charges. It provides examples, such as na...This page discusses mp3 players' design and specifications, along with the naming of compounds with transition metals using the Stock system to indicate ionic charges. It provides examples, such as naming FeCl3 as iron (III) chloride, to illustrate the need for accuracy in naming to reflect the chemical properties of compounds like copper and tin. The summary highlights the significance of proper nomenclature in chemistry.
- https://chem.libretexts.org/Sandboxes/khaas/Inorganic_Chemistry_II_(CHEM4210)/08%3A_Lanthanide_and_Actinide/8.01%3A_The_Lanthanides/8.1.01%3A_Lanthanides-_Properties_and_ReactionsThe Lanthanides consist of the elements in the f-block of period six in the periodic table. While these metals can be considered transition metals, they have properties that set them apart from the re...The Lanthanides consist of the elements in the f-block of period six in the periodic table. While these metals can be considered transition metals, they have properties that set them apart from the rest of the elements.
- https://chem.libretexts.org/Sandboxes/khaas/Inorganic_Chemistry_II_(CHEM4210)/04%3A_d-Block_Metal_Chemistry/4.01%3A_Properties_of_Transition_Metals/4.1.03%3A_General_Trends_among_the_Transition_MetalsTransition metals are characterized by the existence of multiple oxidation states separated by a single electron. Most transition-metal compounds are paramagnetic, whereas virtually all compounds of t...Transition metals are characterized by the existence of multiple oxidation states separated by a single electron. Most transition-metal compounds are paramagnetic, whereas virtually all compounds of the p-block elements are diamagnetic.
- https://chem.libretexts.org/Courses/Westminster_College/CHE_180_-_Inorganic_Chemistry/10%3A_Chapter_10_-_The_Transition_Metals/10.1%3A_Properties_of_Transition_Metals/Introduction_to_Transition_Metals_IIn chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electro...In chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electrons the actual configuration becomes [Ar]3d 5 4s 1 where all the electrons in the outer orbitals are unpaired.
- https://chem.libretexts.org/Courses/Tennessee_State_University/CHEM_4210%3A_Inorganic_Chem_II_(Siddiquee)/04%3A_d-Block_Metal_Chemistry/4.01%3A_Properties_of_Transition_Metals/4.1.04%3A_Introduction_to_Transition_Metals_IIn chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electro...In chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electrons the actual configuration becomes [Ar]3d 5 4s 1 where all the electrons in the outer orbitals are unpaired.
- https://chem.libretexts.org/Courses/Westminster_College/CHE_180_-_Inorganic_Chemistry/10%3A_Chapter_10_-_The_Transition_Metals/10.1%3A_Properties_of_Transition_Metals/Electron_Configuration_of_Transition_MetalsThe noble gas before the first row of transition metals would be the core written with brackets around the element symbol (i.e. [Ar] would be used for the first row transition metals), and the electro...The noble gas before the first row of transition metals would be the core written with brackets around the element symbol (i.e. [Ar] would be used for the first row transition metals), and the electron configuration would follow a [Ar] ns x nd x format. In the case of first row transition metals, the electron configuration would simply be [Ar] 4s x 3d x . The energy level, "n", can be determined based on the periodic table, simply by looking at the row number in which the element is in.
- https://chem.libretexts.org/Courses/CSU_Fullerton/Chem_325%3A_Inorganic_Chemistry_(Cooley)/05%3A_d-Block_Metal_Chemistry-_General_Considerations/5.03%3A_Introduction_to_Transition_Metals_IIn chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electro...In chromium it can be shown that the 4s orbital energy is still below the 3d which suggests a configuration [Ar] 3d 4 4s 2 . However due to the effect of electronic repulsion between the outer electrons the actual configuration becomes [Ar]3d 5 4s 1 where all the electrons in the outer orbitals are unpaired.
- https://chem.libretexts.org/Courses/Northern_Michigan_University/CH_215%3A_Chemistry_of_the_Elements_Fall_2023/07%3A_Descriptive_Chemistry/7.01%3A_Electron_Configuration_of_Transition_MetalsThe noble gas before the first row of transition metals would be the core written with brackets around the element symbol (i.e. [Ar] would be used for the first row transition metals), and the electro...The noble gas before the first row of transition metals would be the core written with brackets around the element symbol (i.e. [Ar] would be used for the first row transition metals), and the electron configuration would follow a [Ar] ns x nd x format. In the case of first row transition metals, the electron configuration would simply be [Ar] 4s x 3d x . The energy level, "n", can be determined based on the periodic table, simply by looking at the row number in which the element is in.
