Transition metals
Cards (16)
- Transition metals exhibit catalytic activity because they can undergo redox reactions by changing their oxidation states.
- Transition metal compounds can be oxidizing or reducing agents depending on their charge.
- Transition metals act as catalysts to lower the activation energy barrier for chemical reactions.
- Transition metals often exhibit variable valence due to their ability to gain or lose electrons easily.
- Transition metals are known for their ability to form complex ions and compounds due to their high affinity for ligands.
- There is an increase in melting point as we move down group 6 due to increased metallic bonding.
- Transition metals have strong metallic bonds that contribute to their physical properties such as ductility, malleability, and thermal conductivity.
- Transition metals have partially filled d orbitals, allowing them to participate in bonding through covalent interactions with other atoms.
- The electronic structure of transition metals allows them to have multiple oxidation states, which is important for their role as catalysts.
- Transition metals have unique magnetic properties due to the presence of unpaired electrons in their atomic orbitals.
- Transition metals can undergo redox reactions due to the presence of unpaired electrons in their outer shells.
- The electronic configuration of transition metals includes one or more unpaired electrons in the outermost shell, leading to paramagnetic behavior.
- Iron (Fe) has a low density compared to other transition metals due to its body-centered cubic structure with large interstitial spaces filled by hydrogen atoms.
- The transition elements show a wide range of colors when they exist as ions in solution because of differences in electron configurations.
- Atomic radius increases going across a period (left to right) due to the addition of one electron into the next higher principal quantum level.
- The first ionization energies decrease from top to bottom of groups 1-7, indicating that it becomes easier to remove outer shell electrons.