Podcast
Questions and Answers
What is the reason behind the high melting and boiling points of transition metals?
What is the reason behind the high melting and boiling points of transition metals?
- Weak interatomic interactions
- High ionization energy of transition metals
- Involvement of both ns and (n-1)d electrons in metallic bonding (correct)
- Presence of fully filled d-orbitals
Why do zinc, cadmium, and mercury have relatively low melting points and boiling points?
Why do zinc, cadmium, and mercury have relatively low melting points and boiling points?
- Strong metallic bonds
- High ionization energy
- Less delocalization of electrons
- Presence of fully filled d-orbitals (correct)
Why do manganese (Mn), Technetium (Tc), and Rhenium (Re) have lower melting points compared to their neighborhood elements?
Why do manganese (Mn), Technetium (Tc), and Rhenium (Re) have lower melting points compared to their neighborhood elements?
- Strong metallic bonding
- Presence of d5 configuration (correct)
- High ionization energy
- Full d-orbitals
What is the trend in melting points of transition metals in a series?
What is the trend in melting points of transition metals in a series?
Why is mercury liquid at room temperature?
Why is mercury liquid at room temperature?
Why are d-block elements called transition elements?
Why are d-block elements called transition elements?
Why are Zn, Cd, and Hg not classified as transition elements?
Why are Zn, Cd, and Hg not classified as transition elements?
Which series of d-block elements includes elements from Scandium (Sc) to Zinc (Zn)?
Which series of d-block elements includes elements from Scandium (Sc) to Zinc (Zn)?
Why is Copper (Cu) considered a transition element despite having a fully filled d-orbital?
Why is Copper (Cu) considered a transition element despite having a fully filled d-orbital?
Why do Zn, Cd, and Hg have the same electron configuration in their ground state?
Why do Zn, Cd, and Hg have the same electron configuration in their ground state?
Study Notes
- D-block elements are in the middle of s and p blocks, comprising groups 3 to 12 in the periodic table, with four transition series: 3d, 4d, 5d, and 6d series.
- The general electronic configuration of d-block elements is (n-1)d(1-10) ns(1-2) for different series.
- Transition elements are called so because they bridge the most electropositive ‘s’ and less electropositive ‘p’ block elements, with incomplete d-orbitals in their ground state or oxidation state.
- Zinc, Cadmium, and Mercury are d-block elements but not called transition elements as their d-orbitals are fully filled in both ground state and common oxidation state.
- Transition metals have high melting points due to the presence of more unpaired electrons in d-orbitals, involving both ns and (n-1)d electrons in metallic bonding.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Description
Learn about the position of d-block elements in the periodic table, which are situated between the s and p blocks. Explore the transition series including the 3d, 4d, 5d, and 6d series.
