The metallic model - physical properties of transition elements Flashcards
What is the definition of a transition metal?
An element with an incomplete d-subshell or an element that can form at least one stable cation with an incomplete d-subshell
This definition excludes scandium and zinc.
Which elements are included in the first transition series?
Titanium to copper
These elements have incomplete d-subshells.
Where are transition metals located on the Periodic Table?
In the d-block
Period 4: From titanium to copper; Period 5: From zirconium to silver.
What is the structure of transition metals?
A metallic lattice structure with layers of positive ions and a sea of delocalised electrons
This structure contributes to their unique properties.
Why do transition metals have high melting points?
Greater electron density due to delocalised d-electrons strengthens electrostatic forces between cations and electrons
More energy is required to overcome these forces.
What is the melting point range of s-block metals?
From 27 °C for francium to 839 °C for calcium
Beryllium is an exception with a melting point of 1,287 °C due to strong metallic bonding.
What causes transition metals to have high electrical conductivity?
A large number of delocalised electrons allows more electrons to move under a potential difference
This property is essential for their use in electrical applications.
Which are the three most conductive metals?
- Silver
- Copper
- Gold
Copper is particularly noted for its use in electrical cables.
What distinguishes transition metals from d-block elements?
Transition metals have an incomplete d-subshell, while some d-block elements like scandium and zinc do not
Scandium forms only Sc3+ and zinc forms only Zn2+.
