d Block Elements : Introduction

The video tutorial introduces D block elements, explaining their electron configurations and why they are termed transition metals. It covers the IUPAC definition of transition metals, highlighting the incomplete D subshell. The tutorial also discusses anomalies in electronic configurations, such as those of chromium and copper, due to stability factors. Group 12 elements, despite having full D10 configurations, are not considered transition metals but are studied alongside them. The video concludes with an invitation to explore the characteristics and trends of transition elements.

Which elements in the periodic table are known as D block elements?

• Elements with electrons in the 6P orbital

• Elements with electrons in the 5S orbital

• Elements with electrons in the 4P orbital

• Elements with electrons in the 3D orbital

Why are D block elements referred to as transition metals?

• They have a complete D subshell

• They are the only metals in the periodic table

• They are located between the S and P block elements

• They transition between solid and liquid states

According to IUPAC, what defines a transition metal?

• An element with a full P subshell

• An element with a full S subshell

• An element with an incomplete D subshell or cations with an incomplete D subshell

• An element with a complete D subshell

What is the electronic configuration anomaly observed in chromium?

• 3D54S1 instead of 3D44S2

• 3D94S1 instead of 3D104S2

• 3D44S2 instead of 3D54S1

• 3D104S2 instead of 3D94S1

Why are zinc, cadmium, and mercury not considered transition metals?

• They are located in Group 11

• They have an incomplete D subshell

• They have a full P subshell

• They have a full D10 configuration in their ground state and common oxidation states