D BLOCK Flashcards
What defines transition metals according to TUPAC?
Transition metals are defined by the presence of partly filled d orbitals in their common oxidation states.
This definition highlights their unique electronic configurations that differentiate them from other elements.
Which group of elements is not regarded as transition metals?
Zinc, cadmium, and mercury are not regarded as transition metals due to their full d subshells.
These elements have d10 configurations in their neutral atoms or ions.
What are the four series of transition metals?
The four series are:
* 3d series (Sc to Zn)
* 4d series (Y to Cd)
* 5d series (La to Hg)
* 6d series (Ac and elements from Rf to Cn)
Each series corresponds to the filling of d orbitals in the periodic table.
What elements are referred to as inner transition metals?
The elements in the f-block, specifically the lanthanoids (4f) and actinoids (5f).
These elements are found in the separate panel at the bottom of the periodic table.
What role do inner transition elements like Th, Pa, and U play in modern times?
They are excellent sources of nuclear energy.
Their properties make them significant in energy production.
Which transition elements have played important roles in the development of human civilization?
Iron, copper, silver, and gold.
These metals have been crucial in various applications throughout history.
Fill in the blank: The d-block of the periodic table contains the elements in which the _______ orbitals are progressively filled.
d
This filling occurs across the groups 3-12 of the periodic table.
True or False: The chemical properties of transition metals are similar to those of s-block and p-block elements.
True
Transition metals exhibit transitional behavior between the s and p-block elements.
What is the significance of the oxidation states of transition metals?
They exhibit a variety of oxidation states, which contributes to their diverse chemical behavior.
This variability is a key characteristic of transition metals.
What is the electronic configuration of transition elements?
(n-1)dⁿs²
Where (n-1) represents the inner d orbitals and n represents the outermost s orbital.
What are the four rows of transition metals in the d-block?
3d, 4d, 5d, 6d
These series correspond to the filling of d orbitals in different energy levels.
Which transition elements are particularly noted for their precious metal properties?
Silver, gold, platinum
These metals are valued for their rarity and applications in jewelry and electronics.
What is a notable exception in the electronic configuration of chromium (Cr)?
3d⁵ 4s¹
This configuration instead of 3d⁴ 4s² is due to stability from half-filled orbitals.
What is the electronic configuration of copper (Cu)?
3d¹⁰ 4s¹
This configuration is favored over 3d⁹ 4s² due to the stability of fully filled d orbitals.
True or False: The d-block elements are located between the s- and p-blocks in the periodic table.
True
The d-block elements are centrally located in the periodic table.
What is the significance of the small energy gap between (n-1)d and ns orbitals?
It leads to exceptions in electronic configurations
The small energy difference allows for electron configurations that deviate from expected patterns.
Fill in the blank: The transition elements can be successfully applied to the usual theory of _______.
valence
This theory describes how elements bond and interact based on their electron configurations.
List the first five transition elements in order.
- Sc (21)
- Ti (22)
- V (23)
- Cr (24)
- Mn (25)
The atomic numbers are provided for reference.
What is the general characteristic of the oxidation states of transition elements?
They can exhibit multiple oxidation states
This variability is due to the involvement of d electrons in bonding.
What is the primary focus of the unit discussed?
Electronic configurations, occurrence, and general characteristics of transition elements
The unit also covers properties and compounds of these elements.
What defines a transition element?
An element with incompletely filled d orbitals in its ground state.
Why is zinc (Z = 30) not regarded as a transition element?
It has completely filled d orbitals in its ground state and in its oxidized state.
What is the general electronic configuration formula for Zn, Cd, Hg, and Cn?
(n-1)d10ns
How do the d orbitals of transition elements differ from s and p orbitals?
They protrude to the periphery of an atom more than s and p orbitals.
What characteristics do transition elements exhibit due to partly filled d orbitals?
Variety of oxidation states, formation of colored ions, complex formation with ligands.
True or False: Transition metals and their compounds exhibit catalytic properties.
True
What type of behavior do transition metals typically exhibit?
Paramagnetic behavior.
What similarities exist among transition elements within a horizontal row?
Greater similarities in properties compared to non-transition elements.
Fill in the blank: The d orbitals of transition elements are more influenced by their _______.
surroundings
What are the characteristic properties of transition elements?
Magnetic and electronic properties.
How are the properties of transition elements studied?
By examining general characteristics and trends in horizontal rows.
What is indicated by the presence of similar magnetic and electronic properties among transition element ions?
They have a similar d configuration (n = 1-9).
What is the significance of the 3d row in transition metals?
It is particularly studied for its general characteristics and trends.
Which transition elements do not show properties like high tensile strength , ductility, malleability etc?
Zn, Cd, Hg, Mn
Why do transition metals have high melting points?
The high melting points of these metal are attributed to the involvement of greater number of electrons from (n - 1)d in addition to the ns electrons in the interatomic metallic bonding.
