Chemistry d & f Block Elements

Elements in groups 3 to 12 of the periodic table. They have their valence electrons in the (n-1)d orbitals, resulting in properties like high melting points and catalytic ability.

Transition elements that don't behave like typical transition metals. They often resemble elements in other groups.

These elements have specific properties and uses, including being essential for production and catalysis.

These compounds involve elements from the d-block and are often used in various applications, from pigments to batteries.

The ability of d-block elements to lose electrons to form cations, leading to variable charges and a variety of compounds.

The tendency of elements within the same group (vertical column) of the periodic table to have similar chemical properties due to their similar electron configurations.

The standard electrode potential (E°) is a measure of the tendency of a species to gain electrons and be reduced. A more negative E° value indicates a greater tendency for the species to be oxidized.

Manganese (Mn), Nickel (Ni), and Zinc (Zn) have less favorable reduction potentials (more negative E° values) than expected based on their position within the group. This indicates they are more easily oxidized.

Iron can exist in two common oxidation states: +2 (ferrous) and +3 (ferric). These different oxidation states lead to different chemical properties and reactivity.

Lanthanides (Ln) are a series of elements with similar chemical properties and electron configurations. They commonly form oxides and sulfides.

The size difference in atomic radii between two metals must be less than 15% for an alloy to form.

A series of elements in the f-block, characterized by their electronic configuration with electrons filling the 4f orbitals.

A series of elements in the f-block with electrons filling the 5f orbitals.

The most common oxidation state for lanthanoids is +3.

The ionic size of lanthanoids gradually decreases as you move across the series from left to right.

The enthalpy change when one mole of gaseous atoms is formed from one mole of the element in its standard state.

The transition metals in the 3d block have high enthalpies of atomization due to the involvement of d-electrons in metallic bonding.

The atomic radius of transition metals generally decreases across a period (from left to right) due to increasing effective nuclear charge.

The atomic radius of transition metals generally increases down a group (from top to bottom) due to the addition of electron shells.

The lanthanide contraction is a phenomenon that occurs in transition metals where the atomic radii of elements in the 4d and 5d series are smaller than expected due to poor shielding by 4f electrons.

The density of transition metals generally increases from left to right across a period because of the increase in atomic mass and decrease in atomic radius.

Transition metals exhibit variable oxidation states because they can lose electrons from both their ns and (n-1)d orbitals.

The ionization enthalpy of transition metals generally increases from left to right across a period because of the increasing effective nuclear charge.

Transition metals are paramagnetic because they have unpaired d-electrons.

Transition metal compounds often exhibit intense colour due to d-d transitions, where electrons absorb and emit light in the visible spectrum.

Transition metals often serve as catalysts in chemical reactions because they can readily change their oxidation states.

Potassium permanganate (KMnO4) is a strong oxidizing agent because it readily accepts electrons.

Potassium dichromate (K2Cr2O7) is a strong oxidizing agent that readily accepts electrons.

The preparation of potassium permanganate involves the oxidation of manganese dioxide (MnO2) in the presence of potassium hydroxide (KOH) and oxygen (O2).

The preparation of potassium dichromate involves the oxidation of chromite ore (FeCr2O4) followed by several chemical steps.

The tendency of a chemical species to gain electrons and be reduced, measured as the standard electrode potential (E°). It indicates the ease of reduction of a substance.

Elements in groups 3 to 12 of the periodic table, characterized by having their valence electrons in the (n-1)d orbitals.

The tendency for transition elements to exhibit multiple oxidation states due to their variable number of electrons that can be lost.

The ability of a substance to lose electrons and be oxidized, indicating its readiness to donate electrons in a reaction.

A type of magnetism where a substance weakly repels a magnetic field. It arises from the absence of unpaired electrons in the atom.

A type of magnetism where a substance weakly attracts a magnetic field. It arises from the presence of unpaired electrons in the atom.

The process of a chemical species gaining electrons, leading to a decrease in oxidation state. It is often accompanied by a color change.

The process of a chemical species losing electrons, leading to an increase in oxidation state. It is often accompanied by a color change.

A compound formed when a transition metal ion combines with oxygen ions. Examples include CrO42- (chromate) and Cr2O72- (dichromate).

A substance with multiple oxidation states, often exhibiting a color change during redox reactions.

d-block elements are those that have their valence electrons in the (n-1)d orbitals; they exhibit properties like high melting points, forming colored ions due to d-d transitions, and catalytic ability.

The formation of colored ions in d-block elements is due to the transitions of electrons within their partially filled d-orbitals, absorbing specific wavelengths of light and reflecting others.

d-block elements participate in the formation of a wide range of complex compounds, involving the coordination of ligands around the central metal ion. These compounds play crucial roles in various applications.

Interstitial compounds are formed by d-block elements where small non-metal atoms occupy the spaces between the metal atoms. These compounds are non-stoichiometric and exhibit unique properties.

Transition metals generally possess variable oxidation states, meaning they can readily lose different numbers of electrons, giving rise to diverse compounds with different properties.

Transition metals are frequently used in various catalytic applications due to their ability to facilitate reactions by providing alternative pathways, often involving intermediate complex formation.

d-block elements exhibit a wide range of magnetic properties, from diamagnetic (no magnetic moment) to paramagnetic (weak magnetic moment) to ferromagnetic (strong magnetic moment), depending on the number of unpaired electrons.

Lanthanoids and actinoids are groups of elements within the d-block, characterized by their partially filled f-orbitals. They are typically reactive and exhibit unique properties due to their 4f and 5f electrons.