The oxidation state of the d-block elements can vary from -2 to +8, depending on the element and the compound it is in. Most of the d-block elements have an oxidation state of +2, +3, +4, or +6 in their compounds.
The d block elements, also known as transition elements, are located in the middle of the periodic table, between groups 2 and 13. They are characterized by having partially filled d orbitals in their outermost shells. Most of the d block elements are metals, although there are some metalloids and nonmetals. They are generally harder, …
Characteristics of d- block elements – ഡി-ബ്ലോക്ക് മൂലകങ്ങളുടെ സവിശേഷതകൾ Read More »
The d-block elements consist of the elements in the middle three columns of the periodic table. These elements are the transition metals. The d-block elements are characterized by having their outermost valence electrons in a d-orbital. The d-block elements are generally hard, have higher melting points, and are more resistant to chemical reactions. Examples of …
P block elements are the elements found in the p-block of the periodic table. They are also known as the “other main group elements” because they are in groups 13-18 on the periodic table. They are characterized by having their outermost electrons in the p-orbital. P block elements are generally reactive and form compounds with …
Characteristics of P block elements – പി ബ്ലോക്ക് മൂലകങ്ങളുടെ സവിശേഷതകൾ Read More »
P block elements are elements in the periodic table that have the highest number of electrons in their outermost shell, typically eight. These elements are located in columns 13 to 18 in the periodic table, and include elements such as boron (B), carbon (C), nitrogen (N), oxygen (O), fluorine (F), neon (Ne), sodium (Na), magnesium …
They all have a valence shell electronic configuration of ns2 np1-6. They all have relatively low ionization energies. They all have relatively high electron affinities. They all form covalent compounds due to their tendency to gain electrons. They all tend to form strong acids. They all have relatively low melting and boiling points.
The subshell electronic configuration is the arrangement of electrons in subshells (or orbitals) of an atom. It is usually expressed as a series of numbers denoting the number of electrons in each subshell (or orbital). The subshells (or orbitals) are grouped into four primary blocks: s, p, d, and f. The s block contains the …
The electronic configuration of chromium (Cr) is [Ar]3d54s1 and that of copper (Cu) is [Ar]3d104s1. Both chromium and copper have incomplete d-orbitals, but chromium has more electrons in its d-orbitals than copper. This is because chromium has two extra electrons in its d-orbital, while copper has one extra electron in its d-orbital. This peculiarity gives …
Noble gas electronic configuration refers to the complete electron configuration of the outermost shell of a noble gas, which is a group of elements in the periodic table that are highly stable due to having full valence shells. The noble gas electronic configuration for the first six noble gases is as follows: Helium (He): 1s2 …
When filling electrons in a subshell, electrons are filled in order of increasing energy, beginning with the lowest energy level. The subshells are filled in the order of 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p.