The elements in group 6a (16) have six valence electrons. The valence electron configuration is Xs2Xp4 , where X is the main energy level (period number).
Selenium is found in Group 6A (Group 16) of the p-block because it has six valence electrons, which places it in the 6th group of the periodic table. It shares similar chemical properties with the other elements in Group 6A, such as oxygen and sulfur, due to its electron configuration.
The elements in group 3A and 6A show a dip in ionization energy due to the presence of a full or half-full subshell. In group 3A, elements have a stable electronic configuration when one electron is removed, resulting in a lower ionization energy. In group 6A, elements exhibit a half-filled p orbital when one electron is added, making it easier to remove an electron and thus lowering the ionization energy.
It is alternatively called the Carbon family.
They should gain 2 electrons to attain noble gas electronic configuration. (it doesn't become a noble gas as the number of protons are not same)
no i believe it has something to do with the group its in on the periodic table. its in group 6a so look up how to write the formula from there and its ionic charge is +4 or a -4 charge because it has four electrons in it's outermost electron level
Selenium is found in Group 6A (Group 16) of the p-block because it has six valence electrons, which places it in the 6th group of the periodic table. It shares similar chemical properties with the other elements in Group 6A, such as oxygen and sulfur, due to its electron configuration.
S [Ne] 3s2 3p4
Sulfur is part of group 16 of the periodic table because it has 6 valence electrons, which gives it similar chemical properties to other elements in the group. Group 16 elements tend to form compounds by gaining or sharing 2 electrons to achieve a stable electron configuration.
6A elements, also known as group 16 elements, have 6 valence electrons. This is because they are located in group 16 of the periodic table, which corresponds to the number of valence electrons. Examples of 6A elements include oxygen, sulfur, and selenium.
The elements in group 3A and 6A show a dip in ionization energy due to the presence of a full or half-full subshell. In group 3A, elements have a stable electronic configuration when one electron is removed, resulting in a lower ionization energy. In group 6A, elements exhibit a half-filled p orbital when one electron is added, making it easier to remove an electron and thus lowering the ionization energy.
The smallest atom in group 6A is oxygen. Oxygen gains 2 electrons to achieve a stable electron configuration by forming an oxide ion with a 2- charge.
oxygen has 6 valence electrons as indicated by the 6A above the group oxygen is in
Sulfur and oxygen are in the same group (Group 6A) because they have similar chemical properties due to their shared number of valence electrons, which influences their reactivity and bonding behavior. They both have six valence electrons, leading to comparable trends in their chemical properties within the same group.
It is alternatively called the Carbon family.
The most probable charge of an ion in the sulfur group (Group 6A) is -2. This is because sulfur typically gains two electrons to achieve a stable electron configuration, resulting in the Sulfide ion (S2-).
They should gain 2 electrons to attain noble gas electronic configuration. (it doesn't become a noble gas as the number of protons are not same)
no i believe it has something to do with the group its in on the periodic table. its in group 6a so look up how to write the formula from there and its ionic charge is +4 or a -4 charge because it has four electrons in it's outermost electron level