There is at least one oxidation number shared by all the elements in a Periodic Table column, but some of the elements may have more than one oxidation number and some of these additional oxidation numbers may not be possible for all the elements in a column.
Elements in the same group have similar chemical properties but not necessarily similar atomic numbers. Elements in the same group have the same number of valence electrons, which determines their reactivity and chemical properties.
Elements in the same group have similar chemical properties because they have the same number of valence electrons. This leads to similar reactivity and tendency to form compounds with the same oxidation number. The oxidation number is related to the number of electrons an atom gains, loses, or shares to reach a stable electron configuration.
The oxidation state varies in periods because elements in the same period have different numbers of electron shells, which affects their ability to gain or lose electrons. In a group, elements have the same number of valence electrons, leading to similar chemical properties and consistent oxidation states.
They have the same number of valence electrons which, in general, gives them similar oxidation numbers and other similar chemical and physical properties. The similarities are most pronounced in the groups at either side of the standard periodic table, and are least pronounced for the transition and rare earth elements.
Because within a group, the elements all have the same number of valence electrons, so their "combining power" (oxidation number) is relatively the same. In a period, the number of valence electrons increases going left to right, so the "combining power" changes.
Elements in the same group have similar chemical properties but not necessarily similar atomic numbers. Elements in the same group have the same number of valence electrons, which determines their reactivity and chemical properties.
Elements in the same group have similar chemical properties because they have the same number of valence electrons. This leads to similar reactivity and tendency to form compounds with the same oxidation number. The oxidation number is related to the number of electrons an atom gains, loses, or shares to reach a stable electron configuration.
The oxidation state varies in periods because elements in the same period have different numbers of electron shells, which affects their ability to gain or lose electrons. In a group, elements have the same number of valence electrons, leading to similar chemical properties and consistent oxidation states.
they have same numbers of electrons.
They share the same number of electrons (=2) in the valence shell: they have the same oxidation state of +2
It determines its place in reactivity. Usually gasesous elements are the electron recipients, except when it's gaseous-to-gaseous reactions (like combustion which turns a hydrocarbon into carbon dioxide and water vapor) while the metals generally are the donors. A case in point is HCl and NaOH make NaCl in a aqueous solution.
No. It is not the same. the number of valence electrons are same for the elements in the same column (group).
They have the same number of valence electrons which, in general, gives them similar oxidation numbers and other similar chemical and physical properties. The similarities are most pronounced in the groups at either side of the standard periodic table, and are least pronounced for the transition and rare earth elements.
generally yes. because they have the same number of valence electrons but there are exceptions as we go down the group due to inert pair effect
Because within a group, the elements all have the same number of valence electrons, so their "combining power" (oxidation number) is relatively the same. In a period, the number of valence electrons increases going left to right, so the "combining power" changes.
Elements with similar chemical properties are found in the same group on the periodic table. This is because elements in the same group have the same number of valence electrons, which determines their chemical behavior. Elements in the same period have different numbers of electron shells, leading to varying chemical properties.
Elements in the same group have more in common because they have the same number of valence electrons, leading to similar chemical properties. Elements in the same period have increasing atomic numbers and electron shells, but their properties can vary widely due to different numbers of electron shells and arrangements.