Atoms with the similar characteristics or properties are found in the same group or chemical family on the Periodic Table. Groups are elements in the same chemical family. Within the same group elements have the same number of valence electrons which determines their chemical properties. Here are some characteristics of some of the groups:
The periodic table also has a special name for its vertical columns. Each column is called a group. The elements in each group have the same number of electrons in the outer orbital. Those outer electrons are also called valence electrons.
The atoms of elements in Group 2 have the same number of valence electrons, which is 2. This gives them similar chemical properties, such as forming 2+ cations in reactions.
Group 2 metals have 2 valence electrons. In fact, the number of valence electrons of elements can be deduced from the group number (e.g. group VII elements have 7 valence electrons).
The outer shell of the atoms in Group D will always be 1 or 2 s orbital electrons. Irregularities occur with Cr where it is s1d5, not s2d4 and in Group 11 metals it is s1d10 not s2d9 so that the d-subshell is complete at Group 11.
Elements in the same group behave similarly because they all have the same number of electrons in their outer-most orbits. These electrons are what determines the types of bonds and chemical reactions the atom can undergo.
number of valence electrons
Such atoms belong to a group in the periodic table of elements.
Atoms of the elements in a group have the same number of electrons in their outer energy shells. This gives the elements similar Chemical Propetries.
The periodic table also has a special name for its vertical columns. Each column is called a group. The elements in each group have the same number of electrons in the outer orbital. Those outer electrons are also called valence electrons.
having the same number of electrons in their outermost electron shell. This is known as the valence electrons, which dictate the elements' reactivity and chemical behavior. Elements in the same group tend to react in similar ways because they have the same number of valence electrons.
Atoms of elements in group (column 2 of the periodic table) have 2 electrons in their outer shell. They have a low electronegativity, which means the electrons are not strongly attracted to the protons in the nucleus when compared to the electrons in atoms of column 6 or 7. For this reason, group 2 elements easily form +2 ion when in the presence of group 6 or7 elements.
The atoms of elements in Group 2 have the same number of valence electrons, which is 2. This gives them similar chemical properties, such as forming 2+ cations in reactions.
The atoms of the elements in the same group have the same number of valence electrons. This means that they react with other elements in a similar way. For example group 1. All the atoms in group 1 react with water and oxygen, so they have to be kept in paraffin-oil. Another example is group 18. They don't react with anything. The atoms of the same row have the same electron shells.
Elements in group have same number of valence electrons. They also have same chemical properties.
Group 2 metals have 2 valence electrons. In fact, the number of valence electrons of elements can be deduced from the group number (e.g. group VII elements have 7 valence electrons).
The outer shell of the atoms in Group D will always be 1 or 2 s orbital electrons. Irregularities occur with Cr where it is s1d5, not s2d4 and in Group 11 metals it is s1d10 not s2d9 so that the d-subshell is complete at Group 11.
Elements in the same group behave similarly because they all have the same number of electrons in their outer-most orbits. These electrons are what determines the types of bonds and chemical reactions the atom can undergo.