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For main group elements (i.e s-block and p-block elements), the valence electrons are the electrons present in the outermost orbit. But for most of the transition and inner transition elements, the valence electrons are the electrons present in the shells outside the noble gas core.
Electron configurations allow us to understand many periodic trends. Covalent radius increases as we move down a group because the n level (orbital size) increases. Covalent radius mostly decreases as we move left to right across a period because the effective nuclear charge experienced by the electrons increases, and the electrons are pulled ...
Explain the relationship between the chemical behavior of families in the periodic table and their valence electrons. Identify elements that will have the most similar properties to a given element.
The commonly used long form of the periodic table is designed to emphasize electron configurations. Since it is the outermost (valence) electrons which are primarily involved in chemical interactions between atoms, the last electron added to an atom in the building-up process is of far more interest to a chemist than the first.
This periodic table shows the valences of element groups. The transition metals make use of the d -subshell, which can accommodate 10 electrons. The f -subshell holds 14 electrons and the g -subshell contains up to 18 electrons.
To solve without a periodic table, find the electron configuration of the element and count the electrons into 1 group of 2, and then into shells of 8. The number in the last group is the amount of valence electrons.
How does an atom's valence electron configuration determine its place in the periodic table? How is the energy level of an atom's valence electrons related to its period in the periodic table? How do you determine valence electrons when given group number?