Electron configuration is the arrangement of elements according to their increasing atomic numbers whiles period is the arrangement of elements according to the increasing number of valence electrons.
As we move across the table we'll find a regular increase trend in the atomic no. of the elements. This implies that there is regular increase in valence electrons ie the valency increases regularly by 1. for eg sodium, magnesium, aluminum atc lies in same period . Their electronic confriguration is
Na=2,8,1
Mg=2,8,2
Al=2,8,3
a decrease in ionization energy
number of electrons keep on increasing but the shell remains the same as we move left to right in a period
Both electronegativity and ionization energy increase across a period from left to right, and decrease down a group from top to bottom.
horizontal and vericle lines in a chart
categories
A repeating pattern
what is the reason for ionization energy across a period
In electronegativity, the first ionization energy increases as it moves from left to right across a period . The nuclear charge also increases and the shielding effect is constant when moving across.
The Pauling electronegativity and the first ionization energy increase from sodium to chlorine.
Across a period, first ionization energy increases. However, when going down a group, first ionization energy generally decreases. As you go down a group, atoms hove more total electrons so they don't really care that much about their outermost ones.
Electronegativity, ionization energy, electron affinity, and atomic number are values that increase from left to right across a period.
Atomic number, ionization energy and electronegativity
what is the reason for ionization energy across a period
In electronegativity, the first ionization energy increases as it moves from left to right across a period . The nuclear charge also increases and the shielding effect is constant when moving across.
The Pauling electronegativity and the first ionization energy increase from sodium to chlorine.
Ionization energy increases as you go across a period, but as you go down a group it decreases.
Across a period, first ionization energy increases. However, when going down a group, first ionization energy generally decreases. As you go down a group, atoms hove more total electrons so they don't really care that much about their outermost ones.
The atomic size decreases (with some exceptions) , the ionization energy , electronegativity and electron affinity also increase from left to right.
Electronegativity, ionization energy, electron affinity, and atomic number are values that increase from left to right across a period.
The trend for first ionization energy
The electronegativity increases
xenon increases from left to right across periods (first ionization energy)
Phosphorus. Across the period, first ionization energy increases.