It increases from left to right across a period because as electrons are added to the same energy level, and the closer an atom gets to having an octet of electrons, the easier it is for the atom to attract electrons from other atoms, either through ionic bonding or covalent bonding.
Elements in a period share the same number of electron shells, leading to similar chemical behaviors. As you move across a period from left to right, the atomic number and number of protons increase, leading to a gradual increase in electronegativity, ionization energy, and atomic size. Elements at the beginning of a period tend to be metals, while those at the end are nonmetals.
atomic size decreases across a period
increase from left to right across a period.
The number of valence electrons for the elements increases across a period, from 1 (group 1) to 8 (group 18).
The second period of the periodic table contains elements from lithium to neon, in increasing atomic number order. These elements have increasing numbers of protons and electrons as you move from left to right across the period, resulting in changes in properties such as atomic size and reactivity.
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Atomic size increase down the group and decreases across the period.
In a group labeled as A, as atomic numbers increase across a period, the reactivity of elements generally decreases. This is because as you move from left to right across a period, the elements have more protons in the nucleus, which leads to stronger nuclear charge and less tendency to lose electrons and react with other elements.
The first ionization energy generally increases across a period for main group elements because as you move from left to right across a period, the effective nuclear charge increases, making it harder to remove an electron from the outer shell. This results in a higher energy requirement to remove an electron, leading to an increase in ionization energy.
Across a period, the metallic character decreases.
Elements in a period share the same number of electron shells, leading to similar chemical behaviors. As you move across a period from left to right, the atomic number and number of protons increase, leading to a gradual increase in electronegativity, ionization energy, and atomic size. Elements at the beginning of a period tend to be metals, while those at the end are nonmetals.
The trend in period 2 ionization energy across the elements increases from left to right.
atomic size decreases across a period
increase from left to right across a period.
The number of valence electrons for the elements increases across a period, from 1 (group 1) to 8 (group 18).
The number of valence electrons for the elements increases across a period, from 1 (group 1) to 8 (group 18).
The second period of the periodic table contains elements from lithium to neon, in increasing atomic number order. These elements have increasing numbers of protons and electrons as you move from left to right across the period, resulting in changes in properties such as atomic size and reactivity.