It decreases because there is an increase in positive charge in the nucleus as you go from left-to-right. Each time you go over an element it has one more electron and proton added to the principal energy level, so the nucleus pull increases and it holds the valence electron in tighter.
Atomic radius decreases because you are adding protons to the nucleus as you move from the left to the right of the period. These additional protons pull with more force on the electrons outside the nucleus, drawing them all in closer, and making the radius of the atom smaller.
Atomic radius is distance from centre of nucleus to the outer most shell of electrons of an atom.
As we go along a period the number of electron shells remain same. But the number of electrons in last shell as well protons in nucleus increase so the outer shell electrons are attracted by an increased amount of electrostatic force( as per coulomb's law) towards nucleus. So the outer shell electrons get closer to nucleus and atomic radius decreases.
The atomic radius actually decreases even as atomic number and mass increase as you go left to right across a period. This is because as you move left to right, you add valence electrons, which are the electrons in the outermost energy level of the atom. The positively charged nucleus of the atom interacts more strongly the more outer-level electrons there are (because oppositely charged bodies attact each other.) This binds the atom closer together, actually making the overall volume of the atom smaller, even though the mass, and therefore the density of that atom, increases. Most periodic trends are caused at least in part by the attraction between nucleus and electrons.
Atomic radius (size) decreases within a period going from left to right because within a period, all the elements have the same number of energy levels. Thus, the valence electrons are all within the same energy level meaning the same distance from the nucleus. However, as you move left to right, the number of protons in the nucleus increases, thus exerting a greater pull on those electrons. This results in a smaller radius.
Across a period, the effective nuclear charge increases. so size decreases.
Atomic radius decreases due to increase in effective nuclear charge.
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
As a general rule, when moving left to right on the periodic table the atomic radius decreases due to increasing electromagnetic attraction of the nucleus to the electrons.
ionization energy
yes
metal--> nonmetal --> metalloid
The atomic number increases
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
from left to right the atomic radius decreases as the electrons that get added are added in the same shell as they are in the same period. the shielding effect remains constant but the proton number increases which inturn increases the effective nuclear pull on the electrons bringing the electrons closer to the nuclei hence decreasing the radius of the atom
Atomic radii decreases on moving from left to right as the effective nuclear charge increases.
Yes.
decreases
As a general rule, when moving left to right on the periodic table the atomic radius decreases due to increasing electromagnetic attraction of the nucleus to the electrons.
ionization energy
they become more reactive since you are moving from left to right on the Periodic Table, the elements in group 17 are the most reactive.
It decreases across a period. Since the atomic number increases, so does no. of protons and electrons. This makes the electrostatic force of attraction between electrons larger and hence the atom shrinks a bit. This makes the radius smaller.
yes