The farther right you go along a Periodic Table, the more protons and elctectrons the atoms have. As the number of protons and electrons increases, the attraction between them increases, which draws the electrons closer to the nucleus (protons and neutrons), thus decreasing the atomic radii.
Atomic radii decreases from left to right in the periodic table
Atomic radii generally increase from top to bottom within a group (with more electron shells) and decrease from left to right across a period (due to increasing nuclear charge). This trend is influenced by the balance between the increasing positive nuclear charge and the increasing number of electron shells, which can shield the outer electrons from the nucleus.
No, the atomic radii of Mn (manganese) and Fe (iron) are not the same. Typically, atomic radii decrease across a period (from left to right on the periodic table), so Fe would have a smaller atomic radius compared to Mn.
As you move across a row on the periodic table, the atomic radii becomes smaller due to the attraction between positive protons and negative electrons. As you move down a column, the radii increase due to the addition of valance electrons.
The atomic radius decrease, with several exceptions in periods 6 and 5.
Atomic radii decreases from left to right in the periodic table
Atomic radii generally increase from top to bottom within a group (with more electron shells) and decrease from left to right across a period (due to increasing nuclear charge). This trend is influenced by the balance between the increasing positive nuclear charge and the increasing number of electron shells, which can shield the outer electrons from the nucleus.
Many properties change as you move from left to right on the periodic table. For example: atomic number increases; electronegativity increases; atomic radii decrease etc. etc.
The atomic radii decrease across a period because as you move from left to right, the number of protons and electrons in the atoms increases, leading to a stronger attraction between the nucleus and the outer electrons. This results in the electrons being pulled closer to the nucleus, making the atomic radius smaller.
No, the atomic radii of Mn (manganese) and Fe (iron) are not the same. Typically, atomic radii decrease across a period (from left to right on the periodic table), so Fe would have a smaller atomic radius compared to Mn.
Atomic radii decreases on moving from left to right as the effective nuclear charge increases.
Increases
I'm unable to graph atomic radii in this text-based format. However, you can find data on atomic radii for the first 20 elements in a periodic table resource or chemistry textbook. Atomic radii generally decrease across a period from left to right and increase down a group from top to bottom.
The radii of elements generally decrease as you move from left to right across a period in the periodic table. The radii then increase as you move down a group in the periodic table. This trend is due to changes in the atomic structure of the elements.
Atomic radii generally decrease across periods 3 through 6 in the periodic table. This is because as you move from left to right across a period, the number of protons and electrons increases, leading to stronger attraction between the nucleus and the electrons, pulling the outer electrons closer to the nucleus, thus decreasing the atomic radius.
The atomic radius decreases from left to right across a period in the periodic table. This is due to the increasing number of protons in the nucleus, which pulls the electrons closer to the nucleus, resulting in a smaller atomic radius.
The atomic radii of elements in period 3 from sodium to argon decrease due to a greater nuclear charge pulling electrons closer to the nucleus. This trend is similar to period 2 because both periods follow the same pattern of increasing nuclear charge as you move across the period, leading to a similar decrease in atomic radii.