How does the atomic radius generally change across period 2?

How does the atomic radius generally change across period 2?

Periodic Trend The atomic radius of atoms generally decreases from left to right across a period. The effect lessens as one moves further to the right in a period because of electron-electron repulsions that would otherwise cause the atom’s size to increase.

How does atomic radius vary across a period?

Atomic radius generally decreases from left to right across a period. This is because within a period, the outer electrons are present in the same valence shell and the atomic number increases from left to right across a period, resulting in an increased effective nuclear charge.

What is the trend for atomic radius across a period horizontally?

Atomic radius decreases across a period because valence electrons are being added to the same energy level at the same time the nucleus is increasing in protons.

Why does the atomic radii decrease across a period?

Across a period, effective nuclear charge increases as electron shielding remains constant. A higher effective nuclear charge causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius.

How does atomic size vary along period 2 from left to right and why?

Experiments have shown that the first case is what happens: the increase in nuclear charge overcomes the repulsion between the additional electrons in the valence level. Therefore, the size of atoms decreases as one moves across a period from left to right in the periodic table.

Why does reactivity decrease across a period?

Period – reactivity decreases as you go from left to right across a period. The farther to the left and down the periodic chart you go, the easier it is for electrons to be given or taken away, resulting in higher reactivity. Group – reactivity decreases as you go down the group.

How do atomic radii vary in a group and why?

Atomic radius generally decreases from left to right across a period. On the other hand, the atomic radius generally increases down a group. This is because down a group, the principal quantum number (n) increases which results in an increase of the distance between the nucleus and valence electrons.

Why does the atomic radii increase?

The gain of an electron adds more electrons to the outermost shell which increases the radius because there are now more electrons further away from the nucleus and there are more electrons to pull towards the nucleus so the pull becomes slightly weaker than of the neutral atom and causes an increase in atomic radius.

What is the trend in atomic radius across a period?

Periodic Trend. The atomic radius of atoms generally decreases from left to right across a period. There are some small exceptions, such as the oxygen radius being slightly greater than the nitrogen radius. Within a period, protons are added to the nucleus as electrons are being added to the same principal energy level.

How does ionic radius change across a period?

Atomic radius decreases across a Period, from left to right, of the Periodic Table 2 . Note trends for ionic radii: ionic radius of a cation is less than atomic radius of the atom ionic radius of an anion is greater than atomic radius of the atom ionic radii of group 1 cations increases down the group

What happens to atomic radius as you move down a group?

Atomic Radius Trend 2: Atomic Radii Increase as You Move Down a Group The second atomic radius periodic trend is that atomic radii increase as you move downwards in a group in the periodic table. For each group you move down, the atom gets an additional electron shell.

How do atomic radii change across the periodic table?

One atomic radius trend occurs as you move left to right across the periodic table (moving within a period), and the other trend occurs when you move from the top of the periodic table down (moving within a group). Below is a periodic table with arrows showing how atomic radii change to help you understand and visualize each atomic radius trend.