From going left to right on a period, the electrons are filled in the same shell. The atomic number increases, hence the number of protons in the nucleus increases. The effective nuclear charge thus increases. As a result the nucleus exerts more attraction on the valence electrons and hence the size / radius decreases.
Atomic size generally decreases as you move across a period from left to right due to increasing effective nuclear charge. However, atomic size tends to increase as you move down a group due to the addition of more electron shells.
decreases
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.
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 decrease in atomic radius as you move across a period on the periodic table is primarily due to increasing nuclear charge and the attraction between the positively charged nucleus and the negatively charged electrons. This stronger attraction pulls the electrons closer to the nucleus, resulting in a smaller atomic radius.
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.
The atomic number increases
Atomic size generally decreases as you move across a period from left to right due to increasing effective nuclear charge. However, atomic size tends to increase as you move down a group due to the addition of more electron shells.
decreases
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.
The atomic radius decrease, with several exceptions in periods 6 and 5.
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.
Atomic radius tends to decrease across a period from left to right. This is because as you move across a period, the number of protons in the nucleus increases, leading to an increase in the effective nuclear charge felt by the outermost electrons, which pulls them closer to the nucleus.
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.
The decrease in atomic radius as you move across a period on the periodic table is primarily due to increasing nuclear charge and the attraction between the positively charged nucleus and the negatively charged electrons. This stronger attraction pulls the electrons closer to the nucleus, resulting in a smaller atomic radius.
atomic size decreases across a period
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.