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As you go across a period, radius shrinks because you are adding protons. The added positive charge increases pull on the electron shells.
As you go down a group, radius gets larger because you are increasing shells of electrons. This increases shielding of the nucleus' positive charge, so the electrons are not pulled in as much.
What else can I help you with?
What is the Group trend Atomic radius?
The group trend for atomic radius is that it tends to increase down a group in the periodic table. This is because as you move down a group, the number of electron shells increases, leading to a larger atomic radius. Additionally, the effective nuclear charge decreases down a group, which also contributes to the increase in atomic radius.
How does calcium's atomic radius compared to magnesium radius and potassium radius?
The atomic radius of calcium is larger than magnesium but smaller than potassium. This trend is consistent with the periodic trend across Group 2 elements where atomic radius increases down the group due to additional electron shells. Additionally, going across a period from left to right, atomic radius decreases due to increasing nuclear charge pulling electrons closer.
How does calcium atomic radius compare to magnesiums radius and potassiums radius?
Calcium has a larger atomic radius than magnesium and a smaller atomic radius than potassium. This trend is due to the increase in number of protons and electrons as you move across the period on the periodic table from magnesium to calcium to potassium.
Which has the larger radius Na or Mg?
Mg has a larger atomic radius than Na. This is because atomic radius generally increases as you move down a group in the periodic table, and Mg is below Na in the same group. Additionally, Mg has more energy levels and electrons compared to Na, contributing to its larger atomic radius.
What pattern or trend do you notice between atomic radius and electronegativity energy?
As atomic radius increases, electronegativity generally decreases. This trend occurs because as the atomic radius increases, the distance between the nucleus and valence electrons increases, resulting in weaker attraction between the nucleus and outer electrons. Consequently, atoms with larger atomic radii tend to have lower electronegativities.
What is the Group trend Atomic radius?
The group trend for atomic radius is that it tends to increase down a group in the periodic table. This is because as you move down a group, the number of electron shells increases, leading to a larger atomic radius. Additionally, the effective nuclear charge decreases down a group, which also contributes to the increase in atomic radius.
Can you describe the general trend in atomic radius in group 2A?
In the group 2 (IUPAC name) of the periodic table the atomic radius increase from beryllium to radium.
How does calcium's atomic radius compared to magnesium radius and potassium radius?
The atomic radius of calcium is larger than magnesium but smaller than potassium. This trend is consistent with the periodic trend across Group 2 elements where atomic radius increases down the group due to additional electron shells. Additionally, going across a period from left to right, atomic radius decreases due to increasing nuclear charge pulling electrons closer.
Is the pattern of atomic radius absolute or general?
The pattern is a general trend that is very consistant
Do transition elements follow the same trend of atomic radius as the main group elements?
NO
What trend does the atomic radius along a period on the periodic table?
The atomic radius decreases along a period. It is because of increasing effective nuclear charge along a period.
How does calcium atomic radius compare to magnesiums radius and potassiums radius?
Calcium has a larger atomic radius than magnesium and a smaller atomic radius than potassium. This trend is due to the increase in number of protons and electrons as you move across the period on the periodic table from magnesium to calcium to potassium.
WHAT BEST STATES THE TREND IN ATOMIC RADIUS ACROSS THE PERIODIC TABLE?
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.
What explains the observed trend in the atomic radii going down the periodic table?
The more energy levels that are occupied by electrons, the larger the atomic radius.
How do you account for the general trend in atomic radius across a row of elements?
The general trend in atomic radius across a row of elements decreases from left to right due to increasing effective nuclear charge, which attracts the electrons closer to the nucleus. As you move across a period, the number of protons in the nucleus increases, resulting in a stronger pull on the electrons and a decrease in atomic radius. Additionally, the shielding effect of inner electrons remains relatively constant, further contributing to the trend.
What trend does the atomic radius follow along period on the periodic table?
The atomic radius gets smaller the farther right it appears on the Periodic Table, until the addition of a new orbital increases the size again.
What trend does the atomic radius following along period on the periodic table?
The atomic radius gets smaller the farther right it appears on the Periodic Table, until the addition of a new orbital increases the size again.
