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Why does the change for the atomic radii of the elements for period 3 from sodium to argon look similar to period 2?
Because the trend is the same. Atomic radius decreases from left to right across a period.
Do the elements to the right of the periodic table have small or large radii?
Elements to the right of the periodic table have smaller radii due to increased effective nuclear charge, which attracts the electrons closer to the nucleus. This results in a greater pull on the outer electrons and smaller atomic radii overall.
In the same period what have large atomic radii alkali metals or noble gases?
Noble gases have larger atomic radii than alkali metals in the same period.
What happens to the atomic radii of the elements as a group is descended?
As we descend down the group, the atomic radii increases. This is because the number of shells increases.
What is the relationship between the atomic numbers and ionic radii of the elements in the group 3A?
I think that the ionic radii decrease
Why does the change for the atomic radii of the elements for period 3 from sodium to argon look similar to period 2?
Because the trend is the same. Atomic radius decreases from left to right across a period.
Why does the change for the atomic radii of elements in period 3 from sodium to argon look similar to period 2?
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.
Graph the atomic radii for the first 20 elements?
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.
What group of elements have members of the smallest atomic radii for a given period?
The group of elements with members of the smallest atomic radii for a given period is the group of noble gases. Noble gases have the smallest atomic radii because they have a completely filled valence shell, which results in strong electron-electron repulsions and a smaller atomic size.
Why are the ionic radii of metallic elements smaller than the atomic radii of the same elements?
The ionic radii of metallic elements is smaller than its atomic radii, because the ion has less electrons. This gives it a smaller electron cloud and makes the atom smaller.
What happens to the radii of the elements between 2 highest peaks?
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.
Do the elements to the right of the periodic table have small or large radii?
Elements to the right of the periodic table have smaller radii due to increased effective nuclear charge, which attracts the electrons closer to the nucleus. This results in a greater pull on the outer electrons and smaller atomic radii overall.
How can you find out the atomic radii?
Look for a reference chart in a book or online. Look for a Periodic Table of the Elements that has the atomic radii on it.
What common characteristic is generally shared by the elements at the center of a period?
Elements at the center of a period tend to have the highest electronegativity and smallest atomic radii compared to the other elements in the period. Additionally, these elements often possess a stable electron configuration.
In the same period what have large atomic radii alkali metals or noble gases?
Noble gases have larger atomic radii than alkali metals in the same period.
What happens to the atomic radii of the elements as a group is descended?
As we descend down the group, the atomic radii increases. This is because the number of shells increases.
Why are the ionic radii of nonmetallic elements larger than the atomic radii of those elements?
When nonmetallic elements gain electrons to form ions, the additional electrons are added to higher energy levels (shells) farther from the nucleus. This increase in the size of the electron cloud leads to an increase in the ionic radii compared to the atomic radii of those elements.
