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Cations are most often metals, as cations are positively charged ions meaning they have lostelectron(s). As a general rule, metals are on the left-hand side of the Periodic Table. Since cations tend to lose electrons, their atomic radius will decrease in size, as the other electrons will be "pulled in" more by the protons in the nucleus (meaning stronger bond). This results in the atomic radius decreasing.
Anions on the other hand are most often nonmetals, as anions are negatively charged ions meaning they have gained electron(s). As a general rule, nonmetals are on the right-hand side of the periodic table. Since anions tend to gain electrons, their atomic radius will increase in size, as the newly added electrons will "shield" the other electrons from the nucleus, meaning they will be less attracted to the protons in the nucleus (meaning weaker bond). This results in the atomic radius increasing.
Note that the above trends mentioned apply mostly to the Group A elements. Many of the transition elements for covalent bonds, meaning they share electrons with other atoms, rather than giving or taking electrons from other atoms. However, many transition metals actually form cations, although there are some exceptions.
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How do the ionic radii vary within a group of metals?
In a group of metals, ionic radii tend to increase as you move down the group. This is because the outermost electron shell becomes farther from the nucleus as you move down the group, leading to larger atomic sizes and therefore larger ionic radii.
How do the ionic radii vary within a group of metals how do they vary within a group of nonmetals?
Within a group of metals, the ionic radii generally increase as you move down the group due to the addition of higher energy levels. Within a group of nonmetals, the ionic radii also increase as you move down the group due to the addition of higher energy levels, but they are typically smaller compared to metal ions of the same period.
Explain the large decrease in atomic radii as you move across a period from group 1 to group 14?
The decrease in atomic radii across a period from group 1 to group 14 is mainly due to increasing effective nuclear charge. As you move across a period, the number of protons in the nucleus increases, pulling the electrons closer to the nucleus. This results in a stronger attraction between the nucleus and the electrons, leading to a decrease in atomic size.
How the ionic radii vary within a group of metals and minerals?
In a group of metals and minerals, ionic radii typically decrease going down the group. This is due to the increasing number of electron shells as you move down the group, causing the outer electrons to be further from the nucleus and increasing the overall size of the ion. However, there can be exceptions based on the electronic configuration of the elements involved.
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.
How do the ionic radii vary within a group of metals?
In a group of metals, ionic radii tend to increase as you move down the group. This is because the outermost electron shell becomes farther from the nucleus as you move down the group, leading to larger atomic sizes and therefore larger ionic radii.
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 trend can be observed among the atomic radii of main-group elements down a group?
The atomic radii of main-group elements generally increase down a group. This is because as you move down a group, the principal quantum number increases, leading to larger atomic orbitals and a greater distance between the nucleus and the outermost electron, resulting in a larger atomic radius.
How do the ionic radii vary within a group of metals how do they vary within a group of nonmetals?
Within a group of metals, the ionic radii generally increase as you move down the group due to the addition of higher energy levels. Within a group of nonmetals, the ionic radii also increase as you move down the group due to the addition of higher energy levels, but they are typically smaller compared to metal ions of the same period.
Explain the large decrease in atomic radii as you move across a period from group 1 to group 14?
The decrease in atomic radii across a period from group 1 to group 14 is mainly due to increasing effective nuclear charge. As you move across a period, the number of protons in the nucleus increases, pulling the electrons closer to the nucleus. This results in a stronger attraction between the nucleus and the electrons, leading to a decrease in atomic size.
How the ionic radii vary within a group of metals and minerals?
In a group of metals and minerals, ionic radii typically decrease going down the group. This is due to the increasing number of electron shells as you move down the group, causing the outer electrons to be further from the nucleus and increasing the overall size of the ion. However, there can be exceptions based on the electronic configuration of the elements involved.
In the alkaline-earth group atoms with the smallest radii?
Atoms with the smallest radii in the alkaline-earth group are found at the top of the group, such as beryllium. This is because as you move down the group, additional electron shells are added, increasing the atomic radius.
What is the ionic radius trend across a period?
Atoms increase in size as you go down a column and are larger going from right to left across a row.because while going from left to right in a period electrons enter in the same orbit and hence the attraction between the nucleus increasees
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 is the trend in atomic radius down a group explain?
The trend in atomic radius increases down a group. This is because as you move down a group, each element has an additional energy level of electrons, leading to a larger atomic radius. The increased number of electron shells results in greater electron-electron repulsion, causing the outermost electrons to be pushed farther away from the nucleus, thus increasing the atomic radius.
What is the relationship of atomic radii for each pair of species shown below?
The relationship of atomic radii for each pair of species shown below is that the atomic radius increases as you move down a group on the periodic table and decreases as you move across a period from left to right.
Why reactivity of metal increases down the group?
As we go down the group, nuclear charge deceases and atomic radii increases. So the element can easily lose electron and hence react.
