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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.
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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.
Why do radii of atoms become smaller from sodium to chlorine?
The atomic radii decrease from sodium to chlorine due to the increase in effective nuclear charge as you move across the period. This results in a stronger pull on the valence electrons, causing the atomic size to decrease. Additionally, the increased number of protons in the nucleus as you move from sodium to chlorine also contributes to this decrease in atomic size.
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 trend in atomic radii do periods 3 through 6 have in common in the periodic table?
Atomic radii generally decrease across periods 3 through 6 in the periodic table. This is because as you move from left to right across a period, the number of protons and electrons increases, leading to stronger attraction between the nucleus and the electrons, pulling the outer electrons closer to the nucleus, thus decreasing the atomic radius.
How are period and group trends in atomic radii are related to electron configuration?
Period trends in atomic radii show a decrease across a period due to increasing nuclear charge and more protons pulling electrons closer. Group trends in atomic radii show an increase down a group due to additional energy levels being added, leading to larger atomic size. Electron configuration influences these trends by determining the number of energy levels and electron shielding in an atom, affecting the distance of the outer electrons from the nucleus.
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.
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.
As you go from left to right across a period the atomic radii does what?
Increases
Why do radii of atoms become smaller from sodium to chlorine?
The atomic radii decrease from sodium to chlorine due to the increase in effective nuclear charge as you move across the period. This results in a stronger pull on the valence electrons, causing the atomic size to decrease. Additionally, the increased number of protons in the nucleus as you move from sodium to chlorine also contributes to this decrease in atomic size.
Are the atomic radii of Mn and Fe same?
No, the atomic radii of Mn (manganese) and Fe (iron) are not the same. Typically, atomic radii decrease across a period (from left to right on the periodic table), so Fe would have a smaller atomic radius compared to Mn.
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 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.
What trend in atomic radii do periods 3 through 6 have in common in the periodic table?
Atomic radii generally decrease across periods 3 through 6 in the periodic table. This is because as you move from left to right across a period, the number of protons and electrons increases, leading to stronger attraction between the nucleus and the electrons, pulling the outer electrons closer to the nucleus, thus decreasing the atomic radius.
How do the radii of metals in each period compare with the radii of nonmetals in that period?
In each period of the periodic table, the atomic radii of metals are generally larger than those of nonmetals. This is due to the fact that metals tend to have fewer valence electrons and a weaker effective nuclear charge, allowing their outer electrons to be located further from the nucleus. In contrast, nonmetals have higher electronegativity and stronger nuclear attraction, resulting in smaller atomic radii. As you move from left to right across a period, the atomic radii of both metals and nonmetals decrease, but the difference in size between the two categories remains consistent.
How are period and group trends in atomic radii are related to electron configuration?
Period trends in atomic radii show a decrease across a period due to increasing nuclear charge and more protons pulling electrons closer. Group trends in atomic radii show an increase down a group due to additional energy levels being added, leading to larger atomic size. Electron configuration influences these trends by determining the number of energy levels and electron shielding in an atom, affecting the distance of the outer electrons from the nucleus.
How does atomic radii increase or decrease in the table?
Atomic radii generally increase from top to bottom within a group (with more electron shells) and decrease from left to right across a period (due to increasing nuclear charge). This trend is influenced by the balance between the increasing positive nuclear charge and the increasing number of electron shells, which can shield the outer electrons from the nucleus.
What element does not fit atomic radii trend?
In the context of atomic radii trends, helium is an element that does not fit the general trend. Typically, atomic radii decrease across a period from left to right due to increasing nuclear charge, but helium has an unexpectedly small atomic radius compared to other noble gases. This is primarily due to its strong effective nuclear charge and the limited electron shielding in its small electron cloud, leading to a compact atomic size.
