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this occurs because of the shielding effect of inner electrons.as we go down the group- number of electronic shells increases, which restricts the outer most electrons from being attracted by the protons of nucleus.as the result of this effect the outer most electrons are loosely attracted by the nucleus,resulting the increase of atomic radii.hence making it easier for atoms to lose electrons down the group.
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What element in Group 1 has the largest atoms?
Cesium, which is in Group 1 of the periodic table, has the largest atoms. This is because as you move down a group, the atomic size generally increases due to the addition of more electron shells.
Why alkali metal density increase going down the group?
The alkali metal density increases going down the group because the atoms have more electron shells as you go down the group, resulting in a larger atomic size. The increased number of electron shells leads to weaker attractive forces between the nucleus and the outermost electron, causing the atoms to be less compact and have lower densities.
The size of atoms has most to do with its?
The size of atoms is primarily determined by the arrangement of electrons in the electron cloud surrounding the nucleus. The number of electron shells and the effective nuclear charge also play a role in determining the size of atoms. Additionally, the atomic radius of atoms generally increases as one moves down a group and decreases across a period on the periodic table.
Why Thermal stability increases when going down the group?
Thermal stability increases down a group because the atomic size increases, leading to weaker intermolecular forces and greater distance between atoms, making it harder for the atoms to come together and react. Additionally, the lower electronegativity of larger atoms down the group makes them less likely to form covalent bonds with other atoms, enhancing their thermal stability.
What is happening to the elements electronic structures in group 1?
In Group 1 of the periodic table, the elements have one valence electron. As you move down the group, the size of the atoms increases due to the addition of more energy levels. As a result, the outermost electron becomes further away from the positively charged nucleus and more shielded by inner electrons. Thus, the electronic structure remains similar, with one valence electron, but the atoms become larger in size.
As you go down in group 1 why do the atoms get bigger in cross section?
As you go down Group 1, the atoms get bigger due to the addition of energy levels (shells) in which electrons can be found. This results in more electron-electron repulsions, causing the atoms to expand in size. Additionally, the increased number of electron shells further away from the nucleus leads to a larger atomic radius.
What happens to the size of atoms down group 1?
The atoms increase in size, because they gain more electron energy shells.
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 element in Group 1 has the largest atoms?
Cesium, which is in Group 1 of the periodic table, has the largest atoms. This is because as you move down a group, the atomic size generally increases due to the addition of more electron shells.
Why alkali metal density increase going down the group?
The alkali metal density increases going down the group because the atoms have more electron shells as you go down the group, resulting in a larger atomic size. The increased number of electron shells leads to weaker attractive forces between the nucleus and the outermost electron, causing the atoms to be less compact and have lower densities.
Why does Lewis acid strength of boron trihalides decreases down the group in periodic table?
The Lewis acid strength of boron trihalides decreases down the group because the size of the halogen atom increases as you move down the group, leading to a weaker attraction between the halogen atom and the electron deficient boron center. Additionally, the ability of the larger halogen atoms to share their electron density with boron decreases, making the boron trihalides less likely to act as Lewis acids.
How does the reactivity of halogens change as you go down group 7?
As you go down group 7 (halogens), reactivity decreases. This is because as you move down the group, the outer electron shells of the halogens are further away from the nucleus, making it harder for them to gain an electron and react with other elements. Additionally, the atomic size increases which leads to weaker intermolecular forces between the atoms.
The size of atoms has most to do with its?
The size of atoms is primarily determined by the arrangement of electrons in the electron cloud surrounding the nucleus. The number of electron shells and the effective nuclear charge also play a role in determining the size of atoms. Additionally, the atomic radius of atoms generally increases as one moves down a group and decreases across a period on the periodic table.
What is the Atomic polarizability trend?
The atomic polarizability generally increases down a group and decreases across a period. This trend occurs because atoms with larger electron clouds (such as larger atomic size) are more easily polarized. Additionally, atoms with higher electronegativity tend to have lower polarizability due to stronger electron-electron repulsion.
Why Thermal stability increases when going down the group?
Thermal stability increases down a group because the atomic size increases, leading to weaker intermolecular forces and greater distance between atoms, making it harder for the atoms to come together and react. Additionally, the lower electronegativity of larger atoms down the group makes them less likely to form covalent bonds with other atoms, enhancing their thermal stability.
Why does not the nucleus attract the atoms from top to bottom in a periodic table?
Down a group, the number of shell increases and the electron enters into a different shell. Hence, the distance between the nucleus and valence electron increases and the nuclear attraction decreases
What is happening to the elements electronic structures in group 1?
In Group 1 of the periodic table, the elements have one valence electron. As you move down the group, the size of the atoms increases due to the addition of more energy levels. As a result, the outermost electron becomes further away from the positively charged nucleus and more shielded by inner electrons. Thus, the electronic structure remains similar, with one valence electron, but the atoms become larger in size.
