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This is due to the electron configuration of Si vs. P. An electron added to P must go into a p orbital that already contains an electron. The electron that is already there repels the added electron and less energy is released during this electron addition, so the electron affinity is lower.
What else can I help you with?
Which atom or ion in each pair has the larger ionization energy Cl or P?
Chlorine, Cl. Elements with the most ionization energy are located at the top right corner of the periodic table. As you travel down a period the ionization energy increases, whereas travelling down a group the ionization energy decreases.
Is it ionization energy is a periodic property?
Ionization energy generally increases across a period as a result of a higher nuclear charge, however there are some exceptions such as Boron which has a lower ionization energy than Beryllium (because it is in a P orbital), and Oxygen which has a lower ionization energy than nitrogen (Because ionization decreases the electron electron repulsion in its orbitals).
What is the reason for decrease in first ionization energy energy from N to O and P to S?
The decrease in first ionization energy from nitrogen (N) to oxygen (O) and from phosphorus (P) to sulfur (S) is primarily due to electron-electron repulsion in filled or partially filled orbitals. In the case of oxygen, the addition of an electron to the already half-filled p-orbital leads to increased repulsion, making it easier to remove an electron compared to nitrogen. Similarly, for sulfur, the added electron in the p-orbital of sulfur experiences repulsion from other electrons, resulting in a lower ionization energy compared to phosphorus.
Why does the Earth have high and low tilts?
cuz the do ;P
How ionisation energy depends on penetration effect?
Ionization energy is influenced by the penetration effect, which refers to how effectively an electron can approach the nucleus. Electrons in orbitals with higher penetration (like s and p orbitals) experience a stronger attraction to the nucleus, leading to higher ionization energies. Conversely, electrons in orbitals with lower penetration (like d and f orbitals) are shielded from the nucleus by inner electrons, resulting in lower ionization energies. Thus, greater penetration generally correlates with higher ionization energy.
Which atom or ion in each pair has the larger ionization energy Cl or P?
Chlorine, Cl. Elements with the most ionization energy are located at the top right corner of the periodic table. As you travel down a period the ionization energy increases, whereas travelling down a group the ionization energy decreases.
How nature of orbitals affect ionization energy?
complexity of shapes of orbitals lead to increase in ionization energy. s orbital is spherical in shape, there is an equal tendency of finding an electron anywhere in the sphere so electron can easily be removed from gaseous atom. hence, ionization energy will be low. while in p orbitals dumb-bell shape provides a bit difficulty to occur electron everywhere with equal probability so it will lead to an increase in ionization energy.
Which element has a lower first ionization energy than element S?
Element P (phosphorus) has a lower first ionization energy than element S (sulfur).
Why is the ionization energy of oxygen less than that of nitrogen even if oxygen is to the right hand side of nitrogen?
half filled P orbitals increase the stability resulting in higher ionization energy
Is it ionization energy is a periodic property?
Ionization energy generally increases across a period as a result of a higher nuclear charge, however there are some exceptions such as Boron which has a lower ionization energy than Beryllium (because it is in a P orbital), and Oxygen which has a lower ionization energy than nitrogen (Because ionization decreases the electron electron repulsion in its orbitals).
What is the reason for decrease in first ionization energy energy from N to O and P to S?
The decrease in first ionization energy from nitrogen (N) to oxygen (O) and from phosphorus (P) to sulfur (S) is primarily due to electron-electron repulsion in filled or partially filled orbitals. In the case of oxygen, the addition of an electron to the already half-filled p-orbital leads to increased repulsion, making it easier to remove an electron compared to nitrogen. Similarly, for sulfur, the added electron in the p-orbital of sulfur experiences repulsion from other electrons, resulting in a lower ionization energy compared to phosphorus.
What exceptions are there in the increase of ionization energies across a period?
There is a slight decrease in ionization energy when moving from Group 2 to Group 13 due to the introduction of a new subshell (s to p transition), causing increased electron shielding. Additionally, there is a slight decrease in ionization energy when moving from Group 15 to Group 16 due to the stable half-filled p orbital that requires more energy to remove an electron.
Which element P or Ca has the highest first ionization energy?
The element P (Phosphorus) has a higher first ionization energy than Ca (Calcium). This is because Phosphorus has a smaller atomic size and higher effective nuclear charge compared to Calcium, making it harder to remove an electron from a Phosphorus atom than a Calcium atom.
Higher ionization energy Br or Bi?
Bismuth (Bi) has a higher ionization energy than bromine (Br) because bismuth is a larger atom with more electron shells, making it more difficult to remove an electron. Additionally, bismuth is in the p-block of the periodic table, where ionization energies generally increase across a period.
Why the elements in group 3A and 6A dips in ionization energy?
The elements in group 3A and 6A show a dip in ionization energy due to the presence of a full or half-full subshell. In group 3A, elements have a stable electronic configuration when one electron is removed, resulting in a lower ionization energy. In group 6A, elements exhibit a half-filled p orbital when one electron is added, making it easier to remove an electron and thus lowering the ionization energy.
Why does the Earth have high and low tilts?
cuz the do ;P
An atom has a first ionization energy of 496 kJmol and a second ionization energy of 4560 kJmol What group of the periodic table would the atom be in?
The significant jump in ionization energy from the first to the second indicates the removal of an electron from a filled energy level. This suggests the atom is in the second group of the periodic table, since elements in this group have a filled outer s sublevel before starting to fill the p sublevel in the subsequent period.
