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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).
Why does the Earth have high and low tilts?
cuz the do ;P
What type of organic compound has high energy bonds?
One that I can think of off the top of my head is Adenosine Triphosphate or ATP. It is the molecule that supplies almost all of your energy in the last covalent bond in the structure. It has three phosphates at the end of it, so imagine...(Rest of molecule)-P-P-P^all the energy is stored here in that bond. When the bond breaks, it releases energy, then forming ADP, or Adenosine Diphosphate.
Which energy levels do not have p orbital?
The energy levels that do not have p orbitals are the first and second energy levels. The first energy level (n=1) contains only an s orbital, while the second energy level (n=2) has both s and p orbitals. Starting from the third energy level (n=3), s, p, and d orbitals are present.
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 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.
Four factors that affect ionization energy?
Size of the atomAs the size of the atom increases the outermost electrons are held less tightly by the nucleus (attractive force between the electron and the nucleus is inversely proportional to the distance). As a result it becomes easier to remove the electron and therefore the ionization energy decreases with the increase in atomic size. Charge on the nucleusThe attractive force between the nucleus and the electron increases with the increase in nuclear charge making it more difficult to remove an electron. The ionization energy thus increases with the increase in the nuclear charge. Screening effectIn multielectron atoms, the outermost electrons are shielded or screened from the nucleus by the inner electrons. This is known as shielding or screening effect. The outer most electrons do not feel the complete charge of the nucleus and the actual charge felt is called the effective nuclear charge. When the inner electrons are more, the screening effect will be large, the nuclear attraction will be less. Thus when the inner electrons increase the ionization energy will decrease. Penetration effectThe 's' electrons are more penetrating (maximum probability of finding near the nucleus) towards the nucleus than the p electrons. The order of penetration power in a given shell is s > p > d > f If the penetration power of the electron is more, it will be closer to the nucleus and will be held more firmly. Thus ionization energy will increase with the increase in the penetration power of the electrons. For the same sub shell the ionization energy would be more to remove an 's' electron than to remove a 'p' electron which in turn will be more than that for removing a 'd' electron.Electronic arrangementCertain electronic configuration like half-filled and completely-filled shells have extra stability. It is more difficult to remove electron from these stable configuration and the ionization energy is very high. For example, the noble gases have the most stable configuration and so have high ionization energy; elements like Be and Mg have completely filled orbitals while N and P have exactly half-filled sub shells. Thus, their ionization energies are high. The more stable the electronic configuration, the higher is the ionization energy.
