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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.
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∙ 16y ago
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∙ 13y agoBecause as you go down a row in the Periodic Table you get more electrons around the nucleus. Because the nucleus is positively charged, as you add more electrons the attraction between the nucleus and the electrons gets stronger
Wiki User
∙ 11y agoBecause oxygen is having smaller size that selenium and hence the electrons are more tightly bound in oxygen than selenium. So, Oxygen has higher Ionization energy than Selenium
Wiki User
∙ 9y agoBecause PS II is non-cyclic whereas PS I is cyclic
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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.
What is the symbols for high and low pressure?
The letter H is used to represent a high pressure system.
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 P or Ca has the highest first ionization energy?
In general, ionization INCREASES as you move to the right and up in the periodic table, making P (Phosphorus) higher than Ca (Calcium).
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).
Why does the Earth have high and low tilts?
cuz the do ;P
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.
Why do non metals have higher ionization energies than metal?
Ionization energy is the energy needed to remove an electron. Elements other than transition metals gain or lose electrons from the s and p orbitals in order gain the more stable electron configuration of a Noble gas. Metals lose electrons to become isoelectronic (that is have the same electron configuration) to a noble gas (previous to them in the periodic table), while nonmetals tend to gain electrons in order to become isoelectronic to a Noble gas (next highest on the periodic table). Since ionization energy is the energy needed to REMOVE an electron, it is low for metals which form positive ions by losing electrons to become more stable, but very high for nonmetals that tend to gain, NOT LOSE, electrons. Most transition metals tend to lose electrons as well (other than Rhenium). Transition metals lose electrons from the d orbital, but still form positive ions, so their ionization energy is also usually lower than nonmetals.
Which one is more dangerous high BP or low BP Why?
High B.P. is more dangerous as we cannot prevent it like low B.P. If we have low B. P. we can prevent it by taking more salt contains. But high B.P. cannot be prevented by anything however there's a fewer chances by yoga but it cannot prevent totally. When B.P. becomes high our arteries burst and there's a chance for heart attack. So, high B. P. is dangerous than low B. P.
What is a area where the air pressure is high?
F=P*A where F is the force and P= pressure and A= area , so if pressure is high the area is to be low to keep the force constant
How are elements ordered by increasing ionization energy?
On the periodic table, ionization energy increases moving left to right within a period and up within a group. It decreases as the atomic radius increases in size.
Does a high wavelength have more energy than a low wavelength?
Your terminologies are inconsistent. Wave lengths are not high and low. They are long and short. Short wave (UHF) radio for example. There are two wave characteristics that can be termed high and low: amplitudes and frequencies. Assuming group S wave characteristics (e.g., water and light beam waves) the higher frequency and higher amplitude waves carry the most energy. Ditto for group P wave characteristics (e.g., seismic waves).
