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What else can I help you with?
What periodic treds exist for ionization energy?
Ionization energy increases to the right and up on the periodic table. Ionization energy is the energy required to remove an electron. It can be conceptualized as the opposite of electron affinity, though this is not precisely true.
Use ionization energy to explain why metals lose electrons more easily than nonmetals?
Metals lose electrons more easily than the non-metals because they require less ionization energy compared with the non-metals. The metals require less ionization energy to lose the electrons than though gain the electrons unlike the non-metals.
Why does ionization energy decrease down the family?
You question is not very clearly stated but I think I know what you are asking. As you go down the column of any family of elements in the periodic table, you move to increasingly heavier and larger atoms. Their outer electrons are therefore farther from the nucleus, and even though the nucleus is larger and has a larger positive charge, the increased distance is the predominant influence, making the outermost electrons less tightly bound, and therefore more easily ionized, with a lower ionization energy.
What elements have the same ionization energy?
None of them do exactly. The elements' ionization energies definitely trend in a couple of ways though. The ionization energy variations tend to decrease as atomic number goes up and tend to increase as you remove more electrons from the atom.
Which has larger atomic size F or F ion?
Ionization energy increase across a period and decreases down a group, therefore the the element with the greater ionization energy would be found in the top right of the periodic table. In this instance fluorine, F would have the greater ionization energy.
What does ionization energy remove from an atom of an element?
Ionization energy and electron affinity for cations and anions, respectively.
Can something small have more thermal energy than something big?
Yes, a small object can have more thermal energy than a larger object if it has a higher temperature. Thermal energy is directly proportional to temperature, so even though the larger object has more mass, the smaller object could have a higher temperature and therefore more thermal energy.
Did Magellan find what he expected?
no, he died halfway though his journey
Can a body of larger mass be hotter than another body of smaller mass if they are at the same temperature?
No. "Temperature" means "how hot it is". (The larger mass could have more or less heat energy in it, though. Even if they're both at the same temperature.)
Why does He have a higher first ionization energy than Ne?
Helium has a higher first ionization energy than neon because helium has a smaller atomic size and a full valence shell of electrons, making it more stable. Neon, while still a noble gas with a full valence shell, has a larger atomic size and therefore experiences less nuclear attraction on its outermost electron, making it easier to remove compared to helium.
What is the first ionization energy for xenon?
It's going to be pretty high, since xenon is a noble gas, and doesn't naturally react with anything, therefore it's not going to naturally want to lose an electron. It can be made to, however, and it's a lot easier for it to lose one than any noble gas above it, because xenon's octet of valence electrons is farther from the nucleus than the others (except radon) so a. it will have a lower ionization energy, b. the octet will experience more nuclear shielding, and c. it will be potentially more reactive (though again, it's not natural.) The actual ionisation energy is 1170.36 kJ per mole
A small hot thing may contain less energy than a larger cooler thing?
Yes, a small hot object can contain less total energy than a larger cooler object because the temperature of an object is not solely determined by its size but also by its mass and specific heat capacity. So, even though the small hot object may have a higher temperature, the larger cooler object can still contain more energy overall.
