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Why the first ionisation energy of potassium is only a little less than the ionisation energy of sodium?
both are in the same period which accounts for closeness. they are nonetheless different because there are more protons in the nucleus which means electrons are brought closer to it so there is a higher ionisation energy or potential
What electronegativity difference is associated with a nonpolar covalent bond?
Less thann 0.5
Elements with high ionisation energy have?
1.A small atomic/ionic radius 2.therefore less number of protons 3. more net nuclear attraction between the positively charged nucleus 4. higher energy is needed to break those bonds. 5. therefore an element has high ionisation energy
Why the first ionisation energy of O is less than that of N?
oxygen is more electronegative and so it wants the electron more than N
Is the ionization energy of alkali metals larger or smaller than the alkaline earth metals in the same period?
It is about first ionization energy. It is less than alkaline earth metals.
Why does bromine have higher ionization energy then lead?
Bromine has less valence shells than lead making the distance between its valence electron and its nucleus less than that of lead. This means that there is greater attraction between the nucleus and electron for bromine and it requires a higher ionisation energy to remove its electron.
Why metal has lower ionisation energy?
Because the force of attraction between the nucleus and the outer most electron is less. In addition, most metals (but not all) will gain the stable electronic configuration of the nearest noble gas if they lose electron.
Why oxygen have less ionisation enthalpy than fluorine?
Oxygen has a lower electronegativity than fluorine (3.5 as compared to 4).
What generally happens to the first ionization energy of the element's within a period as the atomic number of the element's increases?
Ar P Al Na K In general the ionisation energy (this answer refers to first ionisation energy, although most of the principles mentioned here apply to all ionisation energies) increases as one moves across the period, this is due to an increasing nuclear charge and decreasing atomic radius (recall that F=(kq1q2)/r2 ). However there are exceptions to this, notably, on moving from group II to group III we see that ionisation energy decreases, like wise on moving from group V to group VI. The first of these decreases is a result of the additional electron occupying the p orbital (and therefore experiencing a lesser effective nuclear charge). The second decrease (which is less marked) is due to the additional electron being "placed" into an orbital already occupied by another electron (an electron pair is formed), these electrons have the same charge and therefore repel each other, as they are in the same orbital the repulsion is particularly strong, therefore the effective nuclear charge is less and first ionisation energy is lower. I hope this answer is acceptable, for more information see the Wikipedia article on electronic configuration.
What trend in ionization energy occurs going down on the periodic table and why?
when you go down a group you get more shells and in those shell are electrons the further away the electrons are from the protons and neutrons the less energy you need to pull of the electrons.
Which element is more reactive lithium or beryllium?
Lithium is wayy more reactive... like, duh? An elements reactivity depends on its ionisation energy (the amount of energy required to remove one electron from the atom) and if you look at a periodic table the ionisation energy is known to increase across the table and decrease down it. Berylium is further across the table than lithium so you'd expect it to have a lower ionisation energy and be less reactive. This is because beryllium (atomic number 4) has 4 protons, which cause a positive charge and subsequent attraction of electrons, while lithium has the atomic number 3 and therefore only has 3 protons to attract its electrons. Lithium is a Group I alkali metal, while Beryllium is a Group II alkaline earth metal. Group I Alkali metals are generally more reactive as they only need to lose one electron to have a complete outer shell.
Why do elderly require less energy?
They require less energy as they do not do much work compared to teenagers. They should have less energy intake and less energy expenditure.
