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oxygen is more electronegative and so it wants the electron more than N
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∙ 15y ago
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Why are potassium and caesium rather than lithim used in photoelectric cells?
Potassium can loose electron easily . Comparatively Lithium have high ionisation energy and low level of loosing electron while absorbing light energy.
What 'Manufacturing fossil fuel energy is much less efficient than manufacturing?
Manufacturing fossil fuel energy is much less efficient than manufacturing _____.
Helium and neon cant form compounds with fluorine why?
The first Ionization energy of fluorine is less than that of the helium and neon.
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.
Manufacturing fossil fuel energy is much less efficient than manufacturing?
Manufacturing fossil fuel energy is much less efficient than manufacturing _____.
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
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 is the first ionisation energy of strontium larger than the first ionisation energy of rubidium?
Because, as we know that when we go across the period of the periodic table, the number of shells remain the same but the number of electrons and protons increases. So, Rb having its atomic number as 37 and Sr as 38, Strontium has got more nuclear charge as well as more electrons. As a result the first ionisation energy required to remove one electron is more in Strontium than Rubidium.
Why sulfur has a lower ionisation energy than phosphorus?
because it has many number of shells.
What is meant by the first ionisation energy of nitrogen?
THis is the energy required to remove(ionise) one (the first) outer most electron. For nitrogen this would be quite a large figure, because nitrogen, wants to accept electrons ,rather than remove electrons. As a general rule as you go along any given period, the ionisation energies increase. There are two 'humps', with a slight fall in ionisation energiers in this general increase.
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 boron has a lower first-ionization energy than beryllium?
Because in Boron there is a complete 2s orbital and the increased shielding of the 2s orbital reduces the ionisation energy compared to that seen in Beryllium.
Why oxygen have less ionisation enthalpy than fluorine?
Oxygen has a lower electronegativity than fluorine (3.5 as compared to 4).
Why does helium has a higher first ionization energy than argon?
The ionisation energy depends on the orbital from which the electron is removed and also the distance of the orbital from the nucleus. In the case of Helium, the electron is removed from 1s orbital whereas in the case of argon it is from 3p orbital. As 1s is closer to the nucleus, the force of attraction experience by these electrons is higher and hence helium will have higher 1st ionisation energy.
Is ionisation enthalpy of potassium higher than that of sodium?
The ionisation enthalpy of potassium is lower than that of sodium.
Why second ionisation energy is larger than the first ionisation energy?
The reason the second ionization energy is higher than the first relates to the attraction between the electrons and the nucleus. When one electron is removed from an atom, the neutral atom becomes positive. When one attempts to remove a second electron from a positive ion, there is more attraction between the electrons and the nucleus due to the extra proton. Thus, the second electron is harder to remove and the ionization requires more energy.
Why is the first ionization energy of aluminium is less than the first ionisation energy of silicon?
Al has atomic number 13, and silicon has atomic number 14. The extra electron that silicon has is in a 3p orbital. In simple terms the extra charge on the silicon nucleus contracts the electron shell, this increases the energy to remove an electron and also decreases the atomic radius. Al, first ionization energy 577.5 kJ/mol, atomic radius 125pm Si, first ionization energy 786.3 kJ/mol, atomic radius 110pm
