oxygen is more electronegative and so it wants the electron more than N
Manufacturing fossil fuel energy is much less efficient than manufacturing _____.
Nuclear energy.Nucular EnergyNuclear EnergyLess than 1 percent of the worlds commercial energy is supplied by the sun. Solar energy is an under-utilized source of energy.
Geothermal energy currently contributes to less than 1% of the world's energy supply.
Lithium is more reactive than beryllium. This is because lithium has one electron in its outer shell, making it easier for it to lose this electron and form positive ions compared to beryllium, which has two electrons in its outer shell.
Valence electrons occupy higher energy levels first before moving to lower energy levels, according to the aufbau principle. In calcium, the 4s orbital has lower energy than the 3d orbital, so valence electrons fill the 4s orbital first before the 3d orbital.
It is about first ionization energy. It is less than alkaline earth metals.
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
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.
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.
The ionization energy of boron is lower than that of beryllium because in boron, the electron being removed is farther from the nucleus, experiencing less of the nuclear charge, making it easier to remove. Additionally, boron's electron configuration involves removing an electron from a higher energy level, which requires less energy compared to removing an electron from a lower energy level in beryllium.
The second ionization energy for lithium is greater than the first because removing the second electron requires breaking a stronger bond due to the higher effective nuclear charge after the first electron is removed. This leads to a greater energy input to remove the second electron compared to the first.
The ionisation enthalpy of potassium is lower than that of sodium.
The first ionization energy of nitrogen is the energy required to remove one electron from a neutral nitrogen atom to form a positively charged nitrogen ion. It represents the strength of the bond between the electron and the nitrogen atom.
Yes, they are.
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.
Sulfur has a lower ionization energy than phosphorus because sulfur's valence electrons are in a higher energy level, making them easier to remove. Additionally, sulfur's smaller atomic size compared to phosphorus results in stronger nuclear attraction, requiring less energy to remove an electron.
because it lower than Ba as you go down ionization energy increases