because it lower than Ba as you go down ionization energy increases
Ba has greater nuclear charge than than Ra due to difference in energy levels thus it has greater electrostatic attraction which makes it to have bigger ionisation energy
First ionization energy of magnesium = 870/ kj/mol First ionization energy of phosphorous = 589 kj/mol So, magnesium has the larger ionization energy required to pull the first valance electron. Do you know why?
Ne (Highest First Ionization Energy) C Be Mg Sr (Lowest First Ionization Energy)
Because with the 2nd ionisation of K, you are trying to take an electron from a fully filled orbital (octet rule) whereas with calcium it is getting down to a fully filled orbital
You could draw it using Lewis structures, where valence electrons are represented by dots. You can also express it in equation form. The first ionization of calcium, for instance, could be expressed as: Ca --> Ca+ + e- As you can see, neutral calcium loses an electron to form the calcium +1 cation. Of course, we know that calcium will lose another electron as well, which can be expressed in the equation for the second ionization of calcium: Ca+ --> Ca++ + e- Normally, calcium will not experience a third ionization, because with two valence electrons, it has now achieved a full octet and is isoelectronic with argon.
No it has high ionization potential compared to Na, K. This is because it has a very small atomic radius so there is more attraction of the nucleus to the electrons. So it is not easy to remove electrons from it when compared to Na and K.
In general, ionization INCREASES as you move to the right and up in the periodic table, making P (Phosphorus) higher than Ca (Calcium).
First ionization energy of magnesium = 870/ kj/mol First ionization energy of phosphorous = 589 kj/mol So, magnesium has the larger ionization energy required to pull the first valance electron. Do you know why?
Ne (Highest First Ionization Energy) C Be Mg Sr (Lowest First Ionization Energy)
The Chemical equation of calcium hydroxide is Ca(OH)2
Because with the 2nd ionisation of K, you are trying to take an electron from a fully filled orbital (octet rule) whereas with calcium it is getting down to a fully filled orbital
You could draw it using Lewis structures, where valence electrons are represented by dots. You can also express it in equation form. The first ionization of calcium, for instance, could be expressed as: Ca --> Ca+ + e- As you can see, neutral calcium loses an electron to form the calcium +1 cation. Of course, we know that calcium will lose another electron as well, which can be expressed in the equation for the second ionization of calcium: Ca+ --> Ca++ + e- Normally, calcium will not experience a third ionization, because with two valence electrons, it has now achieved a full octet and is isoelectronic with argon.
No it has high ionization potential compared to Na, K. This is because it has a very small atomic radius so there is more attraction of the nucleus to the electrons. So it is not easy to remove electrons from it when compared to Na and K.
Calcium has the larger atomic radius than chlorine. Calcium has four energy levels, whereas chlorine has three energy levels. The higher the energy level, the farther it is from the atomic nucleus.
They ca fill their outmost energy level by gaining or losing electrons.
Both the degrees have there own important. CA is 50 times more tough than MBA. CA qualified individual earn a lot when compare to the MBA student. But again it depends on geographical location. If the demand of MBA is high we will get a higher pay check.
Coastal areas tend to get more storm damage than inland areas.
True. Although lithium is an alkali metal it is quite different from the other alkali metals. In fact it can generally behave more like an alkaline earth metal, such as Magnesium (Mg), Calcium (Ca) Strontium (Sr) and Barium (Ba). One of the major characteristics of the alkali metals is their low ionization energy, which is why lithium can easily be present in its ionic form of Li+. However, lithium posses the highest ionization energy of the alkali metals