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What is the first law of thermodynamics equation and how does it relate to the conservation of energy in a thermodynamic system?
The first law of thermodynamics equation is: U Q - W. This equation states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system. This equation relates to the conservation of energy in a thermodynamic system because it shows that energy cannot be created or destroyed, only transferred between different forms (heat and work) within the system.
What is the energy of a photon of 325nm?
The energy of a photon is determined by the equation E = hf, where E is energy, h is Planck's constant (6.626 x 10^-34 J s), and f is the frequency of the photon. First, calculate the frequency of the photon using the speed of light equation, c = λf. Then, substitute the frequency into the energy equation to find the energy of the photon.
How do you calculate displacement of an object using the work-energy equation?
To calculate displacement using the work-energy equation, first calculate the work done on the object using the force applied and the distance moved. Then, equate the work done to the change in kinetic energy of the object using the work-energy equation: Work = Change in kinetic energy = 0.5 * mass * (final velocity^2 - initial velocity^2). Finally, rearrange the equation to solve for displacement.
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.
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.
What is ionisation energy What is first ionisation energy?
The first ionization energy of an atom or molecule describes the amount of energy required to remove an electron from the atom or molecule in the gaseous state.
First ionisation energy?
the first ionisation energy is the energy required to remove the first most loosely bound elecctron from a neutral gaseous atom in its ground state.
What happens to the first ionisation energy of the elements as a period is crossed?
tinger tinger tales
Which Lewis structure represent an atom x in period 4 with the highest first ionisation energy?
. .x ..
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 are the ionisation energy of isotopes the same?
The ionization energy of isotopes is the same because isotopes have the same number of protons in their nucleus, which determines the ionization energy. Isotopes differ in the number of neutrons they possess, but neutrons do not contribute significantly to the ionization energy compared to protons.
What is the relationship between ionization energy and the alkali metals?
There is no relation ship. They have the lowest ionization energies.
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.
What is meant by the first ionisation energy of nitrogen?
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.
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 is the first ionization energy for sodium?
Na(g) --> Na+(g) + e- First ionisation energy is always: X(g) --> X+(g) + e- with X being an element
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.
