What is the relation between energy and radius?

Therefore the closer the electron to the nuclear the higher the attraction force, and thus the higher the energy required to overcome this attraction and remove the electron. Therefore the smaller the radius the higher the ionization energy, and the bigger the radius the lower the energy need.

What is the effect of the number of energy levels on the radius of an atom?

Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius.

What is the Bohr radius of a hydrogen atom?

The Bohr radius (a0) is a physical constant, approximately equal to the most probable distance between the nucleus and the electron in a hydrogen atom in its ground state. It is named after Niels Bohr, due to its role in the Bohr model of an atom. Its value is 5.29177210903(80)×10−11 m.

What is the relationship between electron affinity and atomic radius Why do you think this relationship occurs?

Electron affinity increases from left to right within a period. This is caused by the decrease in atomic radius. Electron affinity decreases from top to bottom within a group. This is caused by the increase in atomic radius.

What is the relationship between radius and atomic number?

As the atomic number of an element increases, so does the size of its nucleus and the number of electrons around it. The bigger the atomic number, the larger the atom’s radius.

What is the relationship between the atomic numbers and atomic radii of the elements in the group?

Atomic radius becomes smaller as you move across a row/period of the periodic table because it increases the number of protons, But, the Atomic radius becomes larger as you move down the periodic table in a group or column because it increases the number of energy levels.

How does the Bohr model of the hydrogen atom explain the hydrogen emission spectrum?

Bohr’s model explains the spectral lines of the hydrogen atomic emission spectrum. While the electron of the atom remains in the ground state, its energy is unchanged. When the atom absorbs one or more quanta of energy, the electron moves from the ground state orbit to an excited state orbit that is further away.

How has Bohr’s theory helped in calculating the energy of hydrogen electron in different energy levels?

By keeping the electrons in circular, quantized orbits around the positively-charged nucleus, Bohr was able to calculate the energy of an electron in the nth energy level of hydrogen: E ( n ) = − 1 n 2 ⋅ 13.6 eV E(n)=-\dfrac{1}{n^2} \cdot 13.6\,\text{eV} E(n)=−n21⋅13.

Which electron transition between the energy levels of hydrogen causes the emission?

The energy in a hydrogen atom depends on the energy of the electron. When the electron changes levels, it decreases energy and the atom emits photons. The photon is emitted with the electron moving from a higher energy level to a lower energy level.

How can you determine the energy levels in an atom calculate the energy of an atom?

To explain this observation, Niels Bohr proposed that electrons inside an atom occupy only certain allowed orbitals with a specific energy. In other words, the energy of an electron in an atom is not continuous, but ‘quantized. ‘ The energies corresponding to each of the allowed orbitals are called energy levels.