Energy level and Bohr model of hydrogen

Energy level

  • Electron Shell or Energy levels will be the specified distances from the nucleus of an atom where electrons might be found or the highest probability to be found. Electrons are negatively charged particles within a molecule that move round the positive nucleus, usually located in the center. Energy levels are somewhat like the measures of a step’s electron jumps.
  • In most fundamental concepts of an atom; consist of electrons orbiting around a nucleus.
  • Though, the electrons are not capable of choosing any orbit as per their wish. Electrons are restricted to orbits with only a certain energy level. Electrons are only able to jump from one energy level or step to another level. Electrons cannot orbit with any energies other than the specified energy levels.

What is the energy level diagram?

Energy level means of evaluating the amount of energy electron may require and will be released during the transition, if they jump from one orbit to other. The ground or zero-state is the minimum energy state calculated for H2 molecules.

What are the four energy levels?

There are four types of orbitals- s, p, d, and f.

  • Sharp-s 
  • Principle-p
  • Diffuse-d
  • Fundamental-f 

In an atom, there are some combinations of these orbitals

The energy level is a quantity of space or regions, wherever electrons will probably be present. These distances, known as orbitals, are of different shapes, denoted by a letter (s, p, d, f ).

How do you determine energy levels?

Valence electrons

“Electron those is in the highest energy level are called valence electron.”

Ground State

“The minimum energy equilibrium state of the H2 atom is acknowledged as the ground-state.”

Excited-state

When the electron (or atom) has higher energy than this lowest energy, it is said to be in an “excited state.”

If an electron falls from a higher level to a lower, a photon may emits, or energy get released.

Energy Difference

The emitted photon’s energy is the difference amongst the energy levels of the primary (n i ) and final (n f ) state. The energy of the emitted photon is computed using the Rydberg Formula.

The Bohr model of hydrogen

In 1913, Niels Bohr conceptualized the energy levels and spectral freqn of the H2 in considering various simple assumption to fix the hypothetical classical one. The majority of these flaws were solved by Arnold Summerfield’s modification of the Bohr model. For this model, Physicist Niels Bohr has received the Nobel Prize in Physics in the year 1922.

In the fundamental concept that an atom (the Bohr atomic model), electrons are rotating only certain orbits around the nucleus. The electrons going down and up between allowed orbits, in addition to emission or absorption of energy, happens.

Though this basic model is not accepted well because most of the atoms’ structure is more complicated than hydrogen, though this necessitates the new subjects, hence the introduction of quantum mechanics, in quantum mechanics, every orbiting electron is explained by a mathematical expression known as a wave function.


Bohr Atomic Model
WillowWBohr atom modelCC BY-SA 3.0

Bohr Radius

“The Bohr radius (a0) is a constant parameter, is equal to the most predictable distance for hydrogen atom between the nucleus and the electron at the ground state (non-relativistic and having an infinitely heavy proton)

It’s named after Niels Bohr because of its part in the Bohr model of an atom.

Hydrogen Atom using Bohr Model
Hydrogen Atom using Bohr Model
SE3-29XHydrogen GIFCC BY-SA 4.0

Spectral lines

Each component has a particular set of energy levels. Thus, the frequencies in which it absorbs and emits light behave as a sort of mic, identifying the specific compound and particular. These characteristics of atoms have given investigate in subjects called spectroscopy, a science dedicated to identifying molecules and atoms from the type of radiation they absorb or emit.

Balmer Series

Atomic physicist Balmer has analytically noted a relation in the energies during photons release from atom. The various discrete photon energies/wavelengths which were discovered by Balmer is called the Balmer series.

It was later known that energy transitions create the Balmer lines from the Hydrogen atom. The atom’s Bohr model managed to spell out the Balmer series because larger orbits needed electrons to have significantly more adverse power or negative energy to balance with the angular momentum. The Rydberg formula take a broad view of Balmer series for all energylevel adjustments.

Emission Spectrum

The emission spectrum of atomic hydrogen was divided into numerous spectral series and wavelengths provided by the standard Rydberg formula. These detected spectral lines are the result of the electron transition from different energy levels in an atom.

An emission spectrum denotes the variety of wavelengths emitted by an atom or chemical compound stimulated by either heating or electrical current. The emission spectrum of burning gas or other molecules might also be utilized to instance its composition.

Emission spectrum of atomic Hydrogen and Helium
Emission spectrum of atomic Hydrogen and Helium
Image Credit: RanjithsijiAtomic emission spectrum of heliumCC BY-SA 4.0

Potential energy

“This is the energy  of an entity for of its position relative to other objects, stresses, stored electric charge, or other factors within itself.”

Binding Energy

“The binding energy is the minimum energy required to holds a nucleus together.”

Ionization Energy

The energy quantity that an isolated atom in the ground electronic state required to be absorbed to get discharged as an e- “

Ionization energy is described as a step of difficulty in removing an electron in an atom or ion or an atom or ion’s proficiency to surrender an electron. The no of electron reduction usually takes place in the ground state of the species.

The ionization energies are measured in kJ/mol, or the amount of energy it requires for all atoms in a mole to be loosen unity e- respectively.

How does ionization energy work?

Ionization energy is the energy required, in which an isolated, gaseous atom from the ground electronic state should absorb to release an electron. The more electrons lost, the more +ve this ion will be, and it will be more difficult to be separated the e- from atom.

What element has the highest and lowest ionization energy?

  • The element He has the highest ionization energy.
  • Francium has the minimum ionization energy.

An element’s ionization energy becomes higher from left to right across a periodic-table and declines from top to down generally in periodic table. 

Ionization Energy using Periodic Table
Ionization Energy using Periodic Table
Cdang and AdrignolaIonization energy periodic tableCC BY-SA 3.0

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About Dr. Subrata Jana

I am Subrata, Ph.D. in Engineering, more specifically interested in Nuclear and Energy science related domains. I have multi-domain experience starting from Service Engineer for electronics drives and micro-controller to specialized R&D work. I have worked on various projects, including nuclear fission, fusion to solar photovoltaics, heater design, and other projects. I have a keen interest in the science domain, energy, electronics and instrumentation, and industrial automation, primarily because of the wide range of stimulating problems inherited to this field, and every day it’s changing with industrial demand. Our aim here is to exemplify these unconventional, complex science subjects in an easy and understandable to the point manner.
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