Chemistry(Atomic Structure)

Energy levels are fixed orbits around the nucleus where electrons can exist, with the closest orbit having the lowest energy.

Rutherford concluded that the nucleus is a very small portion of the atom that contains concentrated positive charge, which is responsible for repelling and deflecting a few positively charged alpha particles during his experiment.

It determines the orientation of the spin and can have values of +1/2 or -1/2.

The Paschen Series is the series of spectral lines observed when excited electrons in hydrogen atoms fall from higher energy levels to the third energy level, and these lines are observed in the infra-red region.

Quantization is the restriction of a property to discrete values rather than continuous values.

The Lyman Series refers to the series of spectral lines observed when excited electrons in hydrogen atoms fall from higher energy levels to the first energy level, and these lines are observed in the ultraviolet region.

Potential energy is given by U = -K/e^2 * r.

The Schrodinger wave equation is a fundamental equation that describes how the quantum state of a physical system changes over time.

An anomalous electronic configuration refers to exceptions in the expected electron configurations, such as those seen in Chromium (24) and Copper (29).

The relationship is given by the formula C = νλ, where C is the speed of light, ν is the frequency, and λ is the wavelength.

The Thomson Model of Atom, proposed by J.J. Thomson, describes the atom as a uniform sphere of positive charge with electrons embedded within it, resembling a 'raisin pudding' where the positive charge is the pudding and the electrons are the raisins.

No two electrons in an atom can have the same four quantum numbers, meaning an orbital can hold a maximum of two electrons with opposite spin quantum numbers.

It determines the orientation of the orbital and can take integer values between -l and +l, including 0.

The Brackett Series consists of spectral lines observed when excited electrons in hydrogen atoms fall from higher energy levels to the fourth energy level, and these lines are also observed in the infra-red region.

Nucleons are the particles found in the nucleus of an atom, specifically protons and neutrons, which are much heavier than electrons.

The distance at which the maximum probability of finding an electron increases with an increase in the value of the principal quantum number.

The Aufbau principle states that in the ground state of atoms, orbitals are filled in the order of their increasing energies.

The azimuthal quantum number defines the three-dimensional shape of the orbital.

The wave number (ν) is given by the formula ν = 1/λ, where λ is the wavelength.

An atom consists of a tiny positively charged center called the nucleus, which contains protons and neutrons (nucleons). The mass of the atom lies in its nucleus, and electrons revolve around the nucleus in fixed circular paths called orbits.

The Balmer Series refers to the series of spectral lines observed when excited electrons in hydrogen atoms fall from higher energy levels to the second energy level, and these lines are observed in the visible region.

The Magnetic Quantum Number (mi) describes the magnetic orientation of an orbital and can take values from -l to +l.

Bohr's Theory states that an electron does not radiate energy while in a stable orbit and only radiates or absorbs energy when moving between orbits, with energy being radiated when moving towards the nucleus.

Heisenberg's uncertainty principle states that it is impossible to determine simultaneously the exact position and momentum of an electron.

The principal quantum number (n) determines the size and energy of the orbit.

The angular momentum of an electron is given by the formula L = nħ, where n is the principal quantum number and ħ is the reduced Planck's constant.

Electrons are filled in various orbitals in increasing order of their energies, with the lowest energy orbital filled first.

Energy is radiated or absorbed by a body not continuously but in small packets called quanta. In the case of light, the quantum is called a photon, and the energy of a quantum is directly proportional to the frequency of the radiation.

The Angular Momentum Quantum Number (l) determines the shape of the orbital and can have values from 0 to n-1.

Centrifugal forces acting away from the nucleus is equal to 2 mv/r.

The Stark effect is the splitting of spectral lines under the influence of an electric field.

A wave function must be continuous, finite, single-valued at any point, and the probability of finding the electron over the space must equal one.

J.J. Thomson's atomic model is also called the 'watermelon', 'plum pudding', or 'raisin pudding' model.

The energy associated with a photon is given by the formula E = nhν, where h is Planck's constant and ν is the frequency.

Alpha particles are positively charged helium ions with a charge of +2 and a mass of 4u, emitted during the radioactive decay of unstable elements like Uranium.

Rutherford's Gold Foil Experiment demonstrated that most of the atom's space is empty, as most alpha particles passed through the foil undeflected, while a small fraction was deflected, indicating a concentrated positive charge in a small volume called the nucleus.

Planck's constant (h) is a fundamental constant in quantum mechanics, valued at 6.6262 × 10 –34 Js.

The electromagnetic spectrum is an arrangement of all kinds of radiations in order of decreasing frequency or increasing wavelength, differing from one another in wavelength or frequency.

The Rydberg Formula is used to calculate the wavelengths of spectral lines in hydrogen and is expressed as 1/λ = R_H(1/n_1^2 - 1/n_2^2), where R_H is the Rydberg constant, n_1 is the lower energy level, and n_2 is the higher energy level.

For the 1s orbital, the maximum probability is at 0.53 Å, and for the 2s orbital, it is at about 2.6 Å.

The Pauli exclusion principle states that no two electrons can have the same set of four quantum numbers.

The values of 'l' are 0, 1, 2, 3, 4, 5, corresponding to subshells s, p, d, f, g, h respectively.

It indicates the direction in which an electron revolves and is a magnetic property that is quantized, having two permitted values: +1/2 and -1/2, denoted by 's'.

It identifies the subshell, determines the shape of the orbital, and is restricted to positive integers less than n.

The Stark Effect is the splitting of spectral lines in an electric field.

The Electron radial probability distribution function (D) is equal to 4πr²ψ².

The number of radial nodes is given by the formula n - l - 1.

The mass of an electron is approximately 9.1094 × 10^-31 kg.

Nucleons are the protons and neutrons present in the nucleus of an atom.

Isotopes are atoms that have the same atomic number but different mass numbers.

Coulomb's law describes the electrostatic force of attraction between the nucleus and the electron in a hydrogen atom.

They exhibit symmetrical distribution of electrons, leading to greater stability due to maximum exchange energy when electrons can exchange positions.

The Balmer Formula provides a simple empirical relationship to calculate the wave number of any line in the visible spectrum of atomic hydrogen, using the Rydberg constant.

The mass number is the total number of nucleons (protons and neutrons) in the nucleus of an atom.

De Broglie's equation states that λ = h/p, where λ is the wavelength, h is Planck's constant, and p is the momentum.

The atomic theory of matter states that matter is composed of atoms, which are indivisible and indestructible particles.

The magnetic quantum number (m) gives information about the spatial orientation of the orbital.

The work function (W) is the energy required to overcome the attractive forces on the electron in the metal.

It identifies the shell, determines the size and energy of the orbital, and the number of orbitals in the nth shell is equal to n².

The Zeeman Effect is the splitting of spectral lines in a strong magnetic field, associated with the magnetic quantum number.

The Principal Quantum Number (n) specifies the location and energy of an electron, with possible values of 1, 2, 3, etc.

The radius of the n-th orbit is given by r_n = (n^2 * h^2) / (4 * π^2 * m * e^2) or r_n = 0.529 * n^2 A.

The surface at which the probability of finding an electron is zero is called a radial node.

Hund's rule states that pairing of electrons in orbitals belonging to the same subshell does not take place until all the orbitals are singly occupied.

The mass number (A) is the total number of protons (Z) and neutrons (n) in the nucleus of an atom.

The Rydberg equation is used to predict the wavelengths of spectral lines in hydrogen and is given by ν = R(1/n1^2 - 1/n2^2), where R is the Rydberg constant.

The Pfund Series is the series of spectral lines observed when excited electrons in hydrogen atoms fall from higher energy levels to the fifth energy level, and these lines are found in the infra-red region.

The Spin quantum number (s) gives an idea about the spin of the electron and can take the values of +1/2 and -1/2.

The size of the orbital increases in the order of 1s < 2s < 3s < 4s.

An atomic orbital is the three-dimensional space around the nucleus where the probability of finding an electron is maximum.

The atomic number (Z) is the number of protons in the nucleus of an atom, which is also equal to the number of electrons in a neutral atom.

Isobars are atoms that have the same mass number but different atomic numbers.

The photoelectric effect is the ejection of an electron from a metal surface when a photon of energy greater than the threshold energy strikes an electron in the atom.

Bohr's Theory could not explain the spectrum of multi-electron atoms, the Zeeman and Stark effects, the shape of molecules, or align with Heisenberg's uncertainty principle.

The Zeeman effect is the splitting of spectral lines under the influence of a magnetic field.

The number of orbitals in a given sublevel is given by 2l + 1, where l is the azimuthal quantum number.

A black body is a body that emits and absorbs all frequencies of electromagnetic radiation.