Atomic Structure

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Questions and Answers

What determines the main energy level or shell in which the electron is present in an atom?

Azimuthal Quantum Number

Spin Quantum Number

Magnetic Quantum Number

Principal Quantum Number (correct)

Which of the following series corresponds to the ultraviolet region of the electromagnetic spectrum?

Pfund Series

Spectral Series

Lymen Series (correct)

Bracket Series

What is the relationship between the average distance of the electron from the nucleus and the principal quantum number in a hydrogen atom?

rn ∝ 1/n

rn ∝ 1/n^2

rn ∝ n

rn ∝ n^2 (correct)

What is the formula to calculate the wavelength of the spectral series in a hydrogen atom?

λ = 4R/n^2 Signup and view all the answers

What is the minimum value of the principal quantum number in an atom?

1 Signup and view all the answers

What is the orbital quantum number (l) responsible for?

Representing the number of subshells present in the main shell Signup and view all the answers

What is the expression for the orbital angular momentum of the electron?

L = l(l + 1)*h/2π Signup and view all the answers

What is the range of possible values for the magnetic quantum number (ml) for a given value of l?

-l to +l Signup and view all the answers

What is the spin (magnetic) quantum number (ms) responsible for?

Representing the spin of an electron about its own axis Signup and view all the answers

What is the total number of values of ml associated with a particular value of l?

2l + 1 Signup and view all the answers

What is the maximum number of electrons in a subshell with orbital quantum number l?

2(2l + 1) Signup and view all the answers

What is the significance of the spin quantum number in explaining the properties of a substance?

It helps to explain the magnetic properties of the substance Signup and view all the answers

According to the Aufbau principle, what is the order of filling electrons in orbitals?

Electrons enter the orbitals of lowest energy first Signup and view all the answers

What is the significance of the Pauli's exclusion principle in atomic structure?

It sets an upper limit on the number of electrons that can occupy a shell Signup and view all the answers

What is the maximum wavelength of the spectral line in the Balmer series of the hydrogen atom?

36R/5 Signup and view all the answers

What is the value of the principal quantum number (n) for the last line of the Lyman series?

∞ Signup and view all the answers

What is the Rydberg constant (R) in terms of the wavelength of the spectral lines?

1/λ Signup and view all the answers

What is the velocity of the electron in the nth orbit of the hydrogen atom according to the Bohr model?

h/2πn Signup and view all the answers

What is the number of spectral lines in the Paschen series of the hydrogen atom?

infinite Signup and view all the answers

What is the energy of the electron emitted when it makes a transition from a higher energy level E2(n2) to a lower energy level E1(n1)?

Rc h Z^2 (1/n1^2 - 1/n2^2) Signup and view all the answers

What is the frequency of the emitted radiation when an electron makes a transition from a higher energy level E2(n2) to a lower energy level E1(n1)?

Rc Z^2 / h (1/n1^2 - 1/n2^2) Signup and view all the answers

What is the wave number of the emitted radiation when an electron makes a transition from a higher energy level E2(n2) to a lower energy level E1(n1)?

Rc Z^2 / h c (1/n1^2 - 1/n2^2) Signup and view all the answers

If an electron falls from the nth orbit to the ground state, how many spectral lines will be emitted?

n(n-1) Signup and view all the answers

What is the condition for obtaining an absorption spectrum?

Transition from lower energy level to higher energy level Signup and view all the answers

If the energy of the photon absorbed by hydrogen atom is 12.4 eV, what is the quantum number of the excited state?

n = 4 Signup and view all the answers

The wave number of the energy emitted when electron comes from fourth orbit to second orbit in hydrogen is 20,397 cm–1. What is the wave number of the energy for the same transition in He+?

40,994 cm–1 Signup and view all the answers

What is the number of spectral lines in the emission spectrum of hydrogen?

6 Signup and view all the answers

What is the energy of the electron in the nth orbit of a hydrogen atom?

-13.6/n^2 eV Signup and view all the answers

What is the Rydberg constant in the formula for the energy of the photon emitted in the transition from the nth to the mth orbit?

1.097 × 10^7 m^-1 Signup and view all the answers

What is the expression for the velocity of the electron in the nth orbit of a hydrogen atom according to the Bohr model?

v = nh/2πm Signup and view all the answers

Study Notes

Bracket Series and Wavelengths

Bracket series defined by transitions: n2 = 5, 6, 7, …; n1 = 4.
For n1 = 4, n2 = 5: λmax = 400 nm = 9R.
For n1 = 5, n2 = 6: λmax = 900 nm = 11R.

Regions of Electromagnetic Spectrum

Ultraviolet region occurs with n1 = 3, yielding λmin = R/9.
Infrared region appears with various n1 values (e.g., n1 = 4, λmin = R/16).
Different series exist, such as Pfund series for n2 = 2, 3, 4, … with n1 = 1.

Quantum Numbers

Quantum numbers indicate electron location, energy, orbital type, and orientation.
Principal quantum number (n): specifies energy level, n can be any positive integer.
Orbital quantum number (l): distinguishes subshells, where l values range from 0 to (n-1).
Magnetic quantum number (ml): denotes electron orientation in subshells; ml ranges from -l to +l.
Spin quantum number (ms): represents electron spin, with two possible values: +1/2 or -1/2.

Electronic Configuration Rules

Pauli's exclusion principle: No two electrons can have identical sets of quantum numbers.
Aufbau principle: Electrons fill lowest energy orbitals first, following the n + l rule.

Spectral Lines and Emission Spectrum

Spectral lines arise from electrons transitioning between energy levels.
The number of spectral lines (N) can be calculated using the formula N = (n2 - n1 + 1)(n2 - n1)/2.
The transitions from higher to lower orbits produce various spectral lines.

Energy Transitions and Wavelength Calculations

Energy difference for photon emission: ΔE = E2 - E1.
Frequency of radiation: ν = ΔE/h.
Wavelength determination: Integration of wave number and Rydberg formula.

Bohr Model of Atom

Electron motion described in circular orbits; radius quantified by rn = n²h²/(4π²kZ).
Speed of electrons varies with orbit: v ∝ Z/n.
Kinetic energy (KE) and potential energy (PE) contribute to total energy: E = KE + PE.

Ionization Energy

Defined as the energy needed to remove an electron from an atom.
For hydrogen: Ionization energy = 13.6 eV/Z², decreasing with higher Z values.

Other Key Concepts

Electron transitions and energy levels are foundational to understanding atomic structure.
Rydberg constant: R = 1.097 × 10⁷ m⁻¹, crucial for calculating spectral lines and wavelengths.
Underlying physics defines the behavior of electrons and atomic interactions through quantum mechanics.

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Description

Test your understanding of spectral series, including Lyman, Pfund, and other series. Calculate wavelength and energy levels using various formulas. Prepare to ace your physics exam!