Electronic Structure and Periodic Properties of Elements

These flashcards cover key concepts related to the electronic structure and periodic properties of elements from the lecture on college physics.

What is the speed of light in a vacuum?

The speed of light (c) is 2.998 × 10^8 m/s.

Define electromagnetic radiation.

Electromagnetic radiation is energy that travels in waves consisting of oscillating electric and magnetic fields.

What is Planck's constant?

Planck's constant (h) is equal to 6.626 × 10−34 J·s.

What principle explains the wave-particle duality of light?

The principle of wave-particle duality states that light exhibits both wave-like and particle-like properties.

What is the relationship between wavelength and frequency for electromagnetic waves?

The wavelength (λ) and frequency (ν) are inversely proportional; as wavelength increases, frequency decreases.

Who developed the Bohr Model?

The Bohr Model of the hydrogen atom was developed by Niels Bohr in 1913.

What does the principal quantum number (n) represent?

The principal quantum number (n) indicates the energy level of an electron in an atom.

What is the significance of the Pauli Exclusion Principle?

The Pauli Exclusion Principle states that no two electrons in the same atom can have the same set of four quantum numbers.

What are valence electrons?

Valence electrons are the outermost electrons of an atom that participate in chemical bonding.

How do trends in atomic size vary down a group and across a period in the periodic table?

Atomic size increases down a group and decreases across a period.

What is ionization energy?

Ionization energy is the energy required to remove the most loosely bound electron from a gaseous atom in its ground state.

How do electron affinities generally change across a period?

Electron affinities become more negative across a period as the effective nuclear charge increases.

What is a blackbody in terms of radiation?

A blackbody is an ideal emitter that approximates the behavior of many materials when heated.

Define isoelectronic species.

Isoelectronic species are atoms and ions that have the same electron configuration.

What is meant by effective nuclear charge (Zeff)?

Effective nuclear charge (Zeff) is the net positive charge felt by an electron in a multi-electron atom, accounting for shielding.

Describe the wavefunction in quantum mechanics.

The wavefunction (ψ) represents the probability amplitude of a quantum particle’s presence in a particular location in space.

What role does the angular momentum quantum number (ℓ) play?

The angular momentum quantum number (ℓ) defines the shape of the orbital.

How does the energy of atomic orbitals relate to principal quantum number?

The energy of atomic orbitals increases as the principal quantum number (n) increases.

What are core electrons?

Core electrons are electrons in an atom that are not in the outermost shell and have lower energy.

What is the difference between a cation and an anion?

A cation is a positively charged ion formed by the loss of electrons, while an anion is a negatively charged ion formed by the gain of electrons.

What is Hund’s rule?

Hund's rule states that the lowest-energy configuration for degenerate orbitals is the one with the maximum number of unpaired electrons.