Chapter 3: Electronic Structure and Periodic Properties

These flashcards cover key concepts related to electronic structure and periodic properties as discussed in Chapter 3.

Visible light is a type of __.

electromagnetic radiation.

The frequency (𝝂) and wavelength (𝝀) of light are inversely __ to each other.

proportional.

The speed of light (c) is equal to __ times frequency (𝜈).

wavelength (𝜆).

The energy of a photon is given by the formula __.

E = h𝜈.

Planck’s constant is __ J.s.

6.626 x 10^-34.

An object heated to high temperatures emits __ radiation.

electromagnetic.

The lowest energy orbit in the Bohr model is known as __.

the ground state.

Electrons can 'jump' between energy levels by absorbing or __ a photon.

emitting.

Max Planck proposed the concept of __, where energy occurs in fixed quantities.

quantized energy.

_ proposed the wave-particle duality of electrons.

Louis de Broglie.

Erwin Schrödinger developed the __ equation.

Schrödinger's.

An atomic orbital is a 3D standing wave that describes where an electron is most-likely to be __.

found.

The principal quantum number (n) describes the __ of the orbital.

energy level.

The angular quantum number (l) describes the __ of the orbital.

shape.

The magnetic quantum number (ml) describes the __ of the orbital in 3D space.

orientation.

According to the Poisson exclusion principle, no two electrons can have identical values for all __ numbers.

four quantum.

Radiation with a __ frequency has a short wavelength.

high.

An electron emits a photon if it moves from a __ energy orbit to a lower energy orbit.

higher.

Each orbital can hold a maximum of __ electrons.

two.

Quantum numbers can describe inherently __ values.

quantized.

The photoelectric effect is when sufficient frequencies of light cause __ to flow.

current.

The __ energy orbits in the Bohr model are called excited states.

all other.

Electrons in an atom are treated as __ standing waves in quantum theory.

circular.

The wave nature of light is described by the relationship between frequency and __.

wavelength.

When electrons drop in energy levels, they emit specific __ of visible light.

wavelengths.

Heated solid objects give off electromagnetic radiation via __ radiation.

blackbody.

Electrons can spin in one of two possible __.

directions.

In the context of electron configurations, the Pauli-exclusion principle states that two electrons in the same orbital must have __ spins.

opposite.

The wave-particle duality concept applies to both __ and light.

matter.

Quantum numbers can be used to categorize __ in an atom.

orbitals.

The speed of light is approximately __ m/s.

3.00 x 10^8.

Each fixed quantity of energy is referred to as a __.

photon.

In the quantum mechanical model, electrons do not have fixed __, but are described by probability distributions.

orbits.

For the next lecture, students should read sections __ in the text.

3.4.