CHEM 1410 - Chapter 2: Atomic Orbitals - Energy, Shape, and Electron Density

What does the principle quantum number (n) indicate about the electron in an atom?

the most likely distance of the electron from the nucleus

In Bohr's model of the atom, what prevents an electron from spiraling into the nucleus?

quantized energy levels for electrons in orbits

Which concept explains why sodium and other metals are highly reactive with water?

incomplete electron shells increase reactivity

How does the Schrödinger equation contribute to our understanding of electron behavior in atoms?

it predicts the most probable location of electrons

Which description best fits the role of the Hamiltonian operator in Schrödinger’s equation?

it combines kinetic and potential energy calculations for electrons (helps to determine total energy in the system)

What aspect of an atomic orbital does an angular node indicate?

zero probability of finding an electron at a specific angle

Why do quantum numbers play an essential role in understanding atomic structure?

they quantize properties such as energy, shape, and orientation of electrons

What does the spin quantum number (ms) represent?

orientation of an electron’s magnetic field

Which statement correctly explains the concept of orbital penetration?

probability density in regions near the nucleus

What is the significance of radial nodes in an atomic orbital?

smaller probability of finding an electron in a certain region

Which quantum approach explains the likelihood of finding an electron in a given space within an atom?

Schrodinger’s wavefunction model

How does the Bohr model describe the electron's energy in relation to its orbit?

the electron’s energy is quantized according to its orbit’s radius

What is one reason why sodium, potassium, rubidium, and cesium are highly reactive compared to other elements?

Their large atomic radii reduce the energy required to remove an electron.

How does the Bohr model explain the quantization of electron energy levels?

Electrons travel in fixed orbits defined by specific energy levels.

According to Schrödinger's wavefunction, what does |Ψ|² represent in terms of electron location?

The probability density of finding an electron in space.

What characteristic of an atom affects the penetration of orbital electrons towards the nucleus?

The principal quantum number (n).

Why do p-orbitals have a characteristic 'dumbbell' shape?

They possess angular momentum that requires specific spatial orientation.

How are angular nodes in atomic orbitals identified?

They occur where the angular wavefunction changes sign.

What principle determines that no two electrons can have the same set of quantum numbers?

Pauli exclusion principle.

In quantum mechanics, what is the primary limitation of the Schrödinger equation for complex atoms?

Difficulty in accounting for electron-electron interactions.

How does the introduction of quantum numbers enhance the periodic table's structural understanding?

Quantum numbers define electron properties and periodic trends.

In terms of energy hierarchy, which quantum number primarily affects the energy level of an electron in a hydrogen atom?

The principal quantum number (n).