CHEM 231 Inorganic Chemistry - Wave Mechanics

<p>The shape of the atomic orbitals (D)</p> Signup and view all the answers

<p>ml can take any value from -l to +l (A)</p> Signup and view all the answers

<p>Planck's constant (D)</p> Signup and view all the answers

<p>The relationship between wavelength, momentum, and Planck's constant (B)</p> Signup and view all the answers

<p>Their wavefunctions require more complex solutions (C)</p> Signup and view all the answers

<p>8 electrons (A)</p> Signup and view all the answers

<p>d-subshell (D)</p> Signup and view all the answers

<p>5 orbitals (C)</p> Signup and view all the answers

<p>-1, 0, 1 (B)</p> Signup and view all the answers

<p>4 subshells (C)</p> Signup and view all the answers

<p>Principal quantum number and angular momentum quantum number (C)</p> Signup and view all the answers

<p>The angular function defines the 3D orientation (C)</p> Signup and view all the answers

<p>9 orbitals (B)</p> Signup and view all the answers

<p>s atomic orbitals have a finite value of R(r) at the nucleus. (D)</p> Signup and view all the answers

<p>The number of radial nodes increases with the principal quantum number. (A)</p> Signup and view all the answers

<p>RDF = 4πr^2R(r) (D)</p> Signup and view all the answers

<p>1 (A)</p> Signup and view all the answers

<p>At radial nodes. (D)</p> Signup and view all the answers

<p>1s orbital (B)</p> Signup and view all the answers

<p>R(r) has a finite positive value. (C)</p> Signup and view all the answers

<p>2p orbital (B)</p> Signup and view all the answers

<p>The actual nuclear charge experienced by an electron in an atom. (D)</p> Signup and view all the answers

<p>0.35 (B)</p> Signup and view all the answers

<p>3.3 (C)</p> Signup and view all the answers

<p>4s2 is more stable than 3d2. (B)</p> Signup and view all the answers

<p>Shielding decreases the effective nuclear charge experienced by electrons. (B)</p> Signup and view all the answers

<p>18.7 (C)</p> Signup and view all the answers

<p>4s electrons experience a lower Zeff and are lost first. (D)</p> Signup and view all the answers

<p>S = 0.35 + (11x0.85) + (10x1.0) (D)</p> Signup and view all the answers

<p>1 (D)</p> Signup and view all the answers

<p>2 (C)</p> Signup and view all the answers

<p>Energy depends on both n and l. (A)</p> Signup and view all the answers

<p>p-orbitals (D)</p> Signup and view all the answers

<p>Angular nodes = l (B)</p> Signup and view all the answers

<p>2s (D)</p> Signup and view all the answers

<p>7 (B)</p> Signup and view all the answers

<p>They are spherically symmetric. (A)</p> Signup and view all the answers

Matter, like light, exhibits both wave-like and particle-like properties.

The wavelength associated with a particle, calculated using Planck's constant and the particle's momentum.

Solutions to the Schrödinger equation that describe the probability of finding an electron in a specific region around the nucleus.

An equation that describes the wave function of a particle.

Determines the electron's energy level and overall size of the orbital.

Specifies the shape of the electron's orbital (s, p, d, f).

Specifies the orientation of the orbital in space.

Coordinate system used to describe the radial and angular properties of atoms in the Schrödinger Equation.

A region around the atomic nucleus where electrons with similar energy levels are located, determined by the principal quantum number (n).

A region of space around the nucleus where there is a high probability of finding an electron.

A set of orbitals with the same energy level, designated by the values of n and l.

Calculated using the formula 2l + 1, where l is the azimuthal quantum number.

Component of the atom's wave function that describes the variation of the wave function with distance from the nucleus.

Represents the probability of finding an electron at a specific distance from the nucleus, independent of direction. It is denoted as R(r) and is a function of the distance from the nucleus (r).

A point in the radial function where the probability of finding an electron is zero. Occurs when R(r) = 0, excluding the origin.

The probability of finding an s orbital electron at the nucleus is NOT zero; It has a finite value.

The probability of finding an electron at the nucleus is zero for p, d, and f orbitals.

The probability of finding an electron at a particular distance from the nucleus, considering both the radial probability density and the volume at that distance. RDF = 4πr²R(r)².

The RDF becomes zero at radial nodes because R(r) = 0 at these points.

The number of radial nodes is determined by the formula: # of radial nodes = n - l - 1, where 'n' is the principal quantum number and 'l' is the azimuthal quantum number.

A higher peak in the RDF means a higher probability of finding an electron at that specific distance from the nucleus.

The part of the wave function that describes the shape of an atomic orbital. It depends on the angles θ and Ф, but not the principal quantum number (n).

Points in space where the probability of finding an electron is zero. They are flat planes that define the shape of an orbital.

For a given orbital, the number of angular nodes equals the value of the azimuthal quantum number (l).

For atoms with more than one electron, the energy of a subshell depends on both the principal quantum number (n) and the azimuthal quantum number (l). Generally, energy increases with increasing l.

The positive charge experienced by an electron in a multi-electron atom. It's a measure of the net attraction between the nucleus and an electron.

A measure of the reduction in nuclear charge experienced by an electron due to the presence of other electrons in the atom.

A set of empirical rules used to estimate the effective nuclear charge felt by an electron in a multi-electron atom.

Slater's Rules are used to calculate the effective nuclear charge (Zeff) experienced by an electron in a multi-electron atom, providing insights into its energy and stability.

A higher Zeff leads to a stronger attraction between the nucleus and the electron, resulting in a more stable electron configuration.

Electrons experiencing a lower Zeff are more easily lost during ionization because they are less strongly attracted to the nucleus.

Zeff is calculated by subtracting the shielding constant (S) from the nuclear charge (Z): Zeff = Z - S.

The 4s electron in V experiences a lower effective nuclear charge (Zeff) compared to the 3d electrons, making it less tightly bound and easier to remove during ionization.