Atomic Theory Lecture 3

<p>Regions where the probability of finding an electron is zero (A)</p> Signup and view all the answers

<p>D orbitals can contain a maximum of 10 electrons (C)</p> Signup and view all the answers

<p>+1/2 represents spin up and -1/2 represents spin down.</p> Signup and view all the answers

<p>The principal quantum number (n) determines the size of the orbital and the energy level of the electron.</p> Signup and view all the answers

<p>3d orbitals have a 'four leaf clover' shape and contain two nodes that pass through the nucleus.</p> Signup and view all the answers

<p>The number of orbitals in a subshell is determined by the azimuthal quantum number (l) and is calculated as $2l + 1$.</p> Signup and view all the answers

<p>Each shell corresponds to a principal quantum number (n) and contains n subshells characterized by the angular momentum quantum number (l).</p> Signup and view all the answers

<p>The magnetic quantum number (ml) determines the orientation of orbitals in space for a given subshell.</p> Signup and view all the answers

<p>An s orbital is spherical in shape with no nodes, while p orbitals are dumbbell-shaped and d orbitals have a more complex clover shape.</p> Signup and view all the answers

<p>The 4f subshell contains 7 f orbitals, which have complex shapes often described as having multiple lobes.</p> Signup and view all the answers

A fundamental property of electrons, like charge and mass, described by the fourth quantum number (ms), which can be +1/2 (spin up) or -1/2 (spin down).

Set of numbers that describe the properties of an atomic orbital; n determines size, l determines shape, and ml determines orientation.

Determines the size of an atomic orbital. Higher n values mean larger orbitals.

Determines the shape of atomic orbitals. Different l values correspond to different orbital shapes (s, p, d, f).

Determines the spatial orientation of an atomic orbital; controls the number of possible orbitals for a given l value.

The energy of a hydrogen atom's orbital only depends on 'n' (principal quantum number).

A set of orbitals possessing the same value of 'n' (principal quantum number) and, thus, a set of orbitals of the same energy level.

A set of orbitals with the same value of both n (principal quantum number) and l (angular quantum number).

Describes the intrinsic angular momentum of an electron, which is quantized and can have two values: +1/2 (spin up) or -1/2 (spin down).

The principal quantum number (n) determines the size of an atomic orbital. Higher values of n correspond to larger orbitals.

The angular momentum quantum number (l) determines the shape of an atomic orbital. Different values of l correspond to different shapes: s (spherical), p (dumbbell), d (cloverleaf), and f (complex).

The magnetic quantum number (ml) determines the orientation of an atomic orbital in space. For a given l, there are (2l + 1) possible orientations.

The energy of an atomic orbital in a hydrogen atom (or any one-electron atom) depends solely on the principal quantum number (n).

A set of orbitals with the same value of the principal quantum number (n), representing an energy level.

A set of orbitals with the same value of both the principal quantum number (n) and the angular momentum quantum number (l).

The number of orbitals within a subshell is determined by the angular momentum quantum number (l) using the formula: 2l + 1.