Scientists
This scientist is known as the father of quantum mechanics.
Who is Max Planck?
Solution: Max Planck introduced the idea of quantized energy levels in 1900, which led to the creation of quantum mechanics.
This model states
The nucleus is small and made up of protons and neutrons.
The electrons circle around the nucleus.
What is the Bohr Rutherford model?
Solution: Bohr came up with this model due to his famous gold foil experiment.
This quantum number denotes the size and energy level of an orbital.
What is the principal quantum number (n)?
Solution: The principal quantum number (n) indicates the main energy level occupied by the electron, with higher values of n corresponding to higher energy levels and larger orbitals.
The s-orbital has this many possible orientations.
What is 1?
Solution: The s-orbital is spherical and has only one orientation in space.
The electron configuration of Hydrogen (1s^1) is located in which block of the periodic table?
What is the s group?
Solution: Hydrogen, with an electron configuration of 1s^1, is located in the s group, where the outermost electrons occupy s orbitals.
This physicist introduced the concept of wave-particle duality.
Who is Louis de Broglie?
Solution: Louis de Broglie proposed that particles, like electrons, behave both wave-like and particle-like properties, a fundamental concept in quantum mechanics.
This model introduced the concept of electron clouds instead of fixed orbits to describe electron positions around the nucleus.
What is the Quantum Mechanical Model?
Solution: The Quantum Mechanical Model uses complex shapes of electron clouds (orbitals) to predict where electrons are likely to be found, rather than fixed circular orbits.
This quantum number determines the shape of an orbital.
What is the quantum number (l)?
Solution: The quantum number (l), also known as the angular momentum quantum number, defines the shape of the orbital, with values ranging from 0 to (n-1).
The p-orbital can have this many orientations.
What is 3?
Solution: The p-orbital has three orientations corresponding to the three values of the magnetic quantum number m_l (-1, 0, +1).
This rule states that electrons fill the lowest energy orbitals first.
What is the Aufbau principle?
Solution: The Aufbau principle dictates the order in which electrons fill atomic orbitals, starting with the lowest energy levels before filling higher ones.
He developed the uncertainty principle in quantum mechanics.
Who is Werner Heisenberg?
Solution: Werner Heisenberg put together the uncertainty principle in 1927, stating that the position and momentum of a particle cannot both be precisely determined at the same time.
This rule states that electrons will occupy degenerate orbitals singly before pairing up.
What is Hund's rule?
Solution: Hund's rule states that electrons will fill orbitals with the same energy level to maximize the number of unpaired electrons, minimizing electron-electron repulsions.
This quantum number describes the orientation of an orbital in space.
What is the magnetic quantum number (ml)?
Solution: The magnetic quantum number (ml) specifies the orientation of the orbital in space.
This type of orbital is shaped like a dumbbell.
What is a p-orbital?
Solution: The p-orbitals are dumbbell-shaped, with each lobe extending along one of the Cartesian axes (x, y, or z).
The electron configuration of Carbon is 1s^2 2s^2 2p^2. How many unpaired electrons does it have?
What are 2 unpaired electrons?
Solution: Carbon has an electron configuration of 1s^2 2s^2 2p^2. The two 2p electrons occupy separate p orbitals, resulting in two unpaired electrons.
This physicist proposed the exclusion principle which explains why electrons in an atom cannot occupy the same quantum state.
Who is Wolfgang Pauli?
Solution: Wolfgang Pauli introduced the Pauli exclusion principle in 1925, which states that no two electrons in an atom can have the same set of four quantum numbers.
The probability distribution of an electron in an atom is often represented as this, named after a mathematical function.
What is an orbital?
Solution: An orbital is a region of space where the probability of finding an electron is high (Schrödinger equation).
This quantum number specifies the spin of an electron.
What is the spin quantum number (ms)?
Solution:The spin quantum number (m_s) indicates the intrinsic spin of the electron, with possible values of +1/2 or -1/2.
The d-orbital has this many possible orientations.
What is 5?
Solution: The d-orbital has five orientations corresponding to the five possible values of the magnetic quantum number m_l (-2, -1, 0, +1, +2).
The electron configuration for a Neon atom is?
What is 1s^2 2s^2 2p^6?
Solution: Neon has an atomic number of 10, has a complete second energy level, resulting in an electron configuration of 1s^2 2s^2 2p^6.
In 1926 this scientist derived the quantum mechanical model of the atom.
Who is Erwin Schrödinger?
Solution: Described atoms as having wave like properties which came from de Broglie’s hypothesis
Mathematically determined the shape of the orbitals and the probability of an electron being in a certain place at a certain time orbitals are not just spheres anymore
This model describes atoms as indivisible and unique to each element.
What is Dalton’s atomic model?
Solution: Dalton’s atomic model proposed that atoms are the smallest indivisible units of matter and that each element consists of atoms of a single, unique type.
For the quantum numbers n=3, l=2, what are the possible values for ml?
What are -2, -1, 0, +1, +2?
Solution: For n=3 and l=2, the magnetic quantum number (ml) can have values ranging from -l to +l, so the possible values are -2, -1, 0, +1, +2.
The number of electrons that can fill the f-orbitals in a given energy level is?
What is 14?
Solution: The f-orbitals can hold a maximum of 14 electrons, with each of the seven f-orbitals holding two electrons (one with spin +1/2 and one with spin -1/2).
Electron configuration of a chromium atom.
What is [Ar] 3d^5 4s^1?
Solution: Chromium (atomic number 24) has an electron configuration of [Ar] 3d^5 4s^1 due to the extra stability associated with a half-filled d subshell.