Topic S 1.3 - Electron configurations SL .1

What is the Aufbau principle and how does it apply to electron configuration?

• The Aufbau principle dictates that all electrons must occupy the same orbital before filling others.

• The Aufbau principle only applies to the first 20 elements of the periodic table.

• The Aufbau principle guides the filling of electron orbitals in order of increasing energy.

• The Aufbau principle states that electrons fill orbitals in random order.

Explain the Pauli exclusion principle and its significance in electron arrangement.

• It describes how electrons are attracted to protons in the nucleus.

• The Pauli exclusion principle is significant because it explains the unique electron configurations of atoms, influencing their chemical properties and reactivity.

• The principle is only relevant for the arrangement of neutrons in an atom.

• The Pauli exclusion principle states that electrons can occupy the same quantum state.

Describe Hund's rule and its importance in determining electron configurations.

• Hund's rule states that electrons must fill the lowest energy orbitals first, regardless of their spin.

• Hund's rule indicates that all electrons in an atom must have opposite spins to minimize energy.

• Hund's rule applies only to the filling of s orbitals and has no effect on p or d orbitals.

• Hund's rule is important in determining electron configurations as it ensures that electrons fill degenerate orbitals singly first, which minimizes repulsion and stabilizes the atom.

What is electron configuration notation and how is it used to represent electron arrangements?

• It indicates the mass of an atom in atomic units.

• Electron configuration notation represents the arrangement of electrons in an atom using a series of numbers and letters indicating energy levels and orbital types.

• It describes the chemical properties of elements.

• It shows the physical state of an element at room temperature.

Define valence electrons and explain their role in chemical bonding.

• Valence electrons are the protons in an atom that determine its mass.

• Valence electrons are the electrons that are always found in the nucleus of an atom.

• Valence electrons are the inner electrons that do not participate in bonding.

• Valence electrons are the outermost electrons of an atom that participate in chemical bonding.

How are orbital diagrams constructed and what do they represent?

• Orbital diagrams represent the physical shape of an atom.

• Orbital diagrams represent the arrangement of electrons in an atom's orbitals, showing their distribution and spin.

• Orbital diagrams illustrate the temperature of an atom's electrons.

• Orbital diagrams show the chemical bonds between atoms.

What is the electromagnetic spectrum and how does it relate to electron transitions?

• The electromagnetic spectrum is only visible light and has no relation to electron transitions.

• Electron transitions occur only in solid materials and do not involve electromagnetic radiation.

• The electromagnetic spectrum is the range of all electromagnetic radiation, and it relates to electron transitions through the absorption or emission of photons during electron energy level changes.

• The electromagnetic spectrum is a measure of sound waves and does not relate to electron energy levels.

Define ionization energy and explain its significance in chemistry.

• Ionization energy is the energy released when an electron is added to an atom.

• Ionization energy is the temperature at which a substance changes from solid to gas.

• Ionization energy is the energy required to split a molecule into its constituent atoms.

• Ionization energy is the energy required to remove an electron from a gaseous atom or ion.

How is ionization energy calculated for an element?

• Ionization energy is determined by the temperature of the element.

• Ionization energy is calculated by averaging the atomic mass of an element.

• Ionization energy is the energy released when an electron is added to an atom.

• Ionization energy is calculated by measuring the energy needed to remove an electron from an atom in the gas phase.

What are successive ionization energies and how do they differ from the first ionization energy?

• The first ionization energy is the total energy required to remove all electrons from an atom.

• Successive ionization energies refer to the energy needed to remove the last electron only.

• Successive ionization energies are the energies required to remove additional electrons from an atom, differing from the first ionization energy, which is specifically for removing the first electron.

• Successive ionization energies are only relevant for noble gases and not for other elements.