Understanding Electron Configuration

What is the definition of electron configuration?

• The total number of protons in an atom.

• The arrangement of electrons in an atom's orbitals.

• The speed of electrons in an atom.

• The energy levels of an atom's nucleus.

What notation is used in electron configurations to represent subshells?

• p+q notation

• m+n notation

• n+l notation with letters (s, p, d, f)

• n^2 notation

How do superscripts in electron configurations indicate the number of electrons?

• Superscripts in electron configurations indicate the number of electrons in each subshell.

• Superscripts indicate the energy level of the electrons only.

• Superscripts are used to denote the type of subshells present.

• Superscripts represent the total number of electrons in an atom.

Explain the principle of electron pairing in subshells.

• All electrons in a subshell must be paired before any can occupy an orbital.

• Electrons in subshells pair up only after each orbital is singly occupied, following the Pauli Exclusion Principle.

• Electrons in subshells can never pair up in the same orbital.

• Electrons pair up randomly in any available orbital without following any rules.

How do electron configurations illustrate the filling order of orbitals?

• Electron configurations only represent the number of electrons in an atom.

• Electron configurations illustrate the shape of orbitals rather than their filling order.

• Electron configurations are determined solely by the number of protons in the nucleus.

• Electron configurations show the order in which orbitals are filled based on energy levels, following the Aufbau principle.

What is the significance of energy in the filling of orbitals?

• Energy is significant in the filling of orbitals as it dictates the order of orbital occupancy, affecting electron configuration and chemical behavior.

• Higher energy orbitals are filled before lower energy ones.

• Energy has no impact on orbital filling.

• Electrons fill orbitals randomly without regard to energy.

Why is the 1s orbital filled before the 2s orbital?

• The 1s orbital is filled after the 2s orbital due to its larger size.

• The 1s orbital is filled before the 2s orbital because it can hold more electrons.

• The 1s orbital is filled before the 2s orbital because it has a lower energy level.

• The 2s orbital is filled before the 1s orbital because it has a higher energy level.

Describe the filling order of the 2p orbitals in relation to the 1s and 2s orbitals.

• The 2p orbitals are filled after the 3s orbitals.

• The 2p orbitals are filled after the 1s and 2s orbitals.

• The 2p orbitals are filled simultaneously with the 1s and 2s orbitals.

• The 2p orbitals are filled before the 1s and 2s orbitals.

Provide the electron configuration for the first eleven elements of the periodic table.

• 1s1, 1s2, 1s2 2s1, 1s2 2s2, 1s2 2s2 2p1, 1s2 2s2 2p2, 1s2 2s2 2p3, 1s2 2s2 2p4, 1s2 2s2 2p5, 1s2 2s2 2p6, 1s2 2s2 2p6 3s1

• 1s2 2s2 2p6 3p1

• 1s2 2s2 2p6 3p2

• 1s2 2s2 3s2

How does the Aufbau principle relate to electron configurations?

• The Aufbau principle describes the energy levels of protons in an atom.

• The Aufbau principle dictates the order of filling orbitals in electron configurations.

• The Aufbau principle is only applicable to noble gases.

• The Aufbau principle states that electrons can occupy any orbital freely.