Orbital Energy and Electron Configurations Quiz

Periodic Table Structure

• The first period of the Periodic Table has 2 elements.
• The second period of the Periodic Table starts with lithium (Li).
• The third period of the Periodic Table starts with sodium (Na).

Atomic Orbitals

• A boron atom's 2p orbital has 1 electron.
• The energy of the available orbitals 4d, 5s, and 5p increases in the order: 5s < 4d < 5p.
• The 3d orbitals start to get filled at scandium (Sc, Z = 21).

Electron Configuration

• Scandium (Z = 21) has the electron configuration [Ar]3d¹4s².
• Lithium (Li) in Group 1 has the electronic configuration [He]2s¹.

Periodic Trends

• Elements in the same group or column exhibit similar properties due to the same number and distribution of electrons in their outermost orbitals.
• The periodic dependence of an element's properties is determined by the electron configuration.

Blocks in the Periodic Table

• Elements in the same block have similar chemical behavior due to the same number and distribution of electrons in their outermost orbitals.

Ionization Enthalpy

• The size of isoelectronic species like F-, Ne, and Na+ is affected by the nuclear charge.
• Ionization enthalpy increases with increasing nuclear charge.

Valence Shell

• The valence principal quantum number (n) primarily determines the energy level of an electron.
• The valence shell is not affected by the atomic radius.

Ionization Enthalpy Exceptions

• The statement "ionization enthalpy always increases from left to right in a period" is incorrect.
• The biggest jump in ionization enthalpy when removing an electron is expected for boron (B).