CHEM 1030 FINAL EXAM BROERING SECTION
2026 REVISION NOTES AND STRUCTURED
CHEMISTRY OVERVIEW GUIDE
◉ Magnetic Quantum Number (ml). Answer: specifies the three-
dimensional orientation of the orbital
-Values are integers ranging from -l ...0 .... l
◉ Electron Spin Quantum Number (ms). Answer: The "spin" of an
electron describes its magnetic field, which affects its energy.
-Allowed values: +1/2 and −1/2.
◉ Degenerate orbitals. Answer: orbitals on the same energy level
have the same energy
◉ Aufbau principle. Answer: electrons fill orbitals starting with the
lowest n before moving to higher energy obritals
◉ Pauli Exclusion Principle. Answer: No two electrons in the same
atom can have the same set of four quantum numbers, n, l, ml, ms
◉ Hund's Rule. Answer: For degenerate orbitals: electrons fill each
orbital singly before any orbital get a second electron
, ◉ Effective Nuclear Charge (Zeff). Answer: is the actual magnitude
of positive charge that is "experienced" by an electron in the atom
◉ Effective Nuclear Charge Trends. Answer: Row (left to right across
a period), Zeff increases
-Z increases, but the # of core electrons does not change
Column (going down a group), Zeff increases slightly
-larger Z has a larger electron core which is not capable to shield the
outer electrons effectively
◉ Metallic radius. Answer: half the distance between the nuclei of
two adjacent, identical metal atoms
◉ Covalent radius. Answer: half the distance between adjacent,
identical nuclei connected by a chemical bond
◉ Atomic Radius Trends. Answer: Row (left to right across a period):
decreases due to increasing Zeff
Group (from top to bottom): increases due to increasing value of n
2026 REVISION NOTES AND STRUCTURED
CHEMISTRY OVERVIEW GUIDE
◉ Magnetic Quantum Number (ml). Answer: specifies the three-
dimensional orientation of the orbital
-Values are integers ranging from -l ...0 .... l
◉ Electron Spin Quantum Number (ms). Answer: The "spin" of an
electron describes its magnetic field, which affects its energy.
-Allowed values: +1/2 and −1/2.
◉ Degenerate orbitals. Answer: orbitals on the same energy level
have the same energy
◉ Aufbau principle. Answer: electrons fill orbitals starting with the
lowest n before moving to higher energy obritals
◉ Pauli Exclusion Principle. Answer: No two electrons in the same
atom can have the same set of four quantum numbers, n, l, ml, ms
◉ Hund's Rule. Answer: For degenerate orbitals: electrons fill each
orbital singly before any orbital get a second electron
, ◉ Effective Nuclear Charge (Zeff). Answer: is the actual magnitude
of positive charge that is "experienced" by an electron in the atom
◉ Effective Nuclear Charge Trends. Answer: Row (left to right across
a period), Zeff increases
-Z increases, but the # of core electrons does not change
Column (going down a group), Zeff increases slightly
-larger Z has a larger electron core which is not capable to shield the
outer electrons effectively
◉ Metallic radius. Answer: half the distance between the nuclei of
two adjacent, identical metal atoms
◉ Covalent radius. Answer: half the distance between adjacent,
identical nuclei connected by a chemical bond
◉ Atomic Radius Trends. Answer: Row (left to right across a period):
decreases due to increasing Zeff
Group (from top to bottom): increases due to increasing value of n
