CHEM 1030 FINAL EXAM CERTIFICATION
EVALUATION SCRIPT 2026 FULL SOLUTION
◉ Distillation. Answer: Separates a homogeneous mixture based on
differences in boiling points.
◉ Chromatography (paper). Answer: Separates substances on the
basis of differences in solubility in a solvent.
◉ Intensive Properties. Answer: Independent of the amount of
substance present.
-Density, boiling point
◉ Extensive Properties. Answer: Dependent on the amount of
substance present.
-Mass, volume.
◉ Atomic Number and Mass Number. Answer:
◉ Isotopes. Answer: Atoms with identical atomic numbers but
different mass numbers
,◉ Mole. Answer: : the amount of a substance that contains as many
elementary entities as there are atoms in exactly 12 g C-12
◉ Avogadro's Number (NA). Answer: 6.0221418 x10^23
◉ Electrostatic energy. Answer: potential energy that results from
the interaction of charged particle
◉ Quantized energy (Max Planck). Answer: Energy can be absorbed
or released from atoms only in certain amounts (quanta).
◉ Heisenberg's Uncertainty Principle. Answer: the more precisely
the momentum (mu) of a particle is known, the less precisely its
position (x) is known
◉ Principal Quantum Number (n). Answer: designates size of the
orbital (shell)
-n values are integers >0
◉ Angular Momentum Quantum Number (l). Answer: describes the
shape of the orbital (subshells)
-l values are integers ranging from 0 to n − 1 for each value of n
, ◉ 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
EVALUATION SCRIPT 2026 FULL SOLUTION
◉ Distillation. Answer: Separates a homogeneous mixture based on
differences in boiling points.
◉ Chromatography (paper). Answer: Separates substances on the
basis of differences in solubility in a solvent.
◉ Intensive Properties. Answer: Independent of the amount of
substance present.
-Density, boiling point
◉ Extensive Properties. Answer: Dependent on the amount of
substance present.
-Mass, volume.
◉ Atomic Number and Mass Number. Answer:
◉ Isotopes. Answer: Atoms with identical atomic numbers but
different mass numbers
,◉ Mole. Answer: : the amount of a substance that contains as many
elementary entities as there are atoms in exactly 12 g C-12
◉ Avogadro's Number (NA). Answer: 6.0221418 x10^23
◉ Electrostatic energy. Answer: potential energy that results from
the interaction of charged particle
◉ Quantized energy (Max Planck). Answer: Energy can be absorbed
or released from atoms only in certain amounts (quanta).
◉ Heisenberg's Uncertainty Principle. Answer: the more precisely
the momentum (mu) of a particle is known, the less precisely its
position (x) is known
◉ Principal Quantum Number (n). Answer: designates size of the
orbital (shell)
-n values are integers >0
◉ Angular Momentum Quantum Number (l). Answer: describes the
shape of the orbital (subshells)
-l values are integers ranging from 0 to n − 1 for each value of n
, ◉ 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
