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WorksheetsCHM 101
Total questions: 40
Worksheet time: 20mins
Bohr's model failed primarily because it could not explain:
Energy levels.
Atomic spectra.
Elliptical orbits.
Stationary states.
If n = 4, which l value is forbidden?
0
1
3
4
Max electrons in an f subshell (l = 3)?
10
12
14
18
How many m_l values exist for a p subshell?
1
3
5
7
A particle with large mass and low speed has a de Broglie wavelength that is:
Large.
Predictable.
Very small.
Infinite.
Heisenberg's principle limits the simultaneous knowledge of position and:
Energy.
Momentum.
Spin.
Velocity.
Psi² (Psi square) in quantum mechanics represents the:
Wave function.
Orbital shape.
Probability density.
Energy level.
Which quantum number differentiates 2s from 4s?
l
m_l
m_s
n
Which set (n, l, m_l) describes a 3dz² orbital?
3, 2, +3
3, 2, 0
2, 3, +1
3, 1, 0
The arrangement, energy, and count of an atom's electrons define its:
Quantum state.
Atomic structure.
Electronic structure.
Quantum level.
Hund's Rule maximizes stability by ensuring orbitals have:
Paired, opposite spins.
Unpaired, parallel spins.
Paired, parallel spins.
Full capacity.
Which two phenomena confirmed the quantization of energy?
Atomic spectra, de Broglie.
Diffraction, wave-particle duality.
Blackbody, photoelectric effect.
Emission spectra, Heisenberg.
The minimum frequency needed for the photoelectric effect is called the:
Planck frequency.
Quantum frequency.
Threshold frequency.
Wave frequency.
What is the ground state configuration of the Fe³⁺ ion?
[Ar] 3d⁶ 4s⁰
[Ar] 3d⁵ 4s¹
[Ar] 3d⁵
[Ar] 3d³ 4s²
According to the Aufbau principle, which orbital follows 4p?
4d
5p
4f
5s
The classification of s, p, d, and f sections in the periodic table are known as:
Periods.
Rectangular blocks.
Groups.
Main groups.
The first stage of quantum theory treated the electron as a:
Wave.
Particle.
Photon.
Ion.
Elements where d or f subshells are filled are classified as:
Noble gases.
Representative elements.
Transition elements.
Main group elements.
The Lanthanides are part of which group classification?
d-transition.
p-block.
f-transition.
Representative.
The principle that no two electrons can have the same four quantum numbers is:
Hund's rule.
Aufbau principle.
Pauli exclusion principle.
Quantization rule.
The stronger ionic bond in MgO vs. NaCl is due to:
Higher electronegativity.
Smaller ion size.
Greater ionic charge magnitude.
Lower melting point.
A dative bond is unique because:
Sharing is unequal.
Only one sigma bond forms.
One atom contributes both shared electrons.
Electron transfer occurs.
Unequal sharing of electron pairs defines:
Non-polar covalent.
Pure covalent.
Polar covalent.
Ionic.
What is the characteristic bond angle of an sp hybrid orbital?
109.5°
120°
180°
90°
Metallic bonding consists of positive ions surrounded by a:
Crystalline structure.
Network of shared pairs.
Sea of delocalised electrons.
Fixed molecular lattice.
Order the forces: Strongest → Weakest.
Covalent > H-bond > van der Waals.
Ionic > Covalent > H-bond > van der Waals.
H-bond > Ionic > Covalent.
Covalent > Ionic > van der Waals.
The ability of a metal to be drawn into wires is called:
Malleability.
Brittleness.
Ductility.
Expansibility.
VSEPR theory predicts shape by minimizing electronic repulsion in the:
Nucleus.
Pi-electron system.
Valence shell.
Core electron shell.
The phase change from Gas → Solid (bypassing liquid) is called:
Sublimation.
Condensation.
Deposition.
Vaporization.
The complete mixing of different gases is explained by their:
Expansibility.
Compressibility.
Diffusibility.
Low density.
Hybridization involves mixing atomic orbitals of the:
Same shape.
Same spin.
Same energy level.
Same principal quantum number.
The bond angle for an sp² hybrid set is:
180°
120°
109.5°
90°
Strong hydrogen bonding requires the H atom to be bonded to a small, highly:
Electropositive atom.
Electronegative atom.
Partially positive atom.
Polarizable atom.
Hydrogen bonding is a specific, strong type of:
Covalent bond.
Intramolecular force.
Dipole-dipole interaction.
London Dispersion Force.
The abnormally high boiling points of H-bonded compounds are due to the extra energy needed to break:
Intramolecular covalent bonds.
Sigma and pi bonds.
Intermolecular H-bonds.
Ion-dipole forces.
Which gas property is a direct result of perpetual, random molecular motion?
Low density.
Compressibility.
Pressure exertion.
Fixed volume.
The transformation where solid forces are overcome by particle vibration is:
Sublimation.
Condensation.
Melting.
Evaporation.
Dipole-dipole forces occur between the partial positive end of one molecule and the neighboring molecule's:
Nucleus.
Non-polar region.
Partial negative end.
Delocalised electron.
The force holding atoms in a chemical compound together is called a(n):
Van der waals force.
Nuclear force.
Chemical bond.
Gravitational force.
An increase in electrostatic attraction for an ionic bond is favored by:
High atomic mass.
Small ion size.
Low melting point.
High malleability.
