DSC Major Chemistry - UK1DSCCHE100 (Theory) Quiz

Name

What is the main conclusion of the de Broglie equation?

• a) Matter can be considered as particles only.
• b) Electrons have a dual nature, exhibiting both particle and wave characteristics.
• c) Electrons do not exhibit wave properties.
• d) Electrons are not affected by electromagnetic waves.

Which of the following quantum numbers determines the shape of an orbital?

• a) Principal quantum number
• b) Angular Momentum quantum number
• c) Magnetic quantum number
• d) Spin quantum number

According to Slater’s rule, the effective nuclear charge is calculated by:

• a) Adding the number of protons in the nucleus.
• b) Subtracting the shielding constant from the nuclear charge.
• c) Dividing the atomic number by the shielding constant.
• d) Adding the shielding effect to the atomic number.

Which of the following principles is used to fill orbitals with the lowest energy first?

• a) Pauli's Exclusion Principle
• b) Hund’s Rule
• c) Aufbau Principle
• d) Heisenberg's Uncertainty Principle

What is the significance of the Schrödinger equation in quantum mechanics?

• a) It predicts the position of an electron.
• b) It describes the probability of finding an electron in a given region.
• c) It provides a deterministic value for the electron's location.
• d) It determines the mass of an electron.

The metallic bond is characterized by:

• a) Sharing of electron pairs between atoms.
• b) A "sea of electrons" that are free to move.
• c) Transfer of electrons between atoms.
• d) Bonding due to mutual attraction of protons.

In VSEPR theory, the molecular geometry of a molecule with 3 bonding pairs and 1 lone pair of electrons is:

• a) Tetrahedral
• b) Trigonal planar
• c) Bent
• d) Linear

The bond order of the O₂⁺ ion is:

• a) 1
• b) 2
• c) 3
• d) 1.5

In the context of ionic bonds, which of the following describes the Fajan's Rule?

• a) The size of ions and the charge difference determine bond polarity.
• b) The larger the ion, the more ionic the bond.
• c) Higher electronegativity always leads to covalent bonding.
• d) Covalent bonds are stronger than ionic bonds.