Set 1

1. How are many electrons can the p-orbital hold?

   * A p-orbital can hold a maximum of 6 electrons.

2. In a subshell of an atom, the total number of allowed orbitals is equal to:

   * The total number of allowed orbitals in a subshell is equal to 2l + 1, where l is the angular momentum quantum number.

3. Which of the following molecules contain 6 bonding electrons?

   * Without specific molecules listed, I cannot provide a direct answer. However, to determine the number of bonding electrons in a molecule, you would need to draw its Lewis structure and count the shared electron pairs between atoms.

4. Which of the following needs 2 more electrons to become stable?

   * Halogens (Group 17 elements) need 2 more electrons to achieve a stable electron configuration.

5. Which of the following does NOT follow the Octet Rule?

   * Without specific molecules or elements listed, I cannot provide a direct answer. However, some common exceptions to the Octet Rule include elements like boron, beryllium, and elements in the third period and beyond.

6. How many electron(s) do halogens need to become stable?

   * Halogens need 1 more electron to achieve a stable electron configuration.

7. Why do Lewis electron dot diagrams only show electrons in the outermost orbital of an atom?

   * Lewis dot diagrams focus on the valence electrons, which are the electrons in the outermost orbital. These electrons are primarily involved in chemical bonding and reactions.

8. What do you call a particle after gaining or losing an electron?

   * A particle that gains an electron becomes an anion (negatively charged). A particle that loses an electron becomes a cation (positively charged).

9. The atoms or groups of atoms that are electrically charged are called?

   * These are called ions.

10. What type of bond is found in the Lewis structure of Nitrogen gas, N₂?

   * Nitrogen gas (N₂) has a triple bond between the two nitrogen atoms.

### Set 2:

1. What is another name for quantum theory?

   * Wave mechanics

2. This is the three-dimensional regions in space where there is a high probability of finding an electron around an atom.

   * Orbital

3. The following are quantum numbers EXCEPT:

   * Mass number

4. What does the magnetic quantum number describe?

   * The orientation of an orbital in space

5. Which of the following symbolizes the spin of an electron?

   * mₛ

6. How many types of quantum numbers?

   * 4 (principal, angular momentum, magnetic, and spin)

7. What is a diamagnetic atom?

   * An atom with all paired electrons, resulting in no net magnetic moment.

8. Which rule states that electrons will go into empty orbitals of the same energy before entering into an orbital with an electron present?

   * Hund's rule

9. Which of the following electron configurations is NOT possible for an atom?

   * Without specific configurations listed, I cannot provide a direct answer. However, an impossible configuration would violate the Pauli Exclusion Principle or Hund's Rule.

10. Which of the following is NOT paramagnetic?

   * A diamagnetic atom (see question 7)

11. Which element has a completely filled subshell?

   * Noble gases (He, Ne, Ar, Kr, Xe, Rn) have completely filled valence shells.

12. The electrons of this substance are paired resulting to no net magnetic moment.

   * A diamagnetic substance

13. Which element is diamagnetic?

   * Again, noble gases are typically diamagnetic.

### Set 3:

1. Which molecule has a double bond?

   * Without specific molecules listed, I cannot provide a direct answer. However, molecules like O₂, CO₂, and C₂H₄ have double bonds.

2. Which of the following characterizes an ionic compound?

   * It is formed by the transfer of electrons between atoms.

3. It indicates the number of valence electrons in an atom represented by dots scattered on four sides of the atomic symbol.

   * Lewis dot structure

4. How many electrons must be gained or lost by phosphorus to achieve a stable electron configuration?

   * Phosphorus needs to gain 3 electrons to achieve a stable electron configuration.

5. It is formed by the sharing of electrons between atoms.

   * Covalent bond

6. How to apply octet rule in the formation of molecular covalent compounds?

   * Atoms in covalent compounds tend to share electrons to achieve a stable electron configuration of 8 valence electrons (octet rule).

7. Which of the following compounds have covalent molecular structure?

   * Without specific compounds listed, I cannot provide a direct answer. However, compounds like H₂O, CO₂, and CH₄ have covalent molecular structures.

8. What type of bond is formed in the compound Na₃PO₄?

   * Ionic bond

9. How many total valence electrons are there in iodine trichloride?

   * Iodine trichloride (ICl₃) has a total of 28 valence electrons.

10. How many lone pairs are present in the Lewis structure of ammonia, NH₃?

   * Ammonia (NH₃) has 1 lone pair on the nitrogen atom.

11. How many electrons do hydrogen need to fill its outer shell?

   * Hydrogen needs 1 electron to fill its outer shell.

12. Which of the following is the correct Lewis structure of N₂?

   * The correct Lewis structure of N₂ has a triple bond between the two nitrogen atoms.

### Set 4:

1. Which among the following is a symbol used to represent bonding pairs of electrons in a Lewis structure?

   * A line (-)

2. Which of the following is the correct structure of the Lewis structure of iodine fluoride?

   * I-F with 3 lone pairs on I and 3 lone pairs on F

3. Which of the following pairs of element valence is correct?

   * Without specific pairs listed, I cannot provide a direct answer. However, you can determine the valence electrons of an element by its group number on the periodic table.

4. Which of the following is the correct Lewis structure of the cyanide ion?

   * C≡N⁻ with a lone pair on C and a lone pair on N

5. The product of charge, Q, and the distance between the charges, r, to maintain neutrality, the charges on the ends of the molecule must be equal in magnitude but opposite in sign.

   * Dipole moment

6. The angle between two bonds originating from the same atom in a covalent species.

   * Bond angle

7. Which statement correctly describes the Valence Shell Electron Pair Repulsion (VSEPR) theory?

   * VSEPR theory predicts the geometry of molecules based on the repulsion between electron pairs around a central atom.

8. Why is it important to know the geometry of a molecule?

   * Knowing the geometry of a molecule helps predict its polarity, reactivity, and physical properties.

9. The molecule boron trifluoride, BF₃, assumes a trigonal planar geometry with boron as the central atom. Which statement correctly describes the polarity of the B-F bond and the polarity of the molecule?

   * Each B-F bond is polar, but due to the symmetrical arrangement of the bonds, the molecule is nonpolar.