1. Atomic Structure and Periodic Trends
Q1: What is the electron configuration for a neutral atom of sulfur (S)?
● A1: The electron configuration is 1s22s22p63s23p41s^2 2s^2 2p^6 3s^2
3p^41s22s22p63s23p4.
Q2: What trend is observed in atomic radius across a period in the periodic table?
● A2: The atomic radius decreases from left to right across a period due to increasing
nuclear charge, which pulls the electrons closer to the nucleus.
2. Chemical Bonding
Q3: What type of bond forms between sodium (Na) and chlorine (Cl) in sodium chloride (NaCl)?
● A3: An ionic bond forms between sodium and chlorine due to the transfer of an electron
from sodium to chlorine.
Q4: Explain why water (H₂O) has a bent molecular shape.
● A4: Water has a bent shape due to the two lone pairs on the oxygen atom, which repel
the bonded pairs, causing the H-O-H bond angle to be approximately 104.5°.
Q1: What is the electron configuration for a neutral atom of sulfur (S)?
● A1: The electron configuration is 1s22s22p63s23p41s^2 2s^2 2p^6 3s^2
3p^41s22s22p63s23p4.
Q2: What trend is observed in atomic radius across a period in the periodic table?
● A2: The atomic radius decreases from left to right across a period due to increasing
nuclear charge, which pulls the electrons closer to the nucleus.
2. Chemical Bonding
Q3: What type of bond forms between sodium (Na) and chlorine (Cl) in sodium chloride (NaCl)?
● A3: An ionic bond forms between sodium and chlorine due to the transfer of an electron
from sodium to chlorine.
Q4: Explain why water (H₂O) has a bent molecular shape.
● A4: Water has a bent shape due to the two lone pairs on the oxygen atom, which repel
the bonded pairs, causing the H-O-H bond angle to be approximately 104.5°.
