Which is more dense, Silver AG or Carbon C, and why? How many valence electrons do they each have and why?
The Correct Answer and Explanation is :
Density Comparison: Silver (Ag) vs. Carbon (C)
Silver (Ag) is far more dense than Carbon (C). The density of Silver is 10.49 g/cm³, while Carbon, in its graphite form, has a density of ~2.267 g/cm³, and in its diamond form, it is 3.51 g/cm³.
Why is Silver More Dense?
- Atomic Mass and Size: Silver has an atomic mass of 107.87 u, while Carbon has an atomic mass of only 12.01 u. Since silver atoms are much heavier than carbon atoms, they contribute to a significantly higher density.
- Atomic Structure and Packing: Silver is a metal and has a face-centered cubic (FCC) structure, allowing its atoms to be tightly packed together. In contrast, carbon forms different allotropes like graphite and diamond, which have less dense atomic arrangements.
- Bonding Differences: Silver has metallic bonding, which allows electrons to move freely and tightly pack atoms together. Carbon, depending on its form, either has covalent bonding (diamond) or layered structures (graphite), leading to lower density compared to Silver.
Valence Electrons of Silver and Carbon
- Silver (Ag) has 1 valence electron because it is in Group 11 of the periodic table, with an electron configuration of [Kr] 4d¹⁰ 5s¹. The outermost 5s¹ electron is the valence electron.
- Carbon (C) has 4 valence electrons because it is in Group 14, with an electron configuration of [He] 2s² 2p². The 2s² 2p² electrons in the second energy level are its valence electrons.
Thus, Silver has 1 valence electron (due to its s-orbital filling), and Carbon has 4 valence electrons (due to its s and p orbitals).
Here is the image comparing the density differences between Silver (Ag) and Carbon (C) in its graphite and diamond forms. Let me know if you need any modifications or further explanations!