Question

fill out the table below based on the periodic table and the electron configurations given:
element
oxygen (o)
phosphorus (p)
electron configuration

total # of electrons

of valence electrons

Explanation:

Step1: Determine electron configuration

• For Oxygen (O): Atomic number is 8. Electron configuration is \(1s^{2}2s^{2}2p^{4}\)
• For Phosphorus (P): Atomic number is 15. Electron configuration is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{3}\)

Step2: Calculate total number of electrons

• Oxygen (O): From electron configuration \(2 + 2+4=8\)
• Phosphorus (P): From electron configuration \(2 + 2+6 + 2+3 = 15\)

Step3: Calculate number of valence electrons

• For Oxygen (O): Valence shell is \(2s^{2}2p^{4}\), so \(2 + 4=6\)
• For Phosphorus (P): Valence shell is \(3s^{2}3p^{3}\), so \(2+3 = 5\)

Answer:

Element	Electron Configuration	Total # of Electrons	# of Valence Electrons
Phosphorus (P)	\(1s^{2}2s^{2}2p^{6}3s^{2}3p^{3}\)	\(15\)	\(5\)