Which of the following will have the same number of electrons :1 g Hydrogen2 g Oxygen2 g Carbon2 g Nitrogen

To determine which of the given samples have the same number of electrons, we need to follow these steps:

1. Determine the number of moles of each element in the given mass.
2. Calculate the number of atoms in each sample using Avogadro's number.
3. Determine the number of electrons in each atom and multiply by the number of atoms.

Let's go through each element one by one:

1. Hydrogen (H)

• Atomic number of Hydrogen (H): 1 (which means each hydrogen atom has 1 electron)
• Molar mass of Hydrogen (H): 1 g/mol

Given mass = 1 g

Number of moles of Hydrogen = Given mass / Molar mass $\text{Number of moles of H} = \frac{1 \text{ g}}{1 \text{ g/mol}} = 1 \text{ mol}$

Number of atoms in 1 mole = Avogadro's number (approximately $6.022 \times 10^{23}$)

Number of electrons in 1 g of Hydrogen: $\text{Number of electrons} = 1 \text{ mol} \times 6.022 \times 10^{23} \text{ atoms/mol} \times 1 \text{ electron/atom} = 6.022 \times 10^{23} \text{ electrons}$

2. Oxygen (O)

• Atomic number of Oxygen (O): 8 (which means each oxygen atom has 8 electrons)
• Molar mass of Oxygen (O): 16 g/mol

Given mass = 2 g

Number of moles of Oxygen = Given mass / Molar mass $\text{Number of moles of O} = \frac{2 \text{ g}}{16 \text{ g/mol}} = 0.125 \text{ mol}$

Number of atoms in 0.125 mole = Avogadro's number (approximately $6.022 \times 10^{23}$)

Number of electrons in 2 g of Oxygen: $\text{Number of electrons} = 0.125 \text{ mol} \times 6.022 \times 10^{23} \text{ atoms/mol} \times 8 \text{ electrons/atom}$ $\text{Number of electrons} = 0.125 \times 6.022 \times 10^{23} \times 8$ $\text{Number of electrons} = 6.022 \times 10^{22} \times 8$ $\text{Number of electrons} = 4.818 \times 10^{23} \text{ electrons}$

3. Carbon (C)

• Atomic number of Carbon (C): 6 (which means each carbon atom has 6 electrons)
• Molar mass of Carbon (C): 12 g/mol

Given mass = 2 g

Number of moles of Carbon = Given mass / Molar mass $\text{Number of moles of C} = \frac{2 \text{ g}}{12 \text{ g/mol}} = 0.167 \text{ mol}$

Number of atoms in 0.167 mole = Avogadro's number (approximately $6.022 \times 10^{23}$)

Number of electrons in 2 g of Carbon: $\text{Number of electrons} = 0.167 \text{ mol} \times 6.022 \times 10^{23} \text{ atoms/mol} \times 6 \text{ electrons/atom}$ $\text{Number of electrons} = 0.167 \times 6.022 \times 10^{23} \times 6$ $\text{Number of electrons} = 1.005 \times 10^{23} \times 6$ $\text{Number of electrons} = 6.03 \times 10^{23} \text{ electrons}$

4. Nitrogen (N)

• Atomic number of Nitrogen (N): 7 (which means each nitrogen atom has 7 electrons)
• Molar mass of Nitrogen (N): 14 g/mol

Given mass = 2 g

Number of moles of Nitrogen = Given mass / Molar mass $\text{Number of moles of N} = \frac{2 \text{ g}}{14 \text{ g/mol}} = 0.143 \text{ mol}$

Number of atoms in 0.143 mole = Avogadro's number (approximately $6.022 \times 10^{23}$)

Number of electrons in 2 g of Nitrogen: $\text{Number of electrons} = 0.143 \text{ mol} \times 6.022 \times 10^{23} \text{ atoms/mol} \times 7 \text{ electrons/atom}$ $\text{Number of electrons} = 0.143 \times 6.022 \times 10^{23} \times 7$ $\text{Number of electrons} = 0.143 \times 4.215 \times 10^{24}$ $\text{Number of electrons} = 6.03 \times 10^{23} \text{ electrons}$

Conclusion

From the calculations, we see that:

• 1 g of Hydrogen has $6.022 \times 10^{23}$ electrons.
• 2 g of Oxygen has $4.818 \times 10^{23}$ electrons.
• 2 g of Carbon has $6.03 \times 10^{23}$ electrons.
• 2 g of Nitrogen has $6.03 \times 10^{23}$ electrons.

Therefore, 2 g of Carbon and 2 g of Nitrogen have approximately the same number of electrons.