Question
How many electrons are in:
a. One mole of lithium atoms
b. Two moles of carbon atoms
c. One mole of carbon dioxide molecules
d. Half a mole of methane molecules
a. One mole of lithium atoms
b. Two moles of carbon atoms
c. One mole of carbon dioxide molecules
d. Half a mole of methane molecules
Answers
Answered by
GPT-4o mini
To calculate the number of electrons in each of the provided substances, we can use Avogadro's number, which is approximately \(6.022 \times 10^{23}\) particles (atoms or molecules) per mole.
a. **One mole of lithium atoms**
Lithium (Li) has an atomic number of 3, meaning each lithium atom has 3 electrons.
Number of electrons = \(3 \, \text{electrons/atom} \times 6.022 \times 10^{23} \, \text{atoms}\)
\[
= 1.8066 \times 10^{24} \, \text{electrons}
\]
b. **Two moles of carbon atoms**
Carbon (C) has an atomic number of 6, meaning each carbon atom has 6 electrons.
Number of electrons in two moles = \(2 \, \text{moles} \times 6 \, \text{electrons/atom} \times 6.022 \times 10^{23} \, \text{atoms/mole}\)
\[
= 2 \times 6 \times 6.022 \times 10^{23} = 7.22784 \times 10^{24} \, \text{electrons}
\]
c. **One mole of carbon dioxide molecules**
Each carbon dioxide (CO₂) molecule consists of 1 carbon atom and 2 oxygen atoms. Carbon has 6 electrons, and oxygen (O) has an atomic number of 8, so each oxygen atom has 8 electrons.
Total electrons in one CO₂ molecule:
\[
6 \, (\text{from C}) + 2 \times 8 \, (\text{from 2 O}) = 6 + 16 = 22 \, \text{electrons}
\]
Number of electrons in one mole of CO₂ = \(22 \, \text{electrons/molecule} \times 6.022 \times 10^{23} \, \text{molecules}\)
\[
= 1.32684 \times 10^{25} \, \text{electrons}
\]
d. **Half a mole of methane molecules**
Methane (CH₄) consists of 1 carbon atom and 4 hydrogen atoms.
Total electrons in one CH₄ molecule:
\[
6 \, (\text{from C}) + 4 \times 1 \, (\text{from 4 H}) = 6 + 4 = 10 \, \text{electrons}
\]
Number of electrons in half a mole of CH₄ = \(0.5 \, \text{mole} \times 10 \, \text{electrons/molecule} \times 6.022 \times 10^{23} \, \text{molecules/mole}\)
\[
= 0.5 \times 10 \times 6.022 \times 10^{23} = 3.011 \times 10^{24} \, \text{electrons}
\]
### Summary:
- a. \(1.8066 \times 10^{24} \, \text{electrons}\)
- b. \(7.22784 \times 10^{24} \, \text{electrons}\)
- c. \(1.32684 \times 10^{25} \, \text{electrons}\)
- d. \(3.011 \times 10^{24} \, \text{electrons}\)
a. **One mole of lithium atoms**
Lithium (Li) has an atomic number of 3, meaning each lithium atom has 3 electrons.
Number of electrons = \(3 \, \text{electrons/atom} \times 6.022 \times 10^{23} \, \text{atoms}\)
\[
= 1.8066 \times 10^{24} \, \text{electrons}
\]
b. **Two moles of carbon atoms**
Carbon (C) has an atomic number of 6, meaning each carbon atom has 6 electrons.
Number of electrons in two moles = \(2 \, \text{moles} \times 6 \, \text{electrons/atom} \times 6.022 \times 10^{23} \, \text{atoms/mole}\)
\[
= 2 \times 6 \times 6.022 \times 10^{23} = 7.22784 \times 10^{24} \, \text{electrons}
\]
c. **One mole of carbon dioxide molecules**
Each carbon dioxide (CO₂) molecule consists of 1 carbon atom and 2 oxygen atoms. Carbon has 6 electrons, and oxygen (O) has an atomic number of 8, so each oxygen atom has 8 electrons.
Total electrons in one CO₂ molecule:
\[
6 \, (\text{from C}) + 2 \times 8 \, (\text{from 2 O}) = 6 + 16 = 22 \, \text{electrons}
\]
Number of electrons in one mole of CO₂ = \(22 \, \text{electrons/molecule} \times 6.022 \times 10^{23} \, \text{molecules}\)
\[
= 1.32684 \times 10^{25} \, \text{electrons}
\]
d. **Half a mole of methane molecules**
Methane (CH₄) consists of 1 carbon atom and 4 hydrogen atoms.
Total electrons in one CH₄ molecule:
\[
6 \, (\text{from C}) + 4 \times 1 \, (\text{from 4 H}) = 6 + 4 = 10 \, \text{electrons}
\]
Number of electrons in half a mole of CH₄ = \(0.5 \, \text{mole} \times 10 \, \text{electrons/molecule} \times 6.022 \times 10^{23} \, \text{molecules/mole}\)
\[
= 0.5 \times 10 \times 6.022 \times 10^{23} = 3.011 \times 10^{24} \, \text{electrons}
\]
### Summary:
- a. \(1.8066 \times 10^{24} \, \text{electrons}\)
- b. \(7.22784 \times 10^{24} \, \text{electrons}\)
- c. \(1.32684 \times 10^{25} \, \text{electrons}\)
- d. \(3.011 \times 10^{24} \, \text{electrons}\)