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Complete the table below for calculating the molar mass of the ionic compound chromium(II) fluoride.
Formula
Molar mass of ion
Number of ions
mol =
mol =
Mass of ion in one mole of chromium(II) fluoride
9
g
Cation
Cr2+
X
g/mol
Anion
F
X
g/mol
Molar mass chromium(II) fluoride = g/mol
The Correct Answer and Explanation is :
To calculate the molar mass of chromium(II) fluoride (CrF₂), we need to break it down into its components: the cation (Cr²⁺) and the anion (F⁻). Let’s first identify the molar mass of each ion.
- Cation: Cr²⁺ (Chromium ion)
The atomic mass of chromium (Cr) is approximately 52.00 g/mol. Since it has a +2 charge (Cr²⁺), this value is the same as the atomic mass. - Anion: F⁻ (Fluoride ion)
The atomic mass of fluorine (F) is approximately 19.00 g/mol.
Now, let’s use this information to fill out the table:
Table
| Formula | Molar Mass of Ion | Number of Ions | mol = | Mass of Ion in One Mole of Chromium(II) Fluoride |
|---|---|---|---|---|
| Cation (Cr²⁺) | 52.00 g/mol | 2 | mol | 104.00 g/mol (2 × 52.00) |
| Anion (F⁻) | 19.00 g/mol | 2 | mol | 38.00 g/mol (2 × 19.00) |
| Molar Mass CrF₂ | mol | 142.00 g/mol (104.00 + 38.00) |
Explanation:
To determine the molar mass of chromium(II) fluoride (CrF₂), we need to consider the mass of each individual ion and how many ions are present in one formula unit of CrF₂.
- Chromium(II) fluoride has one Cr²⁺ ion and two F⁻ ions in each formula unit (CrF₂).
- The molar mass of Cr²⁺ is 52.00 g/mol.
- The molar mass of F⁻ is 19.00 g/mol.
To find the molar mass of CrF₂, we multiply the number of each ion by its molar mass:
- The Cr²⁺ ion contributes 52.00 g/mol × 1 = 52.00 g/mol.
- The F⁻ ions contribute 19.00 g/mol × 2 = 38.00 g/mol.
Summing these gives us:
[ 52.00 \, \text{g/mol} + 38.00 \, \text{g/mol} = 90.00 \, \text{g/mol} ]
Thus, the molar mass of chromium(II) fluoride is 142.00 g/mol.
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