To determine the charges that each atom typically makes when bonding with other atoms, we can refer to the common oxidation states of the elements based on their position in the periodic table. Here's the correlation for each element:
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Calcium (Ca): h. +2 (Calcium typically loses 2 electrons to achieve a stable configuration.)
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Francium (Fr): b. +1 (As an alkali metal, Francium generally loses 1 electron.)
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Bromine (Br): d. -1 (Bromine, a halogen, typically gains 1 electron.)
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Sulfur (S): f. -2 (Sulfur often gains 2 electrons in compounds.)
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Xenon (Xe): c. 0 (Xenon is a noble gas and is generally inert, not forming bonds.)
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Carbon (C): g. +4/-4 (Carbon can both gain and lose electrons, hence can have oxidation states of +4 or -4.)
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Phosphorous (P): e. +3 (Phosphorus typically has a charge of +3 when it forms bonds, although it can also show other oxidation states.)
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Boron (B): a. -3 (Boron generally can have a charge of +3 in compounds, but is peculiar as it often forms covalent bonds rather than ionic ones; however, if we consider its less common state, it can be -3 in specific circumstances.)
So, the final pairings would be:
- Calcium (Ca) - h. +2
- Francium (Fr) - b. +1
- Bromine (Br) - d. -1
- Sulfur (S) - f. -2
- Xenon (Xe) - c. 0
- Carbon (C) - g. +4/-4
- Phosphorous (P) - e. +3
- Boron (B) - a. -3