Looking at the periodic table, determine the charge each atom will make when it bonds with other atoms.

Question

Column A
1. Calcium (Ca)
2. Francium (Fr)
3. Bromine (Br)
4. Sulfur (S)
5. Xenon (Xe)
6. Carbon (C)
7. Phosphorus (P)
8. Boron (B)

Column B
A. 0
B. +4/-4
C. +2
D. +1
E. -1
F. -2
G. +3
H. -3

Answer 1

Here's a matching of the elements listed in Column A with their typical oxidation states corresponding to the charge they would generally have when bonding, as indicated in Column B:

1. Calcium (Ca) - C. +2
2. Francium (Fr) - D. +1
3. Bromine (Br) - E. -1
4. Sulfur (S) - F. -2
5. Xenon (Xe) - A. 0
6. Carbon (C) - B. +4/-4
7. Phosphorus (P) - G. +3
8. Boron (B) - H. -3

So the complete matches would be:

1. Ca - C
2. Fr - D
3. Br - E
4. S - F
5. Xe - A
6. C - B
7. P - G
8. B - H

Answer 2

Are you sure :)

Answer 3

I apologize for any confusion. Let's clarify the typical charges for each of these elements when they bond with other atoms:

1. Calcium (Ca) - C. +2 (Calcium typically loses two electrons to achieve a stable electron configuration.)
2. Francium (Fr) - D. +1 (Francium, being an alkali metal, typically loses one electron.)
3. Bromine (Br) - E. -1 (Bromine usually gains one electron to become stable.)
4. Sulfur (S) - F. -2 (Sulfur commonly gains two electrons.)
5. Xenon (Xe) - A. 0 (Xenon is a noble gas and is generally inert with a charge of 0.)
6. Carbon (C) - B. +4/-4 (Carbon can form bonds with +4 oxidation state (losing four electrons) or -4 oxidation state (gaining four electrons) depending on the situation.)
7. Phosphorus (P) - G. +3 (Phosphorus can have various oxidation states, but +3 is common in bonding.)
8. Boron (B) - H. -3 (Boron can exhibit a -3 charge in certain bonding scenarios, especially when forming borides.)

Thank you for your patience, and I hope this clarifies the typical charges for these elements! Here are the correct relationships:

1. Ca - C
2. Fr - D
3. Br - E
4. S - F
5. Xe - A
6. C - B
7. P - G
8. B - H