Question 2

Question

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

Column A
1.
Calcium (Ca):
Calcium (Ca)
2.
Francium (Fr):
Francium (Fr)
3.
Bromine (Br):
Bromine (Br)
4.
Sulfur (S):
Sulfur (S)
5.
Xenon (Xe):
Xenon (Xe)
6.
Carbon (C):
Carbon (C)
7.
Phosphorous (P):
Phosphorous (P)
8.
Boron (B):
Boron (B)
Column B
a.-2
b.+2
c.0
d.+3
e.-3
f.+4/-4
g.+1
h.-1

Answer 1

Here is the charge each atom is likely to make when it bonds with other atoms:

1. Calcium (Ca): b. +2
   Calcium is an alkaline earth metal and typically loses two electrons to achieve a stable octet.

2. Francium (Fr): g. +1
   Francium is an alkali metal and typically loses one electron to achieve a stable octet.

3. Bromine (Br): h. -1
   Bromine is a halogen and typically gains one electron to achieve a stable octet.

4. Sulfur (S): a. -2
   Sulfur typically gains two electrons to achieve a stable octet.

5. Xenon (Xe): c. 0
   Xenon is a noble gas and generally does not form bonds, maintaining a stable octet.

6. Carbon (C): f. +4/-4
   Carbon can either gain or lose four electrons to achieve a stable octet, resulting in a charge of either +4 or -4 based on the bonding situation.

7. Phosphorous (P): d. +3
   Phosphorus commonly forms three bonds and can adopt a +3 charge in certain bonding situations.

8. Boron (B): d. +3
   Boron typically forms three bonds and has a +3 charge when bonding.

So, here are the charges for each atom:

• Calcium (Ca): +2
• Francium (Fr): +1
• Bromine (Br): -1
• Sulfur (S): -2
• Xenon (Xe): 0
• Carbon (C): +4/-4
• Phosphorus (P): +3
• Boron (B): +3