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

Question

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.-1
b.+1
c.-3
d.+2
e.+4/-4
f.-2
g.+3
h.0

Answer 1

Here are the charges each atom will typically make when it bonds with other atoms:

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

2. Francium (Fr): b. +1
   Francium is an alkali metal and tends to lose one electron, making its common oxidation state +1.

3. Bromine (Br): a. -1
   Bromine is a halogen and generally gains one electron to achieve a stable electron configuration, resulting in a -1 charge.

4. Sulfur (S): f. -2
   Sulfur typically gains two electrons to fill its valence shell, which gives it a -2 charge.

5. Xenon (Xe): h. 0
   Xenon is a noble gas with a full valence shell and generally does not form bonds in typical chemical reactions, thus it has a charge of 0.

6. Carbon (C): e. +4/-4
   Carbon can form four covalent bonds by either gaining or losing electrons, so it can have a charge of +4 (when it loses electrons) or -4 (when it gains electrons) depending on the context.

7. Phosphorous (P): c. -3
   Phosphorus often gains three electrons to complete its valence shell, giving it a typical charge of -3.

8. Boron (B): g. +3
   Boron typically loses three electrons when it forms bonds, resulting in a +3 charge.

In summary, the paired answers are:

1. d
2. b
3. a
4. f
5. h
6. e
7. c
8. g