3 answers
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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.-1
b.+3
c.+1
d.-3
e.-2
f.+4/-4
g.0
h.+2
Column A:
1. Calcium (Ca): +2
2. Francium (Fr): +1
3. Bromine (Br): -1
4. Sulfur (S): -2
5. Xenon (Xe): 0
6. Carbon (C): +4/-4
7. Phosphorus (P): +3/-3
8. Boron (B): +3
Column B:
a. -1
b. +3
c. +1
d. -3
e. -2
f. +4/-4
g. 0
h. +2
Let's go through the elements in Column A and determine the charges they will make when they bond with other atoms, based on the information provided in Column B.
1. Calcium (Ca):
The charge of Calcium is typically +2 (answer h).
2. Francium (Fr):
The charge of Francium is typically +1 (answer c).
3. Bromine (Br):
The charge of Bromine is typically -1 (answer a).
4. Sulfur (S):
The charge of Sulfur can vary, but it commonly forms a charge of -2 (answer e).
5. Xenon (Xe):
Xenon is a noble gas and generally does not form bonds or charge (answer g).
6. Carbon (C):
Carbon usually forms a charge of -4 or +4, depending on the bonding arrangement (answer f).
7. Phosphorous (P):
Phosphorous commonly forms a charge of -3 (answer d).
8. Boron (B):
Boron commonly forms a charge of +3 (answer b).
So, the charges each atom will make when it bonds with other atoms are:
1. Calcium (Ca): +2
2. Francium (Fr): +1
3. Bromine (Br): -1
4. Sulfur (S): -2
5. Xenon (Xe): 0
6. Carbon (C): +4/-4
7. Phosphorous (P): -3
8. Boron (B): +3
To determine the charge each atom will make when it bonds with other atoms, we need to look at the group or column in which each element is located on the periodic table.
1. Calcium (Ca) - Column B: Calcium is in Group 2, so it tends to lose 2 electrons to achieve a stable configuration. Therefore, the charge it makes when it bonds is +2.
2. Francium (Fr) - Column B: Francium is in Group 1, also known as the alkali metals. These elements tend to lose 1 electron, so Francium's charge when it bonds is +1.
3. Bromine (Br) - Column A: Bromine is in Group 17, also known as the halogens. These elements tend to gain 1 electron, so Bromine's charge when it bonds is -1.
4. Sulfur (S) - Column A: Sulfur is also in Group 17, like Bromine. So, its charge when it bonds is -2, similar to other members of this group.
5. Xenon (Xe) - Column A: Xenon is in Group 18, also known as the noble gases. Noble gases are generally stable and do not readily form bonds with other elements, so Xenon's charge is 0.
6. Carbon (C) - Column A: Carbon is in Group 14. It neither readily gains nor loses 4 electrons to achieve a stable configuration. Instead, it tends to share electrons in covalent bonds. Therefore, Carbon's charge when it bonds is 0.
7. Phosphorous (P) - Column A: Phosphorous is in Group 15. It tends to gain 3 electrons to achieve a stable configuration, so its charge when it bonds is -3.
8. Boron (B) - Column A: Boron is in Group 13. It tends to lose 3 electrons to achieve a stable configuration, so its charge when it bonds is +3.
To summarize:
- Calcium (Ca): +2
- Francium (Fr): +1
- Bromine (Br): -1
- Sulfur (S): -2
- Xenon (Xe): 0
- Carbon (C): 0
- Phosphorous (P): -3
- Boron (B): +3