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.+4/-4
b.0
c.+2
d.+1
e.-2
f.-1
g.-3
h.+3
Column A Column B
1. Calcium (Ca): c. +2
2. Francium (Fr): h. +1
3. Bromine (Br): f. -1
4. Sulfur (S): e. -2
5. Xenon (Xe): g. -3
6. Carbon (C): b. 0
7. Phosphorus (P): a. +4/-4
8. Boron (B): d. +3
To determine the charge each atom will make when it bonds with other atoms, you need to consider the group number or the number of valence electrons.
Let's go through each atom in Column A:
1. Calcium (Ca): Calcium belongs to Group 2 in the periodic table, which means it has 2 valence electrons. Calcium tends to lose these 2 electrons to achieve a stable octet configuration, resulting in a charge of +2.
2. Francium (Fr): Francium is an alkali metal and belongs to Group 1 of the periodic table. As with all alkali metals, Francium tends to lose 1 electron to achieve a stable octet configuration, resulting in a charge of +1.
3. Bromine (Br): Bromine belongs to Group 17 (or Group 7A) in the periodic table. It has 7 valence electrons and tends to gain 1 electron to complete its octet, resulting in a charge of -1.
4. Sulfur (S): Sulfur belongs to Group 16 (or Group 6A) in the periodic table. It has 6 valence electrons and can either gain or lose 2 electrons to achieve a stable configuration, resulting in charges of either -2 or +6, depending on the specific compound it bonds with.
5. Xenon (Xe): Xenon belongs to Group 18 (or Group 8A) in the periodic table. It has a full octet of 8 valence electrons, making it stable and unlikely to form bonds with other atoms. Therefore, xenon usually does not have a charge (-).
6. Carbon (C): Carbon belongs to Group 14 (or Group 4A) in the periodic table. It has 4 valence electrons and can either gain or lose 4 electrons to achieve a stable configuration. Carbon commonly forms bonds by sharing electrons rather than gaining or losing them. Therefore, carbon typically does not have a charge (0).
7. Phosphorus (P): Phosphorus belongs to Group 15 (or Group 5A) in the periodic table. It has 5 valence electrons and tends to gain 3 electrons to achieve a stable Octet configuration, resulting in a charge of -3.
8. Boron (B): Boron belongs to Group 13 (or Group 3A) in the periodic table. It has 3 valence electrons and tends to lose these 3 electrons to achieve a stable configuration, resulting in a charge of +3.
Now let's match each atom in Column A with the appropriate charge in Column B:
1. Calcium (Ca): c) +2
2. Francium (Fr): d) +1
3. Bromine (Br): f) -1
4. Sulfur (S): a) +4/-4 (depending on the specific compound)
5. Xenon (Xe): b) 0
6. Carbon (C): b) 0
7. Phosphorus (P): g) -3
8. Boron (B): h) +3
Note that the charges mentioned here are the most common charges these atoms form when bonding with other atoms, but the actual charges can vary depending on the specific compound and the elements it bonds with.