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): d. +1
3. Bromine (Br): f. -1
4. Sulfur (S): f. -2
5. Xenon (Xe): b. 0
6. Carbon (C): g. -4
7. Phosphorous (P): c. +3
8. Boron (B): h. +3
Column A | Column B
--------------------------------------------------------------
1. Calcium (Ca) | c. +2
2. Francium (Fr) | h. +1
3. Bromine (Br) | f. -1
4. Sulfur (S) | f. -1
5. Xenon (Xe) | e. -2
6. Carbon (C) | d. +1
7. Phosphorous (P) | d. +1
8. Boron (B) | a. +3
To determine the charge each atom will make when it bonds with other atoms, you can refer to the periodic table. Charges are typically determined by the number of valence electrons an atom possesses.
1. Calcium (Ca): Calcium belongs to column 2 of the periodic table, which means it has 2 valence electrons. Calcium tends to lose these electrons when it forms bonds, resulting in a charge of +2.
2. Francium (Fr): Francium belongs to column 1 of the periodic table, which means it has 1 valence electron. Francium tends to lose this electron when it forms bonds, resulting in a charge of +1.
3. Bromine (Br): Bromine belongs to column 17 (Group 7A) of the periodic table and has 7 valence electrons. Bromine tends to gain 1 electron to achieve a stable octet, resulting in a charge of -1.
4. Sulfur (S): Sulfur belongs to column 16 (Group 6A) of the periodic table and has 6 valence electrons. Sulfur tends to gain 2 electrons to achieve a stable octet, resulting in a charge of -2.
5. Xenon (Xe): Xenon belongs to column 18 (Group 8A or noble gases) of the periodic table and has a full octet with 8 valence electrons. Xenon generally does not form bonds with other atoms, so it typically has a charge of 0.
6. Carbon (C): Carbon belongs to column 14 (Group 4A) of the periodic table and has 4 valence electrons. Carbon can either gain or lose electrons to achieve a stable octet, resulting in multiple potential charges. Common charges for carbon include -4, -2, +2, and +4, depending on the specific molecule it forms bonds with. Therefore, the charge of carbon (C) can vary.
7. Phosphorus (P): Phosphorus belongs to column 15 (Group 5A) of the periodic table and has 5 valence electrons. Phosphorus tends to gain 3 electrons to achieve a stable octet, resulting in a charge of -3.
8. Boron (B): Boron belongs to column 13 (Group 3A) of the periodic table and has 3 valence electrons. Boron tends to lose 3 electrons when it forms bonds, resulting in a charge of +3.
Using the information provided in Column B, you can match the charges to the respective atoms:
a. +4/-4: This charge is not matched to any of the given atoms.
b. 0: Xenon (Xe) has a charge of 0.
c. +2: Calcium (Ca) has a charge of +2.
d. +1: Francium (Fr) has a charge of +1.
e. -2: Sulfur (S) has a charge of -2.
f. -1: Bromine (Br) has a charge of -1.
g. -3: Phosphorus (P) has a charge of -3.
h. +3: Boron (B) has a charge of +3.
It is important to note that these charges represent the most common or typical charges for these elements when they form bonds. In certain compounds or under specific conditions, the charges may vary.