Column A Column B
1. Calcium (Ca): b. +2
2. Francium (Fr): a. +1
3. Bromine (Br): d. -1
4. Sulfur (S): e. -2
5. Xenon (Xe): f. 0
6. Carbon (C): f. 0
7. Phosphorous (P): c. -3
8. Boron (B): h. +3
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.+2
c.-3
d.-1
e.-2
f.0
g.+4/-4
h.+3
1. Calcium (Ca): b. +2
2. Francium (Fr): a. +1
3. Bromine (Br): d. -1
4. Sulfur (S): e. -2
5. Xenon (Xe): f. 0
6. Carbon (C): f. 0
7. Phosphorous (P): c. -3
8. Boron (B): h. +3
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
8. Boron (B): +3
Please note that the charges mentioned are general tendencies and may vary depending on the specific compound and bonding context.
1. Calcium (Ca): Calcium is located in Group 2 of the periodic table, which means it has 2 valence electrons. When calcium bonds, it tends to lose these 2 valence electrons, resulting in a charge of +2 (option b).
2. Francium (Fr): Francium is located in Group 1 of the periodic table, which means it has 1 valence electron. When francium bonds, it tends to lose this valence electron, resulting in a charge of +1 (option a).
3. Bromine (Br): Bromine is located in Group 17 of the periodic table, which means it has 7 valence electrons. When bromine bonds, it tends to gain 1 electron to achieve a stable octet configuration, resulting in a charge of -1 (option d).
4. Sulfur (S): Sulfur is located in Group 16 of the periodic table, which means it has 6 valence electrons. When sulfur bonds, it can either gain 2 electrons to achieve a stable octet configuration, resulting in a charge of -2 (option e), or it can lose 6 electrons to form a +6 charge (not listed in the given options).
5. Xenon (Xe): Xenon is located in Group 18 of the periodic table, which means it has 8 valence electrons. Xenon is a noble gas and is generally unreactive, so it commonly has a charge of 0 (option f). However, in certain chemical reactions, it can form compounds with a variety of different charges.
6. Carbon (C): Carbon is located in Group 14 of the periodic table, which means it has 4 valence electrons. Carbon can either gain 4 electrons to achieve a stable octet configuration, resulting in a charge of -4 (option g), or it can lose 4 electrons to form a +4 charge (not listed in the given options).
7. Phosphorus (P): Phosphorus is located in Group 15 of the periodic table, which means it has 5 valence electrons. When phosphorus bonds, it can gain 3 electrons to achieve a stable octet configuration, resulting in a charge of -3 (option c).
8. Boron (B): Boron is located in Group 13 of the periodic table, which means it has 3 valence electrons. When boron bonds, it tends to lose 3 valence electrons, resulting in a charge of +3 (option h).
Please note that there may be other charges possible for each element depending on the specific compounds and bonding situations.