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.+2
c.-3
d.-1
e.-2
f.0
g.+4/-4
h.+3
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 contains different elements from the periodic table, and column B lists the possible charges that each atom will make when it bonds with other atoms. Here are the charges for the atoms in 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
8. Boron (B): +3
Please note that the charges mentioned are general tendencies and may vary depending on the specific compound and bonding context.
To determine the charge each atom will make when it bonds with other atoms, you can refer to the periodic table. The charge of an atom is influenced by its position on the periodic table and the number of valence electrons it has.
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.