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.+1
c.+2
d.-1
e.+3
f.0
g.-3
h.-2
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
Column A:
1. Calcium (Ca): Calcium (Ca) is in Group 2, which means it typically forms a +2 charge.
2. Francium (Fr): Francium (Fr) is in Group 1, which means it typically forms a +1 charge.
3. Bromine (Br): Bromine (Br) is in Group 17, which means it typically forms a -1 charge.
4. Sulfur (S): Sulfur (S) is in Group 16, which means it typically forms a -2 charge.
5. Xenon (Xe): Xenon (Xe) is in Group 18, which means it typically does not form ions and has a 0 charge.
6. Carbon (C): Carbon (C) is in Group 14, which means it can form various charges. It can form a -4 charge (as in CH4 or methane) or a +4 charge (as in CO2 or carbon dioxide).
7. Phosphorous (P): Phosphorus (P) is in Group 15, which means it typically forms a -3 charge.
8. Boron (B): Boron (B) is in Group 13, which means it typically forms a +3 charge.
Column B:
a. +4/-4
b. +1
c. +2
d. -1
e. +3
f. 0
g. -3
h. -2
Matching the atoms from Column A with the corresponding charges in Column B:
1. Calcium (Ca): c. +2
2. Francium (Fr): b. +1
3. Bromine (Br): d. -1
4. Sulfur (S): g. -2
5. Xenon (Xe): f. 0
6. Carbon (C): a. +4/-4 or f. 0 (depending on the compound it forms)
7. Phosphorus (P): g. -3
8. Boron (B): e. +3
To determine the charge each atom will make when it bonds with other atoms, you need to refer to the periodic table and consider the electron configuration of each element.
Column A lists the elements: Calcium (Ca), Francium (Fr), Bromine (Br), Sulfur (S), Xenon (Xe), Carbon (C), Phosphorous (P), and Boron (B).
Column B provides the options for the charges: +4/-4, +1, +2, -1, +3, 0, -3, and -2.
To determine the charge, you need to consider the group or column each element belongs to in the periodic table. Elements in the same group tend to have similar charges because they have the same number of valence electrons.
Here is a breakdown of the charges for each element:
1. Calcium (Ca) - Calcium is in Group 2, so it tends to lose two electrons to form a +2 charge (option c: +2).
2. Francium (Fr) - Francium is in Group 1, so it tends to lose one electron to form a +1 charge (option b: +1).
3. Bromine (Br) - Bromine is in Group 17, so it tends to gain one electron to form a -1 charge (option d: -1).
4. Sulfur (S) - Sulfur is in Group 16, so it tends to gain two electrons to form a -2 charge (option h: -2).
5. Xenon (Xe) - Xenon is in Group 18, which is a noble gas group. Noble gases rarely form bonds and usually have a charge of 0 (option f: 0).
6. Carbon (C) - Carbon is in Group 14, so it can either lose or gain four electrons to form a charge. However, it commonly shares electrons with other atoms through covalent bonds instead of forming ionic bonds. Therefore, it doesn't have a fixed charge and has a charge of 0 (option f: 0).
7. Phosphorous (P) - Phosphorous is in Group 15, so it tends to gain three electrons to form a -3 charge (option g: -3).
8. Boron (B) - Boron is in Group 13, so it tends to lose three electrons to form a +3 charge (option e: +3).
Remember that these charges are not absolute, and they can vary depending on the specific chemical environment and the atoms it interacts with. However, the provided options give you a general idea of the charge each atom tends to form during bonding.