Question

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.-3
b.0
c.+2
d.+4/-4
e.-2
f.-1
g.+1
h.+3

Answer 1

Here’s the determination of the typical charges each of the listed atoms will take when bonding with other atoms:

1. **Calcium (Ca)**:
- Charge: **c. +2** (Calcium is an alkaline earth metal and typically loses two electrons.)

2. **Francium (Fr)**:
- Charge: **g. +1** (Francium is an alkali metal and typically loses one electron, although it is highly radioactive and reactive.)

3. **Bromine (Br)**:
- Charge: **f. -1** (Bromine is a halogen that typically gains one electron.)

4. **Sulfur (S)**:
- Charge: **e. -2** (Sulfur commonly gains two electrons when forming compounds, especially in ionic compounds.)

5. **Xenon (Xe)**:
- Charge: **b. 0** (Xenon is a noble gas and typically does not form bonds, hence it has a formal charge of zero.)

6. **Carbon (C)**:
- Charge: **d. +4/-4** (Carbon can form four bonds (typically loses 4 electrons) or gain 4 electrons, resulting in a variety of possible charges depending on the context of the bonding.)

7. **Phosphorous (P)**:
- Charge: **h. +3** (Phosphorus can have different oxidation states, but it commonly exhibits +3 charge in many of its compounds.)

8. **Boron (B)**:
- Charge: **a. -3** (Boron typically can form covalent bonds and can exhibit positive charges, but when involved in certain types of ionic compounds, it can act as a -3.)

Here are the pairings for clarification:

- **Calcium (Ca)**: +2 (c)
- **Francium (Fr)**: +1 (g)
- **Bromine (Br)**: -1 (f)
- **Sulfur (S)**: -2 (e)
- **Xenon (Xe)**: 0 (b)
- **Carbon (C)**: +4/-4 (d)
- **Phosphorous (P)**: +3 (h)
- **Boron (B)**: -3 (a) (Note: The typical behavior of boron, while it can accept three electrons, is often considered as sharing due to its covalent nature. In ionic contexts, -3 can sometimes be attributed in theoretical models.)