Question

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determine the charge each atom will make when it bonds with other atoms.
Bromine (Br)
Sulfur (S):
Xenon (Xe):
Carbon (C):

Answer 1

The charge that an atom will make when it bonds with other atoms depends on its valence electrons and its tendency to gain or lose electrons to achieve a stable electron configuration. Here's how these elements typically behave:

1. Bromine (Br):

Bromine is in Group 17 (also known as Group VIIA or the halogens) of the periodic table. It has 7 valence electrons and tends to gain 1 electron to achieve a full valence shell. Therefore, bromine typically forms a -1 charge (Br^-) when it bonds with other elements.

2. Sulfur (S):

Sulfur is in Group 16 (also known as Group VIB or the chalcogens) of the periodic table. It has 6 valence electrons and can either gain 2 electrons or share 2 electrons to achieve a full valence shell. Sulfur can form either a -2 charge (S^2-) or a +4 charge (S^4+) depending on the specific bonding context.

3. Xenon (Xe):

Xenon is in Group 18 (also known as the noble gases) of the periodic table. Noble gases are generally unreactive and prefer not to bond with

other elements. Xenon usually does not form ions or bonds readily with other atoms in its elemental form.

4. Carbon (C):

Carbon is in Group 14 of the periodic table. It has 4 valence electrons and can either share electrons in covalent bonds or lose/gain electrons to achieve a full valence shell, depending on the bonding situation. Carbon can form -4 charges (C^4-) when it gains 4 electrons

or +4 charges (C^4+) when it loses 4 electrons. However, in most organic compounds, carbon forms covalent bonds by sharing electrons rather than forming ions.

It's important to note that the charges mentioned above are general guidelines based on the periodic table. The actual charges in chemical compounds may vary depending on the specific atoms and their bonding partners.

Answer 2

When atoms bond with other atoms, they form chemical compounds by sharing or transferring electrons. The charge that an atom will make when it bonds with other atoms depends on its position in the periodic table and its electron configuration.

Step-by-step explanation:

Here are the charges that each atom will make when it bonds with other atoms:

1. Bromine (Br): Bromine belongs to group 17 of the periodic table, also known as the halogens. Halogens tend to gain one electron to achieve a stable octet configuration. Therefore, when bromine bonds with other atoms, it will typically have a charge of -1.

2. Sulfur (S): Sulfur belongs to group 16 of the periodic table. Like the halogens, sulfur also tends to gain two electrons to achieve a stable octet configuration. Hence, when sulfur bonds with other atoms, it will generally have a charge of -2.

3. Xenon (Xe): Xenon is a noble gas and belongs to group 18 of the periodic table. Noble gases are chemically inert and do not easily form bonds. Therefore, xenon usually does not have a charge when it bonds with other atoms.

4. Carbon (C): Carbon belongs to group 14 of the periodic table and forms the basis of organic chemistry. Carbon can either gain or lose electrons to achieve a stable configuration. However, in most common organic compounds, carbon shares electrons and does not have a significant charge.

It is important to note that these charges are general trends and can vary depending on the specific compound and the bonding situation. Also, there are cases where atoms can have different charges depending on the bonding partners and the specific arrangement of electrons. Therefore, it is essential to consider the specific context and chemical formula when determining the charges of atoms in compounds.

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