The oxidation number of an element represents the charge that it would have if all the bonds in the compound were completely ionic.
In Mg3[CrCl5Br]2, Mg has an oxidation number of +2 because it is in Group 2 of the periodic table and typically loses two electrons to achieve a stable octet configuration.
The compound contains one Cr atom, which is a transition metal. The oxidation number of Cr can vary, but in this case, it can be determined by considering the charges of the other ions in the compound. Each Cl ion has a charge of -1, and there are five Cl ions in the compound, so their total charge is -5. Each Br ion also has a charge of -1, and there are two Br ions in the compound, so their total charge is -2.
Since the compound as a whole must be neutral, the sum of the charges of all the ions must equal zero. Therefore, the oxidation number of Cr can be calculated as follows:
Oxidation number of Cr + Sum of charges of Cl ions + Sum of charges of Br ions = 0
Oxidation number of Cr - 5 + (-2) = 0
Oxidation number of Cr = +7
Therefore, the oxidation number of Cr in Mg3[CrCl5Br]2 is +7.
The coordination number in a compound represents the number of atoms, ions, or molecules that are bonded to the central metal ion. In Mg3[CrCl5Br]2, the coordination number of Cr is 6 because it is bonded to five Cl ions and one Br ion.
[Mg3 [CrCl5Br]2 state oxidation number and coordination number
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Mg3 [CrCl5Br]2 state oxidation number and coordination number
Apologies for the mistake in my previous response. Let me correct it.
In the compound Mg3[CrCl5Br]2, the oxidation number of Mg is +2 as it is in Group 2 of the periodic table.
Now let's determine the oxidation number of Cr. Each Cl ion has a charge of -1, and there are five Cl ions present. Each Br ion has a charge of -1, and there are two Br ions present. The total charge of the Cl ions is (-1) * 5 = -5. The total charge of the Br ions is (-1) * 2 = -2.
Since the overall charge of the compound must be neutral, the sum of the charges of all the ions must add up to zero. Therefore, the oxidation number of Cr can be calculated as follows:
Oxidation number of Cr + Sum of charges of Cl ions + Sum of charges of Br ions = 0
Oxidation number of Cr - 5 + (-2) = 0
Oxidation number of Cr = +7
Therefore, the oxidation number of Cr in Mg3[CrCl5Br]2 is +7.
The coordination number of Cr in this compound is 6 because it is bonded to five Cl ions and one Br ion.
In the compound Mg3[CrCl5Br]2, the oxidation number of Mg is +2 as it is in Group 2 of the periodic table.
Now let's determine the oxidation number of Cr. Each Cl ion has a charge of -1, and there are five Cl ions present. Each Br ion has a charge of -1, and there are two Br ions present. The total charge of the Cl ions is (-1) * 5 = -5. The total charge of the Br ions is (-1) * 2 = -2.
Since the overall charge of the compound must be neutral, the sum of the charges of all the ions must add up to zero. Therefore, the oxidation number of Cr can be calculated as follows:
Oxidation number of Cr + Sum of charges of Cl ions + Sum of charges of Br ions = 0
Oxidation number of Cr - 5 + (-2) = 0
Oxidation number of Cr = +7
Therefore, the oxidation number of Cr in Mg3[CrCl5Br]2 is +7.
The coordination number of Cr in this compound is 6 because it is bonded to five Cl ions and one Br ion.
state oxidation number and coordination number for the following
K[Co(H2O)2(C2O4)2]
[Ru(H2O)2(NH3)2Cl2]Br
K[Co(H2O)2(C2O4)2]
[Ru(H2O)2(NH3)2Cl2]Br
In K[Co(H2O)2(C2O4)2], the oxidation number of K is +1 because it is an alkali metal in Group 1 of the periodic table.
To determine the oxidation number of Co, we need to consider the oxidation states of the other elements in the compound. Each water (H2O) molecule is neutral and does not influence the oxidation state, and each oxalate (C2O4)2- ion has an overall charge of -2. Since there are two oxalate ions, their total charge is -4. The compound K[Co(H2O)2(C2O4)2] is neutral, so the sum of the oxidation states must equal zero:
Oxidation number of Co + Sum of charges of C2O4 ions = 0
Oxidation number of Co - 4 = 0
Oxidation number of Co = +4
Therefore, the oxidation number of Co in K[Co(H2O)2(C2O4)2] is +4.
The coordination number of Co in this compound is 6. It is bonded to two water molecules (H2O) and four oxalate ions (C2O4)2-.
In [Ru(H2O)2(NH3)2Cl2]Br, the oxidation number of Br is -1 because it is a halogen in Group 17 of the periodic table.
For Ru, each water (H2O) molecule is neutral, ammonia (NH3) has a neutral charge, and each chloride (Cl) ion has a charge of -1. Since there are two chloride ions, their total charge is -2. The compound [Ru(H2O)2(NH3)2Cl2]Br is neutral, so the sum of the oxidation states must equal zero:
Oxidation number of Ru + Sum of charges of Cl ions + Oxidation number of Br = 0
Oxidation number of Ru - 2 - 1 = 0
Oxidation number of Ru = +3
Therefore, the oxidation number of Ru in [Ru(H2O)2(NH3)2Cl2]Br is +3.
The coordination number of Ru in this compound is also 6. It is bonded to two water molecules (H2O), two ammonia molecules (NH3), and two chloride ions (Cl-).
To determine the oxidation number of Co, we need to consider the oxidation states of the other elements in the compound. Each water (H2O) molecule is neutral and does not influence the oxidation state, and each oxalate (C2O4)2- ion has an overall charge of -2. Since there are two oxalate ions, their total charge is -4. The compound K[Co(H2O)2(C2O4)2] is neutral, so the sum of the oxidation states must equal zero:
Oxidation number of Co + Sum of charges of C2O4 ions = 0
Oxidation number of Co - 4 = 0
Oxidation number of Co = +4
Therefore, the oxidation number of Co in K[Co(H2O)2(C2O4)2] is +4.
The coordination number of Co in this compound is 6. It is bonded to two water molecules (H2O) and four oxalate ions (C2O4)2-.
In [Ru(H2O)2(NH3)2Cl2]Br, the oxidation number of Br is -1 because it is a halogen in Group 17 of the periodic table.
For Ru, each water (H2O) molecule is neutral, ammonia (NH3) has a neutral charge, and each chloride (Cl) ion has a charge of -1. Since there are two chloride ions, their total charge is -2. The compound [Ru(H2O)2(NH3)2Cl2]Br is neutral, so the sum of the oxidation states must equal zero:
Oxidation number of Ru + Sum of charges of Cl ions + Oxidation number of Br = 0
Oxidation number of Ru - 2 - 1 = 0
Oxidation number of Ru = +3
Therefore, the oxidation number of Ru in [Ru(H2O)2(NH3)2Cl2]Br is +3.
The coordination number of Ru in this compound is also 6. It is bonded to two water molecules (H2O), two ammonia molecules (NH3), and two chloride ions (Cl-).
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