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In a neutral compound, the sum of the oxidation states is zero.Note that the sign of the oxidation states and the number of atomsassociated with each oxidation state must be considered. In H2O ,for example, each hydrogen atom has an oxidation state of +1 andeach oxygen atom has an oxidation state of 2 for a total of2(+1)+(-2)=0 .


Part A:

What is the oxidation state of an individual bromine atom in NaBrO3?
Express the oxidation state numerically (e.g., +1).


Part B:

What is the oxidation state of an individual nitrogen atom in NH2OH?
Express the oxidation state numerically (e.g., +1).



In an ion, the sum of the oxidation states is equal to the overallionic charge. Note that the sign of the oxidation states and thenumber of atoms associated with each oxidation state must beconsidered. In OH- , for example, the oxygen atom has an oxidationstate of -2 and the hydrogen atom has an oxidation state of +1, fora total of (-2)+(+1)=-1.

Part C:

What is the oxidation state of each individual carbon atom inC2O4^2- ?
Express the oxidation state numerically (e.g., +1).

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Patrina Schowalter
Patrina SchowalterLv2
6 Nov 2019

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Related questions

Neutral compounds In a neutral compound, the sum of the oxidation states is zero. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In H2O, for example, each hydrogen atom has an oxidation state of +1 and each oxygen atom has an oxidation state of −2 for a total of 2(+1)+(−2)=0.

Part A:

What is the oxidation state of an individual sulfur atom in BaSO4? Express the oxidation state numerically (e.g., +1).

Part B

What is the oxidation state of an individual nitrogen atom in HNO3? Express the oxidation state numerically (e.g., +1).

In an ion, the sum of the oxidation states is equal to the overall ionic charge. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In OH−, for example, the oxygen atom has an oxidation state of −2 and the hydrogen atom has an oxidation state of +1, for a total of (−2)+(+1)=−1.

Part C:

What is the oxidation state of an individual phosphorus atom in PO33−? Express the oxidation state numerically (e.g., +1).

Part D:

What is the oxidation state of each individual carbon atom in C2O42−?

Oxidation states are important for keeping track of electrons in oxidation-reduction reactions. Here are some general rules to remember:
  • In most cases, oxygen has an oxidation state of ?2.
  • Group 1 and group 2 elements on the periodic table have +1 and +2 oxidation states, respectively.
  • In most cases, hydrogen has an oxidation state of +1.
  • Many elements can have more than one oxidation state. In such cases, use the other elements in the compound whose oxidation states are known to determine the oxidation state of the element that varies.

Neutral compounds

In a neutral compound, the sum of the oxidation states is zero. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In H2O, for example, each hydrogen atom has an oxidation state of +1 and each oxygen atom has an oxidation state of ?2 for a total of 2(+1)+(?2)=0.

Part A

What is the oxidation state of an individual carbon atom in CaCO3?

Express the oxidation state numerically (e.g., +1).

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Part B

What is the oxidation state of an individual nitrogen atom in HNO3?

Express the oxidation state numerically (e.g., +1).

SubmitHintsMy AnswersGive UpReview Part

Ions

In an ion, the sum of the oxidation states is equal to the overall ionic charge. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In OH?, for example, the oxygen atom has an oxidation state of ?2 and the hydrogen atom has an oxidation state of +1, for a total of (?2)+(+1)=?1.

Part C

What is the oxidation state of an individual sulfur atom in SO32??

Express the oxidation state numerically (e.g., +1).

SubmitHintsMy AnswersGive UpReview Part

Part D

What is the oxidation state of each individual carbon atom in C2O42??

Express the oxidation state numerically (e.g., +1).

Constants | Periodic Table

A complex ion is a species in which a central metal ion is attached to a group of surrounding ions or molecules by coordinate covalent bonds. The surrounding species are called ligands. Within a ligand, the atoms that are directly attached to the metal ion (or atom) are called donor atoms. Most ligands contain a single donor atom (monodentate), but some contain two donor atoms (bidentate), six donor atoms (hexadentate), or another combination of donor atoms. A complex ion that is associated with one or more counter ions is called a coordination compound. For example [PdCl4]2−is a complex ion, and Na[PdCl4] is a coordination compound. The following table lists some common ligands.
Ligand Number of
donor atoms
Cl− 1
F− 1
Br− 1
CO32− 2
CN− 1
gly− 2
EDTA4− 6
NH3 1
H2O 1
CO 1
The coordination number for a complex is the total number of donor atoms surrounding the central atom. The overall charge on a complex is the sum of the charges of the metal and all the ligands.

Part A

What is the coordination number for each of the following complexes or compounds?

[Co(NH3)4Cl2]+

[Cr(EDTA)]−

[Zn(H2O)4]2+

Na[Ag(CN)2]

Enter the coordination numbers, in the order that the complexes are listed, as four integers separated by commas (e.g., 1,2,3,4).

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Part B

What is the charge on each of the following complex ions?

hexaaquamanganese(II), [Mn(H2O)6]?

tris(carbonato)aluminate(III), [Al(CO3)3]?

amminepentachloroplatinate(IV), [Pt(NH3)Cl5]?

Express the charges numerically, in the order that the complexes are listed, separated by commas. For a nonzero charge, be sure to include the sign (e.g., +1,-2,+3).

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Part C

What is the oxidation number of the central metal ion in each of the following complexes or compounds?

[NiCl2Br2]2−

[Cr(H2O)2(NH3)4]3+

Na[Au(CN)2]

Express the oxidation numbers numerically, in the order that the complexes are listed, separated by commas. For a nonzero oxidation number, be sure to include the sign (e.g., +1,-2,+3).

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