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Polyatomic molecules, oxidation numbers

Hydrogen in a molecule. Hydrogen in a polyatomic ion, oxidation number +1 oxidation number +1... [Pg.217]

The concept of oxidation number is used to simplify the electron bookkeeping in redox reactions. For a monatomic ion (e.g., Na+, S2 ), the oxidation number is, quite simply, the charge of the ion (+1, —2). In a molecule or polyatomic ion, the oxidation number of an element is a pseudo-charge obtained in a rather arbitrary way, assigning bonding electrons to the atom with the greater attraction for electrons. [Pg.87]

Oxidation numbers are just a bookkeeping method used to keep track of electron transfers. In a covalent molecule or a polyatomic ion, the oxidation number of each element does not represent an ionic charge, because the elements are not present as ions. However, to assign oxidation numbers to the elements in a covalent molecule or polyatomic ion, you can pretendthe bonds are ionic. [Pg.473]

You have seen examples of how Lewis structures can be used to assign oxidation numbers for polar molecules such as water, non-polar molecules such as chlorine, and polar polyatomic ions such as the cyanide ion. [Pg.475]

Drawing Lewis structures to assign oxidation numbers can be a very time-consuming process for large molecules or large polyatomic ions. Instead, the results from Lewis structures have been summarized to produce a more convenient set of rules, which can be applied more quickly. Table 10.1 summarizes the rules used to assign oxidation numbers. You may have discovered some of these rules for yourself in the ThoughtLab you just completed. [Pg.476]

The total of the oxidation numbers of all the atoms (not simply all the elements) is equal to the charge on the atom, molecule, or ion. Thus, for any compound, the sum of the oxidation numbers totals zero because the net charge on any compound is zero. The sum of the oxidation numbers of the atoms of any polyatomic ion is equal to the charge on that ion. [Pg.445]

The oxidation number of an uncombined atom is zero. This is true for elements that exist as polyatomic molecules such as O2, CI2, H2, N2, Sg. [Pg.641]

Since the time of Berzelius, there has been a persistent argument used by inorganic chemists that, in many cases, valency as a positive integer should be replaced by negative and positive oxidation numbers adding up to zero in a molecule or solid, and to the ionic charge of a polyatomic cation or anion [9]. The same year, 1916, as the Lewis paradigm was formulated [13,14], emphasiz-... [Pg.10]

Oxygen usually has an oxidation number of-2. Exceptions include molecules and polyatomic ions that contain 0-0 bonds O2, O3, H2O2, and the O2 ion. [Pg.287]

Oxidation numbers, sometimes called oxidation states, are signed numbers given to atoms in molecules and ions to define their positive or negative character. The oxidation number refers to the number of formal charges that an atom would have in a molecule or polyatomic ion in the case of electrons being completely transferred in the direction indicated by the electronegativity difference between atoms. [Pg.60]

These definitions lead to the following rules for assigning oxidation numbers in polyatomic molecules. [Pg.106]

While oxidation number is very useful for keeping track of what the electtons are doing in a redox reaction, we should emphasize that it has been invented to meet a need. It has no experimental basis. Unlike the charge of a monatomic ion, the oxidation number of an atom in a molecule or polyatomic ion cannot be measured in the laboratory. It is all very well to talk about +4 manganese in Mn02 or +6 sulfur in the 864 ion, but take care not to fall into the trap of thinking that the elements in these species actually carry positive charges equal to their oxidation numbers. [Pg.576]

What are the oxidation numbers of each of the following species (a) elemental substance, (b) oxygen (some exceptions), (c) molecule, (d) monatomic ion, (e) hydrogen (one exception), (f) polyatomic ion ... [Pg.576]

The oxidation numbers in any chemical species must sum to the overall charge on the species. That is, oxidation numbers must sum to zero for any molecule and must sum to the charge on any polyatomic ion. The oxidation number of a monatomic ion is equal to the charge on the ion. [Pg.128]

All others—oxidation numbers are determined from the fact that the sum of all oxidation numbers within the molecule or polyatomic ion must add up to either zero (in the case of a neutral molecule) or the charge on the ion (in the case of a polyatomic ion)... [Pg.331]

Other spectral interferences include argide complexes (XAr), oxides (XO), hydrides (XH), doubly charged species (X +, interfering at half the isotopic mass of X) and complex polyatomic molecules such as the nitric acid complex H2 " N 03 on A number of methods... [Pg.62]

Although most of the molecules and polyatomic ions referred to in general chemistry follow the octet rule, there are some familiar species that do not. Among these are molecules containing an odd number of valence electrons. Nitric oxide, NO, and nitrogen dioxide, N02, fall in this category ... [Pg.172]


See other pages where Polyatomic molecules, oxidation numbers is mentioned: [Pg.104]    [Pg.18]    [Pg.128]    [Pg.53]    [Pg.473]    [Pg.210]    [Pg.123]    [Pg.18]    [Pg.20]    [Pg.132]    [Pg.140]    [Pg.141]    [Pg.138]    [Pg.667]    [Pg.108]    [Pg.331]    [Pg.525]    [Pg.1049]    [Pg.15]    [Pg.13]    [Pg.45]    [Pg.41]    [Pg.207]    [Pg.221]    [Pg.358]    [Pg.250]   


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