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Determining Oxidation Numbers

The reaction is exothermic reaction rates decrease with increased carbon number of the oxide (ethylene oxide > propylene oxide > butylene oxide). The ammonia—oxide ratio determines the product spht among the mono-, di-, and trialkanolamines. A high ammonia to oxide ratio favors monoproduction a low ammonia to oxide ratio favors trialkanolamine production. Mono- and dialkanolamines can also be recycled to the reactor to increase di-or trialkanolamine production. Mono- and dialkanolamines can also be converted to trialkanolamines by reaction of the mono- and di- with oxide in batch reactors. In all cases, the reaction is mn with excess ammonia to prevent unreacted oxide from leaving the reactor. [Pg.7]

Determine the oxidation numbers of carbon in the compounds carbon monoxide, CO, carbon dioxide, C02, and in diamond. [Pg.222]

Determine the oxidation number of uranium in each of the known compounds UOj, U3Oe, U2Os, U02, UO, K2U04, Mg-UjO,. [Pg.223]

The following rules apply to the determination of oxidation numbers. [Pg.851]

The O.N. of a compound is always zero, and is determined by the sum of the oxidation numbers of the individual atoms each multiplied by the number of atoms of the element in the molecule. [Pg.852]

The equivalent of an oxidising agent is determined by the change in oxidation number which the reduced element experiences. It is the quantity of oxidant which involves a change of one unit in the oxidation number. Thus in the normal reduction of potassium permanganate in the presence of dilute sulphuric acid to an Mn(II) salt ... [Pg.852]

Oxidation number 851, (T) 853 rules for determining. 851 Oxidation number method 851 Oxidation-reduction cells 64 Oxidation-reduction curve 361 Oxidation-reduction indicators (T) 367 Oxidation-reduction reactions 67, 258, 360,... [Pg.869]

Step 1 Identify the cation and the anion (see Table D.l or Appendix 3A, if necessary). To determine the oxidation number of the cation, decide what cation charge is required to cancel the total negative charge of the anions. Step 2 Name the cation. If the metal can have more than one oxidation number (most transition metals and some metals in Groups 12 through 15/V), give its charge as a Roman numeral. [Pg.56]

STRATEGY First, determine the oxidation numbers of the elements taking part in the reaction. The oxidizing agent is the species that contains an element that is reduced. Similarly, the reducing agent is the species that contains an element that is oxidized. [Pg.106]

Determine the oxidation In Fe24 (reactant) the oxidation number is +2. [Pg.106]

Determine the oxidation number of an element (Toolbox K. I and Example K.l). [Pg.107]

K.4 Determine the oxidation number of the italicized element in each of the following compounds (a). SOCI2 (b) Se03 ... [Pg.108]

K.22 (a) Determine and tabulate the maximum (most positive) and minimum (most negative) oxidation numbers of the elements in the first seven main groups. Hint ... [Pg.109]

Although formal charge and oxidation number both give us information about the number of electrons around an atom in a compound, they are determined by different methods and often have different values. The formal charge exaggerates the... [Pg.196]

Name each of the following complex ions and determine the oxidation number of the metal (a) [Fe(ox)(Cl)4l3 ... [Pg.813]

To determine whether electrons are transferred in chemical reactions, chemists use a procedure that assigns an oxidation number (also known as an oxidation state) to each atom in each chemical species. In a redox reaction, electron transfer causes some of the atoms to change their oxidation numbers. Thus, we can identify redox reactions by noting changes in oxidation numbers. [Pg.1353]

To determine oxidation numbers, we assign each valence electron to a specific atom in a compound. This means that the oxidation number of an atom is the charge it would have if the compound were composed of ions. Ionic FeO, for example, would contain Fe cations and 0 anions. Thus, in FeO we assign iron an oxidation number of +2 and oxygen an oxidation number of-2. [Pg.1353]

It is always possible to determine oxidation numbers starting from electronegativity differences. A more systematic method for determining oxidation numbers uses the following four guidelines ... [Pg.1354]


See other pages where Determining Oxidation Numbers is mentioned: [Pg.1417]    [Pg.1417]    [Pg.492]    [Pg.406]    [Pg.342]    [Pg.80]    [Pg.87]    [Pg.94]    [Pg.260]    [Pg.177]    [Pg.30]    [Pg.108]    [Pg.213]    [Pg.214]    [Pg.215]    [Pg.257]    [Pg.429]    [Pg.772]    [Pg.773]    [Pg.773]    [Pg.817]    [Pg.937]    [Pg.120]    [Pg.1355]    [Pg.1358]    [Pg.1416]   


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