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[GET] Chapter 11 Chemical Reactions Chapter Test B Answer Key
Because the metals have lost electrons to oxygen, they have been oxidized; oxidation is therefore the loss of electrons. Conversely, because the oxygen atoms have gained electrons, they have been reduced, so reduction is the gain of electrons. For...[FREE] Chapter 11 Chemical Reactions Chapter Test B Answer Key | HOT
Atoms in their elemental form, such as O2 or H2, are assigned an oxidation state of zero. In this, and in most cases not involving complex polyatomic ions the oxidation state is equivalent to the usual valence. In redox reactions, there is a net...
- While this is not true, it is almost true, and the oxidation state model can help you understand and predict many reactions. That is the oxidation state model assumes that the hydrogen atoms transfer an electron completely to the oxygen atom. We know this is not the case, but that the electrons from the hydrogen atoms are found closer to the oxygen atom. Again, the idea is that the oxidation state model assumes complete transfer, and the atomic bond model tell us that the transfer is only partial.
- Still, the oxidation state model is useful as we shall see Figure A set of rules for assigning oxidation states to atoms in chemical compounds follows. The principles underlying these rules have been laid out in the atomic and molecular structure in Chapter 2 , Chapter 3 Chapter 4 and Chapter 5. Rules for Assigning Oxidation States: The oxidation state of an atom in any pure element, whether monatomic, diatomic, or polyatomic, is zero. The sum of the oxidation states of all the atoms in a neutral molecule or ion must equal the charge on the molecule or ion. In any chemical reaction, the net charge must be conserved; that is, in a chemical reaction, the total number of electrons is constant, just like the total number of atoms.
- Consistent with this, rule 1 states that the sum of the individual oxidation states of the atoms in a molecule or ion must equal the net charge on that molecule or ion. The net charge is zero, as it must be for any compound. Rule 3 is required because fluorine attracts electrons more strongly than any other element, for reasons you discovered in Chapter 3.
- Hence fluorine provides a reference for calculating the oxidation states of other atoms in chemical compounds. Rule 4 reflects the difference in chemistry observed for compounds of hydrogen with nonmetals such as chlorine as opposed to compounds of hydrogen with metals such as sodium. Rule 5 is necessary because fluorine has a greater attraction for electrons than oxygen does; this rule also prevents violations of rule 2. Non-integral oxidation states are encountered occasionally. They are usually due to the presence of two or more atoms of the same element with different oxidation states, so that the "average" oxidation state is a fraction. As with resonance structures, this is a failure of the model. The reduction of copper I oxide shown in Equation Rule 1 states that atoms in their elemental form have an oxidation state of zero, which applies to H2 and Cu.
- Rule 6 states that the sum of the oxidation states in a molecule or formula unit must equal the net charge on that compound. So this is a redox reaction. Oxidation states are a convenient way of assigning electrons to atoms, and they are useful for predicting the types of reactions that substances undergo. Example
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Chapter 11 - Chemical Reactions - Standardized Test Prep - Page 381: 3
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Chemical Reactions Chapter 11 Test B Answer Key Read Online And Download [PDF]
Ch 11, 12, 4, 13, Chemical bonding; Structure and shape; Introduction to gases; The ideal gas law and its applications; Gas, liquids and solids; Solutions; Net ionic equations; Acid-base proton-transfer reactions; Oxidation-reduction redox reactions. Answer key for Test 3 top of page Chapter handouts; miscellaneous Intro Chem For each chapter I provide a short handout that offers my comments on the chapter. The handout may contain information about homework assignments, priority material within the chapter, known errors, and other comments. See the "Chapter handouts" section of the course syllabus for more information about these handouts.- The following links are to all the major Intro Chem X11 handouts for the entire semester; they are in chronological order. Most of these links are to "chapter handouts", and are here as PDF files. Sample tests are available in the top section of this page. Other course materials, such as practice quizzes and supplementary discussions of various topics, are available from the Intro Chem home page.
- These handouts are specifically keyed to the 2nd edition of the Cracolice book. Much of the content is general, and would be useful with other editions and even other books. For more about the editions of the Cracolice book, see the textbook information on the Introductory Chemistry X11 Supplemental information page. Ch Introduction to chemistry: Introduction to active learning; Matter and energy.
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