- Chapter 1: Chemistry: The Study of Change
- Chapter 10: Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
- Chapter 11: Intermolecular Forces and Liquids and Solids
- Chapter 12: Physical Properties of Solutions
- Chapter 13: Chemical Kinetics
- Chapter 14: Chemical Equilibrium
- Chapter 15: Acids and Bases
- Chapter 16: Acid-Base Equilibria and Solubility Equilibria
- Chapter 17: Entropy, Free Energy, and Equilibrium
- Chapter 18: Electrochemistry
- Chapter 19: Nuclear Chemistry
- Chapter 2: Atoms, Molecules, and Ions
- Chapter 20: Chemistry in the Atmosphere
- Chapter 21: Metallurgy and the Chemistry of Metals
- Chapter 22: Nonmetallic Elements and Their Compounds
- Chapter 23: Transition Metals Chemistry and Coordination Compounds
- Chapter 24: Organic Chemistry
- Chapter 25: Synthetic and Natural Organic Polymers
- Chapter 3: Mass Relationships in Chemical Reactions
- Chapter 4: Reactions in Aqueous Solutions
- Chapter 5: Gases
- Chapter 6: Thermochemistry
- Chapter 7: Quantum Theory and the Electronic Structure of Atoms
- Chapter 8: Periodic Relationships Among the Elements
- Chapter 9: Chemical Bonding I: Basic Concepts
Chemistry 11th Edition - Solutions by Chapter
Full solutions for Chemistry | 11th Edition
ISBN: 9780073402680
Solutions by Chapter
Since problems from 25 chapters in Chemistry have been answered, more than 1091474 students have viewed full step-by-step answer. This expansive textbook survival guide covers the following chapters: 25. Chemistry was written by and is associated to the ISBN: 9780073402680. The full step-by-step solution to problem in Chemistry were answered by , our top Chemistry solution expert on 11/08/17, 03:59AM. This textbook survival guide was created for the textbook: Chemistry, edition: 11.
Key Chemistry Terms and definitions covered in this textbook
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Alkyl group
A group derived by removing a hydrogen from an alkane; given the symbol R!
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atomic weight
The average mass of the atoms of an element in atomic mass units (amu); it is numerically equal to the mass in grams of one mole of the element. (Section 2.4)
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Bimolecular reaction
A reaction in which two species are involved in the rate-determining step.
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bond enthalpy.
The enthalpy change required to break a bond in a mole of gaseous molecules. (9.10)
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core electrons.
All nonvalence electrons in an atom. (8.2)
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diatomic molecule
A molecule composed of only two atoms. (Section 2.6)
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diene
A compound containing two carbon-carbon p bonds.
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Endergonic reaction
A reaction in which the Gibbs free energy of the products is higher than that of the reactants. The position of equilibrium for an endergonic reaction favors starting materials
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glucose
A polyhydroxy aldehyde whose formula is CH2OH1CHOH24CHO; it is the most important of the monosaccharides. (Section 24.8)
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Hyperconjugation
Interaction of electrons in a s-bonding orbital with the vacant 2p orbital of an adjacent positively charged carbon.
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intermediate
A structure corresponding to a local minimum (valley) in an energy diagram.
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Ka
A measure of the strength of an acid: Ka = Keq 3H2O4 = 3H3O+ 4 3A- 4 3HA4
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Ketone
A compound containing a carbonyl group bonded to two carbons.
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LUMO
The lowest unoccupied molecular orbital.
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Messenger RNA (mRNA)
A ribonucleic acid that carries coded genetic information from DNA to the ribosomes for the synthesis of proteins
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nonelectrolyte
A substance that does not ionize in water and consequently gives a nonconducting solution. (Section 4.1)
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partial pressure
The pressure exerted by a particular gas in a mixture. (Section 10.6)
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polar covalent bond
A covalent bond in which the electrons are not shared equally. (Section 8.4)
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reactant
A starting substance in a chemical reaction; it appears to the left of the arrow in a chemical equation. (Section 3.1)
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root-mean-square (rms) speed 1M2
The square root of the average of the squared speeds of the gas molecules in a gas sample. (Section 10.7)