- 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
A group derived by removing a hydrogen from an alkane; given the symbol R!
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)
A reaction in which two species are involved in the rate-determining step.
The enthalpy change required to break a bond in a mole of gaseous molecules. (9.10)
All nonvalence electrons in an atom. (8.2)
A molecule composed of only two atoms. (Section 2.6)
A compound containing two carbon-carbon p bonds.
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
A polyhydroxy aldehyde whose formula is CH2OH1CHOH24CHO; it is the most important of the monosaccharides. (Section 24.8)
Interaction of electrons in a s-bonding orbital with the vacant 2p orbital of an adjacent positively charged carbon.
A structure corresponding to a local minimum (valley) in an energy diagram.
A measure of the strength of an acid: Ka = Keq 3H2O4 = 3H3O+ 4 3A- 4 3HA4
A compound containing a carbonyl group bonded to two carbons.
The lowest unoccupied molecular orbital.
Messenger RNA (mRNA)
A ribonucleic acid that carries coded genetic information from DNA to the ribosomes for the synthesis of proteins
A substance that does not ionize in water and consequently gives a nonconducting solution. (Section 4.1)
The pressure exerted by a particular gas in a mixture. (Section 10.6)
polar covalent bond
A covalent bond in which the electrons are not shared equally. (Section 8.4)
A starting substance in a chemical reaction; it appears to the left of the arrow in a chemical equation. (Section 3.1)
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)