Chapter 4
暂无描述。系统推荐的高质量记忆内容，适合每天坚持背诵学习。
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solutions
homogeneous mixtures of 2+ substances
solvents
present in greatest abundance
solutes
present in lesser abundance
aqueous solution
w/ water
solvation
surrounding of solute by solvent (water); molecular and ionic
dissociation
ionic compounds dissolve by separation into ions
electrolyte
dissociates into ions in aqueous solution; ionic, conducts electricity
nonelectrolyte
doesn’t dissociate (doesn’t form ions); molecular, doesn’t conduct electricity
strong electrolyte
dissociates completely when dissolved - water-soluble ionic compounds
all ionic compounds =
strong electrolytes
weak electrolytes
only dissociate partially when dissolved - chemical equilibrium; reaction goes forwards and backwards
precipitation reactions
2 solutions w/ soluble salts –> insoluble salt (precipitate)
precipitate
insoluble solid formed by 2 soluble salts
solubility
amount of substance can be dissolved in solvent
metathesis reactions (exchange)
partner switching
steps to metathesis reactions
• determine ions present • write formulas for product, cation from 1 reaction w/ anion from other reaction • check solubility; if insoluble, precipitate forms
molecular equation
lists reactants and products w/o ionic values
complete ionic equation
all strong electrolytes dissociated into ions - breaks down aqueous species
net ionic equations
doesn’t include spectator ions (cancel out what’s on both sides)
acids
substances that ionize in aqueous solutions to form H+ ions (protons) - proton donors
monocratic acids
donate 1 H+ per molecule
diprotic acid
donates 2 H+ per molecule
bases
increase amount of OH- ions or accepts H+ ions
strong acids
Hydrochloric acid, HCl hydrobromic acid, HBr Hydroiodic acid, HI Chloric acid, HClO3 perchloric acid, HClO4 nitric acid, HNO3 sulfuric acid, H2SO4