Atomic Structures

The relative ability of an atom to attract electrons in when bonded in a molecule

Energy needed to remove electrons

Distance between nucleus and outermost electrons

Energy released when electrons are added

Isotopes that have unstable nuclei and undergo radioactive decay.Unstable nuclei: When repulsive-electric force of protons is not balanced with the attractive force of neutrons (too many neutrons).

% of a given isotope in nature out of other isotopes of the same element.

Avg. mass of all isotopes of a given element.= (%abundance x amu) + (%abundance x amu)

1.7+ ENHas no IMFSHeld together in crystal structure in an equal ratio indictated by subscripts in formulaProperties:Very strong bonds, requires lots of energy to break them apart into different statesHigh melting and boiling pointsGenerally soluble in water through dissociationCations bond to oxygen while anions bond to hydrogen

Atoms bond through shared electrons. Covalent/molecular refers to the bond within a molecule.

0.5-1.7 ENMolecules held together through dipole-dipole or H-bond IMFSThese seperate when dissolved, boiled, or meltedProperties:Generally high melting/boiling pointsStronger bonds than nonpolar moleculesSoluble in polar solvents, insoluble in nonpolar

0-0.5 ENMolecules held together through LD IMFSThese seperate when boiled, dissolved, or meltedProperties:Lowest melting/boiling pointsDissolves in nonpolar solvents, insoluble in polar solventsWeakest bonds

Forces which hold molecules together in a structureIs broken when changing states or dissolving

MNO3 --> MNO2 + O2

MClO --> MCl + O2

MCO3 --> MO + CO2

Nonmetal Oxide + H2O

MOH + H2O

Element + Element

MHCO3 --> MCO3 + CO2 + H2O

Complete: HC + O2 --> H2O + CO2When sufficient oxygen is presentIncomplete: HC + O2 --> C + CO + CO2 + H2OWhen insufficient oxygen is presentOther types: element + O2 --> Element oxideSynthesis reactions with oxygen can be classified as combustion if light and heat is produced (exothermic)

Acid + MCO3 --> Ionic Compound + H2O + CO2

Ionic Compound + NH3 + H2O

pH <7Higher concentration of hydronium ions in solution10x the concentration of H+ per level of pHIonizes in water to form H+ and non-metal ions*Strength of acid refers to its ionization ability rather than concentration.Strong Acids: HA + H2O --> H3O + A-Ex. HCl + H2O --> H3O + Cl-All molecules ionizeHigh conductivity (because of ions)Weak Acid: HA + H2O --> H3O + A-Ex. HF + H2O --> H3O + F- (only some)Only some molecules ionizeSlight conductivity (less ions)

pH >7Higher concentration of hydroxide ions in solution10x the concentration of OH- per level of pHDissociates in water to form OH- and M+ ions*Strength of base refers to its dissociation ability rather than concentration.Strong Base: MOH --> M + OHEx. LiOH --> Li + OHAll alkali bases are strongDissociates completelyHigh conductivity (because of ions)Weak Base: B + H2O --> BH + OHEx. NH3 + H2O --> NH4 + OHDoesn't dissociate completelySlight conductivity (not as much ions)