Chapter 7: Ionic Compounds and Metals Flashcards
Ionic Bonding
Electrostatic attraction between ions
Covalent Bonding
Sharing of electrons
Metallic Bonding
Metal atoms bonded to several other atoms
Cations
Positively charged ions - formed by electron loss - made from metals - < parent atom
Anions
Negatively charged ions - formed by electron gain - made from nonmetals - > parent atom
Ions
Atoms in which number protons does not equal number electrons
Psuedo-Noble Gas Configuration
Configuration of an ion that has gained or lost electrons to get a full valence shell
Isoelectronic Species
Atoms & ions with same number electrons (always based off a noble gas)
Elements In Compounds Determine Bonding
Covalent - 2 Nonmetals
Ionic - Metal + Nonmetal
Metallic - All Metals
Properties Of Ionic Compounds
- Brittle
- High melting and boiling points
- Solids form a crystalline lattice - orderly arrangement of ions in the solid state
- Non-conductive as solids, conductive when dissolved or melted
- Ionic compounds are electrolytes
Ternary Compounds
Have 3 or more elements in them - polyatomic ion in structure
Polyatomic Ion
Cluster of atoms held together with covalent bonds that has a net charge
“Oxyanions”
Polyatomic ions that contain oxygen
Stock System
Use of Roman Numerals to show charge on transition metal ions
Properties Of Metals That Allows Metallic Bonding
Delocalized valence electrons; Electrons shared frequently among large groups of atoms
“Sea Of Electrons” Model
Model showing group of cations in a “sea of electrons”; explains electrical and thermal conductivity, ductility, and malleability
Alloys
Combination of two or more elements, majority are metals
Substitutional Alloys
Second element takes place of a metal atom
Interstitial Alloys
Second element fills space in lattice of metal atoms
Binary Compounds
Made of cation and anion; combine in ratios that are electrically neutral
Lattice Energy
Energy needed to break ionic bonds; increased lattice energy = increased bond strength = increased effect of properties; increased ionic charge or decreased ionic radius = increased lattice energy; ionic radius more important than charge; increased lattice energy = higher boiling and melting points
Solubility Rules
- Nearly all compounds with nitrate (NO3^-) and acetate (C2H3O2^-) are soluble
- All compounds with chloride (Cl^-), fluoride (F^-), bromide (Br^-), and iodide (I^-) are soluble, except those containing silver (Ag), mercury (Hg), and lead (Pb)
- All compounds with sulfate (SO4^2-) are soluble, except those containing barium (Ba), strontium (Sr), lead (Pb), calcium (Ca), and sliver (Ag)
- Most alkali metal salts (family 1) and ammonium salts (NH4^+) are soluble
- All the common acids (HX) are soluble
- All oxides (O^2-) and hydroxides (OH^-) are insoluble, except those of the alkali metals (family 1) and those containing calcium (Ca), strontium (Sr), barium (Ba), or radium (Ra)
- All sulfides (S^2-) are insoluble, except those of the alkali metals (family 1), alkaline earth metals (family 2), and ammonium sulfide [(NH4)2S]
- All phosphates (PO4^3-), carbonates (CO3^2-), and oxalates (C2O4^2-) are insoluble, except those of the alkali metals (family 1) and ammonium salts (NH4)
Lead (IV) Charge
Pb^4+
Tin (IV) Charge
Sn^4+
Manganese (III) Charge
Mn^3+
Iron (III) Charge
Fe^3+
Gallium Charge
Ga^3+
Cobalt (III) Charge
Co^3+
Chromium (III) Charge
Cr^3+
Aluminium Charge
Al^3+
Zinc Charge
Zn^2+
Tin (II) Charge
Sn^2+
Strontium Charge
Sr^2+
Nickel Charge
Ni^2+
Mercury (II) Charge
Hg^2+
Mercury (I) Charge
(Hg2)^2+
Manganese (II) Charge
Mn^2+
Magnesium Charge
Mg^2+
Lead (II) Charge
Pb^2+
Iron (II) Charge
Fe^2+
Copper (II) Charge
Cu^2+
Chromium (II) Charge
Cr^2+
Calcium Charge
Ca^2+
Cobalt (II) Charge
Co^2+
Beryllium Charge
Be^2+
Barium Charge
Ba^2+
Sodium Charge
Na^+
Silver Charge
Ag^+
Rubidium Charge
Rb^+
Potassium Charge
K^+
Lithium Charge
Li^+
Hydrogen Charge
H^+
Copper (I) Charge
Cu^+
Cesium Charge
Cs^+1
Ammonium Charge
NH4^+
Acetate Charge
C2H3O2^-
Bromate Charge
BrO3^-
Bromide Charge
Br^-
Chlorate Charge
ClO3^-
Chloride Charge
Cl^-
Chlorite Charge
ClO2^-
Cyanide Charge
CN^-
Dihydrogen Phosphate Charge
H2PO4^-
Fluoride Charge
F^-
Hydride Charge
H^-
Hydrogen Sulfate Charge
HSO4^-
Hydrogen Carbonate Charge
HCO3^-
Hydrogen Sulfite Charge
HSO3^-
Hydroxide Charge
OH^-
Hypochlorite Charge
ClO^-
Iodate Charge
IO3^-
Iodide Charge
I^-
Nitrate Charge
NO3^-
Nitrite Charge
NO2^-
Perchlorate Charge
ClO4^-
Permanganate Charge
MnO4^-
Carbonate Charge
CO3^2-
Chromate Charge
CrO4^2-
Dichromate Charge
Cr2O7^2-
Monohydrogen Phosphate Charge
HPO4^2-
Oxalate Charge
C2O4^2-
Oxide Charge
O^2-
Peroxide Charge
O2^2-
Sulfate Charge
SO4^2-
Sulfide Charge
S^2-
Sulfite Charge
SO3^2-
Arsenate Charge
AsO4^3-
Nitride Charge
N^3-
Phosphate Charge
PO4^3-
Phosphide Charge
P^3-
Dot Diagrams For Atoms
- Use elemental symbol for atomic kernel
- Distribute valence electrons around the kernel: put one electron on each of four sides before doubling any electrons up
- Use family number to determine the number of valence electrons
Dot Diagrams For Monatomic Ions
- Draw structure as an atom, adding electrons for anions, removing electrons for cations
- Put in square brackets and place the charge outside the brackets in the upper right hand corner
Dot Diagrams For Molecules
- Tally valence electrons
- Connect all atoms in a symmetrical pattern, using “sticks” for bonds
- Distribute remaining electrons to satisfy the octet and duet rules
- If you run out of electrons, make double or triple bonds
Dot Diagrams For Polyatomic Ions
- Tally valence electrons, adding or removing electrons for charge
- Construct the ion as you would a molecule
- Put the ion in square brackets, placing the charge outside the brackets in the upper right hand corner
Dot Diagrams For Ionic Compounds
- Write a separate ionic structure for each ion in the formula
Ex: SrCl2 would need three structures
Dot Diagrams For Resonance
- Occurs when a mixture of single and double bonds are found between equivalent atoms in the same structure
- Draw a separate structure for each possible double bond position
- Put double headed arrows between the structures
