1. Nearly all compounds with nitrate (NO3^-) and acetate (C2H3O2^-) are soluble 2. All compounds with chloride (Cl^-), fluoride (F^-), bromide (Br^-), and iodide (I^-) are soluble, except those containing silver (Ag), mercury (Hg), and lead (Pb) 3. All compounds with sulfate (SO4^2-) are soluble, except those containing barium (Ba), strontium (Sr), lead (Pb), calcium (Ca), and sliver (Ag) 4. Most alkali metal salts (family 1) and ammonium salts (NH4^+) are soluble 5. All the common acids (HX) are soluble 6. 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) 7. All sulfides (S^2-) are insoluble, except those of the alkali metals (family 1), alkaline earth metals (family 2), and ammonium sulfide [(NH4)2S] 8. 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)

Chapter 7: Ionic Compounds and Metals Flashcards by Xavier P

Ionic Bonding

Electrostatic attraction between ions

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Covalent Bonding

Sharing of electrons

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Metallic Bonding

Metal atoms bonded to several other atoms

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Cations

Positively charged ions - formed by electron loss - made from metals - < parent atom

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Anions

Negatively charged ions - formed by electron gain - made from nonmetals - > parent atom

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Ions

Atoms in which number protons does not equal number electrons

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Psuedo-Noble Gas Configuration

Configuration of an ion that has gained or lost electrons to get a full valence shell

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Isoelectronic Species

Atoms & ions with same number electrons (always based off a noble gas)

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Elements In Compounds Determine Bonding

Covalent - 2 Nonmetals
Ionic - Metal + Nonmetal
Metallic - All Metals

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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

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Ternary Compounds

Have 3 or more elements in them - polyatomic ion in structure

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Polyatomic Ion

Cluster of atoms held together with covalent bonds that has a net charge

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“Oxyanions”

Polyatomic ions that contain oxygen

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Stock System

Use of Roman Numerals to show charge on transition metal ions

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Properties Of Metals That Allows Metallic Bonding

Delocalized valence electrons; Electrons shared frequently among large groups of atoms

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“Sea Of Electrons” Model

Model showing group of cations in a “sea of electrons”; explains electrical and thermal conductivity, ductility, and malleability

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Alloys

Combination of two or more elements, majority are metals

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Substitutional Alloys

Second element takes place of a metal atom

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Interstitial Alloys

Second element fills space in lattice of metal atoms

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Binary Compounds

Made of cation and anion; combine in ratios that are electrically neutral

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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

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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)

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Lead (IV) Charge

Pb^4+

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Tin (IV) Charge

Sn^4+

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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

1. Use elemental symbol for atomic kernel 2. Distribute valence electrons around the kernel: put one electron on each of four sides before doubling any electrons up 3. Use family number to determine the number of valence electrons

Dot Diagrams For Monatomic Ions

1. Draw structure as an atom, adding electrons for anions, removing electrons for cations 2. Put in square brackets and place the charge outside the brackets in the upper right hand corner

Dot Diagrams For Molecules

1. Tally valence electrons 2. Connect all atoms in a symmetrical pattern, using "sticks" for bonds 3. Distribute remaining electrons to satisfy the octet and duet rules 4. If you run out of electrons, make double or triple bonds

Dot Diagrams For Polyatomic Ions

1. Tally valence electrons, adding or removing electrons for charge 2. Construct the ion as you would a molecule 3. Put the ion in square brackets, placing the charge outside the brackets in the upper right hand corner

Dot Diagrams For Ionic Compounds

1. Write a separate ionic structure for each ion in the formula Ex: SrCl2 would need three structures

Dot Diagrams For Resonance

1. Occurs when a mixture of single and double bonds are found between equivalent atoms in the same structure 2. Draw a separate structure for each possible double bond position 3. Put double headed arrows between the structures