To determine the formula of ionic compounds by crossing the numerical charge of each ion.
Positive charge equal to the group number (loss of 1 electron).
–ite or –ate.
Group 5A, 6A, and 7A.
Molecules.
A metal and a nonmetal.
NaCl.
They normally do not form ions.
Zero net charge.
Al 3+.
By subtracting the group number from 8.
Silver (Ag +), Cadmium (Cd 2+), Zinc (Zn 2+).
4 molecules of glucose.
They exist as gases or liquids.
By using their specific names, often ending in -ate or -ite.
To indicate how many atoms of each element are present in the molecule.
CaBr2.
Cu 2+ (Cupric ion).
Gain of 2 electrons (e.g., O 2-).
Mg2+ and Cl-.
Cl + e- → Cl- (Chloride ion).
Relatively low.
Write the name of the cation first followed by the name of the anion ending in 'ide'.
Negative.
12 atoms of Hydrogen.
ANION.
High melting and boiling points.
When the first element is a single atom.
The kind and number of atoms in a molecule.
Ca(NO3)2 or (NH4)2S.
6 atoms of Carbon.
Na → Na+ + e- (Sodium ion).
Nonpolar liquids (like oil), but not in water.
It ends in '-ide'.
A net charge of zero.
You write the cation first followed by the anion.
Three elements: Carbon (C), Hydrogen (H), and Oxygen (O).
CATION.
Two or more nonmetallic elements.
They are crystalline solids.
The cation is named first, followed by the anion.
It loses or gains one or more electrons.
Iron (II) Sulfate.
The 'o' is left out, as in 'monoxide' instead of 'monooxide'.
<p>Ammonium (NH4+), cyanide (CN-), and hydroxide (OH-).</p>
-ate or -ite, except for hydroxide and cyanide.
C₆H₁₂O₆.
Mg → Mg2+ + 2e- (Magnesium ion).
CO2 or H2O.
The system of naming chemical compounds.
They are equal in number.
Group 1A, 2A & 3A.
By balancing the positive charge with the negative charge.
SO3^2- or NO2-.
When more than one polyatomic ion is being used.
So that the net charge is zero.
The ion becomes positive.
Strong ionic bonds.
-ate indicates more oxygen atoms, while -ite indicates fewer.
Use a Roman numeral in the name (e.g., Iron (II), Copper (II)).
Fe 2+ (Ferrous ion).
Gain of 1 electron (e.g., H- and F-).
The ion becomes negative.
O + 2e- → O2- (Oxide ion).
A metallic and a nonmetallic element.
It indicates 1 less oxygen than the –ate form.
Two Br- ions are required for one Ca2+ ion.
Both positive ions (cations) and negative ions (anions).
Fe 3+ (Ferric ion).
6 atoms of Oxygen.
Weak molecular bonds.
NaCl.
Using prefixes to indicate the number of atoms and the more electronegative element is named last.
Li +.
Group 4A and 5A.
Cu 1+ (Cuprous ion).
The number of molecules for the compound.
Na+ and Cl-.
In molecular compounds.
They are poor electrical conductors in all states.
SO4^2- or NO3-.
Gain of 3 electrons (e.g., N 3-).
MgCl2.
No, they never form ions in isolation.
They are good electrical conductors.
Ionic compounds and covalent compounds.
When metallic elements combine with nonmetallic elements.
Soluble in water but not in nonpolar liquids (like oil).
<p>groups of atoms that behave as a unit and carry a charge.</p>
<p>cation</p>
<p>anion</p>
