Unit 4 Flashcards
Main group metal cations are named by identifying the metal, followed by the word ion.
• Recognizing polyatomic ions in a chemical formula helps to name them correctly.
Naming cations
Metals become (+) ions = cations; keep name of element + the word “ion”
• Ex. Na+ , sodium ion
Naming anions
Non-metals become (-) ions = anions; keep 1st syllable of element name, drop ending and add suffix –ide
• Ex. Cl-, chloride ion
Some metal and nonmetal ion names
[metals with variable charge]
Transition metals form two or more positive ions (cations). – except for
Zn2+, Cd2+, and Ag+
[metals with variable charge]
Roman numeral
-A Roman numeral equal to the ion charge is placed in parentheses immediately after the metal name.
-Cu2+ copper(II)
-Cu+ copper(I)
-Fe2+ iron(II)
-Fe3+ iron(III)
-Pb2+ lead(II)
-Pb4+ lead(IV)
-Cr2+ chromium(II)
-Cr3+ chromium(III)
[metals with variable charge]
Names of some transition metal cations
[Polyatomic ions]
a group of atoms with an overall net charge (+ or −).
• Atoms covalently bound—share electrons
• often consist of nonmetals such as P,S,C,N,O and H.
• usually have a negative charge (1−, 2−, or 3−)
• Sum of all e- > sum of all of protons in the combined
atoms. (# e- > # protons)
• except for NH4+, ammonium, which has a (1+) charge
• (#protons > # e-)
Names of Polyatomic ions
Names of most common polyatomic ions end in ate.
SO42− (sulfate)
PO43− (phosphate)
NO3− (nitrate)
a. When a related ion has one less oxygen, its name ends in ite.
SO32− (sulfite)
PO33− (phosphite)
NO2− (nitrite)
b. Exceptions to these rules are the following:
CN− (cyanide)
OH− (hydroxide)
Some common Polyatomic ions
Naming Ionic compounds
Ionic compounds are named by citing first the cation and then the anion, with a space between words.
Flow chart, naming IONIC compounds
[naming ionic compounds]
Type I ionic compounds
Cations of main group elements.
• charges do not vary.
• Do not specify the charge on the cation.
NaCl is sodium chloride.
MgCO3 is magnesium carbonate.
[naming ionic compounds]
Type II ionic compounds
Cations of transition metals
• exhibit more than one charge.
• Specify the charge on the cation in these compounds
**
FeCl2 is iron(II) chloride or ferrous chloride.
FeCl3 is iron(III) chloride or ferric chloride.
Naming covalent compounds
-2 non-metals
-first nonmetal
Use a prefix to match a subscript before the element name
-second nonmetal
Use a prefix to match a subscript before the element name and end with ide
Prefixes used to name molecular compounds
1 mono
2 di
3 tri
4 Tetra
5 penta
6 hexa
7 hepta
8 Octa
9 nona
10 deca
Naming molecular covalent compounds based on formula
• 1st nonmetal – its element name.
(Least electronegative element)
• 2nd nonmetal –first syllable of
the name followed by ide.
• Add prefix to represent subscripts to the names of atoms
• indicates two or more atoms of an element
• doesn’t matter if it is the 1st or 2nd atom in formula
When sodium or other metal reacts with chlorine or any other halogen or nonmetal
the metal transfers an electron from its valence shell to the valence shell of the halogen or nonmetal.
Transition metals
Form cations
-the metal transfers an electron from its valence shell to the valence shell of the halogen or nonmetal.
Ionization energy
• energy absorbed to remove one electron from a single
atom in the gaseous state.
– low values lose electron easily to form cations.
Electron affinity
• energy released on adding an electron to a single atom
in the gaseous state.
– large values—>gain electrons easily to form anions
Ion formation
• Halogens gain electrons most easily.
• Alkali metals lose electrons most easily.
• Elements near the middle of the periodic table do not form ions easily.
• Noble gases do not form ions.
Rules for writing formulas for ionic compounds:
- Determine the numbers and kinds of ions in the compound
- List the cation first and the anion second.
- Do not write the charges of the ions.
- Use parentheses around a polyatomic ion formula if it has a subscript.
Writing formulas with Polyatomic ions