Name ____________________________________ Period _____________________
Use the words below to complete the blanks in questions 1-6. You will not use all the words.
Unit 4 Review
ionic bond
subscript
Transfer
Oxyanions
Loses
Right
ionic compound
Polyatomic ion(s)
electrolyte
Ternary
Crisscross
left
oxidation
number
Lewis dot
structure
Cation
Binary
High
Roman numeral
Formula unit
Anion
Monatomic ion
Less
Nonmetal
Acid
superscript
Valence electrons
Melted
Hydro-
-ite
-ic
-ate
-ous
1. A positive ion, _cation__, is formed when a metal __loses____ electrons. Besides metals, there are two other
positive polyatomic ions on the ion list. List the ions and names. NH4+1 Ammonium H3O+1 Hydronium
2. A negative ion, _anion___, is formed when a _non-metal__ gains electrons. On the ion list there are many
Polyatomic Ions__ are negative. Give an example of a negative one, negative two and a negative three
Polyatomic Ion. See: Polyatomic Ion sheet!
3. The electrostatic force that holds oppositely charged particles together in an _Ionic Compound____ is called an
_Ionic Bond__ and involves transfer of electrons. The electrons transferred are called _valence electrons__. The
number of electrons can be determined by the A group numbers on the periodic table and can be used to draw a
_Lewis Dot Structure__. One element is an exception to the previous statement.
4. Lewis Dot Structures can be used to show the _transfer_ of electrons between a metal and a nonmetal..
5.
Ionic compounds have _high__ melting points and boiling points, and can conduct electricity when _melted_ or
dissolved in water. An _electrolyte__ is an ionic compound whose aqueous solution conducts an electric current.
6. If an ionic compound ends in _ite__ or _ate__, it means that a(n) polyatomic anion is present. –ite is one _less__
oxygen than the –ate.
Lewis Dot Structures
Draw the transfer between the following elements, Rubidium and chlorine, Magnesium and arsenic, and lithium
and
sulfur.
Name ____________________________________ Period _____________________
Define The Following Words
Ionic bond- the electrostatic force that holds oppositely charged particles together.
Monoatomic ion- a one atom ion ie: Ca+2
Cation- a positive ion; forms when an atom loses an eAnion- a negative ion; forms when an atom gains an ePolyatomic Ion- is made up of more than one atom and has an overall charge ex: SO4-2 Use parenthesis to group
Binary Ionic Compound- made up of 2 elements (ions) and the second element (ion) ends in -ide
Determine if each suffix/ prefix is for a non-metal ion, Polyatomic Ion or an Acid,
-ate= Polyatomic Ion
-ide=
non-metal (anion)
-ic=
Acid
-ite=
Polyatomic Ion
-ous
Acid
Hydro- = Binary Acid
Fill in the appropriate oxidation numbers for each family
Oxidation Numbers
Transition Metals
1. What groups are transition metals found in on the periodic table? Groups 3-12
2. Give the charge (oxidation #) of the following transition metals.
Lead II +2
Iron III +3
Au II +2
Name ____________________________________ Period _____________________
Ionic Compounds
1. List three characteristics of Ionic compounds.
High melting points, high boiling points, conduct electricity in aqueous solutions, form salts
2. _Valence__ electrons are involved in the formation of a chemical bond.
3. Cations _lose_ electrons and have a _positive__ charge.
4. Anions __gain__ electrons and have a _negative___ charge.
5. **Most Ionic compounds are made of a _metal_ and a _non-metal_
Element
Oxidation #
Ion Formula
Sodium
+1
Na +1
Bromide
-1
Br-1
Oxide
-2
O-2
Lithium
+1
Li+1
Phosphide
-3
P-3
Potassium
+1
K+1
Element
Oxidation #
Ion Formula
Iron (II)
+2
Fe+2
Mercury (I)
+1
Hg+1
Gold (III)
+3
Au+3
Silver
+1
Ag+1
Nickel (II)
+2
Ni+2
Copper (I)
+1
Cu+1
Zinc
+2
Zn+2
Name of Compound
Formula
Name of Compound
Formula
Potassium Phosphate
K+1 PO4-3 = K3PO4
Ammonium Phosphide
NH4+1 P-3 = (NH4)3P
Calcium Chloride
Ca+2 Cl-1 = CaCl2
Copper (II) Sulfate
Lithium Fluoride
LiF
Magnesium Iodide
MgI₂
CuSO4 = Cu+2SO4-2
Was Reduced
Pb(CrO4)2 = Pb+4(CrO4) -2
Was Reduced
Cs+1 C2H3O2 = CsC2H3O2
Copper (I) Oxide
Iron(III) acetate
Fe+3 C2H3O2-1
Cobalt (III) Carbonate
Cu+1
O-2
= Cu20
Lead (IV) Chromate
Cesium Acetate
Iron (III) Oxide
Sr+2 CrO4-2 = SrCrO4
Was Reduced
Fe2O3 = Fe+3O-2
Lithium Hydroxide
Li+1 OH-1 = LiOH
Strontium Chromate
Fe (C2H3O2)3
Co₂(CO₃)₃
Name ____________________________________ Period _____________________
Write the formula for each
TA – Ternary Acid
BA – Binary Acid
TC – Ternary Compound
BC – Binary Compound
1. Nitrous Acid TA;
Acid H+ Nitrous
Nitrite (NO2) = HNO2
2. Aluminum Hydroxide TC; Al+3 OH-1 = Al(OH)3 (Remember OH is a BASE)
3. Hydroselenic Acid BA ; Acid
H+ Selenic
Selenide Se-2 = H2Se
4. Phosphoric Acid TA;
Acid H+ phosphoric  phosphate (PO4)-3 =H3PO4
5. Strontium Hydroxide TC;
Sr+2 OH-1 = Sr(OH)2
(Remember OH is a BASE)
Write the name for each
6.
7.
8.
9.
HCl BA; Hydrochloric Acid
HNO3 TA ; NO3 is Nitrate
ic Nitric Acid
H2CO3 TA; CO3 is Carbonate
ic = Carbonic Acid
Ca(OH)2 TC; Calcium Hydroxide
(Remember OH is a BASE)