Module 4; Making and Naming Ionic Compounds
Introduction
Elements/Compounds
Matter is anything that has mass and occupies space. Types of matter can be organized into
several different categories. Pure substances are those that cannot be physically separated into
different substances. Compounds are substances that can be separated into simpler
substances only through chemical reactions. Salts, proteins, sugar, and dyes are all examples
of compounds. Elements are the simplest form of matter that can be obtained through chemical
reaction. The elements are all shown on the periodic table and include copper, gold, oxygen,
and sulfur.
Reactions
Chemical reactions are processes in which one set of chemicals combine to form another set of
chemicals. The initial set of chemicals are called reactants and the final set of chemicals are
called products. Sometimes, it is not obvious that a chemical reaction has taken place. More
often, however, there is a change in color, texture, shape, temperature, or other property to
indicate that a reaction has occurred.
Reactions with copper to make ionic compounds
In the first three reactions you will observe the synthesis of ionic compounds from copper and
one other element. Pennies will be the source of copper.
Reactions with oxygen to make ionic compounds
In the last three reactions, you will observe the synthesis of oxides (compounds with oxygen).
Oxygen in the air will be the source of oxygen. Oxygen in the air is diatomic, O2. Sometimes
reactions need a “push” to get started. Usually this push comes in the form of heat, which gives
the reactants a burst of energy to start the reaction. The reactions forming oxides will need heat;
which will be provided by a Bunsen burner flame to get the reaction started. The flame is NOT a
reactant – it is energy used to get the reaction started.
Nomenclature
When the compounds are made in the demonstrations, you will also write the formulas and
names for them. When naming compounds, first determine if the compound is ionic or covalent.
Covalent compounds do not have a metal in them. Prefixes are used to name covalent
compounds (carbon dioxide for CO2 and Dinitrogen pentoxide for N2O5). If the compound is
ionic, determine if the metal is a fixed metal or a variable metal. If it’s a fixed metal, name the
compound without any prefixes or Roman numerals (sodium chloride for NaCl, potassium nitride
for K3N). If the metal is a variable metal, find the charge on that metal and use a Roman
numeral to show the charge (Nickel (III) chloride for NiCl3, Nickel (II) oxide for NiO).
Note: In this lab, you will be observing four demonstrations from YouTube and doing one
“kitchen” experiment. You will need the following materials for your experiment: Ziploc bag,
penny, bleach, vinegar.
1
, Pre-Lab Exercise.
Use the periodic table to answer the pre-lab questions below.
Na3N N 2O 4 CoF3 CF4 Pb3N2 KI S4 N 2
1) Provide the NAME (not the formula) of all the compounds above that are covalent:
- Dinitrogen Tetroxide, Carbon tetrafluoride, Lead nitride, Tetrasulfur Dinitride
2) Provide the NAME (not the formula) of all the ionic compounds with fixed metals.
Identify the charge on each of those fixed metals (don’t forget that a charge has both a
sign and number such as +1 or -3).
- Sodium +1 nitride -3, Potassium +1 Iodide -1, which for both will be Sodium nitride and
Potassium Iodide
3) Provide the NAME (not the formula) of all the ionic compounds with a variable metal.
Identify the charge on each of those variable metals (don’t forget that a charge has both a
sign and number such as +1 or -3).
- Cobalt +3 fluoride -3 which would then nbe Cobalt (III) fluorid
2
Introduction
Elements/Compounds
Matter is anything that has mass and occupies space. Types of matter can be organized into
several different categories. Pure substances are those that cannot be physically separated into
different substances. Compounds are substances that can be separated into simpler
substances only through chemical reactions. Salts, proteins, sugar, and dyes are all examples
of compounds. Elements are the simplest form of matter that can be obtained through chemical
reaction. The elements are all shown on the periodic table and include copper, gold, oxygen,
and sulfur.
Reactions
Chemical reactions are processes in which one set of chemicals combine to form another set of
chemicals. The initial set of chemicals are called reactants and the final set of chemicals are
called products. Sometimes, it is not obvious that a chemical reaction has taken place. More
often, however, there is a change in color, texture, shape, temperature, or other property to
indicate that a reaction has occurred.
Reactions with copper to make ionic compounds
In the first three reactions you will observe the synthesis of ionic compounds from copper and
one other element. Pennies will be the source of copper.
Reactions with oxygen to make ionic compounds
In the last three reactions, you will observe the synthesis of oxides (compounds with oxygen).
Oxygen in the air will be the source of oxygen. Oxygen in the air is diatomic, O2. Sometimes
reactions need a “push” to get started. Usually this push comes in the form of heat, which gives
the reactants a burst of energy to start the reaction. The reactions forming oxides will need heat;
which will be provided by a Bunsen burner flame to get the reaction started. The flame is NOT a
reactant – it is energy used to get the reaction started.
Nomenclature
When the compounds are made in the demonstrations, you will also write the formulas and
names for them. When naming compounds, first determine if the compound is ionic or covalent.
Covalent compounds do not have a metal in them. Prefixes are used to name covalent
compounds (carbon dioxide for CO2 and Dinitrogen pentoxide for N2O5). If the compound is
ionic, determine if the metal is a fixed metal or a variable metal. If it’s a fixed metal, name the
compound without any prefixes or Roman numerals (sodium chloride for NaCl, potassium nitride
for K3N). If the metal is a variable metal, find the charge on that metal and use a Roman
numeral to show the charge (Nickel (III) chloride for NiCl3, Nickel (II) oxide for NiO).
Note: In this lab, you will be observing four demonstrations from YouTube and doing one
“kitchen” experiment. You will need the following materials for your experiment: Ziploc bag,
penny, bleach, vinegar.
1
, Pre-Lab Exercise.
Use the periodic table to answer the pre-lab questions below.
Na3N N 2O 4 CoF3 CF4 Pb3N2 KI S4 N 2
1) Provide the NAME (not the formula) of all the compounds above that are covalent:
- Dinitrogen Tetroxide, Carbon tetrafluoride, Lead nitride, Tetrasulfur Dinitride
2) Provide the NAME (not the formula) of all the ionic compounds with fixed metals.
Identify the charge on each of those fixed metals (don’t forget that a charge has both a
sign and number such as +1 or -3).
- Sodium +1 nitride -3, Potassium +1 Iodide -1, which for both will be Sodium nitride and
Potassium Iodide
3) Provide the NAME (not the formula) of all the ionic compounds with a variable metal.
Identify the charge on each of those variable metals (don’t forget that a charge has both a
sign and number such as +1 or -3).
- Cobalt +3 fluoride -3 which would then nbe Cobalt (III) fluorid
2
