Unit 2: Antacids: adapted from Kendall Hunt Chemistry You Need To KNow
Section 2.1 Types of Matter
 What is matter?
Can be
separated
Pure Substance
Mixture
Define/describe:
Define/describe:
Example:
Example:
Symbol:
Symbol:
Can be
separated
Element
Define/describe:
Can be
separated
Compound
Define/describe:
Homogeneous
Heterogeneous
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
 Mixtures can be any combination of solids, liquids and gases:
Combination
Solid-Solid
Solid-Gas:
Solid-Liquid
Liquid-Liquid:
Gas-Liquid:
Gas-Gas:
 True Solutions
o Particles do not settle out
o Particles are too small to scatter light
o Example:
Diagram:
Example
 Colloids:
o Particles do not settle out
o Particles are large enough to scatter light (Tyndall Effect)
o Example:
Diagram:
 Suspension:
o Particles will settle out over time.
o Example:
Diagram:
Using the above information about true solutions, colloids, and suspensions, write them in order of
Increasing particle size.
 Making Connections
o Consider an antacid like Maalox®, Tums, ®or Mylanta®. Are they pure substances or
mixtures?
o
Antacids contain active ingredients and inactive ingredients. What purposes do inactive
ingredients serve? List 4.
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Complete the Chart by writing in the column on the left if the substance is an element, compound,
homogeneous mixture or heterogeneous mixture.
Aluminum foil
water
a glass of soda
soil
Carbon dioxide
2.2: Naming Chemicals
The language of Chemistry includes element symbols, chemical formulas and chemical equations. Each
element symbol starts with a capital letter.
 Binary Ionic Compounds
Ionic bond:
Binary Ionic Compound
Ionic Compound
Naming ionic compounds:
o
o
Write the name of the cation first.
For the name of the anion, the ending of the element name is changed to “ide”.
o Example: oxygen becomes oxide; sulfur becomes sulfide; fluorine become fluoride
Examples:
Na Br
First element:
cation:
Second element:
anion:
Name of compound:
Ca Br
First element:
cation:
Second element:
anion:
Name of compound:
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
K2O
First element:
Cation:
Second element:
Cation:
Name of compound:
Now you try:
Complete the chart with the missing information.
Formula
1st element
Cation name
2nd element
Anion name
Compound
name
CaF2
Na3P
NaCl
SrBr2
Polyatomic Ions: more than one atom that together have a charge.
Ternary Compounds: compound containing at least one polyatomic ion.
polyatomic ionic compound
Cation
Polyatomic
ion
(Your reference tables have a list of common polyatomic ions: you don’t need to memorize
them.)
Identifying polyatomic ions
o The only cation (front-half) polyatomic ion is ammonium, NH4
o All other polyatomic ions are anions (written second in the formula)
o Several polyatomic ions have the same three elements but the number of oxygen atoms
is different between them so the subscripts on the oxygen atom will be different. Be
careful to choose the correct one.
o Example: sulfate SO4 and sulfite SO3
o If the formula contains parenthesis () the polyatomic ion is always inside the
parenthesis.
You Try: Find the polyatomic ion in the following compounds using your polyatomic ions list:
NaNO3
K2SO4
Ca(OH)2
(NH4)2S
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Naming compounds with polyatomic ions
o There will be more than 2 capital letters (none starting with H)
o Write the name of the cation (the metal element or ammonium if cation is NH4)
o If the polyatomic ion is the anion, then name it just as it is on the list. You do not have
to change the ending of a polyatomic ion to “ide”.
o If the anion is a single element and not a polyatomic ion, then the ending will change to
“ide” .
o Sometimes a compound is composed of 2 polyatomic ions. For these, you name the
first polyatomic ion followed by the name of the second.
Name the four compounds above for which you previously identified the polyatomic ion.
You Try: Practice naming the following compounds:
Ca(NO3)2
Na3PO4
NH4ClO
K2CO3
Naming ionic compounds when the metal is a transition or multi-valent metal.
o Multi-valent metals or the transition metals are metal elements that have more
than one possible charge for the cation.
o Some of the most common multi-valent metals are copper, iron, nickel, lead,
o Write the name of the metal element (cation) first. Write the name of the anion.
Don’t forget the ending “ide” if it’s a single element. Leave a small space
between for a Roman numeral.
o To determine the Roman numeral to use, determine the total negative charge.
o Total negative charge = total positive charge for neutral compounds.
o Determine the charge of the metal ion.
o Write the charge in Roman numerals in parenthesis after the metal name.
Examples:
CuCl2
Fe2(CO3)3
FeCl3
cation:
cation:
cation:
Oanion:
anion:
anion:
total negative charge:
total negative charge:
total negative charge:
Roman numeral:
Roman numeral:
Roman numeral:
Name:
Name:
Name:
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
You try:
Name the following compounds with multi-valent cations.
PbCl2
PbCl4
MnO
Mn2O3
Covalent Compounds
Binary covalent
compound:
Covalent bond:
Non metal
Non metal
Covalent compound
Identifying and Naming Covalent Compounds
o These compounds have 2 elements
o Both elements are non-metal elements
o Write the name of the first non-metal with a prefix indicating the number of atoms. DO
NOT USE the prefix “mono”.
(Including the “mono” prefix if there is only one atom) and the suffix “ide” as the
ending.
Examples:
Prefix Meaning
Mono- 1
P2O5
SiO2
CO
di2
tri3
First:
First:
First:
tetra
4
penta- 5
Prefix:
Prefix:
Prefix:
hexa- 6
hepta- 7
Second:
Second:
Second:
octa8
nona- 9
Prefix:
Prefix:
Prefix:
deca- 10
Name:
Name:
Name:
You try:
NO2
CCl4
Standard & Honors Chemistry
CO2
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
2.3 Writing Formulas for Chemical Compound
 Writing formulas for Binary Ionic Compounds (metal element + non-metal element)
o Write the symbol and charge for the cation (metal).
o Write the symbol and charge for the anion (non-metal).
o The sum of all of the positive charge and all of the negative charge equals zero in a
neutral atom.
o If the total charge is not equal to zero, you must adjust the number of cations or anion
to create a neutral compound.
Note: Use your periodic table to help you determine the charges of most of the common cations and
anions.
Examples:
Sodium chloride
Na = sodium cation with a 1+ charge
Cl= chloride anion with a 1- charge
Formula:
NaCl
If we combined one of each ion we would write: NaCl. Adding up the charges would give an overall
charge of zero since algebraically 1+-1 = 0. Since only one of each ion is needed we do not need any
subscripts.
Calcium bromide
Calcium symbol and charge:
Bromide symbol and charge:
#Ca needed:
# of Br needed
Formula:
You try:
Compound
name
Cesium
chloride
Potassium
oxide
Calcium sulfide
Cation symbol
Cation charge
Anion Symbol
Anion charge
Formula
Lithium nitride
 Writing formulas for Polyatomic Ionic Compounds
The same process is used as for binary ionic compounds except the anion will be a polyatomic ion that
has its own charge. (The exceptions are ammonium NH4 and dimercury Hg2 which will be cations.)
o Write the symbol for the cation (or the polyatomic ion symbol if ammonium or
dimercury).
o Determine the charge of the cation.
o Write the symbol of the anion or polyatomic ion.
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
o
o
o
Determine the charge.
Adjust the number of each ion so that a neutral compound is formed by adding
subscripts to indicate how many of each ion are needed if more than one.
If you need more than 1 of the polyatomic ions, you must place parenthesis around the
formula for the polyatomic ion BEFORE you subscript it. The subscript goes outside the
parenthesis. YOU DO NOT WANT 2 SUBSCRIPTS SIDE BY SIDE---MUST BE SEPARATED BY
THE PARENTHESIS.
Examples:
Sodium carbonate
Na (+1)
CO3 (2-)
Need 2 sodium ions for each carbonate ion
Na2CO3
Magnesium nitrate
Mg (2+)
NO3 (1-)
Formula:
You try:
Sodium nitrate
Calcium chlorate
Potassium sulfite
Calcium hydroxide
 Writing formulas for compounds with multi-valent metals (transition metals)
The same rules apply as for the compounds above. The Roman numeral gives you the charge on
the cation or multi-valent metal (transition metal).
Examples: Iron (III) oxide
Copper (II) nitrate
You try:
Iron (II) nitrate
Copper (I) chloride
Lead (Iv) hydroxide
Tin (II) oxide
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
 Writing formulas for Covalent Compounds
o These compounds contain prefixes in their names. The prefixes indicate how many of
each atom that you need. If there is not a prefix is it understood to be 1. YOU DO NOT
HAVE TO WORRY ABOUT CHARGES FOR THESE.
Examples:
dinitrogen tetraoxide
Silicon dioxide
You try:
Carbon monoxide
Nitrogen dioxide
Dinitrogen pentoxide
NOTE: In chemistry “di” and “bi” prefixes do not refer to the same thing. Use “di” in naming
compounds to indicate that 2 atoms are needed in a covalent compound. When “bi” is used in a name it
means that the polyatomic ion contains a hydrogen atom.
2.4 Defining, Naming and Writing Acids and Bases
 Arrhenius Acid
o Produce ________________________________________in water
o The hydronium ion is H+ and is a ________________.
o According to the Arrhenius definition, if the acid gives a hydrogen to water, then all
acids will contain hydrogen and it will be the __________(first element written).
 Naming non-oxygen acids
o Start with “____________”
o Do NOT contain______________.
o Use “______________________”
o Fill in the _________________________with the _______________________name
without the last syllable.
o Example: HBR
 Naming Oxygen Acids (oxyacids)
o Start with “_____________________________”
o Contain _________________________
o Use “______________________” for “________________” anions
o Use “ ______________________”for “_________________” anions
o Do _____________use “_______________” with these……..acid in the name is how you
know it begins with hydrogen
o Example: H2SO3
o Example: H2SO4
You try:
HCl
HNO3
H2S
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
H3PO4
 Writing formulas for acids
o Acids with “hydro” in the name
 The cation is________________ .
 Write the symbol and ___________.
 Write the symbol for the anion and find its charge.
 Balance the charges by adding ________________to the hydrogen cation if
needed.
 Example: Hydrofluoric acid
formula:
o Acids without “hydro” in the name
 The cation is________________.
 If it is an “_________________” acid, the anion is the “______________”
polyatomic ion.
 If it is an “_________________” acid, the anion is the” _________________”
polyatomic ion.
 Add _________________to the hydrogen cation to ______________________.
 Example: Carbonic acid __________________ nitrous acid_________________
You try:
Phosphoric acid
Hydroiodic acid
Carbonous acid
Perchloric acid
 Arrhenius Base
o Produces _________________________in water
o Most bases are just ______________with “___________________” as their
___________________________.
o The most common exception to this is _______________________. It is a base even
though it does not contain OH- as the ________________.
o Example: NaOH
You try:
Ca(OH)2
KOH
Sr(OH)2
Copper(II)hydroxide
Magnesium hydroxide
Standard & Honors Chemistry