Unit 2: Antacids: adapted from Kendall Hunt Chemistry You Need To Know
INTRODUCTION:
Why do we need Antacids?
Antacids
Acid Inhibitors
What do they do?
How fast do they work
Examples
Section 2.1 Types of Matter
 What is matter?
Can be separated
Pure Substance
Define/describe:
Mixture
Define/describe:
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Can be separated by
chemical means
Element
Describe:
Compound
Can be separated by
physical means
Homogeneous
Describe:
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 (homogeneous mixtures)
o “Small” Particles do not settle out
o Particles are too small to scatter light
o Examples:
 Colloids: (heterogeneous mixture)
o “Medium Sized Particles” do not settle out
o Particles are large enough to scatter light (Tyndall Effect)
o Examples:
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Example
Heterogeneous
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
 Suspension: (heterogeneous mixture)
o “Large” Particles will settle out over time.
o Examples:
Making Connections to Antacids
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.
You Try: Determine if the substance is an element, compound, homogeneous mixture or heterogeneous
mixture.
Aluminum foil (Al)
Water( H2O)
a glass of soda
soil
Carbon dioxide(CO2)
Tap Water
2.2: Naming Chemicals
The language of Chemistry includes element symbols, chemical formulas and chemical equations. Each
element symbol starts with a capital letter.
Ions
 An atom or group of atoms with a _______________________. The number of
________________________ does not equal the number of _____________________.
 WHY? Atoms ______________ or _______________ electrons to acquire stability like a noble
gas.
Monatomic Ions (formed from a single atom)
Cations
 ________________ charge
 _______________ electrons
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Group A (Representative metals) :The group # for metals in columns 1A, 2A, and 3A is equal to the
charge
Naming them: Take the element name and add the word ion
GroupB (Transition Metals): have more than one charge
You should be familiar with the following transition metals with more than one charge.
Fe+2
Fe+3
Sn+2
Sn+4
Pb+2
Pb+4
Co+2
Co+3
Cr+2
Cr+3
Mn+2
Mn+3
Cu+1
Cu+2
Naming them: Take the element name and place in parentheses the charge number as a roman numeral
and add the word ion
Anions
 ________________ charge
 ________________ electrons
Group A (Representative metals) : subtract the group # for nonmetals in columns 4A, 5A, 6A, and 7A
from 8 to get the charge.
Naming them: Drop the ending of the element and add –ide and then ion
Try These: Write the formula for each ion and name it.
Calcium
Aluminum
Chromium
Zinc
Chlorine
Iron
Sulfur
Phosphorus
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Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
 Binary Ionic Compounds
Ionic bond:
Binary Ionic Compound
Ionic Compound
METAL
NONMETAL
BINARY IONIC
Identifying & Naming ionic compounds:
Look for a compound with 2 elements, one metal and one nonmetal
o
o
Write the name of the metals (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:
NaCl Cation: _______________
Name of compound:
Anion: ________________
CaBr2
Cation: _______________
Name of compound:
Anion: ________________
K2O
Cation: ________________
Name of compound:
Anion: _________________
Now you try:
Complete the chart with the missing information.
Formula
Binary Ionic Compound name
CaF2
Na3P
NaCl
SrBr2
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Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Polyatomic Ions: more than one atom that together have a charge.
Ternary Ionic Compounds: compound containing at least one polyatomic ion.
polyatomic ionic compound
Cation
Polyatomic
ion
METAL
POLTATOMIC ION
TERNARY IONIC COMPOUND
(Your reference table has 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
NH4Cl
Ca(OH)2
(NH4)3PO4
K2CO3
Naming compounds with polyatomic ions
Look for a compound with more than 2 capital elements, at least one metal and one nonmetal
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.
Examples:
Ca(NO3)2
Cation_ ______________
Name of compound:
Anion: ________________
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Na3PO4
Cation _______________
Name of compound:
Anion: ________________
K2CO3
Cation: ________________
Name of compound:
Anion: _________________
You Try!
Formula
Ternary Ionic Compound name
Ca(C3H3O2)2
Li2SO3
Ba(OH)2
(NH4)2S
Transition Metals (multi-valent metal).
o Metal elements that have more than one possible charge for the cation.
o a group “B” metal
o Some of the most common transition metals are copper, iron, and nickel.
o Although group B metals, SILVER (+1), CADMIUM (+2), and ZINC (+2) only have 1
charge
o Although the elements of TIN and LEAD are group A elements, they do have
more than one charge(Pseudo-transition) Sn(+2 and +4) and Pb(+2 and +4)
Naming an Ionic Compound with a Transition Metal
 Look for a compound with one of the transition metals, excluding Ag, Cd, and Zn
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.
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
o Total negative charge = total positive charge for neutral compounds.
o Divide total positive charge by the number of metal atoms
o Write the charge in Roman numerals in parenthesis after the metal name.
Examples:
CuCl
Fe2(CO3)3
ZnBr2
cation:
cation:
cation:
anion:
anion:
anion:
total negative charge:
total negative charge:
total negative charge:
Roman numeral:
Roman numeral:
Roman numeral:
Name:
Name:
Name:
You try:
Name the following compounds with transition metals.
PbCl2
PbCl4
MnO
Mn2O3
Covalent Compounds
Covalent bond:
Non metal
Binary covalent compound:
Non metal
Covalent compound
Identifying and Naming Covalent Compounds
 These compounds have 2 elements & both elements are non-metals
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
To Name a Binary Covalent Compound
o
o
Write the name of the first non-metal with a prefix indicating the number of atoms. DO
NOT USE the prefix “mono”.
Write the name of the 2nd nonmetals with prefix indicating the number of atoms
(Including the “mono” prefix if there is only one atom) and the suffix “ide” as the
ending.
Examples
Prefix
Monoditritetra
pentahexaheptaoctanonadeca-
Meaning
1
2
3
4
5
6
7
8
9
10
P2O5
SiF4
Prefix:
Prefix:
1st element:
1st element:
Prefix:
Prefix:
2nd element:
2nd element:
Name:
Name:
You try:
NO2
N2O4
P4O10
CO
Mixed Practice: Need to ask whether the compound is IONIC or COVALENT!
Na2O
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
K3PO4
Cu(OH)2
N2S
MgCl2
2.3 Writing Formulas for Chemical Compound
Identifying Binary Ionic Compounds
 They end in “-ide” (except “hydroxide and cyanide”) & DO NOT contain covalent prefixes
Writing formulas for Binary Ionic Compounds (metal element + non-metal element)
o
o
o
o
o
Write the symbol and charge for the cation (metal).
Write the symbol and charge for the anion (non-metal).
The sum of all of the positive charge and all of the negative charge equals zero in a
neutral atom.
If the total charge is not equal to zero, you must adjust the number of cations or anion
to create a neutral compound.
Use subscripts to show how many of each type of ion is there
Note: Use your periodic table to help you determine the charges of most of the common cations and
anions.
Examples:
Sodium chloride
Sodium symbol & charge:
Chlorine symbol & charge:
Sum of the positive & negative charges:
Formula:
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:
Bromine symbol and charge:
Sum of the positive & negative charges:
Formula:
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
If we combined one of each ion we would write: CaBr . Adding up the charges would give an overall
charge of +1 since algebraically 2+-1 = +1. An additional bromide ion is needed to make the charges
equal to zero so a subscript of 2 is placed under the bromide ion.
The Criss Cross Method is a simple way to determine the subscripts




Write the symbol and charge for the cation (metal).
Write the symbol and charge for the anion (non-metal).
Cross the charge numbers down diagonally as subscripts if they are not equal to each other
Simplify subscripts if you can
Ca +2 Br-1 
You try:
Compound
name
Cesium chloride
Cation symbol &
Charge
Anion Symbol
& charge
Formula
Potassium oxide
Calcium sulfide
Lithium nitride
Writing formulas for Polyatomic Ionic Compounds
 They DO NOT end in “-ide” (except “hydroxide and cyanide”) & DO NOT contain covalent
prefixes
 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 which will be cation.)
o
o
o
o
o
o
Write the symbol for the cation (or the polyatomic ion symbol if ammonium or
dimercury).
Determine the charge of the cation.
Write the symbol of the anion or polyatomic ion.
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 parentheses 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.
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Examples:
Sodium Carbonate
Sodium symbol & charge:
Carbonate symbol & charge:
Sum of the positive & negative charges:
Formula:
Magnesium nitrate
Magnesium symbol & charge:
Nitrate symbol & charge:
Sum of the positive & negative charges:
Formula:
You try:
Sodium nitrate
Calcium chlorate
Potassium sulfite
Calcium hydroxide
Writing formulas for compounds with multi-valent metals (transition metals)
 These compounds will have roman numerals.
 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
Iron symbol & charge:
Oxygen symbol & charge:
Sum of the positive & negative charges:
Formula:
Copper (II) nitrate
Copper symbol & charge:
Nitrate symbol & charge:
Sum of the positive & negative charges:
Formula:
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
You try:
Iron (II) nitrate
Copper (I) chloride
Lead (IV) hydroxide
Tin (II) oxide
Writing formulas for BINARY COVALENT COMPOUNDS
These compounds contain prefixes in their names.
 To write these formulas: 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. NO
CRISS CROSS METHOD EITHER!
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.
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Mixed Practice: Write the formulas for the following chemicals
Magnesium hydroxide
Copper (II) nitrate
Iron (III) oxide
Nitrogen dioxide
Sodium bicarbonate
2.4 Defining, Naming and Writing Acids and Bases
Arrhenius Acids
o Produce ________________________________________in water
o The hydronium ion is a hydrogen ion attached to ________________
o To recognize and ACID, look for a hydrogen ion as the first element in an aqueous
covalent compound.
Naming non-oxygen acids (Binary Acids)
 These compounds start with “____________ & DO NOT contain______________.
To name these compounds:
o Use HYDRO _____________IC acid
o Fill in the blank with the __________________name of the anion
Example: HBr
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Naming Oxygen Acids (oxyacids)
 These compounds start with “_______” & contain ________________
To name these compounds:
o Use __________ IC acids for “________________” anions
o Use ________ OUS acids”for “_________________” anions
Examples: H2SO3
H2SO4
You try: HCl
HNO3
H2S
H3PO4
Writing formulas for Acids
o Acids with “hydro” in the name
To write these formulas
 Write the cation ______ .
 Write the symbol for the anion and find its charge.
 Balance the charges by adding the appropriate ________________to the
hydrogen cation if needed.
Example: Hydrofluoric acid
o
Acids without “hydro” in the name
To write these formulas
 Write the cation H+1
 If it is an “IC ” acid, the anion is the “-ate ” polyatomic ion.
 If it is an “OUS ” acid, the anion is the” -ite” polyatomic ion.
 Add _________________to the hydrogen cation to _________________
charges.
Example:
Carbonic acid
Nitrous acid
You try:
Phosphoric acid
Hydroiodic acid
Carbonous acid
Perchloric acid
Arrhenius Bases
o Produces _________________________in water
Naming Bases
o Most bases are just __________________________with “hydroxide” as their anion.
o The most common exception to this is _______________________. It is a base even
though it does not contain OH- as the ________________.
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Example: NaOH
You try:
Ca(OH)2
KOH
Sr(OH)2
Copper(II)hydroxide
Magnesium hydroxide
2.5 Characteristics of Acids and Bases
Acids
Produces:
Produces:
Tastes:
Tastes:
Reacts with :
Feels:
Bases
Both form ions when dissolved in water. They are called
_____________________
Strength VS Concentration
Strong:
Weak:
Dilute:
Concentrated:
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Combinations of Strength and Concentration
Dilute
Concentrated
Strong
Weak
 pH scale
o
o
A scale that measures the acidity of a sample
Ranges from :
1----------------------------------7-----------------------------------14
Acidic
Neutral
Basic
o Most acidic: _______
o Most basic: _______
o Neutral: __________
 Measuring pH
Indicators change color based on pH
o
Liquid indicators examples are phenolphthalein or bromothymol blue)
phenolphthalein
Acid : clear
Base: pink
bromothymol blue
Acid: yellow Base: blue
o Paper indicator examples are litmus or pH paper
o pH paper allows a color to match to a specific pH number
For LITMUS paper:
BLUE
RED
o
pH probes or pH meters :
Common substances and their pH values
stomach acid
vinegar
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grapes
milk
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
saliva
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blood
ammonia