unit 2: antacids: guided notes: adapted from kendall...
TRANSCRIPT
Unit 2: Antacids: adapted from Kendall Hunt Chemistry You Need To Know
INTRODUCTION:
Why do we need Antacids?
Antacids Acid InhibitorsWhat do they do?
How fast do they work
Examples
Section 2.1 Types of Matter
Matter is anything that has _________________ and takes up space(______________________)
Examples: _______________________________________________________________
Non-examples: __________________________________________________________
Pure Substance Mixture
Define/describe:
Define/describe:
Matter can be broken down into
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
SUBSTANCES MIXTURES
Element Compound Homogeneous Heterogeneous
particle=atom particle= molecule
Mixtures can be any combination of solids, liquids and gases:
Standard & Honors Chemistry
Can be separated by chemical means
Can be separated by physical means
Combination ExampleSolid-Solid
Solid-Gas:
Solid-Liquid
Liquid-Liquid:
Gas-Liquid:
Gas-Gas:
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
True Solutions (homogeneous mixtures)o “Small” Particles do not settle outo Particles are too small to scatter lighto Examples:
Colloids: (heterogeneous mixture)o “Medium Sized Particles” do not settle outo Particles are large enough to scatter light (Tyndall Effect)o Examples:
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?
You Try: Determine if the substance is an element, compound, homogeneous mixture or heterogeneous mixture.
Aluminum foil (Al)Water( H2O)
a glass of sodasoil
Carbon dioxide(CO2)Tap Water
NOTICE: a substance can be represented by a single chemical formula
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 electrons.
WHY? Atoms ______________ or _______________ electrons to acquire stability like a noble gas.
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Monatomic Ions (formed from a single atom)
Cations
________________ charge
metal atoms that_______________ electrons
Group A (Representative metals) :The group # for metals in columns 1A, 2A, and 3A is equal to the charge of the ________________________.
Naming them: Take the element name and add the word ion
Group B (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 Nonmetals that gain ________________ electrons
Group A (Representative nonmetals) : subtract the group # 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
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Chromium
Chlorine
Sulfur
You Try!
Aluminum
Zinc
Iron
Phosphorus
BINARY IONIC COMPOUNDS
METAL NONMETAL BINARY IONIC
How to Identifying & Name an Ionic Compound:
Look for a compound with 2 elements, one metal and one nonmetal
o Write the name of the metal (cation) first. o 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: ________________
Standard & Honors Chemistry
+Cation
-Anion
Ionic bond: Binary Ionic Compound
Ionic Compound
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
K2O Cation: ________________ Name of compound:
Anion: _________________
Now you try:
Complete the chart with the missing information.
Formula Binary Ionic Compound name
Li2O
Sr3P2
MgS
BaI2
Polyatomic Ions: an ion made of more than one atom that together have a single charge.
Ternary Ionic Compounds: compound containing at least one polyatomic ion.
polyatomic ionic compound
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 ionso 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 parentheses () 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
Standard & Honors Chemistry
CationPoly-atomic ion
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
How to Identify and Name compounds with polyatomic ions
Look for a compound with more than 2 capital elements, at least one metal and one nonmetal
o Write the name of the cation (the metal element or ammonium if the cation is NH4)o If the polyatomic ion is the anion, then name it just as it is on the list. 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: ________________
Na3PO4 Cation _______________
Name of compound: Anion: ________________
K2CO3 Cation: ________________
Name of compound: Anion: _________________
You Try!
Formula Ternary Ionic Compound name
Ca(C2H3O2)2
Li2SO3
Ba(OH)2
(NH4)2S
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Transition Metals o Metal elements that have more than one possible charge for the cation. o a group “B” metalo Although group B metals, SILVER (+1), CADMIUM (+2), and ZINC (+2) only have 1
chargeo 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 them 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 Divide total positive charge by the number of metal atomso Write the charge in Roman numerals in parenthesis after the metal name.
Examples:
You try: Name the following compounds with transition metals. PbCl2 PbCl4 MnO Mn2O3
Binary Covalent Compounds
Standard & Honors Chemistry
CuCl
cation:
anion:
total negative charge:
Roman numeral:
Name:
Fe2(CO3)3
cation:
anion:
total negative charge:
Roman numeral:
Name:
ZnBr2
cation:
anion:
total negative charge:
Roman numeral:
Name:
Covalent bond: Binary covalent compound:
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
How to Identify & Name Covalent Compounds These compounds have 2 elements & both elements are non-metals
To Name a Binary Covalent Compoundo Write the name of the first non-metal with a prefix indicating the number of atoms. DO
NOT USE the prefix “mono” if only 1 atom. o Write the name of the 2nd nonmetal with prefix indicating the number of atoms
(Include the “mono” prefix if there is only one atom) and the suffix “ide” as the ending. Examples
You try:
SO2 N2Cl4
P4O10 CO
Standard & Honors Chemistry
Non metal Non metal
Covalent compound
P2O5
Prefix:
1st element:
Prefix:
2nd element:
Name:
SiF4
Prefix:
1st element:
Prefix:
2nd element:
Name:
Prefix Meaningmono- 1 di- 2tri- 3tetra 4penta- 5hexa- 6hepta- 7octa- 8nona- 9deca- 10
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Mixed Practice: Need to ask whether the compound is IONIC or COVALENT!
Na2O
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 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. o 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:
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Formula:
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
Cation symbol & Charge
Anion Symbol & charge
Formula
Cesium chloride
Potassium oxide
Calcium sulfide
Lithium nitride
Writing formulas for Ternary 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 exception is ammonium NH4 which will be a cation.)
o Write the symbol & charge for the cation and aniono 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. o 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.
o Shortcut Rule can work as well.
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 Ionic Compounds with a Transition Metal
These compounds will have roman numerals.
The same rules apply as for the compounds above. The Roman numeral gives you the charge of the 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
Sulfur tetraiodide
Trichlorine pentasulfide
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 BasesArrhenius Acids
o Produce ________________________________________in watero 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.Bronsted Lowry Acids
o Is a proton ___________________________o HCl + H2O H3O+1 + Cl-1
______ ______ _______ ______
Naming non-oxygen acids (Binary Acids) These compounds start with “____________ & DO NOT contain______________.To name these compounds:
o Use HYDRO _____________IC acido Fill in the blank with the __________________name of the anion
Example: HBr
Naming Oxygen Acids (oxyacids) These compounds start with “_______” & contain ________________To name these compounds:
o Use __________ IC acids for “________________” anionso Use ________ OUS acids”for “_________________” anions
Examples: H2SO3
H2SO4
You try: HCl HNO2
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
H2S H3PO4
Writing Formulas for Acidso 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 or do Criss Cross method
Example: Hydrofluoric acid
o Acids without “hydro” in the nameTo 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 or do Criss Cross method
Example: Carbonic acid
Acetic acid
You try: Phosphorous acid Hydroiodic acid
*** 5 Acids You must Know:
1. ____________________________________ 2. _______________________________________
3. _____________________________________ 4. ______________________________________
5. ______________________________________
Arrhenius Baseso Produces _________________________in water
Bronsted Lowry Baseso Is a proton ___________________________o NH3 + H2O OH- + NH4
+ ________ ________ ___________ ______________
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Conjugate Acid-Base Pairs
Conjugate Acid- substance formed when a _____________ gains a [H+] ion. Conjugate Base- substance formed when an ___________ loses a [H+] ion.
Naming Baseso 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- (hydroxide)
Example: NaOH
You try: Ca(OH)2 KOH
Copper(II)hydroxide Magnesium hydroxide
2.5 Characteristics of Acids and BasesAcids Bases
Produces: Produces:
Tastes: Tastes:
Reacts with : Feels:
Neutralizes a base to form: Neutralizes an acid to form:
Both form ions when dissolved in water. They are called _____________________
Strength Vs ConcentrationStrong Acid: Weak Acid:
Dilute: Concentrated:
Standard & Honors Chemistry
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Combinations of Strength and Concentration
Concentrated Dilute
pH scaleo A scale that measures the acidity of a sample
stronger weaker weaker strongero Ranges from : 1----------------------------------7-----------------------------------14
Acidic Neutral Basico Most acidic: _______o Most basic: _______o Neutral: __________
Measuring pHIndicators change color based on pH
o Liquid indicators: examples are phenolphthalein and bromothymol blue)
phenolphthalein Acid : stays clear Base: turns pinkbromothymol blue Acid: turns yellow Base: turns blue
o Paper indicators: examples are litmus and pH paper
pH paper allows a color to match to a specific pH number
LITMUS paper: BLUE
RED
o pH probes or pH meters : __________________________________________
Standard & Honors Chemistry
Concentrated Dilute
Strong
Weak
Unit 2: Antacids: Guided Notes: adapted from Kendall Hunt Chemistry You Need To Know
Standard & Honors Chemistry