Unit 2: Antacids: Guided Notes: adapted from Kendall …sotochem.cmswiki.wikispaces.net/.../U2a_13-14.docx · Web viewUnit 2: Antacids: adapted from Kendall Hunt Chemistry You Need

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 Substances Mixtures

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

Compounds 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:


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.



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



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: ________________


+Cation

-Anion

Ionic bond: Binary Ionic Compound

Ionic Compound


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


CationPoly-atomic ion


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_ ______________


Na3PO4 Cation _______________


K2CO3 Cation: ________________

Name of compound: Anion: _________________

You Try!

Formula Ternary Ionic Compound name

Ca(C2H3O2)2

Li2SO3

Ba(OH)2

(NH4)2S



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


CuCl

cation:

anion:

total negative charge:

Roman numeral:

Name:

Fe2(CO3)3

cation:

anion:


Roman numeral:

Name:

ZnBr2

cation:

anion:


Roman numeral:

Name:

Covalent bond: Binary covalent compound:


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


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


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:




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.



Examples: Sodium Carbonate Sodium symbol & charge:

Carbonate symbol & charge:


Formula:

Magnesium nitrate Magnesium symbol & charge:

Nitrate symbol & charge:


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:


Formula:

Copper (II) nitrate Copper symbol & charge:

Nitrate symbol & charge:


Formula:



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



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



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

+ ________ ________ ___________ ______________



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:



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 : __________________________________________


Concentrated Dilute

Strong

Weak



Documents

Unit 2: Antacids: Guided Notes: adapted from Kendall …sotochem.cmswiki.wikispaces.net/.../U2a_13-14.docx · Web viewUnit 2: Antacids: adapted from Kendall Hunt Chemistry You Need