Name ______________________________________ Date __________________ Hr _____

Chapter 2—Antacids

Introductory Activity List everything you know about acids and bases in your notebook. Where have you used

them or come in contact with them in your life? Explain what you understand about antacids. Share your ideas with the class.

Section 2.1—Types of Matter

Matter can be classified

Matter Anything that has ________ and _______________________ Anything made from ____________ Examples:

o _________________o _________________o _________________

o _________________o _________________

Pure Substances versus Mixtures Pure Substance: Every ___________ of matter is _______________ Mixture: ______________________ type of matter ___________ togetherElements versus Compounds Elements: ________________ is the ________ type of atom Compounds: _______________________ type of atom _______________ together. Every

_________________ is the _______________.Elements Can be found on _________________________________ ________________ be separated by ______________ or _____________ processes.

Compounds

Name _______________________

_______________ be separated by ________________________________

Mixtures Homogeneous (aka “solution”): ________________________ throughout Heterogeneous: Different matter __________________ (chunks, bubbles, floaties, layers,

etc.) ____________ be separated __________________ or ________________

Mixture possibilities Mixtures can be any combination of solids, liquids and gases:

o Solid-solid: _________________

o Solid-gas: _________________

o Solid-liquid: _________________

o Liquid-liquid: _________________

o Gas-Liquid: _________________

o Gas-Gas: _________________

True solutions, Colloids & Suspensions

Particles Scattering Light If the dissolved particles are large enough to ______________, we say it exhibits the

“__________________” Solution: ____________________ through unchanged Colloids: exhibit the _________________

Connect these concepts with Antacids What type of matter do you think antacids are?

o Pure substance (Element or compound)o Mixture (homogeneous or heterogeneous)

Name _______________________

They contact active & inactive ingredients. What purposes could the inactive ingredients serve?

Let’s Practice Determine if each is element, compound, homogeneous or heterogeneous mixtures:

o Tin foilo Copper pipeo Concrete

o Carbon tetrachlorideo Sports drink

Section 2.2—Naming Chemicals

The Language of Chemistry

Each element symbol ________________________________

Binary Ionic compounds Ionic Bond: bond formed by ________________ between ______________________ Binary Ionic Compound: compound containing ____________________________________

Name _______________________

Metals & Non-Metals

Identifying & Naming Binary Ionic These compounds have:

o __________________ (“binary”)o __________________ (“ionic”

To name these compounds:o Write the ______________________________________ (the cation)o Write the ______________________________________ (the anion) with the

suffix _________

Example #1: NaClExample #2: CaBr2

Example #3: K2OLet’s Practice

o CaF2

o Na3Po NaClo SrBr2

Polyatomic Ionic Compounds Polyatomic Ion--________________________ together that have a _____________ Polyatomic Ionic Compound—compound containing _______________________________

Help Identifying Polyatomic Ions

Name _______________________

The only cation (________-half) polyatomic ion is “__________” All ___________ polyatomic ions are anions (_________-half) The ___________________________________ (it must match exactly with the one on your

ion list) If there are ___________________, the polyatomic ion is _______________ (ignore the

number outside)

Practice Identifying Polyatomic Ions NaNO3

NH4Cl Ca(OH)2

(NH4)3PO4

K2CO3

Identifying & Naming Polyatomic Ionic These compounds have:

o _______________________________________ letters (not starting with H)o Contain _____________________________ & 1 non-metal

To name these compounds:o Write the name of the _______________ (the metal element name or

“Ammonium” for “NH4”)o If the anion is a polyatomic ion, write the

_______________________________________o If the anion is a single non-metal _________________, write its

___________________________________

Example #4: NaNO3

Example #5: K2SO4

Example #6: Ca(OH)2

Example #7: (NH4)2S

Let’s Practiceo Ca(NO3)2

o Na3PO4

o NH4ClOo K2CO3

Multivalent Metals Mutlivalent metal—metal that has _____________________________ for cationic charge

Identifying & Naming Multivalent Metals These compounds have:

Name _______________________

o One of the ________________________ in that chart To name these compounds:

o Write the ____________________ element (cation)o Write the ____________________ (element name with “-ide” or polyatomic ion

name)o Determine the ____________________________o Total _________________ charge = total _______________ charge for all neutral

compoundso Determine the _____________________ atomo Write the ______________ in ____________________ in parenthesis after the

metal’s name

Example #8: CuCl Example #9: Fe2(CO3)3

Let’s Practiceo PbCl2

o PbCl4

o MnOo Mn2O3

Binary Covalent Compounds Covalent bond—atoms _____________________________ Binary Covalent Compound—Compound made from _________________________ that

share electrons

Identifying & Naming Binary Covalent These compounds have:

o _______ elements (“binary”)o Both _______________ (“covalent”)

To name these compounds:o Write the __________________ element with the ____________ indicating the

number of atoms (_____________ don’t use “mono-”)o Write the __________________ element with the ____________ indicating the

number of atoms (_____________ “mono-”) and the suffix “ide”

Covalent Prefixes1.mono- 6.hexa-2.di- 7.hepta-3.tri- 8.octa-4.tetra- 9.nona-5.penta- 10.deca-

Name _______________________

Example #10: P2O5

Example #11: SiO2

Let’s Practiceo CO2

o N2O4

o P4O10

o CO

Nomenclature Summary

Mixed Practiceo Na2Oo K3PO4

o Cu(OH)2

o (NH4)2So MgCl2

Section 2.3—Chemical Formulas

Binary Ionic compoundsDefinitions Ionic Bond – bond formed by attraction between __________________________________ Binary ionic compound – compound containing ___________ elements—one ____________

and one ________________________

Identifying & Writing Binary Ionic

Name _______________________

These compounds:o End in “___________” (except “___________” and “_____________”)o Do _______ contain covalent prefixes

To write these formulas:o Write the _________ & ___________ of the first element (the metal, _________)o Write the _________ & ___________ of the second element (the non-metal,

_________)o Add more of the cations and/or anions to have a __________________________o Use ______________________ to show ______________________ of each type

of ion is there.

Example #1: Sodium chloride

Example #2: Calcium bromide

Let’s Practice Cesium chloride Potassium oxide Calcium sulfide Lithium nitride

Polyatomic Ionic CompoundsDefinition Polyatomic ion - _______________________________ that together have a _____________ Polyatomic ionic compound – compound containing at least __________________________

Identifying & Writing Polyatomic Ionic These compounds:

o Do __________________ with “-ide” (except hydroxide & cyanide)o Do _____________ use covalent ____________________

To write these formulas:o Write the ___________ & _____________ of the cation & aniono Add additional cations or anions to have a __________________________o Use _____________________ to show the number of ionso When using subscripts with a polyatomic ion, you must

________________________________________________________________

Example #3: Sodium carbonate

Name _______________________

Example #4: Magnesium nitrate

Let’s Practice Sodium nitrate Calcium chloriate

Potassium sulfite Calcium hydroxide

Multivalent MetalsDefinition Multivalent Metal – metal that has ______________________________________________

Identifying & Writing Multivalent Metals These compounds:

o Will have _______________________ To write these formulas:

o Same as binary ionic or polyatomic ionic.o The ________________________ tell the ________________ of the

______________ (cation)

Example #5: Iron (III) oxide

Example #6: Copper (II) nitrate

Let’s Practice Iron (II) nitrate Copper (I) chloride

Lead (IV) hydroxide Tin (II) oxide

Binary Covalent CompoundsDefinition Covalent bond – atoms __________________________ Binary Covalent compound – compound made from _________________________ that

share electrons

Identifying & Writing Binary Covalent These compounds:

o Use covalent ______________________ To write these formulas:

o Write the ________________ of the first and second elemento Use the covalent ____________________ (assume the first element is “1” if

there’s no prefix) as the __________________ to show number of atoms.

Name _______________________

Example #7: Dinitrogen tetraoxide

Example #8: Silicon dioxide

CAUTION!!!

Let’s Practice Carbon monoxide Nitrogen dioxide Diphosphorus pentaoxide

Nomenclature Summary

Mixed Practice Magnesium hydroxide Copper (II) nitrate Iron (III) oxide

Nitrogen dioxide Sodium bicarbonate

Name _______________________

Section 2.4—Defining, Naming & Writing Acids & Bases

Acids – Arrhenius Definition Produce ______________________________________ in water Hydronium ion is ___________ + a ______________________ By this definition, if an acid is to give a ____________ to water, then all acids will have

_________________ as the _____________ (first element written).

Naming AcidsNaming non-oxygen Acids These compounds have:

o Start with “________” (more than 1 “H” is OK, too).o Do ______ contain _____________

To name these compounds:o Use “______________________________”o Fill in the _____________ with the _____________ name without the last

syllable Example #1: HBr

Naming Oxygen Acids These compounds have:

o Start with “_________” (more than 1 “H” is OK, too).o __________ contain _______________

To name these compounds:o Use “_______________” for “_______” anionso Use “_______________” for “_______” anionso Do _________ use “____________” with these…the word “acid” is how you

know it begins with hydrogen, not “hydro-” Example #2: H2SO3

Example #3: H2SO4

Let’s Practice HCl HNO3

H2S H3PO3

Writing Acid Formulas“Hydro-” acids

Name _______________________

To write these formulas:o The cation is ____________o Write the ___________ and ____________o ____________ the charges by _________________________________ to the

hydrogen cation Example #4: Hydrofluoric Acid

NON “Hydro-” acids To write these formulas:

o The cation is ___________o If it is an “________” acid, the anion is the “________” polyatomic iono If it is an “________” acid, the anion is the “________” polyatomic iono Add ____________ to the hydrogen cation to ___________________________

Example #5: Carbonic Acid

Example #6: Nitrous Acid

Let’s Practice

The most common ______________ to this is __________________o _____________ (ammonia) is a __________ even though it doesn’t contain “-

OH” as the anion Example #7: NaOH

Let’s Practice Ca(OH)2

KOH Sr(OH)2

Copper (II) hydroxide Magnesium hydroxide

Section 2.5—Characteristics of Acids and Bases

Characteristics of Acids & Bases

Strength versus Concentration Strong acid: _____________ of the acid molecules have

_____________________________ to water Weak acid: ____________________ of the acid molecules have

____________________________ to water Lower concentration: ________________________________ (what’s being dissolved)

particles Higher concentration: _____________________ (what’s being dissolved) particles

Combinations of Concentration & Strength

Name _______________________

Other notes All of the _______________ apply to ____________ as well (concentration and strength) Many people think all acids are dangerous and all bases are more safe

o Vinegar is an _____________ we eat…______________________!o Sodium hydroxide is a very ____________________…not all of them are less

harmful than acids!o The __________________ an acid or base is (and the more concentrated it is), the

more ___________________ it is for you

pH scale: Is a scale to measure the acidity of a sample Goes from _________ to __________ ______________ is most ______________ ______________ is neutral ______________ is most _____________ (least acidic)

Ways to measure pH ___________________ change _____________ based on ________

o _______________ indicators – various indicators change colors at different pH’so _______________ indicator – a _____________________ of liquid indicators to

produce a “_______________” changing colors at several pH’s ____________ Indicators

o Paper with a liquid indicator on it (___________ paper or pH paper) pH __________ or pH probes__________________ determine pH and give a read-out

Name _______________________

Section 2.6—Chemical Reactions

Chemical Reactions Bonds and atoms are _________________________________________________

Chemical Equations The _____________ of chemistry that shows the ________________________ and the

__________________________ of a chemical reaction.

Examples of Chemical Equations Word equation: magnesium metal is reacted with aqueous hydrochloric acid to produce

aqueous magnesium chloride and hydrogen gas  Formula equation: Mg (s) + 2 HCl (aq) MgCl2 (aq) + H2 (g) Visualization:

Parts of a Chemical Equation

Writing Chemical Equations You must write each ______________________________________________! (Section 2.2) “and”, “is mixed with” or “reacts with” = ________ “yield”, “produces” and “forms” = __________

Let’s Practice #1 Aluminum metal is reacted with hydrochloric acid to form aluminum chloride and hydrogen

gas

Name _______________________

Let’s Practice #2 Copper (II) nitrate and sodium hydroxide form copper (II) hydroxide and sodium nitrate

Double Replacement Reactions The _____________ from two compounds ____________________________. General format of Double Replacement Reactions:

Products of a Double Replacement Step 1: Combine the ___________________ reactant with the ___________________

reactant Step 2: Combine the ___________________ reactant with the ___________________

reactant Step 3: ________________________________________ when writing formulas

o Only __________________ that are in the original compound there if they are a ________________________________________!

Neutralization Reactions General format of a neutralization reaction:

Neutralization reactions are double replacement reactions where one cation is “H” and one anion is “OH” and water is formed

Products of a Neutralization Reaction Step 1: Combine the ___________________ reactant with the ___________________

reactant Step 2: Combine the ___________________ reactant with the ___________________

reactant Step 3: ________________________________________ when writing formulas

o Only __________________ that are in the original compound there if they are a ________________________________________!

o You can write the water as “HOH” when you combine the cation & anion or you can change it to “H2O”

Name _______________________

Let’s Practice #3 Sr(OH)2 + HBr

Let’s Practice #4 HCl + Ca(OH)2

Section 2.7—Balancing Equations

Law of Conservation of Matter/Mass Law of Conservation of Matter – Matter

___________________________________________ during ________________________________________

Also called the Law of Conservation of __________________________ (since all _________________________)

How Does the Law Lead to Balancing? Law of Conservation of Matter: ____________________________________________

during a chemical or physical change Therefore: The _________________________ and the ______________________________

must be the _____________ So we must: Ensure the ________________________________ are the

_______________________ of the equation…by balancing!

How do we Balance Equations? _________________ balance ____________________________ a compound. _________________ balance ______________ in an ________________.

What do Coefficients Really Mean?

Name _______________________

How to Balance Chemical Equations Make a _________________________ ______________ the number of ___________________________ on the reactants and

products side. Don’t forget to ___________ all the atoms of the ______________________—even if it appears in more than one compound!

Add ___________________ to balance the numbers. Each time you add a coefficient, _______________________ with the new quantities of each atom.

Place a “1” in any empty coefficient location. Filling each coefficient location lets you and the grader know that you finished the problem rather than you left some blank because you weren’t done!

Choosing the Order of Balancing Start: Elements that appear _____________________________. Start: Elements in most _______________________. _______ for later: Elements that ________________________ per side. _______ for later: Elements that are __________________.

What about a different order? You’ll still get to the correct answer, but it will take longer and be more complicated!

Polyatomic Ions Polyatomic ion – ___________________ that together has a net ______________ You may _________________________________—__________________________ on

both sides of the reaction.

Name _______________________

__________ is a polyatomic ion that is sometimes “hidden” in ___________.

Let’s Practice #1__ HCl + __ Ca(OH)2 __ CaCl2 + __ H2O

Let’s Practice #2__ H2 + __ O2 __ H2O

Let’s Practice #3__ Fe + __ O2 ___ Fe2O3

Section 2.8—Speeding Up a Reaction

Kinetics & Reaction Rates _____________ – __________ of the ____________ of reactions Reaction Rate – _____________ at which _________________________________

Collision Theory Defines 3 ____________________ to be met _____________________ to occur. Only a _____________________________ meet the requirements and result in a

______________ ______________ Must Occur Collision with _________________________ Collision with _________________________

Activation Energy _________________________________ to occur during a collision

Reaction Coordinate Diagram Reaction coordinate diagrams show the energy changes throughout the reaction

Activated Complex

Name _______________________

Factors Affecting Reaction Rates Surface Area of Reactants

o Reactants __________________ in order to reacto _________________________ means _____________________ can come in

_____________ with each other at the ____________________o More reactants can collide at the same time and a fraction of those will result in

reactiono As surface area ___________, reaction rate _____________

Concentrations of Reactantso Only a small fraction of the collisions meet the requirements and result in a

reactiono _____________________ mean ____________________ will occuro If ____________________ occur, _____________ will meet the requirements

and _______________________o As reaction concentration ____________, reaction rate _____________

Temperatureo Reactants must collide with ______________ energy equal to the

_______________________o If molecules are at a ________________________, they have a

___________________________________________o With higher energy molecules, ______________ will have __________________

and more often result in reactiono For __________ reactions, as temperature ________________, reaction rate

_____________

Catalysts Substance that ___________________________________________________________

o They increase the __________________________________________ produce a reaction

o For example, catalysts _____________ one or more of the _________________ in place to allow _________________ to occur with the ____________________

o Once the reaction has occurred, the catalyst releases the molecule(s) and finds another one to help

Catalysts & Reaction Diagrams ________________________________________ of the reaction by letting it proceed in a

different way.With ____________________________, a higher percentage of _____________ will be ______________ (they don’t need to collide with as much energy to be successful)