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)
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