chapter 2a: antacids. why do we need antacids? your body needs hydrochloric acid to digest food too...
TRANSCRIPT
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Chapter 2A: Antacids
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Why do we need antacids?
Your body needs hydrochloric acid to digest food
Too much causes heartburn, ulcers and can damage your esophagus
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Antacids versus Acid Inhibitors
Acid InhibitorsAntacids
Neutralizes the acid currently in your system
Controls the amount of acid your body produces
There are two types of medicines you can use
Work quickly but your body will make more acid again
Long-term solution, but needs to build up in your
system to be most effective
Alka-Seltzer ®, Rolaids ®, Tums ®, Malox ®, Mylanta ®
Tagamat ®, Zantac ®, Pepcid AC ®
Is it fair when a commercial compares the fast action of an antacid to an acid inhibitor that takes up to 7 days to build up?
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Antacids
This chapter will introduce the chemistry needed to understand how antacids workSection 2.1: Types of MatterSection 2.2a: Identifying IonsSection 2.2b: Naming Ionic CompoundsSection 2.2c: Naming Covalent CompoundsSection 2.3: Writing Formulas for Ionic &
Covalent compounds
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Section 2.1—Types of Matter
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Matter is….
Anything that has mass and takes up space (volume)
Anything made from atomsExamples: elements, molecules, cells,
people, air, water, paperNon Examples: dreams, energy (light,
heat), emotions
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Pure Substances versus Mixtures
MixturesPure Substances
Contain only 1 type of particle
Elements or Compounds
Contain 2 or more pure substancesHomogeneous or Heterogeneous
Matter is classified as either a pure substance or a mixture
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Pure Substances
CompoundElements
Simplest kind of matter
Made of only 1 kind of atom
Cu, Ag, Fe, Br2
2 or more elements
chemically bonded together to form molecules. Each is the same fixed ratio of elements.H2O, NaCl, CO2
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Elements
Pure substanceEvery atom is the same
Elements can be found on the periodic table!
Element
Single AtomCannot be separated by chemical or physical processes
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Elements
http://www.youtube.com/watch?v=7FesjAdIWBk
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Compounds
Pure substanceEvery molecule is the same
Compound
Single Molecule
Made of more than one type of atom bonded together
Can only be separated by chemical reactions
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Mixtures
Not a pure substancePhysical combination of more than 1 type of pure substance
Mixture
More than 1 different type of matter
Can be separated physically byDistillationFiltrationChromatography
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Mixtures
HeterogeneousHomogeneous (aka “solution”)
It looks the same throughout;
substances evenly dispersed
Ex. salt water, alloys, clean air
Different substances can be seen (chunks,
bubbles, floaties, layers)
Ex. salad dressing, fog, chocolate chip
cookies, soil
Mixtures can be classified as homogeneous or heterogeneous
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Mixture possibilities
Mixtures can be any combination of solids, liquids and gases:Solid-solid: Medicine tabletSolid-gas: Pop Rocks candySolid-liquid: Ice waterLiquid-liquid: lemon waterGas-Liquid: Carbonated waterGas-Gas: Air
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Homogeneous MixturesBrass: copper in zinc
Air: oxygen gas in nitrogen gas
Kool-Aid: sugar in water
Milk: fat, proteins, sugar in water
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Heterogeneous MixturesOil in waterItalian Salad Dressing
Chicken Noodle Soup Fruit Salad
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Classification of Matter
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True Solutions, Colloids & Suspensions
ColloidTrue Solution
SMALL particles don’t settle out
and are too small to scatter lightEx: salt water,
air, brass
INTERMEDIATE particles don’t
settle out but are large enough to
scatter light:Ex: fog, foam,
jello, paint
Suspension
LARGE particles that settle out
over timeEx: oral
medicines, italian dressing, paint
Dissolved Particle Size Increases
Homogeneous Heterogeneous Heterogeneous
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True Solutions
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Suspensions
vinegar and oil salad dressing
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Particles Scattering Light
If the dissolved particles
are large enough to scatter
light, we say it exhibits the
“Tyndall Effect”SolutionLight passes through unchanged
Colloids exhibit the Tyndall EffectLight is scattered by larger solute particles
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Connect these concepts with Antacids
What type of matter do you think antacids are?Pure substance (Element or compound)Mixture (homogeneous or heterogeneous)
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Connect these concepts with Antacids
Antacids are mixtures.They contain active & inactive ingredientsWhat purposes could the inactive
ingredients serve?
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Connect these concepts with Antacids
Inactive ingredients mightAdd volume to make the pill able to be handledAdd color and flavorAllow the tablet to be compressed and formed
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Let’s Practice: Not in Notes
Tin can (Sn)Example:Determine if
each is element,
compound, homogeneous
or heterogeneous
mixtures
Copper pipe (Cu)
Concrete
Carbon tetrachloride(CCl4)
Sports drink
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Let’s Practice
ElementTin Example:Determine if
each is element,
compound, homogeneous
or heterogeneous
mixtures
ElementCopper pipe
Heterogeneous mixConcrete
CompoundCarbon tetrachloride
Homogenous mixSports drink
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You Try! In Notes
Aluminum foil (Al)Example:Determine if
each is element,
compound, homogeneous
or heterogeneous
mixtures
Water (H2O)
soda
soil
Carbon dioxide(CO2)
Tap water
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You Try!
ElementAluminum foil (Al)Example:Determine if
each is element,
compound, homogeneous
or heterogeneous
mixtures
CompoundWater (H2O)
Homogeneous mixFlat soda
Heterogeneous mixsoil
compoundCarbon dioxide(CO2)
Tap water Homogeneous mix
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The Science of Macaroni Salad
http://www.freetech4teachers.com/2013/08/the-science-of-macaroni-salad.html#.UkySCODvSDo
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Section 2.2a—Naming Chemicals
We need to be able to name the chemicals in the antacids!
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Section 2.2a—Identifying Ions
We need to be able to name the chemicals in the antacids!
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The Language of Chemistry
Chemistry has a language all of its own
Each element symbol starts with a capital letter
EnglishChemistry
Element Symbols Letters
Chemical Formulas Words
Chemical Equations Sentences
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ELEMENTS: made of atoms
An atom consists of subatomic particlesThere are 3 subatomic particles: protons,
electrons and neutrons
Neutral atoms have the same number of protons and eletrons
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IONS
An atom or group of atoms with a charge.The number of protons does not equal the
number of electrons.
WHY? Atoms can gain or lose electrons to acquire stability like a noble gas element.
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The Periodic Table of Elements
Metals form cations NonMetals form anions
H He
Li Be B C N O F Ne
Na Mg Al Si P S Cl Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Lr Rf Db Sg Bh Hs Mt Uun Uuu Uub Uut
Metals Metalloids Non-metals
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Monatomic Ions (formed from a single atom)
CationsPositive chargeMetal atoms that lose electrons Group A (Representative metals/Type I ) The group # for metals in columns 1A, 2A, & 3A is equal to the charge of the cation
Naming them: Take the element name and add the word ion
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Monatomic Ions of Group A /Type I Metals
Group B
Group AGroup A
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Group B (Transition/Type II 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
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Monatomic Ions of Transition/Type II Metals
+
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Monatomic Ions (formed from a single atom) Cu+2, F-1
AnionsNegative 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 elementand add –ide and then ion
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You Try!
Try These: Write the formula for each ion and name it.
Calcium Chromium Chlorine Sulfur
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You Try!Try These: Write the formula for each ion and
name it. Calcium Ca+2 calcium ion
Chromium Cr+2 chromium(II) ion
Cr+3 chromium (III) ion
Chlorine Cl-1 chloride ion
Sulfur S-2 sulfide ion
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Self Check
Try These: Write the formula for each ion and name it.
Aluminum Zinc Iron Phosphorus
Al+3 Aluminum IonZn+2 Zinc ionFe+2 Iron (II) ion orFe+3 Iron (III) ionP-3 Phosphide ion
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Section 2.2b—Naming Ionic Compounds
We need to be able to name the chemicals in the antacids!
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Binary Ionic Compounds
Binary Ionic Compound- compound containing 2 elements—one metal and one non-metal
+Cation
+Cation
-Anion
-Anion Ionic Compound
Metal Nonmetal
The atoms are held together by Ionic Bonds- bond formed by attraction between + ions and – ions
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Metals & Non-Metals
Ionic Bonds are between metals & non-metalsH He
Li Be B C N O F Ne
Na Mg Al Si P S Cl Ar
K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe
Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Lr Rf Db Sg Bh Hs Mt Uun Uuu Uub Uut
Metals Metalloids Non-metals
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Look for:2 elements (“binary”)A type I metal & a non-metal (“ionic”)
To name these compounds:Write the name of the type 1 metal (the cation)Write the name of the non-metal (the anion) with
the suffix “-ide”
How to Identify & Name a Binary Ionic Compound
The subscripts in the formula do not matter when naming this type
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Example #1
NaCl
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NaCl
Cation
Anion
“Sodium”
“Chlorine” becomes “Chloride”
Sodium Chloride
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Example #2
CaBr2
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Cation
Anion
“Calcium”
“Bromine” becomes “Bromide”
CaBr2
Calcium Bromide
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Example #3
K2O
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K2O
Cation
Anion
“Potassium”
“Oxygen” becomes “Oxide”
Potassium Oxide
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Self Check
Example:Write the name for the following
compounds
Li2O
Sr3P2
MgS
BaI2
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Answers
Lithium oxide
Strontium phosphide
Magnesium sulfide
Barium iodide
Example:Write the name for the following
compounds
Li2O
Sr3P2
MgS
BaI2
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Ternary Ionic Compounds
+Cation
+Cation
Ternary Ionic Compound- a compound containing at least one polyatomic ion
- PolyatomicAnion
Ternary IonicCompound+
PolyatomicCation
-Anion
Polyatomic Ion- an ion that has more than one atom that together have a single charge
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Common Polyatomic Ions
COMMON POLYATOMIC IONS
Acetate, CH3COO-1 or C2H3O2-1
Ammonium NH4+1
Bromate, BrO3-1
Bromite, BrO2-1
Carbonate, CO3-2
Carbonite, CO2-2
Chlorate, ClO3-1
Chlorite, ClO2-1
Chromate, CrO4-2
Cyanide, CN-1
Dichromate, Cr2O7-2
Dihydrogen phosphate, H2PO4-1
Hydrogen carbonate or bicarbonate, HCO3
-1
Hydrogen phosphate or biphosphate, HPO4
-2
Hydrogen sulfate or bisulfate, HSO4-1
Hydroxide, OH-1
Hypochlorite, ClO-1
Iodate, IO3-1
Iodite, IO2-1
Nitrate, NO3-1
Nitrite, NO2-1
Oxalate, C2O4-2
Perchlorate, ClO4-1
Permanganate, MnO4
-1
Peroxide, O2-2
Phosphate, PO4-3
Phosphite, PO3-3
Silicate, SiO3-1
Sulfate, SO4-2
Sulfite, SO3-2
You don’t need to memorize them. Look at your reference sheet.
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The only cation (front-half) polyatomic ion is “NH4
+”
All other polyatomic ions are anions (back-half)
The subscripts within the polyatomic ion are important (it must match exactly with the one on your ion list)
If there are parentheses, the polyatomic ion is inside (ignore the number outside)
Identifying Polyatomic Ions: Hints
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Practice Identifying Polyatomic Ions
Example:Underline& name the
polyatomic ion in each
compound
NaNO3
NH4Cl
Ca(OH)2
(NH4)3PO4
K2CO3
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Practice Identifying Polyatomic Ions
Example:Identify and name the
polyatomic ion in each
compound
NaNO3
NH4Cl
Ca(OH)2
(NH4)3PO4
K2CO3
Nitrate
Ammonium
Hydroxide
Ammonium & phosphate
Carbonate
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Look for:More than 2 capital letters next to one another
(not starting with H)Contain at least 1 metal & 1 non-metal
To name these compounds:Write the name of the cation (either the metal
element name or “Ammonium” for “NH4+”)
If the anion is a polyatomic ion, write the given polyatomic ion’s name
If the anion is a single non-metal element, write its name with the suffix “-ide”
How to Identify & Name Ternary Ionic Compounds
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Ca(NO3)2
Example # 4
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Ca(NO3)2
Cation
PolyatomicAnion
“Calcium”
“Nitrate”
Calcium Nitrate
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Example #5
Na3PO4
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Cation
PolyatomicAnion
“Sodium”
“phosphate”
Na3PO4
Sodium phosphate
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Example # 6
K2CO3
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K2CO3
Cation
PolyatomicAnion
“potassium”
“carbonate”
Potassium carbonate
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Self Check
Example:Write the name for the following
compounds
Ca(C2H3O2)2
Li2SO3
Ba(OH)2
(NH4)2S
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Answers
Calcium acetate
Lithium sulfite
Barium hydroxide
Ammonium Sulfide
Example:Write the name for the following
compounds
Ca(C2H3O2)2
Li2SO3
Ba(OH)2
(NH4)2S
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Worksheet 1 (1-10 Answers)
1. Sodium sulfide
2. Aluminum oxide
3. Sodium chloride
4. Rubidium iodide
5. Zinc bromide
6. Silver chloride
7. Boron nitride
8. Barium fluoride
9. Strontium nitride
10. Magnesium chloride
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Worksheet 2 (1-10 Answers)
1. copper(I) fluoride
2. copper (II) fluoride
3. chromium (III) oxide
4. lead (II) iodide
5. lead (IV) chloride
6.chromium (VI) oxide
7. gold(I) bromide
8. nickel(II) oxide
9. vanadium(III) iodide
10. tin(IV) oxide
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Worksheet 3 (1-10 Answers)
1. vanadium(V) chlorate
2. rhenium(VI) sulfate3. osmium(III) iodate
4. iridium(IV) phosphate
5. palladium(IV) sulfite
Gold(I) nitrate
7. iron(III) phosphite
8. nickel(II) bromate
9. lead(IV) sulfide
10. Manganese (VII) dichromate
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Worksheet 4 (1-10 Answers)
1. ammonium chloride
2. hydrogen chlorite
3. calcium bromate
4. beryllium sulfate
5. ammonium nitride
6. ammonium nitrate
7. strontium phosphate
8. zinc chlorate
9. silver iodate
10. potassium dichromate
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Transition Metals Revisisted
Transition Metal- group “B” or Type II metal that has the possibility of having more than one cation charge;
IMPORTANT:
Although group B metals, SILVER (+1), CADMIUM (+2), and ZINC (+2) only have 1 charge
Although the elements of TIN and LEAD are group A elements, they do have more than one charge
Sn(+2 and +4) and Pb(+2 and +4)
Common multivalent metals and their charges
Cobalt Co+2 Co+3
Copper Cu+1 Cu+2
Iron Fe+2 Fe+3
Manganese Mn+2 Mn+3
Mercury Hg2+2 Hg+2
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Look for:One of the transition metals, excluding Ag, Cd, and Zn
To name these compounds:Write the name of the Type II metal element (cation)Write the name of the anion (element name with “-ide” or
polyatomic ion name)Determine the charge of the transition metal
1. Total negative charge = total positive charge for all neutral compounds
2. Divide total positive charge by the number of metal atoms
3. Write the charge in roman numerals in parentheses after the Type II metal’s name
How to Identify & Name Ionic Compounds with Transition Metals
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Example # 7
CuCl
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CuCl
Cation
Anion
“Copper”
“Chlorine” becomes “Chloride”
Copper Chloride
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CuCl
Cation
Anion
“Copper”
“Chlorine” becomes “Chloride”
Copper Chloride
Chloride has a –1 charge
-1 charge * 1 ion = -1
A –1 charge needs a +1 charge
Therefore, copper must be +1, (I)
(I)
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Example # 8
Fe2(CO3)3
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Fe2(CO3)3
Cation
Polyatomic Anion
“Iron”
“Carbonate”
Iron carbonate
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Fe2(CO3)3
Cation
Polyatomic Anion
“Iron”
“Carbonate”
Iron carbonate
Carbonate has a –2 charge
-2 charge * 3 ions = -6
A –6 charge needs a +6 charge and there are 2 iron ions
Therefore, iron must be +3 (III)
(III)
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Example # 9
ZnBr2
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ZnBr2
Cation
monatomic Anion
“Zinc”
“bromide”
Zinc bromide
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ZnBr2
Cation
Polyatomic Anion
“Zinc”
“bromide”
Zinc bromide
bromide has a –1 charge
-1 charge * 2 ions = -2
A –2 charge needs a +2 charge and there is 1 zinc ion
Therefore, zinc must be +2 (notneeded) it only has one charge
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Self Check
Example:Write the name for the following
compounds
PbCl2
PbCl4
MnO
Mn2O3
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Answers
Lead (II) chloride
Lead (IV) chloride
Manganese (II) oxide
Manganese (III) oxide
Example:Write the name for the following
compounds
PbCl2
PbCl4
MnO
Mn2O3
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Section 2.2b—Naming Covalent Compounds
We need to be able to name the chemicals in the antacids!
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Binary Covalent (Molecular) Compounds
Nonmetal
Nonmetal
Nonmetal
Nonmetal Covalent compound
Binary Molecular Compounds are made from two non-metals that are covalently bonded Covalent bond a bond formed from atoms that share electrons
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These compounds have:2 elements (“binary”)Both non-metals (“covalent”)
To name these compounds:Write the name of the first element with the
prefix indicating the number of atoms (except don’t use “mono-” if only 1 atom)
Write the name of the second element with the prefix indicating the number of atoms (including “mono-”) and the suffix “ide”
Identifying & Naming Binary Molecular
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Covalent PrefixesPREFIXES USED IN MOLECULAR COMPOUNDS
1.mono2.di-3.tri-4.tetra-5.penta-6.hexa-7.hepta-8.octa-9.nona-10.deca-
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Example #10
P2O5
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P2O5
Phosphorus
Oxygen
2 = “di-”
5 = “penta-” “oxide”
Diphosphorus pentaoxide
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Example #11
SiF4
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Silicon
Fluorine
Don’t use “mono-” on first element
4 = “tetra-” “fluoride”
SiF4
Silicon tetrafluoride
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Self Check
Example:Write the name for the following
compounds
SO2
N2Cl4
P4O10
CO
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Answers
sulfur dioxide
Dinitrogen tetrachloride
Tetraphosphorus decaoxide
Carbon monoxide
Example:Write the name for the following
compounds
SO2
N2Cl4
P4O10
CO
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Mixed Practice: Determine the type of compound, Ionic (m/nm) or Covalent (nm/nm) & then follow rules
Example:Write the name for the following
compounds
Na2O
K3PO4
Cu(OH)2
N2S
MgCl2
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Answers
Sodium oxide
Potassium phosphate
Copper (II) hydroxide
Dinitrogen monosulfide
Magnesium chloride
Example:Write the name for the following
compounds
Na2O
K3PO4
Cu(OH)2
N2S
MgCl2
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Section 2.3—Writing Chemical Formulas For Ionic & Covalent
Compounds
We need to be able to read the formulas for chemicals in the antacids!
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Your Reference sheet has a list of:Common polyatomic ions
Use your periodic table is used to determine the charges of common elements when they form ions
You must memorize the 10 prefixes for covalent compounds
Reminders from Section 2.2
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Binary Ionic Compounds
containing two elements—one metal and one non-metal
formed by attraction between + and - ions
+Cation
+Cation
-Anion
-Anion Ionic Compound
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These compounds:End in “-ide” (except “hydroxide and cyanide”)Do NOT contain covalent prefixes
To write these formulas:Write the symbol & charge of the first element (the metal,
cation)Write the symbol & charge of the second element (the
non-metal, anion)Add more of the cations and/or anions to have a neutral
compoundUse subscripts to show how many of each type of ion is
there.
How to Write Formulas for Binary Ionic Compounds
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Example #1
Sodium chloride
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Sodium chloride
Cation
Anion
Na+1
Cl-1
NaCl
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Example #1
Sodium chloride
Cation
Anion
Na+1
Cl-1
NaCl
Na+1Cl-1
+1 + -1 = 0The compound is neutral…no subscripts are needed.
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Example #2
Calcium bromide
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Example #2
Calcium bromide
Cation
Anion
Ca+2
Br-1
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Example #2
Calcium bromide
Cation
Anion
Ca+2
Br-1
CaBr2
Ca+2 Br-1
+2 + -1 = +1
Ca+2 Br-1 Br-1
The subscript “2” is used to show that 2 anions are needed.
+2 + -1 + -1 = 0
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The Criss - Cross Method:Write the symbol & charge of the first element (the metal,
cation)Write the symbol & charge of the second element (the
non-metal, anion)
Cross ONLY the charge numbers down diagonally to
make subscripts IF they are not equal to each otherSimplify subscripts if you can
Ca +2 Br-1 Ca1Br2 CaBr2
1 2
A Simple Method to Writing Binary Ionic Formulas
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Self Check
Example:Write the following chemical formulas
Cesium chloride
Potassium oxide
Calcium sulfide
Lithium nitride
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Answers
CsCl
K2O
CaS
Li3N
Example:Write the following chemical formulas
Cesium chloride
Potassium oxide
Calcium sulfide
Lithium nitride
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Ternary Ionic Compounds
+Cation
+Cation
compound containing at least one polyatomic ion
Either in the front, the back or in both places
-Polyatomic
Anion
Polyatomic IonicCompound
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These compounds:Do not end with “-ide” (except hydroxide & cyanide)Do not use covalent prefixes
To write these formulas:Write the symbol & charge of the cation & anionAdd additional cations or anions to have a neutral compoundUse subscripts to show the number of ions
When using subscripts with a polyatomic ion, you must put the polyatomic ion in a parenthesis with the subscript on the outside
How to Identify & Name Ternary Ionic Compounds
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Example #3
Sodium carbonate
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Sodium carbonate
Cation
PolyatomicAnion
Na+1
CO3-2
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Sodium carbonate
Cation
PolyatomicAnion
Na+1
CO3-2
Na2CO3
Na1+ CO32-
+1 + -2 = -1
Na+ Na+ CO32-
The subscript “2” is used to show that 2 cations are needed.
+1 + 1 + -2 = 0
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Example #4
Magnesium nitrate
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Magnesium nitrate
Cation
PolyatomicAnion
Mg+2
NO3-1
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Magnesium nitrate
Cation
PolyatomicAnion
Mg+2
NO3-1
Mg(NO3)2 Use parenthesis when adding subscripts to polyatomic ions
Mg+2NO31-
+2 + -1 = 1
Mg+2 NO3- NO3
-
The subscript “2” is used to show that 2 anions are needed.
+2 + -1 + -1 = 0
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Self Check
Example:Write the following chemical formulas
Sodium nitrate
Calcium chlorate
Potassium sulfite
Calcium hydroxide
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Answers
NaNO3
Ca(ClO3)2
K2SO3
Ca(OH)2
Example:Write the following chemical formulas
Sodium nitrate
Calcium chlorate
Potassium sulfite
Calcium hydroxide
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Transition Metals
metal that has more than one possibility for cationic charge
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These compounds:Will have roman numerals
To write these formulas:Same as binary ionic or polyatomic ionic.The roman numerals tell the charge of the
metal (cation)
How to Identify & Name Ionic Compounds with Transition Metals
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Example #5
Iron (III) oxide
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Iron (III) oxide
Cation
Anion
Fe+3
O-2
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Iron (III) oxide
Cation
Anion
Fe+3
O-2
Fe2O3
Fe+3 O2-
+3 + -2 = -1
Fe+3 Fe+3 O2- O2-
The subscript “2” and “3” are used to show the numbers of atoms needed.
+3 + 3 + -2 + -2 + -2 = 0
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Example #6
Copper (II) nitrate
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Copper (II) nitrate
Cation
PolyatomicAnion
Cu+2
NO3-1
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Copper (II) nitrate
Cation
PolyatomicAnion
Cu+2
NO3-1
Cu(NO3)2
Cu+2 NO31-
+2 + -1 = 1
Cu+2 NO3- NO3
-
Use parenthesis when adding subscripts to a polyatomic ion
+2 + -1 + -1 = 0
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Self Check
Example:Write the following chemical formulas
Iron (II) nitrate
Copper (I) chloride
Lead (IV) hydroxide
Tin (II) oxide
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Answers
Fe(NO3)2
CuCl
Pb(OH)4
SnO
Example:Write the following chemical formulas
Iron (II) nitrate
Copper (I) chloride
Lead (IV) hydroxide
Tin (II) oxide
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Binary Covalent Compounds
compound made from two non-metals
between atoms that share electrons
Nonmetal
Nonmetal
Nonmetal
Nonmetal Covalent compound
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These compounds:Use covalent prefixes
To write these formulas:Write the symbols of the first and second
elementUse the covalent prefixes (assume the first
element is “1” if there’s no prefix) as the subscripts to show number of atoms.
How to Identify & Name Binary Covalent Compounds
Atoms do not form charges when bonding covalently…you DO NOT need to worry about charges with this type! NOR CRISS CROSS METHOD!
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Example #7
Dinitrogen Tetraoxide
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Dinitrogen Tetraoxide
N
O
“Di-” = 2
“Tetra-” = 4
N2O4
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Example #8
Silicon dioxide
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Silicon dioxide
Si
O
“Mono-” is not written for the first element
“Di-” = 2
SiO2
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CAUTION!!!
bi-di-
Stands for “2” in covalent compounds
Means there’s a hydrogen in the polyatomic anion
“di” and “bi” do not mean the same thing!
Carbon dioxide = CO2
Sodium biphosphate = Na2HPO4
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Self Check
Example:Write the following chemical formulas
Carbon monoxide
Sulfur tetraiodide
Trichlorine pentasulfide
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Answers
CO
SI4
Cl3S5
Example:Write the following chemical formulas
Carbon monoxide
Sulfur tetraiodide
Trichlorine pentasulfide
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Self Check: Mixed Practice
Example:Write the following chemical formulas
Magnesium hydroxide
Copper (II) nitrate
Iron (III) oxide
Nitrogen dioxide
Sodium bicarbonate
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Answers
Mg(OH)2
Cu(NO3)2
Fe2O3
NO2
NaHCO3
Example:Write the following chemical formulas
Magnesium hydroxide
Copper (II) nitrate
Iron (III) oxide
Nitrogen dioxide
Sodium bicarbonate