Chapter 2A: Antacids. Why do we need antacids? Your body needs hydrochloric acid to digest food Too...

Chapter 2A: Antacids

Why do we need antacids?

Your body needs hydrochloric acid to digest food

Too much causes heartburn, ulcers and can damage your esophagus

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?

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

Section 2.1—Types of Matter

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

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

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

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

Elements

http://www.youtube.com/watch?v=7FesjAdIWBk

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

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

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

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

Homogeneous MixturesBrass: copper in zinc

Air: oxygen gas in nitrogen gas

Kool-Aid: sugar in water

Milk: fat, proteins, sugar in water

Heterogeneous MixturesOil in waterItalian Salad Dressing

Chicken Noodle Soup Fruit Salad

Classification of Matter

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

True Solutions

Suspensions

vinegar and oil salad dressing

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

Connect these concepts with Antacids

What type of matter do you think antacids are?Pure substance (Element or compound)Mixture (homogeneous or heterogeneous)


Antacids are mixtures.They contain active & inactive ingredientsWhat purposes could the inactive

ingredients serve?


Inactive ingredients mightAdd volume to make the pill able to be handledAdd color and flavorAllow the tablet to be compressed and formed

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

Let’s Practice

ElementTin Example:Determine if

each is element,


or heterogeneous

mixtures

ElementCopper pipe

Heterogeneous mixConcrete

CompoundCarbon tetrachloride

Homogenous mixSports drink

You Try! In Notes

Aluminum foil (Al)Example:Determine if

each is element,


or heterogeneous

mixtures

Water (H2O)

soda

soil

Carbon dioxide(CO2)

Tap water

You Try!

ElementAluminum foil (Al)Example:Determine if

each is element,


or heterogeneous

mixtures

CompoundWater (H2O)

Homogeneous mixFlat soda

Heterogeneous mixsoil

compoundCarbon dioxide(CO2)

Tap water Homogeneous mix

The Science of Macaroni Salad

http://www.freetech4teachers.com/2013/08/the-science-of-macaroni-salad.html#.UkySCODvSDo

Section 2.2a—Naming Chemicals

We need to be able to name the chemicals in the antacids!

Section 2.2a—Identifying Ions


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

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

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.

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

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

Monatomic Ions of Group A /Type I Metals

Group B

Group AGroup A

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

Monatomic Ions of Transition/Type II Metals

+

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

You Try!

Try These: Write the formula for each ion and name it.

Calcium Chromium Chlorine Sulfur

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

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

Section 2.2b—Naming Ionic Compounds


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

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

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

Example #1

NaCl

NaCl

Cation

Anion

“Sodium”

“Chlorine” becomes “Chloride”

Sodium Chloride

Example #2

CaBr2

Cation

Anion

“Calcium”

“Bromine” becomes “Bromide”

CaBr2

Calcium Bromide

Example #3

K2O

K2O

Cation

Anion

“Potassium”

“Oxygen” becomes “Oxide”

Potassium Oxide

Self Check

Example:Write the name for the following

compounds

Li2O

Sr3P2

MgS

BaI2

Answers

Lithium oxide

Strontium phosphide

Magnesium sulfide

Barium iodide


compounds

Li2O

Sr3P2

MgS

BaI2

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

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.

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

Practice Identifying Polyatomic Ions

Example:Underline& name the

polyatomic ion in each

compound

NaNO3

NH4Cl

Ca(OH)2

(NH4)3PO4

K2CO3

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

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

Ca(NO3)2

Example # 4

Ca(NO3)2

Cation

PolyatomicAnion

“Calcium”

“Nitrate”

Calcium Nitrate

Example #5

Na3PO4

Cation

PolyatomicAnion

“Sodium”

“phosphate”

Na3PO4

Sodium phosphate

Example # 6

K2CO3

K2CO3

Cation

PolyatomicAnion

“potassium”

“carbonate”

Potassium carbonate

Self Check


compounds

Ca(C2H3O2)2

Li2SO3

Ba(OH)2

(NH4)2S

Answers

Calcium acetate

Lithium sulfite

Barium hydroxide

Ammonium Sulfide


compounds

Ca(C2H3O2)2

Li2SO3

Ba(OH)2

(NH4)2S

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


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


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


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

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

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

Example # 7

CuCl

CuCl

Cation

Anion

“Copper”


Copper Chloride

CuCl

Cation

Anion

“Copper”


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)

Example # 8

Fe2(CO3)3

Fe2(CO3)3

Cation

Polyatomic Anion

“Iron”

“Carbonate”

Iron carbonate

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)

Example # 9

ZnBr2

ZnBr2

Cation

monatomic Anion

“Zinc”

“bromide”

Zinc bromide

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

Self Check


compounds

PbCl2

PbCl4

MnO

Mn2O3

Answers

Lead (II) chloride

Lead (IV) chloride

Manganese (II) oxide

Manganese (III) oxide


compounds

PbCl2

PbCl4

MnO

Mn2O3

Section 2.2b—Naming Covalent Compounds


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

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

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-

Example #10

P2O5

P2O5

Phosphorus

Oxygen

2 = “di-”

5 = “penta-” “oxide”

Diphosphorus pentaoxide

Example #11

SiF4

Silicon

Fluorine

Don’t use “mono-” on first element

4 = “tetra-” “fluoride”

SiF4

Silicon tetrafluoride

Self Check


compounds

SO2

N2Cl4

P4O10

CO

Answers

sulfur dioxide

Dinitrogen tetrachloride

Tetraphosphorus decaoxide

Carbon monoxide


compounds

SO2

N2Cl4

P4O10

CO

Mixed Practice: Determine the type of compound, Ionic (m/nm) or Covalent (nm/nm) & then follow rules


compounds

Na2O

K3PO4

Cu(OH)2

N2S

MgCl2

Answers

Sodium oxide

Potassium phosphate

Copper (II) hydroxide

Dinitrogen monosulfide

Magnesium chloride


compounds

Na2O

K3PO4

Cu(OH)2

N2S

MgCl2

Section 2.3—Writing Chemical Formulas For Ionic & Covalent

Compounds

We need to be able to read the formulas for chemicals in the antacids!

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

Binary Ionic Compounds

containing two elements—one metal and one non-metal

formed by attraction between + and - ions

+Cation

+Cation

-Anion

-Anion Ionic Compound

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

Example #1

Sodium chloride

Sodium chloride

Cation

Anion

Na+1

Cl-1

NaCl

Example #1

Sodium chloride

Cation

Anion

Na+1

Cl-1

NaCl

Na+1Cl-1

+1 + -1 = 0The compound is neutral…no subscripts are needed.

Example #2

Calcium bromide

Example #2

Calcium bromide

Cation

Anion

Ca+2

Br-1

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

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

Self Check

Example:Write the following chemical formulas

Cesium chloride

Potassium oxide

Calcium sulfide

Lithium nitride

Answers

CsCl

K2O

CaS

Li3N


Cesium chloride

Potassium oxide

Calcium sulfide

Lithium nitride

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

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

Example #3

Sodium carbonate

Sodium carbonate

Cation

PolyatomicAnion

Na+1

CO3-2

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

Example #4

Magnesium nitrate

Magnesium nitrate

Cation

PolyatomicAnion

Mg+2

NO3-1

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

Self Check


Sodium nitrate

Calcium chlorate

Potassium sulfite

Calcium hydroxide

Answers

NaNO3

Ca(ClO3)2

K2SO3

Ca(OH)2


Sodium nitrate

Calcium chlorate

Potassium sulfite

Calcium hydroxide

Transition Metals

metal that has more than one possibility for cationic charge

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

Example #5

Iron (III) oxide

Iron (III) oxide

Cation

Anion

Fe+3

O-2

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

Example #6

Copper (II) nitrate

Copper (II) nitrate

Cation

PolyatomicAnion

Cu+2

NO3-1

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

Self Check


Iron (II) nitrate

Copper (I) chloride

Lead (IV) hydroxide

Tin (II) oxide

Answers

Fe(NO3)2

CuCl

Pb(OH)4

SnO


Iron (II) nitrate

Copper (I) chloride

Lead (IV) hydroxide

Tin (II) oxide

Binary Covalent Compounds

compound made from two non-metals

between atoms that share electrons

Nonmetal

Nonmetal

Nonmetal

Nonmetal Covalent compound

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!

Example #7

Dinitrogen Tetraoxide

Dinitrogen Tetraoxide

N

O

“Di-” = 2

“Tetra-” = 4

N2O4

Example #8

Silicon dioxide

Silicon dioxide

Si

O

“Mono-” is not written for the first element

“Di-” = 2

SiO2

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

Self Check


Carbon monoxide

Sulfur tetraiodide

Trichlorine pentasulfide

Answers

CO

SI4

Cl3S5


Carbon monoxide

Sulfur tetraiodide

Trichlorine pentasulfide

Self Check: Mixed Practice


Magnesium hydroxide

Copper (II) nitrate

Iron (III) oxide

Nitrogen dioxide

Sodium bicarbonate

Answers

Mg(OH)2

Cu(NO3)2

Fe2O3

NO2

NaHCO3


Magnesium hydroxide

Copper (II) nitrate

Iron (III) oxide

Nitrogen dioxide

Sodium bicarbonate

Chapter 2A: Antacids. Why do we need antacids? Your body needs hydrochloric acid to digest food Too...

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