Chapter 2: Antacids

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Chapter 2 Antacids
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Antacids

• This chapter will introduce the chemistry needed
  to understand how antacids work
• Section 2.1 Types of Matter
• Section 2.2 Naming Chemicals
• Section 2.3 Writing Formulas
• Section 2.4 Acids Bases
• Section 2.5 Chemical Reactions
• Section 2.6 Balancing Chemical Equations
• Section 2.7 Speeding up Chemical Reactions

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IntroAntacids
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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
There are two types of medicines you can use
Acid Inhibitors
Antacids
Neutralizes the acid currently in your system
Controls the amount of acid your body produces
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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Section 2.1Types of Matter
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Matter is.

• Anything that has mass and takes up space
  (volume)
• Anything made from atoms
• Examples elements, molecules, cells, people,
  air, water, paper
• Non Examples dreams, energy (light, heat),
  emotions

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Pure Substances versus Mixtures
Matter is classified as either a pure substance
or a mixture
Mixtures
Pure Substances
Contain only 1 type of particle Elements or
Compounds
Contain 2 or more pure substances Homogeneous or
Heterogeneous
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Pure Substances
Compound
Elements
2 or more elements chemically bonded together to
form molecules. Each is the same fixed ratio of
elements. H2O, NaCl, CO2
Simplest kind of matter Made of only 1 kind of
atom Cu, Ag, Fe, Br2
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Elements
Single Atom
Cannot be separated by chemical or physical
processes
Element
Pure substance Every atom is the same Elements
can be found on the periodic table!
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Elements
http//www.youtube.com/watch?v7FesjAdIWBk
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Compounds
Single Molecule



Made of more than one type of atom bonded together
Compound
Pure substance Every molecule is the same
Can only be separated by chemical reactions
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Mixtures
More than 1 different type of matter

• Can be separated physically by
• Distillation
• Filtration
• Chromatography

Mixture
Not a pure substance Physical combination of more
than 1 type of pure substance
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Mixtures
Mixtures can be classified as homogeneous or
heterogeneous
Heterogeneous
Homogeneous (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
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Mixture possibilities

• Mixtures can be any combination of solids,
  liquids and gases
• Solid-solid Medicine tablet
• Solid-gas Pop Rocks candy
• Solid-liquid Ice water
• Liquid-liquid lemon water
• Gas-Liquid Carbonated water
• Gas-Gas Air

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Homogeneous Mixtures
Kool-Aid sugar in water
Brass copper in zinc
Air oxygen gas in nitrogen gas
Milk fat, proteins, sugar in water
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Heterogeneous Mixtures
Oil in water
Italian Salad Dressing
Fruit Salad
Chicken Noodle Soup
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Classification of Matter
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True Solutions, Colloids Suspensions
Homogeneous Heterogeneous
Heterogeneous
Colloid
True Solution
Suspension
SMALL particles dont settle out and are too
small to scatter light Ex salt water, air, brass
INTERMEDIATE particles dont settle out but are
large enough to scatter light Ex fog, foam,
jello, paint
LARGE particles that settle out over time Ex
oral medicines, italian dressing, paint
Dissolved Particle Size Increases
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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

Solution Light passes through unchanged
Colloids exhibit the Tyndall Effect Light 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 ingredients
• What purposes could the inactive ingredients
  serve?

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Connect these concepts with Antacids

• Inactive ingredients might
• Add volume to make the pill able to be handled
• Add color and flavor
• Allow the tablet to be compressed and formed

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Lets Practice Not in Notes
Example Determine if each is element, compound,
homogeneous or heterogeneous mixtures
Tin can (Sn)
Copper pipe (Cu)
Concrete
Carbon tetrachloride(CCl4)
Sports drink
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Lets Practice
Example Determine if each is element, compound,
homogeneous or heterogeneous mixtures
Element
Tin
Copper pipe
Element
Heterogeneous mix
Concrete
Compound
Carbon tetrachloride
Homogenous mix
Sports drink
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You Try! In Notes
Example Determine if each is element, compound,
homogeneous or heterogeneous mixtures
Aluminum foil (Al)
Water (H2O)
soda
soil
Carbon dioxide(CO2)
Tap water
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You Try!
Example Determine if each is element, compound,
homogeneous or heterogeneous mixtures
Element
Aluminum foil (Al)
Compound
Water (H2O)
Homogeneous mix
Flat soda
Heterogeneous mix
soil
Carbon dioxide(CO2)
compound
Tap water
Homogeneous mix
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The Science of Macaroni Salad

• http//www.freetech4teachers.com/2013/08/the-scien
  ce-of-macaroni-salad.html.UkySCODvSDo

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Section 2.2Naming Chemicals
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
English
Chemistry
Element Symbols
Letters
Chemical Formulas
Words
Chemical Equations
Sentences
Each element symbol starts with a capital letter
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ELEMENTS made of atoms

• An atom consists of subatomic particles
• There 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 Metals Metalloids Metalloids Non-metals Non-metals
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Monatomic Ions (formed from a single atom)
  Cations Positive charge Metal 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 A
Group A
Group B
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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. Fe2
Fe3 Sn2 Sn4 Pb2 Pb4 Co2
Co3 Cr2 Cr3 Mn2 Mn3 Cu1
Cu2
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) Cu2,
F-1   Anions Negative charge Nonmetals
that gain electrons   Group A (Representative
nonmetals) Subtract the group in columns 4A,
5A, 6A, and 7A from 8 to get the charge. Naming
them Drop the ending of the element and add ide
and then ion
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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 Ca2 calcium ion
• Chromium Cr2 chromium(II) ion
• Cr3 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

Al3 Aluminum Ion Zn2 Zinc ion Fe2 Iron (II)
ion or Fe3 Iron (III) ion P-3 Phosphide ion
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Binary Ionic Compounds
Binary Ionic Compound- compound containing 2
elementsone metal and one non-metal
The atoms are held together by Ionic Bonds- bond
formed by attraction between ions and ions
Metal Nonmetal
Cation
- Anion
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Metals Non-Metals
Ionic Bonds are between metals non-metals
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 Metals Metalloids Metalloids Non-metals Non-metals
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How to Identify Name a Binary Ionic Compound

• 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

The subscripts in the formula do not matter when
naming this type
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Example 1
NaCl
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Sodium
Cation
NaCl
Anion
Chlorine becomes Chloride
Sodium Chloride
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Example 2
CaBr2
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Calcium
Cation
CaBr2
Anion
Bromine becomes Bromide
Calcium Bromide
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Example 3
K2O
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Potassium
Cation
K2O
Anion
Oxygen becomes Oxide
Potassium Oxide
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Self Check
Li2O Sr3P2 MgS BaI2
Example Write the name for the following
compounds
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Answers
Lithium oxide Strontium phosphide Magnesium
sulfide Barium iodide
Li2O Sr3P2 MgS BaI2
Example Write the name for the following
compounds
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Ternary Ionic Compounds
Ternary Ionic Compound- a compound containing at
least one polyatomic ion
Polyatomic Ion- an ion that has more than one
atom that together have a single charge
Cation
- Anion
Polyatomic Cation
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Common Polyatomic Ions
You dont need to memorize them. Look at your
reference sheet.
COMMON POLYATOMIC IONS COMMON POLYATOMIC IONS
Acetate, CH3COO-1 or C2H3O2-1 Ammonium NH41 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
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Identifying Polyatomic Ions Hints

• 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)

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Practice Identifying Polyatomic Ions
NaNO3 NH4Cl Ca(OH)2 (NH4)3PO4 K2CO3
Example Underline name the polyatomic ion in
each compound
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Practice Identifying Polyatomic Ions
NaNO3 NH4Cl Ca(OH)2 (NH4)3PO4 K2CO3
Nitrate Ammonium Hydroxide Ammonium
phosphate Carbonate
Example Identify and name the polyatomic ion in
each compound
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How to Identify Name Ternary Ionic Compounds

• 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 ions name
• If the anion is a single non-metal element, write
  its name with the suffix -ide

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Example 4
Ca(NO3)2
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Calcium
Cation
Ca(NO3)2
Polyatomic Anion
Nitrate
Calcium Nitrate
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Example 5
Na3PO4
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Sodium
Cation
Na3PO4
Polyatomic Anion
phosphate
Sodium phosphate
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Example 6
K2CO3
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potassium
Cation
K2CO3
Polyatomic Anion
carbonate
Potassium carbonate
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Self Check
Ca(C2H3O2)2 Li2SO3 Ba(OH)2 (NH4)2S
Example Write the name for the following
compounds
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Answers
Calcium acetate Lithium sulfite Barium
hydroxide Ammonium Sulfide
Ca(C2H3O2)2 Li2SO3 Ba(OH)2 (NH4)2S
Example Write the name for the following
compounds
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Worksheet 1 (1-10 Answers)
6. Silver chloride

• 1. Sodium sulfide

2. Aluminum oxide
7. Boron nitride
8. Barium fluoride

• 3. Sodium chloride

4. Rubidium iodide
9. Strontium nitride
5. Zinc bromide
10. Magnesium chloride
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Worksheet 2 (1-10 Answers)
6.chromium (VI) oxide

• 1. copper(I) fluoride

2. copper (II) fluoride
7. gold(I) bromide
8. nickel(II) oxide

• 3. chromium (III) oxide

9. vanadium(III) iodide
4. lead (II) iodide
10. tin(IV) oxide
5. lead (IV) chloride
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Worksheet 3 (1-10 Answers)
Gold(I) nitrate

• 1. vanadium(V) chlorate

7. iron(III) phosphite
2. rhenium(VI) sulfate
8. nickel(II) bromate
9. lead(IV) sulfide

• 3. osmium(III) iodate

10. Manganese (VII) dichromate
4. iridium(IV) phosphate
5. palladium(IV) sulfite
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Worksheet 4 (1-10 Answers)
6. ammonium nitrate

• 1. ammonium chloride

2. hydrogen chlorite
7. strontium phosphate
8. zinc chlorate

• 3. calcium bromate

4. beryllium sulfate
9. silver iodate
10. potassium dichromate
5. ammonium nitride
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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
Common multivalent metals and their
charges Cobalt Co2 Co3 Copper
Cu1 Cu2 Iron Fe2
Fe3 Manganese Mn2 Mn3 Mercury
Hg22 Hg2

• 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)

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How to Identify Name Ionic Compounds with
Transition Metals

• 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 metals name

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Example 7
CuCl
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Copper
Cation
CuCl
Copper Chloride
Anion
Chlorine becomes Chloride
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Copper
Cation
Chloride has a 1 charge
CuCl
-1 charge 1 ion -1
A 1 charge needs a 1 charge
Anion
Chlorine becomes Chloride
Therefore, copper must be 1, (I)
(I)
Copper Chloride
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Example 8
Fe2(CO3)3
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Iron
Cation
Fe2(CO3)3
Iron carbonate
Polyatomic Anion
Carbonate
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Iron
Cation
Carbonate has a 2 charge
Fe2(CO3)3
-2 charge 3 ions -6
A 6 charge needs a 6 charge and there are 2
iron ions
Polyatomic Anion
Carbonate
Therefore, iron must be 3 (III)
(III)
Iron carbonate
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Example 9
ZnBr2
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Zinc
Cation
ZnBr2
Zinc bromide
monatomic Anion
bromide
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Zinc
Cation
bromide has a 1 charge
ZnBr2
-1 charge 2 ions -2
A 2 charge needs a 2 charge and there is 1 zinc
ion
Polyatomic Anion
bromide
Therefore, zinc must be 2 (not needed) it only
has one charge
Zinc bromide
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Self Check
PbCl2 PbCl4 MnO Mn2O3
Example Write the name for the following
compounds
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Answers
Lead (II) chloride Lead (IV) chloride Manganese
(II) oxide Manganese (III) oxide
PbCl2 PbCl4 MnO Mn2O3
Example Write the name for the following
compounds
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Binary Covalent (Molecular) Compounds
Binary Molecular Compounds are made from two
non-metals that are covalently bonded Covalent
bond a bond formed from atoms that share
electrons
Non metal
Non metal
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Identifying Naming Binary Molecular

• 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
  dont 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

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Covalent Prefixes
PREFIXES USED IN MOLECULAR COMPOUNDS mono di- tri- tetra- penta- hexa- hepta- octa- nona- deca-
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Example 10
P2O5
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2 di-
Phosphorus
P2O5
Oxygen
5 penta- oxide
Diphosphorus pentaoxide
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Example 11
SiF4
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Dont use mono- on first element
Silicon
SiF4
Fluorine
4 tetra- fluoride
Silicon tetrafluoride
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Self Check
SO2 N2Cl4 P4O10 CO
Example Write the name for the following
compounds
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Answers
SO2 N2Cl4 P4O10 CO
sulfur dioxide Dinitrogen tetrachloride Tetraphosp
horus decaoxide Carbon monoxide
Example Write the name for the following
compounds
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Mixed Practice Determine the type of compound,
Ionic (m/nm) or Covalent (nm/nm) then follow
rules
Na2O K3PO4 Cu(OH)2 N2S MgCl2
Example Write the name for the following
compounds
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Answers
Sodium oxide Potassium phosphate Copper (II)
hydroxide Dinitrogen monosulfide Magnesium
chloride
Na2O K3PO4 Cu(OH)2 N2S MgCl2
Example Write the name for the following
compounds
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Section 2.3Writing Chemical Formulas
We need to be able to read the formulas for
chemicals in the antacids!
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Reminders from Section 2.2

• 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

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Binary Ionic Compounds

• containing two elementsone metal and one
  non-metal
• formed by attraction between and - ions

Cation
- Anion
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How to Write Formulas for Binary Ionic Compounds

• 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 compound
• Use subscripts to show how many of each type of
  ion is there.

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Example 1
Sodium chloride
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Na1
Cation
Sodium chloride
Anion
Cl-1
NaCl
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Example 1
Na1
Cation
Na1Cl-1
Sodium chloride
1 -1 0
Anion
The compound is neutralno subscripts are needed.
Cl-1
NaCl
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Example 2
Calcium bromide
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Example 2
Ca2
Cation
Calcium bromide
Anion
Br-1
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Example 2
Ca2
Cation
Ca2 Br-1
Calcium bromide
2 -1 1
Anion
Ca2 Br-1 Br-1
Br-1
2 -1 -1 0
CaBr2
The subscript 2 is used to show that 2 anions
are needed.
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A Simple Method to Writing Binary Ionic Formulas

• 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
  other
• Simplify subscripts if you can
• Ca 2 Br-1 ? Ca1Br2 ?
  CaBr2
• 1 2

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Self Check
Cesium chloride Potassium oxide Calcium
sulfide Lithium nitride
Example Write the following chemical formulas
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Answers
CsCl K2O CaS Li3N
Cesium chloride Potassium oxide Calcium
sulfide Lithium nitride
Example Write the following chemical formulas
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Ternary Ionic Compounds

• compound containing at least one polyatomic ion
• Either in the front, the back or in both places

Cation
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How to Identify Name Ternary Ionic Compounds

• 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 anion
• Add additional cations or anions to have a
  neutral compound
• Use 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

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Example 3
Sodium carbonate
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Na1
Cation
Sodium carbonate
Polyatomic Anion
CO3-2
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Na1
Cation
Na1 CO32-
Sodium carbonate
1 -2 -1
Polyatomic Anion
Na Na CO32-
1 1 -2 0
CO3-2
Na2CO3
The subscript 2 is used to show that 2 cations
are needed.
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Example 4
Magnesium nitrate
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Mg2
Cation
Magnesium nitrate
Polyatomic Anion
NO3-1
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Mg2
Mg2NO31-
Cation
2 -1 1
Magnesium nitrate
Mg2 NO3- NO3-
Polyatomic Anion
2 -1 -1 0
NO3-1
The subscript 2 is used to show that 2 anions
are needed.
Mg(NO3)2
Use parenthesis when adding subscripts to
polyatomic ions
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Self Check
Sodium nitrate Calcium chlorate Potassium
sulfite Calcium hydroxide
Example Write the following chemical formulas
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Answers
NaNO3 Ca(ClO3)2 K2SO3 Ca(OH)2
Sodium nitrate Calcium chlorate Potassium
sulfite Calcium hydroxide
Example Write the following chemical formulas
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Transition Metals

• metal that has more than one possibility for
  cationic charge

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How to Identify Name Ionic Compounds with
Transition Metals

• 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)

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Example 5
Iron (III) oxide
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Fe3
Cation
Iron (III) oxide
Anion
O-2
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Fe3
Fe3 O2-
Cation
3 -2 -1
Iron (III) oxide
Fe3 Fe3 O2- O2-
Anion
3 3 -2 -2 -2 0
O-2
The subscript 2 and 3 are used to show the
numbers of atoms needed.
Fe2O3
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Example 6
Copper (II) nitrate
129
Cu2
Cation
Copper (II) nitrate
Polyatomic Anion
NO3-1
130
Cu2
Cu2 NO31-
Cation
2 -1 1
Copper (II) nitrate
Cu2 NO3- NO3-
Polyatomic Anion
2 -1 -1 0
NO3-1
Use parenthesis when adding subscripts to a
polyatomic ion
Cu(NO3)2
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Self Check
Iron (II) nitrate Copper (I) chloride Lead (IV)
hydroxide Tin (II) oxide
Example Write the following chemical formulas
132
Answers
Fe(NO3)2 CuCl Pb(OH)4 SnO
Iron (II) nitrate Copper (I) chloride Lead (IV)
hydroxide Tin (II) oxide
Example Write the following chemical formulas
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Binary Covalent Compounds

• compound made from two non-metals
• between atoms that share electrons

Non metal
Non metal
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How to Identify Name Binary Covalent Compounds

• These compounds
• Use covalent prefixes
• To write these formulas
• Write the symbols of the first and second element
• Use the covalent prefixes (assume the first
  element is 1 if theres no prefix) as the
  subscripts to show number of atoms.

Atoms do not form charges when bonding
covalentlyyou DO NOT need to worry about charges
with this type! NOR CRISS CROSS METHOD!
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Example 7
Dinitrogen Tetraoxide
136
Di- 2
N
Dinitrogen Tetraoxide
O
Tetra- 4
N2O4
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Example 8
Silicon dioxide
138
Mono- is not written for the first element
Si
Silicon dioxide
O
Di- 2
SiO2
139
CAUTION!!!
di and bi do not mean the same thing!
bi-
di-
Stands for 2 in covalent compounds
Means theres a hydrogen in the polyatomic anion
Carbon dioxide CO2
Sodium biphosphate Na2HPO4
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Self Check
Carbon monoxide Sulfur tetraiodide Trichlorine
pentasulfide
Example Write the following chemical formulas
141
Answers
CO SI4 Cl3S5
Carbon monoxide Sulfur tetraiodide Trichlorine
pentasulfide
Example Write the following chemical formulas
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(No Transcript)
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Self Check Mixed Practice
Magnesium hydroxide Copper (II) nitrate Iron
(III) oxide Nitrogen dioxide Sodium bicarbonate
Example Write the following chemical formulas
144
Answers
Mg(OH)2 Cu(NO3)2 Fe2O3 NO2 NaHCO3
Magnesium hydroxide Copper (II) nitrate Iron
(III) oxide Nitrogen dioxide Sodium bicarbonate
Example Write the following chemical formulas
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Section 2.4
We need to know how acids behave when talking
about ant-acids!
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What is an Acid? Arrhenius Definition

• A substance that produces hydrogen ions (H1)
  when dissolved in water.
• H1 immediately reacts with water to make the
  hydronium ion, H3O1

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How do Acids produce Hydronium?
water
acid
Hydrogen cation with some anion
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How do Acids produce Hydronium?
1
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How do Acids produce Hydronium?
1
Hydronium ion
Anion
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How to Identify an Acid

• Look for a hydrogen ion, H as the first
  element in an aqueous covalent compound.

H2SO4 HCl H2CO3 HNO3 HC2H3O2
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Naming Binary Acids Non-Oxygen Acids

• These compounds have to
• Start with H (more than 1 H is OK, too).
• Do not contain oxygen
• To name these compounds
• Use hydro____ic acid
• Fill in the blank with the root of the anions
  name

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Example 1
HBr(aq)
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Its an acid
Hydrogen cation
HBr(aq)
Hydrobromic acid
Bromine
No oxygen Use hydro___ic
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Naming Oxyacids contain oxygen

• These compounds have
• Start with H (more than 1 H is OK, too).
• Must contain oxygen
• To name these compounds
• Use ___ic acids for -ate anions
• Use ___ous acids for -ite anions

Do not use hydro with thesethe word acid is
how you know it begins with hydrogen, not hydro-
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Example 2
HNO2(aq)
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Its an acid
Hydrogen cation
HNO2(aq)
nitrite ion
-ite ion Use ___ous acid
Nitrous acid
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Example 3
HC2H3O2(aq)
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Its an acid
Hydrogen cation
HC2H3O2(aq)
acetate ion
-ate ion Use ___ic
acetic acid
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Self Check
HF H2S H3PO4
Example Write the name for the following acids
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Answers
Hydrofluoric acid Hydrosulfuric acid Phosphoric
acid
HF H2S H3PO4
Example Write the name for the following acids
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Writing the chemical formula for Hydro- acids

• To write these formulas
• Write the cation, H1
• Write the anion symbol and charge
• Balance the charges by adding the appropriate
  subscript to the hydrogen cation OR Criss Cross
  Method

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Example 4
Hydrobromic acid
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H1
Hydrogen cation
Hydrobromic acid
Does not contain oxygen
Br-1
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H1
Hydrogen cation
Hydrobromic acid
Does not contain oxygen
H1Br-1
Br-1
1 -1 0
HBr
The compound is neutral. Subscripts are not needed
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Writing chemical formulas for Oxyacids

• To write these formulas
• Write the cation H1
• If it is an -ic acid, determine the polyatomic
  ion ending in -ate
• If it is an -ous acid, determine the polyatomic
  ion ending in -ite
• Add subscript to the hydrogen cation to balance
  charges OR use Criss Cross Method

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Example 5
Carbonic acid
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H1
Hydrogen cation
Carbonic acid
From the ___ate anion
CO3-2
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H1
H CO32-
Hydrogen cation
1 -2 -1
Carbonic acid
H H CO32-
1 1 -2 0
From the ___ate anion
CO3-2
H2CO3
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Example 6
Chlorous acid
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H1
Hydrogen cation
chlorous acid
From the ___ite anion
ClO2-1
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H1
Hydrogen cation
Chlorous acid
HClO2-1
From the ___ite anion
ClO2-1
1 -1 0
HClO2
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Self Check
Phosphorous acid Hydroiodic acid
Example Write the formula for the following acids
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Answers
Phosphorous acid Hydroiodic acid
H3PO3 HI
Example Write the formula for the following acids
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You Really Only Need to Know These Acids!
Memorize them!

• Hydrochloric acid HCl
• Sulfuric acid H2SO4
• Carbonic acid H2CO3
• Nitric acid HNO3
• Acetic acid HC2H3O2

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What is a Base? Arrhenius Definition

• A substance that produces hydroxide ions, OH-1
  in water
• H2O
• NaOH(s) Na1(aq) OH-1(aq)

1
H
Na
O
Na
Hydroxide Ion
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How to Identify a Base

• Look for an ionic compound that has a metal
  paired with the hydroxide ion, OH-
• OR Look for the ammonia molecule

NaOH Ca(OH)2 NH3
Do not assume all compounds ending in OH are
bases CH3OH is not a base but an alcohol
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Naming Writing Formulas for Metal Hydroxides

• Follow the rules for ionic compounds.
• The most common exception to this is ammonia, NH3
• NH3 (ammonia) is a base even though it doesnt
  contain -OH as the anion

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Example 7
NaOH
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Sodium
NaOH
Sodium Hydroxide
Hydroxide
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Self Check
Ca(OH)2 KOH Copper (II) hydroxide Lithium
hydroxide
Example Write the formula or name for each
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Answers
Calcium hydroxide Potassium hydroxide
Cu(OH)2 LiOH
Ca(OH)2 KOH Copper (II) hydroxide Lithium
hydroxide
Example Write the formula or name for each
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What is an Acid according to Bronsted-Lowry?

• Is a substance that is a proton or hydrogen donor
• Example HCl H2O ? H3O1 Cl-1
• acid base

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What is a base according to Bronsted-Lowry?

• Is a substance that is a proton acceptor
• Example NH3 H2O ? OH- NH4
• base acid
  conjugate conjugate
• 
  base acid

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Conjugate Acid-Base Pairs

• Conjugate Acid- substance formed when a base
  gains a H ion.
• Conjugate Base- substance formed when an acid
  loses a H ion.
• Label the acid base on the left side of the
  reaction the conjugate acid conjugate base on
  the right side.
• a) HNO3 H2O ? H3O NO3-
• ______ ______ ______
  ______
• b) NH3 H2O ? NH4 OH-
• _____ ______ ______
  ______

acid
base
C.A.
C.B.
acid
C.B.
base
C.A.
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Characteristics of Acids Bases
Bases
Acids
Produce H3O1 (hydronium ion) in water
Produce OH-1 (hydroxide ion) in water
Tastes Bitter
Tastes sour
Feels slippery
React with active metals to form hydrogen gas
Neutralizes a base to form salt and water
Neutralizes an acid to form salt and water
Both forms ions when dissolved conducts
electricity They are called ELECTROLYTES
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Strength versus Concentration
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• strong acid ALL acid molecules separate
  (dissociate) into H ions in water only ions
  present
• Examples HCl, HNO3, H2SO4
• weak acid Most acid molecules stay together,
  only a FEW separate into H ions when in water
  few ions present, mostly molecules
• Examples HC2H3O2 (vinegar) , H2CO3

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Strong Acid Weak Acid
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Strong versus Weak Acids
How many hydronium ion anion pairs can you find?
3
How many intact acid molecules can you find?
1
Strong acid Most of the acid molecules have
donated the H1 to water
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Strong versus Weak Acids
How many hydronium ion anion pairs can you find?
1
How many intact acid molecules can you find?
3
Weak acid Only a few of the acid molecules have
donated the H1 to water
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Strong Acids vs. Weak Acids
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Concentrated versus Dilute
solvent
solute
DILUTE (low concentration) Very little solute
(whats being dissolved) particles in solution
CONCENTRATED (higher concentration) Lots of
solute (whats being dissolved) particles in
solution
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Combinations of Concentration Strength
Dilute
Concentrated
A lot of acid/base added all dissociates
Not much acid/base added, but all of whats there
dissociates
Strong
A lot of acid/base added, but little dissociates
Not much acid/base added and very little
dissociates
Weak
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Bases Strength Concentration

• Bases follow the same pattern as acids
• A common misconception is acids are dangerous but
  bases are not!
• Vinegar is an acid we eatsome of them are safe!
• Sodium hydroxide is a very caustic basenot all
  of them are less harmful than acids!
• The stronger and acid or base is the more
  concentrated it is), the more dangerous it is for
  you!

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The Power of the Hydrogen pH

• The pH scale to measure the acidity of a sample

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Ways to measure pH

• Indicators change color based on pH
• Liquid indicators phenolphthalein or
  bromothymol blue
• Bromothymol Blue Acid turns Yellow Base
  turns blue
• Phenolphthalein Acid stays clear Base
  turns pink
• pH meters or pH probes
• Electronically determine pH and give a read-out

Base
Acid
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Ways to measure pH

• Indicators change color based on pH
• Paper with a liquid indicator on it (pH paper or
  Litmus paper)
• pH paper turns a color which matches
  to a pH number
• LITMUS PAPER (Mnemomic See board!)
• Blue Litmus stays blue in a base
• but turns pink in an acid
• Red Litmus stays red in an acid
• but turns blue in a base

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