Chapter 2: Antacids.

Chapter 2: Antacids

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

Intro—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
There are two types of medicines you can use Antacids Acid Inhibitors 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?

Section 2.1—Types of Matter

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

Pure Substances versus Mixtures
Matter is classified as either a pure substance or a mixture Pure Substances Mixtures Contain only 1 type of particle Elements or Compounds Contain 2 or more pure substances Homogeneous or Heterogeneous

Pure Substances Elements Compound
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

Elements can be found on the periodic table!
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!

Elements

Every molecule is the same
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

Physical combination of more than 1 type of pure substance
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

Mixtures Homogeneous Heterogeneous (aka “solution”)
Mixtures can be classified as homogeneous or heterogeneous Homogeneous (aka “solution”) Heterogeneous 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

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

Homogeneous Mixtures Kool-Aid: sugar in water Brass: copper in zinc
Air: oxygen gas in nitrogen gas Milk: fat, proteins, sugar in water

Heterogeneous Mixtures
Oil in water Italian Salad Dressing Chicken Noodle Soup Fruit Salad

Classification of Matter

True Solutions, Colloids & Suspensions
Homogeneous Heterogeneous Heterogeneous True Solution Colloid Suspension SMALL particles don’t settle out and are too small to scatter light Ex: salt water, air, brass INTERMEDIATE particles don’t 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

True Solutions

vinegar and oil salad dressing
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” Solution Light passes through unchanged Colloids exhibit the Tyndall Effect Light 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 ingredients What purposes could the inactive ingredients serve?

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

Let’s 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

Let’s Practice Example:
Determine if each is element, compound, homogeneous or heterogeneous mixtures Tin Element Copper pipe Element Concrete Heterogeneous mix Carbon tetrachloride Compound Sports drink Homogenous mix

You Try! In Notes Example: Aluminum foil (Al)
Determine if each is element, compound, homogeneous or heterogeneous mixtures Aluminum foil (Al) Water (H2O) soda soil Carbon dioxide(CO2) Tap water

You Try! Example: Determine if each is element, compound, homogeneous or heterogeneous mixtures Aluminum foil (Al) Element Water (H2O) Compound Flat soda Homogeneous mix soil Heterogeneous mix Carbon dioxide(CO2) compound Tap water Homogeneous mix

The Science of Macaroni Salad

Section 2.2—Naming Chemicals
We need to be able to name the chemicals in the antacids!

The Language of Chemistry
Chemistry has a language all of its own Chemistry English Element Symbols Letters Chemical Formulas Words Chemical Equations Sentences Each element symbol starts with a capital letter

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

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) Cations Positive charge
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

Monatomic Ions of Group A /Type I Metals
Group B

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 Cr+3 Mn+2 Mn+3 Cu 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
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

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 Ion Zn+2 Zinc ion Fe+2 Iron (II) ion or Fe+3 Iron (III) ion P-3 Phosphide ion

Binary Ionic Compounds
Binary Ionic Compound- compound containing 2 elements—one 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 Ionic Compound

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 Metalloids Non-metals

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

Example #1 NaCl

NaCl Sodium Chloride Cation Anion “Sodium”
“Chlorine” becomes “Chloride” Sodium Chloride

Example #2 CaBr2

CaBr2 Calcium Bromide Cation Anion “Calcium”
“Bromine” becomes “Bromide” Calcium Bromide

Example #3 K2O

“Potassium” Cation K2O Anion “Oxygen” becomes “Oxide” Potassium Oxide

Write the name for the following compounds
Self Check Li2O Sr3P2 MgS BaI2 Example: Write the name for the following compounds

Answers Li2O Sr3P2 MgS BaI2 Lithium oxide Strontium phosphide Magnesium sulfide Barium iodide Example: Write the name for the following compounds

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 - Polyatomic Anion + Cation Ternary Ionic Compound + Polyatomic Cation - Anion

Common Polyatomic Ions
You don’t need to memorize them. Look at your reference sheet. 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

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)

Practice Identifying Polyatomic Ions
NaNO3 NH4Cl Ca(OH)2 (NH4)3PO4 K2CO3 Example: Underline& name the polyatomic ion in each compound

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

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 ion’s name If the anion is a single non-metal element, write its name with the suffix “-ide”

Example # 4 Ca(NO3)2

“Calcium” Cation Ca(NO3)2 Polyatomic Anion “Nitrate” Calcium Nitrate

Example #5 Na3PO4

“Sodium” Cation Na3PO4 Polyatomic Anion “phosphate” Sodium phosphate

Example # 6 K2CO3

K2CO3 Potassium carbonate Cation Polyatomic Anion “potassium”

Self Check Ca(C2H3O2)2 Li2SO3 Ba(OH)2 (NH4)2S Example: Write the name for the following compounds

Answers Ca(C2H3O2)2 Li2SO3 Ba(OH)2 (NH4)2S Calcium acetate Lithium sulfite Barium hydroxide Ammonium Sulfide Example: Write the name for the following compounds

Worksheet 1 (1-10 Answers) 1. Sodium sulfide 6. Silver chloride
2. Aluminum oxide 7. Boron nitride 8. Barium fluoride 3. Sodium chloride 4. Rubidium iodide 9. Strontium nitride 5. Zinc bromide 10. Magnesium chloride

Worksheet 2 (1-10 Answers) 1. copper(I) fluoride 6.chromium (VI) oxide
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

Worksheet 3 (1-10 Answers) 1. vanadium(V) chlorate Gold(I) nitrate
7. iron(III) phosphite 2. rhenium(VI) sulfate 8. nickel(II) bromate 3. osmium(III) iodate 9. lead(IV) sulfide 10. Manganese (VII) dichromate 4. iridium(IV) phosphate 5. palladium(IV) sulfite

Worksheet 4 (1-10 Answers) 1. ammonium chloride 6. ammonium nitrate
2. hydrogen chlorite 7. strontium phosphate 8. zinc chlorate 3. calcium bromate 4. beryllium sulfate 9. silver iodate 5. ammonium nitride 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; Common multivalent metals and their charges Cobalt Co Co+3 Copper Cu Cu+2 Iron Fe Fe+3 Manganese Mn+2 Mn+3 Mercury Hg2+2 Hg+2 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)

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 metal’s name

Example # 7 CuCl

CuCl Copper Chloride Cation Anion “Copper”
“Chlorine” becomes “Chloride”

CuCl (I) Copper Chloride Cation Anion “Copper”
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) Copper Chloride (I)

Example # 8 Fe2(CO3)3

“Iron” Cation Fe2(CO3)3 Iron carbonate Polyatomic Anion “Carbonate”

Fe2(CO3)3 Iron carbonate (III) Cation Polyatomic Anion “Iron”
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) Iron carbonate (III)

Example # 9 ZnBr2

“Zinc” Cation ZnBr2 Zinc bromide monatomic Anion “bromide”

ZnBr2 Zinc bromide Cation Polyatomic Anion “Zinc”
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

Self Check PbCl2 PbCl4 MnO Mn2O3 Example: Write the name for the following compounds

Answers PbCl2 PbCl4 MnO Mn2O3 Lead (II) chloride Lead (IV) chloride Manganese (II) oxide Manganese (III) oxide Example: Write the name for the following compounds

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 Covalent compound

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 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”

PREFIXES USED IN MOLECULAR COMPOUNDS
Covalent Prefixes PREFIXES USED IN MOLECULAR COMPOUNDS mono di- tri- tetra- penta- hexa- hepta- octa- nona- deca-

Example #10 P2O5

P2O5 Diphosphorus pentaoxide Phosphorus Oxygen 2 = “di-” 5 = “penta-”

Example #11 SiF4

SiF4 Silicon tetrafluoride Silicon Fluorine
Don’t use “mono-” on first element Silicon SiF4 Fluorine 4 = “tetra-” “fluoride” Silicon tetrafluoride

Self Check SO2 N2Cl4 P4O10 CO Example: Write the name for the following compounds

Answers SO2 N2Cl4 P4O10 CO sulfur dioxide Dinitrogen tetrachloride Tetraphosphorus decaoxide Carbon monoxide Example: Write the name for the following compounds

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

Answers Na2O K3PO4 Cu(OH)2 N2S MgCl2 Sodium oxide Potassium phosphate Copper (II) hydroxide Dinitrogen monosulfide Magnesium chloride Example: Write the name for the following compounds

Section 2.3—Writing Chemical Formulas
We need to be able to read the formulas for chemicals in the antacids!

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

Binary Ionic Compounds
containing two elements—one metal and one non-metal formed by attraction between + and - ions + Cation - Anion Ionic Compound

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.

Example #1 Sodium chloride

Na+1 Cation Sodium chloride Anion Cl-1 NaCl

NaCl Example #1 Sodium chloride +1 + -1 = 0 Na+1Cl-1 Cation Anion Na+1
The compound is neutral…no subscripts are needed. Cl-1 NaCl

Example #2 Calcium bromide

Example #2 Ca+2 Cation Calcium bromide Anion Br-1

CaBr2 Example #2 Calcium bromide +2 + -1 = +1 Ca+2 Br-1 Cation Anion
Ca+2 Br-1 Br-1 Br-1 = 0 CaBr2 The subscript “2” is used to show that 2 anions are needed.

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

Write the following chemical formulas
Self Check Cesium chloride Potassium oxide Calcium sulfide Lithium nitride Example: Write the following chemical formulas

Answers Cesium chloride Potassium oxide Calcium sulfide Lithium nitride CsCl K2O CaS Li3N Example: Write the following chemical formulas

Ternary Ionic Compounds
compound containing at least one polyatomic ion Either in the front, the back or in both places + Cation - Polyatomic Anion Polyatomic Ionic Compound

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

Example #3 Sodium carbonate

Na+1 Cation Sodium carbonate Polyatomic Anion CO3-2

Na2CO3 Sodium carbonate +1 + -2 = -1 Na1+ CO32- Cation Polyatomic
Anion Na+ Na+ CO32- = 0 CO3-2 Na2CO3 The subscript “2” is used to show that 2 cations are needed.

Example #4 Magnesium nitrate

Mg+2 Cation Magnesium nitrate Polyatomic Anion NO3-1

Mg(NO3)2 Mg+2 Magnesium nitrate Mg+2NO31- +2 + -1 = 1 NO3-1 Cation
Polyatomic Anion = 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

Self Check Sodium nitrate Calcium chlorate Potassium sulfite Calcium hydroxide Example: Write the following chemical formulas

Answers Sodium nitrate Calcium chlorate Potassium sulfite Calcium hydroxide NaNO3 Ca(ClO3)2 K2SO3 Ca(OH)2 Example: Write the following chemical formulas

Transition Metals metal that has more than one possibility for cationic charge

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)

Example #5 Iron (III) oxide

Fe+3 Cation Iron (III) oxide Anion O-2

Fe2O3 +3 + -2 = -1 Iron (III) oxide O-2 Fe+3 Fe+3 O2- Cation Anion
Fe+3 Fe+3 O2- O2- Anion = 0 O-2 The subscript “2” and “3” are used to show the numbers of atoms needed. Fe2O3

Example #6 Copper (II) nitrate

Cu+2 Cation Copper (II) nitrate Polyatomic Anion NO3-1

Cu(NO3)2 +2 + -1 = 1 Copper (II) nitrate Cu+2 Cu+2 NO31- NO3-1 Cation
Polyatomic Anion = 0 NO3-1 Use parenthesis when adding subscripts to a polyatomic ion Cu(NO3)2

Self Check Iron (II) nitrate Copper (I) chloride Lead (IV) hydroxide Tin (II) oxide Example: Write the following chemical formulas

Answers Iron (II) nitrate Copper (I) chloride Lead (IV) hydroxide Tin (II) oxide Fe(NO3)2 CuCl Pb(OH)4 SnO Example: Write the following chemical formulas

Binary Covalent Compounds
compound made from two non-metals between atoms that share electrons Non metal Non metal Covalent compound

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 there’s no prefix) as the subscripts to show number of atoms. Atoms do not form charges when bonding covalently…you DO NOT need to worry about charges with this type! NOR CRISS CROSS METHOD!

Dinitrogen Tetraoxide
Example #7 Dinitrogen Tetraoxide

Dinitrogen Tetraoxide
N2O4

Example #8 Silicon dioxide

Silicon dioxide SiO2 “Di-” = 2 Si O
“Mono-” is not written for the first element Si Silicon dioxide O “Di-” = 2 SiO2

CAUTION!!! “di” and “bi” do not mean the same thing! di- bi-
Stands for “2” in covalent compounds Means there’s a hydrogen in the polyatomic anion Carbon dioxide = CO2 Sodium biphosphate = Na2HPO4

Self Check Carbon monoxide Sulfur tetraiodide Trichlorine pentasulfide Example: Write the following chemical formulas

Answers Carbon monoxide Sulfur tetraiodide Trichlorine pentasulfide CO SI4 Cl3S5 Example: Write the following chemical formulas

Self Check: Mixed Practice
Magnesium hydroxide Copper (II) nitrate Iron (III) oxide Nitrogen dioxide Sodium bicarbonate Example: Write the following chemical formulas

Answers Magnesium hydroxide Copper (II) nitrate Iron (III) oxide Nitrogen dioxide Sodium bicarbonate Mg(OH)2 Cu(NO3)2 Fe2O3 NO2 NaHCO3 Example: Write the following chemical formulas

Section 2.4 We need to know how acids behave when talking about ant-acids!

What is an Acid? – Arrhenius Definition
A substance that produces hydrogen ions (H+1) when dissolved in water. H+1 immediately reacts with water to make the hydronium ion, H3O+1 H O water H O +1 H +1

How do Acids produce Hydronium?
- water acid Hydrogen cation with some anion

- +1 H O

- +1 H O Hydronium ion Anion

How to Identify an Acid H2SO4 HCl H2CO3 HNO3 HC2H3O2
Look for a hydrogen ion, “H+” as the first element in an aqueous covalent compound. H2SO4 HCl H2CO3 HNO3 HC2H3O2

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 anion’s name

Example #1 HBr(aq)

HBr(aq) Hydrobromic acid No oxygen Use “hydro___ic” Hydrogen cation
It’s an acid Hydrogen cation HBr(aq) Hydrobromic acid Bromine No oxygen Use “hydro___ic”

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 these…the word “acid” is how you know it begins with hydrogen, not “hydro-”

Example #2 HNO2(aq)

HNO2(aq) Nitrous acid Use “___ous” acid Hydrogen cation nitrite ion
It’s an acid Hydrogen cation HNO2(aq) nitrite ion “-ite” ion Use “___ous” acid Nitrous acid

Example #3 HC2H3O2(aq)

HC2H3O2(aq) acetic acid Use “___ic” Hydrogen cation acetate ion
It’s an acid Hydrogen cation HC2H3O2(aq) acetate ion “-ate” ion Use “___ic” acetic acid

Write the name for the following acids
Self Check HF H2S H3PO4 Example: Write the name for the following acids

Write the name for the following acids
Answers HF H2S H3PO4 Hydrofluoric acid Hydrosulfuric acid Phosphoric acid Example: Write the name for the following acids

Writing the chemical formula for “Hydro-” acids
To write these formulas: Write the cation, H+1 Write the anion symbol and charge Balance the charges by adding the appropriate subscript to the hydrogen cation OR Criss Cross Method

Example #4 Hydrobromic acid

Does not contain oxygen
H+1 Hydrogen cation Hydrobromic acid Does not contain oxygen Br-1

Does not contain oxygen
H+1 Hydrogen cation Hydrobromic acid Does not contain oxygen H+1Br-1 Br-1 = 0 HBr The compound is neutral. Subscripts are not needed

Writing chemical formulas for “Oxyacids”
To write these formulas: Write the cation H+1 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

Example #5 Carbonic acid

From the “___ate” anion
Hydrogen cation Carbonic acid From the “___ate” anion CO3-2

From the “___ate” anion
Hydrogen cation H+ CO32- = -1 Carbonic acid H+ H+ CO32- = 0 From the “___ate” anion CO3-2 H2CO3

Example #6 Chlorous acid

From the “___ite” anion
Hydrogen cation chlorous acid From the “___ite” anion ClO2-1

From the “___ite” anion
Hydrogen cation Chlorous acid H+ClO2-1 From the “___ite” anion ClO2-1 = 0 HClO2

Write the formula for the following acids
Self Check Phosphorous acid Hydroiodic acid Example: Write the formula for the following acids

Write the formula for the following acids
Answers Phosphorous acid Hydroiodic acid H3PO3 HI Example: Write the formula for the following acids

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

What is a Base? – Arrhenius Definition
A substance that produces hydroxide ions, OH-1 in water H2O NaOH(s) Na+1(aq) + OH-1(aq) H O water H O -1 +1 H Na O Na Hydroxide Ion

How to Identify a Base NaOH Ca(OH)2 NH3
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

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 doesn’t contain “-OH” as the anion

Example #7 NaOH

Sodium NaOH Sodium Hydroxide Hydroxide

Write the formula or name for each
Self Check Ca(OH)2 KOH Copper (II) hydroxide Lithium hydroxide Example: Write the formula or name for each

Write the formula or name for each
Answers Ca(OH)2 KOH Copper (II) hydroxide Lithium hydroxide Calcium hydroxide Potassium hydroxide Cu(OH)2 LiOH Example: Write the formula or name for each

What is an Acid according to Bronsted-Lowry?
Is a substance that is a proton or hydrogen donor Example: HCl + H2O  H3O+1 + Cl-1 acid base

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

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) HNO H2O  H3O NO3− ______ ______ ______ ______ b) NH H2O  NH OH− _____ ______ ______ ______ acid base C.A. C.B. base acid C.A. C.B.

Characteristics of Acids & Bases
Produce H3O+1 (hydronium ion) in water Produce OH-1 (hydroxide ion) in water Tastes sour Tastes Bitter React with active metals to form hydrogen gas Feels slippery 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

Strength versus Concentration

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

Strong Acid Weak Acid

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 H+1 to water

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 H+1 to water

Strong Acids vs. Weak Acids

Concentrated versus Dilute
solvent solute DILUTE (low concentration) Very little solute (what’s being dissolved) particles in solution CONCENTRATED (higher concentration) Lots of solute (what’s being dissolved) particles in solution

Combinations of Concentration & Strength
Concentrated Dilute Strong A lot of acid/base added & all dissociates Not much acid/base added, but all of what’s there dissociates Weak A lot of acid/base added, but little dissociates Not much acid/base added and very little dissociates

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 eat…some of them are safe! Sodium hydroxide is a very caustic base…not 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!

The Power of the Hydrogen: pH
The pH scale to measure the acidity of a sample

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 Acid Base

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

Chapter 2: Antacids.

Similar presentations

Presentation on theme: "Chapter 2: Antacids."— Presentation transcript:

Similar presentations

About project

Feedback

Log in

Auth with social network:

Chapter 2: Antacids.

Similar presentations

Presentation on theme: "Chapter 2: Antacids."— Presentation transcript:

Similar presentations

About project

Feedback