Compounds vs. Elements Compound Table Salt : Soluble crystals, stable, edible Elements (Components) Sodium – shiny metal, reactive, poisonous Chlorine.

Molecules and Compounds: Nomenclature: Molecular compound Ionic compound Acid

Compounds vs. Elements Compound Table Salt : Soluble crystals, stable, edible Elements (Components) Sodium – shiny metal, reactive, poisonous Chlorine – pale yellow gas, reactive, poisonous

Law of Constant Composition
Pure substances have constant composition all samples of a pure substance contain the same elements in the same percentages (ratios): Water (H: 11%, O: 89%), Table salt (Na: 39%, Cl: 61%), Sugar Mixtures have variable composition: Air, Seawater, Concrete, Rocky road ice cream, Coke

Chemical Formula Chemical formula shows the number and type of each atom in the simplest unit of the compound Element as letter symbol: H (for hydrogen); Na (for Sodium) #Atoms of each element = subscript on the lower right of Symbol, H2O (two H atoms, one O atom, the 1 subscript is not written) Polyatomic groups (multiple atoms in group, example: SO4) are placed in parentheses if more than one. Example: Al2(SO4)3 (two Al atom, three SO4 groups)

Chemical Formula shows the Composition
H2O = two atoms of hydrogen and 1 atom of oxygen C12H22O11 = 12 atoms of C, 22 atoms of H and 11 atoms O

Classifying Pure Substances
Element Atomic element: consists of single atoms (Metals, Noble gases) Molecular element: consists of multi-atom molecules (O2, N2, Cl2, etc) Compound Molecular compound: consists of molecules made of only nonmetals (CO2, H2O) Ionic compound: consists of cations (Na+) and anions (Cl-)

Elements and Compounds

Classify each of the following: Element atomic/molecular Compound  molecular/ionic
aluminum, Al = atomic element aluminum chloride, AlCl3 = ionic compound chlorine, Cl2 = molecular element acetone, C3H6O = molecular compound carbon monoxide, CO = molecular compound cobalt, Co = atomic element aluminum, Al aluminum chloride, AlCl3 chlorine, Cl2 acetone, C3H6O carbon monoxide, CO cobalt, Co

Molecular Elements H2 N2 O2 F2 Cl2 Br2 I2
Certain elements occur as 2 atom molecules Rule of 7’s there are 7 common diatomic elements find the element with atomic number 7, N make a figure 7 by going over to Group 7A, then down don’t forget to include H2 VIIA H2 N2 O F2 Cl2 Br2 I2

Molecular Elements = Metal = Metalloid H = Nonmetal N O F Cl Br I

Molecular Compounds two or more nonmetals smallest unit is a molecule
Common examples: H2O CO2 (as in soda and dry ice) NH3 (as in Windex), Table sugar C11H22O11

Ionic Compounds Ions: Metals (Cation Mx+) and Nonmetals (Anion Ny-)
No individual molecules!! have a 3-dimensional array of cations and anions made of formula units: NaCl, MgO Na+ Cl- Na+ Cl- Na+ Cl- Cl- Na+ Cl- Na+ Cl- Na+

Naming Binary Molecular Compounds
Name first element in formula first use the full name of the element Name the second element in the formula with an -ide as if it were an anion, however, remember these compounds do not contain ions! Use a prefix in front of each name to indicate the number of atoms Never use the prefix mono- on the first element

Subscript - Prefixes 1 = mono-; 2 = di- 3 = tri- 4 = tetra- 5 = penta-
not used on first nonmetal 2 = di- 3 = tri- 4 = tetra- 5 = penta- 6 = hexa- 7 = hepta- 8 = octa- drop last “a” if name begins with vowel

Exceptions when Naming Molecular Compounds
of course, water  Other common exceptions: NH3: ammonia (as in Windex) H2S: hydrogen sulfide HCl: hydrogen chloride (same for HX, where X = halogen) CH4: methane (as in natural gas) H2O2: hydrogen peroxide

Example – Naming BF3 Is it one of the common exceptions? (H2O, NH3, CH4, C12H22O11 Identify Major Class (Molecular or Ionic) Name the first element Name the second element with an –ide Add a prefix to each name to indicate the subscript: Write the first element with prefix, then the second element with prefix Drop prefix mono from first element boron trifluoride

Variations in Naming molecular compound
Di-, tri- + iodide: keep both “i”s Example: PI3: phosphorous triiodide S2I2: disulfur diiodide Mono-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca- + oxide: drop the vowel CO: carbon monoxide P4O10: tetraphosphorous decoxide

Example – Naming Cl2O7 Is it one of the common exceptions? (H2O, NH3, CH4, C12H22O11 Identify Major Class (Molecular or Ionic) Name the first element Name the second element with an –ide Add a prefix to each name to indicate the subscript: Write the first element with prefix, then the second element with prefix Drop prefix mono from first element Dichlorine heptoxide

Ionic Compounds Made of Cation (+) and Anion (-) Name: Cation Anion
example: NaCl Sodium Chloride Cation: Type I metal Type II metal Polyatomic ion: ammonium NH4+ Anion: Nonmetal: Chloride Cl-, Oxide O2- Polyatomic ion: SO42- , OH- , NO3-

Net charge of Ionic Compound = 0
The ionic compound is neutral Net charge = Positive charge from cation(s) + Negative charge from Anion(s) = 0 Example: Compound Al2S3 Total Positive charge = 2 x (+3) = +6 Total Negative charge = 3 x (-2) = -6 Combined(Net) charge = = 0

Metal Cations: Type I Only have one possible charge
Groups IA, IIA, Ag+, Zn2+, Al3+ Charge by position (group) on the Periodic Table IA = +1, IIA = +2, Ag+ (IB), Zn2+(IIB) Al3+(IIIA) Name like the Element. Example: Ca2+ named as calcium Ag+ named as ______.

How do you know a metal cation is Type II?
Metal Cations: Type II Type II: Metal ions that are other than Type I Common Examples: Fe2+/3+, Cu+/2+, Cr2+/3+, Mn2+/4+, Pb2+/4+, Sn2+/4+, etc) have more than one possible charge Roman numeral in parenthesis to show the charge. Example: Fe2+ named as iron(II) Sn4+ named as _________ How do you know a metal cation is Type II? its not Type I !!!

Metal Cations: Type I vs. Type II
= Type I Metal = Type II Metal Al Zn Ag

Monatomic Nonmetal Anion (An-)
How much is the charge? the position on the Periodic Table Name of the anion: change ending on the element name to –ide Group 5A = -3 6A = -2 7A = -1 2nd period N3- = nitride O2- = oxide F- = fluoride 3rd period P3- = phosphide S2- = sulfide Cl- = chloride

Name of Ionic Compounds
Name: Cation Anion: Sodium Chloride Cation: Type I metal = metal name: Na+ => Sodium, Mg2+ => Magnesium Type II metal = metal name(charge): Fe3+ => Iron(III), Cu2+ Copper(II) Polyatomic ion = name of polyatomic ion, NH4+ => Ammonium Anion: Nonmetal = stem of nonmetal name + ide, Chloride, Oxide

Example – CaF2 Name the cation first, then anion
Is it one of the common exceptions? H2O, NH3, CH4, C12H22O11 Identify Major Class (Ionic or Molecular) Identify cation and anion Is the metal Type I or Type II (Type I = IA, IIA, AZA)? If type I, remember the charge. Name the cation first, then anion if type I, cation is simply the name of the element. Calcium fluoride

Find charge on Type II metal ions
Remember: Net Charge of Compound = 0 Example: Find the charge of IRON in Fe2O3 Which ion has fixed charge? oxide ion = _____ Find the total negative charge = __ x __ = __ Step up equation if you will Net charge = 0 =Total positive charge + Total negative charge 0 = ___ x Fe + ___ Find the charge on Fe ion by solving the equation Fe = ___ Key: remember the charge on ANIONs!

Example – Naming SnS2 Is it one of the common exceptions? H2O, NH3, CH4, C12H22O11 Identify Major Class (Ionic or Molecular) Identify cation and anion Is the metal Type I or Type II (Type I = IA, IIA, AZA)? If Type II metal ion, find the charge on cation Name the cation first, then anion. If type II metal ion,  name(Roman numeral) Tin(IV) sulfide

Polyatomic Ions Mg(NO3)2 Cu2SO4 NO3- : nitrate ion SO42- : sulfate ion
magnesium nitrate Cu2SO4 copper(I) sulfate Two NO3- ions no parentheses for one SO4 One Mg2+ ion Two __________ ions

Polyatomic Anions: -ATE ions (remember the red ones)
CO32- carbonate NO3- nitrate SiO32- silicate PO43- phosphate SO42- sulfate ClO3- chlorate AsO43- arsenate SeO42- selenate BrO3- bromate IO3- iodate

Periodic Pattern of Polyatomic Ions -ate groups
IIIA IVA VA VIA VIIA BO 3 3- CO 3 2- NO 3 - SiO 3 2- PO 4 3- SO 4 2- ClO 3 - AsO 4 3- SeO 4 2- BrO 3 - TeO 4 2- IO 3 -

Patterns for Polyatomic Ions
If the group of the element is even, charge of the ion is even; odd group? odd charge. C (IV)  CO32-; Cl (VII)  ClO3- elements in the same Group form similar polyatomic ions same number of O’s and same charge ClO3- = chlorate (-1 charge) BrO3- = bromate (-1 charge) if the polyatomic ion starts with H, the name adds hydrogen- prefix before name and add 1 to the charge CO32- = carbonate \ HCO3- = hydrogen carbonate

Polyatomic Ions: Same Element, Different #O atoms
-ate ion chlorate = ClO3- -ate ion + 1 O  same charge, per- prefix perchlorate = ClO4- -ate ion – 1 O  same charge, -ite suffix chlorite = ClO2- -ate ion – 2 O  same charge, hypo- prefix, -ite suffix hypochlorite = ClO-

Polyatomic Anions: -ite, hypo-E-ite, (-ate), per-E-ate
ClO- hypochlorite NO2- nitrite PO33- phosphite SO32- sulfite ClO2- chlorite NO3- nitrate PO43- phosphate SO42- sulfate ClO3- chlorate ClO4- perchlorate

-ATE/-ITE ions in Our Lives
ClO- (bleach) NO2- (preserve meat) PO33- (plant medicine) SO32- (wine, oxygen buster) ClO2- (bleach, disinfect) NO3- (fertilizer, explosives) PO43- (bone/teeth, fertilizer, soda) SO42- (plaster, car battery, sea salt) ClO3- (older pyrotechnics) ClO4- (pyrotechnics, solid fuel rocket)

Polyatomic Ions to Remember
Name Formula acetate C2H3O2– carbonate CO32– hydrogen carbonate (aka Bicarbonate) HCO3– hydroxide OH– nitrate NO3– nitrite NO2– permanganate MnO4– chromate CrO42– dichromate Cr2O72– ammonium NH4+ Name Formula hypochlorite ClO– chlorite ClO2– chlorate ClO3– perchlorate ClO4– sulfate SO42– Hydrogen sulfate (aka Bisulfate) HSO4– sulfite SO32– Hydrogen sulfite (aka Bisulfite) HSO3– cyanide CN–

Polyatomic Ions in Our Lives
C2H3O2– vinegar CO32– Soda drink HCO3– Baking soda, baking power, acid spill neutralizer OH– In liquid plumber/Drano as NaOH MnO4– Disinfectant, “aging” for movie making CrO42– Chrome plating (faucet, etc.) CN– Highly Poisonous; Plant seeds; blue pigment NH4+ Fertilizer; metabolic waste from animals

Example – Naming Na2SO4 One of the common exceptions? H2O, NH3, CH4, C12H22O11 Identify Major Class (ionic or molecular) If metal as cation, Type I or Type II? If type II, find the charge of metal ion (starting from charge of anion in your memory) Name cation first, followed by anion sodium sulfate

Example – Naming (NH4)3PO3
One of the common exceptions? H2O, NH3, CH4, C12H22O11 Identify Major Class (ionic or molecular) If metal as cation, Type I or Type II? If type II, find the charge of metal ion (starting from charge of anion in your memory) Name cation first, followed by anion Ammonium phosphite

Example – Naming Fe(NO3)3
One of the common exceptions? H2O, NH3, CH4, C12H22O11 Identify Major Class (ionic or molecular) If metal as cation, Type I or Type II? If type II, find the charge of metal ion (starting from charge of anion in your memory) Name cation first, followed by anion Iron(III) nitrate

Acids Contain H+ cation and anion
Hydrogen (H) as first element in formula Binary acids (HnX) have H+ cation and nonmetal anion. Example: HCl, H2Se Oxyacids (HnXOm) have H+ cation and polyatomic anion Example: HNO3, H2SO4, H3PO4,

Naming Acids All names have acid at end
Binary Acids (HnX) = hydro prefix + stem of the name of the nonmetal + ic suffix Example: HCl (Hydrochloric acid) Oxyacids (HnXOm) if polyatomic ion ends in –ate = name of polyatomic ion with –ic suffix : H2SO4 (Sulfuric acid); HClO4 (Perchloric acid) if polyatomic ion ends in –ite = name of polyatomic ion with –ous suffix H2SO3 (Sulfurous acid); HClO (hypochlorous acid)

Naming Acids – HF Identify if the compound is an acid
Identify the anion (-ide, -ite, or –ate?) Rename the anion with prefix and/or suffix: -ide  hydro-E-ic -ite  -ous -ate  -ic Add the word acid to the end hydrofluoric acid

Naming Acids – HClO2 Identify if the compound is an acid
Identify the anion (-ide, -ite, or –ate?) Rename the anion with prefix and/or suffix: -ide  hydro-E-ic -ite  -ous -ate  -ic Add the word acid to the end chlorous acid

Naming Acids – HIO3 Identify if the compound is an acid
Identify the anion (-ide, -ite, or –ate?) Rename the anion with prefix and/or suffix: -ide  hydro-E-ic -ite  -ous -ate  -ic Add the word acid to the end Iodic acid

Formula-to-Name Flow Chart

Write Chemical Formula using the charge of known ions
Example: Compound between Ca2+ and PO43- There needs to be 3 calcium ion and 2 phosphate ion, so that Total positive charge = 3 x (+2) = +6 Total negative charge = 2 x (-3) = -6 Net charge = +6 + (-6) = 0 Therefore the formula for the compound is Ca3(PO4)2

Write Chemical Formula using the charge of known ions
“Criss-Cross-Simplify”: The charge of an ion turns into the subscript (the number) of the counterpart ion Pb4+ O2- Since the subscripts in an ionic compound represents the RATIO among the ions, we simplify the subscripts to the simplest ratio Pb2O4  PbO2  Pb2O4

Write formula for sodium phosphite
Identify if the compound is an acid Identify cation and anion: find the charge Type II metal ion is given as the Roman numeral  “Criss-Cross-Simplify” Na3PO3

Write formula for chromium(III) selenide
Identify if the compound is an acid Identify cation and anion: find the charge Type II metal ion is given as the Roman numeral  “Criss-Cross-Simplify” Cr2Se3

Write formula for periodic acid
Identify if the compound is an acid Identify cation and anion: find the charge Type II metal ion is given as the Roman numeral  “Criss-Cross-Simplify” HIO4

Naming Molecular Compounds
Practice & Key: Naming Molecular Compounds CO ClO3 SO2 P2O5 N2O4 IF7 SF6 CO carbon monoxide ClO3 chlorine trioxide SO2 sulfur dioxide P2O5 diphosphorus pentoxide N2O4 dinitrogen tetroxide IF7 iodine heptoxide SF6 sulfur hexafluoride

Practice: Naming Ionic compounds
HgF2 CuI2 CaCl2 Fe2S3 SnCl4 Mg3N2 Ag2S

Answer key: names of ionic compounds
HgF2 = Mercury(II) fluoride CuI2 = copper(II) iodide CaCl2 = calcium chloride Fe2S3 = Iron(III) sulfide SnBr4 = tin(IV) bromide Mg3N2 = magnesium nitride Ag2S = silver sulfide

Practice: Naming Ionic compounds
Hg2SO4 CuClO3 Zn(NO3)2 FeCO3 Sn(SO3)2 CoPO4 Al(ClO4)3

Keys: Naming Ionic compounds
Hg2SO4 : mercury(I) sulfate CuClO3 : copper(I) chlorate Zn(NO3)2 zinc nitrate FeCO3 : iron(II) carbonate Sn(SO3)2: tin(IV) sulfite CoPO4 : cobalt(III) phophate Al(ClO4)3 : aluminum perchlorate

Practice: Naming Acids
HNO3 nitrate HClO3 chlorate HBr bromide H2CO3 carbonate H2SO3 sulfite H3PO4 phosphate HClO4 perchlorate H2Se selenide HNO3 HClO3 HBr H2CO3 H2SO3 H3PO4 HClO4

Practice: Naming Acids
HNO3 nitrate  nitric acid HClO3 chlorate  chloric acid HBr bromide  hydrobromic acid H2CO3 carbonate  carbonic acid H2SO3 sulfite  sulfurous acid H3PO4 phosphate  phosphoric acid HClO4 perchlorate  perchloric acid H2Se selenide  hydrobselenic acid

Review: Naming Compounds
CuSO3 copper(II) sulfite AgClO silver hypochlorite N2O5 dinitrogen pentoxide H2S hydrosulfuric acid FeI2 iron(II) iodide Sn(NO3)4 tin(IV) nitrate Ba3(PO4)2 barium phosphate (NH4)2S ammonium sulfide

Practice: Writing formulas (I)
copper(II) chloride aluminum oxide magnesium phosphide iron(II) bromide lead(II) sulfide zinc iodide sodium nitride

Key for Writing formulas (I): use criss-cross-reduce
copper(II) chloride CuCl2 aluminum oxide Al2O3 magnesium phosphide Mg3P2 iron(II) bromide FeBr2 lead(II) sulfide PbS zinc iodide ZnI2 sodium nitride Na3N

Practice: Write Chemical Formulae
Chromium(II) Chloride Cesium phosphate Lead(II) oxide Zinc nitrate Iron(III) sulfite Strontium nitride Ammonium carbonate Bromic acid Hydrosulfuric acid

Key: Write Chemical Formulae
Chromium(II) Chloride Cesium phosphate Lead(II) oxide Zinc nitrate Iron(III) sulfite Strontium nitride Ammonium carbonate Bromic acid Hydrosulfuric acid CrCl2 Cs3PO4 PbO Zn(NO3)2 Fe3(SO3)2 Sr3N2 (NH4)2CO3 HBrO3 H2S

Practice: Writing formulas (I)
copper(I) sulfate aluminum chlorate magnesium phosphate iron(II) carbonate lead(II) acetate zinc sulfite sodium nitrite Nitrogen gas Hypoiodous acid Hydroselenic acid

Hints for Writing formulas (I): Charges on Anions
copper(I) sulfate: -2 for sulfate aluminum chlorate: -1 for chlorate magnesium phosphate: -3 for phosphate iron(II) carbonate : -2 for carbonate lead(II) acetate: -1 for acetate zinc sulfite : -2 for sulfite sodium nitrite: -1 for nitrite Nitrogen gas: atomic or molecular element? Hypoiodous acid: -1 for hypoiodous Hydroselenic acid: -2 for selenide

Key: Writing formulas (I)
copper(I) sulfate: Cu2SO4 aluminum chlorate: Al(ClO3)3 magnesium phosphate: Mg3(PO4)2 iron(II) carbonate : FeCO3 lead(II) acetate: Pb(C2H3O2)2 zinc sulfite : ZnSO3 sodium nitrite: NaNO2 Nitrogen gas: N2 Hypoiodous acid: HIO Hydroselenic acid: H2Se

More on Writing formulae
copper(II) sulfate aluminum perchlorate hydroiodic acid iron(III) bromide Diphosphorus pentoxide lead(IV) nitride zinc carbonate helium gas

Key: Writing formulae copper(II) sulfate CuSO4
aluminum perchlorate Al(ClO4)3 hydroiodic acid HI iron(III) bromide FeBr3 Diphosphorus pentoxide P2O5 lead(IV) nitride Pb3N4 zinc carbonate ZnCO3 ammonium nitrite NH4NO2 helium gas He

Compounds vs. Elements Compound Table Salt : Soluble crystals, stable, edible Elements (Components) Sodium – shiny metal, reactive, poisonous Chlorine.

Similar presentations

Presentation on theme: "Compounds vs. Elements Compound Table Salt : Soluble crystals, stable, edible Elements (Components) Sodium – shiny metal, reactive, poisonous Chlorine."— Presentation transcript:

Similar presentations

About project

Feedback

Log in

Auth with social network:

Compounds vs. Elements Compound Table Salt : Soluble crystals, stable, edible Elements (Components) Sodium – shiny metal, reactive, poisonous Chlorine.

Similar presentations

Presentation on theme: "Compounds vs. Elements Compound Table Salt : Soluble crystals, stable, edible Elements (Components) Sodium – shiny metal, reactive, poisonous Chlorine."— Presentation transcript:

Similar presentations

About project

Feedback