molecules and compounds. section 5.2- 5.5 forming compounds assignment= ws 5.1 top & 5.2 odds
TRANSCRIPT
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Molecules and compounds
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Section 5.2- 5.5Forming compounds
Assignment= WS 5.1 top & 5.2 odds
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All pure substances have constant composition.• All samples of a pure substance contain the
same elements in the same percentages (ratios).• Mixtures have variable composition.
Tro's "Introductory Chemistry", Chapter 53
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The smallest piece of a compound is called a molecule.
Every molecule of a compound has the same number and type of atoms.
Since all molecules of a compound are identical, every sample of the compound will have the same properties.
Tro's "Introductory Chemistry", Chapter 54
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Water has a constant mass ratio of oxygen to hydrogen of 8.0.
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0.8g 2.0
g 0.16
hydrogen of mass
oxygen of mass Ratio Mass
Show how hematite has a constant composition if one sample has 7.2 g Fe and 2.8 g O and a second sample has 18.1 g Fe and 6.91 g O.
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They describe the number and type of each atom in the simplest unit of the compound.• Molecules or ions.
Each element is represented by its letter symbol.
The number of atoms of each element is written to the right of the element as a subscript.• If there is only one atom, the 1 subscript is not
written.
Polyatomic groups are placed in parentheses. • If more than one.
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Ions made of more then one element Not a compound Have a charge Memorize them for your quizzes! See the handout for the list!
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• Chlorate
• Carbonate
• Phosphate
• Nitrate
• Acetate
• Sulfate
• Iodate
• Cyanide
• Bicarbonate
• Hydroxide
• Ammonium
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Metals are written first.• NaCl
If two nonmetals they are written in order from Table 5.1.• CO2
• There are occasional exceptions for historical or informational reasons. H2O, but NaOH .
Tro's "Introductory Chemistry", Chapter 59
Table 5.1Order of Listing Nonmetalsin Chemical Formulas
C P N H S I Br Cl O F
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Tro's "Introductory Chemistry", Chapter 510
Mg(NO3)2
Compound calledmagnesium nitrate.
Symbol of the polyatomic ion called nitrate.
Symbol of the polyatomic ion called sulfate.
CaSO4
Compound calledcalcium sulfate.
Implied “1” subscripton magnesium.
Implied “1” subscripton calcium.
Parentheses to group two NO3s. No parentheses for one SO4.
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Certain elements occur as diatomic molecules.
7 diatomic elements—
12
H2
Cl2
Br2
I2
7
7A
N2 O2 F2
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IONIC COVALENT/MOLECULAR
Formed from two ions
Consists of a METAL and a nonmetal or polyatomic ion
Formed from two NONMETALS
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Two or more nonmetals.
Smallest unit is a molecule.
Tro's "Introductory Chemistry", Chapter 514
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Metals + nonmetals.
No individual molecule units, instead have a 3-dimensional array of cations and anions made of formula units.
Tro's "Introductory Chemistry", Chapter 515
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Aluminum, Al. Aluminum chloride, AlCl3. Chlorine, Cl2. Acetone, C3H6O. Carbon monoxide, CO. Cobalt, Co.
Tro's "Introductory Chemistry", Chapter 516
PRACTICE
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Ionic compounds are made of ions.
Ionic compounds always contain positive and negative ions• Cations = + charged ions; anions = − charged ions.
Ionic compounds have no charge
If there are only two elements = binary
If there are three or more (include a polyatomic)= Ternary
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1. Write the symbol for the metal cation and its charge.
2. Write the symbol for the nonmetal anion and its charge.
3. Switcheroo! Charge (without sign) becomes subscript for the other ion.
4. Reduce subscripts to smallest whole-number ratio.
5. Check that the sum of the charges of the cation cancels the sum of the anions.
Tro's "Introductory Chemistry", Chapter 518
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Potassium ion with a nitride ion.
Calcium ion with a bromide ion.
Aluminum ion with a sulfide ion.
Tro's "Introductory Chemistry", Chapter 519
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5.6-5.8 Naming ionic and molecular compounds
Assignment= Problem set #2
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Tro's "Introductory Chemistry", Chapter 521
H2O = Water, steam, ice. NH3 = Ammonia. CH4 = Methane. NaCl = Table salt. C12H22O11 = Table sugar.
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Tro's "Introductory Chemistry", Chapter 522
Ionic compounds.• Metal + nonmetal(s).
Metal first in formula.
• Binary ionic or compounds with polyatomic ions.
Molecular compounds.• 2 or more nonmetals.• Binary molecular (or binary covalent).
2 nonmetals.
• Acids—Formula starts with H. Though acids are molecular, they behave as ionic
when dissolved in water. May be binary or oxyacid.
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Tro's "Introductory Chemistry", Chapter 523
Made of cation and anion. Name by simply naming the ions.
• If cation is: Type I metal = Metal name. Type II metal = Metal name (charge). Polyatomic ion = Name of polyatomic ion.
• If anion is: Nonmetal = Stem of nonmetal name + -ide. Polyatomic ion = Name of polyatomic ion.
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Tro's "Introductory Chemistry", Chapter 524
Contain metal cation + nonmetal anion.
Metal listed first in formula and name.
1. Name metal cation first, name nonmetal anion second.
2. Cation name is the metal name.3. Nonmetal anion named by changing the
ending on the nonmetal name to –ide.
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Tro's "Introductory Chemistry", Chapter 525
Type I • Metals whose ions can only have
one possible charge. 1A, 2A, (Al, Zn, Ag).
• Determine charge by position on the periodic table. 1A = +, 2A = 2+, Al = 3+.
• Some need to be memorized. Zn = 2+, Ag = +.
Type II• Metals whose ions can have
more than one possible charge.• Determine charge by charge on
anion.
How do you know a metal cation is Type II?
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Tro's "Introductory Chemistry", Chapter 526
Contain metal cation + nonmetal anion. Metal listed first in formula and name.1. Name metal cation first, name nonmetal anion second.2. Metal cation name is the metal name followed by a roman
numeral in parentheses to indicate its charge.• Determine charge from anion charge.• Common Type II cations in Table 5.5.
3. Nonmetal anion named by changing the ending on the nonmetal name to –ide.
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Tro's "Introductory Chemistry", Chapter 527
1. Copper(II) ion with a nitride ion.
2. Iron(III) ion with a bromide ion.
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Tro's "Introductory Chemistry", Chapter 528
KCl
MgBr2
Al2S3
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• Metal and a polyatomic ion
1.Name the metal
2.Name the polyatomic ion
** DO NOT CHANGE THE ENDING!!!!
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KNO3
Mg(OH)2
NH4NO3
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Tro's "Introductory Chemistry", Chapter 531
1. Aluminum ion with a sulfate ion.
2. Chromium(II) with hydrogencarbonate.
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Name FormulaAcetate C2H3O2
–
Carbonate CO32–
Hydrogencarbonate(aka bicarbonate)
HCO3–
Hydroxide OH–
Nitrate NO3–
Nitrite NO2–
Chromate CrO42–
Dichromate Cr2O72–
Ammonium NH4+
Name FormulaHypochlorite ClO–
Chlorite ClO2–
Chlorate ClO3–
Perchlorate ClO4–
Sulfate SO42–
Sulfite SO32–
Hydrogen sulfate(aka bisulfate)
HSO4–
Hydrogen sulfite(aka bisulfite)
HSO3–
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Tro's "Introductory Chemistry", Chapter 533
1. NH4Cl
2. Ca(C2H3O2)2
3. Cu(NO3)2
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Tro's "Introductory Chemistry", Chapter 534
We will not learn the rules for molecular compounds with more than 2 elements.
For binary molecular:• Name first nonmetal.• Then name second nonmetal with -ide
ending.• Then give each name a prefix to indicate its
subscript in the formula.
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1. Name first element in formula first. • Use the full name of the element.
2. Name the second element in the formula with an −ide, as if it were an anion.
• However, remember these compounds do not contain ions!
3. Use a prefix in front of each name to indicate the number of atoms.
• Never use the prefix mono- on the first element.
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Tro's "Introductory Chemistry", Chapter 536
1 = mono-• 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.
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Tro's "Introductory Chemistry", Chapter 537
NO2
PCl5
I2F7
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Review problem set #1&25.9 naming acids
Assignment= Problem set #3
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Bromate
Chromate
Dichromate
Permanganate
Thiosulfate
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Didn’t you say we had to memorize these?
Lets look at the polyatomic ions and how they differ!!!
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Tro's "Introductory Chemistry", Chapter 542
Acids are molecular compounds that often behave like they are made of ions.
All names have acid at end. Binary Acids = Hydro- prefix + stem of
the name of the nonmetal + -ic suffix. Oxyacids:
• If polyatomic ion ends in –ate = Name of polyatomic ion with –ic suffix.
• If polyatomic ion ends in –ite = Name of polyatomic ion with –ous suffix.
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Acids are molecular compounds that form H+ when dissolved in water
Sour taste Dissolve many metals
• Like Zn, Fe, Mg, but not Au, Ag, Pt.
Formula generally starts with H• E.g., HCl, H2SO4.
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Contain H+1 cation and anion•In aqueous solution
Binary acids have H+1 and nonmetal
Oxyacids have H+1 and polyatomic
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45
Write a hydro- prefix. Follow with the nonmetal name. Change ending on nonmetal name to
–ic. Write the word acid at the end of the
name.
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HBr
HF
HI
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48
1. H2S
2. HClO3
3. HNO2
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When name ends in acid, formulas starts with H.
Hydro- prefix means it is binary acid, no prefix means it is an oxyacid.
For an oxyacid, if ending is –ic, polyatomic ion ends in –ate; if ending is –ous, polyatomic ion ends in –ite.
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50
1. Chloric acid
2. Phosphoric acid
3. Hydrobromic acid
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Problem Set #3 • Page 151
# 73, 74, 75, 76
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5.10- Review of Nomenclature5.11-Formula Mass
Assignment= Study for Chapter 5 Quest on day six
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Tro's "Introductory Chemistry", Chapter 553
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Potassium Chloride
Aluminum Oxide
Potassium Sulfide
Magnesium Hydroxide
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HNO3
H2SO4
H2SO3
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Tro's "Introductory Chemistry", Chapter 556
The mass of an individual molecule or formula unit.
Also known as molecular mass or molecular weight.
Sum of the masses of the atoms in a single molecule or formula unit.• Whole = Sum of the parts.
Mass of 1 molecule of H2O = 2(1.01 amu H) + 16.00 amu O =
18.02 amu.
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Tro's "Introductory Chemistry", Chapter 557