Using chemical formulas
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Using Chemical Formulas. 7-3. Beaker Breaker. Name the following compounds: CaCl 2 = ____________ P 3 O 6 = _____________ FeCl 2 =______________ H 2 SO 4 =______________. Formula Masses. sum of the average atomic masses of all the atoms represented in a formula

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Using Chemical Formulas

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Using chemical formulas

Using Chemical Formulas

7-3


Beaker breaker

Beaker Breaker

  • Name the following compounds:

    CaCl2 = ____________

    P3O6 = _____________

    FeCl2 =______________

    H2SO4 =______________


Formula masses

Formula Masses

  • sum of the average atomic masses of all the atoms represented in a formula

  • (can be of a molecule, formula unit or ion)

  • Formula mass of H2O:

  • 2 (ave. atomic mass of H) +1(ave. at. mass of O)

  • = 2(1.01 amu) + 1(16.00 amu)

  • = 2.02 amu + 16.00 amu

  • = 18.02 amu


Calculate the formula mass of the following

Calculate the formula mass of the following:

  • sulfuric acid

  • calcium nitrate

  • phosphate ion

  • magnesium chloride


Using chemical formulas

  • sulfuric acid

  • 98.09 amu H2SO4

  • calcium nitrate

  • 164.10 amu Ca(NO3)2

  • phosphate ion

  • 94.97 amu PO43-

  • magnesium chloride

  • 95.21 amu MgCl2


Molar masses

Molar Masses

  • sum of the masses of the elements present in a mole of the molecules or formula units that make up a compound

  • Molar mass of water, H2O:

  • 1 mole H2O = 2 mol H + 1 mol O

  • 2 mol H x 1.01 g H = 2.02 g H

    1 mol H

  • 1 mol O x 16.00 g = 16.00 g O

    1 mol O 18.02 g

  • Molar mass of water = 18.02 g/mol


What is the molar mass of

What is the molar mass of…

  • aluminum sulfide

  • sodium nitrate

  • barium hydroxide


What is the molar mass of1

What is the molar mass of…

  • aluminum sulfide

  • Al2S3 150.17 g/mol

  • sodium nitrate

  • NaNO3 85.00 g/mol

  • barium hydroxide

  • Ba(OH)2 171.35 g/mol


Beaker breaker1

Beaker Breaker

  • Name the following the compounds:

    CaBr2 =_______________

    H3PO3 =_______________

    C3I7 =_________________

    CuCl3 = _______________


Using chemical formulas

Using Molar Mass as a conversion

factor between “moles” ↔ “mass”

  • What is the mass, in grams, of 0.50000 moles of barium hydroxide?

  • Given: 0.500000 mol Ba(OH)2

  • Find: g Ba(OH)2

  • Know: 1 mol Ba(OH)2 =171.35 g Ba(OH)2

  • 0.500000 mol Ba(OH)2 x 171.35 g Ba(OH)2

    1 mole Ba(OH)2

  • = 85.675 g Ba(OH)2


How many moles are in 6 60 g of ammonium sulfate

How many moles are in 6.60 g of ammonium sulfate?

  • Given: 6.60g (NH4)2SO4

  • Find: 0.0499 mol (NH4)2SO4

  • Know:1 mol(NH4)2SO4 = 132.17 g (NH4)2SO4

  • (NH4)2SO4 = 2(N) + 8(H) + 1(S) + 4(O)

  • = 2(14.01) + 8(1.01) + 1(32.07) + 4(16.00)

  • 132.17 g/mol

  • 6.60g (NH4)2SO4 x 1 mol(NH4)2SO4

    132.17 g (NH4)2SO4

  • = 0.0499 mol (NH4)2SO4(4.99 x 10-2mol)


Remember 1 mole 6 02 x 10 23 things

Remember…. 1 mole = 6.02 x 1023 “things”

  • How many molecules are in 50.0 g of water?

  • Given: 50.0 g H2O

  • Find: molecules H2O

  • Know: 1 mol H2O = 18.02g

  • 1 mol H2O = 6.02 x 1023 molecules H2O

  • 50.0 g H2O x 1 mol H2O x 6.02 x 1023 molecules

    18.02 g H2O 1 mol H2O

  • = 1.67 x 1024 molecules H2O


Using chemical formulas

White Board Practice with PartnersHow many moles of compound are there in the followinga. 6.60g (NH4)2SO4b. 4,500g Ca(OH)2


Answers

Answers

  • A. 0.0500mol

  • B. 61mol


White board practice with partners

White Board Practice with Partners

  • How many molecules are there in the following:

    a. 25.0g H2SO4

    b. 125g of C12H22O11


Answers1

Answers

  • A. 1.53 x1023 molecules

  • B. 2.20 x1023 molecules


Beaker breaker2

Beaker Breaker

  • Write the formulas of the following compounds

  • Nitric Acid =___________

  • Hydroiodic acid =____________

  • Magnesium Fluoride =____________

  • Tetracarbon nonahydride =__________


Percentage composition

Percentage Composition

  • % = part x 100

    whole

  • percentage by mass of each element in a cmpd


Find the copper in copper i sulfide

Find the % copper in copper(I) sulfide

  • % Cu = part Cu x 100

    whole Cu2S

  • % Cu = mass of Cu in 1 mole of Cu2S x 100

    mass of 1 mol of Cu2S

    Or...% Cu= mass of Cu in 1 mole of Cu2S x 100

    molar mass of Cu2S

  • Cu2S = 159.17 g/mol (molar mass..on bottom)

  • 1 mol Cu2S, there are 2 mol Cu = 127.10 g Cu

    (top term)


Find the copper in copper i sulfide1

Find the % copper in copper(I) sulfide

Know:

  • % Cu = mass of Cu in 1 mole of Cu2S x 100

    mass of 1 mol of Cu2S

  • 1 mol of Cu2S = 159.17 g Cu2S

  • 1 mol of Cu2S= 2mol Cu = 2(63.546g)= 127.10g

  • = 127.10 g Cu x 100

    159.17 g Cu2S

  • = 79.852% Cu in Cu2S


What is the percent carbon in ammonium carbonate

What is the percent carbon in ammonium carbonate?

Know: (NH4)2CO3

  • % C = grams of C in 1 mol (NH4)2CO3x 100

    molar mass of (NH4)2CO3

  • 1 mol (NH4)2CO3 = 1 mol C = 12.01 g C

  • 1 mol (NH4)2CO3 = 96.11 g (NH4)2CO3

  • = 12.01 g C x 100

    96.11 g

  • = 12.50% C


Beaker breaker3

Beaker Breaker

  • Phosphoric acid can be used in orthodontics to roughen the surface of teeth before the placement of braces. Write the chemical formula for phosphoric acid.

  • Explain your method used to arrive to that answer.


Homework check pg 236 25

Homework CheckPg 236 #25

a. NH41+

Ammonium

b.ClO3-

Chlorate

c. OH-

Hydroxide

d.SO42-

Sulfate

e. NO3-

Nitrate

f.CO32-

Carbonate

g. PO43-

Phosphate

h. CH3COO-

Acetate

i. HCO3-

Bicarbonate

j. CrO42-

Chromate


Mix review challenge

Mix Review Challenge

Write the name or formula of the following:

  • MgSO3 =______________

  • Sodium Hydroxide = __________

  • Nickel (II) Fluoride =___________

  • P2H3 =__________


Answers2

Answers

  • Magnesium Sulfite

  • NaOH

  • NiF2

  • Diphosphorus Trihydride


Mix review challenge1

Mix Review Challenge

  • Write the name or formula of the following:

    5. Sulfurous acid =___________

    6. Copper (II) Chloride =_________

    7. AlPO4 =____________

    8. TetraSulfur Heptoxide =__________


Answers3

Answers

5. H2SO3

6. CuCl2

7. Aluminum Phosphate

8. S4O7


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