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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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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
slide5
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 = _______________

slide11

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
slide15
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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