activity name that compound - chemistry 7 · 6.022 x 1023 s atoms 32.07 g s . molecular mass and...
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NAME THAT COMPOUND
ACTIVITY
1
Minute to Name It!
A list of chemical formula and names
would be shown on the screen.
Each student would need to identify the
corresponding name (if a formula is given)
or formula (if a name is given).
2
Li2Se
AlCl3
Sr3P2
BaI2
Mg2N2
Ferric oxide
Ferrous oxide
Chromium(II) sulfide
Chromium(III) oxide
Lead(IV) oxide
CsCl
NaBr
BeCl2
Al2O3
BaS
Copper(II) telluride
Mercury(II) oxide
Stannic fluoride
Plumbous bromide
Copper(I) chloride
KF
CaC2
MgH2
BeCl2
Cd3P2
Cobalt(II) fluoride
Lead(IV) oxide
Nickel(II) phosphide
Lead(IV) sulfide
Nickel(II) iodide
Li2Se Lithium selenide
AlCl3 Aluminum chloride
Sr3P2 Strontium phosphide
BaI2 Barium iodide
Mg3N2 Magnesium nitride
KF Potassium fluoride
CaC2 Calcium carbide
MgH2 Magnesium hydride
BeCl2 Beryllium chloride
Cd3P2 Cadmium phosphide
CsCl Cesium chloride
NaBr Sodium bromide
BeCl2 Beryllium chloride
Al2O3 Aluminum oxide
BaS Barium sulfide
Fe2O3 Ferric oxide
FeO Ferrous oxide
CrS Chromium(II) sulfide
Cr2O3 Chromium(III) oxide
PbO2 Lead(IV) oxide
CuTe Copper(II) telluride
HgO Mercury(II) oxide
SnF4 Stannic fluoride
PbBr2 Plumbous bromide
CuCl Copper(I) chloride
CoF2 Cobalt(II) fluoride
PbO2 Lead(IV) oxide
Ni3P2 Nickel(II) phosphide
PbS2 Lead(IV) sulfide
NiI2 Nickel(II) iodide
Stoichiometry of Formulas and
Equations
CHAPTER 3
Burning Magnesium
7
Chemical reaction:
2 Mg(s) + O2(g) 2 MgO(s)
How do we look at this in terms of mass?
48 amu 32 amu 80 amu
? grams ? grams ? grams
Mole (abbreviated mol)
8
SI unit for amount of substance
Number of entities as there are atoms in exactly 12 g of 12C
Equal to 6.022 x 1023 entities
Called the Avogadro’s number
How big is Avogadro’s Number?
9
Spreading 1 mole of marbles over the entire surface of the earth
would produce a blanket of marbles almost 5 km high.
Avogadro’s Number: 602,200,000,000,000,000,000,000
College
tuition
World
population
Distance from
earth to sun (cm)
Age of the
earth (s)
Volume of world’s
oceans (L)
A mole of water
10
A mole of other substances
11
O2 (g)
32.00 g
H2O (l)
18.02 g
Cu (s)
63.55 g
CaCO3
100.09 g
1 mole of Fe vs 1 mole of S
12
The mole allows us to count out exactly the same number of things but use mass to do it!
1 mole Fe
6.022 x 1023 Fe atoms
55.85 g Fe
1 mole S
6.022 x 1023 S atoms
32.07 g S
Molecular Mass and Molar Mass
13
The molecular mass (or molecular weight) is the sum of the
atomic masses (in amu) in a single molecule.
The molar mass of a covalent compound is numerically equal
to the molecular mass, but in grams per mole.
Formula Mass and Molar Mass
14
The formula mass (or formula weight) is the sum of the
atomic masses (in amu) in a formula unit.
The molar mass of an ionic compound is numerically equal
to the formula mass, but in grams per mole.
Summary of Different Mass Terms
15
Term Definition Unit
Isotopic Mass Mass of an isotope of an
element
amu
Atomic Mass
(aka Atomic Weight)
Weighted average mass of an
element’s naturally occurring
isotopes
amu
Molecular or
Formula Mass
(aka Molecular or
Formula Weight)
Sum of the atomic masses of
the atoms (or ions) in a
molecule (or formula unit)
amu
Molar Mass Mass of 1 mole of a chemical
entity (e.g. atoms, ions,
molecules, or formula units)
grams per
mole (g/mol)
Practice Problem
16
What is the molecular mass of glucose (C6H12O6)?
Molecular Mass:
6 x 12.011 + 12 x 1.007 + 6 x 15.99 = 180.16 amu
Practice Problem
17
Complete the table below for glucose (C6H12O6,
MW = 180.16 g/mol)
Carbon Hydrogen Oxygen
Atoms in 1
glucose molecule
Mass C/H/O in 1
glucose molecule
Atoms per mole
of compound
Moles of atoms
in 1 mole cmpd
Mass per 1 mole
of compound
6 12 6
6 x 12.01 =
72.06 amu
12 x 1.008 =
12.10 amu
6 x 15.99 =
96.00 amu
6 (6.022x1023)
atoms 12 (6.022x1023)
atoms
6 (6.022x1023)
atoms
6 moles of
atoms
12 moles of
atoms
6 moles of
atoms
72.06 g 12.10 g 96.00 g
What’s in a Chemical Formula?
18
2 atoms of Al and 3 molecules of (SO4)2-
1 formula unit of Al2(SO4)3 = 342.17 amu
1 mole Al2(SO4)3 = 342.17 g Al2(SO4)3
1 mole Al2(SO4)3 = 6.022 x 1023 formula units Al2(SO4)3
1 mole Al2(SO4)3 = 2 moles Al3+ ions
1 mole Al2(SO4)3 = 3 moles (SO4)2- ions
1 mole Al2(SO4)3 = 12 moles O atoms = 12 x A.N. O atoms
1 mole Al2(SO4)3 = 3 moles S atoms = 3 x A.N. S atoms
1 mole Al2(SO4)3 = 2 moles Al atoms = 2 x A.N. Al atoms
Al2(SO4)3 (s)
Conversion Factors in a Molecular Formula
19
1 molecule of H2O = 2 H atoms and 1 O atom
Molecular mass = (2 x 1.008) + 15.99 = 18.00 amu
Molar mass = 18.00 g/mol H2O
1 mole of H2O = 6.022 x 1023 molecules of H2O
1 mole of H2O = 2 mol H atoms = 2 (6.022x1023) H atoms
1 mole of H2O = 1 mol O atoms = 1 (6.022x1023) O atoms
H2O (l)
Conversion Among Different Quantities
20
Practice Problem
21
1. Silver is often used in jewellery and tableware.
How many grams of Ag are in 0.0342 mol Ag?
2. Iron, the main component of steel, is the most
important metal in industrial society. How many
Fe atoms are in 95.8 g of Fe?
3. Urea, (NH2)2CO, is a nitrogen-containing
compound used as a fertilizer. How many
molecules of urea are in a 25.6 g sample?
4. How many hydrogen atoms are present in a
25.6 g sample of urea, (NH2)2CO?
Practice Problem
22
The plant photosynthetic pigment
chlorophyll contains 2.68% magnesium by
weight. How many atoms of Mg will there
be in 1.00 g of chlorophyll?
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