chemistry 103 lecture 12. outline i. covalent bonding lewis dot diagrams/nomenclature (in review) ...
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Chemistry 103
Lecture 12
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Outline
I. Covalent Bonding Lewis Dot Diagrams/Nomenclature (in review) Bond/Molecular Polarity
II. Counting in Chemistry (CH8) The Mole/Avogadro’s Number
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Ionic vs. Covalent
NaCl (sodium chloride) CH4 (methane)
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4
Learning Check
Name each of these compounds.
A. SO3
B. MnCl2
C. (NH4)3PO4
D. Cu2CO3
E. N2O4
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Bonds and reality
Ionic Covalent
(e-transfer) (e- shared)
NaCl H2
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Bonds and reality
Ionic uneven e- sharing covalent
(e-transfer) (e- shared)
NaCl HCl H2
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Even vs. Uneven sharing of bonding electrons
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
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Bond Polarity
Bond Polarity: a measure of the degree of inequality in the sharing of electrons between two atoms in a chemical bond
The positive end (or pole) in a polar bond is represented + and the negative pole -. The negative end is toward the atom with the higher
electronegativity Example: HCl
H Cl
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Polar v. Nonpolar Bonds
Polar covalent bonds (example: HCl) A covalent bond in which there is unequal sharing
of electrons between two atoms.
Nonpolar covalent bonds (example: H2) A covalent bond in which there is equal sharing of
electrons between two atoms
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Electronegativity
A measure of the relative attraction that an atom has for the shared electrons in a bond Electrons are pulled closer to the atom with the
higher electronegativity
Cl-
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Trends in Electronegativity
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Electronegativity Trends in electronegativity
Electronegativity values increase from left to right on the periodic table
Electronegativity values increase from the bottom to the top of the periodic table
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Range of Bond Types
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Some Rules of Thumb about Bond Polarity If a bond is between two of the same kinds of atoms:
It will be NONpolar
If a bond is between two different atoms: It will be polar to some degree (more so the further apart the two
atoms are on the periodic table) An important exception: C-H bonds are nonpolar
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Some Rules of Thumb about Bond Polarity
RULES: Electronegativity difference between the two
elements in a bond is 0.0 to 0.4 nonpolar covalent. (your book’s convention)
Electronegativity difference between the two elements that make a bond is 1.8 or greater, bond considered ionic
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Polar Bonds?
Example: NaF
Example: O2
Example: NH3
Example: HCl
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Molecular Polarity
A measure of the degree of inequality in the attraction of bonding electrons to various locations within a molecule
Polar Molecule: A molecule in which there is an unsymmetrical distribution
of charge
Why do we care if the molecule is polar? Polar molecules dissolve in polar solvents (like water or
blood) Nonpolar molecules dissolve in nonpolar solvents (like
hexane or cell membranes)
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Molecular Shape and Molecular Polarity For a molecule to be polar:
1. It must contain polar bonds 2. The molecular geometry must not
cancel out the effect of the polar bonds (through vector addition)
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Polar Bonds and Nonpolar Molecules
For example, the bond dipoles in CO2 cancel each other because CO2 is linear.
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Polar Bonds and Polar MoleculesIn water, the molecule is not linear
and the bond dipoles do not cancel each other.Therefore, water is a polar molecule.
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Chemical Quantities
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Atomic Mass
Atomic mass is the Mass of a single atom
in atomic mass units (amu)
Mass of an atom compared to a 12C atom
Number below the symbol of an element
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Periodic Table and Atomic Mass
Ag has atomic mass = 107.9 amu
C has atomic mass = 12.01 amu
S has atomic mass = 32.07 amu
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Molecular and Formula Mass Atomic mass unit (amu) = the unit of mass for
atoms Molecular mass is the sum of the masses of
all atoms in a molecule Formula mass is the sum of the masses of
all atoms in a formula unit of an ionic compound (or molecule - used interchangeably)
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Formula MassThe formula
mass is The mass in
amu of a compound
The sum of the atomic masses of the elements in a formula
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Calculating Formula MassTo calculate formula mass of Na2SO4, Multiply the atomic mass of each element by its subscript Total the masses
2 Na x 22.99 amu = 45.98 amu Formula mass
1 Na Na2SO4
1 S x 32.07 amu = 32.07 amu 142.05 amu1 S
4 O x 16.00 amu = 64.00 amu1 O
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Atomic masses in Grams
107.9g of Ag. How many Ag atoms?
12.01g of C. How many atoms of C?
32.07g of S. How many S atoms?
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The “gram” mass of certain elements from the Periodic Table
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Counting Particles by Mass
Experimentally know conversion:
1 amu = 1.66053 x 10-24 g
Let’s say we want to use the atomic mass number in the periodic table in a way useful for experimentation in the lab - grams units
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Counting Particles by Mass
1 amu = 1.66053 x 10-24 g
C (ave atom) 12.01g - how many atoms of C are in this gram quantity using the conversion above?
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Counting Particles by Mass
1 amu = 1.66053 x 10-24 g
C (ave atom) 12.01g - how many atoms of C are in this gram quantity using the conversion above?
12.01g C x ( 1 amu___ ) x ( 1 ave C atom) 1.66053x10-24 g 12.01 amu
= 6.022 x 1023 C atoms
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The MOLE
Chemists’ counting unit
6.022 x 1023 “anything”
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Avogadro’s Number
Solution = 6.022 x 1023
Avogadro’s number is equal
to 1 mole Makes working with large numbers
easier
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Familiar Collection Terms
A collection term statesa specific number of
items. 1 dozen donuts
= 12 donuts 1 ream of paper
= 500 sheets 1 case = 24 cans
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
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Avogadro’s number 6.022 x 1023 can be written as an
equality and two conversion factors.
Equality:1 mol = 6.022 x 1023 particles
Conversion Factors:
6.022 x 1023 particles and 1 mol___ 1 mol 6.022 x 1023 particles
Avogadro’s Number
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Calculations with Avogadro’s Number
A Tums tablet has 7.224 x 1023 atoms of Ca. How many moles is this?
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Subscripts State Atoms and Moles
1 mole aspirin 9 mol C 8 mol H 4 mol O
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Parts of the Whole
How many “C” atoms are in 125 molecules of C2H2?
How many moles of “C” atom are in 3.0 moles of C2H2?
How many individual “C” atoms are in 3.0 moles of C2H2?
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Molar Mass from Periodic TableMolar mass • Is the atomic
mass expressed in grams
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Molar Mass
The molar mass • Is the mass of one mole of
an element or compound• Is the atomic mass
expressed in grams
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
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Give the molar mass for:
A. 1 mol K atoms = 39.10 g
B. 1 mol Sn atoms = 118.7 g
Solution
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Molar Mass of a Compound
The molar mass of a compound is the sum of the molar masses of the elements in the formula.
Example: Calculate the molar mass of CaCl2.
Element Number of Moles
Atomic Mass Total Mass
Ca 1 40.08 g/mol 40.08 g
Cl 2 35.45 g/mol 70.90 g
CaCl2 110.98 g
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Molar Mass of K3PO4
Calculate the molar mass of K3PO4.
Element Number of Moles
Atomic Mass Total Mass in K3PO4
K 3 39.10 g/mol 117.3 g
P 1 30.97 g/mol 30.97 g
O 4 16.00 g/mol 64.00 g
K3PO4 212.3 g
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Some One-Mole Quantities
32.07 g 55.85 g 58.44 g 294.20 g 342.30 g
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Molar mass factors are used to convert between the grams of a substance and the number of moles.
Calculations Using Molar Mass
Grams Molar mass factor Moles
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Molar mass conversion factors: • Are written from molar mass• Relate grams and moles of an element or compound.
Example: Write molar mass factors for methane CH4 used
in gas cook tops and gas heaters.
Molar mass:
1 mol CH4 = 16.04 g
Conversion factors:
16.04 g CH4 and 1 mol CH4
1 mol CH4 16.04 g CH4
Molar Mass Factors
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Aluminum is often used to build lightweight bicycle frames. How many grams of Al are in 3.00 mol Al?
Moles to Grams
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Aluminum is often used to build lightweight bicycle frames. How many individual Al atoms are in 3.00 mol Al?
Moles to Individual Particles
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Subscripts State Atoms and Moles
1mole aspirin 9 mol C 8 mol H 4 mol O
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Learning Check
Calculate the number of moles of aspirin (C9H8O4) in 52.1 g of aspirin (C9H8O4).