Introduction
to
Chemistry
Chapter 11
Student Learning Objectives
• Distinguish between physical & chemical properties
• Classify, compare, name, & identify
chemical quantities
• Recall properties of solubility
• Apply trends in the periodic table.
What is chemistry?
Chemistry is the study of microscopic properties.
Chemical properties
“Invisible”
How and why atoms combine into molecules
What are some physical and chemical properties?
Physical Properties
Chemical Properties
(Macroscopic)
(Microscopic)
• Density
• Phase
• Appearance
• Size
• Atomic make-up
• Structure
• Reactivity
Practice
1) How many different medicines exist for pain relief?
2) Is surface tension a microscopic or macroscopic
property of matter?
3) What does the image show?
Is it an example of a physical
or chemical property?
More Practice
4) Name the macroscopic properties of water.
5) Name the microscopic properties of water.
6) How do carbon dioxide (CO2) and water (H2O)
compare and contrast?
 The primary difference
between a physical
change and a chemical
change is that a chemical
change produces a new
substance.
Some Chemical
Change Indicators
Color change
Production of a Gas
Temperature Change
Light
Sound
How are elements, molecules, compounds
& mixtures defined?
Element
all of one type of atom
Molecule
Chemical bond
Molecular Formula
atoms in a chemical bond
attraction between atoms
relative numbers of atoms in bond
Question: What are the origins of the elements?
A compound contains two or more types of atoms.
Type
Number of Atoms
Diatomic
Triatomic
Polyatomic
2
3
4+
Practice
1) Which is not a compound?
2) How many atoms are contained in each?
3) Classify as diatomic, triatomic, or polyatomic.
H 2O
CaF2
NH3
O2
Classifying Mixtures
A substance that is pure has only one type of
element, or molecule, present.
Copper
Salt
A mixture contains two or more distinct types
of substances (atoms/molecules).
Homogeneous Mixture
Heterogeneous Mixture
 Same uniform appearance
and composition throughout
 Consists of visibly different
substances and/or phases
 Solution
(same phase)
 Suspension
(particles settle)
Practice: Classify Each Substance
7-up
Aluminum
Homogenized milk
Raw milk
Oil and water
Carbon monoxide
Distilled water
Air
Tap water
How can mixtures be separated?
Filtration
Distilation
Desalination
separate liquids and solids
separate gasses, liquids, solids
combines distillation and reverse osmosis
 Water may cross a semi-permeable
membrane. (Osmosis)
 Osmosis: from less to more concentrated
 Reverse osmosis: from more to less concentrated
Question
Why are distillation and desalination typically not used
to obtain fresh water from salt water?
What is solubility?
 Solubility is a measure of how much solute will dissolve
in a solvent to produce a stable solution.
Solvent (larger amount)
Solute (smaller amount)
Does the dissolving
Dissolves
Water & Sugar
Oil & Water
Liquids may be miscible or immiscible.
(mix or not mix)
 Solubility is variable.
•
•
•
•
•
Bond Strength
Bond Types
Temperature
Pressure
Molecular attractions
 Solubility has a limit,
based on each individual
substance and physical
conditions.
Concentrated
Dilute
Saturated
Concentration = Grams
Liter
Practice
1) If you cannot dissolve anymore sugar in your coffee,
your coffee is?
2) What is the concentration when 5 grams of sugar is
added to ½ a liter of water?
3) If you have 30 mL of 25% HCl solution, how many
grams of HCL are in the solution?
What are the basic trends in the periodic table?
 The periodic table is periodic!
 Most of the elements in the periodic table are metals.
Shiny
Opaque
Good Conductors
Trends
• Chemical reactivity decreases L  R
• Radius decreases along a period L  R
• Ionization energy increases along a period L  R
Practice
1) Which metals are liquid under normal atmospheric
conditions?
2) Which of the following would be most reactive?
a. O
b. He
c. Al
d. Cl
3) Which of the would have the smallest radius?
a. Al
b. Cl
 Atomic Periods (rows) are periodic.
 Atomic Groups (columns) have similar trends.
1 amu = 1.661 x 10-24 grams
Group
Name
Attributes
IA
IIA
Middle
IIIA
VIA
VIIA
VIIIA
Alkali Metals
Alkali Earth Metals
Transition Metals
Metalloids
Highly Reactive
Halogen Gases
Noble Gases
High Melting Point
Metals/ Non-metals
Ore Forming Elements
Salt Forming Elements
Non-Reactive
Emerald is a variety
of beryl, a mineral
that contains the
alkaline earth metal
beryllium.
 Lanthanides (58-71):
found in geologic zones
 Actinides (90-103): most
are synthesized in labs
A Uranium Rock
Practice
1) In which group are the precious metals?
2) List all attributes of Bromine (Br) that can be
determined using the periodic table.
What does the shell model indicate?
No two electrons can have the exact same energy state.
(Pauli Exclusion Principle)
 Electrons are arranged in particular orbitals
 Each electron has its own set of quantum numbers (n,l,ml, ms)
which determine the energy state of the electron
Atomic period indicates the number of main energy
shells available in the ground state.
Shell
n=1
n=2
n=3
n=4
n=5
n=6
n=7
Maximum e- Allowed
2
8
8
18
18
32
32
Practice
Draw the electron configuration for each atom.
(Assume atoms in ground state)
1. N
2. Kr
3. Mg
4. O
Valence Electrons
 Electrons attempt to have configurations that match those
in group VIIIA. (Octet Rule)
8 − Group Number = Number Unpaired e–
 Valence electrons are what make the physical and
chemical properties of the atoms in a group similar.
 More unpaired electrons = more reactive
 Unpaired valence electrons are used to form chemical bonds
What are some rules for naming compounds?
Compounds
 Metal is named first and then
the Non-metal
“Left” then “Right + ide”
NaCl = Sodium Chloride
HF = Hydrogen Fluoride
Prefixes
1.
2.
3.
4.
5.
6.
7.
8.
Mono
Di
Tri
Tetra
Penta
Hexa
Hept
Oct
CO2 = Carbon Dioxide
Polyatomic Ions
Polyatomic Ions are molecules made up of two or
more atoms that are considered an ionic group, that
have charge.
1. Name the cation (+ ion) first
2. Name the anion (- ion) second + ate
CaCO3
Calcium Carbonate
Practice
What is the chemical name?
Does it have a common name?
1. O2
5. SF6
2. H2O
6. CH4
3. KBr
7. NH3
4. O3
8. PCl5
Practice with Polyatomic Ions
What is the chemical name?
Does it have a common name?
1. AlPO4
2. Cu2SO4
3. KClO3
4. Fe(NO3)2
5. NaHCO3
6. NaH2PO4