matter and change
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Matter
and
Change P Squires
General Chemistry
2005-2006
Observing Chemical Change
• Open book to page 55 and conduct Discovery Lab
• (50 pts)
Properties of Matter
•What is a substance?
• Physical Properties
• Chemical Properties
Physical States
Solid
Liquid
Gas
Plasma
What are some characteristics
of each?
Give the physical state of each of these:
1. Silver
2. Gasoline
3. Helium
4. Rubbing alcohol
5. Air
6. Glass
7. Lightning
Solid
Liquid
Gas
Liquid
Gas
Solid or liquid
Plasma
Plasma
Physical Changes
• Physical changes only involve changes in state or
appearance.
• What are some examples of physical change?
Catch words for Physical Change
• Boil
• Freeze
• Melt
• Condense
• Break
•Split
•Grind
•Cut
•Crush
•Bend
Chemical Changes
• Chemical changes and chemical properties always produce new substances.
Chemical or physical change ???
• Food spoiling• Nail rusting• Oil burning• Sugar dissolving• Water boiling• Firefly flashing• Egg cooking• Snowflake melting
Chemical
Chemical
Chemical
Physical
Physical
Chemical
Chemical
Physical
Percent mass
Percent mass (%) = mass of element_ mass of compound
x 100
Calculations
1. A 78.0 g sample of an unknown compound contains 12.4 g of hydrogen. What is the percent by mass of hydrogen in the compound?
2. If 1.0 g of hydrogen reacts completely with 19.0 g of fluorine, what is the percent by mass of hydrogen in the compound that is formed?
Pure Substances
• Elements are the building blocks of matter.
• Atoms are the smallest part of an element.
Mixtures
… do not have a definite composition
… are either heterogeneous, with clearly visible components… or homogeneous,
which are uniform in appearance
Solutions
• Solutions are homogeneous mixtures containing a solute which is dissolved in a solvent.
Classify as heterogeneous, or homogeneous (solution)
• Blood
• Choc. chip ice cream
• Brass (Cu-Zn alloy)
• Homogenized milk
• Hummingbird food
Homogeneous
Heterogeneous
Homogeneous
Homogeneous
Homogeneous (solution)
We separate mixtures …
… based on differences in the chemical and physical
properties of the components in the mixture.
Separating Mixtures
• Quick Lab Handout
• (50 points)
How would you separate the following?
Aluminum filings and iron filings?
Saw dust and sand?
Salt and powdered charcoal?
Water and alcohol?
Elements
• A pure substance that can not be separated into simpler substance by physical or chemical means.
Compounds
• A combination of two or more different elements that are combined chemically.
• What are some examples of compounds?
The Law of Conservation of Mass
Matter can neither be created or destroyed
during a chemical reaction.
Law of Definite Proportions
Elements comprise compounds in definite proportions by mass.
Law of Multiple Proportions
When different compounds are formed, they combine in whole number ratios.
H2O H2O2
ChemLab
• Read and complete ChemLab
page 78. (100 points)
• Answer Questions at end:
Analyze and Conclude.
Structure of the Atom
Part of the Atom
• Electron
• Proton
• NeutronWhat charge does each have?
Where are they found?
Which ones make up the mass of the atom?
Which ones make up the size of the atom?
How Do Atoms Differ?•Atomic Number
•Atomic Mass
Element Atomic Number
Protons Electrons Atomic Mass
He 2
Pb 82
8
30
Mass Number
Number of neutrons = mass number – atomic number
Isotopes …
Therefore, isotopes of the same element have different masses.
…of the same element have the same number of protons and electrons but different numbers of neutrons.
Symbols for Isotopes
EA
Z
Symbol of Element
Mass number
Atomic number
A is the symbol for mass number
Z is the symbol for atomic number
MiniLab
• Do modeling isotope lab on page 102.
Energy and
Electrons
Light and Energy
• Frequency = f or f with units of Hertz (Hz)
• Wavelength = with units of meters (m)
What is the relationship between frequency and
wavelength?
For electromagnetic energy, the equation is:
c is the speed of light c = 3.00 x 108 m/sec
fc
Electromagnetic Spectrum
• Electromagnetic waves carry energy.
• Light is part of the electromagnetic spectrum
The Electromagnetic Spectrum
radi
o
TV
rada
r
mic
row
aves
infr
ared
visi
ble
ligh
t
ultr
avio
let
X-r
ays
gam
ma
rays
Shorter wavelengthHigher frequencyHigher energy
Longer wavelengthLower frequencyLower energy
The Electromagnetic Spectrum
radi
o
TV
rada
r
mic
row
aves
infr
ared
visi
ble
ligh
t
ultr
avio
let
X-r
ays
gam
ma
rays
400 nm 700 nm
Increasing energy
The visible spectrum was discovered by …
Dr. Roy G. Biv
Red Orange Yellow Green Blue Indigo Violet
700 nmLower energy
400 nmHigher energy
Niels Bohr
Bohr said that electrons could exist only in certain discrete energy levels …
… and that electrons can only change energy levels when they absorb or give off a certain amount of energy. (1913)
Hydrogen atom
nucleus
Discrete energy levels for electrons
electron
Hydrogen atom
Electrons can exist in this orbit,
Hydrogen atom
…or in this orbit,
Hydrogen atom
…or in this orbit,
Hydrogen atom
…but not in between the orbits.
Hydrogen atom
Unless the electron is absorbing energy, or …
Giving off energy
When high voltage is connected to the hydrogen discharge tube, a bluish light is given off.
When observed through a diffraction grating, specific lines of color are observed.
The electron in a hydrogen atom gains energy from the electricity passing thru the tube and …
… the electron moves up to a higher energy level.
The electron in the excited state is “unstable”.
The electron drops to a lower energy level, and …
… gives off light of a certain energy and wavelength.
Hydrogen atom
Hydrogen atom
energy
The electron absorbs energy and …
Hydrogen atom…the
electron is elevated
to the next energy level
The electron is unstable and
“wants” to return to a lower
energy level
Hydrogen atom
Hydrogen atom
Light of a particular wavelength is given off
HeliumHelium
NeonNeon
HydrogenHydrogen
“Regardless of it’s shortcomings and the
modifications that were later applied, Bohr’s model of the atom was the first successful attempt to make the internal structure of the atom agree with spectroscopic data.”
Asimov, 1964
Quantum Mechanical Model of the Atom
1. A small, dense positively charged nucleus which contains protons and neutrons.
2. Electrons which exist outside of the nucleus at …
– various distances from the nucleus, and at …
– various energy levels.
The Electrons
3. The electrons can have both a mass, as does matter, and a wavelength, as does light energy.
4. The electrons themselves are not little solid spheres in orbit around the nucleus, but exist as a “fog” of half-energy, half-matter. The electrons can behave as either matter or energy, depending on the experiment.
Energy Levels
5. Based on the ideas of Bohr, the electrons are located …
– … in major energy levels,– … in energy sublevels within major
energy levels, – … in orbitals within each sublevel.
Next up….
The Periodic Table