Matter
Matter
Anything that has _____ and takes up
____.
Matter is made of atoms. Atoms are the
basic UNIT of matter.
Circle the word or phrase that describes an
example of matter.
Proton
lava
air
light electrons
Bria concepts catsup
water vapor thoughts
atom
your breath
ideas
heat
quark
Mira
decisions
a vacuum motion something
(empty space)
without mass
molecule
something that
takes up space
mixture
Atoms are made of
protons, neutrons and
electrons.
The word atom
derives from the
Greek (ατομοζ) for
indivisible.
PROTON
A __________
charged particle found in the ______________.
NEUTRON
A particle in the ________________ with
____
charge (neutral). It has the ______________
mass as a proton.
ELECTRON
A ________________ charged particle found
___________________ the nucleus in a region
called the _______________ ______________.
http://phrenopolis.com/perspective/atom/
(scale of proton vs electron)
NUCLEUS
The center of an atom containing the
_______________ and _________________.
ELECTRON CLOUD
The region surrounding the nucleus of an
atom where _____________ are found.
The Bohr model of the
atom
Each “ring” is called a _________.
These are also called stationary states.
http://www.upscale.utoronto.ca/GeneralInterest/Har
rison/BohrModel/Flash/BohrModel.html (animated
Bohr model)
Element song=
http://www.privatehand.com/flash/elements.html
Helium
Lithium
Beryllium
Boron
2 protons, 2 neutrons and 3 protons, 4 neutrons and 4 protons, 5 neutrons and 5 protons, 6 neutrons and
2 electrons
3 electrons
4 electrons
5 electrons
Valence Shell
The valence shell is the outermost shell of an atom.
Shells #1 holds - 2 electrons max,
#2 -8 electrons max
#3 -18 electrons max
http://www.ndt-ed.org/EducationResources/HighSchool/Electricity/valenceshell.htm
Electron Shells
Electrons are arranged around the Nucleus in SHELLS. For simplicity they can be thought of like miniplanets orbiting a central sun, but it is closer to the truth to think of them as "clouds" of electric charge
around the Nucleus.
The shells are numbered outward from the Nucleus. The maximum number of electrons found in each
shell can be calculated by:
where "n" is the number of the shell.
Maximum
Shell
Number
Number of Electrons in the
Shell
1
2x1=2
2
2x4=8
3
2 x 9 = 18
4
2 x 16 = 32
5
2 x 25 = 50
The Octet Rule:
In general, atoms are most stable when they have 8 electrons in their outer-most shell. (Octet means 8.)
The exception is the first shell which is most stable with TWO electrons. If you know the Atomic Number
and Mass Number of an element and the maximum number of electrons in each electron shell you can
draw a diagram of the element.
For example: Sodium has an Atomic Number of 11 and an Mass Number of 23 ie
This means an atom of Sodium has 11 Protons and therefore 11 electrons.
Since the number of Protons + Neutrons is 23 and there are 11 Protons there must be 12 Neutrons.
From the table above the electrons are arranged as: First Shell = 2, Second Shell = 8, Third Shell = 1
(Giving a total of 11.)
Shells, More Accurately…………..2,8,8,18,18,32
As atomic number increases so too does the number of
electrons in a neutral atom of the element. The valence electrons
are largely responsible for its chemical behavior. If elements
having the same number of valence electrons are grouped
together the elements in each group or family will have similar
chemical properties.
The first short period contains only two elements. These
elements fill the K shell. It ends with helium which contains a full K
shell consisting of two electrons. 2
The second short period contains eight elements beginning
with lithium and ending with neon. Neon has a complete L shell of
eight electrons.
8
The third short period contains eight elements beginning with
sodium. It ends with argon, which contains eight electrons in the
M shell.
8
The fourth period contains eighteen elements beginning with
potassium. It includes a series of elements from scandium
through copper. These elements are known as transition
elements. 18
They are building the M shell from eight to eighteen electrons.
Before this series begins though two electrons enter the
outermost N shell. After the series the N shell then builds up to
eight electrons ending with krypton.
The fifth period is just like the fourth period in which the O
shell takes two electrons then the N shell builds to eighteen
electrons before the O shell continues out to eight electrons
ending with xenon. 18
The sixth period contains 32 elements. It too has a transition
series beginning with lanthanum and ending with gold, in which
the O shell fills to eighteen electrons. 32
Note however that this series is split after lanthanum with a
series of fourteen elements. In these elements the N shell (third
from the outside) is filling from eighteen to 32 electrons. These
are referred to as the inner transition series, lanthanum series
or the rare earth elements. It begins with cerium and ends with
lutetium.
http://www.corrosionsource.com/handbook/periodic/e_shells.htm
Following lutetium the transition series from hafnium to gold completes by building the O shell to eighteen
electrons. The outer P shell then continues to build to eight electrons ending with radon.
The seventh period is incomplete. The first two elements, francium and radium fill the Q shell with
two electrons. Then the P and O shells fill in the same way as the sixth period. This produces the
actinide series.
ATOMIC MASS/WEIGHT
The number of protons and neutrons found
in the nucleus of an atom.
Particle
Location
Charge
Mass
Neutron
Nucleus
None
1.008665
amu
Proton
Nucleus
+1
1.007277
amu
Electron
Shells
around the
nucleus
-1
0.0005486
amu
QUARKS
Six "flavours" quarks: up, down, bottom, top, strange,
and charm
Elements
A material is an element if all its atoms are
the same.
Something is not an element if it contains
different types of atoms.
Elements differ by the number of protons
they contain. This number tends to equal the
same number of electrons.
PERIODIC TABLE 1869
“The BIG DADDY”
OF THE PERIODIC
TABLE
If he was a
rapper, he would
have been called
Heavy D.
Dmitri Ivanovich
Mendeleev (1834-1907)
Mendeleev’s first sketch of a
periodic table of the elements
Lithium reaction
http://www.youtube.com/watch?v=wY0afMI4Jgc&annotatio
n_id=annotation_780828&feature=iv
Synthetic elements are created using
particle accelerators.
A particle accelerator (or atom smasheris a device that uses electric fields to propel
electrically-charged particles to high speeds and to contain them.
A new particle accelerator, the Large Hadron Collider near Geneva,
Switzerland. (Credit: CERN). 27-kilometer Particle Accelerator
http://news.yahoo.com/s/ap/20091123/ap_on_sc/eu_sci_big_bang
_machine
It has massive magnets cooled 1.9 degrees Kelvin (that's cold) .
Fermilab
Aerial photo of the Tevatron at Fermilab. The main accelerator is the ring above; the one below
(about one-third the diameter, despite appearances) is for preliminary acceleration, beam cooling and
storage, etc. http://en.wikipedia.org/wiki/Particle_accelerator
http://gemologyproject.com/wiki/index.php?title
Click table contents=The_Chemistry_of_Gemstones
http://elements.wlonk.com (picture and word table)
Rows called PERIODS; arranged by atomic number =
#protons
horizontal
Columns called FAMILIES; grouped by similar properties
vertical
Element Symbols
Hydrogen
Copper
Carbon
Nitrogen
Chlorine
Iron
Silicon
Sulfur
OxygenCalcium
Top Elements in
Top Elements in Earth
Crust
our Body
Oxygen 65%
Oxygen 47%
Carbon 18%
Hydrogen 10%
Silicon
28%
Aluminum 8%
Top Elements in the
Top Elements in Oceans
Atmosphere
Nitrogen 78%
Oxygen 86%
Oxygen
Hydrogen 10%
21%
Argon <1%
Chlorine
Human Body Elements by %
Element
Percent by mass
Oxygen
65
Carbon
18
Hydrogen
10
Nitrogen
3
Calcium
1.5
2%
Phosphor
us
1.2
Potassium
0.2
Sulfur
0.2
Chlorine
0.2
Sodium
0.1
EARTH’S CRUST ELEMENTS
The 8 most common elements in Earth’s crust (by mass):
46.6% Oxygen (O)
27.7% Silicon (Si)
8.1% Aluminum (Al)
5.0% Iron (Fe)
3.6% Calcium (Ca)
2.8% Sodium (Na)
2.6% Potassium (K)
2.1% Magnesium (Mg)
EARTH’S ATMOSPHERE ELEMENTS
Components of
(volume)
dry air
Nitrogen
78.0842%
Oxygen
20.9463%
Argon
0.9342%
Elements in the Oceans
Oxygen
85.84%
Hydrogen
10.82
Chlorine
1.94
Sodium
1.08
Phases of Matter
The key word to notice is physical. Things only move from one phase to another by
physical means.
Solid:
A solid is matter in which the molecules are very close
together and
cannot move around. Examples of solids include rocks, wood, and ice
(frozen water).
Liquid:
A liquid is matter in which the molecules are close together and move around slowly.
Examples of liquids include drinking water, mercury at room temperature, and lava
(molten rock).
Gas:
A gas is matter in which the molecules are widely separated, move around
freely, and move at high speeds. Examples of gases include the gases we breathe
(nitrogen, oxygen, and others), the helium in balloons, and steam (water vapor).
Plasma:
A plasma is a gas that is composed of free-floating ions (atoms stripped of some
electrons - positively charged) and free electrons (negatively charged). A plasma
conducts electrical currents. Plasma was discovered by William Crookes in 1879.
There are many different types of plasmas. There is plasma in stars (including our
Sun), and the solar wind in our Solar System is made of plasma.
http://www.enchantedlearning.com/physics/Phasesofmatter.shtml
http://www.miamisci.org/af/sln/phases/index.html
MIXTURE
A type of matter made up of substances that
are physically combined.
EX: tossed salad, sugar ice tea
COMPOUND
A type of matter made up of elements
chemically combined.
EX: salt, water, carbon dioxide
PHYSICAL PROPERTY
The properties that can be observed
without changing the chemical
makeup/characteristics.
EX: color, luster, malleability, brittleness,
odor, taste, density, texture, hardness,
electrical conductivity, heat conductivity,
boiling melting and freezing point.
PHYSICAL CHANGE
(no new substance)
Occurs when the physical properties of a
substance changes but no new substance is
formed.
Mixtures may be formed or separated
through physical changes.
1. A change that affects the appearance of
a substance, but does not affect the
composition or chemical properties.
2. Molecules are unchanged.
3. Original substance is still there with only
new physical properties.
4. No new substance is formed.
Examples : evaporating, melting, freezing,
sublimating OR:
Sharpening a pencil
Cut up an apple
Grinding a rock into powder
Dissolving sugar in water
Drying your clothes
Breaking glass
DENSITY
The amount of matter (stuff) in a given
volume (space). It is a physical property of
all matter.
Amount of mass compared to amount of
space taken up (volume). M/V
Mass
Volume
e
Volume is the amount of space an object
takes up.
Can be measured using: graduated cylinder
Ruler/meter stick (LxWxH)
Units of density are: g/mL or g/cm
It is
concept
3
an important
regarding
buoyancy.
http://www.karlyoder.com/flash_density.html (virtual density lab)
The SI unit for density is:
kilograms per cubic meter
(kg/m³) or
g/mL or g/cm3
http://www.world-builders.org/lessons/less/les1/weight_mass.html
Densities of Substances
Substances
Density (kg/m3)
Solids
Substances
Density (kg/m3)
Liquids
Aluminum
2.70 x 10 3
Water (4oC)
1.00 x 10 3
Iron and Steel
7.8 x 10 3
Blood, plasma
1.03 x 10 3
Copper
8.9 x 10 3
Blood, whole
1.05 x 10 3
Lead
11.3 x 10 3
Sea water
1.025 x 10 3
Gold
19.3 x 10 3
Mercury
13.6 x 10 3
Concrete
2.3 x 10 3
Alcohol, ethyl
0.79 x 10 3
Granite
2.7 x 10 3
Wood (typical)
0.3 ~ 0.9 x 10 3
Glass, common
2.4~2.8 x 10 3
Gases
Ice
0.917 x 10 3
Air
1.29
Bone
1.7~2.0 x 10 3
Helium
0.179
Carbon dioxide
1.98
Gasoline
Water (steam
100oC)
0.68 x 10 3
0.598
http://www.angelfire.com/nc3/pweb/charts/density.htm
Chemical Property: a description of how the
matter reacts with other substances.
Example: flammable, reacts with air, reacts
with water, does not react
CHEMICAL CHANGE
Compounds may be formed or broken down
through chemical changes.
The following may occur during a chemical
change:
heat or light is produced
gas is produced (bubbling)
a change of color
a solid is formed(precipitate)
1. Change in matter in which one substance is
_____________________into another
substance.
2. Molecules ________________.
3. Original substance is _____________.
4. An entirely ___________substance is
formed with new physical and new chemical
properties.
Chemical Change Examples:
Rusting or corrosion of any metal (tarnish,
metals reacting with air)
Digestion
Respiration(animals)/Photosynthesis(plants)
Burning anything
A battery producing electricity
Spoiling of food or cooking food
CHEMICAL CHANGE (cont.)
Rotting Plant material
Growth
Acids and Bases reacting
Metals reacting in water
Law of Conservation of Matter (Mass)
Matter (mass) is not created nor destroyed
in an ordinary chemical reaction.
COMPOUNDS
Compound*
*Molecule
Matter that is made up of two or more elements (atoms)
_________________________combined and cannot be
separated by physical means.
The molecule is the smallest unit of a ____________________.
Compound Facts:
The elements that make up a compound are
combined.
chemically
A compound has different
the elements that make it up.
chemical properties than
Energy is always used/applied when a compound is broken
up or put together.
It takes another chemical reaction to change/create
new
a
compound.
The ratio of the elements that make up a compound are always
the same for that compound.
Example: water is always
atom.
2hydrogen atoms and 1oxygen
Parts of a compound:
compound formula(david)
compound name
CO2 = carbon dioxide
subscript
_________ (how many atoms are present)*
*When there is no subscript written, it is assumed that the subscript is 1
A chemical equation uses chemical formulas of elements and compounds
to represent a chemical
change.
Parts of a Chemical Equation
coefficient
2Na + Cl2
reactants
Yields(energy applied)
2NaCl
products
subscript
Balanced equations…. Or not?
Remember ….. reactant + reactant
1. S8 + O2
product
SO3
2. FeCl3 + NaOH
3. HCl + CaCO3
Fe(OH)3 + NaCl
CaCl2 + H2O +CO2
4. C12H22O11 + O2
5.
CO2 + H2O
What is the chemical name for the following compounds?
Word bank:
Sugar
Salt
rust
water
1. H2O _______________________
2. NaCl ______________________
3. Fe2O3 _______________________
hydrogen peroxide
carbon dioxide
4. CO2 _________________________
5. H2O2 ________________________
6. C12H22O11 ____________________
COMPOUNDS OR ELEMENTS?
C=compound E= element
Use your periodic table to determine if the following is an element or compound.
_____1. carbon
_____2. carbon dioxide
_____3. oxygen
_____4. fluorine
_____5. sodium fluoride
_____6. hydrogen
_____7. vinegar
_____8. sodium
_____9. chlorine
____10. sodium chloride
____11. baking soda
____12. sugar
____13. lithium
____14. rust
True or False:
_____ 1. Compounds are made up of only one type of atom.
_____ 2. Compounds can be found on the periodic table.
_____ 3. Subscripts are used in compounds to determine the number of elements in the
compound.
_____ 4. You can separate a compound by a physical change.
_____ 5. It takes a chemical change to form a compound.
_____ 6. The proportions of the elements that make up a compound can change and you
would still have the same compound.
Venn Diagram: Compare Elements to Compounds
Make up your own riddle:
Pick a compound that you already know, or choose one from the list
and come up with a four line poem that rhymes, The students will try
to guess what compound you are talking about.
1. NaCl
2. CaCO3
3. N2O
4. MgSO4
5. FeS2
6. CH4
7. CaSO4
8. SiO2
9. KNO3
10. NaHCO3
11. CaSO4
12. NaF
13. H2O
14. Na2B3O7
15. H4Mg3Si2O9
16. HC2H3O2
17. NH4OH
18. CO
19. CO2
20. C12H22O11
(salt)
(chalk or marble)
(nitrous oxide or laughing gas)
(Epsom salt)
(iron sulfide – fools gold)
(methane)
(plaster of paris)
(quartz or sand)
(saltpeter – used to make gun powder))
(baking soda)
(gypsum)
(sodium fluoride)
(water)
(borax)
(talc)
(vinegar)
(ammonia)
(carbon monoxide)
(carbon dioxide, dry ice)
(sugar)
Compare Contrast
Elements
Compounds
.
.
Chemical Reactions
Reactants
# of atoms here
Product
=
So, it’s balanced!
# of atoms here
Solubility- mixing of two or more
substances together in solution. Simply
defined, it is a measure of how much solute
will dissolve into the solvent. Not all
substances will dissolve in all solvents.
Solubility is the property of a
solid, liquid, or gaseous chemical
substance called solute to
dissolve in a liquid solvent to form
a homogeneous solution.
Solvent-the greater amount
Solute-the lesser amount
Miscibility- the property of
liquids to mix in all
proportions, forming a
homogeneous solution.
Solubility of a substance strongly depends on
the used solvent as well as on temperature and
pressure. Solubility increases with
temperature(energy) increase. Decreases with
temperature (energy) decrease. Similar concept
for pressure.
A solution is said to be SATURATED if no more
solute can dissolve in the solvent.
ISOTOPES
The number of protons determines what the element
the atom is. However, it is possible for an element to
exist in more than one form by having greater or fewer
neutrons in the nucleus. The different forms of the same
element are known as isotopes of an element. Most
elements have a few stable isotopes and a few unstable
isotopes. For example: Carbon exists in 15 isotopes with
the most common forms being the stable C-12,C-13 and
the unstable or radioactive C-14.
Fission
In 1905, in his theory of Special Relativity, Einstein proposed that
mass and energy were indeed equivalent. They are linked by the
immortal formula E = mc2, where E = energy, m = mass, and c = the
speed of light (300,000 kms-1). Thus, a certain quantity of energy is
equivalent to a certain mass. However, even a small amount of mass
is equivalent to a massive quantity of energy.
So, one can see that the mass of the nucleus, and the energy
required to bind it are just different types of the same thing. For each
atom, the mass and binding energy are inversely proportional; that is,
if you increase one, the other must be decreased to minimise energy
expenditure.
OR
http://www.users.bigpond.com/sinclair/fission/Fission2.html
Thus, there are two ways of splitting the atom (scission): either by
increasing its energy, or by increasing its mass.
However, the energy needed to split an atom is enormous, and this
is not a practical possibility. The usual result when a nucleus becomes
excited (extra energy added) is that gamma or beta rays are released
to reduce energy. In other cases where the nucleus is unstable, alpha
or beta particles are released to reduce mass, rather than the atom
splitting. An alpha particle is a helium nucleus (4He), and a beta
particle is a single electron. By releasing mass, the atom is able to
reduce energy, and become stable again.
The other method (adding mass) is achieved by bombarding a
suitable nucleus with neutrons. Suitable nuclei are those with
fissionability parameters close to 1 (e.g. 235U = 0.8). By adding an extra
neutron to the nucleus, mass is increased, and binding energy is
consequently reduced to conserve energy. When the binding energy is
reduced, the electrostatic repulsion within the nucleus is greater than
the binding energy, and the nucleus splits apart.
Top: Expected results: alpha particles passing through the plum pudding model of the atom
undisturbed.
Bottom: Observed results: a small portion of the particles were deflected, indicating a small,
concentrated positive charge.
The Geiger–Marsden experiment (also called the Gold foil
experiment or the Rutherford experiment) was an experiment to
probe the structure of the atom performed by Hans Geiger and Ernest
Marsden in 1909, under the direction of Ernest Rutherford at the
Physical Laboratories of the University of Manchester. The unexpected
results of the experiment demonstrated for the first time the existence
of the atomic nucleus, leading to the downfall of the plum pudding
model of the atom, and the development of the Rutherford (or
planetary) model.
A beam of alpha particles, generated by the radioactive decay of
radium, was directed normally onto a sheet of very thin gold foil. The
gold foil was surrounded by a circular sheet of zinc sulfide (ZnS) which
was used as a detector: the ZnS sheet would light up when hit with
alpha particles. Under the prevailing plum pudding model, the alpha
particles should all have been deflected by, at most, a few degrees;
measuring the pattern of scattered particles was expected to provide
information about the distribution of charge within the atom. However
they observed that a very small percentage of particles were deflected
through angles much larger than 90 degrees. According to Rutherford:
It was quite the most incredible event that has ever happened to me
in my life. It was almost as incredible as if you fired a 15-inch shell at a
piece of tissue paper and it came back and hit you. On consideration, I
realized that this scattering backward must be the result of a single
collision, and when I made calculations I saw that it was impossible to
get anything of that order of magnitude unless you took a system in
which the greater part of the mass of the atom was concentrated in a
minute nucleus. It was then that I had the idea of an atom with a
minute massive centre, carrying a charge