Embed Size (px)
Citation preview
SOL 6.4 The student will investigate and understand that all
matter is made up of atoms. Key concepts include
a) atoms consist of particles, including electrons,
protons, and neutrons;
b) atoms of a particular element are alike but are
different from atoms of other elements;
c) elements may be represented by chemical symbols;
d) two or more atoms interact to form new substances,
which are held together by electrical forces (bonds);
e) compounds may be represented by chemical formulas;
f) chemical equations can be used to model chemical
changes; and
g) a limited number of elements comprise the largest
portion of the solid Earth, living matter, the oceans,
and the atmosphere.
Matter Matter http://quizizz.com/admin/quiz
/571f57f2c5ce8daa34e22198 Review game for the unit
Anything that has MASS and takes up
SPACE.
https://www.youtube.com/watch?v=QG
ytW_C6hR8#t=2.690087 7 min strongest magnet
Matter is made of atoms. Atoms are the
basic UNIT of matter. https://www.youtube.com/watch?v=khy
mS6V_mn0 8:43 10 strangest elements
http://www.youtube.com/watch?v=BhWgv0STLZs&feature=watch-vrec&safety_mode=true&persist_safety_mode=1&safe=active&list=PL4DBBF2210573C31F cartoony history of atom theory
Circle the word or phrase that describes an example of matter.
Proton lava air light electrons Evan concepts catsup water vapor thoughts atom your breath ideas heat quark
Alexa decisions a vacuum motion something (empty space) without mass molecule something that mixture takes up space
Atoms are made of protons, neutrons and electrons.
The word atom derives from the Greek (ατομοζ) for indivisible.
PROTON A positively charged particle found in the
nucleus. NEUTRON A particle in the nucleus with no
charge (neutral). It has the same mass as a proton.
ELECTRON A negatively charged particle found outside
the nucleus in a region called the electron cloud
http://phrenopolis.com/perspective/atom/
(scale of proton vs electron)
NUCLEUS The center of an atom containing the
protons and neutrons. ELECTRON CLOUD The region surrounding the nucleus of an
atom where _____________ are found. http://www.khanacademy.org/video/eleme
nts-and-atoms?playlist=Chemistry atom video
http://www.youtube.com/watch?v=Vi91qyjuknM&feature=watch-vrec&safety_mode=true&persist_safety_mode=1&safe=active
atom video. Protons, neutrons, electrons and quarks 7:44
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)
http://periodictable.com/ photo images of elements.nice
Element song=
http://www.privatehand.com/flash/elements.html http://www.privatehand.com/flash/oxygen.html
Helium
2 protons, 2 neutrons and
2 electrons
Lithium
3 protons, 4 neutrons and
3 electrons
Beryllium
4 protons, 5 neutrons and
4 electrons
Boron
5 protons, 6 neutrons and
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 mini-
planets 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.
Shell Maximum
Number Number
of Electrons in the
Shell
1 2 x 1 = 2
2 2 x 4 = 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
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.
Carbon Diamond Coal Graphite
Simple Idea: If all the atoms are the same, it is one element. If you have more than one type of atom, you have different elements. PERIODIC TABLE 1869
Dmitri Ivanovich Mendeleev (1834-1907)
“The BIG DADDY” OF THE PERIODIC TABLE
Mendeleev’s first sketch of a periodic table of the elements
If he was a rapper, he would have been called
Heavy D.
http://www.npr.org/sections/thetwo-way/2016/01/04/461904077/4-new-elements-are-added-to-the-periodic-table New elements recognized Jan 2016
https://www.youtube.com/watch?v=UeQdIRuIi4Q&feature=youtu.be
Mr Hein discussion of periodic table
Lithium reaction
http://www.youtube.com/watch?v=wY0afMI4Jgc&annotation_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
http://www.foxnews.com/science/2014/11/21/never-before-seen-particles-discovered-at-swiss-collider/
http://www.ck12.org/concept/Chemical-Bonding/?ref=%2Fconcept%2FChemical-Bonding%2F
It has massive magnets cooled 1.9 degrees Kelvin (that's cold) .
http://www.youtube.com/watch?v=TgWd_O8juoU Large Hadron Collider(LHC) Big Bang Theory
58 minutes . Very understandable. Watch it in pieces if too long
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
our Body
Top Elements in Earth Crust
Oxygen 65%
Oxygen 47%
Carbon 18%
Silicon 28% Hydrogen 10%
Aluminum 8%
Top Elements in the
Atmosphere
Top Elements in Oceans
Nitrogen 78%
Oxygen 86%
Oxygen 21%
Hydrogen 10%
Argon <1%
Chlorine 2%
Human Body Elements by %
Element Percent by mass
Oxygen 65
Carbon 18
Hydrogen 10
Nitrogen 3
Calcium 1.5
Phosphorus
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.
http://www.youtube.com/watch?v=uJOGy0
dgmUU&safety_mode=true&persist_safety_mode=1&safe=active video 3 min physical vs chemical properties
http://www.youtube.com/watch?v=3MnAPDyfgLs&safety_mode=true&persist_safety_mode=1&safe=active nice 9 min video on physical vs chemical properties
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 http://www.youtube.com/watch?v=qqqmFFCwd7k&safety_mode=true&persist_safety_mode=1&safe=active physical vs chemical change
http://www.youtube.com/watch?feature=e
ndscreen&v=gCbqjs-pqJo&NR=1&safety_mode=true&persist_safety_mode=1&safe=active physical vs chemical change. Guns and Roses music 3:22
http://www.youtube.com/watch?NR=1&v=hcunQqbNEMQ
&feature=endscreen&safety_mode=true&persist_safety_mode=1&safe=active Physical vs Chemical change 3:46
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
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/cm3
It is an important concept regarding buoyancy.
Mass
Volumee
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) Substances Density (kg/m3)
Solids
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
Gasoline 0.68 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
Water (steam
100oC) 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
http://www.youtube.com/watch?v=UkBhW8Kj3r8&safety_mode=true&persist_safety_mode=1&safe=active chemical reactions 3:48
CHEMICAL CHANGE http://www.youtube.com/watch?v=qqqmFFCwd7k chemical vs physical 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* Matter that is made up of two or more elements (atoms)
_________________________combined and cannot be separated by physical means.
*Molecule The molecule is the smallest unit of a ____________________.
Compound Facts:
The elements that make up a compound are chemically combined.
A compound has different chemical properties than
the elements that make it up.
Energy is always used/applied when a compound is broken
up or put together.
It takes another chemical reaction to change/create a new compound.
The ratio of the elements that make up a compound are always
the same for that compound.
Example: water is always 2hydrogen atoms and 1oxygen
atom.
Parts of a compound:
compound formula(david) compound name
CO2 = carbon dioxide _________ (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
2Na + Cl2 2NaCl reactants products subscript Balanced equations…. Or not? Remember ….. reactant + reactant product
1. S8 + O2 SO3
Yields(energy applied)
coefficient
subscript
2. FeCl3 + NaOH Fe(OH)3 + NaCl
3. HCl + CaCO3 CaCl2 + H2O +CO2
4. C12H22O11 + O2 CO2 + H2O 5. What is the chemical name for the following compounds?
Word bank: Sugar rust hydrogen peroxide Salt water carbon dioxide
1. H2O _______________________ 4. CO2 _________________________ 2. NaCl ______________________ 5. H2O2 ________________________ 3. Fe2O3 _______________________ 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 (salt) 2. CaCO3 (chalk or marble) 3. N2O (nitrous oxide or laughing gas) 4. MgSO4 (Epsom salt) 5. FeS2 (iron sulfide – fools gold) 6. CH4 (methane) 7. CaSO4 (plaster of paris) 8. SiO2 (quartz or sand) 9. KNO3 (saltpeter – used to make gun powder)) 10. NaHCO3 (baking soda) 11. CaSO4 (gypsum) 12. NaF (sodium fluoride)
13. H2O (water) 14. Na2B3O7 (borax) 15. H4Mg3Si2O9 (talc) 16. HC2H3O2 (vinegar) 17. NH4OH (ammonia) 18. CO (carbon monoxide) 19. CO2 (carbon dioxide, dry ice) 20. C12H22O11 (sugar)
Valence Bonding nice youtube explanation http://www.youtube.com/watch?v=rSwnODMNULI&feature=rel
ated&safety_mode=true&persist_safety_mode=1&safe=active
Compare Contrast
Elements Compounds
.
.
Chemical Reactions Reactants Product
# of atoms here = # of atoms here
So, it’s balanced!
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 (4
He), 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. 235
U = 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.
QUARKS
A proton, composed of two up quarks and one down quark. (The color assignment of individual quarks is not important, only that all three colors be present.)
A quark (/ˈkwɔrk/ or /ˈkwɑrk/) is an elementary
particle and a fundamental constituent of matter.
Quarks combine to form composite particles called hadrons, the most stable of which are protons and neutrons, the components of atomic nuclei.
Due to a phenomenon known as color confinement,
quarks are never directly observed or found in isolation;
they can be found only within hadrons, such as baryons (of which protons and neutrons are examples), and mesons.
For this reason, much of what is known about quarks has been drawn from observations of the hadrons themselves.
There are six types of quarks, known as flavors: up,
down, strange, charm, bottom, and top. Up and down quarks have the lowest masses of all quarks. The heavier quarks rapidly change into up and down quarks through a process of particle decay: the transformation from a higher mass state to a lower mass state. Because of this, up and down quarks are generally stable and the most common in the universe, whereas strange, charm, top, and bottom quarks can only be produced in high energy collisions (such as those involving cosmic rays and in particle accelerators).
Quarks have various intrinsic properties, including electric charge, color charge, mass, and spin.
Quarks are the only elementary particles in the Standard Model of particle physics to experience all four fundamental interactions, also known as fundamental forces (electromagnetism, gravitation, strong interaction, and weak interaction), as well as the only known particles whose electric charges are not integer multiples of the elementary charge.
For every quark flavor there is a corresponding type of antiparticle, known as an antiquark, that differs from the quark only in that some of its properties have equal magnitude but opposite sign.
The quark model was independently proposed by
physicists Murray Gell-Mann and George Zweig in 1964. Quarks were introduced as parts of an ordering
scheme for hadrons, and there was little evidence for their physical existence until deep inelastic scattering experiments at the Stanford Linear Accelerator Center in 1968. All six flavors of quark have since been observed in accelerator experiments; the top quark, first observed at Fermilab in 1995, was the last to be discovered.
http://en.wikipedia.org/wiki/Quark
http://www.youtube.com/watch?v=TGrDj5vFefQ quarks explained 4:00
Higgs Boson http://www.youtube.com/watch?v=RIg1Vh7uPyw 3:27 Quantum Mechanics: Structure of Atoms http://www.youtube.com/watch?v=-
YYBCNQnYNM&list=PL606C58D632079215 Higgs Boson and other 6:11 (I’m working on understanding this/not clear yet)
Quick Quiz 1 1. How many protons does an atom of Manganese have? 2. How many electrons does a normal atom of Na have? 3. How many neutrons does a normal atom of Fluorine have? 4. How many atoms does two molecules of water have? 5. How do you know that the substance you are holding is two
elements, not one? Quick Quiz 2 1. Draw a Bohr Model of the atom Oxygen. Label protons,
electrons, neutrons and nucleus. 2. How many electrons does a normal atom of Silver have? 3. How many neutrons does a normal atom of Na have? 4. What is the maximum number of electrons that fit on the second
shell or orbital? 5. What is the difference between a mixture and a compound?
Matter Quick Quiz 3 1. Explain the difference between molecule and compound. 2. How many neutrons does a normal atom of Zinc have? 3. The main element is the air we breathe is what?
4. This image would be an example of what term of matter?
5. This image would be an example of what term of matter?
6.C6H12O6 How many atoms are in the before chunk?
Matter Study Guide Directions:
1. You need to be sure to go over ALL of the pages in your classwork section; these notes
will help you complete this study guide.
2. You should also look back at all of your exit tickets and daily goals to see which topics
you may want to spend extra time on. Your homework worksheets would also be a good
source.
3. Try to complete as much as you can without looking at your notes. After that, go back
through your notes to help you fill in the rest.
Name: __________________________________________________________ Date: ______________________
A. Fill in the missing information in the
chart to the right.
B. Use the electron shells below to draw
a model of a nitrogen atom. Use the
following key to help you complete the model:
C. Now use the electron shells below to draw a model of a fluorine atom.
a. What is the particle that makes these two elements VERY different from each other?
D. Fill in the missing information into the graphic organizer below.
Particle Location Charge
Proton
Neutron
Electron
_________________
make
up
_________________
Two or more elements CHEMICALLY
combined make up
elements
Two or more elements PHYSICALLY
combined make up
_________________
_________________
Key: = protons =
_____ = electrons =
_____ = neutrons =
_____
Key: = protons =
_____ = electrons =
_____ = neutrons =
_____
E. The following circles represent ONE atom. Each color circle represents a DIFFERENT kind of
atom. Use the different circles to draw examples of the following types of matter. Then, below
your picture, give a real life example of each. The example of molecule has been done for you.
F. Use your periodic table to fill in the missing information below.
G. Use your periodic table to fill in the missing information below.
Element Mixture Compound
Molecule (this should be ONE
unit of the compound you drew)
Example: Example: Example: Example: One molecule of salt has 1
sodium atom and 1 chlorine atom.
Chemical Name Chemic
al Symbol Atomic
Number Atomic
Mass Protons Electrons Neutrons
Potassium
Ni
82
One atom of
Element A
One atom of
Element B
One atom of
Element C
This is the ATOMIC NUMBER. The atomic number tells us
_____________________________________
This is the _________________________. This tells us
_____________________________________
This is the ___________________________
This is the ___________________________
H. A chemical formula is a way of writing a compound to tell us what ELEMENTS are in the
compound.
a. Look at the following chemical formulas and identify what ELEMENTS are in the
compound.
b. Then, tell us how many ATOMS of each element are present in the compound.
I. Answer the following questions regarding Silver Nitrate, a compound.
a. Silver Nitrate has the following elements in it, in this exact order:
i. One atom of Silver (Ag)
ii. One atom of Nitrogen (N)
iii. Three atoms of Oxygen (O)
b. Use the above information to write the CHEMICAL FORMULA:
_________________________________
J. Fill in the following venn diagram with information about physical and chemical changes.
N2O H2SO4 C8H10N4O2
Elements # of
Atoms Elements
# of Atoms
Elements # of
Atoms
Physical Changes
Chemical Changes True of
Both
K. Identify which of the following examples are examples of a chemical change by placing an X in
the box. One example has been done for you.
L. A chemical equation is a way to represent a chemical change.
a. Using the chemical equation below, DRAW A CIRCLE around the REACTANTS and
DRAW A SQUARE around the PRODUCTS.
Zn + HCl ZnCl2 + H2
b. When a compound has a coefficient attached, the coefficient tells us how many
MOLECULES of that compound are present. For example:
M. Below are some examples of chemical equations.
a. Determine if each equation is balanced by counting the atoms on each side of the
equation.
b. Then, write a letter B in the space if the equation is balanced and a U in the space if it is
unbalanced.
______ CH4 + 2O2 CO2 + 2H2O
Example of Matter Changing Chemical Change
Bleaching a shirt
Leaves changing color in the fall X
Ice melting
Salt dissolving in water
A necklace tarnishing (when jewelry turns a brownish color)
Cutting pancakes
Cooking pancakes
C =
H =
O =
C =
H =
O =
+ +
______ 2P + 3Cl 2PCl3
N. Use the chart below to fill in the top 3 elements found in each of these locations. Use the
graphs/charts below to help you fill in the missing information.
Earth’s Atmosphere
Earth’s Crust Earth’s Oceans Human Body
Top Element # 1
Top Element # 2
Top Element # 3
P = Cl =
P =
Cl =
