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
58
Embed
Matter /571f57f2c5ce8daa34e22198 · 2017-11-07 · ELECTRON A negatively charged particle found outside the nucleus in a region ... The outer P shell then continues to build to eight
This document is posted to help you gain knowledge. Please leave a comment to let me know what you think about it! Share it to your friends and learn new things together.
Transcript
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
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
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
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.
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
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,
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
____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)
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
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.
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.)
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.
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