Warm-up #11 Jan. 25
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Transcript of Warm-up #11 Jan. 25
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WARM-UP #11 JAN. 25Atomic Theory
States that matter is composed of discrete units called atoms
The word "atom" comes from the ancient Greek adjective atomos meaning 'indivisible’
Essential Question:When and where do you think mankind
originally began to ponder as to what makes up the elements and atoms?
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SUBATOMIC PARTICLESName Symbol Charge Relative
Actualmass mass
Electron e- -1 1/1840 9.11 x 10-28
Proton p+ +1 1 1.67 x 10-24
Neutron n0 0 1 1.67 x 10-24
crap
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SYMBOLS The symbol of an element contains the mass
number and the atomic number:
XMass Number
Atomic Number
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SYMBOLSFind the:1. Number of Protons2. Number of Neutrons3. Number of Electrons4. Atomic Number5. Mass Number Rh104
45
Rhodium - 104
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HISTORY OF THE ATOM The original idea of the atom came from
Ancient Greece (400 B.C.) Democritus – Greek Philosopher He and his mentor Leucippus
first described that all things weremade up of “atoms”
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WHO’S NEXT? Late 1700’s – John Dalton – England Teacher – summarized results of his
experiments and those of others in his Atomic Theory.
His idea combined ideas of elements with atoms
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DALTON’S ATOMIC THEORY All matter is made up of tiny individual
particles called atoms Atoms of the same element are identical,
those of different elements are different Atoms of different elements combine in
whole number ratios to form compounds Chemical reactions involve the
rearrangement of atoms. No new atoms are created or destroyed.
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JJ THOMSON J.J. Thomson – English physicist, 1897 Made a piece of equipment that explored the
properties of cathode rays. Basically discovered that atoms of divisible
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THOMSON’S MODEL Found the electron Couldn’t find positive (for a while) Said the atom was like plum pudding A bunch of positive stuff, with the electrons
able to be removed
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PROTONS Proton – positively charged pieces
1840 times heavier than the electron. Eugene Goldstein used a modified
cathode ray Rutherford predicted its presence in
the atom with gold foil experiment
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RUTHERFORD’S EXPERIMENT Ernest Rutherford was an English Physicist
(1910) Believed in the plum pudding model of the
atom. Wanted to see how big they are Used radioactivity Alpha particles – positively charged pieces
given off by uranium Shot them at gold foil which can be made a
few atoms thick
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HE EXPECTED The alpha particles to pass through without
changing direction very much. Because…
The positive charges were spread out evenly.Alone they were not enough to stop the alpha particles
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WHAT HE GOT
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HOW HE EXPLAINED IT Atom is mostly empty Small dense, positive Piece at center Alpha particle are deflected by it if they get
close enough
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DENSITY OF THE ATOM Since most of the particles went through, it
was mostly empty Because the pieces turned so much, the
positive pieces were heavy Small volume, big mass, big density. This small dense positive area is the nucleus
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BOHR’S MODEL – 1915 Why don’t the electrons fall into the nucleus? Move like planets around the sun. In circular orbits at different levels Amounts of energy separate one level from
another
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BOHR’S MODEL The further an electron is from the nucleus
the more energy it has There is no “in between” energy It is like a ladder
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BOHR’S IS NOT RIGHT EITHER! Bohr got closer than we had been so far, but
it was still not right. He gave us the idea of energy levels for
electrons. BUT his idea only worked for one atom
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NEUTRONS No charge Same mass as the
proton Discovered by James
Chadwick during radioactivity experiments in 1932
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QUANTUM MECHANICAL MODEL 1925 - Erwin Schrondinger used the results of
the experiments done with the hydrogen atom to come up with the quantum mechanical model
This comes from a mathematical solution to the Schrodinger equation
The quantum mechanical model determines the allowed energies an electron can have and how likely it is to find the electron in various locations.
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QMM Has energy levels for electrons Orbits are not circular It can only tell us the probability of finding an
electron a certain distance from the nucleus.
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MODERN VIEW The atom is mostly empty space Two regions Nucleus – protons and neutrons Electron cloud – region where you might find
an electron
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ATOMIC THEORY TIMELINE ASSIGNMENT You are to create a timeline that maps out each
significant event throughout history that involves the atomic theory.
There will be at least 8 events (all were covered in the notes)
For each event I want the: Date Person What they contributed (IN COMPLETE SENTENCES). A drawing or something of what they discovered.
They need to be colored.
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TICKET OUT THE DOOR1. What does the atomic number tell
you about an element?2. What are the three subatomic
particles, their relative masses, relative charges, and location(which region of the atom)?
3. What is a compound?4. What is an isotope?
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WARM-UP #12 JAN. 26
Cations When an element
becomes positively charged it forms a cation
Anion When an element
becomes negatively charged it forms an anion
An ion is an atom or molecule in which the total number of electrons is not equal to the total number of protons
What do you have to lose in order to become positively charged?
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THE PERIODIC TABLE The periodic table is based on the Modern
Periodic Law Came from the QMM Set up in rows called periods
Indicate the main energy level Columns called groups or families
Similar properties
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Dmitri Mendeleev was one of the first scientists to realize there was a trend in the properties of the elements
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CLASSIFYING We separate the periodic table several ways
to help classify the elements This includes dividing it by families, and type
of element
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Representative – group A Transitions – group B
We split the table into these 2 major groups Most of what we deal with deal with is in group A
or the representative elements
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METAL ~ NONMETAL ~ METALLOID These are three of our other main
classifications Elements that fit into these groups have
specific properties
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METALS Most metals are solid at room temperature
Which one is the exception? Mercury – Hg
Generally good conductors of heat and electric current Sea of free floating electrons
Usually form cations Usually malleable and ductile
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NONMETAL Less similarities in the nonmetals Typically poor conductors of heat and electric
current Solid nonmetals tend to be brittle
Carbon, Sulphur
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METALLOID These elements have properties that are
similar to both metals and nonmetals Semiconductors
Can be used to produce superconductors Boron, silicon, arsenic
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PERIODIC TABLE ASSIGNMENT Pick 3 elements, one from each subgroup
(metal, nonmetal, metalloid) Research each element:
Draw the symbol as you would see it on the periodic table
Label the atomic number and mass number Tell me where the element is found and how we
use it Products, industry, etc.
Describe some of its properties Draw a picture of what it looks like naturally These should be colored
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WARM-UP #13 JAN. 27 Valence Electrons - are the electrons of an
atom that can participate in the formation of chemical bonds with other atoms.
Electron dot diagrams - diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule
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HOW DO ELEMENTS FORM IONS AND WHY? All elements are trying to get the same
number of electrons as the nearest noble gas Far column on the right
This is where valence electrons come in
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VALENCE ELECTRONS All atoms have valence electrons These are the electrons responsible for
forming bonds They are the furthest from the nucleus They fill the outermost energy level These determine the properties of the atom,
such as stability.
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Every element can only have 8 valence electrons
They WANT to have 8 like the noble gases
Helium only has 2 electrons TOTAL, so some elements are content
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VALENCE ELECTRONS You can determine how many valence
electrons for Group A by looking at the groups number
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VALENCE ELECTRONS We represent valence electrons using
electron dot diagrams.
Electron dot diagrams show the element symbol with dots representing the valence electrons
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BOHR’S MODELShows ALL of the element’s
electrons
1st – 2e-
2nd – 8e-
3rd – 18e-
4th – 32e-
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NITROGEN
N
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ALUMINUM
Al
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IONSAtoms form ions based on the number of valence electrons
Group VIII A8 valence electrons (8 ve-)
What is the charge as an ion?0
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Positive ions are called cationsThese are formed when an atom
loses electronsThe metals usually form cations
Negative ions are called anionsThese are formed when an atom
gains electronsThe nonmetals usually form anions
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When an atoms forms an ion it changes size because it becomes stableCations are much smaller the
atom in which they formAnions are much bigger than
the atom from which they form
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TICKET OUT THE DOOR1. What does the atomic number tell
you about an element?2. What are the three subatomic
particles, their relative masses, relative charges, and location(which region of the atom)?
3. What is a compound?4. What is an isotope?
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PRACTICE Draw e- dot diagram, bohr model
diagram, and tell what charge each will have as an ionSodiumSulfurSiliconOxygenArgonChlorineBeryllium
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WARM-UP #14JAN. 30
Draw e- dot diagram, bohr model diagram, and tell what charge each will have as an ion:FluorineNeonCarbon
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REVIEW What are your three subgroups of
elements on the periodic table?MetalsNon-metalsMetalloids
What is an isotope?Atoms that have the same number of
protons but different number of neutrons.
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REVIEW What the atomic number equal to?
Number of protons
What is the mass number equal to? Number of protons and neutrons
What is a valence electron? Electron found on the out shell of an atom.
There can only be 8 total.
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TYPES OF CHEMICAL BONDS Ionic Bonds
Form between positive and negative ions Ex: salt forms when sodium reacts with chlorine
Covalent Bonds Form when atoms share electrons Ex: Silicon dioxide forms when one silicon atom
and two oxygen atoms share electrons in that outermost energy level
Metallic Bonds Form when electrons are shared by metal ions
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MINERALS A mineral is a naturally occurring, inorganic
solid with an orderly crystalline structure and definite chemical composition.
There are nearly 4000 known minerals
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NATURALLY OCCURRING A mineral forms by natural geologic
processes. Synthetic gems are not minerals
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SOLID SUBSTANCE Minerals are solids within the temperature
ranges that are normal for Earth’s surface Definite shape Definite volume
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ORDERLY CRYSTALLINE STRUCTURE Their atoms or ions are arranged in an
orderly and repetitive manner
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DEFINITE CHEMICAL COMPOSITION Every mineral is made up of a specific
compound. Each sample of that mineral is made of the same compound.
Different minerals are different compounds Ex: Quartz – Si02
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GENERALLY CONSIDERED INORGANICWhat do you think it means to be
organic?Organic means that it is a compound
containing carbonMost minerals do not contain
carbon We say generally because there are
some animals that secrete compounds considered mineralsEx: Calcite : calium carbonite
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SOURCEhttp://www.rocksandminerals.com/uses.htm
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TICKET OUR THE DOOR1. What is a mineral?2. Give me two characteristics a mineral must
have.3. Give an example of a mineral and one of its
uses.4. Draw an e- dot diagram and Bohr model for
Phosphorus1. LOCATED IN GROUP 5A
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WARM-UP #15JAN. 31What are five
characteristics of a mineral?
Coal forms from ancient plant matter that has been compressed over time. Do you think coal is a mineral?
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HOW MINERALS FORMThere are four major processes by
which minerals form:Crystallization from magmaPrecipitationChanges in pressure and
temperatureFormation from hydrothermal
solutions
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CRYSTALLIZATION FROM MAGMA Magma is molten rock As magma cools, elements
combine to form minerals First minerals are usually rich in
iron, calcium, and magnesium. As minerals continue to form
the magma changes composition forming minerals rich in sodium, potassium, and aluminum
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PRECIPITATION Water contains dissolved substances As the water evaporates some of the
dissolved substances can react to form minerals.
Limestone and Halite are common examples of precipitation
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PRESSURE AND TEMPERATURE Some minerals form when existing minerals
are subjected to changes in pressure and temperature
An increase in pressure can cause a mineral to recrystallize while still solid
Atoms are rearranged Temperature change can cause minerals to
become unstable and form new minerals that are stable at the new temperature.
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HYDROTHERMAL SOLUTIONS 100° C – 300° C Very hot mixture of water and dissolved
substances When they come into contact with existing
minerals, chemical reactions take place and form new minerals
Minerals can also form when these solutions cool
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MINERAL GROUPS There are 6 groups of minerals that we will
discuss Silicates Carbonates Oxides Sulfates/Sulfides Halides Native Elements
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SILICATES Most common Contain silicon-oxygen tetrahedron Groups based upon tetrahedron arrangement
Olivine Pyroxene Amphibole Micas Feldspars Quartz
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OLIVINE Independent tetrahedron
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PYROXENE GROUP Tetrahedrons are arranged in chains
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AMPHIBOLE GROUP Tetrahedron are arranged in double chains
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MICAS Tetrahedron are arranged in sheets Two types
Biotite – dark Muscovite - light
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FELDSPARS Three-dimensional network of tetrahedron Two types:
Orthoclase Plagioclase
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QUARTZ Three dimensional network of tetrahedron
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CARBONATES A major rock-forming group Found in the rocks limestone and marble Calcite and Dolomite are carbonate minerals
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OXIDES Minerals that contain oxygen and one or
more other elements. Rutile – TiO2 form as magma cool Corundum – Al2O3 forms when existing
minerals are subjected to changes in temperature and pressure
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SULFATES AND SULFIDES Minerals that contain sulfur
Anhydrite – CaSO4 Gypsum Pyrite – fools gold
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HALIDES Minerals that contain a halogen Salts Halite – table salt Fluorite
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NATIVE ELEMENTS Group of minerals that exist in relatively pure
form Gold Silver Copper Sulfur Diamond Graphite
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WARM-UP #16FEB. 1
Think of and list as many properties as you can that help us identity minerals. Again, these are different than the characteristics of minerals.
Why is it important to identify minerals?
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MINERAL PROPERTIES Minerals are classified by a set of specific
properties
These are considered intensive properties This means they don’t depend on the amount of
the substance, but the composition instead
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COLOR Color is the first thing you will notice about a
mineral Do you think this is a good indicator of what
a mineral is made of? Not always A very small difference in amount of
elements present can change the color of the mineral
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LUSTER Luster describes how light is reflected off the
surface of a mineral Minerals that have the appearance of metals
are said to be metallic. Nonmetallic luster is described in many
different ways: Vitreous Glassy Pearly Silky Earthy Adamantine Sub-metallic
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STREAK Streak is the color of a mineral in its
powdered form. You can obtain this by rubbing a mineral
across a streak plate (unglazed porcelain) Streak does not usually vary even if the color
does
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CRYSTAL FORM Visible expression of the internal
arrangement of atoms
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HARDNESSA measure of the resistance of a
mineral to being scratched
One of the most useful properties in identifying minerals
We use the Mohs scale of hardness
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CLEAVAGE AND FRACTURE
Cleavage and fracture both deal with how a mineral breaks apart
Cleavage is the tendency to break along a flat even surfaces
Fracture is the uneven breakage of minerals
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Mica shows cleavage; breaking in even flat sheets
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FRACTURE
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DENSITY Density is a property of all matter that is the
ratio of an object’s mass to its volume. Think of it as how compact the substance is
Grams
Cubic centimeters or milliliters
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PRACTICEA 6.75 g solid with a volume of 5.35 cm3. Find the density.
D = 6.75g / 5.35 cm3
D = 1.26 g/cm3
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OTHER PROPERTIESSome minerals have distinctive feelsTalc is soapy, and graphite feels
greasySome minerals are magnetic like
magnetiteSome have distinctive smells
like sulfurCalcite reacts chemically with
hydrochloric acid and will fizz
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REFLECTION In your journals, tell me what you did today
and how it is important. Describe the different properties of minerals
and how you used them today to determine the identity of various minerals.
What were some properties of specific minerals that gave their identity away relatively easily.
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WARM-UP #17 FEB. 2 What are the differences between ionic
bonds, covalent bonds, and metallic bonds? (use your notes)
What are halogens?
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TICKET OUT THE DOOR Name 4 properties of minerals used for
identification. How do we calculate density? What is the difference between cleavage and
fracture?