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The Structure of the AtomOn page 22 of your ISN, don’t forget to add to your TOC!
The Structure of the Atom• The atom is the smallest part of an element, while still maintaining it’s properties. “indivisible”“can not be divided”
Draw an atom
Nucleus- tiny dense cluster of protons and neutrons in the center of the atom
Protons-has a positive (+) charge. The # of protons determines the atomic number Neutron- are neutral
(No charge). The # of neutrons+ the # of protons= Atomic mass
Electrons- have a negative (-) charge. They are in rapid, continuous motion around the nuclues
Electron cloud- surrounds the nucleus and contains the electrons. “empty space”
Out put-Analogy of an Atom•Use Bohrs model and write an analogy comparing the structure of an atom to the solar system.
Digging deeper with atomsPage 24 of your ISN, don’t forget the TOC!
Electrons• Electrons circle the nucleus in an electron cloud.
• The outermost electrons are called valence electrons.
• Each level/shell can only handle so many electrons until it is full and has to send electrons to another level/shell. Level one- 2 electrons Level two- 8 electrons Level three- 18 electrons Level four- 32 electrons
Isotopes•Atoms that can have a wide range of number of neutrons in the nucleus. Different types, have different uses
Atomic Number•Number of protons in the nucleus of each atom of a given element
Mass Number•Number of protons + number of Neutrons
Time to practice- *Output side• Please draw an atom that has 5 protons, 6 neutrons, and 5 electrons. Include their charges and correct locations. (using color!)
What is the atomic number for this atom?
What is the atomic mass for this atom?
Time to practice #2• Please draw the following pair of isotopes. Identify the atomic mass and mass number for each(Use color!)
N N
Periodic TablePage 26 of your ISN, be sure to include in your TOC!
Element•Matter made up of only one kind of atom
Takes up space and has mass*
Mendeleev• Arranged 63 known elements
• Based on chemical properties and atomic weight
• Left gaps for elements he predicted were yet to be discovered
C6
Carbon12.011
Atomic Number- Number of protons in the nucleus
Element Name
Symbol
Atomic MassAverage weight of element isotopes
Physical Properties of metals, nonmetals and metalloids * output
Metals• Shiny/metallic luster
• Solid at room temperature (except Mercury)
• Reflect light when polished (luster)
• Can bent or hammered flat(malleable)
• Strong and resistant to breaking
• Have a characteristic sound when struck with an objet
• Have high melting and boiling points
• Have high densities
• Attracted to a magnet
Non Metals
• Exist as solids, liquids or gases at room temperature
• Do not reflect light well (no luster)
• Are brittle
• Cannot be hammered flat (nonmalleable)
• Can not be drawn into a wire (not ductile)
• Soft and bend or break easily (low tensile strength)
• Don’t have a characteristic sound when struck
• Are poor conductors of heat and electricity
• Have low densities
• Are not attracted to a magnet
Metalloids
• Are generally solid
• Can be shiny or dull
• May or may not be hammered flat
• May or may not be drawn into wire
• May or may not be brittle
• Conduct heat and electricity better than nonmetals, but not as well as metals
• Tend to make good semiconductors
• Have melting and boiling points that are widely varied
• Have densities that are widely varied
Electrons
Electron cloud
Energy Levels
Valence Electrons
Time to move…•We are going to be electrons today! Lets go into the commons and practice
Electron Dot Diagram• Symbol for the element surrounded by as many dots as there are electrons in its outer energy level.
S
Lets Practice ~Complete the electron dot diagram and answer the questions
NElement?
# Electrons?
# Valence Electrons?
Lets Practice ~Complete the electron dot diagram and answer the questions
IElement?
# Electrons?
# Valence Electrons?
Elements, compounds and mixturesPage 37-38
Output part 1
Student Output-part 1Create a Venn diagram
Example
Compounds
Why do element combine?• Atoms are most stable when their electron shells are full.
Compound- a pure substance containing two or more elements that are chemically bonded
Ionic bond• Ionic Bonds form when electrons are transferred from one
atom to another, forming charged Ions which are attracted to each other. Elements tend to lose or gain electrons, forming Ions, to get a 'full other shell'.
• Ion-Atom that is positively or negatively charged because it has gained or lost electrons
Covalent Bond• Covalent Bonds involve the sharing of electrons so that all
atoms have 'full outer shells'.
Metalic Bond• Bond formed when metal atoms share their pooled electrons
Output-• Use the following words to complete the graphic organizer provided
• Covalent Electron cloud Molecule
Nucleus Gain or loss of electrons
Ionic vs Covalent foldable…
FrontIonic Bond
Covalent Bonds
Square # 1Ionic Bond• Atoms lose or gain electrons
• Between Metal and Nonmetal
Covalent Bond• Atoms share an electron
• Between nonmetal and nonmetal
Square # 2
Ionic Bond Covalent Bond
-1 electron+1 electron
Lithium + Flourine
Sharing Electrons
Oxygen+Oxygen
Square #3
Ionic Bond Covalent Bond
Li F
Li F+ -
O O
O O
Square #4
Ionic Bonds
• LiF
•NaCL
•MgO
Covalent bonds
•H2
•H20
•Co2
Chemical Bonds & Reactions
+
-
+
-
How Many Valence Electrons?• Hydrogen
• Lead
• Xenon
• Sulfur
• Rubidium
1 Valence Electron
4 Valence Electrons
8 Valence Electrons
6 Valence Electrons
1 Valence Electron
The Octet Rule• Atoms will combine to form compounds in order to reach eight electrons in their outer energy level. Atoms with less than 4 electrons tend to lose electrons.
Atoms with more than 4 electrons tend to gain electrons.
• Be aware that there are some exceptions!
CONSIDER EIGHT A HAPPY NUMBER FOR ATOMS!
Lewis Structure(Electron Dot Diagram)
• a way of drawing the outer energy level electrons (valence) of an atom
• The symbol for the element surrounded by as many dots as there are electrons in its outer energy level (valence)
• Examples
How many valence electrons do each of these atoms have?
Mg:Magnesium
Al :.
Aluminum
N :.. .
Nitrogen
Making an Electron Dot DiagramElement “X” has 8 valence
electrons
X. X : X :.
X :..
X :.. . X :
. .. . X :
. .: . X :
. .:. .
1 2 3
4 5 6 7
Write down the element’s symbol and place the first two dots on
any side of the symbol.
Place the rest of the dots in either a clockwise or counter clockwise manner
around the symbol, with no side receiving two dots
until each side gets one.
If this were an atom of an elementfrom group 1, you would just place theone dot on any side of the element.
What Would the Electron Dot Diagram Look Like?
H
Sr
O
Ne
How many valence electrons does
each atom have?
1 Valence Electron 6 Valence Electrons
8 Valence Electrons 2 Valence Electrons
Oxidation Number• The charge that an atom would have if it lost or gained electrons; ionic charge
• Can be helpful in determining which atoms will interact or bond with each other
• Example:
Mg:MagnesiumAccording to electron dot diagram for Magnesium,
it has two valence electrons. Because Magnesium is “unhappy” with two, it will typically lose them. If this happens it will turn into a Magnesium ion. At this point it will have an oxidation number of
+2. Mg2+
What Could the Oxidation Number Be?
H O
Ne Sr
+1 or -1 because it can gain or lose one electron
-2 because it will gain two electrons
0 because it will notgain or lose electrons
+2 because it will lose two electrons
3 Types of Chemical Bonds
•Ionic•Covalent•Metallic
What can you describe about each of thesebonds just by looking at the name?
Which different groups or families
of elements will most-likely
interact to create these
typesof bonds?
IONIC BONDS
-
+
++
+
+++
+++
-
-
-
-
--
-
-+
-
-
-
-
-
-
-
-
-
• The force of attraction between oppositely charged ions.
• Occurs after a transfer or loss/gain of electrons
• Usually form between atoms of metals and atoms of non-metals
• Resulting compounds have a name that usually ends in –ide
Example - Sodium Chloride (NaCl)
Cl Na1- 1+
+
++
+
+++
+++
-
-
-
-
--
-
-+
-
-
COVALENT BOND• A force that bonds two atoms together by a sharing of
electrons
• Each pair of shared electrons creates a bond
• Usually occurs between atoms of non-metals
+ ++
++
+
++++
Example – Water (H2O)
-
-
-
-
--
-
--
-
OH H
Results of BondingMolecule
A neutral group of two or more non-metal atoms held together by covalent bonds
Type:
Diatomic - molecules consisting of two atoms of the same element bonded together
Examples:
H2, F2, O2, N2
Compound
A pure substance composed of two or more different elements (atoms) that are chemically combined
Examples:
CO, NO2, NaCl
What would you call something that has characteristics of both?
Molecule, Compound, or Both?
H2
Hydrogen
NO2
Nitrogen Dioxide
Cl2
Chlorine
O2
Oxygen
NO
Nitric Oxide
CO2
Carbon Dioxide
N2
Nitrogen
H2O
Water
CH4
Methane
Chemical Equation• Shorthand form for writing what reactants are used
and what products are formed in a chemical reaction
• Sometimes shows whether energy is produced or absorbed
• Examples:
2H2 + O2 2H2O
CH4 + 2O2 CO2 + 2H2O
C6H12O6 + 6O2 6CO2 + 6H2O + energy
Components of a Chemical Equation
2H2 + O2 2H2O
(Reactants)
(Products)(Yield)
Chemical Formulas
Chemical Formula
Subscripts Coefficient
Sometimes you will see a “yields” sign that looks like this.
What do you think it means?
Coefficient Subscript
Law of Conservation of Mass• Proposed by Antoine Lavoisier
• In a chemical reaction, atoms are neither created nor destroyed
• All atoms present in the reactants are also present in the products
• Chemical equations must account for/show the conservation of mass balancing equations
H2 + O2 H2O
In its present form, does this chemical equation show a conservation of mass?
How would you balance this equation to
show the conservation of mass?
2 2Reactants
H 2O 2
Products
42
H 2O 1
42
Hints For Balancing Equations• Count the atoms
List the number of atoms of each element to see which elements must be balanced
• Use a coefficient to add atoms to one side of the equation Start with the reactant or product that has the
greatest number of different elements
• Add a coefficient to another reactant or product Make sure that the coefficients in your balanced
equation are the smallest whole numbers possible (they should have no common factor other than one)