Download Structure of the Atom

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• Groups of 2 to 3
• These people will check in on you and
make sure you are studying
• You can also reach out to these people
with questions
• Exchange Numbers!
SPS1 Students will investigate our
current understanding of the atom.
• A. Examine the structure of the atom in terms of
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proton, electron, and neutron locations.
atomic mass and atomic number.
atoms with different numbers of neutrons (isotopes).
explain the relationship of the proton number to the
element’s identity.
• B. Compare and contrast ionic and covalent
bonds in terms of electron movement.
Structure of the Atom
• Atoms have 3 sub-particles
– Proton, Neutron, Electron
Charge
Location Mass
Proton
Positive
Nucleus
1 AMU
Neutron
Neutral
Nucleus
1 AMU
Electron
Negative
Electron
Cloud
0 AMU
Mass Number/Atomic Mass
• The mass number is the protons + the
neutrons (since they’re the only particles that
have mass in the atom!)
What is the mass of silver?
Atomic Number
• The atomic number is the number of protons in
the atom
• The atomic number tells us WHO the atom is.
The atomic number (and therefore the protons)
NEVER change! (if they did it would be a
different element!)
What is the atomic # of silver?
Bohr Model
• Draw the Bohr Model for Lithium
Isotopes
• Isotopes:
– Atoms of the same element can have a different
number of neutrons and therefore a different
atomic mass
Isotopic Form
Carbon—12
Atomic Mass
Atomic
Mass
Atomic
Number
𝟏𝟐
𝟔𝑪
Lewis Structures
1) Write the element
symbol.
2) Carbon has 4 valence
electrons.
3) Starting at the right, draw
4 electrons, or dots,
counter-clockwise
around the element
symbol.
Lewis Dot Structure Ex.
• Draw the Lewis Dot
Structure for Bromine
Ions
• An atom that has lost or gained electrons
• The atom has either a positive charge or a
negative charge
• Different number of protons then electrons
Atomic Charge
• To find the total charge of an atom, add the
number of protons (+) to the number of
electrons (-)
• Anion: An ion that has gained electrons and
has a negative charge
• Cation: An ion that has lost electrons and has
a positive charge
Just in case you’re still confused….
• Negative: More electrons; Gaining!
• Positive: Less electrons; giving away! (or
losing)
BONDING
• Octet Rule
– Atoms will always gain or lose electrons in order
to get a complete set of valence electrons (usually
8)
– *Exceptions: Helium and Hydrogen!
How many electrons does Carbon need to gain?
BONDING based on balance of
charges
• Metals want to LOSE electrons (and become
more positive)
• Non-metals want to GAIN electrons (and
become more negative)
Name an element that hydrogen wants to bond with
Ionic Bonds
• Metal and a non metal
• Transfer of electrons from a metal to a nonmetal
Covalent Bonds
• Two non-metals
• Electrons are shared
Flashcard VOCAB Words!
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Proton
Neutron
Electron
Nucleus
Electron Cloud
Mass #/Atomic Mass
Atomic #
Isotope
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Bohr Model
Lewis Dot Structure
Ion
Anion
Cation
Octet Rule
Ionic Bond
Covalent Bond
SPS2. Students will explore the nature of matter, its
classifications, and its system for naming
types of matter.
• A. Calculate density when given a means to
determine a substance’s mass and volume.
• B. Predict formulas for stable binary ionic
compounds based on balance of charges.
• C. Use IUPAC nomenclature for transition between
chemical names and chemical formulas
• D. Demonstrate the Law of Conservation of Matter
in a chemical reaction.
• E. Apply the Law of Conservation of Matter by
balancing the following types of chemical
equations: Synthesis, decomposition, single
replacement, double replacement
Density
• Mass per unit volume of a material (how
much stuff is packed into a certain space)
• Measured in g/mL (liquids) OR g/cm3(solids)
Practice Problems
– A rock has a mass of 5 grams. When placed in a
graduated cylinder filled to 10mL, the water rises
to 12 mL. What is the density of the rock?
– A platinum bar measures 5.0 cm long, 4.0 cm
wide, and 1.5 cm thick. It has a mass of 700.0
grams. What is the density of the platinum bar?
Naming Ionic Bonds
Name to formula
• Criss-cross apple sauce!
• Figure out the charge on your first
element. Then figure out the charge on
your second element
• Cross the charges and you’re done!
Practice
• What is the formula for Lithium Oxide?
Naming Ionic Bonds
Formula to name
• Name the metal normally
• Add the –ide ending to the non
metal
Practice
• What is the name of NaCl?
Naming Covalent Bonds
Formula to name
• Greek prefixes
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Mono (1)
Di (2)
Tri (3)
Tetra (4)
Penta (5)
Hexa (6)
Hepta (7)
Octa (8)
Nona (9)
Deca(10)
**Never use “mono” on the first element
**Still add the “-ide” ending to the second element
Naming Covalent Bonds
Formula to name
Examples:
CO2 = Carbon Dioxide
CO = Carbon Monoxide
C10O4 = Decacarbon Tetraoxide
Naming Covalent Bonds
Name to formula
• Use the prefixes to tell you how many of
each element you have
Practice
• What is the formula for
Octahyrdogen Trifloruide?
Balancing Chemical Equations
• Why do we balance?
–Law of Conservation of Matter states
that matter cannot be created nor
destroyed. Therefore we must have
equal numbers of elements on each
side of our reaction!
Rules of Balancing
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Make a “T” chart at the yield sign
Count how many of each element you have
Use coefficients to balance equation
NEVER EVER EVER change a subscript
Example of balancing
______NaCl + ______F2 _____ NaF + ______Cl2
Four Types of Chemical Reactions
Types of Chemical
Reactions
Synthesis
Equation
A+B AB
Decomposition
AB  A+B
Single Replacement
AB + C  AC + B
Double Replacement
AB + CD  AC + BD
Flashcard VOCAB Words!
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Density
Law of Conservation of Matter
Synthesis Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction