Jeopardy!
• Review Flashcards – Set 2
• Upcoming
– W/R: Review – Final Review
– F/M: Final Cumulative Quiz
• (60 multiple choice questions)
– Final Day: Lab Practical in Groups
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•
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M1 & M2: Tuesday
G1 &G2: Wednesday
M3 & M4: Thursday
G3 & G4: Friday
For the Final: Part 1 – Multiple Choice
• Part 1: Multiple Choice (50% of your final exam
grade)
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–
–
–
60 Questions
Scantron
Friday (Maroon)
Monday (Gold)
• Bring:
– A #2 pencil
• Procedure:
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–
–
–
10-20 minutes of study time at the start of class.
The remainder of the block will be for testing.
You may not leave the room once the test has begun.
When you finish, sit quietly.
Atomic Models: Bohr Diagram
• Definition: Shows ALL
electrons in an atom in
the appropriate energy
level.
How do electrons fill energy levels?
• Electrons occupy the
lowest energy level first.
• Once an energy level is
full it will occupy the
next level.
• How will the electrons
be arranged in a helium
atom?
Arrange the electrons.
Arrange the electrons.
Arrange the electrons.
Atomic Models: Lewis Dots
• Definition: Shows the
number of valence
electrons (electrons in
the outermost energy
level).
Lewis Dot: Lithium
Lewis Dot Diagram: Aluminum
Lewis Dot Diagram: Nitrogen
Lewis Dot Diagram: Helium
Periodic Table
• The row number tells
you the number of
energy levels in an
atom.
• The column number
tells you the number of
valence electrons.
Which Elements have 1 valence
electron?
Which Elements have 5 valence
electron?
Which Elements have 7 valence
electron?
Which Elements have 8 valence
electron?
Which Element?: Period 1, Group 1
Energy Levels? Valence Electrons?
Which Element?: Period 4, Group 2
Energy Levels? Valence Electrons?
Periodic Trends
• Atomic mass: Increases
over and down.
• Atomic radius:
Decreases across,
Increases down
Electronegativity
• Electronegativity: How
strongly one atom pulls
on the electrons of
another atom.
low = weak
high = strong
First Ionization Energy
• First Ionization Energy:
How easily an atom
loses an electron.
low = easy to do
high = hard to do
Chemical Reactions
• Reactants: Molecules at
the start.
• Products: Molecules
formed.
Interpreting a Chemical Reaction
Coefficient:
Number of
molecules
Subscript:
Number of
atoms in a
molecule
1
1
4
4
4
4
Chemical Reactions: Exothermic or
Endothermic?
Chemical Reactions: Exothermic or
Endothermic?
TEMPERUATURE
TIME
Ions and Ionic Bonding
• Definition: An atom with a
charge. It has an unequal
number of protons and electrons.
• Types of Elements: Metals and
Nonmetals
• Cation: Lose electrons, Positive
Ion
• Anion: Gain electrons, Negative
Ion
• Properties: High melting point
Review: Build an Ion
• A neutral atom has NO CHARGE / A NET CHARGE.
• An ion is a variation of an atom with NO CHARGE / A NET CHARGE.
• In a neutral atom the number of protons will be EQUAL / NOT
EQUAL to the number of electrons.
• In an ion the number of protons will be EQUAL / NOT EQUAL to the
number of electrons.
• To make an ion you change the number of PROTONS / ELECTRONS.
Neutral Atoms: Na and Cl
What happens when they are near each
other?
The electron is transferred!
Ions are formed.
What is the charge on each ion?
How many valence electrons does each ion have?
What is the charge of each ion?
Reactivity
• Reactivity depends on
the number of valence
electrons.
• Metal reactivity can be
determined by placing
one metal in a metallic
solution.
Reactivity and Valence Electrons:
Which Groups are the most reactive?
Reactivity of Metals:
Which metal is the most reactive? Least?
NO REACTION
REACTION
NO REACTION
NO REACTION
NO REACTION
NO REACTION
REACTION
REACTION
NO REACTION
Covalent Bonding
• Definition: A bond formed
by sharing electrons
between atoms.
• Atoms will share electrons
until they have a full
outermost energy level.
• Types of Elements:
Nonmetals
• Properties: Low melting
points
What happens as atoms get
close to each other?
The electron from each hydrogen atom feels the
attraction from the proton of the other
hydrogen atom
The hydrogen atoms share the electrons.
What type of bond is this?
Isotopes
• Definition: A variation
of an atom with a
different number of
neutrons.
• # of Neutrons = Atomic
Mass – Atomic Number
• Example: Nitrogen -14
– 14 is the atomic mass
ATOMIC
MASS
JEOPARDY!
• Play JEOPARDY!
– On your own
– In pairs
– Or as a lab group
• As you play
– Try your best
– Use your notes
– Everyone must complete
the provided ANSWER
SHEET!!
For the Final: Part 1 – Multiple Choice
• Part 1: Multiple Choice (50% of your final exam
grade)
–
–
–
–
60 Questions
Scantron
Friday (Maroon)
Monday (Gold)
• Bring:
– A #2 pencil
• Procedure:
–
–
–
–
10-20 minutes of study time at the start of class.
The remainder of the block will be for testing.
You may not leave the room once the test has begun.
When you finish, sit quietly.