ftce chemistry sae preparation course
DESCRIPTION
FTCE Chemistry SAE Preparation Course. Session 2. Lisa Baig Instructor. Course Outline. Session 1 Review Pre Test Competencies 1 & 2 Session 2 Competency 5 Session 3 Competency 3 Session 4 Competency 4 Session 5 Competencies 6, 7 and 8 Post Test. Session Norms. Respect - PowerPoint PPT PresentationTRANSCRIPT
Course OutlineSession 1
Review Pre TestCompetencies 1 & 2
Session 2Competency 5
Session 3Competency 3
Session 4Competency 4
Session 5Competencies 6, 7 and 8
Post Test
Session Norms
• Respect– No side bars– Work on assigned materials only– Keep phones on vibrate– If a call must be taken, please leave the
room to do so
Chemistry Competencies1. Knowledge of the nature of matter (11%)2. Knowledge of energy and its interaction with matter
(14%)3. Knowledge of bonding and molecular structure (20%)4. Knowledge of chemical reactions and stoichiometry
(24%)
5. Knowledge of atomic theory and structure (9%)
6. Knowledge of the nature of science (13%)7. Knowledge of measurement (5%)8. Knowledge of appropriate laboratory use and
procedure (4%)
Two Key Numbers• Atomic Number
– # of Protons in an atom– This determines the type of
element you have!– If atom is electrically neutral,
then the number of electrons is also equal to this number
• Mass Number– # of protons + neutrons in an
atom’s nucleus– Mass # - atomic # = # of
neutrons
P Orbitals• Orbital that can contain
up to 6 electrons• Contains 3 sub-orbitals,
each holding 2 electrons
• “Peanut” or “Dumbbell” shaped
D Orbital• Orbital that can contain
up to 10 electrons• Contains 5 sub-orbitals
that can each hold 2 electrons
F Orbital• Orbital that can contain up to
14 electrons• Contains 7 sublevels each
holding 2 electrons
1s2s 2p3s 3p 3d4s 4p 4d 4f5s 5p 5d 5f6s 6p 6d7s 7p8s
This is the order used to
place electrons- follow the arrows to
their “end”, then move to
the next arrow
Alkali Metals• HIGHLY Reactive Metals• 1 valence electron
– Filling their “S” orbital• Do not occur naturally in nature as
elements– ALWAYS found in compounds
• React with water with increasing violence as atomic number increases
Alkaline Earth Metals• 2 valence electrons• Fill their “S” orbitals• Do not occur in nature as elements
– ALWAYS in compounds• Less reactive than the Alkali Metals
Transitional Metals• Most have 2 valence electrons
– These fill their “D” sublevels• Harder and more brittle than the other
metals• High melting and boiling points• Good heat and electrical conductors• Hg- the ONLY metal to be in the liquid
state at room temperature• Often have colored compounds
Lanthanide Series• Elements Ce thru Lu• Once called the “Rare Earth Metals”• Fill their 4f orbitals• All elements within this section have
amazingly similar chemical and physical properties– This lead to the difficulty in identification of
the elements in this section
Actinide Series• Elements Th thru Lr• Fill their 5f orbital• All elements are radioactive• Beyond Uranium, these elements
have been artificially created
Metalloids/Semi-Metals
• All are solids at room temperature• Semi-conductors of heat and
electricity• Some metal properties and non-
metal properties• Fill their “P” level electrons
Non-Metals
• Poor (Non) Conductors of heat and electricity
• Reactive• Diatomic Elements• Gas
– Nitrogen, Oxygen, Hydrogen• Solid
– Carbon, Phosphorus, Sulfur, Selenium
Halogens
• Diatomic Elements or found in compounds
• HIGHLY Reactive• Gases= Fluorine, Chlorine• Liquid = Bromine• Solid = Astatine, Iodine
Noble Gases
• Non-Reactive• We have FORCED it to react and form
compounds with Fluorine• Uses:
– Neon, Argon, Krypton and Xenon are used for lighting
– Helium is used in balloons
Practice
What is the frequency of a wave whose wavelength is 4.5x10-5m?
• C = l x v• 3x108m/s= 4.5x10-5m •v• 3x108m/s = 4.5x10-5m= 6.7 x 1012 Hz
What’s a Quantum??
The amount of energy that can be gained or lost by an atom
E = h x vE = Energy of Quantum
h = 6.626 x 10-34 J•s (Planck’s Constant)v = frequency of the wave
Practice
• What is the energy of a wave whose frequency is 2.5x10-4Hz?
• E = h x v• E= (6.626 x 10-34 J•s)(2.5x10-4Hz)• E=1.65x10-37J
Practice
• What is the mass of a particle whose energy is 2.41x10-27J?
• E = mC2
2.41x10-27J = m(3 x 108 m/s)2
2.68x10-44kg
Unstable Nuclei
Radioactive DecaySpontaneous disintegration of a nucleus into a
smaller sized nucleusNuclear RadiationParticles emitted by a decaying nucleus
All elements above #83 on the Periodic Table
Two Categories
FissionWhen a heavy nuclei splits into
more stable nuclei of intermediate mass
FusionWhen low mass nuclei combine to
form a heavier more stable nucleus
Types of Particle DecayParticle Symbol What stops this particleProton 1
1p A few sheets of paperNeutron 1
0n A few centimeters of leadBeta
Particle(electron)
b-, 0-1b, 0
-1eA few sheets of aluminum foil
Positron b+, 0+1e
A few sheets of Aluminum Foil
Alpha Particle
42He, a, a2+ Skin or one sheet of paper
Gamma Ray
00g, g Several centimeters of lead
Nuclear Reactions42
19K 0
-1e + ?
4240
Ca239
94Pu ? + 235
92U
42He
2713
Al + 42He 30
15P + ?
10n
? + 10n 142
56Ba + 91
36Kr + 31
0n
23592
U
Half-LivesRemaining Mass = half-life fraction
Total Mass1 = ½ 2 = ¼ 3 = 1/8 4 = 1/16
5 = 1/32 6 = 1/64 7 = 1/128 8 = 1/256
# h.l = time elapsed time of 1 h.l
Amount remaining = (original)(1/2)#h.l
Practice
How much of a 100.0g sample of Gold-198 remains after 8.10 days if its half life is 2.70 days?
12.5gA 50.0g sample of 14N decays to 12.5g in
14.4 seconds. What is its half-life?7.2 seconds