Download Matter and Energy Identify a chemical physical change Identify a

Matter and Energy
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Identify a chemical physical change
Identify a substance as either element compound mixture, etc
Endothermic vs. exothermic
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Physical or chemical change?
You make scrambled eggs
You light a candle
Iron combines with oxygen to form rust
Wood burn in the air
Milk turns sour
Crush a piece of chalk
Steam from your shower condenses on the mirror
Iron metal is melted
A rock is broken into smaller pieces
Salt dissolves in water
2.
Which is an example of a homogeneous mixture?
a. sand
c. vegetable soup
b. clean air
d. fresh-squeezed orange juice
3.
Which of the following is exothermic?
a. Solid to liquid
b. Liquid to solid
c. Solid to gas
d. Liquid to gas
4. Which formula represents a homogeneous mixture?
a. H2O(l)
b. H2S(g)
c. NaH(s)
d. HCl(aq)
Atomic Structure
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Thomson
Dalton
Rutherford
Atomic number
Mass number
How to find the number of protons neutrons and electrons
Isotopes
Part 1 – complete the chart
Atomic
symbol
Atomic
number
Mass Number
Protons
B
Neutrons
Electrons
6
11
24
31
37
39
29
89
35
43
100
207
Pb
102
70
89
Mo
225
53
Part 2 – answer the following
1. Describe Rutherford’s gold foil experiment, his conclusions, and his model of the atom.
2. Draw Thomson’s model of the atom.
3. How did the Dalton’s model of the atom look? Why did it look like that?
Part 3 – multiple choice
1. Today’s model of the atom is due to
a. The work of one scientist today
b. The work of one scientist from a long time ago
c. The work of many scientist today
d. The work of many scientist over a long period of time
2. As an ion is formed, the mass number
a. Increases
b. Decreases
c. Remains the same
3. If a neutral atom loses two electrons, the charge of the ion formed is
a. -2
b. -1
c. 0
d. +1
e. +2
4. Compared to a proton, an electron
a. Is smaller with the same charge
b. Is larger with same charge
c. Is smaller with opposite charge
d. Is larger with opposite charge
Modern Atomic Theory
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ROYGBIV
Energy, frequency
Orbital
Bohr model
Paramagnetic vs. diamagnetic
Isoelectronic
Aufbau Principle
Heisenberg Uncertainty Principle
Hund’s rule
Pauli exclusion Principle
Ground and excited state
Sublevels s p d f
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How many p orbitals can be in an energy level?
o 1
o 3
o 5
o 7
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According to the Pauli exclusion principle,
o Electrons fill in lowest levels possible
o Electrons will be placed in an empty orbital before pairing up to keep lowest energy
possible
o Orbitals can only hold 2 electrons causing no electron to have the same four quantum
numbers
o The exact position of the electron is unknown
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Given the following electron configuration, what are possible quantum numbers for the valence
electrons (in bold)? 1s22s22p1
o n=2, l=0, ml=0, ms=+1/2
o n=2, l=0, ml=0, ms=-1/2
o n=2, l=1, ml=1, ms=+1/2
o n=2, l=2, ml=-1, ms=-1/2
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Which color is associated with longest wavelength?
o Red
o Yellow
o Green
o Blue
How much energy is associated with a wave that has a wavelength of 6.5x10-7 meters?
Write electron configuration for Cl and draw an orbital diagram.
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Periodicity
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Properties of metals and nonmetals
Arrangement of the table
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Which element’s ionic radius is smaller than its atomic radius?
o Neon
o Nitrogen
o Sodium
o Sulftur
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Which group contains a liquid non-metal at STP?
o 12
o 14
o 17
o 18
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Which of these Group 14 elements has the most metallic properties?
o C
o Ge
o Si
o Sn
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At STP, which substance is the best conductor of electricity?
o Nitrogen
o Neon
o Sulfur
o Silver
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Boron and arsenic are similar in that they both
o Have the same ionization energy
o Have the same covalent radius
o Are in the same family
o Are metalloids
Bonding
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Properties of ionic and covalent
Bond formation energy
Polarity of bond
Polarity of molecule
Lewis structures
Part I – Bond Types
Ionic
Covalent
Metallic
Electrons are…
Between elements of…
Hardness…
Boiling Point…
Conductivity…
Example…
Part II – Polarity of a Bond
Polarity of a bond depends on the _______________________________ _____________________.
The more polar the bond the bigger the _________________________ _____________________.
Part III – Polarity of a Molecule
Polarity of a molecule depend on the ______________________ of the molecule.
Polar molecules are ________________________.
Non-polar molecules are ____________________. It is possible to have a non-polar molecule that has
polar bonds. Give an example of such a molecule.
Nomenclature
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How to name and write formulas
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Barium oxide ___________________________________
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Iron (II) Nitride _______________________________
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Cobalt(I) carbonate _____________________________
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Iron(II) Phosphate ________________________________
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(NH4)2SO3 ___________________________________________
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Mn2(CO3)3 _______________________________________________
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Mg(ClO3)2________________________________________
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Potassium Nitrate ____________________________________
Organic Chemistry
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Name
Saturated and unsaturated hydrocarbons
1. Draw the structure of 3-nonyne
2. Draw the structure of butane and state whether its saturated or unsaturated.
3. Draw the structure of 2-hexene.
Scientific Measurement
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Scientific notation
Metric conversion
Significant figures (identify, rounding, calculating)
Dimensional analysis
How many significant figures do the following numbers have?
1)
1234 _____
2)
0.023 _____
3)
890 _____
4)
91010 _____
5)
9010.0 _____
Convert the following numbers into scientific notation:
1)
3,400 _______________________________
2)
0.000023 _______________________________
3)
101,000 _______________________________
Convert the following numbers into standard notation:
9)
2.30 x 104 _______________________________
10)
1.76 x 10-3 _______________________________
11)
1.901 x 10-7 _______________________________