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TEST - UNIT 3 - CHEMISTRY
Name:_______________________________
Date:________________________
You can use your notes, and a calculator. – 132 Points for this Test
Each problem is worth 3 points unless otherwise indicated
-------------------------------------------------------------------------------------------------------------------1. Compounds are produced when _______.
a. physical changes occur
b. a magic wand is waved over something
c. chemical changes occur
d. none of the above
2. The properties of compounds are _________.
a. different from the elements they are made of
b. the same as the elements they are made of
c. irrelevant to the elements they are made of
d. determined by a vote of congress
3. Formulas are _______
a. something scientists make up when they are bored
b. chemical shorthand names for compounds
c. none of the above
d. all of the above
4. In a chemical formula, subscripts show __________
a. the number of electrons in an atom
b. how many atoms there are of each element in a formula
c. how much it will go boom when you ignite it
d. none of the above
5. In a chemical formula, subscripts after parentheses ______
a. apply to every element within the parenthesis
b. apply to only those elements they are near
c. apply to none of the elements
d. they don’t apply, they only annoy
6. When atoms are chemically stable, they become ______
a. more likely to combine with other atoms
b. resistant to change or combination with other atoms
c. loose as a goose
d. none of the above
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7. Atoms become chemically stable when _______
a. they settle down and get a god job
b. they combine with other atoms
c. they are immersed in water
d. their outermost energy level is filled
8. All the noble gas elements are _____
a. stable and do not normally react with other elements
b. on the left side of the periodic table
c. insufferable at parties
d. none of the above
9. Chemical bonds are the forces that _______
a. keep electrons in their orbits
b. hold together the atoms in a compound
c. keep the world safe for democracy
d. none of the above
10. What are the energy levels of an atom?
a. how much vim and vigor the atom has
b. the orbitals in which electrons circle the atom’s nucleus.
c. the numbers of electrons in the atom
d. none of the above
11. We discussed two kinds of chemical bonds. Name them
a. covalent bonds
b. ionic bonds
12. Ions are charged atoms that have _______
a. received an electric shock
b. been dipped in hot sauce
c. lost or gained outer electrons
d. none of the above
13. If atoms lose electrons they become _______ _____ positive ions.
14. If atoms gain electrons they become _______ _____ negative ions.
15. The opposite charges of ions create attractions and make _____ _____.
a. covalent bonds
b. stocks and bonds
c. ionic bonds
d. none of the above
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16. Ionic bonds tend to be _______ _______
a. fairly strong
b. fairly weak
c. completely out of shape
d. none of the above
17. Covalent bonds include atoms that
a. are noble gases
b. shouldn’t be allowed out at night
c. share electrons with other atoms
d. none of the above
16. Covalent bonds tend to be _______ _______
a. fairly strong
b. fairly weak
c. really, really out of shape
d. none of the above
17. In polar molecules, shared electrons are usually _____
equally.
______
_________ not shared
18. This makes certain parts of polar molecules slightly _________ negative and other parts
slightly ________ positive.
19. Nonpolar molecules share electrons _________ equally and have no charged parts.
20. What is the difference between a mixture and a compound? (4 points)
In a mixture, components can be present in any proportion, and no chemical reaction
occurs in its formation. In a compound, the components have a definite proportion by
mass (the mass relationship), and a chemical reaction is required for their formation.
21. List the three Families of metals, and give an example of each (6 points)
a. Alkali Metals, ex. Sodium, Potassium
b. Alkaline Earth Metals, ex. Magnesium, Calcium, Barium
c. Transition Elements, ex. Iron, Copper, Silver, Gold, Zinc, and Mercury
22. List the three Groups of nonmetals
a. Hydrogen
b. Halogens
c. Noble gases
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23. List the three types of solutions
a. Gaseous solutions
b. Liquid solutions
c. Solid solutions
24. List the two parts of a solution, and briefly define what they are. (4 points)
a. Solute - the substance being dissolved
b. Solvent - the substance doing the dissolving
25. You can increase the rate of dissolving in most liquid solutions by three different methods.
List them below.
a. Stirring
b. Powdering the solute
c. Increase the temperature of the solvent
25. You can increase the rate of dissolving in most gaseous solutions by two different methods.
List them below.
a. Cooling
b. Increase pressure
26. Solubility is the _____________ _________ __ maximum number of grams of solute that
will dissolve in 100g of solvent at a certain temperature.
Concentration refers to amount of solute in the solvent.
27. Liquid-liquid solutions may be expressed by percentage by ________ volume.
28. Solid-liquid solutions may be expressed by percentage by ________ mass.
29. __________ Saturated solutions have all the solute dissolved as possible at a certain
temperature.
30. Unsaturated solutions could dissolve _____ ________ more solute.
31. Supersaturated solutions contain less solute than a saturated solution has at a certain
temperature. True or False (circle one)
32. Supersaturated solutions are generally created artificially and result in an _______ ________
unstable situation.
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33. In supersaturated solutions, the solute will quickly __________ crystallize if disturbed.
34. Water solutions of ionic compounds and polar compounds conduct __________ electricity.
35. Ionic compounds dissociate in solution causing ___________ ionization
36. Electrolytes are ____ ions in a water solution.
37. Adding solute to a solvent causes the freezing point of the solvent to____
a. lower
b. elevate
c. discombobulate
d. none of the above
37. Adding solute to a solvent causes the boiling point of the solvent to____
a. lower
b. elevate
c. discombobulate
d. none of the above
38. The amount of energy an electron has determines its _________ distance from the nucleus
39. A valence electrons are the electrons in the ________ outermost and incompletely filled shell
40. As you know, electrons behave like both a wave and a particle, depending on how we
measure them. The properties of a wave and the properties of a particle both contribute to the
stability of an atom. Explain briefly how each property contributes to an atom’s stability. (10
points)
The wave properties of an electron cause it to be repelled from the nucleus, while the particle
properties of an electron cause it to be attracted to the nucleus. This both prevents the atom from
collapsing in on itself, and from flying apart. Both which would be very bad for life as we know
it.
-------------------------------------------------------------------------------------------------------------------Extra Credit
41. List the four quantum numbers (8 points)
a. Principle Quantum Number
b. Orbital Quantum Number
c. Magnetic Quantum Number
d. Spin Quantum Number
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42. Briefly define the four quantum numbers (8 points)
a. The Principle Quantum Number is the electrons distance from the nucleus
b. The Orbital Quantum Number is the shape of the electrons orbital
c. The Magnetic Quantum Number is the electrons three dimensional position in space
d. The Spin Quantum Number is the direction of the electrons spin
43. I listed the first four orbital shapes for the orbital quantum number. What are the four letters
that represent these four shapes. (4 points) s, p, d, and f
44. Bob the neutron walks into a bar and asks the bartender for a glass of beer. The electron says,
"How much do I owe you??" The bartender replies, "For you - no charge!!" Do you think this
joke is funny? Why might it be funny, if one was inclined to laugh at such lame jokes? (2 points)
It’s not really very funny. It might be slightly humorous if one remembers that neutrons have no
charge.
45. Can you tell me who Schroedinger's Cat is? (25 points)
On June 7 of 1935, Erwin Schroedinger wrote to Albert Einstein to congratulate him on what is
now known as the EPR paper, a famous problem in the interpretation of Quantum Mechanics.
Soon thereafter, he published what was to become one of the most celebrated paradoxes in
quantum theory: Schroedinger's Cat. A cat is placed in a box, together with a radioactive atom.
If the atom decays, and the geiger-counter detects an alpha particle, the hammer hits a flask of
prussic acid (HCN), killing the cat. The paradox lies in the clever coupling of quantum and
classical domains. Before the observer opens the box, the cat's fate is tied to the wave function of
the atom, which is itself in a superposition of decayed and undecayed states. Thus, said
Schroedinger, the cat must itself be in a superposition of dead and alive states before the
observer opens the box, ``observes'' the cat, and ``collapses'' it's wave function.
This is much more interesting if one visits the bar with the neutron above.
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