Final Exam Review - KEY
AS – Chem 2012
1. a. variable that is changed by experimenter, the “I” change variable
b. variable that is being tested,
c. variable that is keep the same throughout experiment
2. a. brand of microwave popcorn, b. # of popped kernels, c. microwave, time, bag size, microwave setting
3. a. 2 b. 5 c. 3 d. 5
4. a. 2.40 X 104 b. 4.10 X 104 c. 5040 d. 4.90 X 104 e. 0.00240 f. 0.504
5. a. 1654.2
b. 30,000
c. 7534
d. 31
6. digits before the X as in #.###... X 10#
7. meter, gram, liter
8. a. 2.500 X 104
b. 2.5 X 10-4
c. 2.5 X 106
d. 2.5 X 10-6
9. density = mass/volume
10. a. 1 km = 1000 m
b. 1 cm = 0.01 m
c. 1 mm = 0.001 m
12. solid – definite shape, definite volume, difficult to compress, orderly arrangement of particles, vibrational
motion of particles,
liquid – shape of container, definite volume, difficult to compress, random arrangement of particles, random
motion of particle.
gas - no definite shape, no definite volume, easy to compress, most random arrangement of particles
most random motion of particles
13. melting – solid to liquid, snow to water on morning of potential snow day
vaporization – liquid to gas, boiling a cup of water
condensation – gas to liquid, water on side of cold drink on summer day
freezing – liquid to solid, water into ice cube
sublimation – solid to gas, dry ice
14. Pure substance – only one “thing” (elements or compounds)
Mixture – two or more “things” mixed together (chex mix, lemonade)
15. Heterogeneous mixture – mixture that is different throughout (chef salad)
Homogenous mixture – mixture that is same throughout (tan house paint)
16. Hund’s Rule - When electrons occupy orbitals of equal energy they don’t pair up until they have to
Aufbau Principle - Electrons enter the lowest energy level first.
Heisenberg Uncertainty Principle - It is impossible to predict both the speed and the location of an electron
at the same moment.
Pauli Exclusion Principle - at most 2 electrons per orbital - different spins
17. a. 1
b. 2
18. a. alkali metal
f. oxygen
c. 4
D. 7
b. alkaline earth metal
g. halogens
c. boron
d. carbon
h. noble gases
1
E. nitrogen
19. a. physical
b. physical
c. physical
d. chemical
20. When a substance changes into one or more new substances
21. A change in the physical form or property of a substance without a change in what it’s made of
22. a. physical
f. chemical
b. chemical
g. physical
c. chemical
h. physical
d. physical
i. chemical
23. electron, protons = neutron
24.
25. proton
26. a. 54
b. 18
c. 10
d. 74
27. protons, neutrons
28. a. 1, 2, 1
29. a.
108
47
Ag1+
30. a. 6
b. 43, 55, 43
b.
56
26
c. 34, 45, 34
d. 77, 115, 77
Fe
b. 10
c. 18
31.
32. a. 1s22s22p63s23p6
b. 1s22s22p63s23p64s23d6
c. 1s22s22p63s23p6
2
2
6
2
6
2
10
5
2
d. 1s 2s 2p 3s 3p 4s 3d 4p
e. 1s 2s22p63s23p6
33. a. 0
b. 2
c. 0
34. a. F, Br, Zn, Ba
b. Ba, Zn, Br, F
c. Ba, Zn, Br, F
35. a. Mg, Al, S, Cl
b. Cl, S, Al, Mg
c. Cl, S, Al, Mg
36.
2
e. physical
37. a. linear
b. trigonal planar
c. tetrahedral
d. trigonal pyramidal
e. bent
38. uneven sharing of electrons, a “pull” of electrons
39. yes, polar bonds can “cancel” each other thus making the molecule non-polar
40.
Formula
Lewis Structure
Geometric Shape Name
a. NO2+
b. OF2
c. SeS2
d. TeO3
e. SiBr4
f. PHI2
Linear
Bent
Bent
Trigonal planar
Tetrahedral
Trigonal pyramidal
41. a. ionic start with metal, or NH4, or H3O
42. 1 – mono
9 – nona
2 – di 3 – tri
10 – deca
4 – tetra
43. starts with a hydrogen
Polar or NonPolar
Non-polar
Polar
Polar
Non-polar
Non-polar
polar
b. molecular start with non-metal
5 – penta
6 – hexa
7 – hepta
b. has word acid
44. hydro…ic acid <-> comes from ide ending anions
…ous acid <-> comes from ite ending anions
…ic acid <-> comes from ate ending anions
45. a. has ● H2O
46.
Formula
FeCl3
N2O3
HC2H3O2
MgSO4  7H2O
Ba(OH)2
H2S
CuSO4 ● 5H2O
SO2
b. has hydrate at end of name
Compound Type
Ionic
Molecular
Acid
Hydrate
Ionic
Acid
Hydrate
Molecular
Name
Iron (III) chloride
Dinitrogen trioxide
Acetic acid
Magnesium sulfate heptahydrate
Barium hydroxide
Hydrosulfuric acid
Copper (II) sulfate pentahydrate
Sulfur dioxide
3
8 – octa
47.
Name
potassium iodide
diphosphorous pentaoxide
hydrofluoric acid
Iron(II) sulfate hexahydrate
carbon tetrachloride
calcium sulfate dihydrate
ammonium nitrate
hypochlorous acid
Compound Type
Ionic
Molecular
Acid
Hydrate
Molecular
hydrate
Ionic
Acid
Formula
KI
P2O5
HF
FeSO4 ● 6H2O
CCl4
CaSO4 ● 2H2O
NH4NO3
HClO
48. B, Si, Ge, As, Sb, Te, Po, At
49. non-metals right of metalloids
metals left of metalloids, except hydrogen
50. Element – one type of element
Compound – two or more different elements
51.
S
C
SR
D
DR
a.
b.
c.
d.
e.
Mg
+
Cl2
 MgCl2
2C6H6
+ 15O2
 12CO2 + 6H2O
2Al(NO3)3
+
3Mg
 3Mg(NO3)2 + 2Al
2LiClO3

2LiCl
+ 3O2
3Cu2O
+
2H3PO4  2Cu3PO4 + 3H2O
4