Download Chemistry Fall Semester Review Sheet

Name: ___________________________
Chemistry Fall Semester Review Sheet
Lab Safety & Equipment:
1. What should you do if you get acid on your hands? Rinse with lots of water
2. How should you smell a chemical if you are instructed to do so? waft
3. When are goggles required? When using chemicals, heat or glassware
4. What should you do with broken glass? Dispose of broken glass in the broken glass container
Density, Kinetic Theory & States of Matter:
5. What are the three main states of matter? Solids, liquids & gases
6. Fill out the table below for the three states of matter
State
Compressibility
Shape
Volume
Kinetic energy
(high/low)
(definite/indefinite)
(definite/indefinite)
(high/low)
Solid
LOW
DEFINITE
DEFINITE
LOW
Liquid
LOW
INDEFINITE
DEFINITE
MEDIUM
Gas
HIGH
INDEFINITE
INDEFINITE
HIGH
7. Which phase is the most structured? The least? Solids are the most structured, Gases are the least
8. Label the following on the phase diagram on the right.
Gas
Liquid
Solid
Triple point
Critical point
Freezing
Evaporation/boiling
Sublimation
Condensation
Melting
Deposition
9. What is the density of carbon dioxide gas if 0.196 g occupies a volume of 100 mL?
D=m
V
D = 0.196 g
100 mL
D = 0.00196 g/mL
Directions: Use the data shown below to answer the following questions 10 and 11.
Substance
Density (g/mL)
water
1.00 g/mL
ethanol
0.78 g/mL
benzene
0.88 g/mL
10. If you poured all 3 liquids together and they did not mix, which substance would be the top layer?
Ethanol would be on the top layer
11. Identify the substance that has a mass of 8.1 grams and occupied a volume of 10.3 liters mL.
D = m/V
D = 8.1 / 10.3
D = 0.786 g/mL
= ETHAHNOL
Classification of Matter:
12. Identify each of the following as either an:
element, compound, homogeneous mixture or heterogeneous mixture
A. Pizza
_____Heterogeneous_____
C. Salt (NaCl)
_______Compound____
B. Vanilla Ice Cream
_____Homogeneous_____
D. Carbon
______Element______
13. Identify each of the following as either a: chemical or physical change
A. Burning
_______Chemical____
C. Boiling Water
______Physical______
B. Cutting paper
_______Physical______
D. Iron Rusting
______Chemical_____
14. A __compound__ can only be separated by chemical means.
15. List the 4 indicators of a chemical change:
Bubbles, heat, light & precipitate
16. Define the Law of Conservation of Mass.
Mass can’t be created or destroyed
17. Identify each of the following as either an: intensive or extensive property
A.
B.
C.
D.
Mass
Density
Volume
Texture
_____extensive_____
_____intensive_____
_____extensive_____
_____intensive_____
Atomic Theory:
18. Complete the following chart.
PARTICLE
CHARGE
MASS
LOCATION
proton
Positive
1 amu
nucleus
neutron
Neutral
1 amu
nucleus
electron
Negative
0 amu
Electron cloud
19. Define the law of multiple proportions.
Elements form compounds in simple whole number ratios
20. What do isotopes of the same element have in common and what is different?
Isotopes have the same number of protons, electrons and atomic number
Isotopes have a different mass number and number of neutrons
21. Explain how Rutherford’s gold foil experiment worked and what it proved.
Rutherford shot particles through gold foil. Most went through, but some bounced back. He concluded
that atoms are mostly empty space and the particles bounced off the dense center called the nucleus.
22. What subatomic particle determines the identity of an atom? Protons
23. How do you find the following:
A. Number of protons in an atom = __same as the atomic number__
B. Number of neutrons in an atom = __mass # - atomic #__
C. Number of electrons in an atom = __same as the atomic number__
Symbol
Atomic
Number
Mass Number Number of
Protons
Number of
Electrons
Number of
Neutrons
Ag
47
109
47
47
62
Mg
12
24
12
12
12
Ga
31
72
31
31
41
The Periodic Table & Trends:
24. The horizontal rows found on the periodic table are called __periods__, while the vertical columns are
called ___groups__ or ___families___.
25. The most reactive elements on the periodic table are in group __1A – Alkali Metals__.
26. Electronegativity ____decreases_____ (increases/decreases) going down groups and
______increases_____ (increases/decreases) going across periods from left to right.
27. Ionization Energy ______decreases_____ (increases/decreases) going down groups and
______increases_______ (increases/decreases) going across periods from left to right.
28. Atomic radius ________increases______ (increases/decreases) going down groups and
_______decreases_______ (increases/decreases) going across periods from left to right.
29. The number of valence electrons ________increases______ as you go across a period, but will
______stay the same____ as you go down a group.
30. The most electronegative element is ________Fluorine_____________.
31. The element with the largest atomic radius is _______Francium______.
32. Which of the following has a bigger atomic radius: Cesium or Calcium? (Circle one.)
33. Which of the following has a higher ionization energy: Potassium or Sulfur? (Circle one.)
34. Classify the following as either an: Alkali Metal, Alkaline Earth Metal, Halogen or Noble Gas
A.
Strontium
__Alkaline Earth Metal____
C.
B.
Bromine
___Halogen___
D. Krypton
Potassium
__Alkali Metal___
__Noble Gas____
Electron Configurations & EMR Calculations:
36. Write the long-hand electron configurations AND noble gas notations for the following atoms:
A. Calcium 1s22s22p63s23p64s2
[Ar]4s2
B. Iron 1s22s22p63s23p64s23d6
[Ar]4s23d6
37. What do the superscripts add up to in an electron configuration? ____the atomic number___
38. What is the energy of a photon whose frequency is 6.9 x 1014 Hz?
E=hxV
E = 6.63 x 10-34 x 6.9 x 1014
E = 4.57 x 10-19 J
E=hxv
h = 6.63x10-34 J·s
39. What is the packet of light called that is released when an electron relaxes to the ground state?
photon
Bonding & Ionic Compounds:
40. Name the following compounds:
A. BaCO3
_____barium carbonate____
B. NH4OH
_____ammonium hydroxide_____
C. NiCl2
_____nickel (II) chloride_____
D. MnCl3
_____manganese (III) chloride____
41. Write the formula for each of the following compounds:
A. Aluminum phosphate
______AlPO4____
B. Copper (III) sulfide
_____Cu2S3_____
C. Magnesium chloride
_____MgCl2____
D. Potassium nitrate
______KNO3____
42. Identify each of the following as either an: ionic or covalent bond
A. electrons are shared
__________covalent_______
B. electrons are transferred
_________ionic_________
C. MgCl2
________ionic_______
D. CO2
_________covalent__________
43. Why are metals malleable and ductile? _________metals have a “sea of electrons”______
Covalent Compounds & VSEPR Theory:
44. Write the name for the following compounds:
A.
SF8
____sulfur octafluoride___
B. SiH4
____silicon tetrahydride____
C. F2O
___difluorine monoxide____
45. Write the formula for the following:
A. Diphosphorus pentoxide
_____P2O5___
B. Dinitrogen tetrahydride
____N2H4____
C. Carbon monoxide
____CO_____
46. Show the covalent bonding diagram and identify the shape and polarity for the following:
CO2
CCl4
CH2O
Shape: ____Linear____
Shape: ____Tetrahedral____
Shape: ___Trigonal Planar___
Polarity: ____Nonpolar____
Polarity: ____Nonpolar_
Polarity: ___Polar___
PH3
HCN
H2S
Shape: __Trigonal Pyramidal_
Shape: ___Linear____
Shape: ____Bent____
Polarity: ____Polar___
Polarity: _____Polar____
Polarity: ____Polar____
Dimensional Analysis & Significant Figures
47. Determine the number of significant figures in each of the following numbers.
A. 8603 __4__
D. 52000 __2_
B. 11.00 ___4__
E. 40.5
___3_
C. 0.701 __3__
F. 0.00390 ___3__
48. Determine the answers to the following problems. Round your answer so that it has the correct number of
decimal places or significant figures.
A. 678 / 3.217 = 211
B. 16 + 5.18 = 21
C. 48.968 – 10.5 = 38.5
D. 0.0030 x 4560 = 14
49. Write the following numbers in scientific notation.
A. 456,000
__4.56 x 105_
B. 0.000071
__7.1 x 10-5__
C. 500,000,000
__5 x 10 8__
50. How many minutes are in 6.00 days?
6.00 days x 24 hours x 60 min = 8640 min
1 day
1 hour
51. How many inches are in 17.65 miles? (1 mile = 5280 ft)
(1 ft = 12 inches)
17.65 miles x 5280 ft x 12 inches = 1.12 x 106 inches or 1,120,000 inches
1 mile
1 foot
Mole Calculations
52. Calculate the molar mass for each of the following compounds.
A) KCl
____74.551 g/mol___
D) H2O
_____18.015 g/mol___
B) Mg3(PO4)2
____262.855 g/mol__
E) AlS
_____59.048 g/mol___
C) H2SO4
____98.078 g/mol____
F) Ca(NO3)2
_____164.088 g/mol__
53. How many moles of CO2 are in 56.3 Liters of CO2?
56.3 L x 1 mole = 2.51 moles
22.4 L
54. How many Liters are in 7.32 x 1024 molecules of O2?
7.32 x 1024 molecules
x
1 mole
x 22.4 L
6.02 x 1023 molecules
1 mole
=
272 Liters
55. Convert the following: 2.8 g Na = __________________ atoms Na
2.8 g Na x 1 mole x 6.02 x 1023 atoms = 7.33 x 1022 atoms
22.990 g
1 mole
56. Which of the following contains the smallest number of moles (circle):
1 gram of carbon, 1 gram of copper or 1 gram of barium
Percent Composition:
57. Define percent composition. The relative amount of an element in a compound
58. Calculate the percent composition of each element in CO2.
%C = 12.011 x 100 = 27.3 %C
%O = 31.998 x 100 = 72.7 %O
44.009
44.009
59. Calculate the percent by mass of hydrogen in water.
% H = 2.016 x 100 = 11.2 %H
18.015
60. Calculate the percent by mass of oxygen in water.
%O = 15.999 x 100 = 88.8 %O
18.015