Download Review_WB_1

Review Workbook
By Mrs. Shapiro
Based on the textbook
Chemistry The Study of Matter
by Prentice Hall
Name _____________________________________________________________ Period ______________
Standard1 LAB Learn how to use lab appratus and learn how to write a proper conclusion.
1 Measurement
2 Use of glassware
3 Use of technology
4 Precision and Accuracy
5 % error
Precision and Accuracy
Three arrows are shot at a target. All 3 arrows hit the target within a distance of .1
cm of each. However, each arrow is at least 10 cm away from the bull’s eye of the
target. Does this histogram explain that data? ____________________
Comment on the accuracy and the precision of the arrows.
-10
0
10
Measurement
If I place an object in the graduated cylinder that has a volume of 10
ml, what will the new volume be? ____________ Draw a picture
showing the new volume.
An object measures 12.15 cm x 10.24 cm x 3.78 cm. What is the volume of the object?
___________________ What is the area? ________________ Show your work.
Percent Error Practice
(Observed Value - True Value)
Percent Error = -------------------------------------------------- x 100
True Value
1. Working in the laboratory, a student find the density of a piece of pure aluminum to be 2.85 g/cm3.
The accepted value for the density of aluminum is 2.699 g/cm 3. What is the student's percent error?
Standard 2 DATA Learn to represent and interpret data in a variety of formats.
1 Draw and interpret graphs
2 Make and interpret graphs
3 Significant figures
4 Scientific Notation
5 Record proper units
Graphing
What is the slope of the graph? _______
Based on the graph, estimate what time it will be in 85 meters? _______
Determine the linear equation the graph. y = mx + b
Using the linear equation, determine what the time will be at 100
meters?________________
Kilo Hecto Deca
<unit>
meter, liter, gram
Metric Conversions
1) 268 grams
=_____mg
=_____meters
2) 8 meters
= _____Km
3) 13 liters
=_____dL
4) 2.5 centigrams =_____grams
5) .03 Kilometers =_____cm
deci centi milli
6) 5,638 centimeters
7) .0096 Kilograms =
8) 2.85 milliliters =
9) 28 Decameters =
10) 8 liters =
_____decigrams
_____centiliters
_____Kilometers
_____deciliters
Significant Figures
1) 3.0800 ______
4) 91,600 ______
7) 0.0301 ______
2) 0.00418 ______
5) 0.003005 ______
8) 8000
______
3) 7.09 x 10-5 ______
6) 3.200 x 109 ______
9) 5.20 x 103 ______
a. 802.57 to 3 sf's
b. 802.57 to 2 sf's
Scientific Notation
a. (2.5 x 10-4) x (4.0 x 10-3) =
b. (2.5 x 104) x (4.0 x 103) =
d. (7.0x 107) / (3.5 x 105) =
e. (9.0 x 102) / (3.0 x 10-3) =
________________
________________
________________
________________
Standard 3 GAS LAWS Determine the relationship of a gas to the pressure, volume, temperature
and/or change in state of matter to the Kinetic Molecular theory.
Boyle P x V Practice
1. If some neon gas at 121 kPa were allowed to expand from 3.7 dm3 to 6.0 dm3 without changing the temperature, what
pressure would the neon gas ?
P
V
T
=
P
V
T
2. A quantity of gas under a pressure of 1.78 atm has a volume of 550 cm3. The pressure is increased to 2.50 atm, while the
pressure remains constant. What is the new volume?
P
V
T
=
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V
T
2) 390 cm3
Answers: 1) 75 kPa
Charles V/T Practice
1. What volume will a sample of hydrogen occupy at 28.0 oC at 2.23 dm3 . What will the volume be at temperature of 0.0 oC?
Assume that the pressure remains constant. (Remember Kelvin).
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T
=
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T
2. If a gas occupies 733 cm3 at 10.0 oC, at what temperature will it occupy 950 cm3? Assume that pressure remains constant.
P
V
T
=
P
Answers: 1) 2.02 dm3
V
T
2) 370 K
Gay-Lussac P/T Practice
1) If I initially have a gas at a pressure of 1.1 atm, what will the pressure be if I increase it from 298 K to 360 K?
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=
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2) A toy balloon has an internal pressure of 1.05 atm. If the temperature where the balloon is released is 20 0 C, what will the
temperature have to be when the balloon raises to an altitude where the pressure is 0.85 atm?
P
V
T
Answers
=
P
1.) 1.33 atm
V
2.) 460 K
T
If you place a bottle of seltzer that has pressure of 1.25 atm in the freezer
until it temperature until it reaches 15 C, what will the new temp if the pressure
decreases to 1.01 atm when the bottle is opened. What law would that obey?
Will it freeze when you open it?
Which picture best represents the relationship between volume and pressure?
What would happen to the kinetic energy and the pressure if you doubled the
particles? Draw what the particles look like? How many should be there?
What will happen to the pressure? _____________
What will happen to the volume? _____________
What will happen to the kinetic energy? _____________
What will happen to the temperature? _____________
Standard 4 MATTER Learn to apply the law of conservation of matter during a physical change
Separation of matter
Heterogeneous and homogenous mixtures
States of matter
Determine whether the molecules below are a solid, liquid, or gas. Then decide whether they are an element,
compound or a mixture.
Solid
Liquid
Gas
________
_______
_______
________
________
_______
Element
Compound
Mixture
________
_______
_______
________
________
_______
Physical and Chemical Property Practice
a. water boils at 100C
b. The pH of acid is 2
c. snow is hexagonal
d. the slope is 1 g/ml
e. density of H2O 1g/ml
f. salt is soluble in H2O
g. Floor tile is 1 ft x 1 ft
__________________
__________________
__________________
__________________
__________________
__________________
__________________
Densities
1. A student determines that a piece of an unknown material has a mass of 5.854 g and a volume of 7.57 cm 3.
2. Cobalt is a hard magnetic metal that resembles iron in appearance. It has a mass of 17.8 g and a volume of 2
cm3, what is the density?
3. A piece of was with a volume of 8.50 mL is found to have a mass of 8.06 g. What is the density?
4. What is the density of a piece of concrete has a mass of 8.76 g and a volume of 3.07 ml?
Standard 5 ELEMENTS AND FORMULAS Learn chemical nomenclature.
Symbols and names of elements
Naming and formulas
Atomic models
Element Practice
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
Li
Fe
S
P
Na
Ca
Ar
F
N
Cr
Au
Ga
Ag
Ti
Be
Ne
H
Zn
Co
Ni
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
____________
26. Iron
____________
27. Tungsten ____________
28. Carbon
____________
29. Arsenic ____________
30. Vanadium ____________
31. Platinum ____________
32. Gold
____________
33. Zirconium ____________
34. Tin
____________
35. Bromine ____________
36. Bismuth ____________
37. Antimony ____________
38. Iodine
____________
39. Xenon
____________
40. Gallium ____________
41. Aluminum ____________
42. Chromium ____________
43. Mercury ____________
44. Germanium___________
45. Uranium ____________
Evolution of Atomic Theory
1
1
H
19
9
F
Write the correct formulas and formula names
1. NH4+ and PO43- __________________
________________ _________________
2. H+ and BrO31- __________________
________________ _________________
3. Li+ and CO32- __________________
________________ _________________
4. Na+ and SO42- ____________________
________________ _________________
5. K+ and CrO42- ___________________
________________ _________________
Std 6
11. C4+ and Cl- __________________
________________ _________________
12. Sr+2 and CO32- __________________
________________ _________________
13. Ba+2 and BrO31- ________________
________________ _________________
14. B+3 and PO43- __________________
________________ _________________
15. NH4+ and HPO42- _______________
________________ _________________
PERIODIC TABLE Relate the chemical and physical properties of an element to its subatomic structure
and its position on the Periodic Table
Activity Series within a family
Electron Configuration
Ion formation
Bonding
Trends
Periodic Table Review Questions
1. Arrange the Group I metals in order of reactivity from most reactive to least reactive.
______________________________________________________________________
2. Is the same trend seen in the Alkaline Earth Metals, which was more reactive Ca or Sr?
______________________________________________________________________
3. Compare the reactivity of Na, K & Ca, in water. Which group is more reactive ( I or II)?
______________________________________________________________________
4. What is the trend in reactivity seen within the family 7 of the periodic table?
______________________________________________________________________
5. For metals what is the trend in reactivity seen within the same family of the periodic table?
______________________________________________________________________
6. Which would be the most reactive metal in the periodic table? ______ nonmetal?_______
7. Which metal is a liquid at Room Temperature? ____________nonmetal?_____________
8. What is the trend in reactivity seen within the family 8 of the periodic table? __________
9. Why are the noble gases so “noble”? ________________________________________
10.Complete the following by labeling the periodic table on the next page.
a. Label Group A 1 – 8 and Group B
b. Label Solids, liquids, and gases
c. Label s, p, d, and f sections
d. Label Non metals, metals, semi-metals LINE
e. Label alkali, alkaline, transition, halogens, and noble families
Std 7
EQUATIONS Learn to apply the law of conservation of matter during a chemical change
Recognize types of equations
Balance equations
Predict products
Energy is reactions
Molar ratios
Use the following choices to classify the type of reaction
a. Synthesis
b. Decomposition c. Single replacement
d. double replacement
1. ____Cu + ____ S  ____ Cu2S
2. ____ H2 + ____ Cl2 --> ____ HCl
3. ____ Ca + ____ H2O --> ____ Ca(OH)2 + ____ H2
4. ____ Na2O  ____ Na + ____ O2
Make sure the above equations are balance
2H2O  2H2 + O2
5. What is the volume of 1 mole of oxygen gas at standard temperature and pressure is?
6. How many moles of water are present?
7. How many grams of water will be needed?
Balance
______Na + H2O  _____Na2O + _____H2 + heat
8. Is this an exothermic or endothermic reaction?