Unit 1 Packet - Page 1 of 6
Honors Chemistry - Unit 1 Chapters 1 & 2
Vocabulary:
EQ/Problem Set Due:
Element Quiz:
Test Date:
Vocabulary: Number your vocab and complete in order!
1 matter 2 temperature
3 physical change 4 chemical change
5 precipitate
6 chemistry
7 compounds
8 elements
9 solution
10 quantitative
11weight
13 length
14 SI
15 accuracy
16 precision
7 density
19 significant figures
20 heterogeneous mixture 21 homogeneous 22 endothermic 23 exothermic
Formulas/constants to be memorized:
metric conversions
given elements from handout
percent error (given)
12 mass
18 volume
density(packet)
Conversions that do NOT have to be memorized:
1 lb = 453.6 g
1 mile = 1.609 km
1 L = 1.0567 qts 1 oz = 28.35 g 4 qts = 1 gal
1 m = 39.37 in = 3.2808 ft = 1.0936 yd (all equal! Use any 2 in a conversion)
1 oz = 29.6 mL
OBJECTIVES:
Be able to apply the concept of significant digits when recording lab data
Memorize the metric system; be able to do both pure metric conversions and English-metric conversion. (You will be given
English-metric conversions).
Be able to calculate percent error from lab data.
Use factor label (dimensional analysis) to solve math problems and conversions.
Be able to do density problems.
Be able to explain the difference between accuracy and precision and weight and mass.
Be able to use the above vocabulary properly.
Be able to classify properties and changes as physical or chemical.
Understand and apply basic laboratory safety rules.
Be able to visually identify and correctly use lab equipment and safety equipment.
Know the fire escape route for the classroom and other safety procedures.
Be able to collect, assimilate, and draw conclusions from scientific data.
Unit 1 EQs: We will work on this together in class!
Directions: Please work neatly and follow the directions below. If I cannot find your answer, I cannot grade it!
 Work in order – circle your final answers! Include units on your answers.
 Show your work on all problems. Credit will not be given without work!!
What is chemistry – give 2 examples of chemistry in your everyday life.
List two common sense lab safety rules.
In lab you find the mass of an object to be 5.0 g the correct mass is 5.2 g – calculate your percent error.
ID the following as heterogeneous mixtures, elements, solutions or compounds:
A. Kool-Aid
B. ice C. pure gold coin
D. vegetable soup E. diamond F. salt
5. Id the following as physical or chemical changes:
A. Grass growing B. inflating a tire with air C. ice cream cone melting D. sugar dissolving in water E. water
absorbed by a paper towel
6. How many quarters in $10?
7. Convert: A. 55 meters to kmB. 25 mm to cm
C. 252 g to lb
8. What is the density of 20.0 g of a solution that has a volume of 38.2 ml?
10. When a sample of a metal that has a mass of 15.8 g is placed into a graduated cylinder containing water, the volume
increases from 16.0 ml to 19.5 ml.
A. What is the volume of the substance? B. What is the density of the metal?
C. Using your reference packet identify the metal
Unit 1 PROBLEM SET: Last page of packet – rip off and turn in – review work from past math/science classes.
1.
2.
3.
4.
Unit 1 Packet - Page 2 of 6
ELEMENTS TO BE MEMORIZED
Learn correct symbol and correctly spelled name.
Symbols have the first letter capitalized and the second letter is lower case.
I would recommend writing your elements on note cards!
Element Symbol/
Element Name
Al
Ar
As
Ag
Au
Ba
Be
B
Br
Ca
C
Cl
Cr
Aluminum
Argon
Arsenic
Silver
Gold
Barium
Beryllium
Boron
Bromine
Calcium
Carbon
Chlorine
Chromium
Element Symbol/
Element Name
Co
Cu
F
Au
He
H
I
Fe
Pb
Li
Cobalt
Copper
Fluorine
Gold
Helium
Hydrogen
Iodine
Iron
Lead
Lithium
Element Symbol/Element
Name
Element Symbol/
Element Name
Mg
Mn
Hg
Ne
Ni
N
O
P
Pt
K
Rb
Si
Na
Magnesium
Manganese
Mercury
Neon
Nickel
Nitrogen
Oxygen
Phosphorus
Platinum
Potassium
Rubidium
Sr
S
Sn
Ti
W
U
Zn
Zr
Silicon
Sodium
Strontium
Sulfur
Tin
Titanium
Tungsten
Uranium
Zinc
Zirconium
Notes:
Measurements in Chemistry
Measurements (3.25 cm) are different than other numbers (3.14159265).
Measurements represent an action by someone with some measuring instrument.
Measurements have built-in uncertainty; no measurement is exact.
Measurements have units.
What is accuracy?
Ex:
What is a precision?
Ex:
Practice problems:
Accurate?: Yes / No
Precise?: Yes / No
Accurate?: Yes / No
Precise?: Yes / No
Accurate?: Yes / No
Precise?: Yes / No
A way to measure accuracy is: Percent error: = │ correct value – your value│ X 100
correct value
Unit 1 Packet - Page 3 of 6
Example: In lab you weigh a sample and find the mass to be 28.9 g. The correct mass is 27.0 g. Calculate your
percent error.
Practice problem: You find the volume of a sample of water to be 2.54 ml, the correct volume is 3.21 ml –
Calculate your percent error.
Significant digits (figures): in a measurement consists of all known digits and one final estimated digit
Examples:
A.
B.
C.
____________
Practice on pg:
__________
__________
Scientific notation is used for very large or very small numbers: see worksheet in packet!
Chemistry - Matter and Its Properties pgs 10 -18
1. Differentiate between a physical and chemical property. Give two examples of each
2. Differentiate between a chemical and physical change.
The four signs of a chemical change are:
change in temperature
formation of a gas
formation of a precipitate (a solid from two solutions)
a color change (sometimes)
Endothermic reactions _______________________ heat (feel cold to the touch)
Exothermic reactions _________________________ heat (feel hot to the touch)
3. Describe the 3 states of matter.
4. A. On page 18, answer question # 2 and on page 26, answer question # 19.
Unit 1 Packet - Page 4 of 6
B. Id the following as physical vs chemical changes:
Iron rusts
ice melts
grass grows
salt dissolves in water
Fill in and use the following table to answer # 5
Matter
Looks different
(has different phases)
Looks the same throughout
(one phase)
Heterogeneous mixture
Examples:______________
Homogeneous substance
Element
Made up of one type of
Atom – periodic table
Solution
no set formula
Ex:________
Examples:______________
____________
Compound
has a set formula
Ex:___________
______________
2) Identify the following as heterogeneous mixtures, solutions (homogeneous mixtures), elements or
compounds: A. salt water
B. carbon dioxide
C. sugar
D. paper
E. air
F. pure copper
G. water
H. a pepperoni pizza
The following SI System Units must be memorized:
SI System
Unit
Symbol
Meaning
kilo
k
thousand – 1,000 or 103
hecto
h
hundred – 100 or 102
deca
da
ten – 10 or 101
Base
unit
L, m, g ,s
deci
d
tenth – 1/10 or 10-1
centi
c
hundredth – 1/100 or 10-2
milli
m
thousandth – 1/1000 or 10-3
Conversion Factor
(Examples)
1000m
1km
1 hm
100m
10 m
1 dam
1kL
1000g
1000L 1 kg
100 L
1 hg
1hL
100g
10 L
1 dag
1 daL 10 g
10 dm
1L
10 dg
1m
10 dL 1 g
100 cm 100cL 100 cg
1m
1L
1g
1000 mm 1 L
1000 mg
1m
1000mL 1 g
Base units – volume: L – liter; distance: m – meter; mass: g – gram; time: s – second, etc.
Problem solving in Chemistry and conversions
SI system: international system for measurement (metric system) used by all scientists – including us!
Use it to study quantitative data later we will study qualitative data.
SI – prefixes – base 10 system (see SI sheet)
Unit 1 Packet - Page 5 of 6
We will use the factor label method for problem solving.
Problem solving method where units are treated like algebraic units (may be cancelled out, multiplied etc like X
in algebra!)
STEPS FOR CONVERTING UNITS using factor label method
1. Start with your known information on the left side of math bracket. INCLUDE NUMBER AND
UNIT!!!!!!
2. Put the unit you are converting TO on the far right of the bracket.
3. Let your units drive your math ---- if you need to cancel a unit out that is in the numerator (on top)
THEN that unit needs to be in the denominator (on the bottom)
4. The larger unit gets the number 1, the smaller unit gets the conversion factor
Conversion factor: ratio used to convert from one unit to another
Example: quarters to dollars your original example of a conversion factor:
Example problem using conversion factors:
How many quarters in $75? Copy work!
You try: using a conversion factor: How many minutes in 5 hours?
More examples: you may need to use your SI chart initially – eventually you have to memorize the metric
conversions!
Example 2 : Convert 62 km to m
Example 3 convert 3.2 L to daL
You try: convert 320 cm to m.
Example 4 Convert 17000 mg to kg
You try: Convert 540 mm to dam
Unit 1 Packet - Page 6 of 6
Example 5 Convert 35 km to miles (use the metric to English conversions on the objective sheet – do not
memorize these = they will be given to you on the test!)
You try: Convert 2.31 lbs to g
You try # 2 convert 2 miles to meters
Example 6: 55 miles/hour to m/min
You try: 12.0 g/mL to lb/L
Example 7: You are running 6.8 miles per hour – how many minutes will it take you to travel 4.0 kilometers?
Dimensional Conversions Understand that 1 L = 1000 cm3 , 1 ml = 1 cm3 and 1L = 1 dm3
Volume or area of a solid is l x w x h = cubed unit
Liquid volume is one dimension
For cubed conversion units  # and unit are cubed
Conversions Practice Sheet
Metric Conversions
1. 8.5 dg to g ____________
4. 65 hm to m ____________
2. 0.23 g to cg ____________
5. 1.2 L to ml ____________
3. 876 cg to mg ____________
6. 87 hg to kg ____________
Other Conversions
7. 13 km to miles ____________
10. .72 L to gallons _________
8. 8.35 g to oz.
____________
11. 2760 ft. to miles________
9. 280 g to lbs. ____________
12. 27.3 m to ft. __________