Download 1 st Nine Weeks Study Guide for Chemistry

1st Nine Weeks Study Guide for Chemistry
In Correlation with the Suffolk Public Schools Pacing Guide
Answer each question on a separate sheet.
1. Lab Safety and Equipment
A. If you spill acid on a lab table, what is the best way to clean it up?
Sprinkle baking soda on it. Wipe with paper towel.
B. List at least 5 safety rules and/or procedures in the laboratory classroom that MUST
be followed.
1. Follow directions
2. No horseplay.
3. Throw all broken glass in glass disposal. Not trash can.
4. Wear safety goggles.
5. Tie back long hair.
6. Wear closed toe shoes.
7. No smelling or eating chemicals.
8. No food or drink.
C. What is an MSDS sheet? What is its use?
MSDS Sheet is material safety data sheet. Used to get information about
substances.
D. What can be said about the chemical using the MSDS sheet below?
MATERIALS SAFETY DATA SHEET
PRODUCT IDENTIFICATION PRODUCT NAME
FORMULA
FORMULA WT 36.48 EFFECTIVE 08/07/86 REVISION # 02 PRECAUTIONARY LABELING
BAKER SAF-T-DATA (TM) SYSTEM HEALTH 3 - SEVERE (POISON) FLAMMABILITY 0 - NONE REACTIVITY 2 MODERATE CONTACT 3- SEVERE (CORROSIVE) HAZARD RATINGS ARE 0 TO 4 (0 = NO HAZARD; 4 =
EXTREME HAZARD) LABORATORY PROTECTIVE EQUIPMENT GOGGLES & SHIELD; LAB COAT & APRON;
VENT HOOD; PROPER GLOVES PRECAUTIONARY LABEL STATEMENTS POISON DANGER CAUSES
SEVERE BURNS MAY BE FATAL IF SWALLOWED OR INHALED DO NOT GET IN EYES, ON SKIN, ON
CLOTHING. DO NOT BREATHE VAPOR. CAUSES DAMAGE TO RESPIRATORY SYSTEM (LUNGS), EYES AND
SKIN. KEEP IN TIGHTLY CLOSED CONTAINER. LOOSEN CLOSURE CAUTIOUSLY. USE WITH ADEQUATE
VENTILATION. WASH THOROUGHLY AFTER HANDLING. IN CASE OF SPILL NEUTRALIZE WITH SODA ASH
OR LIME AND PLACE IN DRY CONTAINER.
Most likely an acid.
E. What is the correct way to pour and acid? Pour the acid into the water.
F. An experiment was conducted to test the effectiveness of four different fertilizers on plant
growth. Two grams of each fertilizer were to be diluted in 9 milliliters (mL) of water before
adding to a plant. Which of the following measuring devices would introduce the least error
into the measurement of the 9 mL of water?
a. 10 L graduated cylinder
b. 10 mL graduated cylinder
c. 10 mL beaker
d. 10 L beaker
Probeware is used to measure accurately.
Crucible and cover is used to heat small amounts of
chemicals.
G. What is the correct procedure to measure a liquid with a graduated cylinder? Eye level and
read the bottom of the meniscus.
H. What is the volume in the picture below? 34 mL( Each increment is 2 mL)
2. Experimental Design
A. Define the parts of the experimental design.
Title:
Problem: The question you are trying to find out.
Hypothesis: If _____IV_____ then ____DV_____ statement.
IV: What you know already before the experiment. The manipulated variable.
DV: What you are trying to find out. The results.
Control: The norm you are comparing you results to.
Constants: The things that stay the same.
Materials
Safety
Procedure-Steps in the experiment.
Data and Observations-Everything you observe and record in the experiment.
Conclusion and Analysis: Where you analyze data, graphs, and proving or disproving your
hypothesis with explanation.
B. What are the IV and DV in this data table?
IV: Wave intensity
DV: Crop Yield
Experimental Plot is experimental group
All the other are constants.
Draw a line graph on How far Ms. Jacobs can run in ten minutes. Label: the IV, DV,
Title, Units. X axis is Time in minutes
Y axis is distance in miles
Title: Ms. Jacobs Run
C. What is collaboration? Why is it important?
Collaboration-Working with other scientists or people for a common goal.
It is important because it can lead to more discoveries and information in science.
3. Reporting Scientific Data
A. Define qualitative data. Give three examples.
Data that is observed or changes appearance. Examples include: bubbling, changes color,
smells like rotten eggs.
B. Define quantitative data. Give three examples.
Data that is measured and includes numbers. Examples include: 3 cm, something
45 grams, there are 4 red candies.
weighs
C. Why is it best to do as many trials in an experiment as possible? 3 to see if data is
valid.
D. What are some possible sources of error in experiment?
Measuring incorrectly, using different pieces of equipment, not writing down correct
units.
E. Define accuracy and precision.
Accuracy-How close it is to the true value.
Precision-How many times you can get the same measurement (reproducibility) over
and over.
F. Explain whether the following data is accurate, precise, or both. Explain why.
If you did an experiment where you found the data in a density lab to be (the true value of
the density of aluminum is 3.2 g/mL): (Find average first)
Trial 1 Density
3.98 g/mL
Trial 2 Density
3.7 g/mL
Trial 3 Density
5.85 g/mL
Not accurate not precise
G. What is the formula for percent error?
[measured value-accepted value]/accepted value X 100=%
H. Find the percent error for a measured value of 2.3 g and the accepted value is 3.6 g.
[2.3-3.6]/3.6 X 100=36.11%
I. What would be a possible conclusion for this data?
Amylase increases starch digestion
J. What are the rules for determining significant figures?
K. What are the rules for rounding?
L. What are the rules for adding or subtracting significant figures?
Use the least amount of decimal places
M. What are the rules of multiplying or dividing significant figures?
Use the least amount of sig figs.
N. Do the following problems:
1. 5.678g + 0.895g = 6.573 g
2. 3.456mL - 9.0mL = -5.5 mL
3. 5.34 mol X 400 mol = 2000 mol
4. 3.4 g/20g = 0.2 g
O. Do the following scientific notation problems.
1. 3.4 X 10-6 X 4.3 X 108 = 1.462 X 103
2. 7.8 X 10-23/5.4 X 10-22 = 1.44 X 10-1
P. Convert the following using Dimensional Analysis:
1. 4.5 km to cm = 450,000 cm
2. 3.4 g to mg = 3400 mg
3. 2.45 mL to cm3 = 2.45 cm3
4. Convert 252 K to Celsius 252-273=-21 degrees Celsius
5. Convert 343 K to Celsius 343-273=70 degrees Celsius
6. Convert 25 Celsius to Kelvin add 273. 25+273= 298
4. Matter and Energy
A. What is formula for density? What are the units? D=m/v g/mL
B. What is the density of a liquid that weighs 6.00g and has a volume of 8.7 mL?
0.69 g/mL
C. What is the density of an object that weighs 2.3g and its length, width and height
is 9.0cm? 0.00315 g/cm3
D. What are the two types of matter? Pure substance and a mixture
E. How do you tell an element from a compound? Element is one type of atom, a
compound is two or more elements chemically combined.
F. What are physical properties? Give at least five examples.
Have to do with appearance, density, malleable, ductile. Boiling point
G. What are chemical properties? Give at least three examples.
End up changing the substance in question. Flammability, Corrosive, combustible
H. What is the difference between a chemical and physical change?
Chemical change you cannot get back, it is totally different.
Physical Change you can get back it is still the same substance.
I.
Which of the following is an example of a chemical change?
A. Leaves changing color
B. Dry Ice subliming
C. Melting ice
D. Water evaporating from a watch glass
J. What are the three phases of matter? Describe the characteristics of each. Solid,
liquid, gas (see notes for characteristics)
K. Fill in the chart below:
Phase change
Change
Example
Sublimation
Solid to a gas
CO2
Deposition
Gas to a Solid
Freezing
Liquid to a solid
Ice freezing
Melting
Solid to a liquid
Ice melting
Condensation
Gas to a liquid
Water condensing
(clouds)
Boiling
Liquid to a gas
Steam
L. What the two types of mixtures? Describe each.
Homogeneous-solutions, small size particles cannot differentiate.
Heterogeneous-larger size particles can see them. Different sizes.
M. What is the difference between an atom and a molecule?
Atom is one atom, molecule is two or more chemically combined.
N. What are the parts of a solution? Define each.
solute-What is being dissolved.
Solvent-what is doing the dissolving. Usually water.
O. Fill in the chart below:
Physical Means
Decant
Chromatography
Distillation
Filtration
Description
Pour off
Separates molecules using gravity
Separates by boiling point
Separates using filter paper
5. Atomic Structure
A. Define the Law of Conservation of Matter. Matter cannot be created or destroyed.
Part of Daltons postulates that still is true today.
B. What are the three parts of an atom? Electron, proton, neutron.
C. Fill in the following chart:
Subatomic
Location in the Mass
Charge
Where to find
Particle
Atom
it?
Electron
Outside on
Less than 1
Outside on
orbitals
orbitals
Proton
Inside the
1
+
Inside the
nucleus
nucleus
Neutron
Inside the
1
0
Inside the
nucleus
nucleus
D. List Dalton’s Four Postulates.
1. Law of Conservation of Matter
2. Atom is smallest unit of matter.
3. All atoms of the same element are the same.
4. Combination of atoms makes a compound.
E. Describe Rutherford’s Experiment and his discovery.
Discovered nucleus-gold foil experiment, most of atom is empty space and discovered
heavy mass in center of atom (nucleus)
F. Describe JJ Thomson’s Experiment and his discovery.
Discovered electrons , plum pudding model, used cathode ray tube.
G. Describe Bohr’s Model of the atom and his discovery.
Used several experiments to identify orbitals of electrons outside of nucleus in the
atom.
H. Define isotopes. Same number of protons different number of neutrons.
I.
Look at the table below. What does the data in the table suggest?
Protons
Neutrons
Atom X
1
0
Atom Y
1
1
A.
B.
C.
D.
J.
Electrons
1
1
The atomic mass of Atom X is 2 amu.
Atoms X and Y are two different elements.
Atoms X and Y are isotopes of each other.
The atomic number of Atom Y is 2 amu.
What kind of matter is described below:
Gas bubbles in soda.
a.
b.
c.
d.
A homogeneous mixture
A compound
A heterogeneous mixture
An element
K. When you observe C-12, and C-14, what does this tell you? The numbers represent
the mass of the atom. There are two different masses because they are isotopes of
each other.
L. Fill in the chart below:
Atom or
Ion
Element
Symbol
Atomic
#
Atomic
Mass
Protons
Electrons
Neutrons
Hydrogen
cation
Nitrogen
Anion
Metal or
Nonmetal
Hydrogen
H+1
1
1
1
0
0
Non metal
Nitrogen
N-3
7
14
7
1
7
Non metal
Magnesium
cation
Magnesium Mg+2
12
24
12
10
12
Metal
Silicon
Silicon
Helium
Oxygen
14
2
8
28
4
16
14
2
8
14
2
10
14
2
8
Semimetal
Non metal
Nonmetal
Helium
Oxygen
anion
Si
He
O-2
M. Define allotrope. Give an example. Same chemical formula, different chemical
structure. Example: diamond and graphite. All made of carbon.
N. What are monatomic atoms? Give example. All atoms that are not diatomic. Can
occur independently.
O. What are diatomic atoms? Give all examples. Occur in groups of two when they are
not with other elements. Example: H2, O2, N2, all the halogens.
P. What is radioactive decay? Write the formula below.
Decomposition of a nucleus.
A=Ao X 2 –t/h
A=Final amount
Ao=Initial Amount
t=time
h=half life
6.
A.
B.
C.
Q. You discovered a new radioactive isotope and named it boogonium (don't ask). Its
half life is 1.23 years. If you start with a sample of 45 grams, how much will be left in
6.7 years? h=1.23 years, Ao=45 grams, t=4.5 years, A=?
R. What is half-life? t ½ Time required for the number of nuclides to reach half the
original value.
S. What is amu? Atomic mass units. Units we weigh the atom.
Periodic Table
Define group. Also called families. Columns on the periodic table. There are 18 groups.
Define period. Rows in the periodic table. There are 7.
Fill in the chart below:
Name of Trend
Most
Trend
Atomic radii
Francium
Top to bottom, right to left
Shielding effect
Francium
Top to bottom, right to left
Electronegativity
Fluorine
Bottom to top, left to right
Electron affinity
Fluorine
Bottom to top, left to right
Ionization energy
Fluorine
Bottom to top, left to right
D. Fill in the chart below:
Group #
Group #1 s sublevels
Name
Alkali metals
Group #2 s sublevels
Group #3
Alkali Earth metals
Boron family
Group #17 p sublevels
Halogens
Group #18
Noble gases
Transition elements
Metals are on left side of
periodic table
Characteristics
Highly reactive with halogens
and water.
Found in Earth as ores.
Includes metals and
semimetals.
Highly reactive with alkali
metals. All non metals.
Chemically inert. Cannot bond
with anything.
D sublevels
Nonmetals are on right
side-separated by the
step except H.
E. What are valence electrons? How can they be determined? Valence electrons are in
the outer most shell and deal with bonding. They are determined by counting across
the periodic table.
F. Why do some elements have similar chemical properties? They have the same number
of? Same number of protons and in the same group.