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Chemistry Final Exam Study Guide
What do chemists study?
What are the steps of the scientific method? What occurs at each step?
Be able to identify variables: Independent, dependent, control
Matter
Identify each of the following as either a physical or chemical change.
Melting
evaporation
Rusting
cutting
Bending
tarnishing
Food spoilage
polishing
Freezing
corrosion
Burning
rusting
Exploding
melting
What happens to the atoms that make up a compound involved in a chemical reaction.
What are three ways a mixture of various liquids can be separated into the individual pure
substances.
13. Classify the following as homogeneous or heterogeneous
mayonnaise
pepsi
chunky peanut butter
2% milk
chocolate chip cookie
vanilla milk shake
Which states of matter (gas, solid, liquid) are compressible?
Which states of matter is the volume uniform but the shape depends on its container?
What is the basic principle that allows chromatography to be used as a technique to
separate mixtures. Why does it work?
How does distillation work? What are the key parts of a distillation apparatus? Draw a
diagram.
How does a centrifuge separate a mixture?
What are some indications that a chemical reaction is taking place?
Why are chemical compounds such as water as well as elements such as oxygen both
considered “pure substances”. Explain
Identify the reactants and the products in a chemical reaction such as:
sodium + chlorine sodium chloride
What does the Law of Conservation of Matter say?
Does the following chemical equation obey the law of conservation of Matter? Explain
why.
C2H5OH + 3O2 2CO2 +3H2O
How are chemical changes different from physical changes?
Classify the following as either pure substances, homogeneous mixtures or heterogeneous
mixtures. Air, NaCl, Milk, H2O, sand, gatorade
States of Matter
Characteristics of the states of matter: Check a box if it applies to the state.
SOLID
LIQUID
GAS
change
shape
change
mass
change
volume
change
density
have
"flow"
Which characteristics are physical? Which are chemical? Circle the physical
characteristics.
mass
volume
boiling point
density
rough
solubility
reacts with oxygen reacts with water
viscosity
combustible
reactivity
solvents
melting point
sticky thick
brittle
Measurement
Topics:
Measurement and estimation
Accuracy and Precision
Scientific Notation
Dimensional Analysis/Unit Conversion
Density calculations
Percent Error- know this equation!
Review Homework Packet!
Useful pages: 40, 44, 46-48, 61 (sections 1-3)
11) You have the Heebie-Geebies. Your grandmother sends you a remedy for the
Heebie-Geebies with the following instructions: “Take 1 drop per 10 lbs. of body
weight per day divided into 4 doses until the Heebie-Geebies are gone.” How
many drops do you take per dose??
12) You’re throwing a pizza party for 15 people and figure that each person will eat 4
slices. You call up the pizza place and larn that each pizza will cost you $14.78 and
it will be cut into 12 slices. How much is the pizza going to cost you? You only
have $70. Will you have enough money?
13) Every three times I clean my bedroom, my mother makes me an apple pie. I
cleaned my bedroom 9 times. How many apple pies does she owe me? (What?!
Your mother doesn’t reward you for cleaning your bedroom? Aren’t there child labor
laws? To make up for that injustice, you may have this very easy problem.)
14) In my chemistry class, 28 students are each given 3 pens. If there are 8 pens in
one package, priced at $1.88 per package, what is the total cost of giving away
pens?
Structure of the AtomVocab:
Dalton’s Atomic Theory
Atom
Cathode ray tube
Nucleus
Subatomic particle
Electron
Proton
Dalton’s atomic model
Thompson’s atomic model
Rutherford’s atomic model
Neutron
Atomic number
Isotope
Mass number
Atomic mass unit (AMU)
Alpha particleBe able to
illustrate/interpret the following:
Atom Model: location and charge of Protons, neutrons, and electron
Cathode ray tube- all parts and it worked
Gold Foil Experiment- all parts and how it worked
Who are the following and how did they contribute to our knowledge of the Atom?
Democritus
J. Dalton
J.J Thomson
E. Rutherford
J. Chadwick
1. What is the smallest particle of an element that retains the properties of that
element?
2. What is the definition of an AMU of atomic mass unit?
3. Diagram an atom such as Lithium, showing where the protons, neutrons and
electrons are located in an atom, as well as the correct number of each.
4. Describe the characteristics such as mass and charge for protons, neutrons and
electrons.
5. Which of Dalton’s original theories of the atom are still considered true today?
b. Which are incorrect and why?
6. Determine the number of protons, neutrons and electrons in the following
elements: He, Au, Hg
7. What does the atomic number represent?
8. What does the atomic mass represent?
9. What is an isotope. How are they different form the normal atom?
10. Calculate the average atomic mass. See practice probs on worksheet.
Example: If an element is 69.2% of mass 62.93 amu and 30.8% of mass 64.93,
Calculate the average atomic mass.
11. Review each of the labs and demos we did in class.
a. What was the point of the Nuclear Marbles lab? How does this lab relate
to Rutherford’s Gold Foil Experiment?
b. How can one calculate the diameter of a marble by simply rolling and
colliding lots of marbles?
c. What was thee point of the Vegium Isotope Lab? What information is
needed to calculate the average atomic mass of an element?
d. What was the purpose of the Cathode Ray Tube Demonstration? What
does this demo show about the charge of an electron?
Atomic Structure
Fill in the blanks for the elements in this chart. For the purposes of this chart,
round all atomic masses to the nearest whole number.
Element
lithium
carbon
chlorine
silver
lead
calcium
Number of
Protons
Number of
Neutrons
Number of
Electrons
Atomic
Mass
Atomic
Number
Electrons
Vocab:
Electron
Valence electron
Frequency
Amplitude
Electromagnetic
spectrum
Quantum
Photon
Ground state
Quantum mechanical
model
Atomic orbital
Energy sublevel
Aufbau principle
Pauli Exclusion
Principle
Hund’s rule
1. Diagram a Bohr model of a Neon -20 atom. What do the rings represent?
2. What is Quantum of energy?
3. How is the Quantum Mechanical model of the atom different from the Bohr model?
How is the location of electrons described?
4. Write the electron configurations for any element using the periodic table. A table will
be provided BUT it will NOT be colored. Know your blocks and levels!
Such as sodium, and argon.
Na_____________________
Fe_____________________
Be able to write the noble gas configuration
Be able to identify elements from an electron configuration.
5. What are Hund’s Rule and Pauli’s Exclusion pricnciple, and the Aufbau principle?
6. Why does each element give off its own unique bright line spectrum of colors? How is
this phenomenon explained?
Is the amount of energy needed to move an electron up a level the same for every
element? Explain…
7. How did the flame test demo correlate with what we studied? Why was it such a crude
method to determine an unknown element?
8. Where in the “real world” would you observe the quantizing of elements and the
atomic spectra they emit?
9. Be able to calculate wavelength and frequency using (c=λν). Equation not provided
on test.
Nucleosynthesis
1.
2.
3.
4.
Where did all matter in the universe come from?
What is nuclear Fusion?
How to stars create new elements?
What is the biggest element (atomic number wise) that a star can
produce? What happen to the star after this element is made?
5. What is a super nova? What elements can be made here?
The Periodic Table and Periodic Law
Vocab:
Periodic law
Group
Period
Representative element
Transition metal
Metal
Alkali metal
Alkaline earth metal
Inner transition metal
Lanthanide
Actinide
Nonmetal
Halogen
Noble gas
Valence electron
Metalloid
Ion
Ionization Energy
Electronegativity
Atomic radii
1. How is the modern periodic table arranged? How are successive elements in a row
different from one another? Give some examples…
2. Who was the first to arrange the elements into a periodic table? What scientist help to
create the table we currently use today?
3. Identify the locations of metals, metalloids and non-metals. What are the general
characteristics of each type?
4. What elements are Noble Gases? What are the characteristics of these?
5. What elements are the halogens? What are the characteristics of these?
6. What elements are in the Alkali metal family. What are the characteristics of these?
7. How do valence electrons relate to reactivity?
8. Periodic Trends- Be able to explain how the following trends show up in the P-table.
 Atomic radii and Ionic radii
 Electronegativity
 Ionization energy
 Metal to Nonmetal
Ions
1. What is a valence electron? How can they be found using electron configurations
2. What is the Octet Rule? Explain.
3. How are Lewis dot structures written? How do they relate to valence electrons?
4. Define a cation and anion. Give an example of each.
5. Determine the number of electrons in a cation like Ca 2+ and anion like S26. Write the electron configuration of a Ca 2+ ion.
What is the relationship between the column number and the valence electrons in a
element? Give an example.
Ionic Bonding:
What force holds a cation to an anion when creating an ionic bond?
Identify the recipes for an ionic bond.
What charges do metal and nonmetals take on when e- are gained or lost.
What are the major characteristics of ionic compounds?
Why do ionic solutions conduct electricity and ionic solids do not?
Be able to write chemical formulas for ionic compounds.
Ionic Formula and Name Practice
Be able to write chemical names USING chemical Formulas.
1) zinc bicarbonate __________________________________
2) cobalt (III) phosphate _____________________________
3) gallium selenide __________________________________
4) strontium iodide __________________________________
5) titanium (IV) fluoride ______________________________
6) silver hydroxide __________________________________
7) lead (IV) perchlorate ______________________________
8) zinc hydride _____________________________________
9) potassium chromate _______________________________
10) iron (III) oxalate ______________________
Name these formulas:
11) PbO ________________________
12) Li3PO4 ______________________
13) TiI4 _________________________
14) Co3N2 ______________________
15) Mg3P2 ______________________
16) Ga(NO2)3 ____________________
17) Ag2SO3 ______________________
18) NH4OH ______________________
19) Al(CN)3 ____________________
20) Be(CH3COO)2 ________________