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Semester #1 Exam Review
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I. The Study of Matter and the Changes It Undergoes
1. Definitions: Matter, Physical Changes, Chemical Changes
Mattter –
Physical Changes –
Chemical Changes -
2. Classify the following as physical or chemical changes:
a. spoiling of milk ____________________
b. bending wire ______________________
c. cutting paper ______________________
d. rusting of a nail ____________________
3. Put the following into a graphic organizer/flowchart and define each: Matter, Pure substances - elements
and compounds, Mixtures - homogeneous (solutions) and heterogeneous
4. Identify the following as pure substances, homogenous mixtures or heterogeneous mixtures:
a. copper _________________________
b. sweetened tea ___________________
c. sand and water_____________________
d. d. calcium carbonate (CaCO3) _____________________
5. Sketch particles in the three states of matter. How close are the particles and how much do they move?
Solid
Liquid
Gas
II.
Atom
1. Definitions: Atom, atomic number, proton, neutron, electron, isotope, mass number, atomic mass
Atom Atomic number Proton Neutron Electron Isotope -
Mass number Atomic mass 2. Use the following diagram of Rutherford’s Gold Foil Experiment to draw conclusions.
What are four conclusions that can be draw from the illustration?
a) _______________________________________________________________________________________
b) ______________________________________________________________________________________
c) ______________________________________________________________________________________
d) ______________________________________________________________________________________
3. Characteristics of subatomic particles
Particle
Proton
Neutron
Electron
Mass
Charge
Location in Atom
4.
Element/Ion
7
Atomic
Number
Mass
Number
56
137
Protons
Neutrons
Electrons
20
20
56
18
Li
19 -
F
5. Why are enormous amounts of energy needed to separate the nucleus of an atom into its component protons
and neutrons even though protons in the nucleus repel each other?
________________________________________________________________________________________
________________________________________________________________________________________
6. Determine whether the following statements about protons and neutrons are true or false? (T or F)
_______Protons are twice as massive as neutrons.
_______Protons carry a +1 charge while neutrons have -1 charge.
_______Protons and neutrons are both composed of particles called quarks.
_______Protons and neutrons are both found in the nucleus of the atom.
_______Protons contain 2 up quarks and 1 down quark.
_______Stable nuclei for elements with atomic numbers less than 20 have a ratio of
protons: neutrons which is very close to 1:1
_______Isotopes of elements heavier than bismuth contain both radioactive and
stable isotopes.
7. Define ion:_________________________________________________________________________
_____________________________________________________________________________________
8. Complete the table.
Fluorine Atom
Fluoride Ion
Atomic Symbol
Protons
Electrons
Valence Electrons
9. Using Bohr Models, draw the formation of LiF salt.
Calcium Atom
Calcium Ion
III. Periodic Table
1. Locate or define parts of the periodic table:
GroupsPeriodsTransition metalsInner Transition metalsRepresentative ElementsAlkali metalsAlkaline-earth metalsHalogensNoble Gases-
2. Elements in the same __________ have similar physical and chemical characteristics because the
(group, period)
they have the same number of _________________ _
(atoms, protons, neutrons, electrons,
valence electrons)
3. Draw a electron dot diagram (or Lewis Dot structure) for Be and for N showing the correct number of
valence electrons
4. From their positions on the periodic table, what charges would the ions of Be and N have? Write the
dot diagram for the ions.
IV. Chemical Bonding, Formula Stoichiometry
1. Properties of Ionic Bonding: _______________________________________________________________
_________________________________________________________________________________________
2. Properties of Covalent Bonding (Including Polarity): ____________________________________________
_________________________________________________________________________________________
3. Identify as ionic or covalent compounds:
a. CaCl2 __________________
b. KI __________________
c. CH4 ___________________
d. Fe2O3__________________
e. C6H12O6__________________
f. SO2 ___________________
4. Explain the rules for writing formulas for ionic compounds._______________________________________
_________________________________________________________________________________________
5. Explain the rules for writing formulas for molecular compounds ___________________________________
_________________________________________________________________________________________
Chemical Formula
Chemical Formula
Lead (II) Hydroxide
Sulfur Dioxide
Chromium (III) Sulfate
Dinitrogen Pentoxide
Ba2+ and OH-
Carbon Monoxide
Iron (III) Sulfide
Heptaphosphorus Hexachloride
Na+ and OH-
Iodine Trifluoride
Ammonium Phosphate
Tetraphosphorus Decoxide
Magnesium Oxide
Carbon Tetrachloride
Chemical Name
Chemical Name
CaCl2
FeO
Mg(OH)2
N2O4
Fe2O3
P2O5
(NH4)2CO3
NO
V. Chemical Reactions
1. Definitions: chemical reaction, reactant, product, endothermic, exothermic
Chemical reactionReactantProductEndothermicExothermic-
2. Use the terms endothermic and exothermic correctly to describe chemical reactions in the laboratory.
_____________________a. A piece of magnesium metal is burned in the presence of oxygen
producing a bright light, heat, and magnesium oxide.
_____________________ b. A small amount of ammonium nitrate, a white solid, is placed in a baggie
and 10 mL of water is added. As the solid dissolves, the baggie begins to feel cold to the touch.
_____________________c. A small amount of vinegar is poured into a beaker and the temperature is
recorded at 22.0 oC. A spoonful of baking soda is added to the beaker causing the solution to bubble
and fizz. The temperature is found to decrease to 20.5 oC.
_____________________d. A small piece of magnesium metal is place in a test tube containing
hydrochloric acid. The solution bubbles and fizzes until all of the metal has reacted. The tet tube feels
warm to the touch.
_____________________e. Lighting the Bunsen burner in the lab requires methane gas to burn in the
presence of oxygen producing heat and light as well as carbon dioxide gas and water vapor.
3. Balance the following equations.
a. ____ Al + ____ O2  ____ Al2O3
b. ____ Cu + ____ AgNO3  ____ Ag + ____ Cu(NO3)2
c. ____ Zn + ____ HCl  ____ ZnCl2 + ____ H2
d. ____ Fe + ____ Cl2  ____ FeCl3
4. Write a balanced chemical equation for the following reactions.
a. Aqueous solutions of ammonium chloride and lead(II) nitrate produce lead(II) chloride precipitate
and aqueous ammonium nitrate.
b.
Solid carbon disulfide burns in oxygen to yield carbon dioxide and sulfur dioxide gases.
c.
Iron metal reacts with aqueous silver nitrate to produce aqueous iron(III) nitrate and silver metal.
d.
Solid potassium nitrate yields solid potassium nitrite and oxygen gas.