Name_____________________________________
Period___
Practice Final 1st Semester 2011-2012
Chemistry 1
USE YOUR SPECIAL SHEET. YOU WILL HAVE ONE ON YOUR FINAL!!!!
Use your notes and textbook if that is helpful.
Properties of Matter
1.
State whether the following are observations or inferences and qualitative or quantitative:
a. A block of aluminum
weighs 5.2 g
b. A block of aluminum has
rust on one end
c. When exposed to a flame,
aluminum heats rapidly
2.
State whether the following are physical or chemical changes:
• Blue ink from a piece of paper turns water blue
• An electric current is passed through copper metal
• Sugar dissolves in hot coffee
3.
What is the mass of a cube that has a density of 0.9g/ml and a volume of 20ml?
4.
State whether the following are homogeneous mixtures, heterogeneous mixtures, compounds or
elements
• salt water
• Hydrogen gas
• gold
• Water and oil mixed together
5.
Explain the difference between an endothermic and exothermic reaction
6.
State whether the following are Chemical or Physical properties
• Iron can bend when exposes to extreme heat
• Pennies corrode when left out in the rain
• Alkali metals are highly reactive in the presence of water
History
7.
What did the Greek model of the atom look like?
8.
Draw a picture of Thomson’s and Rutherford’s models. How are they different?
9.
Draw a picture showing how “light” helped Bohr understand that Hydrogen atoms have energy
levels.
Atoms/Atomic Model
10. If chlorine has 2 naturally occurring isotopes, Cl-35 at 75% and Cl-37 at 25%, what is the atomic
mass of the element?
11. What is the relationship between the wavelength, frequency, and energy of electromagnetic
waves?
12. What is the speed of electromagnetic waves? What is the equation for speed, frequency and
wavelength?
13. Draw the Electromagnetic Spectrum of white light from lowest to highest energy
14. Explain why hydrogen emits 3 different colors when subject to electromagnetic radiation. Draw a
picture to illustrate this
15. Draw the Bohr model AND Lewis Dot structure for the following element:
a.
a. F
b. Ca
16. Fill in the following Chart:
Element/Charge Atomic
Number
Na
11
Mass
Number
23
Al3+
28
239
94
S
2-
# of
Protons
# of
Neutrons
# of
Electrons
15
16
18
18
17. Why does ionization energy increase as you go from left to right across a period?
18. Why does atomic radius increase as you go from top to bottom of the periodic table?
19. Name 4 properties of Metals and Nonmetals:
20. Do metals normally gain or lose electrons when forming bonds? Why?
21. Name 5 of the “Families”. Give an example of an element in each group and give a reason why is
is in that particular family.
22. Name 2 properties of Ionic compounds:
23. Name 2 properties of covalent compounds:
24. Write the following for each ionic compound:
Cation Charge
Anion Charge
Formula
Magnesium Bromide
Copper (II) Nitrate
Aluminum Sulfate
25. Write the names for the following ionic compounds:
• Na2SO4
• FeCl2
• Mg3(PO4)2
26. Fill in the appropriate blanks for the following molecular compounds
•
Dicarbon Tetrachloride
____________________
•
Hexane
____________________
•
____________________
N2I2
•
____________________
SiO2
27. Draw the Lewis Dot structure for the following molecular compounds:
• State whether it is polar or Nonpolar
• Include the shape or bond angle of each compound
NH3
CO2
CH3F
28. Complete, balance and state the type of reaction for the following:
b.
____ Ca(OH)2 + ____ Al2(SO4)3  ____ CaSO4 + ____ Al(OH)3
Type of reaction: _____________
c. ____ CH4 + ____ O2  ____CO2 + ____H2O
Type of reaction: _____________
29. Write the balanced equation out for the following word equations. Also state the type of reaction:
When isopropanol (C3H8O) burns in oxygen, carbon dioxide, water, and heat are produced.
When dissolved beryllium chloride reacts with dissolved silver nitrate in water, aqueous
beryllium nitrate and silver chloride powder are made.
30. Circle whether the following are acids or bases, and write the chemical equation for the following when
dissociated in water
HCl - Acid/Base
H2SO4 – Acid/Base
KOH – Acid/Base
31. Write the chemical equation for the neutralization of KOH with HCl
d.
Why is it a neutralization Reaction?
32. What is the principle reason why substances like oxygen have a low boiling point, but salt has a
very high melting point?
33. Draw a “general” graph of temperature over time, for the heating of solid Lauric Acid before,
during, and after its melting point.
34. Give three qualitative properties and one quantitative the property of acids and bases?
35. How do catalysts, temperature increases, and concentration increases allow chemical reactions to
occur more quickly?
36. Draw a graph showing how raising the temperature of a sample increases the rate of reaction.
Include: Collision Energy, # of particles, and Activation energy.
37. Why does the addition of a catalyst increase the rate of reaction?
Practice Final Answers
Chemistry 1
USE YOUR SPECIAL SHEET. YOU WILL HAVE ON ON YOUR FINAL!!!!
Use your notes and textbook if that is helpful.
Properties of Matter
1. State whether the following are observations or inferences and qualitative or quantitative:
a. A block of aluminum weighs 5.2 g
b. A block of aluminum has rust on
one end
c. When exposed to a flame,
aluminum heats rapidly
Quantitative
Observation
Inference
Qualititive
Observation
Qualitative
2. State whether the following are physical or chemical changes:
a. Blue ink from a piece of paper turns water blue
b. An electric current is passed through copper metal
c. Sugar produces heat and gasses in the presence of sulfuric Acid.
Physical
Physical
Chemical
3. What is the mass of a cube that has a density of 0.9g/ml and a volume of 20ml?
Mass
= Density x Volume
= 0.9 g/mL x 20 mL
= 18 grams
4. State whether the following are homogeneous mixtures, heterogeneous mixtures, compounds or
elements
a. salt water
homogeneous mixture
b. Water Vapor
Compound
c. Gold
Element
d. Water and oil mixed together
Heterogeneous Mixture
5. Explain the difference between an endothermic and exothermic reaction
Exothermic = A reaction that releases energy
Endothermic = A reaction that absorbs energy
6. State whether the following are Chemical or Physical properties
a.
b.
c.
Iron can bend when exposes to extreme heat
Pennies corrode when left out in the rain
Alkali metals are highly reactive in the presence of water
Physical
Chemical
Chemical
History
7. What did the Greek model of the atom look like?
Earth Wind Fire Water
8. Draw a picture of Thomson’s and Rutherford’s models. How are they different?
9. Draw a picture showing how “light” helped Bohr understand that Hydrogen atoms have energy levels.
Atoms/Atomic Model
10. If chlorine has 2 naturally occurring isotopes, Cl-35 at 75% and Cl-37 at 25%, what is the atomic mass
of the element?
Atomic Mass
=
=
=
(mass of isotope 1)(% abundance isotope 1)
+ (mass of isotope 2)(% abundance isotope 2)
+etc…
(35 amu x .75)
+ (37 amu x .25)
35.5 amu
11. What is the relationship between the wavelength, frequency, and energy of electromagnetic waves?
As wavelength ↑ Frequency and Energy ↓
As wavelength ↓ Frequency and Energy ↑
12. What is the speed of electromagnetic waves? What is the equation for speed, frequency and
wavelength?


The Speed of light=
=
c= λν
c
3 x 108 m/s
13. Draw the Electromagnetic Spectrum of white light from lowest to highest energy
14. Explain why hydrogen emits 3 different colors when subject to electromagnetic radiation. Draw a
picture to illustrate this
15. Draw the Bohr model AND Lewis Dot structure for the following element:
a. F
b. Ca
Will go over in class if needed
16. Fill in the following Chart:
Element/Charge
Na
P3Al3+
Pu
S2-
Atomic
Number
11
15
13
94
16
Mass
Number
23
31
28
239
34
# of
Protons
11
15
13
94
16
# of
Neutrons
12
16
15
145
18
# of
Electrons
11
18
10
94
18
17. Why does ionization energy increase as you go from left to right across a period?
As you go across the periodic table from left to right the following contributes to the increase in ionization
energy:
 Atomic Numbers increase (meaning the number of protons) and consequently electron numbers
increase as well
 Therefore, there is a greater attraction between the nucleus and the electron cloud because of the
increase in electric charge.
18. Why does atomic radius increase as you go from top to bottom of the periodic table?
As you go from top to bottom within a family on the periodic table the following contributes to the increase
in atomic radius:
 Each period increase means the increase of an energy level.
 An electron in the highest energy level is “shielded” from the attraction of the nucleus by the inner
electron energy levels.
19. Name 4 properties of Metals:






Good conductor of electricity and heat
On the left of the PT
Typically solid at room temp
Shiny, luster, malleable
Lose electrons to form positively charged atoms
Usually between 1 and 4 valence electrons
20. Do metals normally gain or lose electrons when forming bonds? Why?
Metals lose electrons more easily because:
 They have a large atomic radius
 They have a low ionization energy
 It is easier to lose electrons rather than gain in order to have a stable noble gas configuration (rule
of 8).
21. Name 5 of the “Families”. Give an example of an element in each group and give a reason
why it is in that particular family.





Alkali Metal
Alkaline Earth Metal
Transition Metals
Halogens
Nobel Gasses








22. Name 2 properties of Ionic compounds:
High melting point
Typically dissolves in water
Conducts electricity when dissolved



23. Name 2 properties of covalent compounds:
Any Phase
Made of nonmetals
Do not conduct electricity.
24. Write the following for each ionic compound:
Cation Charge





Na
Mg
Fe
Cl
Ar



Ends in s1
Ends in s2
Ends with d
Ends in p5
Ends in p6 (full valence shell)
Hard
Solids
Made of metals and non metals
Anion Charge
Formula
a.
Magnesium Bromide
Mg 2+
Br-
MgBr2
b.
Copper (II) Nitrate
Cu 2+
NO3-
Cu(NO3)2
Al 3+
SO42-
Al2(SO4)3
c. Aluminum Sulfate
25.
a.
b.
c.
Write the names for the following ionic compounds:
Na2SO4
Sodium Sulfate
FeCl2
Iron II Chloride
Mg3(PO4)2
Magnesium Phosphate
26. Fill in the appropriate blanks for the following molecular compounds
a. Dicarbon Tetrachloride
C2Cl4
b. Hexane
C6H14
c. Dinitrogen diiodide
N2I2
d. Silicon Dioxide
SiO2
27. Draw the Lewis Dot structure for the following molecular compounds:
a. Give the shape and bond angle of each
a. NH3
b.
Polar
107.3
Trigonal Pyramidal
Non-Polar
180
Linear
CO2
c. CH3F
Polar
109.5
Tetrahedral
Will go over in class if needed
28. Complete, balance and state the type of reaction for the following:
3Ca(OH)2 + ____Al2(SO4)3  2Al(OH)3 + 3CaSO4
Type of reaction: Double Displacement
____ CH4 + 2 O2  CO2 + 2H2O
Type of reaction: Combustion
29. Write the balanced equation out for the following word equations. Also state the type of
reaction:
When isopropanol (C3H8O) burns in oxygen, carbon dioxide, water, and heat are produced.
2C3H8O(l) + 9O2(g)+  6CO2(g) + 8H2O(g)
When dissolved beryllium chloride reacts with dissolved silver nitrate in water, aqueous
beryllium nitrate and silver chloride powder are made.
BeCl2(aq) + 2AgNO3(aq)  Be(NO3)2(aq) + 2AgCl(s)
30. Circle whether the following are acids or bases, and write the chemical equation for the following
when dissociated in water
a. HCl - Acid/Base
b.
H2SO4 – Acid/Base
c.
KOH – Acid/Base
31. Write the chemical equation for the neutralization of KOH with HCl
HCl(aq) + KOH(aq)  H2O(l) + KCl(aq)
Why is it a neutralization Reaction?
Assuming the acid and base are of equal concentrations and volumes, the acid and base ions become water
while the Metal and nonmetal ions become an aqueous salt.
32. What is the principle reason why substances like oxygen have a low boiling point, but salt has
a very high melting point?
The attraction between the molecules through electrostatic forces (charge) Ionic compounds have a greater
attraction of charge, while nonpolar molecules, like oxygen, have relatively little charge to attract to one
another.
33. Draw a “general” graph of temperature over time, for the heating of solid Lauric Acid before,
during, and after its melting point.
34. Give three qualitative properties and one quantitative the property of acids and bases?
Acids
Bases
H+ or H3O+ ions
OHSour
Slippery feeling
Dissolve metal and carbonates
Does not dissolve Metal or Carbonates
Litmus blue turns red
Litmus red turns blue
pH < 7
pH > 7
35. How do catalysts, temperature increases, and concentration increases allow chemical
reactions to occur more quickly?



Temperature: By increasing temperature there are more molecules that are moving at or above the
Activation Energy. Therefore, there is a greater probability of collision between these molecules
and the reaction speed is increased.
Concentration: By increasing concentration there are more molecules that are moving at or above
the Activation Energy. Therefore, there is a greater probability of collision between these
molecules and the reaction speed is increased.
Catalyst: The addition of a catalyst decreases the activation energy allowing there to be more
molecules moving at or above the Activation Energy. Therefore, there is a greater probability of
collision between these molecules and the reaction speed is increased.
36. Draw a graph showing how raising the temperature of a sample increases the rate of reaction.
Include: Collision Energy, # of particles, and Activation energy.
37. Why does the addition of a catalyst increase the rate of reaction?
A catalyst lowers the activation energy. There will be a greater amount of particles colliding at or
above activation energy (Ea), thus increasing the chances of a reaction to occur. A catalyst does not affect
the concentration or temperature.