Name: __________________________________________
Date: _________________
Class/Period: _____________________________________
Chemistry
Matter
1. Calculate the density of an object with a volume of 25 cm3 and a mass of 50. g.
2.0 g/cm3
D = m/V = 50. g/25 cm3 = 2.0 g/cm3
2. Find the mass of an object with a density of 5.0 g/cm3 and a volume of 20. cm3.
100 g
m = DV = 5.0 g/cm3 x 20. cm3 = 1.0 x 102 g
3. Find the volume of an object with a mass of 200 g and a density of 100 g/mL.
2 mL
V = m/D = 200 g/100 g/mL = 2 mL
4. How many significant figures are in the following numbers:
a. 5370
b. 200.
3
3
c. 2410.10
d. 2001
6
4
5. A mixture that is uniform throughout is classified as a
is not uniform in appearance is known as a
Homogeneous mixture whereas a mixture that
Heterogeneous
mixture.
6. A type of homogeneous mixture made of two or more metals is known as a(n)
Alloy.
7. Identify the following as a chemical or physical property or chemical or physical change.
a. copper reacts with oxygen to form a green patina
chemical
b. milk spoils
chemical
c. copper compounds are blue
physical
d. ice melts
physical
e. pancakes burn on a griddle
chemical
f. fermentation
chemical
g. an iron nail rusts
chemical
h. combustion
chemical
8. What is the difference between an element and compound?
An element is a pure
substance that appears on the periodic table and consists of
one type of atom. A compound is a pure substance that is
composed of 2 or more elements combined chemically and in
definite proportions.
9. Identify the following as elements, compounds or mixtures – if a mixture identify as homogeneous or
hetergeneous
Exampe
Element
Compound
Homogeneous
Air
Nitrogen
Mixture (tell type
Element
Compound
Potassium Chloride
Gasoline
Homogeneous
Gravel (with rocks and
Heterogeneous
sand)
Bromide
Copper (II) sulfate
Element
Compound
Atomic Structure
10. Define the term atom in your own words (do not copy the definition from the book)!
Class
consensus _______________________________________________________________________
11. C2H6 is an example of what?
a. ion
b. element
c. atom
12. Fill in the chart below concerning subatomic particles.
Subatomic Particle
Location
Proton
Nucleus
d. compound
Charge
Positive
e. mixture
Job of Particle
Identifies the
element
Adds to
Nucleus
0
atomic
mass
Balances
electron
Outside
Negative
charge of
nucleus
nucleus
What is an isotope? An isotope is an atom of the same element
Neutron
13.
with the same number of protons but a different number of
neutrons.
14. Calculate the number of protons, neutrons, and electrons of Magnesium-25.
# protons:
# neutrons:
12
13
# electrons
:12
15. Find the average atomic mass of Element X if 51.83% of Element X occurring in nature has a mass of 106.905
amu and 48.17% of the atoms have mass of 108.905 amu.
107.868 amu
Identity of Element X:
Isotope
X-107
X-109
Abundance (%)
51.83
48.17
Atomic Mass (amu) Decimal Product
106.905
.5183
55.4088615
108.905
.4817 + 52.4595385
107.8684
16. Circle the most abundant isotope of hydrogen:
know?
Ag
hydrogen-1, hydrogen-2, or hydrogen 3.
How do you
It is the closest to the atomic mass of hydrogen
appearing on the periodic table. Which has only 1 proton? They all have
one proton.
17. What is the atomic number of Uranium-238?
92
18. Write the full electron configuration for the following elements AND circle the valence electrons.
a.
titanium
b. bromine
1s2 2s2 2p6 3s2 3p6 4s2 3d2
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
19. Write the noble-gas configurations for the following elements AND circle the valence electrons:
a.
Calcium
[Ar] 4s2
b. Francium [Rn] 7s1
20. Draw the Lewis/Electron Dot structure for the following elements:
a. Sodium
b. Iodine
21. Fill in the following chart.
Sublevel
s
See whiteboard
c. Aluminum
d. Oxygen
# of Orbitals
# of electrons in sublevel
1
3
5
7
2
6
10
14
p
d
f
22. Explain the octet rule and the role of valence electrons in bonding.
The octet rule says that atoms tend to gain, lose or share
electrons so as to achieve eight electrons in their outer or
valence electron shell.
23. The fact that electrons occupy the lowest energy levels possible is known as the Aufbau Principle
whereas the idea that only two electrons of opposite spin can occupy a single orbital is known as the
exclusion Principle.
Finally,
Pauli
Hund's Rule states that single electrons with the same spin must
occupy each orbital before additional electrons with opposite spins can occupy the same orbitals.
Nuclear Chemistry
24. What type of radiation is emitted when Uranium-238 decays to Thorium-234?
Show the nuclear reaction below.
238
92U
-->
234
90Th
+
4
2He
Beta radiation
25. Fill in the chart below.
Type of Decay
Particle Emitted
What Can Stop It?
Rank from Least (1) to
Most Penetrating (3)
Alpha Decay (α)
Helium nucleus (42He)
Beta Decay ()
Gamma Decay
()
0-1e
Skin
Metal foil
Thick
concrete,
steel, lead
1
2
3
0
0
26. Use the chart below to answer questions a, b, and c.
Isotope 1
Mass Number
50
Percent Abundance/Occurrence
4.35 %
Isotope 2
52
83.79 %
Isotope 3
53
9.50 %
Isotope Mass Number(amu) Abundance (%) Decimal
1
50
4.35
0.0435
Isotope 4
54
2.36 %
Product
2.175
2
52
83.79
0.8379
43.5708
3
53
9.50
0.0950
5.035
4
54
2.36
0.0236
Totals
52.0552
a. What is the average atomic mass of this element?
b. What is the name of this element?
c. Isotope 4 has how many protons?
+ 1.2744
52.1 amu
Chromium
24
neutrons?
30
electrons?
24
27. The half life of DDT, a pesticide is 15 years. If 60 grams of DDT is released into the environment, how much
will remain after 60 years?
O years
15 years
30 years
45 years
60 years
60 grams
30 grams
15 grams
7.5 grams
3.75 grams
AR = IA(1/2)n
AR= 60 (1/2)60/15
AR = 60 (1/2)4
AR = 3.75 grams
Periodic Table
28. Fill in the following chart.
Group Name
Number
Valence
Electrons
Number of
Electrons
Lost/Gained
Oxidation
Number
1
2
1
2
+1
+2
3
4
5
3
4
3
+3
+/- 4
-3
6A
6
2
-2
7A
7
8*
1
0
-1
0
Group
Number
Alkali Metals
Alkaline Earth
Metals
Boron Group
Carbon Group
Nitrogen Group
(Pnictogens)
Chalcogens
Group
Halogens
Noble Gases
1A
2A
3A
4A
5A
8A
* Helium has 2 valence electrons and is happy
29. All elements except Hydrogen and Helium want to achieve
valence shell.
This is known as the
Octet rule.
8 electrons in the outermost or
30. Name any element with properties similar to calcium.
Magnesium
31. Alkali metals are most likely to react with what group to produce a compound with a 2:1 ratio? Explain.
They would most likely react with any member of the oxygen
group because the oxygen group requires two electrons to
make a complete octet.
33. Mendeleev arranged the periodic table by
arranged by
Atomic Mass whereas the modern periodic table is
Atomic Number.
34. Rows on the periodic table are called
Periods
35. Which group of metals is the most reactive group?
and columns are called
Groups or Families.
Alkali Metals
Why?
They have only
one valence electron to lose
36. Which group of nonmetals is the most reactive group?
Halogens
Why?
They have seven
valence electrons and only require one more for a complete
octet.
37. Which group of elements is the least reactive?
complete octets
Noble gases
Why?
They have
38. Fill in the chart below by placing a check mark by the properties that match each type of element.
Physical/Chemical
Property
Lustrous
Metal
Nonmetal
x
X
Brittle
Malleable
Conductive
X
X
X
Dull
Reacts with Acid and CuCl2
X
X
Gaseous
Solid
x
39. Which of the following elements is not in the same family?
a. calcium
b. strontium
40. List all the metalloids.
c. beryllium
d. potassium
Boron, Silicon, Germanium, Arsenic, Antimony,
Tellurium, Polonium, Astatine
41. What is:
a. atomic radius:
The size of an atom
b. electronegativity:
The ability of an atom to attract an electron
when it makes a chemical bond
c. ionization energy:
The amount of energy required to remove an
electron from an atom's outermost shell.
What does:
a. atomic radius do across a period?
It gets smaller
down a group?
It gets bigger
b. electronegativity do across a period?
It gets larger
c. ionization energy do across a period?
It gets larger down a group? It gets smaller
down a group?
It gets smaller
Cations form when neutral atoms lose
42. How do cations form from neutral atoms?
electrons
43. How do anions form from neutral atoms?
Anions form when neutral atoms gain
electrons
Bonding
44. Explain the difference between Mg and Mg+2. Mg
is a neutral atom while Mg+2 is a
cation that results from Mg losing 2 electrons.
45. Explain the difference between Cl and Cl-1.
Cl is a neutral atom while Cl-1 is an
anion that results from Cl gaining an electron
46. Name the following compounds.
a. CaOH
Calcium Hydroxide
b. C3H8
Propane
d. SO3
c. CuSO4
Copper(II) Sulfate
Sulfur Trioxide
47. Complete an atom inventory for 5 (NH4)3PO4. Also indicate the number of formula units for each.
15 N, 60H, 5P, 20O
There are 5 Formula Units of Ammonium Phosphate
48. When Pb+4 and SO4-2 combine, what is the formula of the compound formed?
covalent?
Pb(SO4)2
Is it ionic or
Ionic How do you know? The compound is made from a metal and a
polyatomic anion.
49. Which of the following IS a polyatomic ion?
a. Cl
b. O-2
d. PO4-2
c. Ca+2
The # of electrons an atom loses or gains
when it forms an ion is the oxidation number for an element!
51. What is the oxidation number for the cation in FeCl ? +3
50. What is an oxidation number?
3
52. Circle the set of formulas and names that IS CORRECT. There can be more than one answer!
a. Al2O3 (dialuminum trioxide)
c. FeSO4 (Iron (II) sulfate)
b. CS2 (carbon disulfide)
d. PbO2 (lead (IV) oxide)
53. Label the above compounds (in number 60) as ionic or covalent.
a. Ionic
c. Ionic
b. Covalent
d. Ionic
Organic Chemistry
54. What element does an organic compound contain?
Carbon
55. List the prefixes for alkanes containing from 1 to 10 carbon atoms in order.
Meth, Eth, Prop,
But, Pent, Hex, Hept, Oct, Non, Dec
56. (a) What is a hydrocarbon?
A hydrocarbon is an organic compound made
of only hydrogen and carbon.
(b) List three compounds in the body that contain hydrocarbons.
and
Proteins
Fats and Carbohydrates
57. Name the organic compounds below.
Ethene
a. C2H4
c. C8H14
Methane
b. CH4
d. C10H22
Octyne
Decane
Chemical Equations
58. Balance the following equations AND identify the type of reaction as single replacement, double replacement,
synthesis, decomposition, or combustion in the blank space to the far right.
a.
1
b.
2 Al
c.
2 KIO
d.
2C
e.
2H
Li2SO4
+
12H26
+
1 Pb(NO )

3 2
3 CuSO
2

3
2
+
4

1
KI
+
3O
37 O
+
2
1O
2

2 LiNO
3
Al2(SO4)3
+
+
1 PbSO
3 Cu
4
Double Replacement
Single Replacement
Decomposition
2

24 CO + 26 H O
2
2
2H O
2
Combustion
Synthesis
60. Write a balanced equation from the sentence below and identify the type of reaction in the blank.
a. Hydrogen gas reacts with oxygen gas to produce dihydrogen monoxide.
See 67 e
61. Explain the Law of Conservation of Matter.
Matter can be neither created nor
destroyed only rearranged.
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