SAINT VIATOR HIGH SCHOOL
CHEMISTRY 722
MRS. COYLE
STUDY GUIDE FOR SEMESTER 1 EXAM 2013-2014
Material to know
Safety in the Lab Rules
Review those safety rules.
Chapter 2
1.
2.
3.
4.
5.
6.
What is matter?
What are the three states of matter ?
Describe each one of the states of matter
Know what is a pure substance
What are physical and chemical properties?
Make sure that you know what are the characteristics (signs) that it is either physical or a
chemical property
7. What is a mixture?
8. What is a heterogeneous and homogeneous mixtures
Chapter 3
1.Scientific Notation
2. Significant figures: rules and the operations with significant figures
3. Quantitative measurement
4. Accuracy
5. Precision
6. Dimensional analysis
7. Temperature scales: Celcius to Kelvin and Kelvin to Celcius
Chapter 4
1. What is the smallest part of an element that still has all the properties of that element?
2. Role of Democritus with the atom
3. Dalton’s atomic theory- know the four postulates
4. Particles of an atom and its charge
5. Know how to calculate protons, electrons, and neutrons
6. Atomic number
7. Mass number
8. Isotopes
Chapter 5
1.
2.
3.
4.
5.
6.
Metals, non-metals, and metalloids
Location of metals, non-metals and metalloids in the periodic table
Name of vertical columns and horizontal rows
Know what are the majority of the elements classified as: metals, non- metals or metalloids
How is the modern periodic table arranged
Know which subatomic particle is the most important in determining how elements will react
with each other?
Chapter 7 and 9
1. Why type of ions do metals become?
2. Know the endings of monoatomic and polyatomic ions
3. What is the electrical charge of a cation and an anion?
4. How do ions form?
5. Name compounds are made of anions and cations
6. Which compounds are made of a non- metal combining with a non metal?
II. Practice Problems
Express each of the following numbers in scientific notation.
a. 230
b. 5601
c. 14 100 000
d. 56 million
e. 2/10
f. 0.450 13
g. 0.089
h. 0.000 26
i. 0.000 000 698
1. Perform the following operations and express the answers in scientific notation.
a. (1.2 x 105) + (5.35 x 106)
(1.2 x 105) + (5.35X 106)
b. (6.91 x 102) + (2.4 x 103)
c. (9.70 x 106) x (8.3 x 105)
(9.70 x 106) x(8.3 x 105)
d. (3.67 x 102) ÷ (1.6 101)
Signficant Figures
How many significant figures do the following numbers have?
1)
1234 _____
2)
0.023 _____
3)
890 _____
4)
91010 _____
5)
9010.0 _____
6)
1090.0010 _____
7)
0.00120 _____
8)
3.4 x 104 _____
9)
9.0 x 10-3 _____
10)
9.010 x 10-2 _____
11)
0.00030 _____
12)
1020010 _____
13)
780. _____
14)
1000 _____
15)
918.010 _____
16)
0.0001 _____
17)
0.00390 _____
18)
8120 _____
19)
7.991 x 10-10_____
20)
72 _____
Solve the following mathematical problems such that the answers have the correct number of significant
figures:
1)
334.54 grams + 198 grams = ___________________
2)
34.1 grams + 1.1 grams = ___________________
3)
2.11 meters ÷34 meters = ___________________
4)
0.0010 meters – 0.11 m = ___________________
5)
349 cm + 1.10 cm + 100 cm = ___________________
6)
450 meters ÷ 114 meters= ___________________
7)
298.01 kilograms + 34.112 kilograms = ___________________
8)
84 s x 31.221 s = ___________________
1. List the three states of matter and describe their basic properties:
2)
Classify the following as either elements, compounds, homogeneous mixtures (solutions) or
heterogeneous mixtures:
a)
copper (II) sulfate
b)
Kool Aid
c)
wood
d)
plastic
e)
lined paper
3)
Why are homogeneous mixtures more difficult to separate than heterogeneous mixtures?
4)
Why can’t elements be separated into smaller parts using chemical means?
Protons, Neutrons, and Electrons Practice Worksheet
Fill in the blanks in the following worksheet. Please keep in mind that the isotope
represented by each space may NOT be the most common isotope or the one closest in
atomic mass to the value on the periodic table.
Atomic
symbol
Atomic
number
Protons
B
Neutrons Electrons
6
11
24
31
37
39
29
89
35
43
100
207
Pb
102
70
89
Mo
225
53
81
100
206
159
No
Yb
261
172
106
159
Which group of the periodic table is most likely described by questions 1-5?
1)
Atomic
mass
These elements have a charge of +2 when forming ionic compounds.
2)
These elements are almost entirely unreactive. _____________________
3)
These elements are found in group 1 of the periodic table. ____________
For problems 12-15, determine the number of valence electrons each element has:
4)
sulfur _________
6)
helium _________
5)
carbon _________
7)
hydrogen _________
Electron Configuration
In the space below, write the unabbreviated electron configurations of the following
elements:
1)
sodium________________________________________________
2)
iron
________________________________________________
3)
bromine
________________________________________________
4)
barium
________________________________________________
5)
neptunium
________________________________________________
In the space below, write the abbreviated electron configurations of the following elements:
6)
cobalt
________________________________________________
7)
silver
________________________________________________
8)
tellurium
________________________________________________
9)
radium ________________________________________________
10)
lawrencium
________________________________________________
Determine what elements are denoted by the following electron configurations:
11)
1s22s22p63s23p4 ____________________
12)
1s22s22p63s23p64s23d104p65s1 ____________________
13)
[Kr] 5s24d105p3 ____________________
14)
[Xe] 6s24f145d6 ____________________
15)
[Rn] 7s25f11 ____________________
Determine which of the following electron configurations are not valid:
16)
1s22s22p63s23p64s24d104p5 ____________________
17)
1s22s22p63s33d5 ____________________
18)
[Ra] 7s25f8 ____________________
19)
[Kr] 5s24d105p5 ____________________
20)
[Kr] ____________________
Name the following ionic compounds:
1)
NH4Cl _____________________________________
2)
Fe(NO3)3 _____________________________________
3)
TiBr3 _____________________________________
4)
Cu3P _____________________________________
5)
SnSe2 _____________________________________
6)
GaAs _____________________________________
7)
Pb(SO4)2 _____________________________________
8)
Be(HCO3)2 _____________________________________
9)
Mn2(SO3)3 _____________________________________
Write the formulas for the following compounds:
11)
chromium (VI) phosphate _____________________________________
12)
vanadium (IV) carbonate _____________________________________
13)
tin (II) nitrite _____________________________________
14)
cobalt (III) oxide _____________________________________
15)
titanium (II) acetate _____________________________________
16)
vanadium (V) sulfide _____________________________________
17)
chromium (III) hydroxide _____________________________________
18)
lithium iodide_____________________________________
19)
lead (II) nitride
Write the names of the following chemical compounds:
1)
BBr3 ______________________________________
2)
CaSO4 ______________________________________
3)
C2Br6 ______________________________________
4)
Cr(CO3)3 ______________________________________
5)
Ag3P ______________________________________
6)
IO2 ______________________________________
7)
VO2 ______________________________________
8)
PbS ______________________________________
9)
CH4 ______________________________________
10)
N2O3 ______________________________________
Write the formulas of the following chemical compounds:
11)
tetraphosphorus triselenide ____________________________________
12)
potassium acetate ______________________________________
13)
iron (II) phosphide ______________________________________
14)
disilicon hexabromide ______________________________________
15)
titanium (IV) nitrate ______________________________________
16)
diselenium diiodide ______________________________________
17)
copper (I) phosphate ______________________________________
18)
gallium oxide ______________________________________
19)
tetrasulfur dinitride ______________________________________
20)
phosphorus ______________________________________
Name the following acids and bases:
1)
NaOH _______________________________________
2)
H2SO3 _______________________________________
3)
H2S _______________________________________
4)
H3PO4 _______________________________________
5)
NH3 _______________________________________
6)
HCN _______________________________________
7)
Ca(OH)2 _______________________________________
8)
Fe(OH)3 _______________________________________
9)
H3P_______________________________________
Write the formulas of the following acids and bases:
10)
hydrofluoric acid _______________________________________
11)
hydroselenic acid _______________________________________
12)
carbonic acid _______________________________________
13)
lithium hydroxide _______________________________________
14)
nitrous acid _______________________________________
15)
cobalt (II) hydroxide _______________________________________
16)
sulfuric acid _______________________________________
17)
beryllium hydroxide _______________________________________
18)
hydrobromic acid _______________________________________