Download Honors Chemistry Semester 1 Exam Review

Name: __________________________
Unit 1: Nature of Science
1. Using the picture above, list lab safety rules that are
being ignored.
2. What are the steps to the scientific method?
3. Convert the following into scientific notation:
a) 1500 = ____________
c) 0.001012 = ____________
b) 123 = ____________
d) 1.52 = ____________
4. Convert the following into decimal notation (ordinary notation):
a) 4.59 x 103 = ____________ c) 280 x 10-4 = ____________
b) 5 x 102 = ____________
d) 1.4 x 10-5 = ____________
5. Indicate the number of significant figures:
a) 34 g ___
b) 564 L ___
d) 23.45 mg ___
e) 101 km ___
c) 19.3 mm ___
f) 3400 g ___
6. Round the following numbers to 2 significant figures:
a) 0.826mg ___
b) 19.88mL ___
c) 19250cm ___
d)950L ___
7. What is the SI unit for the following measurements:
a) length _____
b) mass _____
c) time _____
d) volume _____
8) What measurement in millimeters is indicated on the ruler below? _____
9. ) Convert the following:
a) 850cm to _________ mm
b) 2500 mg to __________ kg
c) 0.2598kL to _________ L
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Chemistry Semester 1 Review
10) Suppose a lab refrigerator should hold a constant temperature of 38.0 F. A temperature sensor is tested 10 times in the
refrigerator. The temperatures from the test yield the temperatures of: 37.8, 38.3, 38.1, 38.0, 37.6, 38.2, 38.0, 38.0, 37.4,
38.3. Is the distribution of values from the test: accurate (yes or no), precise (yes or no).
11) Explain the Big Bang Theory. ______________________________________________________________________
__________________________________________________________________________________________________
________________________________________________________________________________________________
Unit 2: Atomic Structure
1. What is an atom?
_________________________________________________________________________________________
2. What is the overall charge of an atom? Why? _________________________________________________________
______________________________________________________________________________________________
3. Isotopes are atoms of the same element, which have the same number of (protons / neutrons) but a different number
(protons / neutrons).
4. How do isotopes C-12 and C-14 differ from each other? ________________________________________________
How are they similar? ___________________________________________________________________________
5. What parts of Dalton’s atomic theory are now known to be incorrect? ______________________________________
______________________________________________________________________________________________
______________________________________________________________________________________________
6. Progression of the atomic model:
Dalton
Thompson
Rutherford
Description of
supporting
evidence &
experiments
Major
findings
Drawing and
description of
atomic model
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7. Identify the three basic particles in the atom. Give their location, charge, and mass. (Fill in the table)
Particle
Location
Charge
Mass (amu)
8. Fill in the blanks for the elements using the periodic table
Element
Symbol
Atomic #
#Protons
Carbon-14
# Electrons
#Neutrons
Mass #
29
16
131
53 I
47
Unit 3: Electron
1. Electrons can act as a __________ or ___________ according to the _____ -__________ duality model.
2. What is a quantum of energy? __________________________________________________________________
3. When an electron absorbs energy, it jumps to the ___________ state.
4. How does an electron produce light in things such as fireworks or neon signs? ______________________________
________________________________________________________________________________________
Use the diagram to answer questions 5-7:
5. Which region is referred to as the s-block on the diagram? ____
How many electrons can each level of the s-cloud hold? ____
6. Which region is referred to as the p-block on the diagram? ____
How many electrons can each level of the p-cloud hold? ____
7. Which region is referred to as the d-block on the diagram? ___ How many electrons can each level of the d-cloud
hold? ___
8. What energy level are the outer electrons for Potassium found? ______ This is indicated by Potassium’s
______________.
9. Indentify the number of valance electrons for the following elements and draw the corresponding electron-dot
structure:
a) Calcium
b) Carbon
c) Neon
10. Draw the shape of the s-sublevel:
Draw the shape of the p-sublevel:
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11. Write the electron configuration for:

Lithium:

Argon:


Iron:
Barium:
12. Identify the element with the electron configuration of 1s22s22p63s23p3 ____________________
13. According to the quantum mechanical model, the location of an electron is based on ______________.
14. What does the electromagnetic spectrum show? ______________________________________________________
____________________________________________________________________________________________
15. On the electromagnetic spectrum, as the wavelength increases, frequency ___________, and energy ____________.
16. A barium atom (gains / loses) ______ electrons when it forms a barium ion. What is the symbol for a barium ion?
______
A fluorine atom (gains / loses) ______ electrons when it forms a fluorine ion. What is the symbol for a fluorine
ion? ______
Unit 4: Periodic Table
Use the diagram to answer questions 1-3 :
1. Which region contains group 18? ___ What is the name of this group? ____________
2. Which region contains the alkaline earth metals? _____
3. Which region contains elements with an electron configuration that ends with p5? _____
4. The 10 short columns in the middle of the periodic table make up the ___________________ _________________.
5. The order of the elements on the periodic table is based upon the ____________ ______________. What particle of
the atom is represented by this number? __________________
The diagram below lists the information found on the periodic table. Use this diagram to answer question 6.
79
Au
Gold
107.86
6. The element’s _____________ _____________ is 79, the _______________ is Au, and the Atomic mass is
______________.
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7. How many groups are on the periodic table? ____________
8. How many periods are on the periodic table? ____________
Use the diagrams below to answer questions 9-10.
9. Which diagram correctly depicts the trend in electronegativity? ________
10. Which diagram correctly depicts the trend in atomic radius? ________
11. Elements in the same group have similar ______________. They behave similarly because they have the same
number of ________________.
12. Metals are located on the ____________ side of the periodic table and nonmetals are on the ____________ side.
Unit 5: Bonding
1. How does a intermolecular forces differ from a intramolecular force? ____________________________________
____________________________________________________________________________________________
2. Which electrons are involved in bonding? _________________________________
3. What types of elements are involved in ionic bonding? ________________________
Covalent?___________________
4. What type of bond is formed by the transferring of electrons? ______________ Sharing electrons? ___________
5. How does an element form a cation?___________________________ Anion? __________________________
6. Why does Magnesium form a +2 charge? __________________________________________________________
7. How many valance electrons does each of the following elements have?
a. Sodium ________
b. Oxygen __________
c. Krypton __________
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8. List the general characteristics of ionic and covalent bonds (i.e. physical properties (hardness, state of matter,
boiling point, melting point, conductivity), strength)
Ionic
Covalent
Unit 6: Chemical Nomenclature
Practice:
1. Identify all seven diatomic elements: ___________________________________________________
2. For the following ionic names, write the missing chemical formula or chemical name.
a. nickel (II) oxide
_____________
b. calcium carbonate _____________
c. potassium nitrate
_____________
d. ammonium bromide _____________
e. gold (III) iodide
_____________
f. zinc phosphide
g. lithium sulfate
_____________
h. Na2SO4
____________________
i. Al2O3
______________
j. SnO
___________________________
_____________
k. K2S
_____________________
l. (NH4)3PO4
___________________________
m. ZnCl2
______________________
n. PbCO3
___________________________
3. For the following molecular (covalent) compounds write the missing formula or name.
a. carbon monoxide
____________
b. xenon tetrafluroide ____________
c. silicon dioxide
____________
d. iodine pentachloride ____________
e. P2O5
g. SF7
Unit 7: The Mole
1.
2.
___________________________
f. P4O10
___________________________
___________________________
h. NI3 ___________________________
Show all work for calculations:
Give conversion factors (in fraction form) for converting between the following
A.) FROM moles TO atoms
B.) FROM grams TO moles of Boron
C.) FROM atoms TO moles
What is the molar mass of Rb2Cr2O7?
3. What is the number of molecules in 16.75 g of H2O ?
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4.
What is the mass of 1.75 x 1024 molecules of NH3 ?
5.
How many molecules are in 0.26 mol of CO2 ?
6.
Which of the following are empirical formulas?
Unit 8: Chemical Reactions
H2O
H2O2
C6H12O6
N2H5
1. Differentiate between a precipitate and an aqueous solution. ______________________________________________
____________________________________________________________________________________________
_____________________________________________________________________________________________
2. List the 5 types of chemical reactions AND state how you would identify their type simply by looking at the equation:
Type of reaction:
How you would identify the type simply by looking at the form of the equation?
S = Synthesis (Combination)
2 or more reactants and only 1 product
D=
SR =
DR =
C=
3. Why do chemical equations need to be balanced? ______________________________________________________
______________________________________________________________________________________________
4. Balance the following equations and identify the type of reaction occurring:
a. ____Zn + ____HCl ---> _____ZnCl2 + ____H2
type ___________________________
b. _____KClO3 ---> _____KCl + ____O2
type ___________________________
c. ____S8 + ____F2 ---> _____SF6
type ___________________________
d. _____Fe + ____O2 ---> ____Fe2O3
type ___________________________
e. ____C2H6 + ____O2 ---> ____CO2 + ____H2O
type ___________________________
f. _____MgO  _____Mg + _____O2
type ___________________________
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Chemistry Semester 1 Review (Honors)