Quarter 1 Exam Review
Chapter 1 – Matter, Energy, and Change
 What is chemistry?
 What are the 5 branches of chemistry? What is studied in each branch?
 What is the difference between mass and weight? What are the units on each?
 What is matter?
 List and describe the various states of matter.
 What are basic research, applied research, and technological development?
 What is meant by the following terms & how are they related:
Atom and element
Molecule and compound
 What is meant by properties? What is the difference between extensive properties and
intensive properties? What are some examples of each? Be able to classify properties as being
either extensive or intensive.
 How are physical properties different from chemical properties? Give examples of each and be
able to classify properties as being either physical properties or chemical properties.
 How is a physical change different from a chemical change? Give examples of each and be
able to classify changes as either physical changes or chemical changes. What does the law of
conservation of mass have to do with these changes?
 How are chemical changes indicated?
 In a chemical equation, where are the products? The reactants? What does the arrow mean?
 How is energy involved in physical and chemical changes? What is the difference b/w
endothermic reactions & exothermic reactions? In which type does the reaction mixture get
cold? Hot?
 What are the 2 main categories of matter? What are the 2 types of mixtures? What are the 2
types of pure substances? Give examples of each and be able to classify examples of matter
into their correct category. (See the chart on p. 11 of the textbook.)
 On the Periodic Table, what are groups? Periods? What is another name for a group?
Elements in the same ___________________ have similar chemical properties.
 Define metals, nonmetals, and metalloids. Give examples of each. Where is each type of
element located on the Periodic Table?
 What makes the noble gases so “noble”?
Chapter 2 – Measurements and Calculations
 What are the steps of the scientific method?
 Be able to carry out metric conversions.
You need to know the following prefixes: milli-, centi-, kilo-, deci-.
 What is meant by base (fundamental) quantities? (See the chart on p. 32.)
 What do we call combinations of base quantities? Be able to classify various quantities as
being either base or derived quantities. Compare the chart on p. 32 w/ the chart on p. 34.
 If you had several substances with different densities and put them all into a graduated cylinder,
how would they be layered – from most dense at the top to least dense at the bottom OR least
dense at the top to most dense at the bottom?
 Be able to find the density, mass or volume of an object when given 2 of the 3 quantities.
 Be able to convert between the 3 temperature scales.
 Using Q = mcT, be able to find any one of the quantities when given the other quantities.
 If one object gains energy, what must another object do? What law is this based on? When
does this law NOT hold true?
 What is the difference between accuracy and precision? Be able to describe a set of
measurements in terms of accuracy and precision.
 Be able to calculate percent error.
 Be able to determine the # of significant digits in a measurement. How many significant digits
in each of the following measurements:
 Be able to perform calculations involving significant digits and scientific notation.
Chapter 3 – Atoms: The Building Blocks of Matter
 Describe the 3 particles of an atom in terms of their location, their charge, their symbol, and
their relative atomic mass. Which particles make up the bulk of an atom’s mass?
 What are isotopes? What are the two ways to illustrate an isotope?
 Be able to find the average atomic mass of the isotopes of an element.
 What does Dalton’s atomic theory say?
 Be able to fill in a chart on the number of electrons, protons, neutrons, atomic number, and
mass number for various elements without using a Periodic Table.
 Be able to convert moles to mass to atoms and vice versa.
 What atom is set as the standard to which the mass of all other atoms is based upon?
Chapter 4 – Arrangement of Electrons in Atoms
 In section 1, know the terms associated with light waves.
 What is the relationship between wavelength, frequency, and energy of an electromagnetic
wave?
 From our flame test lab, which color of flame has the most energy? The least energy?
 What is meant by the photoelectric effect?
 Why does hydrogen have 4 wavelengths in its visible spectrum?
 What is the difference between the ground state of an atom and the excited state? How does an
electron move from the ground state to the excited state? What happens when an electron
drops down from the excited state back to the ground state?
 What is the name of the current theory that describes the wave properties of electrons and other
very small particles?
 What is meant by an orbital?
 Know the 4 quantum numbers and what each represents. What is the relationship between the
PQN and the number of sublevels per main energy level? Between the PQN and total number
of orbitals per main energy level? Between the PQN and the number of electrons per main
energy level? See the chart on p. 104. See problem 18 on p. 119.
 How many orbitals are there for each of the following sublevels: s, p, d, f?
 How is the period related to the highest occupied energy level?
 What does each of the following principles/rules say?
1. Aufbau Principle
2. Pauli Exclusion Principle
3. Hund’s rule
 Be able to apply the above principles/rules to write complete electron configuration, noble gas
configurations, and orbital notations for an element.
Ex. Give the above information for phosphorus.
 Be able to write the electron-dot symbol for a given element. What electrons are indicated on
such a symbol? How can you determine this from just using the Periodic Table?
Ex. Write the electron dot symbol for each of the following: Cs, Ca, N, S, Br
 Given an electron configuration, be able to identify the element.
 What are meant by inner-shell electrons? Outer shell electrons?
 See the following problems as samples- pages 119-121: 22, 30, 31, 33, 36, 37, 38, 40
 How do you know that there must be a strong force holding the nucleus together?
 Be able to identify the shapes of the s and p orbitals.
NOTE: This is intended as an overview of what we covered this quarter. ANYTHING covered in
class AND anything in Chapters 1 – 4 could be on the Quarter 1 Exam.
Chemistry Q1 Practice Problems
1. The density of lead is 11.3 g/cm3. What would be the volume of 410 g of lead? Write your answer
with the correct number of significant digits.
2. A 45.0 g sample of iron absorbs 501 J of energy as it is heated from 20.0 oC to 45.0 oC.
A. Find the specific heat of the iron to the correct number of significant digits.
B. If the accepted value is 0.449 J/g. oC, find the percent error to the nearest tenth of a percent.
3. Name the 3 particles in an atom and give their charge, their location, and their symbol.
4. Convert each of the following to moles.
A. 6.2 g Fe
C. 325.0 g Ca
B. 5.67 x 1025 atoms Li
D. 1.34 x 1024 atoms S
5. Convert each of the following to grams.
A. 0.55 mol K
C. 1.35 mol P
C. 4.56 x 1026 atoms Mg
D. 3.54 x 1024 atoms Si
6. Convert each of the following to atoms:
A. 34.5 g Na
C. 2.356 g B
B. 4.36 mol Al
D. 0.74 mol Cu
7. Calculate the average atomic mass of uranium to 3 places past the decimal places given the information in
the chart below:
Relative Atomic Mass (amu)
% Abundance
234.040947
0.005
235.043924
0.720
238.050784
99.275
8. Write the electron configuration for tellurium (atomic # = 52)
9.
10.
Write the noble gas notation for arsenic (atomic # = 33)
Draw the electron dot symbol for each of the following:
A. Calcium
B. Sulfur
C. Aluminum
D. Sodium
FOR EACH PROBLEM BELOW, YOU WILL ONLY BE ABLE TO USE A 4-FUNCTION
CALCULATOR AND NO PERIODIC TABLE.
1. Complete the following table. Show your work in the space provided.
o
F
o
C
K
92
-27
420
2. Write the following numbers in proper scientific notation:
A. 530.9 x 1018 g
E. 0.000506 L
B. 2563.34 x 10-23 Gm
F. 12023.0 kg
C. 0.000076 x 106 mL
D. 0.0003120 x 10-12 Tm
3. Perform the following calculations. Round off your answer to reflect the correct number of significant
digits. Include units on your answer. (4 Points Each)
A. 5.07 g + 2.8613 g
C.
58.2 g
3 mL
B. 1.46 kg - 25 g
D. 19.20 cm x 1.6 cm
4. Perform the following calculations. Write your answer in scientific notation AND with the correct number
of significant digits.
A. (4.15 x 104 g) + (9.6 x 105 g)
B. (12.6 x 105 cm) x (2.125 x 107 cm)
C. (2.35 x 1012 cg) - (1.13 x 1012 mg)
D. (2.56 x 10-7 kg)
(3 x 108 m3)
5. Fill in the missing parts of the chart below:
ELEMENT SYMBOL
ATOMIC
NUMBER
*Strontium
MASS
NUMBER
PROTONS NEUTRONS ELECTRONS
88
17
38
35
potassium
ion
20
S-2
*
32
*
15
31
18
Iron II ion
6.
18
30
24
Give the hyphen notation and nuclear symbol notation for the elements is the chart above that have an
asterisk (*) by them.
7. Convert each of the following measurements to the indicated units:
A. 12.3 cg/mL
to g/L
B. 256 cg to kg
C. 25 cm3 to dm3
8. How many significant digits are in each of the following numbers?
A. 15.0 g
B. 0.0008070
C. 1250
D. 2.4500 x 106 L