Name: __________________________
Chemistry: Exam Review Worksheet, Part 1
Chapter 3
1. Label the following as either a chemical (C) or physical (P) change.
a. ________ water is heated and is changed to steam.
b. ________ milk sours
c. ________ sugar dissolves in water
d. ________ tire going flat
e. ________ sodium pellet gets sliced in two
f. ________ evaporation
g. ________ wood rotting
h. ________ chewing gum
i. ________ a plant growing
j. ________ hydrochloric acid reacts with potassium hydroxide forming H2O, a
salt, and heat.
2. Label the following as either a chemical (C), intensive physical (IP) or extensive
physical (EP) property.
a. ________ color
b. ________ density
c. ________ weight
d. ________ failure to react with another substance
e. ________ oxidation
f. ________ volume
g. ________ combustibility
h. ________ melting point
i. ________ hardness
j. ________ tendency to corrode
3. If you have 55 grams of reactants, how many of grams of product should you have
according to the law of conservation of mass?
4. Fill in the blanks.
Matter can be classified into two main groups: _________________ (which can be
represented by symbols and formulas) and _______________________(which cannot be
represented by symbols or formulas). Either an ______________ or a ________________
can be referred to as a substance. A physical combination of different substances that retain
their individual properties is called a _________________. These can be broken down into
two main types: ____________________ (not mixed evenly throughout) and
_____________________( mixed evenly throughout). Another name for a mixture that is
evenly mixed is a _____________. Two types of mixtures that are not evenly mixed are a
___________________ and a _____________________.
A characteristic by which a variety of matter can be recognized is called a
____________________. A ______________ ______________ is a characteristic that
depends on how a kind of matter changes during interactions with other matter. A
_______________ _______________ can be observed without changing the make-up of the
matter. If the property depends on how much of a substance we have it is referred to as an
_____________ _______________ property. If it does not matter how much of a substance
we have it is referred to as an _________________ _______________ property.
Chapter 4
1. Describe the basic structure of an atom. Include the 2 main areas, and subatomic
particles. Include details about each subatomic particle (location, charge, general size).
2. What was Rutherford’s gold foil experiment designed to study and how did it result in the
discovery of the nucleus?
3. Opposites attract and likes repel. If a nucleus is made up of only positive protons and
neutral neutrons, what holds an atom together?
4. What is an isotope?
5. Complete the following chart:
Isotope Name
Isotope
Symbol
Atomic
Number
Mass
Number
30
64
#of
Protons
# of
Electrons
# of
Neutrons
O
18
8
Mercury- 204
16
19
18
21
Name: __________________________
Chemistry: Exam Review Worksheet, Part 2
Chapter 5:
1. Describe how electrons are arranged outside of the nucleus. Use the following terms:
electron cloud, principal energy level, sublevel, and orbital.
2. Please list the filling order for through 5s.
3. Write the full electron configurations for the following elements:
a. Lithium
___________________________________________________
b. Bromine
___________________________________________________
c. Silicon
___________________________________________________
4. Write noble gas configurations for the following elements:
a. Potassium
___________________________________________________
b. Nitrogen
___________________________________________________
c. Phosphorous ___________________________________________________
5. Please describe what an atomic emission spectrum is and what causes it.
Chapter 6-7
Fill in the blank:
1. Atoms, ions and isotopes are differentiated by their numbers of _________________,
______________________, and _________________.
2. On the periodic table, elements are arranged by increasing numbers of ______________
3. Vertical groups are referred to as ___________________, and elements within those
vertical groups have similar _________________ and chemical _________________,
because they all have the same number of _________________ __________________.
4. Which group contains the most active nonmetals?_______________________________
5. What is the name of that group? ___________________________________________
6. Which group are the most active metals located in? ____________________________
7. What is the name of that group? ___________________________________________
8. What is the name of the group 2A elements? _________________________________
9. What is the name of the group 8A elements? _________________________________
10. What is the name of the B elements? ________________________________________
11. What type of electron sublevels are filling across the transition elements? ___________
12. Elements in a period have electrons all filling the same __________________________
13. An element with both metallic and nonmetallic properties is called _________________
14. The majority of the elements on the periodic table are ___________________________.
15. Elements with an atomic number higher than 92 are ____________________________.
16. Which element has the highest electronegativity? ______________________________
17. Which element has the lowest electronegativity? ______________________________
18. Which element is more reactive: 37 or 38? __________________________________
19. Which element is more reactive: 18 or 7? __________________________________
20. As you move from left to right on the periodic table, atomic size (increases
decreases).
Why? ________________________________________________________________
21. As you travel down a group, the atomic size (increases
decreases).
Why? ________________________________________________________________
22. As you move from left to right on the periodic table, ionization energy (increases decreases).
Why? _______________________________________________________
23. As you travel down a group, the ionization energy (increases
decreases).
Why? ________________________________________________________________
24. Review the historical development and changes to the periodic table, and then list the
significant impact that each of the following people had on the development of the
periodic table.
a. LaVoisier
b. Newlands
c. Mendeleev
d. Moseley
25. List the common state at room temperature, an example of an element, and 3 properties
for each of the following: metal, metalloid, and nonmetal.
Name: __________________________
Chemistry: Exam Review Worksheet, Part 3
Chapter 8 and 9
1. Please complete the following chart.
Element
# Valence e-
How many elose or gain
Oxidation
Number
Symbol
Strontium
Nitrogen
Potassium
Oxygen
Chlorine
2. A negative ion is generally (larger smaller) than its parent atom. Why?
3. A positive ion is generally (larger smaller) than its parent atom. Why?
4. What is the difference between covalent, metallic, and ionic bonds? How can you tell them
apart by looking at formulas?
5. Write an “I” for ionic or “C” for covalent to the left of each name. Then, to the right, write
formulas for the following compounds:
_________Sodium chloride
____________________
_________Chromium (II) Nitrate
____________________
_________Carbon Tetrachloride
____________________
_________Magnesium Nitride
____________________
_________Nitrogen Trifluoride
____________________
_________Calcium Chloride
____________________
_________Nitrogen
____________________
_________Dihydrogen Monoxide
____________________
_________Potassium Sulfide
____________________
6. For those labeled as “Covalent” in number 5, please draw structural formulas and label them
as polar or nonpolar.
7. Name the elements necessary for hydrogen bonding: __________ __________ __________
8. Why do ionic compounds have greater melting points than covalent compounds?
9. List the following compounds from lowest to highest melting point: NaCl, CH4, H2O. Then,
explain the differences between their melting points.
10. Why is chlorine a gas at room temperature, while iodine is a solid. (Both are covalent
compounds).
11. Explain the differences in melting points, conductivity, and malleability for ionic, covalent,
and metallic compounds.
12. Name the following:
Na3PO4 ___________________________
CoCl2
___________________________
CCl4
HCl
___________________________
SF6
___________________________
___________________________
Mg(OH)2 ___________________________