Name _____________________________________
Date_________________ Block # ___________
Chemistry Unit Test Study Guide - KEY
***To prepare for the test, you must study your notes and past quizzes as well. ***
Directions: Use your Chemistry Part 1, 2 & 3 Notes to complete this review.
Part 1:
1.
Matching:
Rutherford
Bohr
Dalton
Thomson
Modern (Quantum) Theory
______Dalton_________ believed the atom was a solid sphere with no charges
______Thomson________ theorized that the atom looked like Plum Pudding (positive sphere with
negatives sprinkled throughout)
______Rutherford_________ believed that the atom had a positive nucleus with electrons surrounding
it. The Gold Foil Experiment was the basis for his theory.
______Bohr_________ believed the atom had a nucleus containing protons and neutrons, and that the
electrons were in fixed energy shells around the nucleus.
____Modern (Quantum) Theory___________ the current theory of the atom – the atom has a nucleus
containing protons and neutrons, and the electrons are in a cloud around the nucleus.
2.
Draw a Bohr model of oxygen.
Oxygen has 8 protons & 8 neutrons in its nucleus. The atomic
number tells you how many protons oxygen has. You can figure
out the number of neutrons by subtracting the atomic number
from the atomic mass (16-8 = 8). A neutral atom of oxygen
would have 8 electrons. 8 positive protons and 8 negative
electrons would cancel each other out, leaving the atom with an
overall neutral charge.
3.
Fill in the chart.
Subatomic Particle
Proton
Neutron
Electron
Charge
Positive +1
Neutral 0
Negative -1
4. _______Atoms______ are the basic building blocks of all matter.
5. A(n) ______element____ is a substance that is made entirely from one type of atom.
6. _______Quarks___________ are the subatomic particles that make up protons and neutrons.
7. The atomic _____number_______ is the number of protons.
8. The atomic ______mass_____ is the number of protons + neutrons.
9.
Fill in the table below.
Lithium
Atomic number
3
Atomic mass
7
Number of protons
3 (atomic number
tells you how many
protons)
4 (atomic mass –
atomic number)
Li
Number of neutrons
Chemical symbol
State of matter at room
temperature
Natural or Man-made
solid
natural
10. An element's identity is directly related to the number of ___protons_____ in its nucleus. This is
the basis for the arrangement of the elements on the periodic table.
11. What is an isotope? What is the difference between Carbon 12 and Carbon 14? Isotopes are
atoms that have the same number of protons, but different numbers of neutrons.
Part 2:
Hydrogen is also
a nonmetal.
12. Label the diagram.
13. List 4 properties of metal.




Shiny (Luster)
Ductile – can be drawn out into thin wires
Malleable – can be pound into thin sheets
Good conductors of heat and electricity
14. List 3 properties of nonmetals.
 Dull (not shiny or not a lot of luster)
 Poor conductors of heat and electricity
 Brittle
15. Describe the properties of metalloids.
 Metalloids share properties of both metal and nonmetals. For example: they may be shiny,
but poor conductors.
16. The rows on the periodic table are called _____periods_______.
17. The columns on the periodic table are called _____families______ or ____groups_____.
18. Which element is in the same family as Silicon?
a. Carbon
b. Phosphorus
c. Helium
19. Which element is in the same period as Potassium?
a. Titanium
b. Lithium
c. Boron
20. What are valence electrons? Why are they important? They are the electrons in the outermost
energy level (shell) of an atom. They are important because they are the electrons that
participate in chemical bonding.
21. How many valence electrons does one atom of Xenon have? 8 electrons. If you label the tall
columns on the periodic table, Xenon is in column 8, so it has 8 valence electrons.
Xenon has 8
electrons in the
energy level
furthest from
the nucleus.
22. How many valence electrons does Aluminum have?
3 valence electrons.
Part 3:
23. When 2 or more different elements chemically combine together they form a
__compound_____.
24. When elements chemically combine they form compounds that have totally __different___
properties from themselves.
25. How many atoms total are in the following compound:
2C6H12O6
Carbon = 12, Hydrogen = 24, Oxygen = 12, Total atoms = 48
26. How many atoms of hydrogen are in the compound
Hydrogen = 18 (3 times 6)
3C2H6?
27. How many atoms of oxygen are in the compound Au(OH)3
Oxygen = 3 (3 times 1)
28. Atoms bond to other atoms to become more chemically stable by having their outer energy
shell __full______. If the atom has only one energy shell, then it is stable with 2 valence
electrons. If an atom has more than one energy shell, then it is stable with 8 valence electrons.
29. What is an ion? An ion is a charged particle that forms during a chemical change when one or
more valence electrons transfer from on atom to another (ionic bonding).
30. In ___covalent____ bonding that atoms will share electrons in order to have a full outer shell.
31. In ___ionic_____ bonding a metal gives valence electrons to a nonmetal in order to have a full
outer shell. Two ions are formed (one positive & one negative) and their opposite charges
attract to form a compound.
32. What type of bond will each pair of atoms create? (ionic or covalent)
Hydrogen and chlorine ___Covalent bond_______ (covalent bonds form between
nonmetals)
Potassium and Iodine ___Ionic bond___ (Ionic bonds form between metals and
nonmetals. Potassium is a metal & Iodine is a nonmetal.)
Calcium and chlorine ___Ionic bond____ (Calcium is a metal & Chlorine is a nonmetal)
33. Which element is more chemically reactive, Sodium or Xenon? Sodium is more reactive.
Sodium will give up a valence electron to have a full outer shell. Xenon already has a full outer
shell of 8 valence electrons, so it does not need to bond with other atoms to be stable.
34. Ionic bonds form between ___metals____ and ____nonmetals_________.
35. Covalent bonds form between ___nonmetals___ and ____nonmetals_______.