2016 – 2017 Chemistry end of semester test study guide. (Ch. 3/4)
Name _______________________________________
Period ____
Test Date:
Key concepts to review.

Periodic table trends
o
Element families and characteristics (ex. Nobel Gasses don’t react)
o
Where are metals and nonmetals found on the periodic table?

Reactive characteristics of metals and nonmetals.

Chemical bonding and the rule of Octet.

Ions, what creates a charged particle or atom? (Think electrons) Gain and loss of electrons.

Practice reading periodic table including atomic mass, tendencies to gain or lose electrons,
number of sub atomic particles (protons, neutrons, electrons)

Electronegativity Trends. What type of bond will form and what are the physical characteristics
of that type of bond.

Electron configurations, Lewis and Bohr diagrams.

Rutherford experiment, and design of the atom

Bohr’s spectrum and electron orbitals

Polar, Non Polar, and Ionic molecules.
o
Mix or does not mix, will this solid dissolve in this type of liquid? Why?
o
Key characteristics of each type of bond.

Metals and Non Metals on the periodic table, reactive characteristics

Conservation of matter

Balancing Chemical Equations

Hydrogen bonding, why does water stick together and attract to a charge.
1. Identify the tendency to lose or gain ___ # of electrons and how or what they are likely to react with.
1b. Color the section of the blank periodic table to show the periodic table families location.
1c. draw a line to separate the metals from the nonmetals and label.
Group 1/Alkali Metals (red)
lose or gain _1_ # of electrons
_1_ # of valence electrons
Group 2/Alkali Earth Metals (orange)
lose or gain _2__ # of electrons
_2__ # of valence electrons
Group 17/Halogens (blue)
lose or gain _1__ # of electrons
_7__ # of valence electrons
Group 18/Nobel Gasses (purple)
lose or gain _0__ # of electrons
_2/8__ # of valence electrons
What is the “trend” as you move from left to right across the periodic table?
Valence electrons:
INCREASE as you move from Group 1 to Group/column 18
Electronegativity:
INCREASES as you move from Group 1 to Group/column 18
Non
Metals
2. Compare and contrast metals and nonmetals. (Circle the Non Metals in the periodic table above)
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2016 – 2017 Chemistry end of semester test study guide. (Ch. 3/4)
a. Metals;
LOSE electrons to non metals, Form positive (+) ions, found on the left side of the Periodic Table.
b. Non Metals;
STEAL electrons from metals or SHARE with other non metals. Form negative (-) ions and found
on the right side of the periodic table (includes hydrogen).
3. If a compound is soluble in water (a polar solvent) and conducts electricity strongly, what type of bond do you
think the compound is made from?
IONIC compound. The freely moving ions allow electricity to flow through the solution.
Use the electronegativity numbers in the chart on page 127 in your book to answer questions 4-6:
4. Which two elements have the largest electronegativity difference? If they bonded, what type of bond would they
form and why?
Either Cesium or Francium (0.7) bonded with Florine (4.0) to form an ionic bond.
5. What is the electronegativity difference between Potassium (K) and Fluorine (F)? (See the p.127). Show your
work! What kind of bond is this?
4.0 – 0.8 = 3.2 ionic bond.
6. Identify the type of bond (Ionic/Polar/Non-polar) for the following compounds: (See the p.127).
a. Magnesium and Fluorine
Ionic; 4.0 – 1.2 = 2.8 electronegativity difference
b. Carbon and Oxygen
Polar Covalent; 3.5 – 2.5 = 1.0 electronegativity difference
c. Beryllium and Sulfur
Polar Covalent; 2.5 – 1.5 = 1.0 electronegativity difference
d. Silicon and Oxygen
Even though the electronegativity difference is 3.5 – 1.8 = 1.7,
because both atoms are non-metals, the bond type is Polar covalent. Don’t stress, I won’t try to
trick you on the test!
7. Explain why water will bead up on a window (stick to the other water molecules).
Hydrogen bonds; the dipoles (+ & –) are attracted to each other because they have opposite charges on
each side of the molecule. This makes the water molecules “sticky”.
8. Explain in words and drawings why a butter stain (made from fat/oil) will not come out of a shirt if it is just
washed with plain water. In other words, explain and SHOW why the stain won’t dissolve.
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2016 – 2017 Chemistry end of semester test study guide. (Ch. 3/4)
9. Chemical Bonding REVIEW – In general, the three types of bonds between atoms that we see formed in
nature have some COMMON characteristics, which we have been studying and testing during this chapter. See if
you can figure out what those common characteristics are by filling in the table below. Use your lab data,
worksheets, books, brains and teammates to figure them out!
Bond
Type
Physical
characteristics
(color & texture)
Hardness
Conductivity
of Solid
Soluble
in
water?
Conductivity
in water
Melting
Point
Ionic
Salts, Crystals
form
Very hard
and
brittle
No
Yes
Yes
High
temp
Big difference;
> 1.6, but only
between metals &
nonmetals
Polar
Covalent
Medium
characteristics
will be half
way between
the other two.
Medium
No
Yes or
partially
Yes or
partially
Medium
Temp
Medium
difference;
0.5 – 1.6
Non
Polar
Covalent
Soft, greasy,
smooth
Soft
No
No
No
Low
Temp
Low difference;
< 0.5
12.
3 Rules for charges:
(1) ALL MATTER contains ______ charges ____.
(3)
Electronegativity
Difference (tug of
war)
(2) Like (+,+ or -,-) Charges REPEL.
__ Opposite ___ Charges ATTRACT.
Rules for solvation:
13.
“Like dissolves like”. This means that a polar covalent solution should dissolve a polar covalent
compound. (And a nonpolar covalent solution should dissolve a nonpolar covalent compound. And of course,
polar solvents like water dissolve/mix with ionic compounds (salts)).
14. What did Rutherford’s experiment prove about the atom? How did Rutherford accomplish this discovery?
The atoms have a small, dense positively charged nucleus at the center, and the majority of the
atom is empty space.
15. What did Niels Bohr discover about the atom, and how did he use the emission of light spectra from
elements to make this discovery?
When excited, electrons jump up to a higher energy level or valence shell, then they drop back to the
original position. Using this information, he was able to map out the electron configuration of atoms
which was highly useful to predict how chemicals will react with each other.
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2016 – 2017 Chemistry end of semester test study guide. (Ch. 3/4)
16. Define each of the following and give an example illustrating the term from a class activity.
a. Conservation of Matter- Atoms are not created or destroyed, only changed, This means in
chemistry all the matter or atoms found in the reactants will also be found in the final
product.
b. Reactants- The stuff you put into a chemical reaction.
c.
Products- The stuff you have after a chemical reaction.
d. Chemical Change- When atoms attach to other atoms in a new configuration to create new
molecules with different chemical characteristics.
17. Using the information given for Carbon on the periodic table and in the picture below to determine each of
the items below.
__6__ Protons
___6____ Electrons
___6___ Neutrons
___4___ Valence Electrons
18. Balance the following chemical Equations. For more practice go to
https://phet.colorado.edu/sims/html/balancing-chemical-equations/latest/balancing-chemical-equations_en.html
5
3
2
2
3
2
2
2
4
2
6
6
6
4