NAME ___________________________________________________ PER_____Standard 3 Self Check!
Science Benchmark Standard III- Valence Electrons & Bonding
Instructions: Read through the standard, the objective and the indicator from our State Chemistry Core. On
your own paper, answer the questions next to each indicator. Mark the box next to each question as to
whether or not you Got IT!, Almost! Or Not YET!
Determine the number
of valence electrons in
atom using the
periodic table.
Predict the charge an
atom will acquire when it
forms an ion by gaining or
losing electrons.
Predict the bond types
based on the behavior
of valence (outermost)
electrons
1.
2.
3.
a.
Use a chemical formula to
represent the names of
elements and numbers of
atoms in a compound and
recognize that the
formula is unique to the
specific compound.
1.
2.
3.
4.
5.
6.
7.
Write the formula for copper (II) phosphate
How many atoms are in one molecule of copper (II) phosphate?
Name Ca(OH)2
Name CF4
Name H2SO3
Write the formula for carbonic acid
Write the formula for Triphosphorus pentasulfide
b.
Compare the physical
properties of a compound
1.
Which physical properties does sodium chloride have compared to the
elements sodium and chlorine that it is formed from? 2Na (soft reactive
metal) + Cl2 (green poisonous gas) →2NaCl (table salt )
An oxygen atom gains 2 electrons to form a stable molecule. What
would the charge be on an oxygen atom?
2. What is the charge on an aluminum ion?
3. An atom loses 4 electrons, what charge would the ion formed have?
c.
1. Which bond type occurs when atoms of an element with few valence
electrons bonds with an element that have many valence electrons?
2. Which bond type occurs when atoms containing similar numbers of
valence electrons bond?
3. Which bond type occurs when atoms are closely packed, positively
charged cations?
d. Compare covalent,
1. How do electrons in an ionic bond behave?
ionic, and metallic
2. How do electrons in a metallic bond behave?
bonds with respect to
3. How do electrons in a covalently bonded substance behave?
electron behavior and
4. A substance with which bond type would dissolve readily in water?
relative bond strength.
5. A substance with which bond type would have a high melting point?
6. Dynamite releases energy when nitrogen bonds are broken. Which type
of bond contains
Objective 2: Explain that the properties of a compound may be different from those of the elements or compounds from
which it is formed.
Indicator
Main Ideas/ILOS
QUESTIONS
Almost!
1.
Got IT!
b.
Where are valence electrons located?
How many valence electrons does an atom in group 2 row 4 have?
How many valence electrons does chlorine have?
Not YET!
a.
Almost!
Got IT!
STANDARD III: Students will understand chemical bonding and the relationship of the type of bonding to the chemical and
physical properties of substances.
Objective 1: Analyze the relationship between the valence (outermost) electrons of an atom and the type of bond formed
between atoms.
Indicator
Main Ideas/ILOS
QUESTIONS
Not YET!
Atoms form bonds with other atoms by transferring or sharing electrons. The arrangement of electrons in an atom,
particularly the valence electrons, determines how an atom can interact with other atoms.
The types of chemical bonds holding them together determine many of the physical properties of compounds. The
formation of compounds results in a great diversity of matter from a limited number of elements.
d.
2.
How do the properties of a compound compare to the elements that
formed it?
Compare the chemical
properties of a compound
to the elements that form
it.
Explain that combining
elements in different
proportions results in the
formation of different
compounds with different
properties.
1.
Write complete sentences explaining how the chemical properties of a
compound compare to the elements that form it. Use an example such
as sodium metal and chlorine gas in your explanation.
1.
Using complete sentences, explain that combining elements in different
proportions results in the formation of different compounds with
different properties. Use examples such as carbon monoxide and carbon
dioxide in your explanation.
a.
Generalize, from
investigations, the
physical properties of
substances with different
bond types.
b.
Given a model, describe
the shape and resulting
polarity of water,
ammonia, and methane
molecules.
c.
Identify how
intermolecular forces of
hydrogen bonds in water
affect a variety of
physical, chemical, and
biological phenomena
Suppose you conducted an experiment to test several different substances
with different bond types for solubility and conductivity. The results of the
experiment are listed in the chart below. Use them to answer the next three
questions.
Material
Solubility Conductivity of
Conductivity when
Solid
Dissolved in Water
Sucrose
Soluble
Did not conduct Did not conduct
NaCl
Soluble
Did not conduct Good conductor
Copper
Insoluble
Good conductor (Insoluble)
Wax
Insoluble
Did not conduct (Insoluble)
Potassium bromide Soluble
Did not conduct Good conductor
Brass
Insoluble
Good conductor (Insoluble)
1. Based on these results, which materials contain metallic bonds?
2. Which materials contain ionic bonds?
3. Which materials would most likely conduct electricity when heated to
form a liquid?
1. Draw the lewis structure of water.
a. What is its shape?
b. Is the molecule polar or nonpolar?
2. Draw the Lewis structure of ammonia (NH3)
a. What is its shape?
b. Is the molecule polar or nonpolar?
3. Draw the Lewis structure of methane (CH4)
a. What is its shape?
b. Is the molecule polar or nonpolar?
1. How does the shape of a molecule predict its polarity?
2. How do hydrogen bonds affect the boiling point of water?
Almost!
Got IT!
Objective 3: Relate the properties of simple compounds to the type of bonding, shape of molecules, and intermolecular
forces.
Indicator
Main Ideas/ILOS
QUESTIONS
Not YET!
c.
to the elements that form
it.