Unit 4-Chemical Bonds
Level 2 Review
Instructions: All questions in this review booklet must be answered and checked
prior to taking the level 2 assessment.
1. Learning Target: Predict the relative electronegativity of any two
elements on the periodic table.
a.
Practice: circle the element that has the higher electronegativity value.
i.
Na or Al
vi.
Cl or Br
ii.
K or Ca
vii.
P or Mg
iii.
Rb or Cs
viii.
I or N
iv.
As or P
ix.
H or Fr
v.
B or F
x.
H or Na
2. Learning Target: Identify the number of valence electrons in a neutral
atom and explain why these electrons are important in chemical
bonding.
a.
Practice: explain in one or two concise, grammatically correct sentence(s) why
valence electrons are important in chemical bonding.
b.
Practice: identify the number of valence electrons in each neutral atom:
i.
Na ____
vi.
At ____
ii.
Ca ____
vii.
Se ____
iii.
P ____
viii.
Ar ____
iv.
B ____
ix.
Si ____
v.
K ____
x.
C ____
3. Learning Target: Predict whether an atom will gain or lose electrons
when bonding using:
a.
Its location on the periodic table,
i. Practice: indicate whether each group will gain an e-, lose an e-, could both
gain an e- and lose e- (depending on what it’s bonding to), or neither gain or
lose e-.
(1) Group 1: Alkali metals
______
(2) Group 2: Alkaline earth metals
______
(3) Groups 3-12: Transition metals
______
(4) Group 13: Boron Family
______
(5) Group 14: Carbon Family
______
(6) Group 15: Nitrogen Family
______
(7) Group 16: Oxygen Family
______
(8) Group 17: Halogens
______
(9) Group 18: Noble Gases
______
b.
Its oxidation number(s),
i. Practice: use the element’s oxidation number(s), determine the number of
electrons it will gain and/or lose
Oxidation #s
Gain and/or Lose
(1)
Vanadium
__________
_____
(2)
Selenium
__________
_____
(3)
Iodine
__________
_____
(4)
Sodium
__________
_____
(5)
Nitrogen
__________
_____
(6)
Carbon
__________
_____
(7)
Sulfur
__________
_____
(8)
Calcium
__________
_____
(9)
Argon
__________
_____
(10) Tin
__________
_____
c.
Its Lewis Dot Structure & number of valence electrons
i. Practice: identify the number of valence electrons in each element, diagram
its Lewis Dot structure, whether it is more likely to gain or lose electrons, and
the number it will likely gain or lose.
d.
Its relative electronegativity value.
i. Practice: look back at your answers to question 1a. The same elements are
listed below. Underline the atom that will lose an electron and circle the one
that will gain an electron.
(1) Na or Al
(6) Cl or Br
(2) K or Ca
(7) P or Mg
(3) Rb or Cs
(8) I or N
(4) As or P
(9) H or Fr
(5) B or F
(10) H or Na
4. Learning Target: predict the formation of anions and cations, and the
relative strength of charges.
a.
Practice: Explain in a concise, grammatically correct sentence how cations are
formed.
b.
Practice: Explain in a concise, grammatically correct sentence how anions are
formed.
c.
Practice: identify the charge of each ion and whether each is a cation or anion.
5.
Learning Target: Predict the type of bond (ionic, polar covalent, nonpolar covalent, metallic) that will form between two atoms if by
calculating the electronegativity difference between them.
a.
Practice: complete the table below using the electronegativity value and scale in
Figure 5-1
6.
Learning Target: Describe what is happening at the molecular level
when ionic compounds or covalent molecules are created, and identify
the types of atoms that typically create those types of bonds.
a.
b.
c.
d.
Practice: an ionic bond is formed when atoms (share/transfer) electrons. They are
most often formed between (non-metals and metals/non-metals and nonmetals).
Practice: a covalent bond is formed when atoms (share/transfer) electrons. They
are most often formed between (non-metals and metals/non-metals and nonmetals).
If atoms share electrons evenly, a (non-polar/polar) covalent bond is formed.
If atoms share electrons unevenly, a (non-polar/polar) covalent bond is formed.
7. Learning Target: Define intermolecular forces as the force of attraction
between separate molecules.
a.
Practice: use the diagram below to answer the following questions.
i. What is the main difference between intermolecular forces and covalent &
ionic bonds?
ii.
State two similarities between intermolecular forces and covalent & ionic
bonds.