Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I would like to you help me with my homework because I struggled with step 6. Can you help me with step 6, please?
Transcribed Image Text:A₁ By E₁ = AB4
Molecular Shape of CC14
(1) Carbon central atom A
(4) Chlorine Batom surrounding central atom)
4 (0) lone pair Elone pair central atom)
Step 1: Find the Central Atom
Central atom is:
Look your line bond structure on
page 1.
: či:
4-C-C1:
fcr
Step 3: Choose the ABE classification
Circle the correct AB,Ey notation.
Recall, we use (A) to represent the
central atom, (B) to represent the
number of atoms bonded to the central
atom, and (E) to represent the number
of lone pairs
AB₁E3 AB₁E2 AB₁E
AB₂E2 AB₂
AB3E AB3 AB4
Step 5: Use the Molecular Shape
table from your notes to draw the
ball and stick representation
AB₂E
CI
Step 2:
Count number of atoms bonded to the central
atom (B)
# of atoms bonded to central atom= B =
Count number of lone pairs on the
central atom (E)
# of lone pairs on central atom = E=
Step 4: Use the Molecular Shape Table from
your notes to select the molecular shape and
bond angles.
Molecular Shape-tetrahedral
•110°
Bond angles.
4
Step 6: Determine Polarity
Is the central atom surrounded by identical
electron groups?
Circle one: yes
no
If the answer was yes, then the molecule is
nonpolar. If the answer is no, then the molecule
is polar.
Is the molecule polar?
Circle one: yes
/no
20
Expert Solution
Step 1
The polarity of the molecule can be decided by dipole moment of the molecule.
If the net dipole moment of the molecule not equals to zero, then the molecule exists as polar molecule.
If the net dipole moment of the molecule equals to zero, then the molecule exists as non polar molecule.
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