Question

1. What is the formal charge on each of the Oxygen atoms in the
chlorate ion, ClO_{3}^{-1}?

a. -1

b. 0

c. +1

d. +2

2. Draw the Lewis structure and predict the geometry for
SO_{4}^{-2}.

a. Bent

b. Linear

c. Tetrahedral

d. Trigonal Bipyramidal

3. Which of the following is **not** planar?

a. SO_{3}

_{b.} NO_{3}^{-}

^{c.} BCl_{3}

d. ClO_{3}^{-}

4. Draw the Lewis
structure and predict the geometry for SF_{4}.

a. Trigonal Pyramidal

b. Linear

c. Seesaw

d. Trigonal Bipyramidal

5. Write a Lewis structure for PF_{3} and then predict
the geometry.

a. Tetrahedral

b. Seesaw

c. Trigonal pyramidal

d. Bent

6. What is the number of **bonding electron pairs**
on the central atom in the chlorate ion,
ClO_{3}^{-1}.

a. 2

b. 0

c. 1

d. 3

7. All of the following species are best described by writing
more than one Lewis structure **except**

a. NO_{3}^{-}

^{b.} SO_{3}

_{c.} O_{3}

_{d.} IF_{3}

_{8.} Draw the Lewis structure and predict the geometry
for NH_{3}.

a. Trigonal Pyramidal

b. Bent

c. Tetrahedral

d. Square Planar

9. Which of the following has a **double
bond**?

a. CCl_{4}

_{b.} CO_{2}

_{c.} N_{2}

_{d. CO}

_{10.} The **total** number of
**nonbonding pairs** of electrons on **all
atoms** in CCl_{4} is

a. 24

b. 12

c. 32

d. 8

11. Draw the Lewis structure and predict the geometry for HCN

a. Linear

b. Trigonal Planar

c. T-shaped

d. Bent

12. Which of the following has a **triple
bond**?

a. NO_{3}^{-}

^{b.} Cl_{2}

_{c.} CN^{-}

^{d.} O_{2}

_{13.} Draw the Lewis structure and predict the geometry
for IF_{4}^{+1}.

a. Octahedral

b. Trigonal Bipyramidal

c. Seesaw

d. Square Pyramidal

14. What is the formal charge on Chlorine in the chlorate ion,
ClO_{3}^{-1}?

a. -1

b. +2

c. +1

d. 0

15. Why does H_{2}O have a bent geometry and not a
linear geometry?

a. Oxygen has 2 lone pairs of electrons

b. Oxygen has 0 lone pairs of electrons

c. Whatcha talkin bout Willis? It IS Linear!!

d. Oxygen has 1 lone pair of electrons

16. Draw the Lewis structure and predict the geometry for
SO_{3}.

a. Trigonal Pyramidal

b. Trigonal Planar

c. Bent

d. Linear

17. What is the formal charge for an Oxygen atom that has two bonds and two lone pairs of electrons in a molecule?

a. -2

b. -1

c. 0

d. +1

18. Carbon will try to form ____ bonds in order to have a 0 formal charge.

a. 3

b. 1

c. 2

d. 4

19. How many dots will the Lewis dot structure for Ra have?

a. 8 dots

b. 0 dots

c. 2 dots

d. 1 dot

20. What is the **formal charge** on the sulfur
atom in SO_{3}?

a. +2

b. +1

c. -1

d. -2

Answer #1

1.) An AB4 molecule has two lone pairs of electrons on the A
atom (in addition to the four B atoms). What is the electron-domain
geometry around the A atom?
square pyramidal
seesaw
T-shaped
trigonal pyramidal
linear
octahedral
trigonal planar
square planar
tetrahedral
trigonal bipyramidal
bent
2.) For the AB4 molecule in Part B, predict the molecular
geometry.
T-shaped
bent
trigonal pyramidal
trigonal planar
seesaw
tetrahedral
trigonal bipyramidal
square pyramidal
square planar
octahedral
linear

A)Draw a Lewis structure for BCl3 (remember that B is a frequent
exception to the octet rule).
Part B
Determine molecular geometry of BCl3.
A)linear
B)bent
C)trigonal planar
D)trigonal pyramidal
Part C
What kind of intermolecular forces are present in BCl3? (Can be
more then one)
A) dispersion force
B) dipole-dipole force
C) hydrogen bond
Part D
Draw a Lewis structure for HCOH (carbon is central; each H and O
bonded directly to C)
Part E
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Check all that apply.******
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of two sp2 orbitals C) a sigma (σ) bond formed by overlap of two
sp3 orbitals D) a pi (π) bond formed by overlap of two sp orbitals
E) a pi (π) bond formed by overlap of two p orbitals
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Problem 8.51
Part A
Write Lewis structure that obeys the octet rule for OCS and
assign formal charges to each atom.
Draw the molecule by placing atoms on the grid and connecting
them with bonds. Include all lone pairs of electrons. Show the
formal charges of all atoms in the correct structure.
SubmitMy AnswersGive
Up
Correct
Part B
Assign oxidation numbers to each of the atoms O, C, S in
OCS.
Express your answers as an integers. Enter your answers...

Draw the correct Lewis structure and calculate the formal charge
of each atom in the N2O molecule (N is the central
atom.). Use the resonance structure of the molecule N=N and N=O
bonds, (i.e., N=N=O) to determine the formal charges.
A. N = 0; N = –1, O = +1
B. N = +1; N = 0, O = -1
C. N = -1; N = +1, O = 0
D. N = 0; N = 0, O = 0...

1.First you need to find the number of valance electrons in
Ch3Cl. The number of valance electrons in an atom of an element is
equal to the last digit in the group number of that element in the
periodic table.
C is in group____ H is in group ____ Cl is in group _____
In CH3Cl there is a total of ____ valence electrons.
2. the model consists of balls and sticks. What kind of ball
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a) CSe2 b) AlF2I c)
N2O4
d)XeS64-
e)POCl3
the central atom is in bold
1.Total number of valance electrons
2.Draw the most appropiate Lewis Diagram
.Write the formal charges for the central atom
4.Does the structure exhibits resonance (are there equally
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If you can help me with at least one I will appreciate a lot.
Thank you

Natural Bond Orbitals
Natural Bond Orbitals (NBOs) convert molecular orbitals to the
form of localised bonding orbitals that correspond to Lewis
structures. Natural bond orbitals attempt to provide the most
accurate natural Lewis structure. The NBOs are localised and are
thus different to MOs - it is important not to over-interpret NBOs
- NBOs give an indication of bonding and electronic structure in
the framework of Lewis structures.
In this exercise you will explore the bonding description of
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