Upload
others
View
5
Download
0
Embed Size (px)
Citation preview
Chapter 01: 1
Chapter 01: 2 1) How many total electrons does a neutral atom of each element have? (Periodic Table above)
Oxygen Sulfur Nitrogen Aluminum
Sodium (Na) 2) Give the ground‐state electron configuration of each element. Use ( ) and ( ) arrows to show electrons when they are paired. Oxygen Nitrogen Sulfur
3) Identify the neutral atom that corresponds to the ground state electron configuration.
1s22s22p4 1s22s22p5 1s22s22p2
1s22s22p3 1s22s22p63s23p5 4) How many valence shell electrons does each element have?
Iodine Silicon Carbon Nitrogen
Sulfur Oxygen Sodium (Na) Aluminum
5) Draw a Lewis dot structure for the following atoms:
C O F H Br S
Cl I P N
8 16 7 13
11
↑↓↑↓↑↓ ↑ ↑
↑↓↑↓↑ ↑ ↑
↑↓↑↓↑↓
↑ ↑
↑↓ ↑↓
↑↓↑↓
O F C
N Cl
7 4 4 56 6 1 3
... . .
.: : : .‥
. .‥‥
‥: .
.: :
.‥‥:
.‥‥:
‥... . .
.‥
Chapter 01: 3 6) How many valence electrons does each of the following atoms have?
B Li Ne H Al Si
7) Clearly draw in all of the lone pair electrons ( ) (as large as these) on the structure below?
8) The compound above has...?
π‐bonds σ‐bonds
3 1 8 1 3 4
::
:
::
‥‥
‥
4 25
Chapter 01: 4 9) Draw a Lewis structure for each of the following. CLEARLY show each electron as a dot( ) (as large as this) . Ambiguous markings will not be scored.
C2H6
[C2H5]+
CH4O
BH3
CH2O
C2H4
10) Complete the partial Lewis structure of C3H9N below by filling in the missing hydrogens and electrons (as dots ( )).
C CHH
HHH H:
:
::‥‥‥‥
H
C CHH
H H
H‥‥‥‥: +
C O
B
HH
HH‥‥: : :‥‥
H HH‥: :
C OH
H::‥‥
C C:: ::H H‥ ‥H H
:: : :‥ ‥ ‥ ‥‥ ‥ ‥ ‥H H H
H
H H H H
Chapter 01: 5 11) What are the likely formulas? Place the numerical value for 'x' in the box. Consider that the other atoms or groups are attached to the atom underlined.
CClx CHxCl2
AlHx SiFx
AlClx CFxCl2 12) Write the number 2 in a box to indicate a non‐bonding electron pair is present on an atom. Write 0 in a box if no additional non‐bonding electron pairs are present. All boxes should be filled with a number.
4 2 23 4 2
3 2
22
0 22
0
20 0
0
2 2
20
0
2
22
22
Chapter 01: 6 13) Given the following electronegativities for the atoms below, circle the compound that contains the MORE POLAR bond (indicated) of each pair. (https://www.youtube.com/watch?v=6twRHdevc‐A) Relative electronegativities chart on first page:
14) For the molecules below with a dipole moment, indicate approximately the expected direction of the dipole moment with an arrow drawn in the box? (Note: trajectory of arrow is key). Otherwise, draw an 'X' in box if no dipole is present. (https://www.youtube.com/watch?v=TyFd94TbdXU)
X X
X
X
Chapter 01: 7 15) Calculate the formal charge on the atoms indicated. All electron pairs are shown. (Hint: use the Group numbers on the periodic table). (https://www.youtube.com/watch?v=otYj92d7rB0)
+1+1 0
–1
0 –1
–10
+1
0 –1
+1
0
+1
–1
–1 +1 –1
+1
0
–1 +1 –1 +1
0
0 +1
–1
0
–1
0
–1+1 0
0
+1
+1 +1
0
+1 –1
Chapter 01: 8 16) What is the molecular orbital hybridization, ie, spx, of the indicated atom? (https://www.youtube.com/watch?v=u1eGSL6J6Fo)
H3CCH3
H H
H H
N
sp3
sp3
sp3
sp3
sp2sp2 sp2
sp2
sp2
sp2
sp2
sp2
sp2
Chapter 01: 9 17) Identify the hybridization of the carbon atom shown, and then describe the nature of the orbitals used to create the bond between them.
C C
H
C
C
H
H
C
C
H
CC
C
O
C
H H
HH
HH
H
H
18) Predict the geometry as (B)ent (TPy) trigonal pyramidal (Tet)rahedral (TPn) trigonal planar (L)inear for all atoms (except hydrogens) in the compounds below. (Place B, TPy, Tet, TPn or L in the box).
OC C
CC
H H
HH
NH H
sp
sp
sp-sp
sp3
sp2
sp3-sp2
TPy Tet
B
TPnTPn
B
Tet
TPy
L
TPnB
B
Tet
TPn
TPn
TPnTPn
TPn
Chapter 01: 10 19) How many hydrogens (hidden in the skeletal drawing) are bonded to the atom indicated? If none, write 0 in the box.
O
11
3
0
1
00
0
2
0
0
1
22
2
0
3
Chapter 01: 11 20) How many sp3 and sp2 hybridized carbons do the following molecules have?
sp3 sp2 sp3 sp2
OH
O
Ibuprofen
sp3 sp2 sp3 sp2 HO
N
H
O
Acetaminophen
sp3 sp2
74 6 3
6 7 3 11
1 7
Chapter 01: 12 21) Arrange the following in order of increasing boiling point from 1 (LOWEST b.p) to 4 (HIGHEST b.p.)
22) For each of the following pairs of compounds CIRCLE the HIGHEST boiling point compound.
12 3 4