H
2.2
3 Li
2He
1
4Be
5B
2.0
13Al
1.6
31Ga
1.8
49In
1.8
81Tl
1.8
.98 1.6
11Na 12Mg
.93
19K
.82
37Rb
.82
55Cs
.79
87Fr
.70
1.3
20Ca
1.0
38Sr
.95
56Ba
.89
88Ra
.90
21Sc
22Ti
1.1
1.5
39Y
40Zr
1.2
1.3
57La*
72Hf
1.1
1.3
89Ac**
104Rf
1.1
Lanthanides *
Actinides **
23V
1.6
41Nb
1.6
73Ta
1.5
24Cr
25Mn 26Fe 27Co 28Ni 29Cu 30Zn
1.7 1.6
1.8 1.9 1.9 1.9 1.7
42Mo
43Tc
44Ru 45Rh 46Pd 47Ag 48Cd
2.2
2.1
2.2
2.3 2.2 1.9 1.7
74W
75Re
76Os
77Ir
78Pt 79Au 80Hg
1.7
1.9 2.2
2.2 2.2 2.4 1.9
6C
2.6
14Si
1.9
32Ge
2.0
50Sn
2.0
82Pb
1.8
7N
3.0
15P
2.2
33As
2.2
51Sb
2.1
83Bi
1.9
8O
9F
3.4 4.0
16S
17Cl
2.6 3.0
34Se 35Br
2.6 3.0
53I
52Te
2.7
84Po 85At
2.0 2.2
105Db
106Sg
107Bh
108Hs 109Mt
58Ce
59Pr
60Nd
61Pm
62Sm
63Eu 64Gd 65Tb
66Dy
67Ho
90Th
91Pa
92U
93Np
94Pu
95Am 96Cm 97Bk
98Cf
99Es 100Fm 101Md 102No 103Lr
Uun
Uuu
Uub
Uuq
Uuh
68Er
69Tm 70Yb 71Lu
0
10Ne
0
18 Ar
0
36Kr
0
54Xe
0
86 Rn
0
Uuo
1. What force of attraction is responsible for chemical bonding between the two fluorine atoms
in the diagram below? ________ 1pt
F
F
F F
a) An electrostatic force of attraction between the protons of one fluorine atom and the electrons
of the other fluorine atom
b) An electrostatic force of attraction between the electrons of one fluorine atom and the
electrons of the other fluorine atom
c) the magnetic force of attraction between the nucleus of one fluorine atom and the nucleus of the other
fluorine atom
d) the magnetic force attraction between the electrons of one fluorine atom and the electrons of
the other fluorine atom
e) the gravitational force of attraction between the nucleus of one fluorine atom and the nucleus of
the other fluorine atom
2. What type of bond / attraction is this and how do you know? 1pt
a) ionic b) metallic c) polar covalent d) nonpolar covalent e) London forces
f) dipole-dipole
g) hydrogen bonding
Why? 2pts nonmetal to nonmetal therefore covalent “0” electronegavitity difference indicates it
is a nonpolar covalent bond
3. What force of attraction is responsible for hydrogen fluoride molecules attraction to other
hydrogen fluoride molecules? _____1pts
H
F
H
F
a) the magnetic force of attraction between the nucleus of one hydrogen fluoride molecule and a the nucleus of a
neighboring hydrogen fluoride molecule
b) the magnetic force attraction between the electrons of one hydrogen fluoride molecule and the
electrons of another hydrogen fluoride molecule
c) the gravitational force of attraction between the nucleus of one hydrogen fluoride molecule and the
nucleus of another hydrogen fluoride molecule
d) the electrostatic force of attraction between a positive portion of one hydrogen fluoride molecule and
and the negative portion of a different hydrogen fluoride molecule
e) the electrostatic force of attraction between the a negative portion of one hydrogen fluoride molecule
and the positive portion of the same hydrogen fluoride molecule
4. What type of bond / attraction is this and how do you know? 1pt
a) ionic b) metallic c) polar covalent d) nonpolar covalent e) London forces
f) dipole-dipole
g) hydrogen bonding
Why? 2pts It is an attraction between the HF molecules that is caused by the attraction of a
hydrogen attracted to a fluorine of a neighboring molecule characteristic of hydrogen bonding.
5. What type of bond / attraction occurs between a hydrogen (H) and bromine (Br) in hydrogen
bromide which reacts with water to form an acid? How do you know this? 3pts
H-nonmetal Br-nonmetal therefore covalent, H-2.2 electronegativity Br-3.0 with a difference
of 0.8 indicating a polar covalent molecule
6. What type of bond / attraction occurs between a tungsten (W) atom and another tungsten(W)
atom? How do you know this? 3pts
metal to metal=metallic
7. What type of bond / attraction occurs between a oxygen atom (O) and another
oxygen atom ( O )? How do you know this? 3pts
nonmetal to nonmetal therefore covalent “0” electronegavitity difference indicates it is a nonpolar
covalent bond
8. What type of bond / attraction occurs between a tungsten (W) and a bromine (Br) atom?
How do you know this? 3pts
metal to nometal=ionic
9. Which of the following would have a relatively large atomic radius, require a small 1st ionization
energy, have low attraction for electrons, tend to lose electrons, and be described as positive ions
immersed in a sea of mobile electrons? 2pts This properties are characteristic of a metal
a) Hydrogen (H)
b) Sulfur (S)
e) Selenium (Se) f) none of these
c) Strontium (Sr) d) Scandium (Sc)
10. Which of the following are bonded because of a transfer of electrons that result in compound
that will not conduct as a solid but will conduct electricity in an aqueous solution? 2pts
This is characteristic of an ionic compound composed of a metal and a nonmetal
a) Strontium (Sr) and Sulfur (S)
b) e) Hydrogen (H) to Hydrgoen (H)
d) Hydrogen (H) and Selenium (Se)
c) Scandium (Sc) and Sulfur (S)
d) Hydrogen (H) and Sulfur (S)
11. Which of the following molecules attract each other because of momentary shifts in electrons
that create short lived positive and negative regions on one molecule that then attract negative
and positive regions on neighboring atoms 1pt-this describes London Dispersion Forces
Polar molecule
a) HCl—HCl
Dipole-Dipole
Nonpolar Molecule
Polar molecule-special
b) Cl-Cl ---Cl-Cl
c) H2O ---H2O
d)
London Dispersion Forces
Hydrogen bonding
none of these
12. Which of the following would have the highest melting point and boiling point because there
would be a greater probability of momentary shifts in electrons that would create short lived
positive and negative regions on one molecule that then attract negative and positive regions on
neighboring atoms? 1pt London dispersion forces increase with an increase in the number of
atoms/electrons in molecule causing higher melting and boiling points.
a) C4H10 b) C3H8
c) C2H6 d) CH4
13. How can a molecule like carbon tetrachloride CF4 contain polar bonds but is a nonpolar
molecule? 2pts - Although CF4 contains polar bonds it has a symmetrical shape that cancels
the polarity associated with each bond resulting in a nonpolar molecule. In order for a molecule to
have polarity it must contain polar bonds and an asymmetrical shape like H-O
H
14. What do each of the following have in common? 2pts
London dispersion forces
Dipole - Dipole Hydrogen bonding
They are intermolecular forces of attraction between molecules based on positive / negative regions
that are present or develop on the molecules that attract each other.
15 and 16 ( 14pts)
Molecule – Draw the
Molecule.
Total
number of
valence
electrons
OCl2
Cl - O - Cl
Total
valence
electrons
8
H3P
H
P H
Number of
Electrons
surroundin
g the
central
atom
Octet
Incomplete
Expanded
Number of
non-bonding
pairs of
electrons
surrounding
the central
atom
Bond
angle
90
104.5
107
90/120
109.5
120
180
Shape
Bent
Linear
Pyrimidal
Square Planar
Tetrahedral
Trigonal bypyrimidal
Trigonal planar
Octahedral
How
many
electron
surround
the O?
8
What type
of
arrangement
is found
around the
O?
Octet
How
many
NBPE’s
Surround
The O?
2
Bond
Angles
Around
The O
Molecular shape
associated with the
O?
What type
of
arrangement
is found
around the
P?
Octet
How
many
NBPE’s
surround
the P?
___1____
How
many
electrons
surround
the P
8
H
<109.5
Bent
Bond
angles
around
the P
Molecular shape
pyrimidal
<109.5_
17. How do atomic orbitals overlap in single double and triple covalent bonds. You can use diagrams to
illustrate your understanding. 3pts A sigma bond forms by an overlap of atomic orbitals between
the nuclei of the two atoms bonding. A Pi bond forms by an overlap of atomic orbitals above and
below the axis of between the nuclei of the two atoms bonding. Single covalent bonds form as a
result of sigma bonds. Double covalent bonds contain a sigma and a Pi bond. Triple covalent
bonds contain one sigma and two Pi bonds.
H O
H
H
C
C
C
C
H
18
C
O
H
H
19
What is the shape
and bond angle
associated with
this carbon and why?
3pts
4 to 1 0NBPE
Therefore 109.50
tetrahedral shape
20
What is the shape
and bond angle
associated with
this carbon and why?
3pts
3 to 1 0NBPE
Therefore 1200
trigonal planar
21
What is the shape
and bond angle
associated with
This carbon and why?
3pts
2 to 1 0NBPE
Therefore 1800
Linear
What is the shape
and bond angle
associated with
This oxygen and why?
3pts
2 to 1 2NBPE
Therefore <109.50
Bent
23. Which of the following can be used to illustrate the arrangement of atoms in SF2 ? Why? 2pts G_____
F–S
F
2 to 1 and 2 non bonding pairs of electrons therefore bent with angles <109.5o
22..Which of the following can be used to represent the arrangement of atoms in BCl3?
Why2pt B 3 to 1 and 0 non bonding pairs of electrons therefore bent with angles 120
24. Which of the following have both 90 and 120 degree bond angles and is trigonal bipyrimidal? D 1pt
A.
65 to 70.
B
F
C
D
E
G