IB HL Chem Bonding Test

Name _______________________ Per ____
Bonding Review Sheet
Why do atoms form chemical bonds?
To satisfy the octet rule
1.
2.
Define the following terms:
a) chemical bond: attraction of atoms
b) octet rule: 8 valence electrons, noble gas configuration
c) covalent bond: sharing of electrons to satisfy the octet rule
d) ionic bond: transfer of electrons (metal  nonmetal) to satisfy the octet rule
e) electrostatic forces: the forces that keep molecules together
3.
Explain how an ionic bond forms.
Metal transfer its valence electrons to a non-metal creating ions that are attracted by opposite charges
4.
An ionic bond is characterized as the transfer of electrons between an element with low electronegativity
and an element with high electronegativity. Covalent bonding is defined as the sharing of electrons
between an element with medium electronegativity and another element with higher electronegativity.
5.
An element has 19 protons. What will be the charge of ions it forms?
+1
6.
What will be the charge of the ions formed by an element with an electron structure of 1s22s22p63s23p5?
-1
7.
Valence electrons are only found in the __s__ and __p__ sublevels, not in the __d__ or __f__.
8.
What is a Lewis dot structure?
Visual representation of an element with its valence electrons
9.
Write dot structures for: potassium, arsenic, bromine, silicon, tellurium, aluminum, oxygen, sodium, and
radon.
K(1x)
Na(1x)
As(5x)
Rn(8x)
Br(7x)
Si(4x)
Te(6x)
Al(3x)
O(6x)
10.
An element forms a covalently bonded compound with hydrogen, and has the formula XH3. In which group
of the periodic table would X be found? What is the name of this group?
5A (15), Nitrogen family
11.
Two atoms each provide 3 electrons that are shared by the two atoms. This is an example of a:
a. single covalent bond
b. double covalent bond
c. triple covalent bond
d. quadruple covalent bond
12.
Two atoms each provide 1 electron that are shared by the two atoms. This is an example of a:
a. single covalent bond
b. double covalent bond
c. triple covalent bond
d. quadruple covalent bond
13.
A certain nonmetal usually forms two covalent bonds in its compounds. How many valence electrons does
this element have?
6 valence electrons
14.
Noble gases do not form chemical compounds because:
Have a full octet
15.
Which of the following compounds contains ionic and covalent bonds?
a. SiO2 (covalent)
b. BaF2 (ionic)
c. Na2CO3 (ionic)
d. Cl2O (covalent)
Complete the table for the following molecular compounds
Formula Lewis
3-d picture with dipole
Molecular
Structure
arrows
geometry
SO2
..
Bent 117
O
S
O
16.
SCl2
Cl
..
S
``
Cl
S
C
S
Polar?
Hybrid. of
center atom
Yes
Sp2
Bent 105
Yes
Sp3
Linear
No
Sp
Tetrahedral
No
Sp3
Trigonal
pyramidal
Yes
Sp3
Linear
No
--
Trigonal Planar
Yes
Sp2
Trigonal Planar
Yes
Sp2
CS2
CCl4
Cl
Cl
C
Cl
Cl
Cl
..
P
Cl
PCl3
Cl
O2
..
O
``
SO3
..
O
``
O
O
COCl2
S
O
O
Cl
C
Cl
Which of the molecules in the table above have possible resonance structures?
SO3, COCl2, CS2, SO2
17.
What elements are allowed to break the octet rule? Explain why they can do that.
Elements in period 3 -7 within the p sublevel, empty d sublevel to fill
18.
Compare and contrast Dipole-dipole and Van der Waal’s forces. Include their relative strengths and how
they arise.
Vdw are created by the presence of electrons, whereas dipole-dipole require two polar molecules, the
opposite (slightly negative and positive charges attract each other). Van der Waals weakest, dipole-dipole
stronger
19.
20.
In order to melt solids of each of the following substances, tell what type of bonding or forces of attraction
must be disrupted.
a) Zinc metallic
b) methane (CH4) van der Waals
c) ammonia (NH3) Hydrogen bonds
d) potassium chloride ionic
e) diamond network
What are some differences between molecules (covalent compounds) and network solids?
Covalent compounds are held together by forces and are weak compared to network solids that are
covalent lattice that is very strong.
21.
Explain why metallic bonding leads to good electrical conductivity.
Free floating electrons align to the electrical charge.
22.
23.
For each of the following pairs, circle the substance that would have the higher boiling point. Explain your
answer in terms of bonding principles.
a)
Rb or NaF
b)
PCl3 or MgCl2
c)
I2 or Cl2
NaF: ionic compound higher melting point (Rb is metallic, which has weaker
attractions)
MgCl2: ionic compound higher melting point (PCl3 is polar covalent, which has
weaker attractions)
I2: stronger van der Waals forces (both are nonpolar, but I2 is larger than Cl2)
PF3: polar, stronger forces (dipole-dipole) (SO3 is nonpolar and has which has
weaker attractions)
e) MgF2 or Ba
MgF2: ionic compound higher melting point (Rb is metallic, which has weaker
attractions)
f) CH3-CH2 -OH or CH3-O-CH3
CH3CH2OH: Has O-H bonds so molecule has hydrogen bonding
forces (CH3OCH3 is polar but has no O-H bonds, only has dipole-dipole forces)
g) H2O or H2S
H2O: Has O-H bonds so molecule has hydrogen bonding forces (H2S is polar but has
no O-H bonds, only has dipole-dipole forces)
d)
PF3 or SO3
What must be done to solid sodium chloride to allow it to conduct electricity? Explain
Become aqueous so the ions can be mobile (need moving charged particles in order for something to be
conductive, carry charge).
24.

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