If today were the test – Bonding and Nomenclature
Name:
Period:
Chemistry
Date:
Part I
Define the following bonds.
1.
Ionic –
2.
Covalent – a shared pair of electrons between 2 nonmetals in a molecule
3.
Intermolecular Force, IMF – attractive force between particles in a substance
4.
Significance of an IMF – the melting point and boiling point temperatures increase with the IMF’s strength
attraction of opposite ions
Part II
Formula
NAME
5.
CO2
carbon dioxide
6
P2O5
diphosphorus pentoxide
7.
CCl4
carbon tetrachloride
8.
N 2O 5
dinitrogen pentoxide
Part III CHOOSE…
9.
Which term describes a shared pair of electrons between two nonmetal atoms?
A. covalent bond
B. dipole interaction
C. ionic bond
D. lone pair of electrons
10.
Which term describes an unshared pair of electrons on a nonmetal atom?
A. covalent bond
B. dipole interaction
C. ionic bond
D. lone pair of electrons
11.
Which term describes a molecule with a nonsymmetrical electron distribution causing a build-up of charge?
A. isomer
B. nonpolar
C. polar
D. resonance
12.
Which statement best describes a stable atom?
A. A carbon atom with four covalent bonds.
B. A nitrogen atom with three covalent bonds and a lone pair of electrons.
C. An oxygen atom with two covalent bonds and two lone pairs of electrons.
D. An atom obeying the octet rule and having a filled valence energy level.
13-15 A. bent
16.
17.
18.
B. linear
C. planar
D. pyramidal
13.
What is the geometry of ammonia, NH3?
D
14.
What is the geometry of water, H2O?
A
15.
What is the geometry of carbon dioxide, CO2?
B
E. tetrahedral
Which molecule has a Lewis structure with a tetrahedral geometry?
A. CH4
B. COCl2
C. HCN
D. AsCl3
Which molecule has a Lewis structure with a trigonal planar geometry?
A. CH4
B. COCl2
C. HCN
D. AsCl3
Which molecule does not contain any covalent bonds?
A. CH4
B. CuCl2
C. H2SO4
D. PBr3
If today were the test – Bonding and Nomenclature
Part IV
Write the formula for the neutral molecule created from each pair of ions.
19.
3K1+
+
1PO43-

K3PO4
20.
1Cr3+
+
3CN1-

Cr(CN)3
21.
2Ni3+
+
3S2-

Ni2S3
22.
1Pb4+
+
2O2-

PbO2
23.
2Ag1+
+
1SO32-

Ag2SO3
Part V
Dissociate each of the following neutral molecules.
24.
AgCl

Ag1+
+
Cl1-
25.
FeBr2

Fe2+
+
2Br1-
26.
Al(NO3)3

Al3+
+
3NO31-
27.
Na2SO4

2Na1+
+
1SO42-
28.
CaCO3

Ca2+
+
CO32-
Part VI
Write the corresponding ions and molecular formula for each name.
29.
magnesium sulfate
1Mg2+
+
1SO42-

MgSO4
30.
iron (III) oxide
2Fe3+
+
3O2-

Fe2O3
Part VII
Write the name of each ionic molecule. (you must name the ions!! not the formulas)
31.
Mg3N2
1Mg2+ + 1SO42- magnesium nitride
32.
Co(OH)3
Co3+ + 3OH1- cobalt (III) hydroxide
33.
Cu(NO3)2
Cu2+ + 2NO31- copper (II) nitrate
Part VIII
Draw the structure and state the geometry and polarity, and isomers (yes/no)
34.
O2 linear nonpolar, no isomers
35.
SiF4 tetrahedral, nonpolar, no isomers
36.
C2H2Cl2
37.
PBr3
planar, polar, yes isomers – 1st Cl’s on same carbon, 2nd Cl’s on diff C’s same side of double bond,
3rd Cl’s on diff C’s opposites sides of double bond
pyramidal, polar, no isomers