Supplemental Instruction
Iowa State University / Leader: / Natalie
Course: / Chem 163
Instructor: / Burke
Date: / 2-28-14
1) Suppose a red laser pointer emits light with a wavelength of 600 nm, calculate the energy in kJ (E=hc/ λ) (h=6.626x10-34J*s) (c=3.00x108 m/s).
1x109nm 6.626x10-34 J*s 3.00x108m 1 kJ
600 nm 1 m 1 s 1000 J
2) Which of the following is symmetrical?
a) CH2Cl2
b) COH2
c) Water
d) Carbon Dioxide
3) Write the subshells corresponding to the following shell and the max number of electrons each shell and subshell hold and the shape of the subshell.
a) n=1:s (2 e-) total electrons for n=1 (2e-), s subshell= sphere shaped
b)n=2:s (2e-), p (6e-), total electrons for n=2 (8 e-), s= sphere, p= dumbbell
c)n=3:s (2e-), p (6 e-), d (10 e-), total electrons for n=3 (18e-) s= sphere, p=dumbbell, d= clover
d)n=4:s (2e-), p (6 e-), d (10e-), f (14 e-), total electrons for n=4 (32 e-) s= sphere, p= dumbbell, d= clover, f you don’t need to know the shape
4)Write an electron configuration for a stable ion of S.
1s22s22p63s23p4 or [Ne]3s23p4
5) Define Symmetry:
a compound is symmetrical when there are no lone pairs around the central atom and when all the binding elements are the same.
6)Give the element symbol and name for the following:
a)[Ar]4s23d2Ti
b)1s2s222p63s23p4 S
7) Explain the difference between ground state and excited state:
Ground State: where you expect electrons to be.
Excited State: when electrons are not where you expect them to be.
8) Circle the following that does not correspond to a condensed phase of matter
a) Water Vapor
b) Motor Oil
c) PVC Pipe
d) Rubbing Alcohol
9) Give the chemical formula and name of the compound formed between the given elements:
a) Barium (Ba) and Phosphorous (P) Ba3P2 Barium Phosphide
b) Potassium (K) and Sulfur (S) K2S Potassium Sulfide
10) Explain the difference between an ionic and covalent bond. Are these intermolecular or intramolecular forces?
Ionic: transfer of electrons.
Covalent: sharing of electrons
11) Circle the following statement that is true
a) London> Dipolar
b)Intermolecular forces are most important in the liquid state of matter.
c)Hydrogen bonding is the weakest intermolecular force
d) Dipolar intermolecular forces are 10% as strong as intramolecular forces.
12) Which is the most electronegative?
a. Se b. Cr c. S d. P e. Cs
13)Choose the element with the highest ionization energy.
a. Na b. Ni c. As d.N e. Si
14) Arrange the following according to increasing atomic size.
a. Ba b. Sr c. Sn d. Te Te<Sn<Sr<Ba
15) Arrange in order of increasing polarity.
Na-F O-F N-F F-F F-F<F-O<F-N<F-Na
16) Complete this table with the missing chemical formula or name.
Chemical formula / Chemical nameBaOH / Barium Hydroxide
AlN / Aluminum Nitride
K3P / Potassium Phosphide
CaCl2 / Calcium Chloride
17) Fill in this table:
Compound name / FormulaIron(II) Bromide / FeBr2
Chromium(III) Nitride / CrN
Mercury(I) Cyanide / HgCN
18) Complete this table
Compound / Lewis Dot StructureAXE / # of bonding sites & # of lone pairs / Molecular shape / Bond angles / Polarity
AsBr3 / AX3E1
..
Br-As-Br
|
Br / #bonds: 3
#lp:1 / Trigonal Pyramidal / 107.5o / Polar
CO2 / O=C=O
AX2E0 / #bonds: 2
#lp: 0 / linear / 180o / Nonpolar
NCl3 / AX3E1
..
Cl-N-Cl
|
Cl / #bonds: 3
#lp: 1 / Trigonal Pyramidal / 107.5o / Polar
19) Draw a resonance structure for the carbonate ion (CO3-2)
O=C-O O-C=OO-C-O
| | ||
O O O
20) Define Hydrogen Bonding and draw an example of it.
Intermolecular force of compounds with FON bonded to hydrogen and has alone pair.
H
| ..
:O: |||||||||H-O-H
| ..
H
21) Draw an example of Dipolar bonding.
δ+ δ- δ+ δ-
22) Determine the correct number of valence electrons for all of the groups on the periodic table and the type of ion they will form (anion vs. cation).
Group 1:1, cation
Group 2:2, cation
Group 3:3, cation
Group 4:4, both, variable upon situation
Group 5:5, anion
Group 6:6, anion
Group 7:7, anion
Group 8:8, none, noble gas
23) An electron moves from level N=4 to N=1 calculate the wavelength of light that is produced. Is this light visible? Why or why not? (N=1 has 1.0 eV of energy, N=4 has 13.8 eV of energy), (1 eV= 1.6023x10-19 J) (E=hc/ λ) (h= 6.626x10-34J*s) (c=3.00x108m/s).
1.0 eV- 13.8 eV= -12.8 eV
λ= 6.626x10-34J*s 3.00x108m 1 eV 1x109nm = -97 nm, no this is not visible, it
1 s 1.60233 x10-19 J 1 m does not fall within the range
of visible light.