STRUCTURE OF MATTER
ATOMIC THEORY & STRUCTURE
Major Developments of Atomic & Quantum Theory
Scientist
Discovery
Experiment
Dalton (~1800)
JJ Thomson (1897)
Millikan (1909)
Rutherford (1911)
Planck (1900)
Einstein (1905)
Bohr (1913)
de Broglie (1923)
Chemical calculations
1. (a)What is an isotope?
(b)From the following data, what is atomic mass of chlorine?
mass in amu
Cl-35
34.96885
Cl-37
36.96590
fractional abundance
0.75771
0.24229
2. What is the %composition of Ba(NO3)2?
3. The % composition of a compound is 39.9% C, 6.7%H, 53.4%O.
(a) What is the empirical formula?
(b) If the molecular weight of this compound is 60.0 amu, what is the molecular compound?
Quantum Numbers
1. Define each of the following quantum numbers. What values are allowed?
n=
l=
ml =
ms =
2. For the highest energy electron in a P atom:
n = ____
l = ____
ml = ____
ms = ____
3. An electron transitions from n=2 to n=4. Is it endothermic or exothermic? _________________
a. Calculate the energy of the transition.
b. What wavelength of light is associated with this transition?
Electron Configurations & Orbital Diagrams
Atom/Ion
Electron Configuration
Orbital Diagram (valence)
Ge
Co3+ ion
Cu2+ ion
CHEMICAL BONDING
Types of bonds
a.
b.
c.
d.
e.
f.
g.
Explain each of the following and give an example.
ionic bond
covalent bond
metallic bond
van der Waals forces
London dispersion
Dipole attraction
Hydrogen bonding
Rank the above bond/forces from strongest to weakest _______________________________
Molecular Models
Molecule
Lewis
Diagram
Geometry
Bond Angle
Hybridization
NI3
CO2
CCl4
CH2O
ClO3
-
XeF4
ClF3
1. (a) Draw 3 different structures for COCl2
(b) Explain how you know which one is the correct structure.
2. Draw the nitrate ion and explain how it shows resonance.
#sigma
bonds
#pi bonds
PERIODIC PROPERTIES
1. Atomic Radius
Definition:
a. Draw a (mini) periodic table to show the trends across and down.
b. Explain why these trends happen. Use and explain the terms effective nuclear charge &/or
shielding in your answers.
2. Ionization Energy
Definition:
a. Draw a (mini) periodic table to show the trends across and down.
b. Explain why these trends happen. Use and explain the terms effective nuclear charge &/or
shielding in your answers.
3. Electron Affinity
Definition:
a. Draw a (mini) periodic table to show the trends across and down.
4. Electronegativity
Definition:
a. Draw a (mini) periodic table to show the trends across and down.