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Chemistry 1st Quarter Review
Dimensional Analysis
Do the following showing all work and putting into correct significant figures.
1. 0.75 kg is _________ grams
2. 1500 millimeters to __________ km
3. 65 kg to _______________ pounds
4.
How many nanometers in a micrometer?
Density Problems
1. Calculate the density of sulfuric acid if 35.4 mL of the acid weighs 65.14 g.
2. Find the mass of 250.0 mL of benzene. The density of benzene is 0.8765 g/mL.
3. What is the density of water? What is its slope on a graph? (Be able to use graphs
as we did in class.)
Classifying matter
Classify the following as either elements, compounds, homogeneous mixtures (solutions)
or heterogeneous mixtures:
1. copper (II) sulfate _________________
2. Kool Aid _________________
3. wood ________________
4. air ________________
5.
Br2________________
6. CO2________________
7.
Be able to explain the similarities and differences of Compounds and
Heterogeneous Mixtures.
Vocabulary
Proton
Neutron
Electron
Average atomic mass
Atomic Number
Mass number
Isotope
Periodic Table
Groups
Periods
Noble Gases
Electron Configuration
Energy levels
Valence Electrons
Orbitals (S,P,D,F)
Lewis structure
Bohr diagram
Quantum mechanical model
Wavelength
Frequency
Photon
Ground state
Excited State
Isotope Notation
Homogeneous Liquid
Heterogeneous Liquid
Element
Compound
Atom
Molecule
Physical Change
Chemical Change
Density
People (Who were they and what did they do?)
Rutherford
John Dalton
J.J. Thomson
Average atomic mass calculation
Element X has two natural isotopes. The isotope with a mass number of 6 has a relative
abundance of 7.5%. The isotope with a mass number of 7 has a relative abundance of
92.5%. Determine the average molar mass for the element from these figures. What is the
true identity and atomic number of element X?
Explain why the atomic mass of most elements is not a whole number.
Lewis Dot
Draw Lewis dot for the following:
Li
B
S
Cl
Ca
Ar
Electron Configuration
Write the complete electron configurations for the following, including the orbital
diagrams:
1. Lithium ________________________________________
2. Chlorine ________________________________________
3.Calcium ______________________________________________
4. Rubidium __________________________________________________
Abbreviated version: Write the complete electron configurations for the following,
including the orbital diagrams
1.
Sodium
2. Argon
3.
Titanium
4.
Lead
Write the Isotope notation for
1. U-234
2. Carbon 13
3. A copper atom with 34 neutrons
Labs that you need to be able to explain what was happening.
1. Mass and Change Mini Lab
2. Flame Lab
3. Density Lab
4. Candium Lab