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MID TERM STUDY GUIDE:
October 30th
CONCEPTS:
• Chemical Bonding
– Types of Bonding
– Valence electrons
– Types of reactions
• Chemical Reactions
– Balancing
– Writing equations
– Types of reactions
• The Mole
– Molar Mass
– Conversions
– Empirical Formula
– Trends
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Electronegativity
Ionization energy
Atomic radius
Electron configuration
• Atoms
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Protons
Neutrons
Electrons
Ions, Isotopes
Bohr Models
Lewis Diagrams
• Periodic Table
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Groups Periods
Metals vs Non Metals
Atomic Number vs Mass
History
Trends
• Electronegativity
• Ionization energy
• Atomic radius
1. How many protons, electrons, and neutrons are there in an atom of chlorine-37?
2. How many protons, electrons, and neutrons, are in an atom of Bromine-80?
3. Write the nuclear symbol for carbon-13.
4. Write the nuclear symbol for an isotope with a mass number of 28 and atomic number of 14.
5. Write the hyphen notation for the element that has a mass number of 20 and atomic number 10.
6. Write the hyphen notation for the element that contains 15 protons and 15 neutrons.
7. Write the nuclear symbol and hyphen notation for an isotope with 26 protons and 30 neutrons.
8. Write the nuclear symbol and hyphen notation for an isotope with 56 electrons and 82 neutrons.
9. Determine the number of protons, neutrons, and protons for
64
29
Cu.
10. What family and period are the following in: 1. Ca 2. O 3. Ar
11. Draw and label an atom (include all the parts with charges)
12. Calculate the average atomic mass for copper if 69% has a mass of 63 amu and 31% has a mass of 65
amu.
13. Find the number of protons, neutrons, and electrons in the following:
p+
no
e-
A. Sodium
B.
89
38Sr
C. Aluminum-25
D. Ba2+
E. Iron-57
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Use the nomenclature rules and the flowchart to write formulas for the following compounds
1
calcium chloride
2
calcium carbonate
3
sodium cyanide
4
magnesium oxide
5
sodium fluoride
6
zinc iodide
7
aluminum chloride
8
rubidium acetate
9
cobalt (II) chloride
10 potassium hydride
11 copper (II) carbonate
12 potassium hydroxide
13 hydrogen bromide
14 rubidium cyanide
15 potassium fluoride
1. 1.20 x 1025 atoms of N to moles
2. 11.5 g of carbon to moles
3. 1.00 x 1026 atoms of Tl to grams
4. 0.400 moles of Cd(IO3)2 to formula units
5. 76.0 g of Ca to moles
6. 46.0 g of potassium nitride to formula units
7. 1.00 x 1023 formula units of CsBr to grams
8. 3.00 moles of Cl to grams
9. 9.30 moles of carbon dioxide to molecules
10. 8.00 x 1019 formula units of copper (II) sulfate to grams
11. 34.2 g of trisulfur dioxide to moles
12. 3.01 x 10 23 atoms of Mg to moles
13. 2.1 g of Ni to atoms
Write the electron configuration for the following elements, Noble gas configuration and uncondensed.
1. Neon
2. Ca
3. Oxygen
4. Iodine
5. Silicon
6. Iron
DRAW THE FOLLOWING molecules
a. CH4
b. NH3
c. H2O
d. SF6
e. CO2
f. C2H4
g. NH4+
f. NO3-
Be able to define these words
Isotope:
Ion:
Cation:
Anion:
Electronegativity:
Ionization energy:
Atomic Radius:
Covalent bonds:
Ionic Bond:
Atomic Mass:
Atomic Number:
Dalton:
Democritus:
Mendeleev:
Aufbau Principle:
Mole:
Molar Mass:
Valence Electrons:
Neutrons:
Protons:
Electrons: