Download Year End Chemistry Review

Fall Semester Chemistry Final Review
1. Homogeneous vs heterogeneous
2. Physical vs chemical changes
3. Metric System and metric conversions: 2 km = _____cm 100 cm = ____mm 5 m = ____km
4. Density as measured by water displacement: Find the density of a metal if its mass = 5.0 grams, the
initial volume of water without metal = 10.0 mL and the final volume of water with metal = 12.5 mL.
5. Significant figures: How many significant figures are in each of the following:
a) 0.003 g
b) 0.0300 g
c) 1.03 cm
d) 750 mL
e) 3.0 g – 2.5g / 5.0mL
f) 2.0mL + 3.02mL
g) 12.17cm X 3.2cm
h) 1.2g/5mL
Round each number to 2 sig figs: a) 0.0855
b) 0.9999
c) 1125 d) 1961
6. Periodic Table, periods and group names
7. Periodic trends: (ionization energy, electron affinity, electronegativity, atomic radius)
8. Atomic number = # of _____ Mass number = # of ________ Isotopes are atoms of the same element,
therefore having the same number of __________, but different number of ____ and a different
_______number.
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9.Isotopic symbols:
6 C:#
p = ___#e =___ # n =___ Calcium-41: # p = ___#e =___ # n =___
10. Fission vs Fusion. Describe each process and explain how atoms were made.
11. Place the following numbers into or take them out of scientific notation:
a) 3,000,000 b) 321,000 c) 0.00000000248 d)74.3 e) 7.419 x 104 f) 9.16 x 10-8
12. How many valence electrons are in each of the following elements:
a) He
b) F
c) N
d) Mg
e) Al
f) Na
g) S
13. For the above, show the charge of the ion formed, if any.
14. If oxygen goes from a charge of zero to –2, are electrons lost or gained? How many electrons?
15. Give the name or formula as needed
a) sodium sulfate
b) iron (III) sulfide
c) lead (IV) oxide
d) copper (II) hydroxide
e) CaCO3
g) Mg(NO3)2
h) CCl4 i) SO3
f) Ag2CrO4
16. Electron configuration: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 etc.
What is the electron configuration for Al?
17. Balance the equations: ___Fe + ___O2 _____ Fe2O3
18. Draw the Lewis (electron dot) structure:
a) NH3 b) O2
c) Cl2
d) CH4
____Ag2SO4 + ___AlCl3  ___AgCl
e) N2
+ Al2(SO4)3
f) water
19. What’s the difference between ionic bonding and covalent bonding? Between polar and nonpolar covalent?
20. What’s the difference between ionic properties and covalent properties? Consider melting and boiling points,
physical state, flammability, water-solubility and electrical conductivity as solutions or molten.
21. What is the molar mass? What is the molar mass of nitrogen atoms?___ Of Al2(SO4)3 ?_______
22. How many atoms of each element are in Mg3(PO4)2 ?
23. Avogadro’s number = ____________particles in one mole. Particles = _____ or _________________, not grams.
24. Converting grams to moles or moles to grams. Convert 42 grams of N2 to moles: ____
25. 2 H2O (g)  2 H2 (g) + O2 (g)
If 5.0 moles of water are decomposed, how many moles of oxygen are formed?
If 5.0 liters of water are decomposed, how many liters of oxygen are formed? (Notice this is the same
problem and can be done the same way.)
26. You have 3.1 moles of gas at STP, find the volume:
27. How many atoms are in 6.0 g of lithium?
28.You were given 100g of NaCl, how many moles were you given?
29. Convert 74.3 moles to grams of CO2: ___________________
30. Convert 2.718 x 105 grams of V(NO3)2 to moles:_________________________