Download CHM134 General Chemistry I Semester Review – Dr. Steel This list

CHM134 General Chemistry I
Semester Review – Dr. Steel
This list represents the most important topics we covered in CHM134 this semester. It is not a complete list of every
topic that might appear on the final exam.
Formulas and Constants
K = °C + 273
M
D=
1 in = 2.54 cm
V
metric conversions
Chapter 1:
Properties of matter
Significant figures
Dimensional analysis – unit conversions
Chapter 2:
Atomic theories
1 mole = 6.022×1023 particles
Atomic mass and weight
Isotopes
Mole relationships for elements (moles, mass, number of particles)
Chapter 3:
Compounds: types and formulas
Prefixes (mon-, di-, etc.)
Naming and formulas (ionic compounds, molecular compounds, acids)
Polyatomic ions
Mole relationships for compounds
mass X
mass% =
× 100%
Percent composition
mass compound
Determining formulas from experimental data
Chemical equations
Chapter 4:
Reaction stoichiometry
mass formed
Limiting reactant problems
% yield =
× 100%
theoretical yield
Percent yield
Solubility rules
moles solute
Reaction types
Molarity =
V solution
Titrations
Solutions – concentration and dilution
M 1V1 = M 2 V2
Redox reactions – ox. numbers, e- transferred, oxidation, reduction
pH scale
Chapter 7:
Properties of light
Quantum mechanical model of the atom
Atomic orbitals
Chapter 8:
Electron configurations
Orbital diagrams
Periodic table and trends
Chapter 9:
Lewis dot structures
Resonance structures
Octet exceptions
Formal charges
Bond polarity
Energy changes for reactions
Chapter 10:
VSEPR
Molecular polarity
Valence bond theory
Orbital hybridization
σ- and π-bonding
Molecular orbital theory
MO diagrams – bond order
c=λ×ν
E=h×ν
c = 3.00×108 m/s
h = 6.626×10-34 J·s
Formal Charge Formula
Δ
∑
∑
Bond Order Formula
1. The density of a liquid is 0.835 g/L. What is the density in mg/mL?
2. Convert 45.9 km3 to mm3.
3. How many significant figures does the answer to this calculation have?
(4.16 + 2.4)×(1.37 – 1.01)
4. What is the formula of calcium nitrate?
5. What is the correct formula of cobalt(III)sulfate?
6. Name the compound FeCO3
7. Name this binary acid: HF
8. Name this ternary acid: HClO3 (ClO31- = chlorate ion)
9. Consider the bromide ion:
81
Br1-. How many protons, neutrons, and electrons does it contain?
10. What is the mass percent of fluorine in PF5?
11. Balance this equation: C3H8 + O2 Æ CO2 + H2O. What is the coefficient of O2?
12. Calculate the number of molecules in 2.50 grams of CO2.
13. Calculate the mass of 8.60×1024 atoms of Neon, Ne.
14. Balance the equation: P4O10 + H2O Æ H3PO4. How many grams of water are needed to react completely with 750.
g of P4O10?
15. 14.3 g of boron trichloride is hydrolyzed with 6.95 g of water according to the balanced equation:
BCl3 + 3 H2O Æ H3BO3 + 3 HCl. What mass of excess reactant remains?
16. What is the molarity of a solution prepared by adding 10.0 grams of NaOH per 500 ml of solution?
17. A solution is prepared by adding 55 mL of concentrated H2SO4 (18 M) to a small volumetric flask and diluting it to a
final volume of 800 mL. What is the approximate molarity of the solution?
18. What is the likely precipitate formed by the reaction: CrCl3(aq) + AgNO3(aq) Æ
19. What salt is formed when potassium hydroxide and sulfuric acid react?
20. Calculate the oxidation number of chromium in K2Cr2O7.
21. If n = 3, what are the allowed quantum numbers for l?
22. What element has the ground state electron configuration: [Ar]4s13d5?
23. What element has the ground state electron configuration: [Kr]5s2?
24. What is the maximum number of electrons permitted in a d sublevel?
25. Green light has a wavelength 512 nm. Calculate is frequency.
26. What bond angles are present between sp2 hybridized orbitals?
27. What geometry is associated with sp3d hybridization?
28. The ClF3 molecule will have what type of geometry?
29. The SF4 molecule will have what type of geometry?
30. What atomic orbital hybridization is used by Si in SiCl4?
31. In what molecular orbital is the highest energy electron of N2?
32. What is the bond order of N2?
Answers:
(1) 0.835 mg/mL (2) 4.59×1019 mm3 (3) 2 figures, the answer is 2.4 (4) Ca(NO3)2 (5) Co2(SO4)3
(6) iron(II)carbonate
(7) hydrofluoric acid (8) chloric acid (9) 35 p, 46 n, 36 e (10) 75.3% (11) 5 (12) 3.42×1022 molecules (13) 288 g (14) 286 g
(22) Cr (23) Sr
(15) 0.36 g H2O remain (16) 0.500 M (17) 1.2 M (18) AgCl (19) K2SO4 (20) +6 (21) 0, 1, 2
(24) 10 (25) 5.8×1014 Hz (26) 120° (27) trigonal bipyramidal (28) T-shaped (29) see-saw (30) sp3 (31) σ2p (32) 3