Chemistry 11A Review

1. Describe:

(a) Bohr’s model of the atom (b) The Quantum Mechanical model of the atom

2. How many electrons, protons and neutrons are in an atom for which the atomic number is 92 and the mass number is 235?

3. Draw an energy level diagram for K.

4. Give complete electron configurations and abbreviated electron configurations for: B, Ca, Ar

5. (I) Give the number of protons, electrons and neutrons in each of the following.

(II) State if they are anions or cations.

(III) Name the element they are isoelectronic with.

(a) Mg2+ (b) F- (c) N3- (d) Al3+

6. Name the element in:

(a) group 6A, period 4 (e) the metalloid in the halogen group

(b) the alkaline earth metals group, period 5 (f) the alkali metals group, period 3

(c) the halogen group, period 5 (g) the noble gas group, period 6

(d) the oxygen group, period 3

7. State if the element is a representative element, a transition metal, lanthanide, actinide, or a metalloid:

(a) N (b) Na (c) Ni (d) Nd (e) Zr (f) Ge

(g) Ga (h) Os (i) At (j) Al

8. For the following, list which are isoelectronic with each other and state which are isotopes. Identify X for each.

168X 168X2- 2010X 158X

9. Give the complete symbol (include atomic number, mass number and charge) for:

(a) an atom with 17 electrons, 18 neutrons.

(b) an ion with 19 protons, 18 electrons, 20 neutrons.

(c) an ion with a -1 charge, 10 electrons, 10 neutrons.

(d) an atom with 31 protons and 39 neutrons.

10. Complete the following table:

Element / Symbol / Atomic # / Mass # / # of Neutrons
nitrogen-15 / 8
2210Ne
beryllium-9 / 4

11. Define:

(a) valence electrons (b) anion (c) cation (d) ionization energy (e) electronegativity

(f) octet rule (g) ionic bond (h) covalent bond (i) polar bond (k) nonpolar bond

(l) intermolecular forces (m) hydrogen bonding (n) dispersion forces (o) dipole-dipole forces

12. Give complete electron configurations for:

(a) K (b) K+ (c) O (d) O2- (e) Mg (f) Mg2+ (g) Ar

13.What is the frequency of 480 nm wavelength of light?

14.What is the change in energy for when (a) n=3 to n=1 (b)n=6 to n=7 (c)n=4 to n=1

15. What are the quantum numbers for (a) 2s (b) 4p (c) 5d (d) 4f

16. Describe hybridization. Discuss sp, sp2 and sp3. Can you provide examples of each type of hybrid orbital? Can you use an energy level diagram to demonstrate hybrid orbitals forming? Ex: Discuss the bond type in methane and show how carbon has 4 bonding sites. What are sigma and pi-bonds. Where do they occur? How are they different?

13. Complete the following table:

Element / # of Valence Electrons / Dot Structure / Ion formed / Cation or Anion / Noble gas it is isoelectronic with
O
Na
P
Ca

For questions 14 to 17 can you explain these trends?

14. Circle the element with the larger atomic size:

(a) N or O (b) Ag or Au (c) K or Ca (d) Ge or Ga

15. Circle the element with the larger ionization energy.

(a) N or O (b) Ag or Au (c) K or Ca (d) Ge or Ga

16. Circle the element with the larger electro negativity value.

(a) N or O (b) Ag or Au (c) K or Ca (d) Ge or Ga

17. Arrange the following in order from least electronegative to most electronegative.

Ge, Mg, Fr, F, C, Te

18. Circle the bond that is the most polar: You will be given an electro negativity table on the exam

(a) C-O, C-N, C-F (b) P-N, As-Se, Br-Cl

(c) I-Cl, I-Br, I-F (d) Si-P, C-N, Ge-As

19. What is the most electronegative element? What is the least electronegative element?

20. (I) Determine if the following are ionic or covalent.

(II) If it is ionic, list the ions involved in the bonding

(III) If it is covalent, draw the Lewis structure, the actual structure, give the name of the shape and say if it is polar or nonpolar.

(a) MgCl2 (b) H2O (c) SeBr2 (d) NBr3 (e) Al2S3 (f) CH2S

(g) Na3N (h) CaO (i) CH2ClBr (j) SiO2 (k) AsCl3 (l) PCl5

(m) NH4+ (n) CO32- (o) KrF4 (p) BrF5 (q)ICl3 (r) SBr4

21. Naming:

(I) Name each of the following compounds: (italics = organic naming)

(a) Li2O (f) CuI (k) NH4Cl (p) H2S

(b) MgS (g) MgCO3 (l) Cu3(PO4)2 (q) HCN(aq)

(c) CuS (h) Be(NO3)2 (m) P4O10 (r) CH3COOH

(d) MnO (i) FeSO4 (n) ClO2 (s) CH4

(e) FeBr2 (j) Al2(CO3)3 (o) CBr4 (t) C5H12

(II) Write formulas for each of the following compounds:

(a) Iron(II) sulfide (e) iodine monochloride (i) calcium nitride

(b) lithium sulfide (f) sulfur hexafluoride (j) calcium nitrite

(c) silver carbonate (g)hydrogen chloride (k) calcium nitrate

(d) ammonium acetate (h) hydrogen bromide (l) potassium phosphide

Chemical Reactions: For the following reactions, complete and balance and state what reaction type.

1. (a) zinc + copper(II) sulfate à (b) silver nitrate + sodium bromide à

(c) aluminum + oxygen à (d) boron trioxide + magnesium à

(e) silver cyanide + potassium à (f) magnesium + nitrogen à

(g) potassium sulfate + barium chloride à (h) barium bromide + sodium phosphate à

(i) iron(III) oxide à (j) potassium iodide + chlorine à

(k) ethene + fluorine à (l) 1-pentanol + hexanoic acid à

(m) propane + chlorine à (n) pentane + oxygen à

2. Write balanced chemical equations for the following reactions:

(a) Calcium reacts with water to form calcium hydroxide and hydrogen gas.

(b) When heated, silicon and water produce silicon dioxide and hydrogen.

(c) When ammonium dichromate is heated, chromium (III) oxide, nitrogen, and water are produced.

3. Balance the following equations:

(a) Fe + H2O à Fe3O4 + H2 (b) NH3 à N2 + H2

(c) C5H10 + O2 à CO2 + H2O (d) Ca + NH3 à CaH2 + Ca3N2

(e) Al + H2SO4 à Al2(SO4)3 + H2

Chemical Calculations:

1. Determine the number of moles in:

(a) 25.0 g of NaCl (b) 125 g of H2SO4 (c) 35.0 g of CuSO4·5H2O

2. Determine the number of grams in:

(a) 1.70 moles of KMnO4 (b) 0.25 moles of KCl (c) 25.6 mL of CO2

3. Calculate the number of molecules in:

(a) 3.23 moles of H2O (b) 0.500 moles of CO2 (c) 2.11 g of NaCl

4. Calculate the number of moles in:

(a) 3.11 x 1025 molecules NH3 (b) 1.22 x 1024 atoms of Fe

5. How many atoms total are there in 1.3 x 1022 molecules of CO2?

6. Determine the percent composition of each element in (NH4)3PO4

7. In 5.00 g of a sample, 3.75 grams were carbon, and 1.25 g were hydrogen. Calculate the percent composition and the empirical formula.

8. The empirical formula of a compound is CH2. Its molecular molar mass is 70 g/mol. What is its molecular formula?

9. A compound is 64.9% C, 13.5% H and 21.6% O. What is its empirical formula?

10. A compound is 54.5% C, 9.1% H and 36.4% O. Its molecular molar mass is 88 g/mol. What is its molecular formula?

11. For the reaction N2(g) + 3H2(g) à 2NH3(g)

(a) How many moles of hydrogen are needed to completely react with two moles of nitrogen?

(b) How many grams of hydrogen are necessary to react completely with 50.0 g of nitrogen?

(c) How many grams of NH3 can be produced from the reaction of 28 g of N2 and 25 g of H2?

(d) How much of the excess reagent in part (c) is left over?

(e) 46.5 g of N2 are reacted with excess hydrogen. If 50.9 g of NH3 are produced, what is the percent yield?

(f) If I have 450.0 mL of nitrogen gas and 350.0 mL of hydrogen gas at STP, how many millilitres of ammonia gas will I produce at STP?

Organic Chemistry:

1. Draw structures for the following compounds:

(a) butane (b) 2-chloropentane (c) 3-methylhexane

(d) 2,2,4-trimethylheptane (e) 4-chloro-2,3-dimethyloctane (f) 2,3-dimethyl-3-hexene

(g) 4-ethyl-2,3-dimethyl-3-nonene (h) 1,5-dibromo-2,2-dichloro-3-heptyne

(i) 2-pentanol (j) 2,4,4-trimethyl-2-heptanol (k) heptanal

(l) 3-ethyl-2-methylhexanal (m) methyl ethyl ether (n) 2,3-dibromobutanoic acid

(o) 2-chloro-2,4-dimethyl-3-hexanone (p) ethyl pentanoate

2. Name the following compounds:

(a) (b)

(c) (d)

(e) (f)

(g) (h)

(i) (j)

3. Draw and name (3) isomers for (a) C7H16 (b) C8H16 (c) C6H12F2

4. Give the reaction for the combustion of pentane.

5. Complete the following reactions: (draw and name structures)

(b) 1-butene + chlorine

(d) butane + bromine

(e) methanoic acid + 1-hexanol

(f) Esterfication: making propyl butanoate