CHM 2041 - Chemistry Fundamentals IB

Final Exam Study Union Packet (Peer Tutor Lily L.)

Disclaimer: Pictures from above are from the 4th Edition of the textbook. Practice

problems are modified and compiled by the tutor. They do not serve as a replacement for

studying; they are a supplement.

Ch. 8

1. A photon has a frequency of 6.12 * 10^14 1/s. How much energy would half a mole of these

photons possess?

a) 3.46E5 J b) 1.22E5 J c) 6.98E4 J d) 2.73E5 J

2. Orange light has a wavelength around 640 nm and blue is around 475 nm. Which has a higher

frequency?

a) Orange b) Blue c) Neither (same frequency) d) Not enough info

3. Paola needs to determine the amount of kilojoules needed to excite a hydrogen atom from

second principal energy level to the fifth. Help her out.

a) 4.60E-19 kJ b) 4.58E-22 kJ c) 4.57E-20 kJ d) 4.55E-16 kJ

4. Find the uncertainty in position of an electron that is going about 76050 m/s. (m of e- =

9.11E-28 g)

a) 8.20E-11 m b) 5.79E-11 m c) 2.62E-11 m d) 9.00E-11 m

5. Which would result in the absorption of the photon with the shortest wavelength?

a) n: 3->5 b) n: 2->4 c) n: 4->2 d) n: 5->3

6. Circle the correct possible quantum number values for an electron with a principle level of 4.

a) l: 1, 2, 3, 4. ml: -4, -3, -2, -1, 0, 1, 2, 3, 4. ms: -1/2, +1/2

b) l: 0, 1, 2, 3, 4. ml: -4, -3, -2, -1, 0, 1, 2, 3, 4. ms: -1/3, +1/3

c) l: 1, 2, 3. ml: -3, -2, -1, 0, 1, 2, 3. ms: -1/2, +1/2

d) l: 0, 1, 2, 3. ml: -3, -2, -1, 0, 1, 2, 3. ms: -1/2, +1/2

7. The de Broglie wavelength of a certain electron is 8.03E-12 m. Find its velocity. (m of

electron = 9.11E-28 g)

a) 8.43E7 m/s b) 2.73E8 m/s c) 8.25E6 m/s d) 9.06E7 m/s

8. Identify the incorrect match.

a) d: l=2

b) s: l=1

c) red: lowest energy of visible light spectrum

d) Gamma rays: shortest wavelength

Ch. 9

9. Which element has an electron configuration of [Ar] 4s1 3d5?

a) Co b) Cr c) Cu d) Invalid configuration

10. Which trend is matched to its correct definition?

a) Ionic radius: increases upwards and to the right

b) Electron affinity: increases upwards and to the left

c) Electronegativity: increases upwards and to the right

d) Effective nuclear charge: increases downwards and to the left

11. Select the correct representation of Hund’s Rule (and Aufbau Principle).

a)

b)

c)

d)

12. Arrange these from smallest radius to largest: P^3-, K+, Ar, Ca^2+

a) Ca^2+<K+<Ar<P^3- b) P^3-<Ar<K+<Ca^2+

c) K+<Ar<Ca^2+<P^3- d) Ca^2+<Ar<K+<P^3-

13. Below is a list of successive ionization energies for a third period element. What is the

element? IE1: 1012 kJ/mol IE4: 4960 kJ/mol

IE2: 1900 kJ/mol IE5: 6270 kJ/mol

IE3: 2910 kJ/mol IE6: 22200 kJ/mol

a) S b) P c) Mg d) Sc

14. Which is not a viable representation of ionization energy?

a) K->e- + K+ b) Mg+->e- + Mg^2+

c) F- -> F + e- d) e- + Li+ -> Li

__ __ __ __ 2s 2p

__ __ __ __ 2s 2p

__ __ __ __ 2s 2p

__ __ __ __ 2s 2p

15. The orbital diagram of an anion of 3- is shown:

Identify the element.

a) Mg b) F c) C d) Al

16. Which element has the greatest magnitude of electron affinity?

a) Te b) Sr c) Rb d) Xe

Ch. 10

17. Which has the smallest lattice energy in terms of magnitude?

a) LiF b) SrTe c) BeO d) RbI

18. Which is the most stable Lewis structure for the carbonate ion?

a) b)

c) d)

19. How is it possible to have a molecule like SBr5?

a) The amount of protons is strong enough to keep all the atoms in place

b) Sulfur’s size allows enough room for all the bromines to bond

__ __ __ __ __ __

c) Bromine contains a large d orbital which can hold more than eight e-

d) None of the above

20. Choose the endothermic reaction.

C-F: 552 kJ/mol

a) CH3CH2CH2CHO + O2 -> CO2 + H2O b) CH4 + H2O -> H2 + CO2

c) CH3CH2OH + HCl -> CH3CH2Cl + H2O d) CH2CH2 + F2 -> CH2FCH2F

21. Which is the longest bond?

a) HBr b) HAt c) HF d) HH

22. What is the formal charge of oxygen in CH2O?

a) -1 b) 0 c) +1 d) +2

23. Which has the largest electronegativity difference?

a) HF b) CO c) NaCl d) F2

24. Calculate the heat of formation of NaCl(s) from its elements in their standard states and the following: Given information ∆H°

Na(g) -> Na(s) -108 kJ

1/2 Cl2 (g) -> Cl(g) +122kJ

Na+(g) + e- -> Na(g) -496kJ

2Cl(g) + 2e- -> 2Cl-(g) -698kJ

Na+(g) + Cl-(g) -> NaCl(s) -788 kJ

a) -411 kJ b) 410 kJ c) -511 kJ d) 114 kJ

Ch. 11

25. Using formal charge, how many sigma and pi bonds are present in the best resonance

structure for PO4^3-

a) 4, 0 b) 3, 1 c) 5, 0 d) 4, 1

26. What is the electronic geometry of Al(Br3)?

a) Trigonal Planar b) Tetrahedral c) Trigonal Pyramidal d) Bent

27. Between CH3CH2CH2CH2CH2CH2CH3 and CH3CH2CH2CH3, which has the highest

boiling point?

a) CH3CH2CH2CH2CH2CH2CH3 b) CH3CH2CH2CH3

c) They have the same boiling point d) Not enough information

28. What is the hybridization of IF4^+?

a) sp5 b) sp3d2 c) sp4d d) sp3d

29. Select the true statements: I. Sigma bonds take the most energy to break.

II. Single bonds take the most energy to break.

a) I. only b) II. only c) I. and II. d) None

30. Some molecule is composed of a central atom attached to two lone pairs and three chlorines.

What is the molecular geometry and is this molecule polar or nonpolar?

a) Trigonal Bipyramidal; nonpolar b) Distorted tetrahedron; polar

c) T-shaped; polar d) See-saw; nonpolar

31. What is the bond order of HCl?

a) -1 b) 0 c) -2 d) +1

32. How many antibonding electrons are in F2?

a) 7 b) 6 c) 5 d) 4

Ch. 6

33. A sample of oxygen was collected by displacement of water at 25 . The system’s pressure ℃was 90 torr. What is the mole fraction of O2? Vapor pressure of water = 24 torr at 25 .℃

a) 94/100 b) 56/100 c) 73/100 d) 82/100

34. What is the density of I2 gas at STP?

a) 11.33 g/L b) 22.4 g/L c) 27.3 g/L d) 31.3 g/L

35. Laura opens a previously-closed container of gas. What is the direct effect on pressure?

a) Increases

b) Decreases

c) No effect

d) There’s like no information in this question, how am I supposed to ans--

36. A 1.25 g gas sample occupies 663 mL at 14 and 50.66 kPa. What is the gas?℃a) Rb b) Sr c) Y d) Zr

37. Lowest volume at STP?

a) 5.0 g Rn b) 7.0 g Xe c) 10.0 g Kr d) 14.0 g Ar

38. 4.91 g of methane gas is occupying a volume of 7 kL. How many moles would there be if the

volume was lowered by 2 kL?

a) 0.22 mol b) 0.45 mol c) 0.09 mol d) 2.14 mol

39. Carbon monoxide versus carbon dioxide; who would win (i.e which gas would diffuse

faster)? By a factor of how much?

a) CO; 0.798X b) CO; 1.253X c) CO2; 0.798X d) CO2; 1.253X

40. Hampton is conducting an experiment on the Free Speech Lawn on diatomic gases. 3 moles

of each species is being held separately in a 100 mL container. The temperature outside is 30 . ℃Hypothesize with this information which element will have the

highest pressure.

a) H2 b) N2 c) O2 d) Cl2