C) selenium oxide

D) triselenium oxide

E) sulfur trioxide

10. When an amide (e.g. acetanilide) is hydrolyzed with NaOH, the products are ________.

A) acetic acid and aniline

B) sodium acetate and anilinium chloride

C) sodium benzoate and aniline

D) sodium benzoate and anilinium chloride

E) sodium acetate and aniline

11. The shape of the HCN molecule is ________.

A) linear

B) tetrahedral

C) trigonal pyramidal

D) bent (109°)

E) trigonal planar

12. The elements sodium, magnesium, and silicon ________.

A) are in the same group

B) have the same number of neutrons

C) have the same mass number

D) are isotopes of each other

E) are in the same period of elements

13. A solution with the same osmotic pressure as the blood is ________.

A) hypertonic

B) molar

C) isotonic

D) hypotonic

E) nontonic

14. Which of the following is not a chemical?

A) Water

B) Carbon dioxide

C) Salt

D) Sugar

E) Light

15. According to atomic theory, which statement is true?

A) all matter is made of electrons

B) atoms are neither created nor destroyed

C) atoms of different elements are same

D) atoms are same element have different mass

E) atoms can be split in chemical reactions

16. What is the classification for this reaction: SO3 + H2O → H2SO4?

A) Decomposition

B) Replacement

C) Combination

D) Combustion

E) Double replacement

17. A mixture is prepared by dissolving 2 g of KCl in 100 g of H2O. KCl is the ________.

A) covalent compound

B) solvent

C) solution

D) solute

E) liquid

18. What element has the electron arrangement 2, 8, 8?

A) Neon

B) Sulfur

C) Silicon

D) Argon

E) Oxygen

19. In the number 12.345, the 4 is in the ________ place.

A) tens

B) ones

C) tenths

D) hundredths

E) thousandths

20. Which of the following examples illustrates a number correctly rounded to three significant figures?

A) 0.03954 to 0.040

B) 4.05438 to 4.054

C) 109 526 to 109 500

D) 103.692 to 103.7

E) 20.0332 to 20.0

21. Chlorine has two isotopes, Cl-35 (75.8%) and Cl-37 (24.3%). The atomic mass of Cl is ________.

A) exactly 35

B) more than 37

C) 24.3

D) less than 35

E) between 35 and 37

22. The correct formula for the compound formed from K and P is ________.

A) K3P

B) KP

C) K2P

D) KP2

E) KP3

23. The molecule N2O4 has ________ valence electrons.

A) 16

B) 11

C) 6

D) 34

E) 22

24. Which of the following is not a characteristic of Group 1A elements (alkali metals)?

A) Good conductors of heat

B) Most are liquids at room temp

C) React vigorously with water

D) Shiny

E) Good conductors of electricity

25. 9.31 g is the same mass as ________.

A) 9310 mg

B) 931 μg

C) 0.0931 dg

D) 931 kg

E) 93.1 cg

26. Fe2(SO4)3 is called ________.

A) iron(III) sulfate

B) iron trisulfate

C) diiron trisulfate

D) iron(II) sulfate

E) iron sulfate

27. If the temperature is 20 °C, what is the temperature in Fahrenheit?

A) 94 °F

B) 43 °F

C) -22 °F

D) 239 °F

E) 68 °F

28. In 2Al + 3Br2 → 2AlBr3, what is oxidized and what is reduced?

A) AlBr3 oxidized, Al reduced

B) AlBr3 reduced, Al oxidized

C) Al reduced, Br2 oxidized

D) Al oxidized, Br2 reduced

E) Al oxidized, AlBr3 reduced

29. An L-enantiomer is defined by having the furthest chiral -OH group on the ________ side.

A) Bottom

B) Top

C) Right

D) Left

E) Middle

30. Ribulose is a 5-carbon ketone sugar. To what class does it belong?

A) Aldopentose

B) Aldotetrose

C) Ketopentose

D) Ketotetrose

E) Ketohexose

31. What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH?

A) 13 mL

B) 0.13 mL

C) 18 mL

D) 800 mL

E) 120 mL

32. Evaluate: (-4) x (-5) = ________.

A) 0

B) 20

C) -1

D) -20

E) 1

33. Which of the following contains an aldehyde functional group?

A) CH3-O-CH3

B) CH3-CH2-OH

C) CH3-CHO

D) CH3-CO-CH3

E) CH3-CH3

34. The main type of intermolecular force between particles of CH2I2 is ________.

A) ionic bonds

B) hydrogen bonds

C) dispersion

D) dipole-dipole

E) dispersion forces

35. 13.2 kJ is the same amount of energy as ________.

A) 36.2 kcal

B) 3.15 kcal

C) 3.15 cal

D) 55.2 kcal

E) 55.2 cal

36. An aldehyde forms a carboxylic acid by ________.

A) hydrogenation

B) oxidation

C) neutralization

D) hydrolysis

E) reduction

37. The function of the enzyme-substrate complex is to ________.

A) raise the energy of products

B) increase reactant concentration

C) change the product formed

D) lower the substrate energy

E) lower activation energy

38. Which is not a characteristic of the solid state?

A) Definite shape

B) Fixed positions

C) Definite volume

D) Particles move fast

E) Close together

39. What coefficient goes in front of O2 to balance: C5H8 + ? O2 → 5CO2 + 4H2O?

A) 3

B) 1

C) 5

D) 9

E) 7

40. What is molarity of KCl made by diluting 75.0 mL of 0.200 M to 100 mL?

A) 0.267 M

B) 6.67 M

C) 0.150 M

D) 0.200 M

E) 0.100 M

41. Identify the Brønsted-Lowry base in: H2O + CO32- ⇌ HCO3- + OH-.

A) HCO3-

B) CO32-

C) OH-

D) H2CO3

E) H2O

42. What is the IUPAC name of the ester formed from butanoic acid and ethanol?

A) Butyl ethanoate

B) Propyl ethanoate

C) Ethyl butyrate

D) Ethyl propanoate

E) Ethyl butanoate

43. How many moles of CaCl2 are in 250 mL of a 3.0 M solution?

A) 750 moles

B) 0.75 mole

C) 83 moles

D) 3.0 moles

E) 1.3 moles

44. A value of 36 mL is a measure of ________.

A) density

B) temperature

C) volume

D) mass

E) length

45. What is the IUPAC name of the 5-carbon alkane with methyl groups on C2 and C4?

A) 1,1,3-trimethylbutane

B) 2,4-dimethylpentane

C) 2-methylhexane

D) Heptane

E) 2,2-dimethylpentane

46. The ionization energy of atoms ________ going down within a group.

A) increases

B) decreases

C) stays same

D) doubles

E) vanishes

47. If apples are $0.67/lb, what is the cost of 2.5 kg of apples? (1 kg = 2.205 lb)

A) $ 1.68

B) $ 0.27

C) $ 3.69

D) $ 2.63

E) $ 0.76

48. Which of the following could be a buffer?

A) NaF(aq)

B) NaF(aq) + H2O(l)

C) HF(aq) + NaF(aq)

D) HF(aq) + H2O(l)

E) NaCl(aq) + HF(aq)

49. How many centimeters are there in 57.0 in.? (1 in = 2.54 cm)

A) 0.0445 cm

B) 145 cm

C) 22.4 cm

D) 140 cm

E) 22 cm

50. What is the mass number of an isotope of silver (At# 47) with 62 neutrons?

A) 107.9

B) 62

C) 109

D) 76

E) 47

A. 9310 mg. 9.31 g * 1000 mg/g = 9310 mg.

Step-by-Step Answer Key (26-50)

CHEM 1406 Finals Mastery

26

A. Iron(III) sulfate. Fe is +3 here to balance 3 sulfates (-2 each).

27

E. 68 F. Temp = 1.8(20) + 32 = 36 + 32 = 68.

28

D. Al oxidized, Br2 reduced. Al loses e- (0 to +3); Br gains e- (0 to -1).

29

D. Left. L for Left. The OH on the chiral center furthest from carbonyl is on left.

30

C. Ketopentose. Keto = ketone; pentose = 5 carbons.

31

D. 800 mL. 15 g / 100 mL = 120 g / X mL. X = (120 * 100) / 15 = 800.

32

B. 20. Negative times negative equals positive.

33

C. CH3-CHO. CHO is the condensed formula for an aldehyde group.

34

E. Dipole-dipole. (Correcting original key: CH2I2 is polar, so dipole-dipole is dominant).

35

B. 3.15 kcal. 13.2 kJ / 4.184 kJ/kcal = 3.154... kcal.

36

B. Oxidation. Adding an O atom or removing H atoms is oxidation.

37

E. Lower activation energy. Enzymes provide an easier path for reaction.

38

D. Particles move fast. In solids, particles vibrate in fixed positions; they move fast in gases.

39

E. 7. Right side has (5*2) + 4 = 14 Oxygen atoms. 14 / 2 = 7 in front of O2.

40

C. 0.150 M. M1V1 = M2V2. (0.200 M)(75 mL) = (X M)(100 mL). X = 15 / 100 = 0.150.

41

B. CO3^2-. It accepts the H+ from water to become bicarbonate.

42

E. Ethyl butanoate. Named alcohol-part (ethyl) + acid-part-oate (butanoate).

43

B. 0.75 mole. M = mol / L. Mol = 3.0 M * 0.250 L = 0.75.

44

C. Volume. mL is a unit of volume.

45

B. 2,4-dimethylpentane. 5C chain (pentane) with methyls at 2 and 4.

46

B. Decreases. Atoms get larger, valence e- are further from nucleus and easier to remove.

47

C. $3.69. 2.5 kg * 2.205 lb/kg = 5.5125 lb. 5.5125 lb * $0.67/lb = $3.69.

48

C. HF + NaF. Weak acid (HF) and its conjugate base salt (NaF).

49

B. 145 cm. 57.0 in * 2.54 cm/in = 144.78 cm. Round to 145.

50

C. 109. Mass Number = 47 (protons) + 62 (neutrons) = 109.