1. How Many Significant Figures Are There in the Number 0.02051?

1.  How many significant figures are there in the number 0.02051?

a.  2

b.  3

c.  4

d.  5

e.  6

2.  How many protons, neutrons, and electrons are found in a 65Cu+2 isotope?

a.  29 protons, 65 neutrons, and 27 electrons

b.  65 protons, 29 neutrons, and 27 electrons

c.  29 protons, 36 neutrons, and 29 electrons

d.  29 protons, 36 neutrons, and 27 electrons

e.  29 protons, 36 neutrons, and 31 electrons

3.  Which one of the following is a (an) Ionic compound ?

I.  NH4Cl (aq)

II.  Na2S

III.  CO2

IV.  I2

a.  I only

b.  II only

c.  III only

d.  IV only

e.  I & II only

4.  Which of the following pairs have compounds with the same empirical formula?

I.  C3H8 and CH4

II.  SO2 and CO2

III.  C6H12O6 and C2H4O2

IV.  NCl3 and NBr3

a.  I only

b.  II only

c.  III only

d.  IV only

e.  II and IV only

5.  Which one of the following is the correct formula resulting from a combination of the common ions from these elements: Mg and I?

a.  MgI

b.  MgI2

c.  Mg2I

d.  MgI3

e.  Mg3I2

6.  What is the formula of the compound, tin (II) cyanide ?

a.  Ti(CN)2

b.  Ti2CN

c.  Ti2CON

d.  Sn(CN)2

e.  Sn2CN

7.  Which chemical formula is NOT represented with its correct name?

a.  SO3 sulfite ion

b.  SiO2 silicon dioxide

c.  CO carbon monoxide

d.  CCl4 carbon tetrachloride

e.  All are correct.

8.  When the following reaction is balanced, what are the values of x & y?

____As4S6 + __x__O2 ® ____ As4O6 + __y__SO2

x / y
a. / 6 / 6
b. / 9 / 6
c. / 18 / 12
d. / 6 / 9
e. / 4 / 2

9.  Calculate the number of grams in 0.5 mol of Ge(NO3)4.

a.  160.30g

b.  158.90g

c.  139.30g

d.  67.30g

e.  0.002g

10.  How many molecules of C7H16 are in 200.0 g of this compound?

a.   3.01 x 1023 molecules

b.   1.20 x 1024 molecules

c.   1.20 x 1026 molecules

d.   3.01 x 1021 molecules

e.   2.57 x 1022 molecules

11.  What mass, in grams, of hydrogen is produced by the reaction of 5.63g strontium hydride with 4.80 g water? The balanced chemical equation is:

Reaction: SrH2 (s) + 2 H2O (l) → Sr(OH)2 (s) + 2 H2 (g)

Compound / SrH2 / H2O / H2
init. grams / 5.63 / 4.80 / 0.0
molar mass (g/mol) / 90.0 / 18.0 / 2.02

a.   1.08g

b.   5.63g

c.   0.06g

d.   0.54g

e.   0.25g

12.  You are a student worker assigned to make solutions in the first floor stockroom of Choppin Hall for the CHEM 1212 labs. Mr. Roya Hughes needs you to make 5.8 L of 1.25 M Na2S solution. How many grams of Na2S will you require?

a.  399.48 g

b.  566.23 g

c.  16.832 g

d.  362.38 g

e.  582.12 g

13.  How many mL of 10.5 M HCl solution is needed to make 2.5 liters of a 3.00 M HClsolution?

a. 1400 mL

b. 114 mL

c. 8.75 mL

d. 714 mL

e. Not enough information.

14.  An aqueous solution of chromium (III) chloride, CrCl3, reacts with an aqueous solution of sodium sulfide, Na2S. Which one of the following represents the complete molecular equation?

CrCl3 (aq) + Na2S (aq) ®

a.  2 CrCl3 (aq) + 3 Na2S (aq) ® Cr2S3 (s) + 3 Na2Cl2 (aq)

b.  2 CrCl3 (aq) + 3 Na2S (aq) ® Cr2S3 (s) + 6 NaCl (aq)

c.  CrCl3 (aq) + Na2S (aq) ® CrClS (s) + Na2Cl2 (aq)

d.  CrCl3 (aq) + Na2S (aq) ® Na2Cr (s) + SCl3 (aq)

e.  2 CrCl3 (aq) + 3 Na2S (aq) ® 2 CrS (s) + 6 NaCl (aq)

15.  An aqueous solution of sodium phosphate, (NH4)3PO4, reacts with an aqueous solution of copper (I) nitrate, CuNO3. Which one of the following represents the NET IONIC equation for the reaction?

(NH4)3PO4 (aq) + CuNO3 (aq) ®

a.  NH4+ (aq) + NO3- (aq) ® NH4NO3 (s)

b.  Cu+ (aq) + PO4-3(aq) ® CuPO4 (s)

c.  (NH4)3PO4 (aq) + CuNO3 (aq) ® CuPO4 (aq) + 3 NH4NO3 (s)

d.  3 Cu+ (aq) + 2 PO4-3 (aq) ® Cu3(PO4)2 (s)

e.  3 Cu+ (aq) + PO4-3 (aq) ® Cu3PO4 (s)

16.  Cr+6 is a fairly toxic form of chromium in comparison to Cr+3. A solution of Cr+6 can be titrated with a base like NaOH or KOH, as follows:

Cr+6 (aq) + 6 OH- (aq) ® Cr(OH)6 (s)

Calculate the number of grams of Cr+6 (MM of Cr = Cr+6 is 52.00g/mol) in an unknown sample that required 28.7 ml of 0.68M OH- solution to reach the end point.

a.  0.0696 g

b.  0.1691 g

c.  0.2487 g

d.  1.0148 g

e.  6.0890 g

17.  A source of electromagnetic radiation has a frequency, v, or 2.79 x 1013 s-1. What is its wavelength in nm?

a.  10,752.7 nm

b.  93,000.0 nm

c.  8.37 x1014 nm

d.  857.89 nm

e.  3.12 x 104 nm

18.  Calculate the energy (J) for one quantum of electromagnetic radiation, which operates at a frequency of wavelength of 720.6 nm.

a.  216.18 J

b.  4.77 x 10-31 J

c.  2.76 x 1049 J

d.  2.76 x 10-19 J

e.  2.76 x 10-37 J

19.  Which one of the following sets of quantum numbers are allowed?

n / l / ml
I. / 1 / 1 / -1
II. / 2 / 1 / -1
III. / 3 / 1 / -3
IV. / 4 / 2 / 0

a.  I & II only

b.  II only

c.  II& III only

d.  II & IV only

e.  All are allowed.

20.  What is the correct “long form” electronic configuration for the Co atom?

a.  1s2 2s22p6 3s23p64s24d7

b.  1s2 2s22p6 3s23p64s23d7

c.  1s2 1p62s2 2p63s23d7

d.  1s2 2s22p6 3s23p63d9

e.  1s2 2s22p6 3s23p64s23d5

21.  Based on “orbital” configuration, how many unpaired electrons are their in the highest occupied orbital/subshell for the nitrogen atom?

a.  0

b.  1

c.  2

d.  3

e.  4

22.  Which of the following has the higher ionization energy: C or Pb? Then select the correct statement that explains why your choice is correct.

Explain…………………………………………………….

23.  Which of the following sets of elements (Si, C, Zn, Ta) is correctly arranged in order of INCREASING atomic radius (smallest atoms listed first)?

a. / C / Si / Zn / Ta
b. / C / Zn / Si / Ta
c. / Zn / Zn / Ta / C
d. / Al / C / Ta / Si
e. / Ta / Al / Si / C

24.  Based on the trends of the periodic table, arrange the following atoms in order of INCREASING Ionization Energy: Fe, Ge, Si, Rb, O.

a. / Rb / Fe / Si / Ge / O
b. / Rb / Fe / Ge / Si / O
c. / Fe / Rb / O / Ge / Si
d. / Si / Ge / O / Fe / Rb
e. / O / Si / Ge / Fe / Rb

25.  Which of the following ions and/or elements form an ISOELECTRONIC set?

N , O, Ar, S-2, Ne

a.  N, O, Ne

b.  Ar, S-2, Ne

c.  Ar, S-2

d.  N, O

e.  Ar , Ne

26.  Given the electronegativity values for the following elements, place the following bonds in order of increasing polarity. Electronegativities: Si: 1.7 C: 2.5 F: 4.0 As: 2.2

Si-C Si-F Si-Si Si-As

a. / Si-F / Si-C / Si-As / Si-Si
b. / Si-F / Si-C / Si-Si / Si-As
c. / Si-As / Si-F / Si-C / Si-Si
d. / Si-Si / Si-As / Si-F / Si-C
e. / Si-Si / Si-As / Si-C / Si-F

27.  Which of the following is the most electronegative in each pair?

(i) Ca, Mg (ii) F, Cs (iii) Fe, As

a.  Mg, F, As

b.  Mg, F, Fe

c.  Ca, F, As

d.  Ca, Cs, As

e.  Ca, Cs, Fe

28.  Which species has a central atom which does violate the octet rule ?

I.  BH3

II.  ClF3

III.  H2O

a.  I only

b.  II only

c.  III only

d.  I and II only

e.  No violations

29.  The Lewis electron-dot structure of SBr4 gives the central atom:

a.  3 bonding pairs and 1 non-bonding pairs

b.  4 bonding pairs and 0 non-bonding pair

c.  4 bonding pairs and 1 non-bonding pair

d.  4 bonding pairs and 2 non-bonding pairs

e.  5 bonding pair

30.  How many resonance structures are there for HNO3?

a.  0

b.  1

c.  2

d.  3

e.  4

31.  What is the Electron Domain Geometry for NBr3?

a.  linear

b.  trigonal planar

c.  trigonal pyramidal

d.  tetrahedral

e.  trigonal bipyramid

32.  What is the Molecular Geometry for CH3- molecule?

a.  trigonal planar

b.  trigonal pyramid

c.  tetrahedral

d.  bent

e.  trigonal bipyramid

33.  Which of the following statements is correct?

a.  NF3 is polar.

b.  SF4 is nonpolar.

c.  XeF4 is polar.

d.  BF3 is polar.

e.  CF4 is polar.

34.  For the following molecule, what is the Hybrid Orbital Set around the N atom in the molecule NBr3?

a.  sp

b.  sp2

c.  sp3

d.  sp3d

e.  sp3d2

35.  Determine the volume in liter’s for a 43 g of NBr3 gas sample at a pressure of 850 torr and a temperature 20˚ C.

a.  0.24 L

b.  0.28 L

c.  1.22 L

d.  3.64 L

e.  877 L

36.  A sample of gas is confined to a cylinder housed with a movable piston. The gas occupies a volume of 1.8 L at 1.8 atm and 25°C. Calculate the volume of the gas sample if the pressure is increased to 8.6 atm at constant temperature.

a.  0.116 L

b.  0.377 L

c.  2.654 L

d.  2.845 L

e.  8.600 L

37.  A sample of a gas mixture with a total pressure of 18.9 atm contains 0.15 moles of N2, 0.67 moles of C2H2, and 0.27 moles of He. What is the partial pressure of C2H2 in the sample?

a. 5.722 atm

b. 6.240 atm

c. 11.62 atm

d. 12.66 atm

e. 18.90 atm

38.  Place the following gases in order of increasing rms velocity, u, at 25°, starting with the slowest first. H2, Rn, F2, CH4

a. / H2 / Rn / F2 / CH4
b. / F2 / CH4 / H2 / Rn
c. / Rn / CH4 / F2 / H2
d. / H2 / CH4 / F2 / Rn
e. / Rn / F2 / CH4 / H2

39.  What are all the Intermolecular Forces associated with CH3CH2SH?

a.  Ion-dipole; Hydrogen bonding; Dipole-dipole; Dispersion

b.  Hydrogen bonding; Dipole-dipole; Dispersion

c.  Dipole-dipole; Dispersion

d.  Dispersion only

e.  None of the above

40.  Which of the following substances would be likely to be miscible or dissolve in an polar solvent such as water, H2O?

I. NF3 (l)

II. CF4 (l)

III. C6H6 (l)

IV. NH4NO3 (s)

a. I only

b. I and II only

c. III only

d. I and IV only

e. II and IV only