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MRII INORG REVIEW QUESTION Flashcards

1
Q

Arrange the proton, neutron and electron in increasing mass.

a. proton electron < neutron
b. electron < proton < neutron
c. electron neutron < proton
d. neutron electron < proton

A

b. electron < proton < neutron

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2
Q

The constant known as the fundamental number of hydrogen is the

a. Rydberg constant
b. Planck’s constant
c. Fine-structure constant
d. Balmer constant

A

d. Balmer constant

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3
Q

In Rutherford’s experiment, which of the following is true?

a. the proton is evenly distributed in the nucleus of an atom
b. the atom is almost an empty space
c. the nucleus contains proton, neutron and electron
d. all of the these

A

b. the atom is almost an empty space

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4
Q

The sum of the number of protons, neutrons and electrons of a zinc ion, Zn^+2 is

a. 94
b. 92
c. 95
d. 93

A

d. 93

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5
Q

The region in space where an electron is most likely to be found is called

a. orbital
b. energy level
c. shell
d. nucleus

A

a. orbital

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6
Q

Calculate the series limits of
Balmer series (m = 2)

a. 4389 cm ^ - 1
b. 27434 cm ^ - 1
c. 12193 cm ^ - 1
d. 6859 cm ^ - 1

A

b. 27434 cm ^ - 1

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7
Q

Calculate the series limits of
Brackett series (m = 4)

a. 4389 cm ^ - 1
b. 27434 cm ^ - 1
c. 12193 cm ^ - 1
d. 6859 cm ^ - 1

A

d. 6859 cm ^ - 1

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8
Q

Atoms with the same atomic number but different mass number is called

a. isobars
b. isotopes
c. isotherms
d. isoelectronic

A

b. isotopes

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9
Q

The quantum number that has an allowable value of 0, 1, 2, etc. is the

a. Magnetic Quantum Number
b. Spin Quantum Number
c. Angular Momentum Quantum Number
d. Principal Quantum Number

A

c. Angular Momentum Quantum Number

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10
Q

Calculate the minimum wavelength of light necessary to overcome the work functions for Li (phi = 2.9eV)

a. 248 nm
b. 428 nm
c. 575 nm
d. 581 nm

A

b. 428 nm

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11
Q

Calculate the minimum wavelength of light necessary to overcome the work functions for Ge (phi = 5eV)

a. 248 nm
b. 428 nm
c. 575 nm
d. 581 nm

A

a. 248 nm

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12
Q

It states that no two atoms will have the same set of quantum numbers.

a. Heisenberg Uncertainty Principle
b. Pauli’s Exclusion Principle
c. Aufau Building Up Principle
d. Hund’s Rule of Multiplicity

A

b. Pauli’s Exclusion Principle

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13
Q

What is the speed of an electron being emitted by Rb (phi = 2.16eV) when 350 nm of light shined on the metal in the vacuum?

a. 1.87 x 10 ^ 5 m/s
b. 4.60 x 10 ^ 5 m/s
c. 7.00 x 10 ^ 5 m/s
d. 9.94 x 10 ^ 5 m/s

A

c. 7.00 x 10 ^ 5 m/s

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14
Q

What is the maximum number of electrons in an atom that can have the quantum number: n = 2, ms = - 1/2 ?

a. 8
b. 6
c. 1
d. 4

A

d. 4

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15
Q

The atomic weight of chlorine is 35.45 and its naturally occurring isotopes are Cl-35 and Cl-37. What is the percentage abundance of Cl-35?

a. 95.8%
b. 98.7%
c. 77.5%
d. 75.0%

A

c. 77.5%

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16
Q

Which of the following properties do not depend on the electronic configuration of the atoms?

a. physical
b. chemical
c. nuclear
d. none of the above

A

c. nuclear

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17
Q

Which of the following sets of quantum numbers is incorrect?

a. n = 1, l = 0, ml = - 1, ms = - 1/2
c. n = 3, l = 1, ml = 0, ms = - 1/2
b. n = 1, l = 0, ml = 0, m, = 1/2
d. n = 4, l = 2, ml = - 1, ms = 1/2

A

a. n = 1, l = 0, ml = - 1, ms = - 1/2

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18
Q

In what group of the periodic table is the element with the following electron configuration? [Ar] 4s^2 3d^10 4p^3

a. 1A
b. 2A
c. 3A
d. 5A

A

d. 5A

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19
Q

Which of the following pairs are isoelectronic?

a. Mn^+2 and Ar
b. Zn^+2 and Cu^+2
c. S^-2 and Cl^-1
d. Na^+ and Cl^-1

A

c. S^-2 and Cl^-1

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20
Q

The change in energy when an electron is accepted by a gaseous atom to form an anion.

a. Electronegativity
b. Electron Affinity
c. Ionization Energy
d. Activation Energy

A

b. Electron Affinity

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21
Q

Which of the following halogens is the most electronegative?

a. F
b. Cl
c. Br
d. I

22
Q

Among the members of the Chalcogen Family, which is the most non-metallic?

a. Sulfur
b. Selenium
c. Tellurium
d. Oxygen

23
Q

Arrange the following in increasing ionization energy:
C-1
Na-2
Mg-3
B-4
N-5
a. 41532
b. 51432
c. 23415
d. 23514

24
Q

The theory that states that bonding is caused by overlapping of two atomic orbitals.

a. Valence Bond Theory
b. Molecular Orbital Theory
c. Vital Force Theory
d. Valence Shell Electron-Pair Repulsion

A

a. Valence Bond Theory

25
Q

It pertains to single bond, double bond, triple bond and those intermediate between single and double bonds, etc.

a. Bond Order
b. Bond Length
c. Bond Strength
d. Bond Degree

A

a. Bond Order

26
Q

Which of the following molecules/compounds is formed by covalent bonds?

a. LiF
b. MgO
c. ZnS
d. BeCl2

27
Q

A compound whose molecules are not associated by hydrogen bonding is

a. CH3CH2OH
b. (CH3)2NH
c. HCOOH
d. (CH3)3COCH3

A

d. (CH3)3COCH3

28
Q

Type of equilibrium that exists between similar phases is called

a. physical equilibria
b. homogeneous equilibria
c. chemical equilibria
d. heterogeneous equilibria

A

b. homogeneous equilibria

29
Q

Which of the following equilibrium system will have its Kp equal to its Kc?’

a. 2NO(g) + Br2(g) = 2NOBr(g)
b.CO(g) + Cl2(g) = COCl2(g)
c. H2(g) + l2(g) = 2HI(g)
d. N2(g) +3H2(g) = 2NH3(g)

A

c. H2(g) + l2(g) = 2HI(g)

30
Q

Consider the reaction: PCl5(g) = PCl3(g) + Cl2(g) (Hrxn = 87.9 kj/mol)
Which of the following will result in the increase in concentration of Cl2 gas?

a. add PCl3
b. cool the mixture
c. add PCl5
d. increase the pressure

A

c. add PCl5

31
Q

Consider the following reaction at 1600 C: Br2(g) = 2Br(g). When 1.05 moles of Br2 are placed in a 2 L flask, 2.50% of Br2 undergoes dissociation. Calculate the Kp for the reaction.

a. 0.20689
b. 0.001346
c. 3.7216
d. 0.0953

A

a. 0.20689

32
Q

NaCIO2 is

a. sodium chloride
b. sodium hypochlorite
c. sodium chlorite
d. sodium chlorate

A

c. sodium chlorite

33
Q

oxalic acid + sodium hydroxide = ______

a. Na2CO3
b. NaC2H3O2
c. NaCHO
d. Na2C2O4

A

d. Na2C2O4

34
Q

Which of the following is an acidic oxide?

a. MgO
b. SO2
c. Na2O
d. CaO

35
Q

Which of the following substances in aqueous solution of the same concentration will have the highest boiling point elevation?

a. KCI
b. Na2SO4
C. CH3COOH
d. NaCl

36
Q

The vapor pressure of water at 25 C is 23.756 torr. A solution consisting of 18.913 grams of a non-volatile substance in 36 grams of water has a vapor pressure of 20.324 torr. What is the molecular weight of the solute?

a 62
b. 56
c. 48
d. 39

37
Q

What is the freezing point of a 30% wt urea, (NH)2CO solution in water?

a. -13.29 C
b. -16.45 C
c. -9.18 C
d. -11.77 C

A

a. -13.29 C

38
Q

What would be the freezing point of a 0.205 molal solution with respect to urea (60) g/mol) when 200 grams of this solution is diluted with 250 grams of water?

a. -0.168 C
b. -0.172 C
c. -0.174 C
d. -0.176 C

A

a. -0.168 C

39
Q

The osmetic pressure of a dilute aqueous ethyl alcohol solution at 25°C is 38 mmHg Calculate the boiling point elevation of this solution.

a. 0.0038 C
b. 0.0025 C
c. 0.0041 C
d. 0.0011 C

A

d. 0.0011 C

40
Q

Ra-226 decays by alpha emission. What is its decay product?

a. 228 87 Fr
b. 227 86 Rn
c. 230 90 Th
d. 226 89 Ac

A

b. 227 86 Rn

41
Q

The half-life of 90Sr is 29 years. What fraction of the atoms in a sample of 90Sr would remain 100 years later?

a. 0.29
b. 0.14
c. 0.18
d. 0.09

42
Q

A sample of radioactive material was found to be 90% disintegrated after 50 years. What is the half-life of the material?

a. 7.5 yrs
b. 8.7 yrs
c. 15.1 yrs
d. 22.2 yrs

A

c. 15.1 yrs

43
Q

Radium-226, which undergoes alpha decay, has a half-life of 1600 years. How many alpha particles are emitted in 10 min by 10 mg sample of radium-226?
Assume one year to have 365 days.

a. 1.1 x 10^11
b. 2.2 x 10^11
c. 3.3 x 10^11
d. 4.4 x 10^11

A

b. 2.2 x 10^11

44
Q

Radium-226, which undergoes alpha decay, has a half-life of 1600 years. What is the activity of the sample in mCi? ( 1Ci = 3.7 * 10 ^ 10 disintegration/s)

a. 7.9 mCi
b. 8.9 mCi
c. 9.9 mCi
d. 10.9 mCi

A

c. 9.9 mCi

45
Q

If (238 92 U) undergoes decay and found to produce (234 90 Bi) what other particle was emitted?

a. alpha
b. gamma
c. positron
d. electron

46
Q

Potassium-40 decays to argon-40 with a half-life of 1.27 x 10^9 years. What is the age of the rock in which the mass ratio of 40 Ar to 40 K is 4?

a. 1.4 * 10 ^ 9 years
b. 2.9 * 10 ^ 9 years
c. 4.2 * 10 ^ 9 years
d. None of these

A

b. 2.9 * 10 ^ 9 years

47
Q

It is equivalent to the rate of disintegration of 1 gram of radium

a. becquerels
b. curie
c. gray
d. rem

48
Q

Which of the following particles cannot be accelerated in a particle accelerator?

a. alpha
b. electron
c. neutron
d. proton

A

c. neutron

49
Q

What is the binding energy per nucleon for C-13 (13.003355 amu) in MeV?

a. 4.5
b. 5.5
c. 6.5
d. 7.5

50
Q

Starting with 1.000 gram of Sr-90, 0.953 gram will remain after 2 years. Calculate the initial activity of Sr-90 in Ci? 1 Curie (Ci) = 3.7 x 10^10 disintegration/sec

a. 70
b. 140
c. 210
d. 280

CI (8 decks)

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