Multiple Choice by chapter
Supplemental Instruction
IowaStateUniversity / Leader: / Sara
Course: / Chem 177
Instructor: / Kingston
Date: / December 15, 2014

1.1)Which of the following is a physical change?

I.H2O (s)  H2O (l)

II.CH4 (s) + O2 (g)  H2O (g) + CO2 (g)

III.NaCl (s)  Na+(aq) + Cl- (aq)

IV.C6H12O6 (s) + H2O (l)  C6H12O6 (aq) + H2O (l)

  1. I only
  2. III only
  3. I and III
  4. I and IV
  5. I, III and, IV
  6. All of the above

1.2)What is NOT a Pure substance?

  1. Nickel
  2. Brass
  3. Nitrogen
  4. C6H12O6

1.3)Which would have the lowest density?

  1. Water
  2. Alcohol with a density of .79 g/mL
  3. 10.3 mL of an oil that has a mass of 13.3 g
  4. Not enough information

1.4)Convert the following measurement to scientific notation: 101,000 grams

  1. 1.01000 x 10-5 g
  2. 1.0100 x 10-5 g
  3. 10.1 x 104 g
  4. 1.01 x 105 g

1.5)Solve: 345.009 g - 23.009 g =?

  1. 322 g
  2. 322
  3. 322.00 g
  4. 322.000 g
  5. 3.22 * 102 g

2.1)What is the name of HBrO

  1. Hydrobromic acid
  2. Hypobromous acid
  3. Bromic acid
  4. Perbromic acid

2.2)If there are 2 isotopes of carbon and three isotopes of oxygen, how many lines of a mass spectrometry would Carbon monoxide give?

  1. 3
  2. 4
  3. 5
  4. 6

2.3)What is the formula of the compound arsenic (III) oxide?

  1. As2O3
  2. Ar3O
  3. AsO3
  4. Ar2O3
  5. ArO3

2.4)How many electrons are there in S2-?

  1. 14
  2. 16
  3. 17
  4. 18
  5. 32

2.5)What is the element that has 38 protons, 37 electrons, and 40 neutrons?

  1. Rb
  2. Sr
  3. Y
  4. Zr

2.6)Which of the following is a cation of antimony?

  1. Te+
  2. Sb+
  3. Sn+
  4. Te-
  5. Sb-
  6. Sn-

3.1)A compound contains 6.0 grams of carbon and 1.0 grams of hydrogen, and the molecular weght is 140 grams/mol. What is the molecular formula for the compound?

  1. C10H20
  2. C2H5
  3. CH2
  4. C11H8
  5. C6H12

3.2)In the combustion of C3H7OH, how many moles of oxygen are needed to combust 2 moles of C3H7OH?

  1. 4.5
  2. 5
  3. 7
  4. 9
  5. 11

3.3)If you want to balance the final equation, what is the sum of the coefficients:

___Al2(SO3)3 + ___NaOH ___Na2SO3 + ___Al(OH)3

  1. 10
  2. 11
  3. 12
  4. 13
  5. 14

3.4)In the production of Potassium Oxide from solid potassium and gaseous oxygen, how many atoms of Potassium are needed to react with 4.0 moles of gaseous Oxygen?

  1. 4.0 molecules
  2. 8.0 molecules
  3. 2.4 *1024 molecules
  4. 4.8 *1024 molecules
  5. 9.6 *1024 molecules

For the next three questions use the following scenario:CuCl2 + 2 NaNO3Cu(NO3)2 + 2NaCl

3.5)If 15.0 grams of copper (II) chloride (Μ= 134.5 g/mol) reacts with 20.0 grams of sodium nitrate (Μ= 85.0 g/mol), what is the limiting reagent?

  1. Sodium Chloride
  2. Copper (II) chloride
  3. Copper (II) nitrate
  4. None of the above

3.6)How much sodium chloride (Μ= 58.4 g/mol) will be produced

  1. 6.5 g
  2. 13.7 g
  3. 13.0 g
  4. 27.4 g

3.7)In lab 6.1 grams of sodium chloride is produced, what is the percent yield?

  1. 93%
  2. 45%
  3. 47%
  4. 22%

4.1)Which of the following ionic hydroxides is a soluble base?

  1. Fe(OH)2
  2. Fe(OH)3
  3. Sr(OH)2
  4. Al(OH)3

4.2)Which are strong electrolytes?

I.K2CO3

II.HNO3

III.H2SO4

IV.CuCO3

  1. II only
  2. I and II
  3. I and IV
  4. II, III, and IV
  5. III and IV
  6. I, II and III

4.3)What is (are) the spectator ion(s) in the following reaction:

2HClO3(aq) + Sr(OH)2(aq) → Sr(ClO3)2(aq) + 2H2O(l)

  1. H+,OH-
  2. Sr2+,ClO3-
  3. Sr2+,OH-
  4. OH-

4.4)What is the mass of Potassium (M=39.1 g/mol) contained in 40. mL of a 3.0 M solution of KCl?

  1. 8.9 g
  2. 4.7 g
  3. 4.26 g
  4. 9.0 g

4.5)The total concentration of ions in a 0.250 M solution of H2SO4 is:

  1. 0.250 M
  2. 0.500 M
  3. 0.750 M
  4. 1.00 M
  5. 1.75 M

4.6)Calculate the newmolarityif 275.0 mL of water is added to 25.0 mL of a 2.40 M HCl solution.

  1. 0.200 M
  2. 0.218 M
  3. 2.18 M
  4. 0.400 M

4.7)A 31.5 mL aliquot of a diprotic acid of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration of the acid was______.

  1. 0.0102 M
  2. 0.00508 M
  3. 0.0204
  4. 0.102

5.1)The internal energy of a system is always increased by ____.

  1. Adding heat to the system
  2. Having the system to work on the surroundings
  3. Withdrawing heat from the system
  4. Adding heat to the system and having they system do work on the surroundings
  5. A volume compression
  6. The heat of combustion for one mole of carbon to carbon dioxide is -410 kJ. How many kJ of heat would be liberated from the complete combustion of 60.0 g carbon?

  1. -82 kJ
  2. -2050 kJ
  3. -24,600 kJ
  4. -32,000 kJ

5.3)Water has a specific heat of 4.184 J/g deg while glass (Pyrex) has a specific heat of 0.780 J/g deg. If 10.0 J of heat is added to 1.00 g of each of these, which will experience the larger increase of temperature?

  1. Glass
  2. Water
  3. They both will experience the same change is temperature
  4. Given the following data at 1 atm of pressure and 25.0oC...

DHoformation= +64.4 kJ/mole for Cu2+

DHoformation= -152.4 kJ/mole for Zn2+

Calculate the standard heat of reaction: Zn(s)+Cu2+(aq)Zn2+(aq) + Cu(s)

  1. -217 kJ/mol
  2. +217 kJ/mol
  3. -88.0 kJ/mol
  4. +88.0 kJ/mol

5.5)For the above reaction, what is being reduced?

  1. Solid Zinc
  2. Copper ion
  3. Zinc ion
  4. Copper solid

5.6)100.0 grams of water was placed in a simple, constant-pressure calorimeter. The temperature of the water was recorded as 295.0 K. A 20.0 gram copper bloc heated to 353.0 K and then dropped into the water in the calorimeter. What was the final temperature of the water if the specific heat capacity of water and copper are4.18 and 0.385 J K-1 g-1, respectively?

  1. 296.0 K
  2. 293.9 K
  3. 28.3 K
  4. 307.2

6.1) Electromagnetic radiation travels through vacuum at a speed of ______m/s.

  1. 186,000
  2. 125
  3. 3.00*108
  4. 10,000
  5. It depends on wavelength

6.2)Helium can be ionized by losing one electrons to become the He+ cation. The line spectrum of this cation will resemble the line spectrum of

  1. A hydrogen atom
  2. A lithium atoms
  3. A lithium cation
  4. A helium atom, nothing changed

6.3)A mole of yellow photons of wavelength 527 nm has ______kJ of energy.

  1. 165
  2. 227
  3. 4.56*10-46
  4. 6.05*10-3
  5. 2.74*10-19

6.4)What color of visible light has the longest wavelength?

  1. Blue
  2. Violet
  3. Red
  4. Yellow
  5. Green

6.5)Of the following transitions in the Bohr hydrogen atom, which transition results in the emission of the highest-energy proton?

  1. n=1  n=6
  2. n=6  n=1
  3. n=6  n=3
  4. n=3  n=6

6.6)The total number or orbitals in a shell is given by _____.

  1. I2
  2. n2
  3. 2n
  4. 2n+1
  5. 2l+1

6.7)The n=1 shell contains ____ p orbitals. All other shells contain _____ p orbitals.

  1. 3,6
  2. 0,3
  3. 3,3
  4. 0,6

6.8)The elements in what period have the same core-electron configuration as neon’s electron configuration

  1. First
  2. Second
  3. Third
  4. Fourth

7.1)The size of an element’s atomic radius ______from left to right across the periodic table.

  1. Increases
  2. Decreases
  3. Remains constant
  4. Is random

7.2)Arrange the following elements from lowest to highest ionization energy: Be, Mg, Ca, Rb, Sr

  1. Be, Mg, Ca, Rb, Sr
  2. Rb, Sr, Ca, Be, Mg
  3. Rb, Sr, Ca, Mg, Be
  4. Be, Mg, Ca, Sr, Rb

7.3)The alkali metals tend to form anions because….

  1. They have low first ionization energies
  2. They have low electron affinities
  3. They have high electron affinities
  4. They don’t; they form cations
  5. Electon affinity…
  1. Is always positive
  2. May be positive or negative
  3. Is always negative
  4. Is typically higher in metals than nonmentals
  5. Which of the following statements about the general valence electron configuration of ns2np5 and are true?

(i)Elements with this electron configuration are expected to form -1 anions

(ii)Element with this electron configuration are expected to have large positive electron affinities

(iii)Elements with the electron configuration are nonmetals

(iv)Elements with this electron configuration form acidic ocides

  1. (i) and (ii)
  2. (i), (ii), and (iii)
  3. (ii) and (iii)
  4. (i),(iii), and (iv)
  5. All statements are true

7.6)The electron affinity of chlorine is -349 kJ/mol. What is the correct equation for the formation of chloride?

  1. Cl (s) + e- → Cl- (s) + 349 kJ
  2. Cl (g) + e- → Cl- (g) + 349 kJ
  3. Cl (s) + 349 kJ + e- → Cl- (s)
  4. Cl (g) + 349 kJ + e- → Cl- (g)

7.7)What is true of the oxide formed when magnesium reacts with oxygen

  1. Its formula is Mg2O
  2. It is acidic
  3. It is basic
  4. It is atmospheric

7.8)An electron in a ____ subshell experiences the greatest Zeff in a many-electron atoms

  1. 3f
  2. 3p
  3. 3d
  4. 3s
  5. 4s
  6. 4d

7.9)In general, as you go across a period in the periodic table from left to right: The atomic radius _____; the electron affinity becomes ______negative; and the first ionization energy ______.

  1. Decreases, decreasingly, increases
  2. Increases, increasingly, decreases
  3. Increases, increasingly, increases
  4. Decreases, increasingly, increases

89.1)The C2 molecule has 6 bonding and 2 antibondinge-. What’s the bond order?

  1. -2
  2. -1
  3. 0
  4. 1
  5. 2

89.2)Constructive overlap of atomic orbitals give:

  1. Antibonding molecular orbitals
  2. Hybrid orbitals
  3. Other atomic orbitals
  4. Bonding molecularorbitals
  5. Resonant structures

89.3)A polar bond between two atoms is best described as

  1. Equal sharing of electrons
  2. Between H and O
  3. Induced charge
  4. Unequal sharing of electrons
  5. Transferring of electrons

89.4)The molecule of NH4+ is best described as…

  1. Linear
  2. Planar
  3. Three-dimensional
  4. ionic

89.5)Which of the following molecules does not have resonance forms?

  1. SO2
  2. O3
  3. CH3OH
  4. ClO3-

89.6)Which of the following atoms is most likely to have an incomplete octet?

  1. Li
  2. C
  3. F
  4. N

89.7)In the molecule N2 which of the following statements correctly describe the bonds?

(I)There is one head on bond between two sp orbitals

(II)There are three sigma bonds made from sp orbitals

(III)There are two pi bonds made from sp3orbitals

(IV)There are three pi bonds made from sp orbitals

(V)There are two pi bonds made from p orbitals

  1. (I) only
  2. (II) only
  3. (III) only
  4. (II) and (V)
  5. (II) and (III)
  6. (III) and (IV)
  7. (I) and (III)
  8. (I) and (V)

89.8)Which of the following molecules has a see saw geometry?

  1. NCl3
  2. PF5
  3. NO3-
  4. BrF4+
  5. BrF4-
  6. SiCl4

89.9)Which of the following molecules is the molecular geometry the same as the electron geometry.

(i)PCl3

(ii)CCl4

(iii)TeCl4

(iv)XeF4

(v)SF6

  1. (i) and (ii)
  2. (ii) and (iii)
  3. (ii) and (v)
  4. (iv) and (v)
  5. (v) only

89.10)Of the molecules below only ______is polar

  1. CCl4
  2. CH4
  3. SeF4
  4. SiCl4

10.1)Which of the following is false about gases?

  1. They take the shape of their container
  2. They have the lowest densities
  3. They take the volume of their container
  4. They have the strongest IMF

10.2)Which of the following has the highest density at STP?

  1. Vapor water
  2. Nitrogen gas
  3. Carbon dioxide
  4. Hydrogen gas

10.3)There are two boxes at the same pressure, and each contains the same number of molecules. Box A has twice the volume as the Box B. The smaller box (Box B) has a temperature of 300K. What is the Temperature of Box A?

  1. 300 K
  2. 150 K
  3. 600 K
  4. 450 K

10.4)At the top of mount Everest the atmosphere is .03 molar percent Carbon monoxide. The temperature is negative thirty degrees Celsius, and the pressure is .35 atm. How many carbon monoxide molecules are in 1.0 L of atmosphere.

  1. .018
  2. 1.1 x 1022
  3. 5.3 x 10-6
  4. 3.2 x 1018

10.5)Under conditions of fixed temperature and moles of gas. Boyle’s Law states that:

  1. P1V1 = P2V2
  2. PV = constant
  3. P1/P2 = V2/V1

  1. I only
  2. II only
  3. III only
  4. All the above
  5. None of the above

10.6)Which of the following gases would have the smallest rate of effusion?

  1. CH4
  2. He
  3. N
  4. Ne
  5. CO

10.7)A gas mixture contains 2.0 moles of helium and 8.0 moles of carbon dioxide, and is held under conditions of standard temperature and pressure. What is the partial pressure of carbon dioxide?

  1. 2.0 atm
  2. 0.20 atm
  3. 8.0 atm
  4. 0.80 atm

11.1)The boiling point of a substance is most strongly influenced by:

  1. The molecular weight of a substance
  2. The specific heat of a substance
  3. The melting point
  4. The strength/weakness of the intermolecular forces
  5. The amount of substance involved
  6. Which of the following molecule will have the largest heat of vaporization?

  1. I2
  2. Br2
  3. Cl2
  4. F2
  5. O2

Substance / Molecular Mass (amu) / Dipole Moment (D)
CH3CH2CH3 / 44 / 0.1
CH3OCH3 / 46 / 1.3
CH3Cl / 50 / 1.9
CH3CHO / 44 / 2.7
CH3CN / 41 / 3.9

11.3)Using the table below, predict the substance with the highest boiling point

  1. CH3CH2CH3
  2. CH3OCH3
  3. CH3Cl
  4. CH3CHO
  5. CH3CN
  6. Which of the following exhibits dipole-dipole attractions between molecules?

  1. XeF4
  2. AsH3
  3. CO2
  4. BCl3
  5. Cl2

11.5)What types of IMF exist between a molecule of HF and a molecule of H2S?

  1. Dipole-dipole and ion-dipole
  2. Dispersion forces, dipole-dipole, and ion-dipole
  3. Dispersion forces, hydrogen bonding, dipole-dipole
  4. Dispersion and dipole-dipole
  5. Dispersion forces, dipole-dipole, and ion-dipole