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Chemistry 151 Final

Question 1 of 55

1

A 9.0 g sample of solid sodium bicarbonate completely decomposes into solid sodium hydroxide and carbon dioxide gas when heated. After the sodium hydroxide cools it has a mass of 4.74 g. According to the Law of Conservation of Mass, what mass of carbon dioxide must have been formed?

Select one of the following:

  • a) 4.67 g

  • b) 4.26 g

  • c) 4.3 g

  • d) 13.7 g

  • e) none of the above

Explanation

Question 2 of 55

1

A substance that can only be separated by chemical means is:

Select one of the following:

  • an element

  • a compound

  • either a compound or an element

  • a homogenous mixture

  • a heterogeneous mixture

Explanation

Question 3 of 55

1

Which of the following statement(s) is(are) not correct?

Select one of the following:

  • a) The conversion of compounds into elements is a chemical change.

  • b) The conversion of sugar into carbon and water is a chemical change.

  • c) The conversion of liquid water into gaseous water is a chemical change.

  • d) The conversion of elements into compounds is a chemical change.

  • e) The evaporation of water is a physical change.

  • f) d and e

Explanation

Question 4 of 55

1

Which of the following is a mixture?

Select one of the following:

  • a) sucrose (C12H22O11)

  • b) solder (an alloy made of varying amounts of Sn and Pb)

  • c) the diatomic gas bromine (Br2)

  • d) both a and b

  • e) both b and c

Explanation

Question 5 of 55

1

If the distance between layers of silicon atoms in graphite is given as 823 pm, what is the distance in cm?

Select one of the following:

  • 8.23 x 10^-10

  • 8.23 x 10^-12

  • 8.23 x 10^-7

  • 8.23 x 10^-8

  • 8.23 x 10^-6

Explanation

Question 6 of 55

1

A 0.75 kg sample of methylene chloride has a density of 1.32 x 10^3 mg/cm^3. What is the volume in L of methylene chloride?

Select one of the following:

  • 0.99 L

  • 5.7 L

  • 5.68 x 10^-1 L

  • 5.7 x 10^-1

  • 0.5682 L

Explanation

Question 7 of 55

1

The British physicist who won the Nobel Peace prize in 1906 for the discovery of the electron was:

Select one of the following:

  • Ernest Rutherford

  • JJ Thomson

  • Robert Millikan

  • James Chadwick

Explanation

Question 8 of 55

1

Which statement is not true of the nucleus of an atom?

Select one of the following:

  • a) it contains the neutrons, protons and electrons

  • b) it is at the center of an atom

  • c) its overall charge is positive

  • d) it contains most of the mass of an atom

  • e) both a and d

Explanation

Question 9 of 55

1

The number of protons in a neutral atom of a given element is equal to:

Select one of the following:

  • a) the mass number

  • b) the nuclear number

  • c) the atomic number

  • d) the number of electrons

  • e) both b and c

  • f) both c and d

Explanation

Question 10 of 55

1

How many protons, neutrons and electrons are in the isotope of Ni+2 having a mass number of 57?

Select one of the following:

  • 28p, 29n, 30e-

  • 57p, 29n, 28e-

  • 28p, 29n, 26e-

  • 28p, 57n, 26e-

Explanation

Question 11 of 55

1

The formulas of the phosphate ion, the ammonium ion and the perchlorate ion are represented by:

Select one of the following:

  • PO4-3, NH4+, ClO3-

  • PO3-2, NH3+, ClO2-

  • PO4-3, NH4+, ClO4-

  • PO4-2, NH4+, ClO4-

Explanation

Question 12 of 55

1

The formula for potassium sulfide is:

Select one of the following:

  • KS

  • KS2

  • K2SO4

  • K2S

Explanation

Question 13 of 55

1

How many atoms of Ca are there in 2.11 g of Ca?

Select one of the following:

  • 3.11 x 10^+22

  • 8.75 x 10^-26

  • 1.27 x 10^+24

  • 3.11 x 10^+23

Explanation

Question 14 of 55

1

Which of the following statements is true for acetic acid, C2H4O2?

Select one of the following:

  • 2 mole C2H4O2 contains 2 moles C

  • 3 mole C2H4O2 contains 8 moles H

  • 5 mole C2H4O2 contains 10 moles O

  • 1 mole C2H4O2 contains 1 moles C

Explanation

Question 15 of 55

1

How many grams of oxygen are there in 25 g of Al2O3?

Select one of the following:

  • 1.17 x 10^1 g

  • 12 g

  • 3.9 g

  • 1.2 x 10^25 g

Explanation

Question 16 of 55

1

What is the mass percentage of Cl in 1 mole C14H9Cl5?

Select one of the following:

  • 50.02%

  • 47.42%

  • 10.01%

  • 75.09%

Explanation

Question 17 of 55

1

What is the percent yield of Cu in an experiment if the actual yield is 12.01 g and the theoretical yield is 14.15 g?

Select one of the following:

  • 117.8%

  • 84.87%

  • 2.14%

  • 71.09%

Explanation

Question 18 of 55

1

A soluble molecular compound has the ability to conduct electricity.

Select one of the following:

  • True
  • False

Explanation

Question 19 of 55

1

Which of the following is(are) example(s) of a weak electrolyte?

Select one of the following:

  • a) HCl

  • b) NH3

  • c) KOH

  • d) HCN

  • e) b and c

  • f) b and d

Explanation

Question 20 of 55

1

When AgNO3 reacts with HCl the products are:

Select one of the following:

  • a) H2 (g)

  • b) nitric acid

  • c) AgCl (s)

  • d) AgCl (aq)

  • e) b and c

  • f) b and d

Explanation

Question 21 of 55

1

What is the net ionic equation when HC2H3O2 reacts with NaOH?

Select one of the following:

  • HC2H3O2(aq) + NaOH(aq) -> C2H3O2Na(aq) + H2O(l)

  • H+(aq) + OH-(aq) -> H2O(l)

  • HC2H3O2(aq) + 2OH-(aq) -> C2H3O2-(aq) + 2 H2O(l)

  • HC2H3O2(aq) + OH-(aq) -> C2H3O2-(aq) + H2O(l)

Explanation

Question 22 of 55

1

A Bronsted-Lowry acid/base reaction is best defined as:

Select one of the following:

  • a combination reaction

  • a redox reaction

  • a loss of a proton

  • a proton transfer reaction

Explanation

Question 23 of 55

1

A diprotic acid has ___ acidic protons.

Select one of the following:

  • many

  • 2

  • 3

  • 4

  • d

Explanation

Question 24 of 55

1

The gas formed when Na2S reacts with H2SO4 is:

Select one of the following:

  • SO3

  • SO2

  • H2S

  • Cl2

Explanation

Question 25 of 55

1

What are the oxidation sates of each element in KClO2?

Select one of the following:

  • K=+1, Cl=+5, O=-2

  • K=-1, Cl=+5, O=-2

  • K=+1, Cl=-5, O=-2

  • K=+1, Cl=+5, O=+2

Explanation

Question 26 of 55

1

CuCl2(aq) + Mg(s) -> MgCl2(aq) + Cu(s) is an example of a:

Select one of the following:

  • a) combination reaction

  • b) combustion reaction

  • c) displacement reaction

  • d) redox reaction

  • e) b and d

  • f) c and d

Explanation

Question 27 of 55

1

The kinetic energy of a 151 lb person with a velocity of 2.0 m/s is: (given 1lb=0.4536kg)

Select one of the following:

  • a) 1.4 x 10^2 J

  • b) 1.4 x 10^-2 kgm^2/s^2

  • c) 1.4 x 10^-2 J

  • d) 1.4 x 10^2 kgm^2/s^2

  • e) a and d

  • f) b and c

Explanation

Question 28 of 55

1

Calculate the quantity of heat required (q) to raise the temperature of a 0.103 g sample of Cu by 10.0°C given a specific heat of 0.384 J/g°C.

Select one of the following:

  • 0.0396 J

  • 03.84 J

  • 0.3955 J

  • 0.396 x 10^3 kJ

  • 0.396 J

Explanation

Question 29 of 55

1

Internal energy, U is best defined as:

Select one of the following:

  • the sum of the kinetic and potential energies of all particles making up a substance

  • the total sum of all energies contained within a system

  • positional energy

  • the energy contained within the nucleus of an atom

Explanation

Question 30 of 55

1

What is true of the relationship between the energy, the frequency and the wavelength of light:

Select one of the following:

  • as energy increases, frequency decreases and wavelength decreases

  • as energy decreases, frequency decreases and wavelength decreases

  • as energy increases, frequency increases and wavelength decreases

Explanation

Question 31 of 55

1

When an electron transitions from the n=1 to the n=4 energy level light is emitted.

Select one of the following:

  • True
  • False

Explanation

Question 32 of 55

1

Which transition below best describes the absorption of the longest possible wavelength of light?

Select one of the following:

  • n=1 to n=6

  • n=2 to n=1

  • n=7 to n=8

  • n=8 to n=7

Explanation

Question 33 of 55

1

The value of the principal quantum number is referring to:

Select one of the following:

  • the shape of an atom

  • the energy level of an electron

  • the number of electrons in an atom

  • the size of the electron

Explanation

Question 34 of 55

1

An electron having n=3 and a l=2 must be in the:

Select one of the following:

  • 3p subshell

  • 3d subshell

  • 3s subshell

  • 3f subshell

Explanation

Question 35 of 55

1

A 2p subshell contains how many orbitals?

Select one of the following:

  • 1

  • 2

  • 3

  • 5

Explanation

Question 36 of 55

1

When l=4, n must have a minimum value of :

Select one of the following:

  • 4

  • 5

  • 6

  • 1

Explanation

Question 37 of 55

1

According to the energy order building up principle which statement(s) below is never correct.

Select one of the following:

  • a) 3p fills after 3s

  • b) 4s fills before 3d

  • c) 2s fills after 1s

  • d) 5s fills before 4p

  • e) a and d

  • f) b and d

Explanation

Question 38 of 55

1

Choose the correct statement below in terms of atomic size.

Select one of the following:

  • Te<Ag<Ru<Rb<Cs

  • Ru<Ag<Te<Rb<Cs

  • Cs<Ag<Te<Rb<Cs

  • Cs<Rb<Ru<Ag<Te

Explanation

Question 39 of 55

1

Ionization energy refers to the amount of energy required to add an electron to the valence shell of a gasoline atom.

Select one of the following:

  • True
  • False

Explanation

Question 40 of 55

1

Which species would you expect to have the greatest ionization energy associated with it?

Select one of the following:

  • Al+2

  • Al+1

  • Al

  • Al+3

Explanation

Question 41 of 55

1

How many electrons are shared when the ionic compound MgS2 is formed?

Select one of the following:

  • 0

  • 2

  • 3

  • 1

Explanation

Question 42 of 55

1

Which of the following is correct in terms of ionic radii:

Select one of the following:

  • Te-2<At-1<Cl-<S-2<P-3

  • S-2<Cl-<At-1<P-3<Te-2

  • Cl-<S-2<P-3<Te-2<At-1

  • P-3<Te-2<At-1<Cl-<S-2

Explanation

Question 43 of 55

1

Which of the following would you expect to have the highest melting point?

Select one of the following:

  • BaS

  • LiCl

  • Al2O3

  • MgCl2

Explanation

Question 44 of 55

1

Which noble gas is Ca+2 isoelectronic with?

Select one of the following:

  • Ne

  • Ar

  • Kr

  • Xe

Explanation

Question 45 of 55

1

Which is the most electronegative atom?

Select one of the following:

  • Cl

  • H

  • O

  • F

Explanation

Question 46 of 55

1

Which atoms are most likely to form triple bonds?

Select one of the following:

  • C, N, O and Cl

  • C and P

  • C and O

  • C, N and S

Explanation

Question 47 of 55

1

Which bond is most polar?

Select one of the following:

  • HCl

  • HBr

  • HO

  • HI

Explanation

Question 48 of 55

1

How many resonance Lewis electron dot structures does O3 have?

Select one of the following:

  • 1

  • 2

  • 3

  • 4

Explanation

Question 49 of 55

1

Which bond would require the most energy to break?

Select one of the following:

  • H-C

  • C=C

  • C≡C

  • C-C

Explanation

Question 50 of 55

1

The molecule CO2 is a polar molecule.

Select one of the following:

  • True
  • False

Explanation

Question 51 of 55

1

Which of the following describes the bond angles if a central atom has 5 groups around it?

Select one of the following:

  • 90° and 180°

  • 90°, 120° and 180°

  • 120°

  • 90°

Explanation

Question 52 of 55

1

What is the name of the molecular geometry about the central atom in PCl3?

Select one of the following:

  • trigonal pyramidal

  • tetrahedral

  • bent

  • distorted tetrahedron

Explanation

Question 53 of 55

1

Which of the following is a nonpolar molecule?

Select one of the following:

  • KrF2

  • AsF3

  • SF2

  • CH3F

Explanation

Question 54 of 55

1

What is the hybridization about the Xe atom in XeF4?

Select one of the following:

  • sp3

  • sp

  • sp3d

  • sp3d2

Explanation

Question 55 of 55

1

Which statement below is most accurate with regard to the total number of σ and π bonds in HCOCH3?

Select one of the following:

  • 5 σ and 2 π bonds

  • 7 σ bonds

  • 6 σ and 1 π bonds

  • 1 π bond

Explanation

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