General Chemistry 1, In Class Quizzes

(Chapter 1) Perform the following calculation and report the answer to the correct number of significant figures.

 

0.0042

(Chapter 1) A graduated cylinder is filled with water to the 25.0 mL mark. After 27.5 g of titanium dioxide (TiO2) is added, the volume is 31.5 mL. Calculate the density of TiO2.

4.2 g/cm3

(Chapter 1) What value should be reported as the volume of a strip of aluminum foil measuring

15.37 cm x 42.5 cm x 0.0010 cm?

0.65 cm3

(Chapter 1) Which of the following is a chemical property of copper (Cu) metal?

It reacts with nitric acid (HNO3) to produce copper(II) nitrate (Cu(NO3)2).

It melts at 1085°C

It has an orange color

It conducts electricity

It reacts with nitric acid (HNO3) to produce copper(II) nitrate (Cu(NO3)2).

Which of the following is NOT a pure substance?

dry ice (solid CO2)

gold metal

sparkling water

water vapor

Sparkling water

A molecule ________

can be an element or a compound

contain only one atom.

must contain at least two types of atoms

cannot form a solid.

can be an element or a compound

Which of the following is a heterogeneous mixture?

sweet tea

mercury metal

concrete

black coffee

concrete

(Chapter ) If you had equal masses of each of the following substances, which would occupy the greatest volume?

 

aluminum (d = 2.70 g/mL)

 

cocoa butter (d = 0.910 g/mL)

 

beeswax (d = 0.960 g/mL)

 

ice (d = 0.917 g/mL)

cocoa butter (d = 0.910 g/mL)

A ₈¹⁶O^2- ion has ________ protons, ________ neutrons, and ________ electrons.

 

 

8; 8; 10

If the nucleus of an atom had a diameter of 1 cm (roughly that of a dime), what would be the approximate diameter of the atom? The radius of the nucleus is approximately 10,000 times smaller than the radius of an atom.

 

100m

In J. J. Thomson's cathode ray experiment, what are cathode rays?

 

protons

 

neutrons

 

alpha particles

 

electrons

electrons

Which subatomic particles have opposite charges?

 

neutrons and electrons

 

protons and electrons

 

protons and alpha particles

 

protons and neutrons

protons and electrons

What is the symbol for potassium?

 

P

 

Po

 

Sb

 

K

K

A strontium-90 atom that has lost 2 electrons has ________ protons, ________ neutrons, and ________ electrons.

 

38; 52; 36

Gallium has two naturally occurring isotopes with the following masses and natural abundances. Calculate the average atomic mass of Ga.

                                    ⁶⁹Ga      68.9256 amu       60.108%

                                    ⁷¹Ga      70.9247 amu       39.892%

 

69.723 amu

Cyanidin chloride (C₁₅H₁₁O₆Cl, 322.7 g/mol) contains the cyanidin ion, a pigment found in many berries. Calculate the number of moles of cyanidin chloride equivalent to 7.2 mg.

 

2.2 X 10^-5 mol

How many grams of water (18.02 g/mol) would contain 6.54 x 10²⁴ hydrogen atoms?

97.9 g

Calculate the number of hydrogen atoms in 0.25 mol of strychnine, C₂₁H₂₂N₂O₂.

 

3.3 x 10²⁴ atoms

What is the wavelength (Lamina, in meters) of a radio station operating at a frequency of 99.6 MHz?

 

mega = 10⁶

1Hz = sec^-1

1 m = 10⁹ nm

speed of light = 2.998 x 10⁸ m/s

 

3.01m

The energy of a 500 nm photon is 4 x 10^-19 J. What is the energy of a 250 nm photon?

 

8 x 10^-19 J

Mercury lamps emit blue light with wavelength of 436 nm. What is the energy of these photons in joules?

light speed = 2.998 x 10⁸ m/s

h = 6.626 x 10^-34 J. s.

 

4.56 x 10^-19 J

Which transition in a hydrogen atom will cause emission of the shortest wavelength photon?

 

n_initial = 3 to n_final = 2

 

n_initial = 5 to n_final = 3

 

n_initial = 4 to n_final = 3

 

n_initial = 3 to n_final = 1

n_initial = 3 to n_final = 1

What is the change in energy of the hydrogen atom when it undergoes an electronic transition from n_initial = 5 to n_final = 2?

E =

, Z = atomic number

 

4.57 x 10^-19 J

Determine the wavelength of the line in the hydrogen atomic emission spectrum corresponding to the n_initial = 4 to n_final = 3 transition.

 

 

1875nm

What is the orbital designation for an electron with the quantum numbers n = 3, l = 2?

 

3d

Which of the following are NOT valid sets of quantum numbers

               n           l            m_l           m_s

  A        3          2          1          –½

  B        3          1          2          +½

  C        2          1          –1        +½

   D       4          3           0         –½

 

B

Which of the following is NOT an allowed value for the principal quantum number?

 

0

 

1

 

3

 

2

0

Which of the following is the correct electron configuration for copper?

 

1s²2s²2p⁶3s²3p⁶4s¹3d¹⁰

Which set of quantum numbers could be correct for the highest energy electron in tin, Sn?

 

n = 5, l = 2, m_l = 0, m_s = +½

 

n = 5, l = 1, m_l = 0, m_s = ½

 

n = 4, l = 1, m_l = -1, m_s = -½

 

n = 5, l = 0, m_l = 0, m_s = -½

n = 5, l = 1, m_l = 0, m_s = ½

Which row 2 element probably has the following successive ionization energies:

       IE₁, 1314            IE₂, 3389              IE₃, 5298                IE₄, 7471

       IE₅, 10,992         IE₆, 13,329            IE₇, 71,345           IE₈, 84,087

 

O

Which arrangement is correct for increasing atomic radius?

 

Rb < K < Li

 

Sc < Ge < Br

 

C < N < F

 

Se < Cu < Ca

Se < Cu < Ca

Which of the following species is NOT isoelectronic to the others?

 

Cl^-

 

P^3-

 

Sc³⁺

 

Mg²⁺

Mg²⁺

Which of the following atoms has NO unpaired electrons?

 

Zn

 

Cr

 

Se

 

Sn

Zn

Which compound below is molecular (covalent)?

 

SF₄

 

K₂S

 

AlCl₃

 

BaF₂

SF₄

What would be the ionic compound formula between Na and N atoms?

 

NaN₃

 

Na₂N₃

 

Na₂N₂

 

Na₃N

Na₃N

What is the formula for potassium oxide?

 

P₂O

 

PO

 

K₂O

 

PO₂

K₂O

Which formula-name combinations below is NOT correct?

a.	chlorine monoxide: ClO	c.	dichlorine monoxide: Cl2O
b.	chlorine dioxide: ClO2	d.	chlorine hexoxide: Cl2O6

 

d

The proper name for Cr₂S₃ is ________

 

chromium(III) sulfide

How many valence electrons does antimony have?

 

5

Which Lewis symbol below is correct?

 

d.

In which bond does the Cl atom have the highest electron density?

 

Br-Cl

 

N-Cl

 

O-Cl

 

H-Cl

H-Cl

How many shared electron pairs are there in the Lewis structure of OF₂?

 

2

How many non-bonding electron pairs are there in the Lewis structure of HCN?

 

4

1

What is the bond order of the carbon–oxygen bond in COF₂?

 

2

Nitrite (NO₂^-) is an important nutrient in the eutrophic zone of the ocean. Which set of resonance structures below best describes the bonding in this ion?

 

a

What is the approximate nitrogen–oxygen bond order in NO₂^- ion?

 

1.33

What is the formal charge on the terminal nitrogen atom in the best Lewis structure for dinitrogen sulfide (N₂S)?

 

-1

Which molecule below contains a central atom with an expanded octet?

 

PF₃

 

AsCl₅

 

N₂O

 

BF₃

AsCl₅

Which molecule below contains an exception to the octet rule?

 

PCl₃

 

NO₂

 

CO₂

 

CCl₄

NO₂

From the below, identify the molecule or ion with large CO bond length.

CO, CO₂, CO₃^2-

 

CO₃^2-

Which molecule below is a hypovalent?

 

N₂O

 

BF₃

 

AsCl₅

 

PF₃

BF₃

What is the steric number of the central phosphorus atom in PF₃?

 

4

What is the hybridization of the central atom of SCN^-?

 

sp

What is the hybridization of selenium in SeCl₄?

 

sp³d

What are the ideal bond angles around a central atom with a steric number of 3?

 

all 120°

What is the electron pair geometry of the triiodide ion (I₃^-)?

 

trigonal bipyramidal

Which molecule or ion below is linear?

 

IBr₂^-

 

H₂S

 

H₂Se

 

SO₂

IBr₂^-

For which one of the following molecules (BF₃, CF₄, NF₃, OF₂) is the electron pair geometry tetrahedral and the molecular geometry triangular pyramidal?

 

NF₃

What is the hybridization of the central iodine atom in I₃⁺?

 

sp³

Which molecule below is NOT polar?

 

CS₂

 

SO₂

 

N₂O

 

H₂O

CS₂

Which molecule below is polar?

 

CF₄

 

SiH₄

 

BF₃

 

CH₂Cl₂

CH₂Cl₂

Which diagram below shows the correct orientation of the dipole in sulfur dioxide?

a.

b.

c.

d.

 

a.

Cryolite %composition is the following:

%Al = 12.85

%Na = 32.85

%F = 54.30

What is the empirical formula?

AlNa₃F₆

Metallic chromium can be obtained from the mineral chromite (FeCr₂O₄). What is the mass percent of chromium in chromite?

 

46.46% (Chrom)

Ibuprofen is 75.69% C, 8.80% H, and 15.51% O by mass. What is its empirical formula?

 

C₁₃H₁₈O₂

Which of the following does NOT share the same empirical formula as the others?

 

lactic acid, CH₃CH(OH)COOH

 

acetic acid, CH₃COOH

 

butyric acid, CH₃CH₂CH₂COOH

 

glucose, C₆H₁₂O₆

butyric acid, CH₃CH₂CH₂COOH

Phthalocyanine is a large molecule used in printing inks and dyes. Elemental analysis showed that it consists of 74.69% C, 3.525% H, and 21.77 % N and has a molar mass of 514.54 g/mol. What is its molecular formula?

 

C₃₂H₁₈N₈

How many grams of aluminum nitrate (Molar mass = 213.00 g/mol) are required to make 500.0 mL of a 0.0525 M aqueous solution?

 

5.59 g

If 0.10 L of 3.0 M sucrose solution were diluted to 250 mL, what would the concentration be?

1.2M

How many grams of solid potassium chlorate (KClO₃) are needed to make 150 mL of 0.50 M solution?

9.2 g

How many moles of nitrate ions are present in exactly 275 mL of a 1.25 M copper(II) nitrate solution, Cu(NO₃)₂(aq)?

0.688 mol

If 75.0 mL of a 0.20 M solution of sodium nitrate (NaNO₃) is mixed with 25.0 mL of 0.10 M barium nitrate (Ba(NO₃)₂), what is the molar concentration of nitrate in the resulting solution?

0.20 M

Identify the set of stoichiometric coefficients (in the order of C₈H₁₈, O₂, CO₂, H₂O) that balance the reaction equation for the combustion of octane.

C₈H₁₈ (l) + O₂ (g) --> CO₂ (g) + H₂O (l)

 

2, 25, 16, 18

How many grams of CO₂ would result from the complete combustion of 4.00 mol butane (C₄H₁₀)?

 

704g

Hydrogen peroxide decomposes to produce water and oxygen. Which relationship regarding the quantities of reactants and products associated with this reaction is NOT correct?

 

2 mol   2 mol +  1 mol

 

2g —> 2g + 1g

 

68.0 g  36.0 g  + 32.0 g

 

2 molecules 2 molecules +  1 molecule

2g —> 2g + 1g

What is the formula of the precipitate that forms when aqueous Fe(NO₃)₃ and aqueous Na₂CO₃ are mixed?

Fe₂(CO₃)_{3 (Precipitate)}

Write the net ionic equation for the reaction that takes place between aqueous magnesium chloride and aqueous sodium hydroxide.

 

 

 

 

Identify the acid in the following acid–base reaction.

H₂PO₄^-

Select the net ionic equation for the reaction of rubidium hydroxide with nitric acid.

d (Net ionic)

When the oxidation–reduction reaction shown here is balanced using the smallest whole-number coefficients, how many electrons are transferred?

 

Sn(s) + Cl₂ (g) —> SnCl₄ (s)

 

4

What is the oxidizing agent in the following reaction?

2N₂H₄ (l) + N₂O₄ (l) ----> 3 N₂ (g) + 4 H₂O (g)

N₂O₄

In its reaction with water, ammonia (NH₃)

 

acts as an acid

 

acts neither as an acid nor as a base

 

serves as both an acid and as a base

 

acts as a base

acts as a base

In which compound does iodine have an oxidation number of +3?

 

HIO3

 

HIO

 

HIO4

 

HIO₂

HIO₂

Balance the following redox reaction under acidic aqueous conditions using the smallest whole-number coefficients possible. What is the coefficient of HSO₃^-?

5

Balance the following redox reaction under acidic aqueous conditions using the smallest whole-number coefficients possible. On which side does H₂O(l) appear, and what is its coefficient?

right; 8

Water can be separated into its elements according to the following equation by electrolysis. If 20.0 g of water is decomposed by this method, how much oxygen gas is produced?

17.8g

Assuming complete combustion, how many grams of butane (C₄H₁₀) would be required to consume 32.0 g O₂?

8.94g

Which of the following should have the highest conductivity?

 

Conductivity [total ion], [ ] represents concentration

 

2.4 M CaCl₂

 

3.0 M NaCl

 

2.1 M Na₃PO₄

 

3.2 M NH₄NO₃

2.1 M Na₃PO₄

Calcium hydroxide is slightly soluble in water. About 1 gram will dissolve in 1 liter. What are the spectator ions in the reaction of such a dilute solution of calcium hydroxide with hydrochloric acid?

 

 

 

 

Hard water, which contains  and  ions, tends to form a ring in a bathtub due to its reaction with the soluble anions in soap. The formation of this insoluble material is an example of

 

a redox reaction

 

an acid–base reaction

 

a combustion reaction

 

a precipitation reaction

a precipitation reaction

Which of the following ionic compounds is insoluble in water?

 

KCl

 

Cu₃(PO₄)₂

 

AgNO₃

 

FeCl₃

FeCl₃

In the following reactions, which species is oxidized?

 

Cu

 

S

 

Fe

 

O

Cu

An organic acid with a molar mass of 228 g/mol, is composed of carbon, hydrogen, and oxygen. Analysis of a 10.000 g sample yielded 6.314 g C and 0.883 g H. What is its molecular formula?

 

C₁₂H₂₀O₄

 

16.7g

How many moles of chlorine are in 25.0 g of calcium chloride (CaCl₂)?

 

0.451 mol

What mass of phosphoric acid (H₃PO₄) is produced from the reaction of 10.00 g of P₄O₁₀ with 6.00 g water?

13.8 g

A mass of 11.60 g of phosphoric acid (H₃PO₄) was produced from the reaction of 10.00 g of P₄O₁₀  with 6.00 g water. What was the percent yield for this reaction?

84.00%

How many mL of 0.116 M Ba(OH)₂ are required to completely neutralize 150.0 mL of 0.280 M HNO₃?

181 mL

A 25.00 mL sample of H₂SO₄ requires 31.43 mL of 0.110 M NaOH to reach the equivalence point. What is the molarity of the H₂SO₄?

0.0692 M

How many grams of iron(III) hydroxide (106.87 g/mol) will precipitate if excess iron(III) nitrate is added to 0.850 L of 1.26 M sodium hydroxide?

38.2 g