Chem152FinalExamQuestions&KeySpr24 (2).docx Notes

Part 1: Multiple Choice Questions

Which of the following is an example of a scientific law?

A) All matter is composed of small, indestructible particles called atoms.

B) In a chemical reaction, matter is neither created nor destroyed.

C) When a can of soda pop is opened, a fizzing sound is heard.

D) Flammable objects contain phlogiston.E) none of the above

Which of the following is an example of an observation?

A) All matter is composed of small, indestructible particles called atoms.

B) Reactions occur due to the transfer of electrons.

C) When a can of soda pop is opened, a fizzing sound is heard.

D) Flammable objects contain phlogiston.E) none of the above

A sample of wood with a mass of 3.0 grams was burned in an open dish. The ashes weighed 1.2 grams. What happened to the rest of the wood?

A) The remaining mass was destroyed.

B) The remaining 1.8 grams was converted into gaseous compounds.

C) Nothing, the burned wood simply has a mass of 1.2 grams.

D) The remaining 1.8 grams was converted into heat.E) none of the above

Which of the following would be considered a theory?

A) Glass is fragile.B) Hot air rises.C) Gasoline has a very strong odor.

D) Helium balloons float because helium is less dense than air.E) none of the above

Which of the following is considered a hypothesis (as opposed to an observation)?

A) Spiders have eight legs.B) Birds can fly because they have hollow bones.

C) Fresh lava from a volcano is hot.D) The Washington Monument is 555 feet tall.E) none of the above

The correct scientific notation for the number 0.00050210 is:

A) 5.0210 × 104B) 5.021 × 10-4C) 5.021 × 104D) 5.0210 × 10-4E) none of the above

The correct scientific notation for the number 500.0 is:

A) 5 × 102B) 5.00 × 102C) 5.000 × 102D) 5 × 10-2E) none of the above

The correct decimal representation of 1.201 × 10-7 is:

A) 12010000B) 0.0001201C) 0.0000001201D) 1201.000E) none of the above

The correct decimal representation of 6.453 × 103 is:

A) 6,453B) 0.006453C) 6.5 × 103D) 6.453E) none of the above

The correct number of significant figures in the number 865,000 is:

A) 3B) 6C) 4D) 2E) none of the above

The correct number of significant figures in the number 0.002320 is:

A) 7B) 4C) 3D) ambiguousE) none of the above

When the value 4.449 is rounded to three significant figures, the number should be reported as:

A) 4.4B) 4.5C) 4.44D) 4.45E) none of the above

The base SI unit for temperature is:

A) Fahrenheit.B) Kelvin.C) Celsius.D) atmospheres.E) none of the above

The common English unit in which the speed of an automobile is expressed is miles/hr. What is the set of base SI units for speed?

A) mile/sB) km/hrC) km/sD) m/sE) none of the above

Given the following list of densities, which materials would float in a molten vat of lead provided that they do not themselves melt? Densities (g/mL): lead = 11.4, glass = 2.6, gold = 19.3, charcoal = 0.57, platinum = 21.4.

A) gold and platinumB) glass and charcoalC) gold, platinum, glass and coal

D) gold and charcoalE) none of the above

The Olympic Games shot put field event uses a 16 pound (lb) shot. Identify the correct solution map to convert from pounds to kilograms using prefix multipliers and the given conversions of and .

A) 16 lb × × × B) 16 lb × × ×

C) 16 lb × × × D) 16 lb × × ×

Which among the following statements is false?

A) A solid has a definite shape and a definite volume.

B) A liquid has a definite volume; but it has no definite shape.

C) A gas has neither definite volume nor definite shape.

D) Both solids and liquids are incompressible while gases are compressible.E) none of the above

A pure substance is:

A) composed of two or more different types of atoms or molecules combined in variable proportions.

B) composed of only one type of atom or molecule.

C) composed of two or more regions with different compositions.

D) composed of two or more different types of atoms or molecules that has constant composition.

E) none of the above

Which of the following statements about compounds is TRUE?

A) A substance that cannot be broken down into simpler substances.

B) A pure substance that has variable composition throughout.

C) A substance composed of two or more elements in fixed, definite proportions.

D) A substance that is not as common as pure elements.E) none of the above

Which of the following statements is FALSE?

A) Matter may be a pure substance or it may be a mixture.

B) A pure substance may either be an element or a compound.

C) A mixture may be either hom*ogeneous or heterogeneous.

D) Mixtures may be composed of two or more elements, two or more compounds, or a combination of both.

E) All of the above statements are true.

How would you classify salt water?

A) pure substance-compoundB) mixture-heterogeneousC) pure substance-element

D) mixture-hom*ogeneousE) none of the above

A solution is an example of a (an):

A) pure substance.B) element.C) compound.D) hom*ogeneous mixture.E) heterogeneous mixture.

Physical properties are:

A) those that a substance displays only through changing its composition.

B) those that cause atoms and molecules to change.

C) those that a substance displays without changing its composition.

D) identical for all solid matter.E) none of the above

All of the following can be considered physical properties EXCEPT:

A) taste.B) color.C) flammability.D) density.E) boiling point.

Which of the following is NOT an example of a physical property?

A) Solid ice can be very brittle.B) Water can freeze solid at 32 degrees Fahrenheit.

C) Water can form hydrogen and oxygen gas under electrolysis conditions.

D) Liquid water can turn into steam in a heated tea kettle.E) none of the above

Which of the following statements about physical and chemical changes is FALSE?

A) In a chemical change, matter changes its composition.

B) In a physical change, matter does not change its composition.

C) Phase changes are always physical changes.D) Chemical reactions are chemical changes.

E) All of the above statements are true.

If you hold a solid piece of pure gallium metal in your hand, your body heat will melt the gallium into its liquid form. This illustrates which of the following?

A) distillationB) physical changeC) chemical changeD) chemical propertyE) none of the above

Which of the following is NOT a technique that could be used to separate a mixture into its components?

A) stirringB) decantingC) filtrationD) distillationE) none of the above

When methane is burned with oxygen, the products are carbon dioxide and water. If you produce 18 grams of water from 8 grams of methane and 32 grams of oxygen, how many grams of carbon dioxide were produced in the reaction?

A) 40B) 22C) 58D) 18E) none of the above

Which of the following statements about energy is FALSE?

A) An object possessing energy can do work on another object. B) Energy can neither be created nor destroyed.

C) Energy is the single main component of the universe.D) Energy is the capacity to do work.

E) All of the above statements are true.

Which type of energy is associated with motion?

A) chemicalB) electricalC) potentialD) kineticE) none of the above

Which of the following items is NOT a common unit of energy?

A) jouleB) torrC) calorieD) kilowatt-hourE) none of the above

How many calories are there in a 255 Calorie snack bar?

A) 2.55 × 105B) 1.07 × 103C) 60.9D) 1 × 103E) none of the above

Which of the following is NOT true?

A) The degree "symbol" is not used with the Kelvin scale.B) A kelvin degree is the same size as a Celsius degree.

C) The Kelvin temperature scale avoids use of negative numbers.

D) Water boils at the same temperature value on both the Kelvin and Celsius scales.E) none of the above

Melting point can be defined as the temperature when a solid becomes a liquid. The melting point of the chemical acetone is -95°C. Which state of matter would you expect to exist for acetone at a temperature of -94°C?

A) solidB) liquidC) gasD) plasmaE) none of the above

In calculating the relationship between the amount of heat added to a substance and the corresponding temperature change, the specific heat capacity is usually represented by which symbol?

A) CB) QC) ΔTD) mE) K

Which of the following statements about atoms is FALSE?

A) Atoms compose all matter.B) Atoms are responsible for the sensation of smell.

C) Atoms are the basic building block of nature.D) An atom is the smallest identifiable unit of an element.

E) All of the above statements are true.

Which of the following is NOT part of Dalton's Atomic Theory?

A) Each element is composed of tiny indestructible particles called atoms.

B) All atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements.

C) Atoms combine in simple, whole-number ratios to form compounds.

D) Most of the atom's mass and all of its positive charge is contained in a small core called the nucleus.

E) All of the above are part of the atomic theory.

Which statement below is NOT consistent with the nuclear theory of the atom as proposed by Rutherford?

A) Most of the atom's mass and all of its positive charge is contained in a small core called the nucleus.

B) Electrical charge is a fundamental property of protons and electrons in which like charges repel and opposite charges attract.

C) Most of the volume of the atom is empty space occupied by tiny, negatively charged electrons.

D) There are as many electrons outside the nucleus as there are protons inside the nucleus in a neutral atom.

E) All of the above statements are consistent.

An atom containing 7 protons, 8 neutrons, and 7 electrons:

A) is charge-neutral.B) is an ion.C) is an oxygen atom.D) cannot exist.E) none of the above

The atomic mass unit is defined as:

A) the mass of the hydrogen atom containing only one proton.

B) the mass of electrons found in a carbon atom containing six protons and neutrons.

C) 1/12 the mass of a carbon atom containing six protons and six neutrons.

D) 1/14 the mass of a nitrogen atom containing 7 protons and 7 neutrons.E) none of the above

Which of the following elements has an atomic number of 4?

A) HB) CC) HeD) BeE) none of the above

Which of the following elements has only 12 protons?

A) CB) ZnC) MgD) OE) none of the above

Which one of the following is a main-group element?

A) CeB) CoC) CuD) CsE) none of the above

Metals are located where on the periodic table?

A) left sideB) right sideC) middleD) zig-zag diagonal line E) none of the above

Nonmetals are located where on the periodic table?

A) left sideB) right sideC) middleD) zig-zag diagonal line E) none of the above

Metalloids are located where on the periodic table?

A) left sideB) right sideC) middleD) zig-zag diagonal line. E) none of the above

Group 1A elements are also called:

A) noble gasesB) halogensC) alkaline earth metalsD) alkali metals E) none of the above

Group 7A elements are also called:

A) noble gasesB) halogensC) alkaline earth metalsD) alkali metals E) none of the above

Mg is a member of which family?

A) noble gasesB) halogensC) alkaline earth metals D) alkali metals. E) none of the above

Xe is a member of which family?

A) noble gasesB) halogensC) alkaline earth metals D) alkali metals. E) none of the above

Examine the elements listed below and identify the one element that is from a different periodic table group than the others.

A) SiB) SnC) TiD) GeE) All of these are from the same group.

Cr is a member of which family?

A) noble gasesB) halogensC) alkaline earth metals D) alkali metalsE) none of the above

All of the following statements about different elements are true EXCEPT:

A) Barium is an alkaline earth metal.B) Manganese is a transition metal.

C) Sulfur is considered a metalloid.D) Krypton is one of the noble gases.E) Iodine is a halogen.

Which of the following statements about ions is INCORRECT?

A) Cations are positive ions and anions are negative ions.B) Cations are formed when an atom loses electrons.

C) Anions are formed when an atom gains electrons.

D) Cations always have the same number of protons as electrons.E) All statements are correct.

What is the correct formula for a potassium ion with 18 electrons?

A) P+B) K+C) K-D) P-E) none of the above

How many electrons are in Br-?

A) 4B) 7C) 34D) 36E) none of the above

How many protons and electrons are present in O2-?

A) 8 protons and 8 electronsB) 10 protons and 8 electronsC) 8 protons and 10 electrons

D) 16 protons and 8 electronsE) none of the above

What is the charge on the barium ion?

A) 1-B) 2-C) 1+D) 2+E) none of the above

What is the charge on the ion formed by selenium?

A) 1-B) 2-C) 1+D) 2+E) none of the above

What is the charge on the ion formed by aluminum?

A) 5-B) 3-C) 13+D) 3+E) none of the above

How many electrons would be in a -2 charged anion of sulfur?

A) 2B) 16C) 18D) 36E) none of the above

Isotopes are:

A) atoms of the same element that have different number of neutrons.

B) atoms of the same element that have different number of protons.

C) atoms of the same element that have different number of electrons.

D) atoms of the same element that have the same number of neutrons.E) none of the above

The number of protons in the nucleus of an atom:

A) is called the atomic number.B) is given the symbol "Z."C) identifies the atom as a particular element.

D) is the same for all isotopes of an element.E) all of the above

The nucleus of an atom consists mainly of:

A) neutrons and electrons.B) protons and electrons.C) protons and neutrons.

D) protons, neutrons, and electrons.E) none of the above

How many neutrons are present in Ne-22?

A) 12B) 10C) 22D) 32E) none of the above

What is the mass number of the hydrogen isotope that contains 2 neutrons?

A) 1B) 2C) 3D) 4E) none of the above

How many protons and neutrons are in Cl-37?

A) 20 protons, 17 neutronsB) 17 protons, 37 neutronsC) 17 protons, 20 neutrons

D) 37 protons, 17 neutronsE) none of the above

An atom that has the same number of neutrons as Ba is:

A) CsB) BaC) LaD) XeE) none of the above

A specific isotope of an element is known to have 15 protons and 16 neutrons. Which symbol would properly represent this isotope?

A) GaB) PC) XD) SE) none of the above

What is the charge on an ion that has an atomic number of 24 and contains 22?

A) 2+B) 2-C) 1+D) 1-E) none of the above

Given that the molecular mass of bromine is 79.90 grams, which of the following isotopes would you expect to have the greatest natural abundance?

A) Br-79B) Br-80C) Br-81D) Br-82E) none of the above

When elements combine to form compounds:

A) their properties are an average of all elements in the compound.B) their properties change completely.

C) their properties do not change.D) their properties are completely random.

E) none of the above

The law of constant composition states:

A) Matter cannot be either created or destroyed in a chemical reaction.

B) The nucleus is a dense region of positive charge that always contains protons and neutrons.

C) All samples of a given compound have the same proportions of their constituent elements.

D) All atoms of a given element have a constant composition and are different than atoms of any other element.

E) none of the above

The oxygen-to-hydrogen mass ratio of water is always 8.0 is an example of what fundamental law?

A) Law of Constant CompositionB) Law of Constant Mass Ratio

C) Law of Conservation of MassD) Law of Constant Whole Number Ratio

E) none of the above

What is the oxygen-to-hydrogen mass ratio for H2O2?

A) 0.125B) 4C) 8D) 16E) none of the above

Which of the following statements about chemical formulas is FALSE?

A) The subscripts represent the relative number of each type of atom in the compound.

B) The subscripts represent the relative mass of each type of atom in the compound.

C) The subscripts do not change for a given compound.

D) Different compounds made of the same elements have different subscripts.

E) All of the statements are true.

How many total atoms are in the formula Al2(CO3)3?

A) 8B) 9C) 12D) 14E) none of the above

How many of each type of atoms are there in the formula NH4C2H3O2?

A) N = 4, H = 7, C = 2, O = 2B) N = 1, H = 4, C = 2, O = 2C) N = 1, H = 3, C = 2, O = 2

D) N = 1, H = 7, C = 2, O = 2E) none of the above

What is the correct formula of a compound that has ten oxygen atoms and four phosphorus atoms?

A) O10P4B) 10OP4C) 4PO10D) P4O10E) none of the above

Carbon is considered which of the following?

A) atomic elementB) molecular elementC) molecular compound

D) ionic compoundE) none of the above

Which among the following elements does NOT exist as a diatomic molecule in nature?

A) hydrogenB) nitrogenC) fluorineD) neonE) none of the above

Ammonium fluoride is considered which of the following?

A) atomic elementB) molecular elementC) molecular compound

D) ionic compoundE) none of the above

Which of the following is a molecular compound?

A) barium sulfideB) calcium acetateC) potassium hydroxide

D) nitrogen monoxideE) none of the above

What is the formula for an ionic compound made of barium and nitrogen?

A) Ba3N2B) Ba2N3C) BaND) Ba2N4E) none of the above

What is the formula for an ionic compound made of carbon and oxygen?

A) CO2B) C2OC) COD) CO3

E) Carbon and oxygen do not form an ionic compound.

What is the formula for an ionic compound made of aluminum and oxygen?

A) AlO2B) Al2O3C) Al3O2D) AlOE) none of the above

What is the name of the ionic compound made of beryllium and chlorine?

A) beryllium(II) chlorideB) beryllium dichlorideC) beryllium chloride

D) monoberyllium dichlorideE) none of the above

What is the name of the compound made from lithium and oxygen?

A) lithium dioxideB) lithium(I) oxideC) oxygen lithideD) lithium oxideE) none of the above

Which metal atom below cannot form a cation of several different charges?

A) CrB) MnC) FeD) BaE) none of the above

What is the name of CoS?

A) cobalt(II) sulfideB) cobalt sulfideC) cobalt monosulfide

D) cobaltous sulfurE) none of the above

Which formula shown is incorrect for the name given?

A) magnesium nitrite: Mg(NO2)3B) calcium carbonate: CaCO3C) aluminum sulfate: Al2(SO4)3

D) sodium hydrogen carbonate: NaHCO3E) potassium hydroxide: KOH

Which formula shown is incorrect for the name given?

A) strontium carbonate: SrCO3B) ammonium cyanide: NH4CNC) potassium acetate: KC2H3O2

D) calcium nitrate: Ca(NO3)2E) lithium sulfate: LiSO4

What is the name of the compound whose formula is Na2O?

A) sodium monoxideB) disodium oxideC) disodium monoxide

D) sodium oxideE) none of the above

What is the formula for the acetate polyatomic ion?

A) C3H2O3-B) C2H3O22-C) C2H3O2-D) C2H3O-E) none of the above

What is the correct formula for ammonium hydrogen sulfate?

A) NH4HSO4B) (NH4)2HSO4C) (NH4)2SO4D) Am2HSO4E) none of the above

The charge of a vanadium ion in the compound V2O5 is:

A) 5+B) 2+C) 10+D) 10-E) none of the above

What is the correct formula for the hypochlorite polyatomic ion?

A) ClO-B) ClO2-C) ClO3-D) ClO4-E) none of the above

The name trisodium phosphate is incorrect for the compound Na3PO4 because:

A) this compound should be called trisodium monophosphate.B) the sodium has a negative 3 charge.

C) you cannot use a prefix for the first element in a molecular compound.

D) you cannot use a prefix for the first element of an ionic compound.E) none of the above

What is correct name of the compound whose formula is N2O4?

A) nitrogen dioxideB) nitrogen tetroxideC) dinitrogen oxide

D) dinitrogen tetroxideE) none of the above

What would the formula of diiodine pentasulfide be?

A) I5S2B) I2S5C) I4S9D) I2S7E) none of the above

What is the proper name for HBr (aq)?

A) hydrobromous acidB) hydrousbromic acidC) hydrobromic acid

D) bromous acidE) none of the above

What is the name of HIO3?

A) iodic acidB) hydroioidic acidC) hydroiodous acidD) iodous acidE) none of the above

What is the name of HNO2?

A) nitric acidB) nitrous acidC) hydronitrous acidD) hydronitric acidE) none of the above

A certain oxyacid is derived from the oxyanion SO32-. The formula for the oxyacid is:

A) H2SO4.B) HSO3.C) H2SO3.D) H3SO3.E) none of the above

What is the formula mass for diboron tetrachloride?

A) 127.98 amuB) 198.89 amuC) 234.34 amuD) 163.43 amuE) none of the above

What is the formula mass of copper (II) fluoride?

A) 101.55B) 146.10C) 90.00D) 165.10E) none of the above

The number of cycles of a wave that passes a stationary point in one second is called its:

A) wavelength.B) frequency.C) crest.D) trough.E) none of the above

What is the correct order of the electromagnetic spectrum from shortest wavelength to longest?

A) Gamma Rays→X-rays→Ultraviolet Radiation→Visible Light→Infrared Radiation→Microwaves→Radio Waves

B) Visible Light→Infrared Radiation→Microwaves→Radio Waves→Gamma Rays→X-rays→Ultraviolet Radiation

C) Radio Waves→X-rays→Ultraviolet Radiation→Visible Light→Infrared Radiation→Microwaves→Gamma Rays

D) Gamma Rays→X-rays→Visible Light→Ultraviolet Radiation→Infrared Radiation→Microwaves→Radio Waves

E) Gamma Rays→X-rays→Infrared Radiation→Visible Light→Ultraviolet Radiation→Microwaves→Radio Waves

When sunlight is passed through a prism, what is observed?

A) continuous spectrumB) nothingC) bright spots and linesD) white lightE) none of the above

When Hydrogen light is passed through a prism, what is observed?

A) continuous spectrumB) nothingC) a line spectrumD) white lightE) none of the above

Which statement below does NOT follow the Bohr Model?

A) When energy is absorbed by atoms, the electrons are promoted to higher-energy orbits.

B) When an atom emits light, electrons fall from a higher orbit into a lower orbit.

C) The energy emitted from a relaxing electron can have any wavelength.

D) Electrons exist in specific, quantized orbits.E) none of the above

The principal quantum number (n):

A) specifies the 3-D shape of the orbital.B) specifies the subshell of the orbital.

C) specifies the maximum number of electrons.D) specifies the principal shell of the orbital.

E) none of the above

The subshell letter:

A) specifies the 3-D shape of the orbital.B) specifies the principal quantum number of the orbital.

C) specifies the maximum number of electrons.D) specifies the principal shell of the orbital.

E) none of the above

How many subshells are there in the n = 4 principal shell?

A) 1B) 2C) 3D) 4E) not enough information

How many subshells are there in the n = 2 principal shell?

A) 1B) 2C) 3D) 4E) not enough information

The n = ________ principal shell is the lowest that may contain a d-subshell.

A) 1B) 2C) 3D) 4E) not enough information

Which subshell letter corresponds to a spherical orbital?

A) sB) pC) dD) fE) not enough information

Which subshell letter corresponds to a 4-leaf clover orbital pattern?

A) sB) pC) dD) fE) not enough information

Which statement is NOT true about "p" orbitals?

A) A subshell contains three "p" orbitals.B) These orbitals are shaped like dumbbells.

C) A 3p orbital has a higher energy than a 2p orbital.D) All three of these statements are true.

E) none of the above

How many electrons can exist in an orbital?

A) 1B) 2C) 3D) 4E) none of the above

"When filling orbitals of equal energy, electrons fill them singly first with parallel spins." This is known as:

A) Hund's rule.B) Pauli exclusion principle.C) Bohr's model.D) Ground state. E) none of the above

The subshell that has three orbitals and can hold up to six electrons is the:

A) s subshellB) p subshellC) d subshellD) f subshellE) none of the above

The subshell that has five orbitals and can hold up to ten electrons is the:

A) d subshellB) f subshellC) s subshellD) p subshellE) none of the above

An accepted abbreviation format is to write an electron configuration that includes a noble gas symbol in brackets. If you were writing an electron configuration for a bromine atom, which elemental symbol would you place in the bracket?

A) HeB) NeC) ArD) KrE) Xe

What is the electron configuration for Kr?

A) 1s22s22p63s23p43d104s24p6B) 1s22s22p63s23p64s23d24p6C) 1s22s22p63s23p64s23d104p6

D) 1s22s22p63s23p24s23d104p6E) none of the above

What is the electron configuration for Ga?

A) 1s22s22p63s23p63d104s24p6B) 1s22s22p63s23p64s23d104p1C) 1s22s22p63s23p53d104s24p1

D) 1s22s22p63s23p64s24d104p1E) none of the above

What is the electron configuration for P?

A) [Ar]3s23p64s23d104p3B) [Ne]1s21p62s22p3C) [Ne]3s23p3D) [Ar]3s23p3E) none of the above

The element with a completely filled p-subshell is:

A) NaB) AlC) PD) ArE) none of the above

What is the element in which at least one electron is in the d-orbital?

A) ArB) KC) CaD) ScE) none of the above

How many valence electrons are in a chlorine atom?

A) 1B) 17C) 10D) 7E) none of the above

The size of an atom generally increases:

A) down a group and from right to left across a period.B) up a group and from left to right across a period.

C) down a group and from left to right across a period.D) up a group and from right to left across a period.

E) up a group and diagonally across the Periodic Table.

Which of the following elements has the lowest ionization energy?

A) RbB) NaC) CD) FE) He

Which of the following atoms is the largest?

A) LiB) NaC) KD) RbE) Cs

Which of the following atoms has the greatest metallic character?

A) CsB) BeC) CuD) TiE) Au

What is the correct value for Avogadro's number?

A) 6.022 × 1023B) 6.022 × 1033C) 6.023 × 1022D) 6.022 × 102.3E) none of the above

One half of a mole of atoms would contain how many atoms?

A) 0.5B) 3.011 × 1023C) 6.022 × 1023D) 6.022 × 1011.5E) none of the above

In comparing a balloon containing 25 grams of helium to a balloon containing 25 grams of neon, which one of the following statements is TRUE?

A) Each balloon has an equal number of atoms.B) The helium balloon has more atoms.

C) The neon balloon has more atoms.D) This scenario cannot happen because gases have no mass.

E) none of the above

In comparing 1 mole of carbon atoms to one mole of magnesium atoms, which statement is TRUE?

A) The mass of 1 mole of carbon is greater than the mass of 1 mole of magnesium.

B) The mass of 1 mole of magnesium is greater than the mass of 1 mole of carbon.

C) The mass of 1 mole of carbon is the same as the mass of 1 mole of magnesium.

D) There are more atoms in 1 mole of magnesium than in 1 mole of carbon.E) none of the above

One mole of (NH4)2HPO4 contains how many moles of hydrogen atoms?

A) 4B) 2C) 8D) 9E) none of the above

One mole of ammonium nitrite contains:

A) 2 moles of nitrogen atoms.B) 4 moles of hydrogen atoms.C) 2 moles of oxygen atoms.

D) All of A, B, and C.E) None of A, B, and C.

The mass of one mole of carbon dioxide is ________ g.

A) 28.01B) 384.4C) 32.00D) 44.01E) none of the above

What is the molar mass of aluminum sulfate?

A) 123.0 g/molB) 278.0 g/molC) 306.2 g/molD) 315.2 g/molE) 342.2 g/mol

Which of the following statements about empirical formulas is incorrect?

A) An empirical formula represents a molecule.

B) An empirical formula gives the smallest whole number ratio of each type of atom in a molecule.

C) An empirical formula must be multiplied by an integer to obtain the molecular formula.

D) The molecular formula can be the same as the empirical formula in some situations. E) All statements are correct.

The simplest formula for hydrogen peroxide is HO. To determine its molecular formula, it is necessary to know:

A) the properties of hydrogen peroxide.B) the density of hydrogen peroxide.

C) the molar mass of hydrogen peroxide.D) the number of moles of hydrogen peroxide in 1.00 g of the substance.

E) none of the above

Which of the following is already in its empirical formula?

A) C22H34O10B) C6H6C) C6H12O3D) C5H12O2E) none of the above

A reaction which forms a gaseous product is an example of a(n)________.

A) oxidation-reduction reactionB) combustion reaction C) precipitation reaction

D) gas evolution reactionE) none of the above

A reaction which forms a solid product is an example of a(n):

A) oxidation-reduction reaction.B) combustion reaction. C) precipitation reaction.

D) gas evolution reaction.E) none of the above

A reaction in which a substance reacts with oxygen, emitting heat and forming oxygen-containing compounds is an example of a(n):

A) acid-base reaction.B) combustion reaction.C) precipitation reaction.

D) gas evolution reaction.E) none of the above

When water is heated, bubbles form in the water. Is this evidence of a chemical reaction? Why?

A) No, boiling water is a physical change.B) Yes, the formation of a gas is evidence of a chemical reaction.

C) No, the formation of gas bubbles is a secondary chemical reaction which is ignored.

D) Yes, the formation of a gas is proof a new compound has been made.E) none of the above

Which of the following is NOT evidence that a chemical reaction has occurred?

A) color change when chemicals are contacted with each other

B) solid formation when chemicals are contacted with each other

C) gas formation when chemicals are contacted with each other

D) emission of light when chemicals are contact with each other

E) All of the above are evidence of a chemical reaction.

Before a chemical equation can be written, one must know:

A) the atomic mass of all the elements involved.B) the molar mass of all the compounds.

C) the symbols and formulas of all reactants and products.D) the number of moles of all reactants and products.

E) none of the above.

When the equation, ___O2 + ___C5H12 → ___CO2 + ___H2O is balanced, the coefficient: of O2 is:

A) 3B) 4C) 5D) 8E) none of the above

What are the coefficients for the following reaction when it is properly balanced?

___Na3PO4 + ___Ba(NO3)2 → ___NaNO3 + ___Ba3(PO4)2

A) 2, 1, 1, 3B) 2, 3, 1, 6C) 2, 3, 6, 1D) 6, 1, 3, 2E) none of the above

An aqueous solution is:

A) any liquid with another compound dissolved in it.B) an ionic compound with water dissolved in it.

C) water with a molecular compound dissolved in it.D) water with another compound dissolved in it.

E) none of the above

All of the following compounds are soluble in water EXCEPT:

A) NaCl.B) CaCl2.C) FeCl3.D) NH4Cl.E) PbCl2.

The compound sodium sulfate is soluble in water. When this compound dissolves in water, which ion listed below would be present in solution?

A) SO42-B) S2-C) O2-D) Na22+E) none of the above

When solid NaCl is stirred into water, which of the following is NOT true?

A) Individual sodium and chloride ions are present.B) The solution will conduct electricity.

C) The solution will taste salty.D) The NaCl will fail to dissociate.E) none of the above

Several grams of sodium chloride are stirred into a glass of water and are no longer visible to the eye. Which of the following statements is FALSE?

A) The sodium chloride solid has dissociated into its component ions. B) An aqueous solution has been prepared.

C) No precipitate has formed.D) Sodium chloride is insoluble in water.E) All of the statements are true.

In writing the chemical equation for a precipitation reaction, what abbreviation of the physical state must appear with one of the products?

A) (s)B) (g)C) (l)D) (w)E) none of the above

What type of a reaction occurs when a potassium nitrate solution is mixed with a barium acetate solution?

A) precipitationB) acid-base neutralizationC) oxidation-reduction

D) gas evolutionE) no reaction

What would be the formula of the precipitate that forms when Pb(NO3)2 (aq) and K2SO4 (aq) are mixed?

A) K(NO3)2B) PbSO4C) PbK2D) H2OE) none of the above

Considering the following precipitation reaction:Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq). Which compound would not form ions in the total ionic equation?

A) PbI2B) KNO3C) Pb(NO3)2D) KIE) All compounds form ions in the total ionic equation.

Considering the following precipitation reaction:Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq). Which ion(s) would NOT be present in the net ionic equation?

A) Pb2+, NO3- B) K+, NO3- C) K+, Pb2+D) K+, I- E) All the above ions are in the net ionic equation.

Considering the following precipitation reaction:Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq). Which ion(s) would NOT be spectator ions?

A) Pb2+, NO3-B) K+, I- C) NO3-, Pb2+. D) Pb2+, I - E) All the above ions are in the net ionic equation.

Considering the following precipitation reaction:Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq). What is the correct total ionic equation?

A) Pb2+ + (NO3)2- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3- B) Pb2+ + 2NO3- +2K+ + I- → PbI2(s) + 2K+ + NO3-

C) Pb2+ + 2NO3- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-D) Pb2+ + 2NO3- + 2K+ + 2I- → Pb2+ + 2I- + 2K+ + 2NO3-

E) none of the above

Considering the following precipitation reaction:Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq). What is the correct net ionic equation?

A) Pb2+ + I2- → PbI2(s) B) 2NO3- + 2K+ → 2KNO3 C) Pb2+ + 2NO3- + 2K+ + 2I- → PbI2(s) + 2K+ + 2NO3-

D) Pb2+ + 2I- → PbI2(s) E) none of the above

Which is a spectator ion from the following complete ionic equation:

Ag+(aq) + NO3-(aq) + K+ (aq) + Br-(aq) → AgBr(s) + K+(aq) + NO3- (aq)

A) Ag+B) Br-C) K+D) AgBr E) none of the above

Which of the following is NOT an acid?

A) HClO4B) HNO3C) HC2H3O2D) H2SO4E) none of the above

What is the net ionic equation for the reaction of hydrochloric acid with potassium hydroxide?

A) H+ + Cl- + K+ + OH- → H2O + K+ + Cl- B) HCl + KOH → H2O + KCl

C) H+ + OH- → H2O D) 2H+ +2Cl- + K2+ + 2OH- → H2O + K2+ +2 Cl- E) none of the above

What is the molecular equation for the reaction of hydrochloric acid with potassium hydroxide?

A) H2Cl + 2KOH → H2O +2KCl B) 2HCl + K(OH)2 → 2H2O + KCl2C) H+ + OH- → H2O

D) HCl + KOH → H2O + KCl E) none of the above

What is the complete ionic equation for the reaction of hydrochloric acid with potassium hydroxide?

A) H+ + Cl- + K+ + OH- → H2O + K+ + Cl- B) H+ + Cl- + K+ + OH- → 2H+ + O2- + K+ + Cl-

C) H+ + OH- → H2O D) 2H+ +2Cl- + K2+ + 2OH- → H2O + K2+ +2 Cl- E) none of the above

As defined in the text, identify the "gas evolution" reactions among the following:

1. 2HCl(aq) + K2CO3(aq) → H2O(l) + CO2(g) + 2KCl(aq)

2. CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)

3. 2HCl(aq) + K2S(aq) → H2S(g) + 2KCl(aq)

A) 1 and 2 onlyB) 1 and 3 onlyC) 2 and 3 onlyD) All of 1, 2, and 3E) None of 1, 2, and 3

Methane gas (CH4), on complete combustion in air, produces:

1. CO22. H23. H2O

A) 1 and 2 onlyB) 1 and 3 onlyC) 2 and 3 onlyD) All of 1 and 2 onlyE) None of 1, 2, and 3

What type of reaction is the generic equation ?

A) synthesis/combinationB) decompositionC) single displacement

D) double-displacementE) none of the above

What type of reaction is the generic equation A + BC → AC + B?

A) synthesis/combinationB) decompositionC) single displacement

D) double-displacementE) none of the above

What type of reaction is the generic equation ?

A) synthesis/combinationB) decompositionC) single displacement

D) double-displacementE) none of the above

Identify the double displacement reactions among the following:

1. KCl(aq) + AgNO3(aq) → AgCl(s) + KNO3(aq)

2. Na2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2NaCl(aq)

3. H2SO4((aq) + 2NaOH(aq) → Na2SO4((aq) + 2H2O(l)

A) 1 and 2 onlyB) 1 and 3 onlyC) 2 and 3 onlyD) All of 1, 2, and 3E) None of 1, 2, and 3

Which of the following is TRUE?

A) Stoichiometry shows the numerical relationship between chemical quantities in a balanced chemical equation.

B) Stoichiometry allows prediction of the amounts of products that form in a chemical reaction based on the amounts of reactants.

C) Stoichiometry allows prediction of how much of the reactants are necessary to form a given amount of product.

D) All of the above are true.E) None of the above are true.

Diatomic N2 can react with diatomic H2 to form ammonia (NH3). The balanced chemical equation is:

If 6 moles of H2 totally reacted with more than enough N2, how many moles of ammonia would be expected to form?

A) 2 molesB) 3 molesC) 4 molesD) 6 molesE) not enough information

Given the balanced equation CH4 + 2 O2 → CO2 + 2 H2O, which of the following is NOT a correct conversion factor?

A) 2 mole H2O = 18.02 gB) 1 mole O2 = 32.00 gC) 1 mole CH4 = 2 mole H2O

D) 2 mole O2 = 1 mole CO2E) none of the above

Which of the following statements is false?

A) The limiting reactant is completely consumed in a chemical reaction.

B) The theoretical yield is the amount of product that can be made based on the amount of limiting reagent.

C) The actual yield is the amount of product actually produced by a chemical reaction.

D) The percent yield = × 100%.E) All of the above are true statements.

Given the balanced equation CO2 + Si → SiO2 + C, if you were to react 1 mole of CO2 with 1 mole of Si, which statement is TRUE?

A) The CO2 is the limiting reactant.B) The Si is the limiting reactant.C) The SiO2 is the limiting reactant.

D) You have equal stoichiometric amounts of reactants.E) none of the above

In order to determine the limiting reactant in a particular reaction, one must know each of the following EXCEPT:

A) the mass of each reactant present.B) the molar mass of each reactant present.

C) the coefficient of each reactant in a balanced equation.D) the mass of each product formed.

The reaction of one mole of nitrogen gas with three moles of hydrogen gas releases 92 kJ of thermal energy to the surroundings. Which of the following is TRUE?

A) This reaction is exothermic.B) This reaction has a negative enthalpy of reaction.

C) Complete reaction of two moles of nitrogen gas would release 184 kJ of thermal energy in this reaction.

D) All of the above are true.E) None of the above are true.

Hexane, a nonpolar solvent, will dissolve which of the following substances?

A) sodium chlorideB) oilC) ammonium acetateD) vinegar (acetic acid)E) none of the above

Which compound below forms an electrolyte solution when dissolved in water?

A) Cl2B) KOHC) CH3CH2OHD) C12H22O11 (sucrose)E) none of the above

In order for a solute to dissolve in solution:

A) the solute-solvent forces must be greater than the solute-solute forces.

B) the solute-solute forces must be greater than the solute-solvent forces.

C) the solute-solvent forces must equal the solute-solute forces.

D) the polarity of the solute and solvent must be opposite.E) none of the above

If you prepare a solution by adding sufficient amount of solute so that after heating and cooling the solution there is a visible amount of solid solute left in the bottom of the beaker, the solution would be considered ________.

A) unsaturatedB) saturatedC) supersaturatedD) thermally saturated E) none of the above

Which of the following compounds is a strong electrolyte?

A) B) C) D) NaE) all of the above

When an ionic compound dissolves in water:

A) the solvent-solute attractive forces overcome the solute-solute attractions.

B) the positive end of water dipoles attract the negative ions.

C) the negative end of water dipoles attract the positive ions.

D) each of the above (A, B, and C) occurs.E) none of the above (A, B, or C) occurs.

The solubility of gases in water:

A) is independent of temperature.B) increases with increasing temperature.

C) decreases with increasing temperature. D) gases are not soluble in water.E) none of the above

Which one of the following aqueous solutions would have the higher concentration of K+ (aq) ions? (Assume total solubility in water.)

A) 1.0 M KC2H3O2B) 1.0 M KNO3C) 1.0 M K2CO3D) 1.0 M K3PO4

E) All of these solutions have the same concentration of K+ (aq).

A 0.15 M solution of BaCl2 contains:

A) 0.15 M Ba2+ ions and 0.15 M Cl- ions.B) 0.15 M Ba2+ ions and 0.30 M Cl- ions.

C) 0.30 M Ba2+ ions and 0.15 M Cl- ions.D) 0.30 M Ba2+ ions and 0.30 M Cl- ions. E) none of the above

After you have completed the task of diluting a solution, which statement below must be TRUE?

A) The new solution has more volume but has a lower concentration than before.

B) The new solution has more volume but has a higher concentration than before.

C) The new solution has less volume but has a lower concentration than before.

D) The new solution has less volume but has a higher concentration than before.E) none of the above

Which of the following is NOT a property of acids?

A) Acids have a slippery feel.B) Acids have a sour taste.C) Acids turn litmus paper red.

D) Acids dissolve many metals.E) All of the above are properties of acids.

Which of the following is NOT a property of bases?

A) Bases have a slippery feel.B) Bases have a bitter taste.C) Bases turn litmus paper blue.

D) Bases dissolve many metals.E) All of the above are properties of bases.

The Arrhenius definition of an acid is:

A) a proton donor.B) a proton acceptor.C) produces H⁺ in solution.

D) produces OH⁻ in solution.E) none of the above

The Bronsted-Lowry definition of a base is:

A) a proton donor.B) a proton acceptor.C) produces H⁺ in solution.

D) produces OH⁻ in solution.E) none of the above

The Bronsted-Lowry definition of an acid is:

A) a proton donor.B) a proton acceptor.C) produces H⁺ in solution.

D) produces OH⁻ in solution.E) none of the above

Which of the following is NOT true?

A) The Bronsted-Lowry Model applies to a wider range of acid-base phenomena than does the Arrhenius Model.

B) The Arrhenius Model of acids and bases was developed before the Bronsted-Lowry Model.

C) The Bronsted-Lowry Model can apply to bases that do not contain hydroxide ions.

D) The Arrhenius Model of acids and bases applies toward substances that are nonaqueous. E) none of the above

In the following reaction:HCO3- (aq) + H2O (aq) → H2CO3 (aq) + OH- (aq)

A) HCO3- is an acid and H2CO3 is its conjugate base.B) H2O is an acid and OH- is its conjugate base.

C) HCO3- is an acid and OH- is its conjugate base.D) H2O is an acid and H2CO3 is its conjugate base.

E) H2O is an acid and HCO3- is its conjugate base.

Which of the following statements about water are TRUE?

A) Water can act as an acid.B) Water can act as a base.C) The conjugate base of water is OH-.

D) The conjugate acid of water is H3O+.E) All of the above are true.

What are the products of a neutralization reaction?

A) salt and carbon dioxideB) carbon dioxide and waterC) water and salt

D) oil and waterE) none of the above

A neutralization reaction between KOH (aq) and H2SO4 (aq) would give which two products?

A) H2O (l) and H2S (g)B) H2O (l) and KSO4 (aq)C) H2O (l) and K2SO4 (aq)

D) SO2 (g) and KH2 (g)E) none of the above

Which of the following acids is a diprotic, weak acid?

A) sulfuric acidB) phosphoric acidC) hydrobromic acidD) carbonic acidE) none of the above

Which of the following acids is a monoprotic, strong acid?

A) sulfuric acidB) phosphoric acidC) hydrobromic acidD) carbonic acidE) none of the above

Which of the following is a weak base?

A) calcium hydroxide. B) sodium fluorideC) potassium hydroxideD) ammoniaE) none of the above

A 0.10 M solution of an electrolyte has a pH of 4.5. The electrolyte is:

A) a strong acid.B) a strong base.C) a weak acid.D) a weak base.E) none of the above

What is the concentration of H⁺ in 0.50 M hydroiodic acid?

A) 0.50 MB) 1.0 MC) <0.50 MD) 1.50 ME) none of the above

Substances that can act both as an acid and as a base are called:

A) neutral.B) buffers.C) indicators.D) amphoteric.E) none of these

Which solution below has the highest concentration of hydroxide ions?

A) pH = 3.21B) pH = 12.49C) pH = 7.00D) pH = 10.12E) pH = 7.93

In order for a solution to be acidic:

A) [H3O+] < [OH-]B) [H3O+] > [OH-]C) [H3O+] = [OH-]D) pH = pOHE) none of the above

In order for a solution to be basic:

A) [H3O+] > [OH-]B) [H3O+] < [OH-]C) [H3O+] = [OH-]D) pH = pOHE) none of the above

What is the concentration of the hydroxide ions in an acidic solution?

A) 0.0 MB) 1.0 MC) 1.0 MD) > 1.0 ME) < 1.0 M

In a solution that has a pH = 7.0:

A) [H3O+] > [OH-]B) [H3O+] < [OH-]C) [H3O+] = [OH-]D) [H3O+] + [OH-] = Kw. E) none of the above

A solution at 25°C has a hydrogen ion concentration of 2.6 × 10-5 M. Which of the following is TRUE?

A) [H3O+] > [OH-]B) [H3O+] < [OH-]C) [H3O+] = [OH-]D) [H3O+] = E) none of the above

What is the concentration of the hydronium ions in a neutral solution?

A) 0.0 MB) 1.0 MC) 1.0 MD) > 1.0 ME) < 1.0 M

If the pH of an aqueous solution changed from 9.10 to 4.67, what happened to the hydronium ion concentration?

A) It decreased.B) It became zero.C) It became less than zero.D) It increased. E) none of the above

Which solution below is considered to have basic character?

A) pOH = 7B) pH = 2C) pOH = 4D) pOH = 13E) none of the above

All of the following statements are consistent with the kinetic molecular theory of gases EXCEPT:

A) The size of the gas molecules is negligible compared to the total volume of the gas.

B) The average kinetic energy of the molecules of a gas is proportional to the temperature of the gas in kelvins.

C) Gas particles collide with each other and surfaces without losing any energy.

D) Strong attractive forces hold the gas molecules together.E) none of the above

A barometer uses mercury because:

A) it is a convenient, safe, lightweight material.

B) the density of mercury is very large which allows the barometer to be short.

C) it is the traditional substance used, water could be as easily used.

D) it is the only liquid metal at room temperature.E) All of the above are true.

To solve problems using Boyle's Law, which mathematical equation should be used?

A) = B) = C) = D) = E) none of the above

To solve problems using Charles's Law, which mathematical equation should be used?

A) = B) =C) = D) = E) none of the above

When must temperature values in gas law calculations be expressed in kelvin units?

A) only for Charles's lawB) only for the Ideal Gas lawC) only for the Combined Gas law

D) neverE) always

Gas density can be calculated by dividing the mass of gas by its volume. If you took a balloon of gas and then warmed the balloon in a sunny window, what can now be said about the density of the gas in the balloon?

A) The gas density will remain the same.B) The gas density will increase.

C) The gas density will decrease.D) The density of gases is independent of temperature.

E) none of the above

Which of the following statements is TRUE for gases?

1. The temperature of a gas is inversely proportional to its pressure.

2. The volume of a gas is directly proportional to the pressure in torr.

3. The pressure of a gas is due to collisions of the gas molecules.

A) 1 only B) 2 only C) 3 only D) 1 and 2 only E) 1 and 3 only

What is the proper form of the combined gas law?

A) = B) = C) = D) = E) none of the above

To solve problems using Avogadro's Law, which mathematical equation should be used?

A) = B) = C) = D) = E) none of the above

The ideal gas law is:

A) PV = nRTB) P = C) T = D) V =

E) All of the above are forms of the ideal gas law.

Which set of conditions reflect STP?

A) 298 K, 1 atmB) 25°C, 14.7 psiC) 373 K, 760 torrD) 273 K, 1 PaE) 273 K, 760 mm Hg

Which of the following statements about Lewis structures is FALSE?

A) An octet is when an atom has 8 valence electrons.B) A duet is a stable electron configuration for helium.

C) An ionic bond occurs when electrons are transferred.D) A covalent bond occurs when electrons are shared.

E) All of the above statements are true.

Which Lewis structure below correctly represents KCl?

A) K⁺ []⁻B) K⁺ [::]⁻C) K ::D) :: ::E) none of the above

Which Lewis structure below correctly represents the compound formed between magnesium and sulfur?

A) Mg⁺ [::]⁻B) Mg⁺ [::]⁻2 Mg⁺C) [::]⁻ Mg⁺2 [::]⁻D) Mg⁺2 [::]⁻2E) none of the above

The Lewis model predicts that the formula of a compound formed between bromine and aluminum is:

A) AlBrB) Al2BrC) AlBr3D) AlBr2E) none of the above

The Lewis model predicts that the formula for a compound between fluorine and calcium is:

A) CaFB) Ca2FC) CaF2D) CaF3E) none of the above

The Lewis model predicts that the formula for a compound between barium and sulfur is:

A) BaSB) Ba2SC) BaS2D) BaS3E) none of the above

The Lewis model predicts that the formula for a compound between potassium and sulfur is:

A) KSB) K2SC) KS2D) K3SE) none of the above

When a nonmetal bonds with a nonmetal:

A) a molecular compound forms.B) a covalent bond is involved.C) electrons are shared.

D) all of the above are trueE) none of the above

What is the correct Lewis structure for water?

A) H-::-HB) :--:C) H==HD) H--HE) none of the above

What is the correct Lewis structure for Br2?

A) Br-BrB) : - :C) =D) : Br≡ Br :E) none of the above

What is the correct Lewis structure for O2?

A) O-OB) :-:C) =D) : O ≡ O :E) none of the above

What is the correct Lewis structure for N2?

A) N-NB) :-:C) =D) : N ≡ N :E) none of the above

How many bonding electrons are in the Lewis structure of N2?

A) 2B) 3C) 4D) 6E) none of the above

How many bonding electrons are in the Lewis structure of carbon monoxide, CO?

A) 2B) 3C) 4D) 6E) none of the above

The Lewis structure for carbon monoxide is This structures shows:

A) 4 lone pairs and 1 bonding pair. B) 4 lone pairs and 3 bonding pairs.

C) 2 lone pairs and 3 bonding pairs.D) 2 lone pairs and 1 bonding pair.E) none of the above

Which sequence below represents the proper order of increasing bond strength?

A) single < double < tripleB) double < single < tripleC) single < triple < double

D) triple < double < singleE) none of the above

How many valence electrons are in the nitrate ion?

A) 18B) 22C) 23D) 24E) 26

The total number of electrons to be counted for the Lewis structure of the PO43- polyatomic ion is:

A) 8.B) 26.C) 29.D) 32.E) none of the above

The central atom in the chlorate anion, ClO3- is surrounded by:

A) two bonding and two unshared pairs of electrons.B) one bonding and three unshared pairs of electrons.

C) three bonding and one unshared pair of electrons.D) two double bonds and no unshared pairs of electrons.

E) none of the above.

The central atom in the chlorite anion, ClO2- is surrounded by:

A) one bonding and three unshared pairs of electrons.B) two bonding and two unshared pairs of electrons.

C) two bonding and one unshared pair of electrons.D) two double bonds and no unshared pairs of electrons.

E) none of the above

What is the correct Lewis structure for CO2?

A) : --:B) : ==:C) : = C=:D) : = C= :E) none of the above

The Lewis structure, [:-=] best represents:

A) NO2+B) NO2- C) NO2D) both NO2+ and NO2-E) answers A, B, and C

What is the correct Lewis structure for CN⁻?

A) [C-N]⁻B) [:-:]⁻C) [=:]⁻D) [: C≡ N :]⁻E) none of the above

The correct Lewis structure for BF3 would have exactly:

A) 1 double bond.B) 2 double bonds.C) 1 triple bond.D) no double bonds.E) none of the above

Which molecule below would have a Lewis structure that is an exception to the octet rule?

A) BH3B) NOC) SI6D) PF5E) all of these

What is the angle between electron groups in the linear electron geometry?

A) 90°B) 109.5°C) 120°D) 180°E) not enough information

What is the angle between electron groups in the trigonal planar electron geometry?

A) 90°B) 109.5°C) 120°D) 180°E) not enough information

What is the angle between electron groups in the tetrahedral geometry?

A) 90°B) 109.5°C) 120°D) 180°E) not enough information

What is the electron geometry if you have 4 electron groups around the center atom?

A) linearB) trigonal planarC) tetrahedralD) trigonal bipyramidal

E) not enough information

What is the electron geometry if you have 2 electron groups around the center atom?

A) linearB) trigonal planarC) tetrahedralD) trigonal bipyramidal

E) not enough information

What is the electron geometry if you have 3 electron groups around the center atom?

A) linearB) trigonal planarC) tetrahedralD) trigonal bipyramidal

E) not enough information

What is the molecular geometry if you have 3 single bonds and 1 lone pair around the central atom?

A) bentB) linearC) tetrahedralD) trigonal pyramidal

E) not enough information

What is the molecular geometry if you have 4 single bonds around the central atom?

A) bentB) linearC) tetrahedralD) trigonal pyramidal

E) not enough information

What is the molecular geometry if you have a double bond, a single bond and 1 lone pair around the central atom?

A) bentB) linearC) tetrahedralD) trigonal pyramidal

E) not enough information

Which of the following compounds would have a linear molecular geometry?

1. N22. H2S3. CO2

A) 1 and 2 onlyB) 1 and 3 onlyC) 2 and 3 onlyD) 1, 2 and 3E) neither 1, 2,or 3

What is the molecular geometry of carbon dioxide, ?