STRAIGHTERLINE CHEMISTRY FINAL EXAM TEST WITH COMPLETE SOLUTIONS LATEST UPDATE 2023- 2024, Exams of Chemistry

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STRAIGHTERLINE CHEMISTRY FINAL EXAM TEST

WITH COMPLETE SOLUTIONS LATEST UPDATE 2023-

2024 GUARANTEED PASS!!

What is the term used for findings that are summarized based on a pattern or trend? a. Law b. Hypothesis c. Theory d. Phenomena e. Prediction

a. Law

Which of the following is a tentative explanation for a set of observations? Select one: a. Law b. Hypothesis c. Theory d. Phenomena e. Prediction

b. Hypothesis

If a liquid contains 60% sugar and 40% water throughout its composition then what is it called? Select one: a. Solute b. Compound c. Homogeneous mixture d. Heterogeneous mixture e. Solvent

c. Homogeneous mixture

Which of the following does not have a uniform composition throughout? Select one: a. Element b. Compound c. Homogeneous mixture d. Heterogeneous mixture e. Solvent

d. Heterogeneous mixture

Which one of these represents a physical change? Select one: a. Water, when heated, forms steam. b. Bleach turns hair yellow. c. Sugar, when heated, becomes brown. d. Milk turns sour. e. Apples, when exposed to air, turn brown.

a. Water, when heated, forms steam.

How many micrograms are in 65.3 kg? Select one: a. 0.653 μg b. 6.53 × 107 μg c. 6.53 × 104 μg d. 6.53 × 10-8 μg e. 6.53 × 1010 μg

e. 6.53 × 1010 μg

A smart phone has dimensions of 4.9 inches (height), 2.3 inches (width) and 8.0 millimeters (depth). What is the volume of the smart phone in cubic centimeters? (1 in = 2.54 cm) Select one: a. 58 cm b. 1.7 x 105 cm c. 90 cm d. 3.4 cm e. 34 cm

a. 58 cm

Given that 1 inch = 2.54 cm, 1.00 cm3 is equal to Select one: a. 16.4 in b. 6.45 in c. 0.394 in d. 0.155 in e. 0.0610 in

e. 0.0610 in

What terms defines a mass which is exactly equal to 1/12 the mass of one carbon-12 atom?

Select one: a. Isotope number b. Mass number c. Mass-to-charge ratio

d. Atomic number e. Atomic mass unit

e. Atomic mass unit

How many neutrons are there in an atom of lead whose mass number is 208?

Select one: a. 82 b. 126 c. 208 d. 290 e. none of them

b. 126

Which of these elements is chemically similar to magnesium?

Select one: a. Sulfur b. Calcium c. Iron d. Nickel e. Potassium

b. Calcium

C(graphite) and C(diamond) are examples of:

Select one: a. isotopes of carbon. b. allotropes of carbon. c. the law of definite proportions. d. different carbon ions.

b. allotropes of carbon.

The 80Br- ion has

Select one: a. 45 protons, 35 neutrons, 45 electrons. b. 35 protons, 45 neutrons, 34 electrons. c. 35 protons, 45 neutrons, 36 electrons. d. 45 protons, 35 neutrons, 46 electrons. e. 35 protons, 45 neutrons, 46 electrons.

e. 35 protons, 45 neutrons, 46 electrons.

The formula for sodium sulfide is Select one: a. NaS b. K2S c. NaS d. Na2S e. SeS

d. Na2S

Which one of the following formulas of ionic compounds is the least likely to be correct? Select one: a. NH4Cl b. Ba(OH) c. Na2SO d. Ca2NO e. Cu(CN)

d. Ca2NO

What is the name of ClO - ion? Select one: a. hypochlorite b. chlorate c. chlorite d. perchlorate e. perchlorite

a. hypochlorite

Which of the following is a molecular formula for a compound with an empirical formula of CH? Select one: a. C2H b. C3H c. C4H d. C6H e. None of the answers is correct.

d. C6H

Which is the correct electron configuration for gold?

Select one: a. [Xe]4f145d96s b. [Xe]4f145d106s c. [Xe]4f135d106s

d. [Xe]4f145d106s e. None of the electron configurations is correct.

d. [Xe]4f145d106s

A(n) _________ is a point at which a standing wave has zero amplitude. Select one: a. crevice b. node c. pit d. burrow e. orbital

b. node

The Pauli exclusion principle states that no ____ electrons within an atom can have the same ____ quantum numbers. Select one: a. 4; 6 b. 2; 4 c. 3; 6 d. 6; 10 e. 3; 8

b. 2; 4

Emission spectra

Select one: a. cannot be used to identify an unknown atom. b. can be used to identify unknown atoms. c. can be explained by the movement of protons colliding with electrons. d. none of the.

b. can be used to identify unknown atoms.

Which one of the following equations correctly represents the process relating to the ionization energy of X? Select one: a. X(s) → X+(g) + e- b. X2(g) → X+(g) + X-(g) c. X(g) + e- → X-(g) d. X-(g) → X(g) + e- e. X(g) → X+(g) + e-

e. X(g) → X+(g) + e-

Consider the element with the electron configuration [Kr]5s24d105p5. This element is Select one:

a. a halogen. b. a transition metal. c. an alkali metal. d. an actinide element. e. a noble gas.

a. a halogen.

Consider the element with the electron configuration [Kr]5s24d7. This element is Select one: a. a halogen. b. a transition metal. c. a nonmetal. d. an actinide element. e. a noble gas.

b. a transition metal.

How does atomic radius change as you move across the periodic table? Select one: a. Atomic radius decreases moving from left to right across a period and increases from top to bottom. b. Atomic radius increases moving left to right across a period and decreases from top to bottom. c. Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy. d. Atomic radius increases diagonally across the periodic table. e. None of the answers is correct.

a. Atomic radius decreases moving from left to right across a period and increases from top to bottom.

Which of these choices is the electron configuration of the iron(III) ion? Select one: a. [Ar]3d b. [Ar]4s13d c. [Ar]4s23d d. [Ar]3d e. [Ar]4s23d

a. [Ar]3d

An element with the general electron configuration for its outermost electrons of ns2np1 would be in which element group? Select one: a. 2A b. 3A c. 4A d. 5A e. 8A

b. 3A

The effective nuclear charge for an atom is less than the actual nuclear charge due to Select one: a. shielding. b. penetration. c. paramagnetism. d. electron-pair repulsion. e. relativity.

a. shielding.

Which pair of ions exhibits the greatest attractive force between them? Select one: a. Na+ and Cl- b. Ca2+ and Cl- c. Na+ and S2- d. Al3+ and Mg2+ e. Mg2+ and O2-

e. Mg2+ and O2-

Which of the following is a basic oxide?

Select one: a. P4O b. MgO c. Al2O d. SO e. Cl2O

b. MgO

Which of these compounds is most likely to be covalent? Select one: a. Rb2S b. SrCl c. CS d. CaO e. MgI

c. CS

In the Lewis structure of the iodate ion, IO3-, that satisfies the octet rule, the formal charge on the central iodine atom is

Select one: a. 2. b. 1. c. 0.

d. -1. e. -2.

a. 2.

Which molecule has the largest dipole moment?

Select one: a. HF b. HI c. HBr d. HCl e. All of the molecules have the same dipole moment.

a. HF

In which of the following species does the central atom violate the octet rule?

Select one: a. CH b. SF c. PCl4+ d. CCl3+ e. NH

b. SF

Which of these ionic solids would have the largest lattice energy? Select one: a. NaCl b. NaF c. CaBr d. CsI e. CaCl

e. CaCl

The total number of bonding electrons in a molecule of formaldehyde (H2CO) is

Select one: a. 3. b. 4. c. 6. d. 8. e. 18.

d. 8.

Which of the following molecules has a nonzero dipole moment? Select one: a. BeCl b. SF c. KrF d. CO e. CCl

b. SF

According to the VSEPR model, a molecule with the general formula AB5 with one lone pair on the central atom will have a ______ molecular geometry. Select one: a. tetrahedral b. trigonalbipyramidal c. square pyramidal d. octahedral e. seesaw

c. square pyramidal

Which is the most reasonable prediction for the three F-Br-F bond angles in BrF3? Select one: a. 90°, 90°, and 180° b. 86°, 94°, and 180° c. 86°, 86°, and 172° d. 94°, 94°, and 172° e. 120°, 120°, and 120°

c. 86°, 86°, and 172°

When PCl5 solidifies it forms PCl4+cations and PCl6- anions. According to valence bond theory, what hybrid orbitals are used by phosphorus in the PCl4+cation? Select one: a. sp b. sp c. sp d. sp3d e. sp3d

c. sp

What is the number of lone electron pairs on the central atom of a molecule having a trigonal pyramidal molecular geometry, such as NH3? Select one: a. 1

b. 2 c. 3 d. 0 e. 4

a. 1

For which one of the following molecules is the indicated type of hybridization not appropriate for the central atom? Select one: a. BeCl2; sp b. SiH4; sp c. BF3; sp d. C2H2; sp e. H2O; sp

a. BeCl2; sp

According to the VSEPR model, the predicted molecular geometry of ammonia, NH3, is Select one: a. linear. b. trigonal planar. c. bent. d. tetrahedral. e. trigonal pyramidal.

e. trigonal pyramidal.

What is the mass of one copper atom? (NA = 6.022 × 1023 mol-1) Select one: a. 1.055 × 10-22 g b. 63.55 g c. 1 amu d. 1.66 × 10-24 g e. 9.476 × 1021 g

a. 1.055 × 10-22 g

What is the percent sulfur in iron(III) sulfate? Select one: a. 28% b. 32% c. 24% d. 48% e. 42%

c. 24%

Proteins found in humans are polymers that consist of different combinations of 20 amino acids. Proline, one of the 20 amino acids, has the molecular formula, C5H9NO2. If a human protein has 25 proline monomers, how many carbon atoms from proline are present in the protein?

Select one: a. 4 C atoms b. 25 C atoms c. 40 C atoms d. 100 C atoms e. 125 C atoms

e. 125 C atoms

Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al2O3.

Select one: a. 2.377 mol b. 2.146 mol c. 1.105 mol d. 0.4660 mol e. 0.4207 mol

d. 0.4660 mol

Once the following equation is balanced with the smallest set of whole number coefficients, what is the sum of the coefficients? (Don't forget to include coefficients of one.)

__ SF4 + __ H2O → __ H2SO3 + __ HF Select one: a. 4 b. 6 c. 7 d. 9 e. None of these answers is correct.

d. 9

What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum according to the chemical equation below?

2Al + Cr2O3 → Al2O3 + 2Cr Select one: a. 7.7 g b. 15.4 g c. 27.4 g

d. 30.8 g e. 49.9 g

b. 15.4 g

Which one of the following is a strong acid? Select one: a. CH3COOH b. H2SO c. NH d. H3PO e. HClO

e. HClO

Which is a Lewis acid? Select one: a. CH3NH b. BCl c. F- d. BF4- e. CH

b. BCl

Which is an amphoteric oxide? Select one: a. Na2O b. MgO c. Al2O d. SO e. Cl2O

c. Al2O

What is the value of the equilibrium constant for the autoionization of water at 25°C? Select one: a. 1.0 × 10- b. 1.0 × 10- c. 1.0 × 1014 d. 1.0 × 107 e. 14

b. 1.0 × 10-

Which is the strongest acid? Select one: a. SO42- b. H2SO

c. H2SO d. HSO4- e. HSO3-

C. H2SO

In the van der Waals equation, the constant b is a constant that is part of a correction factor for _________. Select one: a. the volume of the gas b. the temperature of the gas c. the pressure of the gas d. the ideal gas constant

a. the volume of the gas

A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the pressure is increased to 894 torr at constant temperature? Select one: a. 22.3 L b. 31.2 L c. 44.9 L d. 112 L e. 380 L

b. 31.2 L

If the atmospheric pressure in Denver is 0.8800 atm, what is this pressure expressed in mmHg? (1 atm = 101,325 Pa = 760 torr, 1 torr = 1 mmHg)? Select one: a. 151.5 mmHg b. 1.16 × 10-3 mmHg c. 863.6 mmHg d. 8.92 × 104 mmHg e. 668.8 mmHg

e. 668.8 mmHg

What are the conditions of STP? Select one: a. 0 K and 1 atm b. 273.15 K and 760 torr c. 0°C and 760 atm d. 273.15°C and 760 torr e. 0°C and 1 torr

b. 273.15 K and 760 torr

In the van der Waals equation, the constant a is a constant that is part of a correction factor for _________. Select one: a. the volume of the gas b. the temperature of the gas c. the pressure of the gas d. the ideal gas constant

c. the pressure of the gas

Which substance will exhibit hydrogen bonding between molecules? Select one: a. (CH3)3N b. CH3-O-CH c. CH3CH2-OH d. CH3CH2-F e. HI

c. CH3CH2-OH

Which of the following statements is true? Select one: a. The higher the viscosity, the faster a liquid flows. b. The viscosity increases with increasing temperature. c. The stronger the intermolecular forces, the higher the viscosity. d. Hydrogen bonding in water gives rise to its unusually low viscosity. e. The viscosity of gases is larger than the viscosity of liquids.

c. The stronger the intermolecular forces, the higher the viscosity.

If liquid bromine is cooled to form a solid, which type of solid does it form? Select one: a. atomic b. metallic c. molecular d. ionic e. covalent

c. molecular

In a sample of hydrogen iodide, __________________ are the most important intermolecular forces. Select one: a. dipole-dipole forces b. London dispersion forces c. hydrogen bonding d. covalent bonds e. polar covalent bonds

a. dipole-dipole forces

Krypton has a higher melting point than argon because of its Select one: a. hydrogen bonding. b. stronger dispersion forces. c. permanent dipole moment. d. ionic bonds. e. greater ionization energy.

b. stronger dispersion forces.

Lead crystallizes in the face-centered cubic lattice. What is the coordination number for Pb? Select one: a. 4 b. 6 c. 8 d. 10 e. 12

e. 12

What states that the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution? Select one: a. Entropy b. Henry's law c. Dissolution d. Vapor pressure e. Enthalpy of salvation

b. Henry's law

Which of the following pairs of liquids is least likely to be miscible?

Select one: a. Hexane-heptane b. Hexane-benzene c. Hexane-acetic acid d. Hexane-diethyl ether e. Acetic acid-acetone

c. Hexane-acetic acid

What is the name given to a solution that contains less solute than it has the capacity to dissolve? Select one: a. Unsaturated

b. Saturated c. Solvented d. Oversaturated e. Supersaturated

a. Unsaturated

An emulsion is a dispersion consisting of a Select one: a. solid in a liquid. b. liquid in a liquid. c. gas in a liquid. d. liquid in a solid. e. gas in a solid.

b. liquid in a liquid.

Which is true regarding the solvation of a solute in a solvent?

Select one: a. Separation of solute molecules from one another is an endothermic process, and separation of solvent molecules from one another is an exothermic process. b. Separation of solute molecules from one another is an exothermic process, and separation of solvent molecules from one another is an endothermic process. c. Separation of solute molecules from one another, and separation of solvent molecules from one another, are both endothermic processes. d. Separation of solute molecules from one another, and separation of solvent molecules from one another, are both exothermic processes. e. Separation of solute molecules from one another, and separation of solvent molecules from one another, both result in a decrease in entropy.

b. Separation of solute molecules from one another is an exothermic process, and separation of solvent molecules from one another is an endothermic process.

What name is given to a minor component in a solution? Select one: a. Solvent b. Unsaturated c. Saturated d. Solute e. Supersaturated

d. Solute

Which compound has the lowest solubility in pure water? Select one: a. Ag2C2O4, Ksp = 1.0 × 10- b. PbCl2, Ksp = 1.7 × 10-

c. FePO4, Ksp = 1.3 × 10- d. Ca3(PO4)2, Ksp = 1.2 × 10- e. MgF2, Ksp = 6.9 × 10-

c. FePO4, Ksp = 1.3 × 10-

What happens to the solution if sodium acetate is added to a solution of acetic acid? CH3COOH(aq) Picture H+(aq) + CH3COO-(aq) Select one: a. The equilibrium shifts to the right. b. There is an increase in percent ionization of acetic acid. c. Less of hydrogen ion is consumed. d. There is an increased concentration of acetate ions. e. Less of the acetate ion is consumed.

d. There is an increased concentration of acetate ions.

Which is more soluble in an acidic solution than in pure water? Select one: a. CuI b. PbCl c. Ca3(PO4) d. NaNO e. NaBr

c. Ca3(PO4)

What is the name of the principle of selective precipitation used to identify the types of ions present in a solution? Select one: a. Ionization b. Selective ion precipitation c. Selective ion typing d. Limited precipitation e. Qualitative analysis

e. Qualitative analysis

Methyl red is a common acid-base indicator. It has a Ka equal to 6.3 × 10-6. Its un-ionized form is red and its anionic form is yellow. What color would a methyl red solution have at pH = 7.8? Select one: a. green b. red c. blue d. yellow e. violet

d. yellow

When a strong acid is titrated with a weak base, the pH at the equivalence point Select one: a. is greater than 7.0. b. is equal to 7.0. c. is less than 7.0. d. is equal to the pKa of the conjugate acid. e. is equal to the pKb of the base.

c. is less than 7.0.

Which is necessary for a process to be spontaneous? Select one: a. ΔHsys < 0 b. ΔSsys > 0 c. ΔSsurr < 0 d. ΔSuniv > 0 e. ΔGsys = 0

d. ΔSuniv > 0

As the molar mass of a compound increases, the entropy ______. Select one: a. decreases b. is constant c. increases

c. increases

The most probable state is the one with the _______. Select one: a. highest energy b. largest number of possible arrangements c. lowest number of possible arrangements d. most symmetry e. highest enthalpy

b. largest number of possible arrangements

A spontaneous endothermic reaction always Select one: a. causes the surroundings to get colder. b. bursts into flame. c. requires a spark to initiate it. d. releases heat to the surroundings.

a. causes the surroundings to get colder.

Which of the following is used to image the brain? Select one: a. 18O b. 131I c. 123I d. 24Na e. 99Tc

c. 123I

Which of the following is an advantage of nuclear power plants over coal-burning plants? Nuclear power plants Select one: a. form numerous radioactive fission products. b. do not pollute the air with SO2, soot, and fly-ash. Correct c. produce more thermal pollution than coal plants. d. use more fuel.

b. do not pollute the air with SO2, soot, and fly-ash.

Which isotope, when bombarded with nitrogen-15, yields four neutrons and the artificial isotope dubnium-260? Select one: a. Californium- b. Thorium- c. Nobelium- d. Californium- e. Dubnium-

d. Californium-

Which isotope, when bombarded with bismuth-209, would yield two neutrons and an isotope with atomic number 121 and mass number 299?

Select one: a. Pb- b. Po- c. Sr- d. Rn- e. Sr-

c. Sr-

Which name could correspond to the following coordination compound, where M represents a transition metal cation and L represents a ligand?

Picture

Select one: a. Hexachloroferrate(III) b. Hexaammineiron(III) c. Hexaaquochromium(II) d. Hexacyanomanganate(II) e. All of the above are possible.

e. All of the above are possible

Ethylenediaminetetraacetic acid (EDTA) is Select one: a. not useful as a chelating agent. b. an effective antidote for heavy metal poisoning (e.g., Pb2+ and Hg2+). c. a monodentate ligand. d. known to form unstable complex ions with Fe3+, Hg2+, and Zn2+. e. known to form complexes with platinum that inhibit the growth of cancerous cells.

b. an effective antidote for heavy metal poisoning (e.g., Pb2+ and Hg2+).

In the coordination compound [Pt(NH3)2Cl2], the coordination number and oxidation number of the central atom are_____ and _____, respectively.

Select one: a. 2; 0 b. 4; + c. 5; 0 d. 4; + e. 6; +

d. 4; +

What is the systematic name for [CoCl3(H2O)]-? Select one: a. cobalt(III) chloride monohydrate b. aquatrichlorocobalt(II) c. aquatrichlorocobaltate(II) d. aquatrichlorocobaltite(I) e. monoaquotris(chloro)cobalt(IV)

c. aquatrichlorocobaltate(II)

In K4[Fe(CN)6], how many 3d electrons does the iron atom have? Select one: a. 3 b. 4 c. 5

d. 6 e. 7

d. 6

Write the formula for diamminedichloroethylenediaminecobalt(III) bromide. Select one: a. [CoCl2(en)(NH3)2]Br b. [CoCl2(en)(NH3) 2]Br2 c. [CoCl2(en)2(NH3)2]Br d. [CoCl2(en)2(NH3)2]Br2 e. (NH3)2Cl2(en)Co3Br

a. [CoCl2(en)(NH3)2]Br

In the complex ion [Co(en)2Br2]+, what is the oxidation number of Co? Select one: a. +1 b. +2 c. +3 d. -2 e. -1

c. +3

In which type of isomerism is there restricted rotation around a bond? Select one: a. Stereoisomers b. Geometrical isomers c. Constitutional isomers d. Conformational isomers e. Connectivity isomers

b. Geometrical isomers

What name is given to a compound containing a -CONH2 group? Select one: a. Aldehyde b. Amine c. Amide d. Carboxylic acid e. Ester

c. Amide

Bromination of benzene (C6H6), an aromatic compound, Select one: a. occurs by substitution rather than addition. b. occurs by addition rather than substitution.

c. occurs more rapidly than bromination of a nonaromatic compound. d. results in the formation of 1,2,3,4,5,6-hexabromocyclohexane. e. occurs in the absence of a catalyst.

a. occurs by substitution rather than addition.

The density of a substance is an intensive property.

Select one: True False

True

The rusting of a piece of iron under environmental conditions is a physical change.

Select one: True False

False

77 K is colder than 4 K.

Select one: True False

False

Zero kelvin 0 K < 0°F < 0°C

Select one: True False

True

The number 6.0448, rounded to 3 decimal places, becomes 6.045.

Select one: True False

True

A scoop of vanilla ice cream is a pure substance.

Select one:

True False

False

The juice from an orange is a mixture.

Select one: True False

True

The ripening of fruit, once picked, is an example of physical change.

Select one: True False

False

A particular temperature in degrees Celsius is larger than the temperature in kelvins.

Select one: True False

False

Matter is anything that has mass and occupies space.

Select one: True False

True

Elements in which the outermost electron has the same principal quantum number, n, show similar chemical properties.

Select one: True False

False

Atomic size decreases across a period due to an increase in the effective nuclear charge, Zeff.

Select one:

True False

True

The radii of ions are always smaller than the radii of the corresponding atoms of the same element.

Select one: True False

False

The electron configuration of atomic argon is the same as the chloride ion (Cl-).

Select one: True False

True

Moseley's measurements of nuclear charges of the elements provided the basis for arranging the elements of the periodic table in order of increasing atomic number.

Select one: True False

True

Only valence electrons are shown in the Lewis structure held together by covalent bonds.

Select one: True False

True

Unshared electrons are always shown in pairs around an atom.

Select one: True False

False

Lewis theorized the octet rule to describe chemical bonding where atoms lose, gain, or share electrons in order to achieve a noble gas configuration.

Select one:

True False

True

Ionic compounds tend to form between metals and nonmetals when electrons are transferred from an element with high ionization energy (metal) to an element with a low electron affinity (nonmetal).

Select one: True False

False

When an alkali metal combines with a nonmetal, a covalent bond is normally formed.

Select one: True False

False

The empirical formula is the simplest whole number ratio of atoms representing a chemical formula of a molecule.

Select one: True False

True

Many compounds can be represented with the same empirical formula.

Select one: True False

False

The molecular formula is a whole number multiple of the empirical formula.

Select one: True False

True

There is only one distinct empirical formula for each compound that exists.

Select one: