Chem 101 Final Review Baylon University of Idaho

Which of the following has 8 electrons in the outer shell?

A) Cl+

B) Fe3+

C) Ca2+

D) S2+

Ca2+

What is the oxidation state of chromium in the compound K2Cr2O7?

A) +7

B) -1

C) +6

D) +4

+6

Which atom in the compound K2C2O4 has a positive oxidation state?

A) potassium

B) both potassium and carbon

C) both potassium and oxygen

D) carbon

both potassium and carbon

Which atom(s) has a more positive oxidation state on the product side than the reactant side?

Fe2O3 + 3CO 2Fe + 3CO2

A) oxygen

B) carbon and iron

C) carbon

D) iron

carbon

In a chemical bond, which atom gets ownership the shared electrons?

A) the larger element

B) the most electropositive element

C) the more electronegative element

D) the smaller element

the more elecrtonegative element

The only element that is more electronegative than oxygen is ________.

A) sulfur

B) chlorine

C) nitrogen

D) fluorine

fluorine

Identify the compound that contains bromine with a +3 oxidation state.

A) NaBrO4

B) NaBrO

C) NaBrO3

D) NaBrO2

NaBrO2

Which of the following is true for the following reaction?

Cu + ZnCl2 CuCl2 + Zn

A) Zn+2 is reduced.

B) Cu is oxidized.

C) Cu is a reducing agent.

D) All of the above statements are correct.

All of the above statements

380 mm Hg is equal to ________ atm.

A) 5.0

B) 2.0

C) 20.0

D) 0.50

.50

How many moles of gas are found in a container that occupies a volume of 5.50 L with a pressure

of 0.335 atm at 25 °C?

A) 0.898 moles

B) 13.3 moles

C) 0.0753 moles

D) 1.11 moles

0.0753

A fixed amount of a gas has both its temperature and volume doubled. What happens to its

pressure? 11)

A) It remains the same.

B) It doubles.

C) It quadruples.

D) It is halved.

It remains the same

Assuming that the pressure and quantity of a gas sample remain constant, what will be the final

volume of a 4.86 L sample of a gas at 281 °C when it is heated to 300 °C?

A) 3.89 L

B) 2.92 L

C) 2.78 L

D) 5.03 L

5.03

Which statement is true for an ideal gas?

A) The pressure of a gas increases when the number of gas moles increases.

B) The pressure of a gas increases when its volume decreases.

C) The pressure of a gas increases when its temperature increases.

D) All of the above statements are correct

All of the above statements are correct

0.024 moles of nitrogen gas occupy 4.0 L at 0.90 atm pressure. What will be the final volume if the

container is allowed to expand and the pressure is reduced to 0.30 atm while the temperature is

kept constant?

A) 12 L

B) 6.0 L

C) 1.33 L

D) 3.6 L

12 L

A gas occupies 2.00 L at 298 K and 2.10 atm. The volume of this gas at STP is ________.

A) 22.4 L

B) 3.84 L

C) 2.00 L

D) 2.24 L

3.84 L

Which of the following gases will have the same density at STP?

A) carbon monoxide and nitrogen

B) hydrogen chloride and fluorine

C) oxygen and methane

D) hydrogen and helium

carbon monoxide and nitrogen

Solutions are considered to be which general type of matter?

A) pure elements

B) heterogeneous mixtures

C) homogeneous mixtures

D) pure substances

homogeneous mixtures

Which of the following solutions are possible?

A) The solvent is a liquid and the solute is a gas.

B) Both the solvent and solute are solids.

C) Both the solvent and solute are liquids.

D) All of them are possible

all of them are possible

Which of the following has the lowest hydration energy?

A) aluminum chloride

B) magnesium chloride

C) silicon tetrachloride

D) sodium chloride

sodium chloride

How are the solubilities of gases (solutes) in liquids (solvents) affected by changing pressure?

A) Gases are less soluble in liquids when the pressure is increased.

B) Gases are more soluble in liquids when the pressure is decreased.

C) Pressure has no effect on how soluble a gas is in a liquid.

D) Gases are more soluble in liquids when the pressure is increased.

gases are more soluble in liquids when the pressure is increased

Which of the following is the most water soluble at 50°C?

A) Ce2(SO4)3

B) CH3COONa

C) NaNO3

D) KBr

NaNO3

To prepare 100 mL of 0.4 M HCl solution from a stock solution of 2 M HCl solution one needs to

________.

A) dilute 20 mL of 2 M HCl solution with 100 mL of HCl solution.

B)dilute 20 mL of 2 M HCl solution with enough water to make a total volume of 100 mL of

solution.

C) dilute 80 mL of 2 M HCl solution to a total volume of 100 mL of solution.

D) use 500 mL of 2 M HCl solution and boil it down to a final volume of 100 mL of solution.

dilute 20 ml of 2 M HCl solution with enough water to make a total volume of 100 . ml of solution

25 mL of a 0.1 M NaCl solution contains ________ g of NaCl.

A) 0.15

B) 0.0025

C) 2.5

D) 0.25

0.15

7.5 g of calcium carbonate in 150 mL of aqueous solution will provide a ________ M

solution.

A) 0.50

B) 2.0

C) 0.10

D) 1.0

0.50

500 mL of a 0.4 M calcium nitrite contains ________ moles of calcium ions and ________ moles of

nitrite ions.

A) 0.4; 0.2

B) 0.2; 0.4

C) 0.4; 0.6

D) 0.2; 0.2

0.2; 0.4

Which of the three phases of matter (solid, liquid, or gas) has particles separated by the least

amount of distance?

A) solid

B) gas

C) liquid

D) The separation distance is about the same in all three phases

solid

A change of state from a gas to a liquid is called ________.

A) evaporation

B) melting

C) sublimation

D) condensation

condensation

Which of the following statements is true about intermolecular forces of attraction between

molecules?

A) They tend to hold molecules together.

B) The solidification of a substance usually requires lower temperatures than in the case of

liquefaction.

C) Cooling is responsible for the substance's liquefaction.

D) All of the above are true

all of the above are true

Which of the following chemical substances would you expect to have the lowest boiling point (you

may consider molecular mass and the degree of intermolecular forces as primary controlling

factors)?

A) CH4

B) CH3CH2CH3

C) CH3CH3

D) CH3CH2CH2CH3

CH4

Which of the following statements about London forces is correct? 5)

A) London forces are also called dispersion forces.

B) London forces occur between polar and nonpolar molecules.

C) London forces are relatively weakly attractive.

D) All the above statements are true.

All of the above

Polar molecules may exhibit ________.

A) dipole-dipole forces

B) London forces

C) hydrogen bonding

D) all of the above

all of the above

Which of the following experiences the strongest London forces?

A) carbon tetrachloride

B) helium

C) water

D) hydrogen

Carbon tetrachloride

Which of the following will have the lowest boiling point?

A) HOCH2-CH2OH

B) CH3CH2OH

C) CH3OCH3

D) CH3CH3

HOCH2-CH2OH

Which process absorbs energy?

A) bond formation

B) bond breaking

C) both A and B

D) none of the above

bond breaking

Which of the following has 6 as one of the coefficients when the equation is balanced?

A) Al(OH)3 + HCl AlCl3 + H2O

B) C2H6O +O2 CO2 + H2O

C) Mg + HCl H2 + MgCl2

D) H2SO4 + Al(OH)3 Al2(SO4)3 + H2O

H2SO4 + Al(OH)3----> Al2(SO4)3+ H20

What is the coefficient for iron after the following reaction is balanced?

Fe + O2 Fe2O3

A) 3

B) 6

C) 1

D) 4

4

What is the sum of all coefficients after the following equation is balanced?

C8H18 + O2 CO2 + H2O

A) 4

B) 61

C) 18

D) 32

61

What is the sum of all coefficients after the following equation is balanced?

K2CrO4 + Al(NO3)3 Al2(Cr O4)3 + KNO3

A) 15

B) 12

C) 4

D) 8

12

Which of the following is an example of a combination reaction?

A) 2 Na + Cl2 2NaCl

B) KClO3 KCl + O2

C) Mg + HCl H2 + MgCl2

D) HCl + NaOH NaCl + H2O

2 Na + Cl2 ---> 2NaCl

Which of the following equations is not a combustion reaction? A) CH4 + O2 CO + H2O

B) Fe + O2 FeO

C) KClO3 KCl +O2

D) C2H6O + O2 H2O + CO2

KClO3 ----> KCl + O2

When aqueous solutions of sodium phosphate and calcium nitrite are mixed, the spectator ions are

________.

A) sodium and phosphate

B) calcium and nitrite

C) calcium and phosphate

D) sodium and nitrite

Sodium and Nitrite

The following equation is an example of a ________ reaction.

AgNO3 + NaCl ----> AgCl + NaNO3

A) single replacement

B) decomposition

C) precipitation

D) combination

Precipitation

If the following ions Ba2+, Cl-, K+ and SO4

2- are placed in a test tube, the precipitate formed is

________.

A) BaCl2

B) K2SO4

C) BaSO4

D) KCl

BaSO4

The number of oxygen atoms in 1 mole of Al2(SO4)3 is ________.

A) 12

B) 3

C) 4

D) none of the above

None

The molar mass of Ca3(PO4)2 is ________.

A) 279

B) 310

C) 246

D) 215

310

The molar mass of a compound XClO3 is 106.5. The molar mass (rounded to the nearest whole

number) of X is ________, which is ________.

A) 23; Na

B) 39; K

C) 7; Li

D) 1; H

23, Na

Which reactant is the limiting reagent if 6 mol of H2 and 4 mol of O2 are used?

2H2 + O2 2H2O

A) O2

B) H2

C) neither H2 nor O2

D) both H2 and O2

H2

Which statement is true about the empirical formula?

A) The empirical formula is always different than the molecular formula.

B) The empirical formula may be different than the molecular formula.

C) The empirical formula is always the same as the molecular formula.

D) The empirical formula cannot be determined solely by the % composition.

The empirical formula may be different than the molecular formula

A certain compound is found to contain 1.45 g of Na, 2.05 g of S and 1.5 g of O. Its empirical

formula is ________.

A) NaSO2

B) Na2SO

C) NaS2O

D) Na2S2O3

Na2S2O3

If the empirical formula is CH2, and the molecular weight is equal to 180 ±10, then the molecular

formula is ________.

A) C14H21

B) C8H12O4

C) C13H26

D) C6H12O6

C13H26

Which color light is composed of photons having the largest energy? 1

A) yellow

B) red

C) green

D) blue

Blue

Calculate the energy in joules of microwave radiation of wavelength 12.7 centimeters.

(E = hΑ, h = 6.63 × 10-34 J.sec; speed of light = wavelength ×ȱΑ, speed of light = 3.0 × 108

meters/sec.)

A) 4.9 × 1019 J

B) 7.3 × 10-19 J

C) 1.6 × 10-24 J

D) 3.6 × 10-18 J

1.6 x 1--24 J

What is the main difference between "classical physics" and "quantum physics"?

A) Classical physics requires that only certain, allowed values for energy be used.

B)Quantum physics can only describe the behavior of very small objects, like atoms and

molecules.

C) Quantum physics requires the speed of light to be a constant value.

D) Quantum physics requires that only certain, allowed values for energy be used.

Quantum physics requires that only certain, allowed values for energy be used.

In a single atom, what is the maximum number of electrons that can have quantum number n = 4?

A) 14

B) 10

C) 32

D) 18

32

Which of the following subshells appear in the second shell? A) s, p, d

B) p

C) s, p

D) s

s, p

What is the maximum number of electrons in a 3p subshell?

A) 3

B) 5

C) 10

D) 6

6

Which of the following elements has the electronic configuration: 1s22s22p63s23p3? A) P

B) Al

C) S

D) Si

P

How many valence electrons are in silicon?

A) 4

B) 5

C) 7

D) 2

4

What is the number of outer shell electrons in fluorine? A) 2

B) 7

C) 5

D) 9

7

A non-metal is an element that tends to ________ valence electrons in chemical reactions, becoming

a(n) ________ in the process.

A) gain; anion

B) lose; anion

C) lose; cation

D) gain; cation

gain, anion

9) A metal is an element that tends to ________ valence electrons in chemical reactions, becoming

a(n) ________ in the process.

A) lose; anion

B) gain; cation

C) gain; anion

D) lose; cation

Lose, cation

Which of the following statements best describes an ionic bond?

A) the bonding type present in bound, non-metal atoms

B) the equal sharing of two electrons between adjacent atoms

C) a strong lattice of positively and negatively charged atoms held together by electrical forces

D) the bonding type present between two metal atoms

a strong lattice of positively and negatively charged atoms held together by electrical forces

Which of the following exists as a diatomic molecule? A) phosphorus

B) silicon

C) neon

D) oxygen

oxygen

The number of valence electrons in sulfur is ________.

A) 2

B) 4

C) 6

D) 8

6

Which of the following elements has the highest number of valence electrons?

A) lithium

B) phosphorus

C) argon

D) magnesium

Argon

Which of the following represents the correct Lewis dot structure for selenium (Se)? 16) A) B) C) D)

c

Which of the following has the same number of valence electrons as sulfur?

A) arsenic

B) oxygen

C) boron

D) nitrogen

Oxygen

) The expected formula between sodium and oxygen is ________.

A) NaO

B) Na2O

C) Na2O3

D) Na2O2

Na2O

Water has ________ covalent bonds and ________ lone pairs. A) 2; 4

B) 2; 6

C) 2; 2

D) 2; 0

2; 2

Which of the following anions has the lowest number of oxygen atoms per formula unit?

A) hydrogen phosphate

B) carbonate

C) perchlorate

D) dichromate

carbonate

In a molecule having four pairs of electrons around the central atom and a pyramidal shape, how

many bonding pairs of electrons does the central atom have?

A) 4

B) 2

C) 3

D) 1

3

Which of the following pictures best illustrates a tetrahedral shape for the molecule AB4?

B

The angle around boron in boron trifluoride is ________.

A) 60°

B) 109.5°

C) 90°

D) 120°

120 degrees

What is the molecular shape of CC14?

A) bent

B) linear

C) pyramidal

D) tetrahedral

tetrahedral

What is the steric number of the central atom in CH4?

A) 1

B) 2

C) 3

D) 4

4