Deck 2: Chemistry

Question 1

Which of the following pairs of compounds are allotropes?

A)CO₂ and CH₄
B)NH₄+ and NH₃
C)NaCl and LiCl
D)O₂ and O₃
E)Ne and Ar

Answer 1

O₂ and O₃

Question 2

What is the expected H-C-H bond angle in a molecule of CH4?

A)90 degrees
B)109.5 degrees
C)120 degrees
D)60 degrees
E)100 degrees

Answer 2

109.5 degrees

Question 3

Which of the following gases is the third most abundant in the Earth's atmosphere?

A)Oxygen
B)Argon
C)Nitrogen
D)Carbon dioxide
E)Radon

Answer 3

Argon

Question 4

A neutral element has a mass number of 23 and 12 neutrons. What is the identity of this element?

A)Sodium
B)Magnesium
C)Vanadium
D)Krypton
E)Iodine

Question 5

Which of the following is the correct molecular formula for hydrobromic acid?

A)HBrO
B)HBr
C)H₂Br
D)H₂OBr
E)H₂O₂Br

Question 6

Find the pH of the a 0.500M solution of the weak base Ammonia (NH₃). The K_b = 1.78*10^-5NH₃ +H₂O --> NH₄+ + OH^-

A)13.01
B)9)13
C)10.52
D)11.48
E)12.37

Question 7

What property of a metal refers to its ability to be hammered into sheets?

A)Ductility
B)Thermal conductivity
C)Electrical conductivity
D)Malleability
E)Density

Question 8

You are dissolving a gas in water. If the partial pressure of the gas is 1 atm, and the concentration is .5g per 50mL of solution, then what is the concentration of gas at 800mmHg? How many grams of gas are dissolved in the water now?

A)0.66g dissolved at a concentration of 0.013 g/mL
B)0.66 g dissolved at a concentration of 0.02 g/mL
C)0.5 g dissolved at a concentration of 0.013 g/mL
D)0)5 g dissolved at a concentration of 0.02 g/mL
E)1.0 g dissolved at a concentration of 0.02 g/mL

Question 9

Which of the following is the correct molecular formula for magnesium phosphate?

A)MgPOb₄
B)Mg₃(PO₄)₂
C)Mg(PO₄)₂
D)MgP
E)MgP₂

Question 10

Which of the following elements is most easily reduced?

A)Chlorine
B)Phosphorous
C)Sodium
D)Potassium
E)Lithium

Question 11

Which of the following is false about the ionic character of bonds?

A)Covalent bonds never have ionic character
B)Covalent bonds have some ionic character because not all electron sharing is equal
C)Due to partial ionic character, one atom in a covalent bond will have a partial positive charge
D)Due to partial ionic character, one atom in a covalent bond will have a partial negative charge
E)The ionic character of a bond is due to the polarity of the atoms in the bond.

Question 12

You have a closed container filled with 1L of pure air at STP. Assume that this air is made of only nitrogen (79%) and oxygen (21%). What are the partial pressures of nitrogen and oxygen in the box?Hint: X_N = P_N/PTotal= N_N/N_Total

A)P_N = 0.5 atm PO = 0.5 atm
B)P_N = 1.0 atm PO = 1.0 atm
C)P_N = .21 atm PO =.79 atm
D)P_N = .79 atm PO = .21 atm
E)P_N = .75 atm PO = .25 atm

Question 13

A fixed quantity of a gas undergoes a change in temperature from 100 K to 200 K and a change in pressure from 2 atm to 1 atm. After theses changes, the volume of the gas is

A)Half of the original volume
B)Unchanged
C)Twice the original volume
D)Four times the original volume
E)Eight times the original volume

Question 14

Which of the following elements is the most electronegative?

A)Cesium
B)Sodium
C)Lithium
D)Boron
E)Fluorine

Question 15

1)75 moles of NaCl are dissolved in 1.00 kg of water. What is the boiling point of this solution (k_b = .512 degrees C·kg/mol for water)?

A)101.79 degrees Celsius
B)100.00 degrees Celsius
C)98.21 degrees Celsius
D)102.22 degrees Celsius
E)100.50 degrees Celsius

Question 16

What is the order of reaction for the following equation?A + B --> 2C

A)Zero order
B)First order
C)Second order
D)Third order
E)Fourth order

Question 17

Calculate the bond dissociation energy in the following equation:CH₄(g) + 2O₂(g) --> CO₂(g) + 2H₂0 (g)Given the following:DH_f° C-H = 87 Kcal/molDH_f° O=O = 118 Kcal/molDH_f° C=O = 178 Kcal/molDH_f° O-H = 111 Kcal/mol

A)+584 KCal
B)+216 KCal
C)-584 KCal
D)-216 KCal
E)-228 KCal

Question 18

Which of the following sets of quantum numbers is impossible for an electron?

A)n = 4, l = 3, m_l = 2, s = ½
B)n = 2, l = 1, m_l = 2, s = -½
C)n = 3, l = 2, m_l = -1, s = ½
D)n = 4, l = 1, m_l = 1, s = -½
E)n = 2, l = 1, m_l = 1, s = ½

Question 19

Which of the following hybridizations would allow for the formation of one pi bond?

A)sp³
B)sp²
C)sp¹
D)sp
E)s²

Question 20

A cell placed in pure water has swelled. Why?

A)The cell was in an isotonic environment, so water flowed into it.
B)The cell was in a hypotonic environment, so water flowed into it.
C)The cell was in a hypertonic environment, so water flowed into it.
D)The cell was in a hypotonic environment, so water flowed out of it.
E)The cell was in a hypertonic environment, so water flowed out of it.

Question 21

Which of these elements is most likely to have the highest second ionization energy? Hint: think of Lewis structures.

A)Aluminum (Al)
B)Phosphorus (P)
C)Chlorine (Cl)
D)Magnesium (Mg)
E)Sodium (Na)

Question 22

One liter of hydrogen gas is placed in a vacuum. The emission spectrum of hydrogen shows a red line of wavelength 650 nm. What was the energy of the photon that released it?

A)2)9 * 10^-28 J
B)4)1 * 10^-31 J
C)2)9 * 10^-19 J
D)4)1 * 10^-19 J
E)2)9 * 10^-15 J

Question 23

When sodium acetate, NaCH₃COO, is added to water the resulting solution is basic. True or false?

Question 24

The following equation is under thermodynamic control. Assuming a temperature of 273K and using the provided information, find the K_eq:A + B --> CDG_f° (A) = -200 kJ/molDG_f° (B) = -100 kJ/molDG_f° (C) = -50 kJ/mol

A)K_eq = 1.46 * 10^-14
B)K_eq= 1.46 * 10^-38
C)K_eq = 1.46 * 10^-48
D)K_eq = 0.83 * 10^-27
E)K_eq = 0.83 * 10^-32

Question 25

Which of the following compounds contains a double bond?

A)C₂H₆
B)C₂H₄
C)C₃H₈
D)CH₄
E)C₄H₁₀

Question 26

H₂S + H₂O --> HS^- + H₃O⁺ In the reaction above, what is the conjugate base of H?S?

A)H₂O
B)HS^-
C)H₃O⁺
D)H₂S has no conjugate base
E)H₂S acts as its own conjugate base

Question 27

What term classifies a phase change from a solid directly to a gas?

A)Vaporization
B)Deposition
C)Effervesence
D)Fusion
E)Sublimation

Question 28

Which of the following molecules does not display hydrogen bonding in the liquid phase?

A)H₂O
B)CH₃CH₂NH₂
C)CH₄
D)NH₃
E)HF

Question 29

Which of the following elements is the most electronegative?

A)Boron
B)Lithium
C)Potassium
D)Oxygen
E)Cesium

Question 30

Which of the following molecules acts as a Lewis acid?

A)HCl
B)SO₄^2-
C)CCl₄
D)H₃PO₄
E)BH₃

Question 31

Which of the following elements exists as a liquid at 25 degrees Celsius?

A)Silicon
B)Chlorine
C)Boron
D)Arsenic
E)Mercury

Question 32

How many molecules are in .275 grams of SO₃?

A)3)22x10²⁰
B)4)50x10²¹
C)2)07x10²¹
D)1)12x10²⁰
E)4)56x10²²

Question 33

Which of the following molecules displays planar geometry?

A)NH₃
B)BH₃
C)XeO₄
D)CH₄
E)SiF₆

Question 34

What volume of .250 M potassium hydroxide is needed to neutralize 1.25 liters of .500 M hydrochloric acid?

A)2)50 liters
B)1)25 liters
C))625 liters
D))375 liters
E)5)0 liters

Question 35

Which of the following conditions guarantees that a reaction will occur spontaneously in the forward direction?

A)The temperature is negative
B)Change in enthalpy is positive
C)Change in entropy is negative
D)Change in Gibbs free energy is negative
E)Change in temperature is positive

Question 36

What is the concentration of H⁺ ions in a solution that has an OH^- concentration of 1x10^-4molar?

A)1x10^-10 molar
B)1x10^-9 molar
C)1x10^-8 molar
D)1x10^-5 molar
E)1x10^-4 molar

Question 37

Ag⁺(aq) + e- --> Ag(s)In an electrolytic cell, where could this chemical reaction occur?

A)Anode
B)Cathode
C)Salt bridge
D)In solution
E)This reaction could not occur in an electrolytic cell

Question 38

Electrolysis requires energy input to force a non-spontaneous reaction to occur. True or false?

Question 39

Which of the following elements has the largest atomic radius?

A)Lithium
B)Boron
C)Fluorine
D)Potassium
E)Rubidium

Question 40

Which pair of elements and/or ions is isoelectronic?

A)F^- and Cl^-
B)O and Na
C)K⁺ and Ar
D)Mg²⁺ and S
E)Br and Kr

Question 41

Cu + 2AgNO₃--> 2Ag + Cu(NO₃)₂In the reaction above, which element is oxidized?

A)Cu
B)Ag
C)N
D)O
E)Oxidation does not occur in this reaction

Question 42

____CH₃OH(l) + _____O₂(g) --> _____CO₂(g) + _____H₂O(g)What set of coefficients correctly balances this equation?

A)2, 3, 2, 1
B)1, 2, 2, 1
C)2, 3, 4, 2
D)2, 3, 3, 4
E)2, 3, 2, 4

Question 43

2SO₂(g) + O₂(g) --> 2SO₃(g)What is the correct rate law for this reaction?

A)r = k[SO₂][O₂]
B)r = k[SO₃]
C)r = k[SO₂]²[O₂]
D)r = k[SO₃]²
E)r = k[SO₃][SO₂][O₂]

Question 44

80)0 grams of NaOH is dissolved in 3.0 moles of H?0. What is the mole fraction of NaOH in this solution?

A))20
B))37
C))40
D))64
E))79

Question 45

NH₃(g) + CuO(s) --> N₂(g) + Cu(s) + H₂O(g)What set of coefficients correctly balances the above equation?

A)3, 3, 1, 2, 3
B)3, 2, 1, 2, 2
C)2, 3, 1, 3, 3
D)1, 2, 3, 2, 2
E)3, 2, 1, 2, 3

Question 46

Which of the following elements displays bonding characterized by a delocalized "sea of electrons?"

A)Fluorine
B)Nitrogen
C)Copper
D)Sulfur
E)Argon

Question 47

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

A)[Ar] 4s²3d⁹
B)[Ar] 4s¹3d¹⁰
C)[Ar] 3s²3d⁹
D)[Ar] 3s¹3d¹⁰
E)[Kr] 4s²3d⁹

Question 48

Which of the following laws states that it is impossible to known the position and momentum of an electron simultaneously?

A)Pauli exclusion principle
B)Heisenberg's uncertainty principle
C)Hund's rule
D)Grahm's law
E)Ampere's law

Question 49

What is the percentage carbon by mass of glucose, C₆H₁₂O₆?

A)14.7 percent
B)40.0 percent
C)6)7 percent
D)19.2 percent
E)59.9 percent

Question 50

What element has isotopes known as deuterium and tritium?

A)Bromine
B)Helium
C)Oxygen
D)Hydrogen
E)Chlorine