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General Chemistry Flashcards

1
Q

Mass _________
A. has the SI unit of pounds.
B. is the amount of matter that occupies space.
C. is the quantitative measure of acceleration, a fundamental property of all matter.
D. constitutes the force exerted on matter by the gravitational attraction of Earth, and so it varies slightly from place to place.

A

B

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2
Q

Which of the following is described as having components that CANNOT be physically separated?
A. mixture
B. solution
C. suspension
D. pure substance

A

D

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3
Q

Which of the following is TRUE?
A. Compounds have only one type of atom.
B. Elements can be chemically decomposed.
C. Solutions are considered as pure substances.
D. Heterogeneous mixtures have phase boundaries.

A

D

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4
Q

Mothballs are used as deodorizer and as pesticides. Upon exposing them in air for a few hours, they disappeared. Which of the following BEST explains the scenario?
A. It underwent sublimation.
B. It melted then vaporized.
C. It reacted with something in the air.
D. None of the above.

A

A

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5
Q

Which does NOT indicate a chemical change?
A. change in color
B. increase in temperature
C. change in shape
D. evolution of gas

A

C

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6
Q

Which of the following is an extensive property of matter?
A. density
B. viscosity
C. freezing point
D. number of moles

A

D

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7
Q

Which of the following is an intensive property?
A. density
B. melting point
C. electric potential
D. all of the above

A

D

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8
Q

The standard pressure of the atmosphere at sea level is
A. 1 atm
B. 760 mmHg
C. 760 torr
D. all of the above

A

D

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9
Q

The flasks (1-4), increasing in size, contains the same number of molecules. In which flask is pressure the highest?
A. flask 2
B. flask 1
C. flask 3
D. flask 4

A

B

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10
Q

What is the molar mass of an unknown gas if 1.60 g of the gas occupies a volume of 2.24 L at STP?
A. 35.8 g/mol
B. 160 g/mol
C. 16.0 g/mol
D. 81.0 g/mol

A

C

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11
Q

Which of the following is TRUE for C-13 isotope?
A. It has 6 neutron and 7 protons.
B. It has 6 protons and 7 neutrons.
C. It has 6 neutron and 13 protons.
D. It has 6 protons and 13 neutrons.

A

B

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12
Q

What is the most common isotope of Hydrogen?
A. Hydrogen only has one isotope
B. Deuterium
C. Tritium
D. Protium

A

D

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13
Q

From left to right in a periodic table
A. atomic radius increases
B. ionization energy decreases
C. electronegativity increases
D. none of the above

A

C

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14
Q

Which of the following atoms is the largest? a
A. Cesium
B. Strontium
C. Gallium
D. Arsenic

A

A

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15
Q

Chromium is a member of which of the following?
A. Actinides
B. Lanthanides
C. Alkali metals
D. Transition metals

A

D

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16
Q

Fluorine is capable of forming covalent bonds with which of the following element?
A. Zinc
B. Boron
C. Lithium
D. Calcium

A

B

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17
Q

Which is NOT an acceptable name for Hg2Cl?
A. Mercury(II) chloride
B. Mercury(I) chloride
C. Mercurous chloride
D. Dimercury dichloride

A

A

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18
Q

Noble gases are unreactive because they have complete outer electron shells. Which of the following elements is NOT a noble gas?
A. Chlorine
B. Krypton
C. Helium
D. Argon

A

A

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19
Q

What is the chemical formula of diphosphorus monobromide?
A. PBr2
B. PBr
C. P2Br2
D. P2Br

A

D

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20
Q

Sodium carbonate is also known as?
A. baking soda
B. soda ash
C. caustic potash
D. caustic soda

A

B

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21
Q

All of these elements are strict followers of the octet rule, EXCEPT
A. Boron
B. Carbon
C. Nitrogen
D. Oxygen

A

A

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22
Q

Which of the following does NOT describe a nonpolar bond?
A. It is a bond between similar nonmetals.
B. It is a bond between different nonmetals.
C. It has a dipole moment.
D. All describes a nonpolar bond.

A

C

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23
Q

Which of the following statements is TRUE?
A. Double bonds are shorter than triple bonds.
B. Double bonds are stronger than triple bonds.
C. Single bonds have lower energy than double bonds.
D. None of the statements above is true

A

C

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24
Q

Which of the following covalent compounds has a tetrahedral geometry?
A. CH4
B. NH3
C. H20
D. BF3

A

A

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25
Q

Which of the following is a polar molecule?
A. CO2
B. SF4
C. CCl4
D. XeF4

A

B

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26
Q

Polar molecules include which of the following?
I. CO2 II. COCl2 Ill. CH2Cl2
A. I only
B. I and Il only
C. l and Ill only
D. II and IIl only

A

D

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27
Q

Which of the following is NOT an indication of strong IMFA?
A high viscosity
B. high volatility
C. high boiling point
D. high melting point

A

B

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28
Q

What is the principal intermolecular force that must be overcome when hexane is vaporized?
A. Hydrogen bonding
B. Covalent bonding between carbons
C. Dipole-dipole forces
D. London dispersion forces

A

D

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29
Q

Which compound has the strongest intermolecular forces of attraction?
A. CO
B. CH4
C. CH3OH
D. CH3OCH3

A

C

30
Q

A polar solute dissolves in a polar solvent and a nonpolar solute dissolves in a nonpolar solvent. This is the ________
A. Hund’s rule
B. Henrys law
C. solubility rule
D. ‘like dissolves like’ rule

A

D

31
Q

Tin(II) fluoride (156.7 g/mol) is often added to toothpaste as an ingredient to prevent tooth decay. What is the mass of fluoride (19 g/mol) in 24,6 g of tin(II) fluoride?
A. 0.31 g
B. 2.98 g
C. 5.97 g
D. 101.4

A

C

32
Q

Tin(II) fluoride (156.7 g/mol) is often added to toothpaste as an ingredient to prevent tooth decay. What is the mass of fluoride (19 g/mol) in 24,6 g of tin(II) fluoride?
A. 0.31 g
B. 2.98 g
C. 5.97 g
D. 101.4

A

C

33
Q

The empirical formula of a compound is CH. The molar mass of the compound is 78 g/mol,
what is its molecular formula?
A. C2H2
B. C5H6
C. C8H8
D. None of the above

A

B

34
Q

For which compound are the empirical and molecular formulas the same?
A. C6H5COOH
B. C6H4(COOH)2
C. HOOCCOOH
D. CH3COOH

A

A

35
Q

Which of the following is a chemical equation?
A. CO2
B. C+O2 -> CO2
C. Ice + Heat -> Water
D. Iron + Oxygen -> Rust

A

B

36
Q

Consider the combustion of butane, where in a particular reaction, 5 mol of C4H10 are reacted with excess O2. Calculate the mol of CO2 formed.
A. 1.25 mol
B. 10 mol
C. 12.5 mol
D. 20 mol

A

D

37
Q

Ammonia is produced in according to the equation N2 + 3H2 -> 2NH3. In a particular experiment, 0.25 mol of NH. is formed when 0.25 mol of NH3 is reacted with 0.5 mol of H2. What is the percent yield?
A. 75%
B. 50%
C. 33%
D. 25%

A

A

38
Q

The synthesis of ammonia from nitrogen and hydrogen is an exothermic reaction. Which of the following will favor the formation of ammonia?
A. decrease in temperature
B. increase in temperature
C. removal of nitrogen
D. addition of ammonia

A

A

39
Q

Which of the following can change the value of the equilibrium constant?
A. addition of a catalyst
B. change in temperature
C. change in concentration
D. change in pressure or volume

A

B

40
Q

Which statement is TRUE?
A. The greater the activation energy, the faster the rate of reaction.
B. A catalyst speeds up both the forward and reverse reaction rates.
C. The value of the equilibrium constant increases with the addition of a catalyst.
D. A catalyst increases the rate of reaction by decreasing the number of collisions.

A

B

41
Q

A solution is _______ if more solute can dissolve in it.
A. saturated
B. unsaturated
C. supersaturated
D. concentrated

A

B

42
Q

How many grams of NaOH (40 g/mol) is needed to prepare 500 mL of 0.500 N solution of NaOH?
A. 4.00 g
B. 5.00 g
C. 10.0 g
D. 10.3 g

A

C

43
Q

An exact amount of 0.8214 g of KMnO. (158 g/mol) was dissolved in water and made up to volume in a 500-mL volumetric flask. A 2.00-mL portion of this solution was transferred to a 1000-mL flask and diluted to volume. Then 10.00 mL of the diluted solution was transferred to a 250-mL flask and diluted to volume. What is the molar concentration of the final solution?
A. 0.104 M
B. 2.08x10-5 M
C. 8.32x10-7 M
D. none of the above

A

C

44
Q

Which procedure produces a 0.2 M solution of Na2SO4?
A. Dissolving 0.2 M solid Na2SO4 in 500 mL water.
B. Diluting 400 mL of 0.3 M Na2SO, to a final volume of 1.0 L
C. Mixing 500 mL of 0.4 M NaOH with 500 mL of 0.2 M Na2SO4.
D. Mixing 300 mL of 1.2 M NaOH with 600 mL of 0.3 M Na2SO4.

A

D

45
Q

The lining of the stomach contains cells that secrete a solution of HCl. Which drink would best alleviate heartburn, i,e., excess acid in the stomach?
A. diet soda (pH 4.3)
B. milk of magnesia (pH 10.5)
C. milk (pH 6.5)
D. wine (pH 3.8)

A

B

46
Q

Which of the following is NOT an acid-base conjugate pair?
A. NH3 and NH4+
B. H2S and OH-
C. H2O and OH-
D. HCN and CN-

A

B

47
Q

The acid secreted by the cell of the stomach lining is a hydrochloric acid solution that typically contains 1.2x10-3.M. Whatis the pH of the acid in the stomach?
A. 1.50
B. 2.92
C. 3.50
D. 6.19

A

B

48
Q

When ammonium chloride undergoes ionization, the resulting solution will have a pH ______
A. <7
B. 7
C. >7
D. 14

A

A

49
Q

Which of these conjugate acid-base pairs must be used to prepare a buffer with pH near 7.15?
A. formic acid and sodium formate (pK. 3.74)
B. succinic acid and sodium succinate (pKa 5.64)
C. glycylglycine and sodium glycylglycate (pKa 8.35)
D. sodium dihydrogen phosphate and sodium hydrogen phosphate (pKa2 7.20)

A

D

50
Q

What are the products for the reaction between HNO3 and NH4OH?
A. HNO2 + H2O
B. NH2OH + H2O
C. NH4NO3 + H2O
D. No reaction will occur

A

C

51
Q

In NaH what is the oxidation state of hydrogen?
A. -1
B. 0
C. 1
D. 2

A

A

52
Q

When Cr3+ changes from an oxidation state of +3 to +6, Cr3+ will _______
A. gain 6 electrons
B. lose 6 electrons
C. lose 3 electrons
D. gain 3 electrons

A

C

53
Q

Reduction involves _________ oxidation number.
A. increase of
B. decrease of
C. independence of
D. no change in

A

B

54
Q

For the reaction Mg + H20 -> MgO + H2, which is FALSE?
A. H2O is the oxidizing agent
B. Mg lost electrons
C. Mg is the oxidizing agent
D. H2O gained electrons

A

C

55
Q

Oxidation is the same as
A. addition of hydrogen
B. removal of oxygen
C. addition of oxygen
D. removal of Nitrogen

A

A

56
Q

Which part of an electrochemical cell maintains electrical neutrality?
A. anode
B. salt bridge
C. cathode
D. voltmeter

A

B

57
Q

It is an electrochemical cell where electrical energy is used to drive a nonspontaneous redox reaction.
A. Daniell cell
B. Voltaic cell
C. Galvanic cell
D. Electrolytic cell

A

D

58
Q

In an electrolytic cell, oxidation occurs
A. at the anode
B. at the cathode
C. at either the cathode or the anode
D. between the cathode and the anode

A

A

59
Q

During electroplating of silver, silver ions in solution
A. are oxidized at the anode
B. are oxidized at the cathode
C. are reduced at the cathode
D. remain in solution unchanged

A

C

60
Q

In maintenance and storage of pH meters, which of the following must NOT be done?
A. Use mild soap solution in general cleaning of electrode.
B. Store the electrode in distilled water to keep the electrode bulb moist during storage.
C. Blot electrode dry after rinsing the pH electrode.
D. Rinse pH electrode in between measurements.

A

B

61
Q

Express the number 0.051065 to four significant figures
A. 0.051
B. 0.051
C. 0.05106
D. 0.0511

A

C

62
Q

The number 2.34x107 is the scientific notation for _______
A. 234000
B. 23400
C. 23400000
D. 2340000

A

C

63
Q

The volume of a liquid is 20.5 mL. Which of the following sets of measurement represents the value with good accuracy?
A. 19.2 mL, 19.3 mL, 18.8 mL, 18.6 mL
B. 18.9 mL. 19.0 mL. 19.2 mL, 18.8 mL
C. 18.6 mL, 17.8 mL, 19.6 mL, 17.2 mL
D. 20.2 mL, 20.5 mL, 20.3 mL, 20.1 mL

A

D

64
Q

A prediction or a possible explanation to the question or problem which can be tested in an experiment is called
A. hypothesis
B. procedure
C. graph
D. data

A

A

65
Q

A colorless liquid and a yellowish liquid were mixed in a test tube. Which of the following statements is FALSE?
A. There will be no reaction if the test tube will get hot.
B. There will be a reaction if a precipitate will be formed.
C. There will be no reaction if the liquids will be on top of each other.
D. There will be a reaction it the yellow color will drastically disappear.

A

A

66
Q

Which of the following is the closest to being an ideal gas?
A. Oxygen
B. Nitrogen
C. Helium
D. Hydrogen

A

C

67
Q

What happens to the volume of a fully inflated balloon when it is taken outside on a cold day?
A. its volume decreases
B. its volume increases
C. it remains the same
D. it’s volume becomes equal to zero

A

A

68
Q

Whose atomic model illustrates that negative charges are scattered around an atom?
A. Dalton
B. Thomson
C. Rutherford
D. Bohr

A

B

69
Q

An element has a notation 18^40 Ar. How many neutrons does this element have?
A. 18
B. 22
C. 40
D. 58

A

B

70
Q

What is the name of Cu2O?
A. Dicopper monoxide
B. Cupric oxide
C. Copper(I) Oxide
D. Copper (II) Oxide

A

C

71
Q

Which of the following is arranged in increasing atomic size?
A. Cs < Ca < O < Ne
B. Cs < O < Ca < Ne
C. Ne < Ca < O < Cs
D. Ne < O < Ca < Cs

A

D

72
Q

Which of the following does NOT follow octet rule?
A. CH
B. CCl
C. HCI
D. NO

A

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