June 2017 Chemistry Regents Questions 31-40 Question Preview (ID: 59775)

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Which electron configuration represents the electrons of an atom of neon in an excited state?

a) 2-7

b) 2-8

c) 2-7-1

d) 2-8-1

Which numerical setup can be used to calculate the atomic mass of gallium?

a) (0.6011)(68.926 u) + (0.3989)(70.925 u)

b) (60.11)(68.926 u) (39.89)(70.925 u)

c) (0.6011)(70.925 u) + (0.3989)(68.926 u)

d) (60.11)(70.925 u) + (39.89)(68.926 u)

A student measures the mass and volume of a sample of copper at room temperature and 101.3 kPa. The mass is 48.9 grams and the volume is 5.00 cubic centimeters. The student calculates the density of the sample. What is the percent error of the studen

a) 7.4%

b) 8.4%

c) 9.2%

d) 10.2%

What is the chemical formula for sodium sulfate?

a) Na2SO4

b) Na2SO3

c) NaSO4

d) NaSO3

If 46 grams of Na and 71 grams of Cl2 react completely, what is the total mass of NaCl produced?

a) 58.5 g

b) 117 g

c) 163 g

d) 234 g

The mole ratio of NO to NO 2 is

a) 1 to 1

b) 2 to 1

c) 3 to 2

d) 5 to 2

Which type of bonding is present when valence electrons move within the sample?

a) metallic bonding

b) hydrogen bonding

c) covalent bonding

d) ionic bonding

Which statement explains why the molecule is nonpolar?

a) Electrons are shared between the carbon atoms and the hydrogen atoms.

b) Electrons are transferred from the carbon atoms to the hydrogen atoms.

c) The distribution of charge in the molecule is symmetrical.

d) The distribution of charge in the molecule is asymmetrical.

A solid sample of a compound and a liquid sample of the same compound are each tested for electrical conductivity. Which test conclusion indicates that the compound is ionic?

a) Both the solid and the liquid are good conductors.

b) Both the solid and the liquid are poor conductors.

c) The solid is a good conductor, and the liquid is a poor conductor.

d) The solid is a poor conductor, and the liquid is a good conductor.

Which statement explains why 10.0 mL of a 0.50 M H2SO4(aq) solution exactly neutralizes 5.0 mL of a 2.0 M NaOH(aq) solution?

a) The moles of H+(aq) equal the moles of OH-(aq).

b) The moles of H2SO4(aq) equal the moles of NaOH(aq).

c) The moles of H2SO4(aq) are greater than the moles of NaOH(aq).

d) The moles of H+(aq) are greater than the moles of OH-(aq).

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