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WorksheetsChemistry Regent Exam-June 2010
Total questions: 50
Worksheet time: 49mins
Name
Class
Date
1.
The gold foil experiment led to the conclusion that each atom in the foil was composed mostly of empty space because most alpha particles directed at the foil
a)
passed through the foil
b)
remained trapped in the foil
c)
were deflected by the nuclei in gold atoms
d)
were deflected by the electrons in gold atoms
2.
Which subatomic particles are located in the nucleus of a carbon atom?
a)
protons, only
b)
neutrons, only
c)
protons and neutrons
d)
protons and electrons
3.
Which part of a helium atom is positively charged?
a)
electron
b)
neutron
c)
nucleus
d)
orbita
4.
The mass of a proton is approximately equal to the mass of
a)
an alpha particle
b)
an electron
c)
a neutron
d)
a positron
5.
At STP, solid carbon can exist as diamond and graphite. Compared to the molecular structure and chemical properties of diamond, graphite has
a)
a different molecular structure and different properties
b)
a different molecular structure and the same properties
c)
the same molecular structure and different properties
d)
the same molecular structure and the same properties
6.
Which Group 14 element is classified as a metal?
a)
carbon
b)
germanium
c)
silicon
d)
tin
7.
The light emitted from a flame is produced when electrons in an excited state
a)
absorb energy as they move to lower energy states
b)
absorb energy as they move to higher energy states
c)
release energy as they move to lower energy states
d)
release energy as they move to higher energy states
8.
An atom of which element has the greatest attraction for electrons in a chemical bond?
a)
As
b)
Ga
c)
Ge
d)
Se
9.
Which formula represents a polar molecule?
a)
H2
b)
H2O
c)
CO2
d)
CCl4
10.
Two categories of compounds are
a)
covalent and molecular
b)
covalent and metallic
c)
ionic and molecular
d)
ionic and metallic
11.
Which type of bond is found between atoms of solid cobalt?
a)
nonpolar covalent
b)
polar covalent
c)
metallic
d)
ionic
12.
Which equation represents sublimation?
a)
I2(s) → I2(g
b)
I2(s) → I2(l)
c)
I2(l) → I2(g)
d)
I2(l) → I2(s)
13.
Which sample of ethanol has particles with the highest average kinetic energy?
a)
10.0 mL of ethanol at 25 degrees C
b)
10.0 mL of ethanol at 55 degrees C
c)
100.0 mL of ethanol at 35 degrees C
d)
100.0 mL of ethanol at 45 degrees C
14.
The molarity of an aqueous solution of NaCl is defined as the
a)
grams of NaCl per liter of water
b)
grams of NaCl per liter of solution
c)
moles of NaCl per liter of water
d)
moles of NaCl per liter of solution
15.
A real gas behaves least like an ideal gas under the conditions of
a)
low temperature and low pressure
b)
low temperature and high pressure
c)
high temperature and low pressure
d)
high temperature and high pressure
16.
Which sample of matter can be separated into different substances by physical means?
a)
LiCl(aq)
b)
LiCl(s)
c)
NH3(g)
d)
NH3(l)
17.
At STP, 1.0 liter of helium contains the same total number of atoms as
a)
1.0 L of Ne
b)
2.0 L of Kr
c)
0.5 L of Rn
d)
1.5 L of Ar
18.
Which statement describes the particles of an ideal gas?
a)
The particles move in well-defined, circular paths
b)
When the particles collide, energy is lost
c)
There are forces of attraction between the particles
d)
The volume of the particles is negligible
19.
A chemical reaction between iron atoms and oxygen molecules can only occur if
a)
the particles are heated
b)
the atmospheric pressure decreases
c)
there is a catalyst present
d)
there are effective collisions between the particles
20.
Which statement describes this equilibrium?
a)
The H2O(s) melts faster than the H2O(l) freezes.
b)
The H2O(l) freezes faster than the H2O(s) melts.
c)
The mass of H2O(s) must equal the mass of H2O(l).
d)
The mass of H2O(l) and the mass of H2O(s) each remain constant.
21.
A molecule of an organic compound contains at least one atom of
a)
carbon
b)
chlorine
c)
H2O(l).
d)
oxygen
22.
In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is equal to the
a)
activation energy
b)
entropy of the system
c)
heat of fusion
d)
heat of reaction
23.
A carbon-carbon triple bond is found in a molecule of
a)
butane
b)
butanone
c)
butene
d)
butyne
24.
Which statement describes one characteristic of an operating electrolytic cell?
a)
It produces electrical energy.
b)
It requires an external energy source
c)
It uses radioactive nuclides.
d)
It undergoes a spontaneous redox reaction
25.
Which compound when dissolved in water is an Arrhenius acid?
a)
CH3OH
b)
HCl
c)
NaCl
d)
NaOH
26.
An acid can be defined as an
a)
H+ acceptor
b)
H+ donor
c)
OH- acceptor
d)
OH- donor
27.
Which nuclear emission has no charge and no mass?
a)
alpha particle
b)
beta particle
c)
gamma ray
d)
positron
28.
During which process can 10.0 milliliters of a 0.05 M HCl(aq) solution be used to determine the unknown concentration of a given volume of NaOH(aq) solution?
a)
evaporation
b)
distillation
c)
filtration
d)
titration
29.
Which radioisotope is matched with its decay mode?
a)
H-3 and γ
b)
K-42 and β+
c)
N-16 and α
d)
P-32 and β-
30.
Which reaction is accompanied by the release of the greatest amount of energy?
a)
combustion of 10. g of propane
b)
electrolysis of 10. g of water
c)
nuclear fission of 10. g of uranium
d)
oxidation of 10. g of iron
31.
Which two atoms are isotopes of the same element?
a)
A and D
b)
A and Z
c)
X and D
d)
X and Z
32.
Which Lewis electron-dot diagram represents an atom in the ground state for a Group 13 element?
a)
1
b)
2
c)
3
d)
4
33.
Which element forms a compound with chlorine with the general formula MCl?
a)
Rb
b)
Ra
c)
Re
d)
Rn
34.
A sample of an element has a mass of 34.261 grams and a volume of 3.8 cubic centimeters. To which number of significant figures should the calculated density of the sample be expressed?
a)
5
b)
2
c)
3
d)
4
35.
Which characteristics both generally decrease when the elements in Period 3 on the Periodic Table are considered in order from left to right?
a)
nonmetallic properties and atomic radius
b)
nonmetallic properties and ionization energy
c)
metallic properties and atomic radius
d)
metallic properties and ionization energy
36.
Which formula is both a molecular and an empirical formula?
a)
C6H12O6
b)
C2H4O2
c)
C3H8O
d)
C4H8
37.
An atom of argon in the ground state tends not to bond with an atom of a different element because the argon atom has
a)
more protons than neutrons
b)
more neutrons than protons
c)
a total of two valence electrons
d)
a total of eight valence electrons
38.
Which formula represents a molecule having a nonpolar covalent bond?
a)
1
b)
2
c)
3
d)
4
39.
Which compound has the lowest vapor pressure at 50 degrees C?
a)
ethanoic acid
b)
ethanol
c)
propanone
d)
water
40.
Given the potential energy diagram and equation representing the reaction between substances A and D:
a)
HI(g)
b)
HI(g)
c)
CO2(g)
d)
C2H6(g)
41.
A sample of gas confined in a cylinder with a movable piston is kept at constant pressure. The volume of the gas doubles when the temperature of the gas is changed from
a)
400. K to 200. K
b)
200. K to 400. K
c)
400. degrees C to 200. degrees C
d)
200. degrees C to 400. degrees C
42.
According to Table F, which compound is soluble in water?
a)
barium phosphate
b)
calcium sulfate
c)
silver iodide
d)
sodium perchlorate
43.
Which changes occur when the temperature of this system is decreased?
a)
The concentration of H2(g) increases and the concentration of N2(g) increases.
b)
The concentration of H2(g) decreases and the concentration of N2(g) increases.
c)
The concentration of H2(g) decreases and the concentration of NH3(g) decreases.
d)
The concentration of H2(g) decreases and the concentration of NH3(g) increases
44.
Which formula represents an unsaturated hydrocarbon?
a)
1
b)
2
c)
3
d)
4
45.
Which half-reaction equation represents the reduction of an iron(II) ion?
a)
Fe2+ → Fe3+ + e-
b)
Fe2+ + 2e- → Fe
c)
Fe3+ + e- → Fe2+
d)
Fe → Fe2+ + 2e-
46.
Which metal is more active than H2?
a)
Ag
b)
Au
c)
Cu
d)
Pb
47.
Given the balanced ionic equation representing the reaction in an operating voltaic cell: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) The flow of electrons through the external circuit in this cell is from the
a)
Cu anode to the Zn cathode
b)
Cu cathode to the Zn anode
c)
Zn anode to the Cu cathode
d)
Zn cathode to the Cu anode
48.
Which laboratory test result can be used to determine if KCl(s) is an electrolyte?
a)
pH of KCl(aq)
b)
pH of KCl(s)
c)
electrical conductivity of KCl(aq)
d)
electrical conductivity of KCl(s)
49.
Which compound is produced when HCl(aq) is neutralized by Ca(OH)2(aq)?
a)
CaCl2
b)
CaH2
c)
HClO
d)
HClO2
50.
Which nuclides are used to date the remains of a once-living organism?
a)
C-14 and C-12
b)
Co-60 and Co-59
c)
I-131 and Xe-131
d)
U-238 and Pb-206
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