UNIT 3 TEST - ADV. CHEM.
1. The total number
of electrons in a neutral atom of every element is always equal to the atom's
(A) mass
number (B) # of
neutrons (C)
# of protons (D) # of nucleons
2. Compared to an
atom of calcium-40, an atom of calcium-39 contains fewer
(A)
electrons (B)
protons (C)
neutrons (D) occupied energy
levels
3. An experiment
using alpha particles to bombard a thin sheet of gold foil indicated that most
of the volume of the
atoms in the foil is taken up by
(A)
electrons (B)
protons (C)
neutrons (D)
empty space
4. All isotopes of a
given element must have the same
(A) atomic
number (B) mass
number (C) number of neutrons
(D) number of nucleons
5. An atom of
carbon-14 contains
(A) 8 protons, 6 neutrons, and 6
electrons (B) 6 protons, 6 neutrons,
and 8 electrons
(C) 6 protons, 8 neutrons, and 8
electrons (D)
6 protons, 8 neutrons, and 6 electrons
6. What is the
atomic number of an atom which contains 28 protons, 28 electrons, and 34
neutrons?
(A) 28
(B) 56 (C)
62 (D) 90
7. As the mass
number of the isotopes of hydrogen increases, the number of protons
(A)
decreases (B)
increases (C)
remains the same
8. What is the total
number of electrons present in an atom of 59Co?
(A) 27
(B) 32 (C)
59 (D) 86
9. The development
of the concept that elements have isotopes helps explain why
(A) atomic nuclei are
neutral
(B) average atomic masses are not whole numbers
(C) atomic masses differ from the
atomic numbers (D) atomic nuclei are
charged
10. The standard now
used in determining the atomic masses of all other elements is
(A)
hydrogen-1 (B)
sulfur-32 (C)
carbon-12 (D) oxygen-16
11. The symbols 1H,
2H, and 3H indicate that the three kinds of hydrogen
atoms have
(A) the same atomic
mass
(B) different numbers of neutrons
(C) different numbers of
electrons (D) different atomic
numbers
12. The most common form of hydrogen has
(A) no
neutrons (B) one
neutron (C) two
neutrons (D) three neutrons
13. An element
consists of atoms, all of which have the same
(A) mass
number (B) neutron
number (C) Avogadro's
number (D)
atomic number
14. The average
atomic mass of an element
(A) is the mass of the most abundant
isotope (B)
may not equal the mass of any of its isotopes
(C) cannot be
calculated
(D) always adds up to 100
15. If Z represents
the atomic number and A represents the mass number of an isotope, then the
number of
neutrons in the atom is equal to
(A) A +
Z (B) A - Z
(C) Z - A (D)
Z x A (E)
none of these
16. The main idea of
Dalton's theory about the nature and properties of atoms could be used to
explain all of
the following EXCEPT
(A) the way in which substances
combine (B)
the definite composition of substances
(C) the
composition of isotopes
(D) that matter could not be created or destroyed
17. Electrons were
discovered as a result of investigations by
(A)
Dalton (B)
Bohr (C)
Chadwick (D)
Thomson (E) Rutherford
18. Combining
Thomson's work on the charge-to-mass ratio of an electron with Millikan's work
on the
charge of an electron made it possible to
determine the
(A) mass of
an electron
(B) pathway of an electron
(C) diameter of an
electron (D)
speed of an electron
19. To determine the
molar mass of an element, one must know the element's
(A) Avogadro's
number (B)
atomic number
(C) number of
isotopes (D) average atomic mass
20. Which pair of
substances illustrates the phenomenon of isotopes?
(A) 12C
and 14C
(B) SO3-2 and SO3
(C) H2O and H2O2
(D) 14C and 14C
21. A single atom
does not have a(n)
(A) relative atomic
mass (B)
atomic number
(C) mass
number
(D) average atomic mass
22. The charge on
the electron cloud
(A) prevents compounds from
forming
(B) balances the charges in the nucleus
(C) attracts electron clouds in other
atoms (D) does not exist
to form compounds
23. Which of the
following has the smallest mass?
(A) a Br atom
(B) 1 x 10-20 mole of
Br (C) 1 x 10-20
grams of Br
(D) a Br2 molecule
24. Which two
compounds are examples of the law of multiple proportions?
(A) FeCl3 and Fe2(SO4)3
(B) O2 and O3
(C) CO and CO2
(D) FeCl2 and Fe(NO3)2
25. A
positively-charged particle with a mass of 1.67 x 10-27 kg is a(n)
(A) proton
(B) neutron
(C) electron
(D) positron
(E) nucleon
*26. Deuterium
contains one proton and
(A) two
neutrons (B) one neutron
(C) no
neutrons (D)
two electrons
27. The carbon-12
atom is assigned a relative mass of exactly
(A) 1 amu
(B) 6 amu
(C) 12 amu
(D) 100 amu
28. The average
atomic mass of an element depends on both the masses of its isotopes and each
isotope's
(A) atomic
number (B)
radioactivity
(C) percent abundance
(D) mass number
29. Sulfur-34
contains
(A) 34
protons (B)
18 protons (C) 18 neutrons
(D) 16 neutrons
30. The atomic
number of neon is 10. The atomic number of calcium is 20. Compared
with a mole of neon, a
mole of calcium contains
(A) twice as many
atoms
(B) half as many atoms
(C) an equal
number of atoms
(D) 20 times as many atoms
31. A quantity of
sodium contains 6.022 x 1023 atoms. The mass of the sodium is
(A) 6.022 x 1023
grams (B)
3.88 grams (C) 22.99 grams
(D) not determinable
32. The mass of a sample
containing 3.5 moles of silicon atoms is
(A) 28
grams (B) 35
grams (C) 72
grams (D) 98 grams
33. The mass of a
sample of nickel is 176.1 grams. It contains
(A) 1.761 x 1024
atoms (B) 1.807 x 1024 atoms
(C) 5.869 x 1023
atoms (D)
5.869 x 1024 atoms