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Chapter 5 Development Of The Modern Theories Of Atomic Structure Flashcards | StudBud
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Chapter 5 Development Of The Modern Theories Of Atomic Structure
Chapter 5 Development Of The Modern Theories Of Atomic Structure
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1
The ratio of the mass of one element that combine with other elements in simple whole number is
the law of definite composition
The law of the conservation of mass
the law of multiple proportions
the law of mass action
2
Carbon-14 (atomic number 6) the radioactive nuclide used in dating fossils has
8 neutrons
10 neutrons
6 neutrons
14 neutrons
3
He 1st recognized that the ratio of the number of atoms is the same as the ratio of the masses
Jons Berzelius
John Dalton
Edward Morley
Jon Newlands
4
Protons have
no charges
negative charges
an attraction for neutrons
no mass
5
Dalton's atomic theory did NOT explain the law of
definite proportions
conservation of mass
conservation of energy
whole-number ratios
6
Isotopes of an element contain different number of _______________.
neutrons
nuclides
electrons
protons
7
The law of conservation of mass follows from the concept that
atoms are indivisible
matter is composed of atoms
atoms of different elements have different properties
atoms can be destroyed in chemical reactions
8
The most common form of hydrogen has _________________.
three neutrons
one neutron
two neutrons
no neutrons
9
The atomic mass listed in the periodic table is the _____________.
average atomic mass
mass number of the most abundant
relative atomic mass of the most stable radioactive isotope
relative atomic mass of the most abundant isotope
10
The mass of a neutron is
double that of a proton
about the same as that of a proton
about the same as that of an electron
double that of an electron
11
According to the law of definite proportions, any two samples of KCl have
the same mass
the same melting point
the same ratio of elements
slightly different molecular structures
12
Atoms of the same element can differ in ______________.
chemical properties
mass number
atomic number
number of protos and electrons.
13
The hydrogen isotope with the least mass is named:
helium
protium
tritium
deuterium
14
Protons within a nucleus are attracted to each other by
nuclear forces
opposite charges
electron repulsion
their energy levels
15
Isotopes of each element differ in ______________.
atomic number
the total number of electrons
the number of electrons in the highest energy level
the number of neutrons in the nucleus
16
An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is:
27
40
13
14
17
The smallest particle that can exist alone or combined with such particles of other elements is
neutron
atom
electron
proton
18
As the atomic number increases, the number of electrons in an atom ________________.
remains the same
is undertermined
increases
decreases
19
The charge on the electron cloud
balances the charge on the nucleus
does not exist
attracts electron clouds in other atoms to form compound
prevents compounds from forming
20
Because most alpha particles fired at the gold foil passed straight through, Rutherford
concluded that atoms contained no charged particles
concluded that atoms were indivisible
concluded that atoms were mostly empty space
concluded that electrons formed the nucleus
21
The total number of protons and neutrons in the nucleus of an atom is its ___________.
Avogadro constant
number of atoms
mass number
atomic number
22
In the periodic table below, a neutral atom of silicon contains _____________.
38 electrons
28.09 electrons
14 electrons
16 electrons
23
The mass of the compound is _______ the sum of the individual elements.
less than
greater than
either greater than or less than
equal to
24
The rays produced in a cathode tube in early experiments were
found to carry a positive charge
deflected away from a negative plate
striking the cathode
unaffected by a magnetic field
25
The average atomic mass of an element depends on the masses of its isotopes and each isotope's:
atomic number
relative abundance
radioactivity
mass number
26
As the mass number of the isotope of an element increases, the number of protons _____________.
increases
decreases
doubles each the mass number increases.
remains the same
27
The principles of atomic theory recognized today were conceived by
Rutherford
Avogadro
Bohr
Dalton
28
The radius of an atom extends to the outer edge of the ____________.
region occupied by the electrons
positive charge
region occupied by the neutrons
nucleus
29
A nuclear particle with about the same mass as a proton, but has no electrical charge, is a(n)
neutron
nuclide
electron
isotope
30
The relative atomic mass of an atom can be found by comparing the mass of the atom to the mass:
of one atom of carbon-12
of one atom of hydrogen-1
of uranium-235
of a proton
31
Isotopes are atoms of the same element that have different_________
principle chemical properties
masses
numbers of neutrons
numbers of protons
32
All isotopes of hydrogen contain ____________.
one neutron
two electrons
two nuclei
one proton
33
In oxides of N, e.g. N
2
O, and NO, atoms combine in small whole-number ratios. This supports
the law of definite proportions
mass action
the law of multiple proportions
the law of conservation of mass
34
An atom of potassium has 19 protons, 20 neutrons, what is its mass number?
39
19
20
10
35
Chlorine has atomic number 17 and mass number 35. It has:
18 protons, 18 electrons, and 17 neutrons
17 protons, 17 electrons, and 18 neutrons
17 protons, 17 electrons, and 52 neutrons
35 protons, 35 electrons, and 17 neutrons
36
Deuterium contains one proton and ______________.
no neutron
two electrons
one neutron
two neutrons
37
After measuring the ratio of the charge of cathode-ray particle to the mass, Thomson concluded
The particles had no mass
The particles had a very large mass
The particles has a very small mass
The particles carried a positive charge
38
Most of the volume of an atom is occupied by the
nucleus
nuclides
protons
electron cloud
39
Helium-3 and Helium-4 are ____________.
compounds
isotopes
nuclei
different elements
40
The carbon-12 atom is assigned a relative mass of exactly ____________.
6 amu
12 amu
100 amu
1 amu
41
Rutherford's experiments led to the discovery of the
electron
neutron
nucleus
cathode ray
42
A positively charged particle with a mass of 1.673 X 10
-24
g is a(n)
positron
electron
proton
neutron
43
What is the atomic number for aluminum from the periodic table below
26.98
13
14
26.982
44
The average atomic mass of an element is the average of the atomic masses of its ____________.
artificial isotopes
naturally occuring isotopes
nonradioactive isotopes
two most abundant isotopes
45
Rutherford's experiments concluded that atoms contain massive central regions that have
a positive charge
both protons and neutrons
a negative charge
no charge
46
The abbreviation for atomic mass unit is ______________.
mu
μ
amu
a
47
The atomic number of oxygen, 8, indicates that there are eight______________.
oxygen nuclides
energy levels in the oxygen atom's nucleus
protons in the nucleus of an oxygen atom.
neutrons outside the oxygen atom's nucleus
48
An atom is electrically neutral because
neutrons balance the protons and electrons
the numbers of the protons and the neutrons are equal
nuclear forces balance the charges
the numbers of the protons and electrons are equal
49
How many isotopes of hydrogen are known?
3
4
5
2
50
Experiments with cathode rays led to the discovery of the
nucleus
proton
electron
neutron
