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Atomic Structure Chapter 4 Flashcards | StudBud
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Atomic Structure Chapter 4
Atomic Structure Chapter 4
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1
2 isotopes w/AMU's of 10.01 and 11.01. Abundances are 19.8% and 80.2%. Calc average atomic mass
21.02 amu
10.81 amu
2.102 amu
10.51 amu
2
Using the periodic table; determine the # of neutrons in
16
O.
24
4
16
8
3
Which of Argons isotopes is most abundant?
Argon-38
Argon-40
All are equally abundant
Argon-36
4
Rutherford proposed the + charge of an atom was in the nucleus, What evidence supported this?
He observes Au atoms slightly deflected alpha particles
His observation that beta particles acted the same as e-
his measurements of the mass of Au, Ag, and other elements
He observes that Au atoms greatly deflected alpha particles
5
What instrument can be used to observe individual atoms?
Scanning Electron Microscope
Light Microscope
Optical telescope
X-Ray machine
6
How does Rutherford's model describe the structure of atoms?
negatively charges e-s embedded in a +charges solid core
+ charged particles embedded in a - charged solid core
a dense +charged nucleus surrounded by - charged electrons
a dense - charged nucleus surrounded by + charged protons
7
What distinguishes atoms of one element from another?
# of protons in the nucleus
the total # of protons, neutrons, and electrons
total # of protons and neutrons in the nucleus
# of neutrons in the nucleus
8
All of the atoms of the same element have the same
mass #'s
# of protons
mass
# of neutrons
9
What are the relative charges of the 3 main subatomic particles?
Proton +1, electron -1, neutron 0
Proton +2, electron -1, neutron 0
Proton +2, electron +1, neutron -1
Proton +1, electron -1, neutron +1
10
N exists as N14 and N15. What info about the 2 isotopes is needed to calc the atomic mass of N?
The # of protons in a nitrogen atom
Both A and B
The natural percent abundance of each isotope
The mass, in amu, of an atom of each isotope
11
The atomic # of an element is the total # of which particles in the nucleus?
protons
protons and electrons
electrons
neutrons
12
Which of the following equals 1 atomic mass unit?
1/12 the mass of 1 carbon 12 atom
the mass of one carbon 12 atom
the mass of 1 helium 4 atom
the mass of 1 electron
13
An element has an atomic of 76. The # of protons and electrons in a neutral atom are:
152 portons and 76 electrons
38 protons and 38 electrons
76 protons and 76 electrons
76 protons and 0 electrons
14
What are the 3 types of subatomic particles?
protons, electrons, nucleus
ions, neutrons, nucleus
protons, neutrons, electrons
muons, ions, electrons
15
What does the #84 in the name krypton 84 represent?
The sum of the protons and electrons
The atomic #
the mass #
twice the # of protons
16
How did Rutherford's model differ from Thompson's?
all outside the nucleus
Ruther:-charges in nucleus;Thomp: in lump of - charge
all inside the nucleus
Ruther: - charge around nucleus; Thomp: in lump of + charge
17
How do the isotopes of a given element differ from each other?
they have the same mass #'s but different #'s of protons
They gave the same mass #'s but different #'s of electrons
They have different mass #'s and different #'s of neutrons
18
How did Democritus characterize atoms?
as a form of energy, and not matter
As particles of matter that heat could destroy
as particles that could be divided into small pieces
As indivisible, indestructible particles
19
According to Dalton's postulates how do atoms relate to elements?
All elements are made of and all atoms are identical
the same atom may be part of 2 or more elements
None of the above
atoms of one lement differ from atoms of other elements
20
How is atomic number different than mass number?
atomic #=p+ and n; mass#= e-
atomic#= p+ and e-; atomic mass is p+ + n
they are the same
atomic# = n and mass# p+ and e-
21
Isotopes of the same element have different
atomic #'s
mass #'s and neutrons
chemical behavior
positions on the periodic table
22
According to Daltons theory is it possible to convert atoms of 1 element to another?
No, atoms are never changed into atoms of another element
yes, they can be converted through physical changes
yes, they can be converted through chemical changes
No atoms can change to other elements,it can't be controlled
23
Calc the relative abundance for these isotopes; amu's= 112.90 and 114.90; %'s= 4.29% and 95.71%
113.9 amu
114.8 amu
22.78 amu
227.8 amu
24
Rutherford performed the gold foil experiment in the diagram. What did he conclude from this?
the atoms in the foil have + charge distributed throughout
The atoms in the gold foil are mostly empty space
alpha particles were attracted to - particles in the foil
alpha particles bounced off the foil when collided w/a atom
25
How many protons, neutrons, and electrons does an atom w/ atomic #50 and mass # 125 contain?
120 neutrons, 50 protons, 75 electrons
75 electrons, 50 protons, 50 neutrons
70 neutrons, 75 protons, 50 electrons
50 protons, 50 electrons, 75 neutrons
26
Calc the Atomic mass of B. 19.9% (10.013 amu) and 80.1% (11.009 amu)
10.8
10.9
11.1
10.7
27
How do you calc. the # of neutrons in an atom?
Add 1 to the atomic #
Add the atomic # and the mass #
subtract 1 from the mass #
subtract the atomic # from the mass #
28
What are the relative masses of the 3 main subatomic particles?
Proton=1, neutron=1, electron=1
Proton=1,neutron=1.5, electron=0.5
Proton=1,neutron=1,electron=1/1840
Proton=1,neutron=1.25, electron=0.25
29
The atomic mass of oxygen is 15.999 amu. What does this value equal?
The mass of an atom of the most common oxygen isotope
The mass of every oxygen atom
The weighted average mass of oxygen atoms in nature
The mass of a randomly chosen oxygen atom
