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Chapter 4 'Atomic Structure' Review Flashcards | StudBud
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Chapter 4 'Atomic Structure' Review
Chapter 4 'Atomic Structure' Review
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1
What is this part of the atom
Proton
Orbit
Electron
Nucleus
2
Mass Number is
n0 - p+
p+ + n0
n0 + e-
e- + p
3
What is the Mass Number?
56
136
<p>80</p>
137.327
4
Who discovered the proton?
Dalton
Milikan
<p>Goldstein</p>
Thompson
5
Who measured the cathode ray prtcles mass and found out it was smaller than the mass of anatom?
Democritus
Dalton
Thomson
Rutherford
6
Isotopes differ how?
Neutrons
Electron
<p>Protons</p>
Atomic Number
7
How many protons are in the nuclei of lead- 201?
201
207
82
119
8
What is this experiment?
Plum Pudding
Dalton' atomic theory
Breaking apart an apple
Gold foil
9
What is the average AMU of Boron
22.022
5
10.811
1.993
10
<p>Isotopes are Chemically Alike</p>
False
True
11
Aweighted average mass reflects both the _____ and _____ of theisotopes as they occur in nature
Relative abundance and Neutrons
Mass and Neutrons
Protons and Neutrons
mass and relative abundance
12
Solve the following:
259.65 amu
35.49 amu
36.95 amu
238.922 amu
13
What is the Mass Number of this Element?
50
87.62
38
1377
14
<p>Who stated atoms are indivisible in his atomic theory?</p>
Democritus
Rutherford
Thomson
Dalton
15
According to Dalton's atomic theory, atoms can do all but the following during a chem rxn:
be seporated
be destroyed
be rearranged
be joined
16
How many protons are in the nuclei of aluminum?
18
27
5
13
17
What is this Model Called?
Planetary Model
Electron Cloud Model
Lewis Dot Model
Plum Pudding Model
18
What is the Atomic Number
<p>56</p>
137.327
<p>80</p>
136
19
Each Isotope has a fixed mass
True
False
20
Average atomic masses are not generally whole numbers, why?
significant figures
I don't know
weighted average
to make things more difficult
21
What was Rutherford trying to prove?
Electron Cloud Model
<p>Dalton's Atomic Theory</p>
Planetary Model
Plum Pudding Model
22
How is atomic mass calculated?
for each isotope, + it's a.m. by its % ab. and + products.
for each isotope, * it's a.m. by its % ab. and * products.
for each isotope, * it's a.m. by its % ab. and + products.
for each isotope, * it's a.m. by its % ab. and - products.
23
Two electrons would repel each other.
True
False
24
Which of the following is not needed to calculate the atomic mass of an element?
which isotopes exist
masses
% abundance
Number of Protons
25
What is the mass of 4.42 cm
3
of platinum? the density of platinum is 22.5 g / cm
3
99.5 g
105 g
3.52 g
0.196 g
26
How many protons are in the nuclei of molybdenum?
95
15
12
25
27
James Chadwick discovered the
Proton
Neutron
An Apple
Electron
28
What is Lithium-7's mass number?
10
7
3
13
29
Cathode ray particles have a _______ charge
<p>Negative</p>
Blue
Neutral
Postive
30
Who discovered the charge of an electron?
Thomson
Rutherford
Milikan
Dalton
31
What makes isotopes of the same element chemically alike?
Mass Number
Electrons
Protons
They are both the same element
32
Who proposed this model?
Democritus
<p>Rutherford</p>
Dalton
Thomson
33
Who stated atoms are indivisible and indestructible; but did not explain chem. behavior?
Democritus
Rutherford
Thomson
Dalton
34
Elements are different because they contain different numbers of
Nucleous
Electron
Neutron
Proton
35
Alpha Particles have a _______ charge
Pegative
Green
Neutral
Positve
36
What subatomic particle did Thomson discover?
Proton
<p>Electron</p>
Neutron
<p>Nucleous</p>
37
Because Isotopes have a different number of neutrons; what else must change?
Atomic Number
Protons
Electrons
Mass Number
38
How many Protons does this isotope have?
56
<p>137.327</p>
<p>80</p>
136
39
What is an atom?
smallest prtcle of an element that still has it's properties
A man
something that cannot be broken down anyfarther
smallest prtcle of an element that has different properties
