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Chapter 3: Atoms - The Building Blocks of Matter Flashcards | StudBud
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Chapter 3: Atoms - The Building Blocks of Matter
Chapter 3: Atoms - The Building Blocks of Matter
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atomic theory
Flashcards
30 cards
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Questions
30
Answers
1
Which of the following isotopes represents an atom that has 17 protons and 20 neutrons?
17Cl
37Ca
35Cl
37Cl
2
Which scientist thought atoms were simply solid spheres?
John Dalton
James Chadwick
Ernest Rutherford
JJ Thomson
3
How many electrons are in a neutral sodium atom?
13
11
12
23
4
Why were some particles deflected in the experiment shown here?
Atoms are mostly empty space.
The electrons caused the particles to bounce back.
They could not pass through the atoms.
They were repelled by the nucleus.
5
What is the atomic number of
207
Pb?
84
82
207
125
6
How many neutrons are in sodium-23?
14
11
12
23
7
Which of the following points from Dalton's atomic theory is incorrect?
All matter is composed of atoms.
Atoms can be joined, separated, or rearraged in reactions.
Atoms cannot be created or destroyed.
Atoms cannot be subdivided.
8
How many neutrons are in a zinc-65 atom?
40
65
30
35
9
Atoms have a _______ charge.
positive
negative
none of these
neutral
10
The picture shown below represents which of the following concepts?
Law of definite proportions
law of multiple proportions
law of conservation of mass
Dalton's atomic theory
11
According to Rutherford, where in the atom are electrons located?
in the nucleus
in the empty space surrounding the nucleus
distributed evenly all throughout the atom
in circular orbits called electron shells
12
Atoms of the same element with different masses are called ____.
ions
multiples
anions
isotopes
13
Why were some of the alpha particles in Rutherford's experiment able to pass through the foil?
because neutrons are neutral
because they were positively charged
because atoms contain a large amount of empty space
they were deflected by the nucleus
14
What subatomic particle(s) are located in the nucleus?
protons only
protons and neutrons
protons and electrons
electrons and neutrons
15
The law of multiple proportions was developed by _____.
Niels Bohr
John Dalton
Antoine Lavoisier
Joseph Proust
16
Calculate the number of protons, electrons, and neutrons in Phosphorus-30.
p+ = 15 e- = 15 no = 15
p+ = 30 e- = 15 no = 30
p+ = 15 e- = 30 no = 30
p+ = 30 e- = 30 no = 30
17
The smallest subatomic particle is the ______.
neutron
electron
proton
none of these; they are all the same size
18
Whose model of the atom is shown below?
Dalton's
Rutherford's
Thomson's
Chadwick's
19
The number of protons in the atom is the ____.
atomic number
mass number
isotope number
nuclear force
20
Which of the following was accomplished by Ernest Rutherford?
performed experiments with cathode ray tubes
developed the plum pudding model of the atom
proposed the first atomic theory
discovered that atoms contain large amounts of empty space
21
The first atomic theory was proposed by ________.
Thomson
Chadwick
Lavoisier
Dalton
22
The law of conservation of mass was developed by _______.
John Dalton
Antoine Lavoisier
Joseph Proust
Niels Bohr
23
Neutrons have a ________ charge and are found _________.
negative, in the electron shells
neutral, in the empty space around the nucleus
neutral, in the nucleus
positive, in the nucleus
24
Mass number can be calculated by ____.
subtracting atomic number and protons
adding protons and electrons
adding protons and neutrons
subtracting atomic number and neutrons
25
The first person to suggest the idea of atoms was ________.
an alchemist
Dalton
Democritus
Aristotle
26
Which of the following statements supports the law of definite proportions?
All matter is composed of atoms.
The mass of the reactants is always the same as the products
Water is always 1 oxygen to 2 hydrogen.
All atoms of the same element are identical.
27
Electrons were discovered by _______.
JJ Thomson
Ernest Rutherford
John Dalton
James Chadwick
28
Isotopes are atoms of the same element that have different numbers of ____.
neutrons
protons
electron shells
electrons
29
The weighted average of all the naturally occurring isotopes for an element is ________.
percent abundance
relative mass
relative abundance
average atomic mass
30
The picture below depicts the cathode-ray tube experiment that led to the discovery of _____.
protons
neutrons
electrons
the nucleus
