stud
bud
Sign up
Log in
Home
Library
Explore
SAT
More
Higgins Atomic Theory Flashcards | StudBud
Explore
/
Higgins Atomic Theory
Higgins Atomic Theory
30 terms
·
StudBud Administration
·
136 plays
atomic theory
Flashcards
30 cards
F
Practice quiz
P
Host live
L
Questions
30
Answers
1
Atoms of the same element with different masses are called ____.
anions
multiples
isotopes
ions
2
The picture below depicts the cathode-ray tube experiment that led to the discovery of _____.
neutrons
the nucleus
electrons
protons
3
Electrons were discovered by _______.
JJ Thomson
Ernest Rutherford
James Chadwick
John Dalton
4
Whose model of the atom is shown below?
Dalton's
Rutherford's
Chadwick's
Thomson's
5
How many electrons are in a Ca
+2
ion?
22
20
18
40
6
Isotopes are atoms of the same element that have different numbers of ____.
neutrons
electron shells
protons
electrons
7
Which of the following isotopes represents an atom that has 17 protons and 20 neutrons?
17Cl
35Cl
37Ca
37Cl
8
Which of the following points from Dalton's atomic theory is incorrect?
Atoms can be joined, separated, or rearraged in reactions.
All atoms of the same element are identical.
All matter is composed of atoms.
Atoms cannot be created or destroyed.
9
What subatomic particle(s) are located in the nucleus?
protons and electrons
protons and neutrons
protons only
electrons and neutrons
10
Which of the following symbols represents a phosphorus atom that has gained three electrons?
P-3
P
P+4
P+3
11
The number of protons in the atom is the ____.
isotope number
nuclear force
mass number
atomic number
12
How many electrons are in an O
-2
ion?
8
-2
6
10
13
Atoms have a _______ charge.
negative
positive
neutral
none of these
14
According to Rutherford, where in the atom are electrons located?
in the empty space surrounding the atom
distributed evenly all throughout the atom
in the nucleus
in circular orbits called electron shells
15
How many electrons are in a neutral sodium atom?
11
23
12
13
16
How many neutrons are in a zinc-65 atom?
65
40
30
35
17
The first person to suggest the idea of atoms was ________.
Dalton
Democritus
Aristotle
an alchemist
18
The smallest subatomic particle is the ______.
proton
electron
neutron
none of these; they are all the same size
19
The Greek word "atomos" means _______.
uncuttable
invisible
very small
indestructible
20
The mass number of an atom can be determined by ___.
subtracting atomic number and protons
adding protons and electrons
adding protons and neutrons
subtracting neutrons and protons
21
The first atomic theory was proposed by ________.
Lavoisier
Chadwick
Thomson
Dalton
22
Why were some of the alpha particles in Rutherford's experiment able to pass through the foil?
they were deflected by the nucleus
because they were positively charged
because neutrons are neutral
because atoms contain a large amount of empty space
23
Why were some particles deflected in the experiment shown here?
Atoms are mostly empty space.
They were repelled by the nucleus.
The electrons caused the particles to bounce back.
They could not pass through the atoms.
24
All isotopes of an element have the same ____.
atomic mass
number of protons
number of neutrons
mass number
25
Which scientist thought atoms were simply solid spheres?
James Chadwick
Ernest Rutherford
John Dalton
JJ Thomson
26
What is the atomic number of
207
Pb?
82
207
125
84
27
James Chadwick made which of the following contributions to the atomic theory?
discovered neutrons
discovered protons
discovered electrons
discovered that atoms are neutral
28
Mass number can be calculated by ____.
subtracting atomic number and protons
subtracting atomic number and neutrons
adding protons and electrons
adding protons and neutrons
29
Which of the following was accomplished by Ernest Rutherford?
discovered that atoms contain large amounts of empty space
performed experiments with cathode ray tubes
developed the plum pudding model of the atom
proposed the first atomic theory
30
Neutrons have a ________ charge and are found _________.
neutral, in the nucleus
neutral, in the empty space around the nucleus
positive, in the nucleus
negative, in the electron shells
