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Chapter 4 Review-Physical Science 2020 Flashcards | StudBud
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Chapter 4 Review-Physical Science 2020
Chapter 4 Review-Physical Science 2020
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Chapter 4 Atomic Structure Review
Flashcards
30 cards
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Practice quiz
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Questions
30
Answers
1
How was Bohr's atomic model similar to Rutherford's model?
It describes electron position by using electron cloud model
It describes a nucleus surrounded by a large volume of space
It assigned energy levels to electrons.
It described how electrons gain or lose energy.
2
What does the electron cloud model describe?
the number of electrons in atoms
the mass of the electrons in an atom
the most likely location of electrons in atoms
the precise location of electrons in atoms
3
Democritus coined what word for a tiny piece of matter that cannot be divided?
atom
electron
molecule
element
4
Which of the following is NOT part of John Dalton's atomic theory?
All atoms of the same element have the same mass.
All elements are composed of atoms.
Atoms contain subatomic particles.
A compound contains atoms of more than one element.
5
In a Bohr model, electrons
only pair once every spot in the energy level is filled with on electron
fill the highest energy level first
always pair before every spot is filled with an electron
6
What element is this?
Kr
Cl
Br
S
7
Which of the following is unique for any given element?
the mass of a neutron
the number of protons
the charge on the electrons
the number of neutrons
8
Which statement about particles is TRUE?
Neutrons have no charge and no mass.
Protons, neutrons & electrons all have about the same mass.
An electron has far less mass than a proton or a neutron.
Unlike protons and neutrons, electrons have no mass.
9
Which statement about subatomic particles is NOT true?
Unlike protons and electrons, neutrons have no charge.
Protons and neutrons have almost the same mass.
Protons and electrons have opposite charges.
Protons and neutrons have the same charge.
10
The glowing of a neon light is caused by electrons emitting energy as they
move from higher to lower energy levels.
collide with other electrons.
move from lower to higher energy levels.
collide with the nucleus.
11
What can you assume has happened if an electron moves to a higher energy level?
The electron has lost energy.
The atom has lost an electron.
The electron has gained energy.
The atom has become more stable.
12
J. J. Thomson's experiments provided evidence that an atom
has a positive charge.
contains negatively charged particles.
has a negative charge.
is the smallest particle of matter.
13
The amount of ____ changes in an isotope
electrons
neutrons
protons
14
Which of the following is the correct number of electrons each energy level can hold in order from CLOSEST to FARTHEST
8, 18, 32, 64
2, 8, 18, 32
64, 32, 18, 8
32, 18, 8, 2
15
The number of protons in one atom of an element is that element's
balanced charge.
isotope.
mass number.
atomic number.
16
Which sentence states what Rutherford concluded from the gold foil experiment?
Thomson's model of the atom was correct.
The atom's positive charge is spread evenly about the atom.
At atom's positive charge is concentrated in it's nucleus.
An atoms negative charge is concentrated in it's nucleus.
17
Which statement is true about oxygen-17 and oxygen-18?
They are isotopes of oxygen.
Their atoms have an identical mass.
They have the same mass number.
They do not have the same number of protons.
18
Which is true when all of an atoms electrons are in orbitals with the lowest possible energies?
The atom is in its ground state.
The atom is in an excited state.
The electrons are in the most stable configuration.
The electrons are in an unstable configuration.
19
What is the smallest particle of an element that maintains the characteristics of the element?
electron
alpha particle
atom
isotope
20
The nucleus of an atom has what kind of charge?
neutral
positive
negative
21
Which expression accurately compares the masses of neutrons and protons?
mass of 1 neutron = mass of 1 electron
mass of 1 neutron = mass of 1 proton
mass of 1 electron = mass of 1 proton
mass of 2000 neutron = mass of 1 proton
22
What do scientists use to predict the locations of electrons in atoms?
probability
geometry
algebra
ratios and proportions
23
Which statement tell's how Bohr's model of the atom differed from Rutherford's model?
Bohr's model focused on the electrons.
Bohr's model focused on the protons.
Bohr's model focused on the nucleus.
Bohr's model focused on the neutrons.
24
All hydrogen atoms have 1 proton. Which is the number of neutrons in an atom of hydrogen-3?
2
0
3
1
25
Which subatomic particle has a negative charge?
proton
alpha particle
electron
neutron
26
Who provided evidence for the existence of a nucleus in an atom?
J. J. Thomson
John Dalton
Ernest Rutherford
Democritus
27
How many neutrons does Phosphorous-31 have?
31
5
16
15
28
In Niels Bohr's model of the atom, electrons move
like planets orbiting the Sun.
like popcorn in a popcorn popper.
like beach balls on water waves.
like balls rolling down a hill.
29
Which quantity is always equal to the element's atomic number?
number of neutrons
number of nuclei
number of electrons
number of protons
30
To find the number of neutrons in an atom, you would subtract
Atomic number - mass number
mass number + atomic number.
mass number - atomic number
atomic number - electron number.
