Font size
WorksheetsTest Review Atomic Structure 2024
Total questions: 76
Worksheet time: 3hrs 16mins
Calculation used to find the number of neutrons in an atom
Mass Number - Atomic Number
Atomic Number - Atomic Mass
Atomic Mass - Electrons
none of these
Found in the nucleus of an atom. This particle has a positive charge.
Neutron
Proton
Electron
Decepticon
Found orbiting outside the nucleus, this subatomic particle has a negative charge.
Neutron
Proton
Electron
Idontknowatron
The periodic table is in order by the
Mass number
Neutron number
Atomic number
APE MAN Number
The smallest subatomic particle is the
proton
neutron
electron
decepticon
What is the atomic mass of barium
56
82
137
138
How many neutrons does platinum have?
78
117
195
196
Which of the following is correct?
Protons are positive, electrons are negative, neutrons are neutral.
Protons are neutral, electrons are negative, neutrons are positive
Protons are negative, electrons are positive, neutrons are neutral
Protons are positive, electrons are neutral, neutrons are negative
The atomic mass of an atom is equal to
number of protons plus number of neutrons
number of protons plus number of electrons
number of electrons plus the number of neutrons
What were J. J. Thomson's three contributions to the atomic theory?
Discovered the electron
Discovered the nucleus -did the gold foil experiment
Used the cathode ray tube in his discovery
Created a model of the atom with electrons moving around the nucleus in fixed orbits
Created the "plum pudding" model of the atom
What were John Dalton three contributions to atomic history?
Created the atomic theory
Discovered that the atom is mostly empty space
Believed that atoms of a given element are identical
Hypothesized that the atom is a tiny, hard sphere
Believed that the universe was made of tiny "uncuttable" particles
What is Neils Bohr's contribution to the atomic theory?
Created the atomic theory
Created a model of the atom with electrons moving around the nucleus in a fixed orbits
Discovered that the proton had a positive charge
Believed that atoms of a given element are identical
Discovered the electron
What were Ernest Rutherford's three contributions to atomic theory?
Discovered that the atom is mostly empty space
Discovered the nucleus- did the gold foil experiment
Used the cathode ray tube in his discovery
Discovered the electron
Discovered that the proton had a positive charge
Rutherford referred to the center of the atom, where the mass was concentrated, as _____
the center
the nucleus
the middle
What is a positive ion called?
anion
cation
isotope
covalent
What is a negative ion called?
anion
cation
covalent
isotope
How many electrons would a Calcium ion gain/lose? If it has 2 valence electrons.
lose 1
gain 1
lose 2
gain 2
If an atom loses electrons, the charge will be positive.
true
false
A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?
Br-1
Br+1
Br+7
Br-7
An atom with 2 protons, 3 neutrons, and 4 electrons has a charge of ____.
+2
-2
+3
0
Isotopes of an element have a different number of...
Protons
Neutrons
Electrons
Mass
Potassium-39 has how many neutrons?
19
18
20
21
Bromine-80 has how many neutrons?
41
42
44
45
76 protons and 114 neutrons
Osmium-114
Osmium-76
Osmium-190
Osmium-190.23
The photo above shows the isotopic notation for which isotope?
Carbon 12
Carbon 13
Carbon 14
Carbon 15
An element has three isotopes. Given the abundances and relative masses, calculate the average atomic mass and determine (from the periodic table) which element it is.
Abundances | Relative masses
0.005% | 234.04 amu
0.720% | 235.04 amu
99.275% | 238.05 amu
Uranium (#92, Atomic Mass: 238.03 amu)
Fluorine (#9, Atomic Mass: 19.00 amu)
Mercury (#89, Atomic Mass: 200.59 amu)
Polonium (#84 209 amu)
Rubidium has two naturally occurring isotopes, 85Rb (relative mass 84.9118 amu) and 87Rb (relative mass 86.9092 amu). The abundance of 87Rb is 27.8%, If rubidium has an average atomic mass of 85.47 amu, what is the % abundance of 85Rb (in percent)?
27.9%
72.1%
74.63%
34.29%
Isotopes definition
Species of atoms of a chemical element with the same atomic number but different amounts of neutrons or electrons
Species of atoms of a chemical element with the same atomic number but different amounts of protons
Species of atoms of a chemical element with the same atomic number but different amounts of energy
None of the above
Why is the atomic number a decimal
It includes electrons
It's an average
It's an average of all isotopes
It has to be
What is different in isotopes
Identity
Protons
Element
Atomic mass
What kind of element has isotopes
Metals
Metalloids
Non-metals
All
What is emission spectra?
The emission spectra is the absorption of light by an atom or molecule.
The emission spectra is the unique pattern of light emitted by an atom or molecule when it transitions from a higher energy state to a lower energy state.
The emission spectra is the reflection of light by an atom or molecule.
The emission spectra is the scattering of light by an atom or molecule.
What causes the bright lines in emission spectra?
Photon absorption
Chemical reactions
Nuclear reactions
Electron transitions
What happens when an electron absorbs a photon?
The electron loses energy and moves to a lower energy level or orbital.
The electron remains in the same energy level or orbital.
The electron is destroyed and ceases to exist.
The electron gains energy and moves to a higher energy level or orbital.
What happens when an electron emits a photon?
The electron transitions from a higher energy state to a lower energy state and emits a photon.
The electron absorbs a photon and transitions to a higher energy state.
The electron emits multiple photons simultaneously.
The electron remains in the same energy state and emits a photon.
What is the relationship between energy levels and bright line spectra?
Bright line spectra are produced when electrons in an atom move from higher energy levels to lower energy levels, emitting specific wavelengths of light.
Bright line spectra are produced when electrons in an atom move from one energy level to another without emitting any light.
Bright line spectra are produced when electrons in an atom move from higher energy levels to lower energy levels, absorbing specific wavelengths of light.
Bright line spectra are produced when electrons in an atom move from lower energy levels to higher energy levels, emitting specific wavelengths of light.
How can bright line spectra be used to identify elements?
By comparing the observed bright line spectra of an unknown sample with the known spectra of different elements.
By observing the color of the unknown sample.
By measuring the temperature of the unknown sample.
By analyzing the mass of the unknown sample.
True or False: The ground state is the highest energy state of an atom.
True
False
All stars are composed of a mixture of elements. When these elements are heated they emit specific amounts of electromagnetic radiation, known as an emission spectrum. Each element emits a unique, identifiable, spectrum.
Using the Bright-line emission spectrum chart below, identify the elements present in this modeled star (found in the line labeled “mixture”).
Lithium and cadmium are in the mixture. Strontium is not in the mixture.
Lithium and strontium are in the mixture. Cadmium is not in the mixture
Cadmium and strontium are in the mixture. Lithium is not in the mixture
All of the shown elements are present in the mixture.
The unknown emissions spectra belongs to the element
Hydrogen
Mercury
Neon
Sodium
The picture shows an atom in the ground state absorbing energy and the electron jumps to the excited state. Which state has higher energy?
Ground State
Excited State
Each element produces its own pattern of emission spectra lines because each element has its own distinct
Speed of light
Electron configuration
Number of neutrons
None of these
When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.
lose, absorb
absorb, lose
lose, lose
absorb, absorb
In which state does an electron have the least amount of energy?
Excited state
Ground state
Orbital
Bohr model
Which is a possible excited state for an element?
2-8-8-2
2-8-18-8-2
2-7-8-3
2-8-18-8-3
Which is the ground state configuration for Cobalt?
2-8-15-2
2-8-17
2-8-16-1
2-8-9-8
What is the excited state electron configuration of Sodium, Na
1
2-8-1
2-7-1
2-7-2
