Use the Venn Diagram below to identify where the listed characteristics belong.
Venn Diagram comparing/contrasting protons and neutrons
Question 2 options:
In the nucleus
Contribute to the mass of an atom
Mass equals 1 amu
Determine the identity of an atom
Number is atomic number of element
Neutral charge
1.
BOTH
2.
PROTON
3.
NEUTRON
In the nucleus - BOTH
Contribute to the mass of an atom - BOTH
Mass equals 1 amu - BOTH
Determine the identity of an atom - BOTH
Number is atomic number of element - PROTON
Neutral charge - NEUTRON
Match the definitions to the atomic models. Model names may be used more than once.
Question 3 options:
Supported by Rutherford's gold foil experiment
This is the current model of atomic structure which explains the existence of electron clouds and their discrete energy levels.
Negatively-charged electrons randomly dispersed in a sea of positive charge.
The atom has a small positively-charged nucleus with negatively-charged electrons orbiting in different energy levels.
Sometimes referred to as the Planetary Model
Was disproved by Rutherford's gold foil experiment
A small, dense, positively-charged nucleus surrounded by a negatively-charged electron cloud.
1.
Plum Pudding Model
2.
Bohr Model
3.
Quantum Mechanical Model
4.
Nuclear Model
Supported by Rutherford's gold foil experiment - Nuclear Model
This is the current model of atomic structure which explains the existence of electron clouds and their discrete energy levels - Quantum Mechanical Model
Negatively-charged electrons randomly dispersed in a sea of positive charge - Plum Pudding Model
The atom has a small positively-charged nucleus with negatively-charged electrons orbiting in different energy levels - Bohr Model
Sometimes referred to as the Planetary Model - Bohr Model
Was disproved by Rutherford's gold foil experiment - Plum Pudding Model
A small, dense, positively-charged nucleus surrounded by a negatively-charged electron cloud - Nuclear Model
Relative abundance and atomic mass of the naturally occurring isotopes of hafnium:
5% - 176 amu
19% - 177 amu
27% - 178 amu
14% - 179 amu
35% - 180 amu
What is the average atomic mass of hafnium?
Question 4 options:
179 amu
177 amu
180 amu
176 amu
To calculate the average atomic mass of hafnium, we need to multiply the relative abundance of each isotope by its atomic mass, and then sum them up:
(0.05 * 176) + (0.19 * 177) + (0.27 * 178) + (0.14 * 179) + (0.35 * 180) = 8.8 + 33.63 + 48.06 + 25.06 + 63 = 178.55 amu
Therefore, the average atomic mass of hafnium is 178.55 amu.
Neils Bohr published his model of the atomic structure in 1913. He introduced the theory of electrons traveling in orbits around the atom's nucleus, with electrons orbiting only in certain orbits called shells. Each shell can contain a fixed number of electrons.
According to this model of the atom, the chemical properties of an element are mainly determined by
Question 5 options:
the difference between number of electrons and protons.
the total number of electrons in all shells.
the number of electrons in the outer shells.
the number of electrons in the inner shells.
According to Niels Bohr's model of the atom, the chemical properties of an element are mainly determined by the number of electrons in the outer shells.
Which pair below describes isotopes of the same element?
Question 6 options:
an atom with 6 protons and 8 neutrons - an atom with 8 protons and 6 neutrons
an atom with 6 protons and 6 neutrons - an atom with 6 protons and 7 neutrons
an atom with 7 protons and 6 neutrons - an atom with 6 protons and 6 neutrons
an atom with 8 protons and 8 neutrons - an atom with 7 protons and 8 neutrons
The pair that describes isotopes of the same element is:
an atom with 6 protons and 6 neutrons - an atom with 6 protons and 7 neutrons
Match each term and definition.
Question 1 options:
This is a subatomic particle with a positive charge and a mass of 1 amu.
This is a subatomic particle with no charge and a mass of 1 amu.
Atoms of the same element with varying number of neutrons.
This is a subatomic particle with a negative charge and very little mass.
This is a group of protons and neutrons in the center of all atoms.
This is an atom that has lost or gained electrons.
1.
Neutron
2.
Isotopes
3.
Electron
4.
Ion
5.
Nucleus
6.
Proton
This is a subatomic particle with a positive charge and a mass of 1 amu - Proton (6)
This is a subatomic particle with no charge and a mass of 1 amu - Neutron (1)
Atoms of the same element with varying number of neutrons - Isotopes (2)
This is a subatomic particle with a negative charge and very little mass - Electron (3)
This is a group of protons and neutrons in the center of all atoms - Nucleus (5)
This is an atom that has lost or gained electrons - Ion (4)
The atomic number is considered a unique atom and element identifier. Describe the associated subatomic particle, and how it can be used to identify the atom.
Question 2 options:
The number of electrons changes in a unique way as the charge on the atom changes.
As the atom absorbs photons the way the photons interact in the nucleus gives the atomic number.
The proton number remains constant through changing the atomic charge, energy, and isotopes.
All isotopes of the an element have the same number of neutrons allowing it to describe the unique atom.
The option that accurately describes the associated subatomic particle and how it can be used to identify the atom is:
The proton number remains constant through changing the atomic charge, energy, and isotopes.
The associated subatomic particle is the proton. The atomic number of an atom corresponds to the number of protons in its nucleus. Each element has a unique atomic number, which means it has a specific number of protons. This number remains constant for a particular element, regardless of changes in the atomic charge, energy, or even isotopes. Therefore, by knowing the atomic number, one can accurately identify the atom and its corresponding element.
Many people believe that the atomic number of the atom is the number of electrons in the atom. Describe when this is the case.
Question 3 options:
As the atom absorbs photons the electrons excite and produce unique emission spectrum.
Through radioactive decay the electrons and neutrons form unique atomic number isotopes.
Whether the atom is neutral or charged the number of electrons is always a unique identifier.
When the atom is neutral and the number of electrons and the number of protons are equal.
The option that accurately describes when the atomic number of the atom is the number of electrons in the atom is:
When the atom is neutral and the number of electrons and the number of protons are equal.
In a neutral atom, the number of electrons is equal to the number of protons. This balance of positive and negative charges ensures electrical neutrality. Therefore, in a neutral atom, the atomic number represents both the number of protons and the number of electrons. It serves as a unique identifier for the atom and helps determine its position in the periodic table.
Question 4 (1 point)
orbital diagrams for 4 elements - Li, He, N, S
Which two from this group have an identical number of energy levels?
Question 4 options:
Li and N
N and S
Li and He
He and N
The two elements from the group (Li, He, N, S) that have an identical number of energy levels are:
Li and He
Both lithium (Li) and helium (He) have 1 energy level.
What is true of valence electrons?
Question 5 options:
They easily move from one orbital to another.
They have difficulty moving from one orbital to another.
They exist in the outer orbital.
They are always the lowest energy electrons of the atom.
The option that is true of valence electrons is:
They exist in the outer orbital.
Valence electrons are the electrons that occupy the outermost energy level, also known as the valence shell, of an atom. These electrons have the potential to engage in bonding interactions with other atoms, as they are located in the outermost orbital.
Which statement is true about the electrons in the Bohr model of an atom?
Question 6 options:
They are equally close to the nucleus.
They give off energy as they jump to a higher level.
They exist at specific energy levels.
They cannot move from one orbital to another.
The statement that is true about the electrons in the Bohr model of an atom is:
They exist at specific energy levels.
In the Bohr model, electrons are depicted as orbiting the nucleus in specific energy levels or shells. Each energy level corresponds to a specific energy value, and electrons can occupy these levels without existing in between. This concept lays the foundation for understanding the quantized nature of electron energy in atoms.
What is the maximum number of electrons that can occupy a box in an orbital filling diagram at any energy level?
Question 7 options:
6
2
8
14
The maximum number of electrons that can occupy a box in an orbital filling diagram at any energy level is:
2
In accordance with the Pauli exclusion principle, each orbital can hold a maximum of 2 electrons with opposite spins. Therefore, a single box in an orbital filling diagram can represent the occupancy of 2 electrons.
An atom has a charge of −3 in its orbitals. Which statement must be true for this atom to have no net charge?
Question 13 options:
There are three positively charged protons in the nucleus.
There are three neutral neutrons in the nucleus.
There are three positively charged protons outside the nucleus.
There are two positively charged protons in the nucleus and one in an orbital.
To have no net charge, an atom with a charge of -3 must have three positively charged protons in the nucleus.
When an atom has a charge, it means that there is an imbalance between the number of protons (positive charge) and electrons (negative charge). In this case, the atom has a charge of -3, indicating that there are three more electrons than protons. To neutralize this charge and have no net charge, the atom would need three positively charged protons in the nucleus.
Choose the term from the item bank to its matching definition.
Question 2 options:
Noble Gas
Periodic Table
Halogen
Metals
Nonmetals
Element
Metalloids
period
1.
This is an element with full valence shell, very unreactive.
2.
This is the highly reactive family of elements with 7 valence electrons.
3.
This is a type of element that has many valence electrons, not a conductor.
4.
This is a substance that cannot be broken down further by chemical means.
5.
A horizontal row of elements in the periodic table.
6.
An arrangement of elements into rows and columns according to similarities in their properties.
7.
One of a class of elements having properties intermediate to metals and nonmetals.
8.
This is a group of elements with few valence electrons that conducts heat and electricity.
Noble Gas - 1. This is an element with a full valence shell, very unreactive.
Halogen - 2. This is the highly reactive family of elements with 7 valence electrons.
Nonmetals - 3. This is a type of element that has many valence electrons, not a conductor.
Element - 4. This is a substance that cannot be broken down further by chemical means.
Period - 5. A horizontal row of elements in the periodic table.
Periodic Table - 6. An arrangement of elements into rows and columns according to similarities in their properties.
Metalloids - 7. One of a class of elements having properties intermediate to metals and nonmetals.
Metals - 8. This is a group of elements with few valence electrons that conducts heat and electricity.