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