Module 3
1.Explain how scientific observations led to the development of the periodic table.
Dmitri Mendeleev- first periodic table, organized 63 known elements according to properties, organized
into rows and columns and wrote name, mass, chemical properties on each
Henry Gwyn Jefferys- worke with Earnest Rutherford, experimented with 38 metals,he found in
Mendeleev's periodic table ,led to modern definition of atomic number and the recognition the atomic
number was to the periodic table
2.Describe the organization of the modern periodic table.
A modern periodic table arranges the elements in increasing order of their atomic numbers and groups
atoms with similar properties in the same vertical column (Figure 3.2.23.2.2). Each box represents an
element and contains its atomic number, symbol, average atomic mass, and (sometimes) name. The
elements are arranged in seven horizontal rows, called periods or series, and 18 vertical columns,
called groups. Groups are labeled at the top of each column.
3.Identify groups and sections of the periodic table by group name and common
properties.
There are multiple ways of grouping the elements, but they are commonly divided into metals,
semimetals (metalloids), and nonmetals. You'll find more specific groups, like transition metals, rare
earths, alkali metals, alkaline earth, halogens, and noble gasses.
4.Define ionic and covalent bonding.Relate knowledge of the periodic trends to chemical bonding.
An ionic bond essentially donates an electron to the other atom participating in the bond, while
electrons in a covalent bond are shared equally between the atoms.
6. Determine ionic charge based on location of the periodic table.
An element's placement on the periodic table indicates whether its chemical charge is negative or
positive. Looking at the table, one can see that the positive charges are on the left side of the table and
the negative charges are on the right side of the table.
7. Determine how atoms will covalently bond together based on location on the periodic
table.
The number of electrons in the outermost shell of a particular atom determines its reactivity, or
tendency to form chemical bonds with other atoms. This outermost shell is known as the valence shell,
and the electrons found in it are called valence electrons.
8. Compare and contrast intermolecular forces and bonding.
Both types of forces determine the chemical and physical characteristics of substances. The main
difference between intermolecular and intramolecular forces is that intermolecular forces exist between
the molecules themselves, whereas intramolecular forces exist between atoms within a molecule.
9. Identify the intermolecular forces for 3 different types of compounds.
There are three types of intermolecular forces: London dispersion forces (LDF), dipole- dipole
interactions, and hydrogen bonding.
10. Provide an example where you calculate the molar mass of a given compound.
To calculate the molar mass of a compound with multiple atoms, sum all the atomic mass of the
constituent atoms. For example, the molar mass of NaCl can be calculated for finding the atomic mass of
sodium (22.99 g/mol) and the atomic mass of chlorine (35.45 g/mol) and combining them.
This study source was downloaded by 100000857952895 from CourseHero.com on 01-10-2023 11:24:43 GMT -06:00
https://www.coursehero.com/file/119019433/0308-Molecules-and-Compounds-Discussion-Based-Assessmentdocx/
1.Explain how scientific observations led to the development of the periodic table.
Dmitri Mendeleev- first periodic table, organized 63 known elements according to properties, organized
into rows and columns and wrote name, mass, chemical properties on each
Henry Gwyn Jefferys- worke with Earnest Rutherford, experimented with 38 metals,he found in
Mendeleev's periodic table ,led to modern definition of atomic number and the recognition the atomic
number was to the periodic table
2.Describe the organization of the modern periodic table.
A modern periodic table arranges the elements in increasing order of their atomic numbers and groups
atoms with similar properties in the same vertical column (Figure 3.2.23.2.2). Each box represents an
element and contains its atomic number, symbol, average atomic mass, and (sometimes) name. The
elements are arranged in seven horizontal rows, called periods or series, and 18 vertical columns,
called groups. Groups are labeled at the top of each column.
3.Identify groups and sections of the periodic table by group name and common
properties.
There are multiple ways of grouping the elements, but they are commonly divided into metals,
semimetals (metalloids), and nonmetals. You'll find more specific groups, like transition metals, rare
earths, alkali metals, alkaline earth, halogens, and noble gasses.
4.Define ionic and covalent bonding.Relate knowledge of the periodic trends to chemical bonding.
An ionic bond essentially donates an electron to the other atom participating in the bond, while
electrons in a covalent bond are shared equally between the atoms.
6. Determine ionic charge based on location of the periodic table.
An element's placement on the periodic table indicates whether its chemical charge is negative or
positive. Looking at the table, one can see that the positive charges are on the left side of the table and
the negative charges are on the right side of the table.
7. Determine how atoms will covalently bond together based on location on the periodic
table.
The number of electrons in the outermost shell of a particular atom determines its reactivity, or
tendency to form chemical bonds with other atoms. This outermost shell is known as the valence shell,
and the electrons found in it are called valence electrons.
8. Compare and contrast intermolecular forces and bonding.
Both types of forces determine the chemical and physical characteristics of substances. The main
difference between intermolecular and intramolecular forces is that intermolecular forces exist between
the molecules themselves, whereas intramolecular forces exist between atoms within a molecule.
9. Identify the intermolecular forces for 3 different types of compounds.
There are three types of intermolecular forces: London dispersion forces (LDF), dipole- dipole
interactions, and hydrogen bonding.
10. Provide an example where you calculate the molar mass of a given compound.
To calculate the molar mass of a compound with multiple atoms, sum all the atomic mass of the
constituent atoms. For example, the molar mass of NaCl can be calculated for finding the atomic mass of
sodium (22.99 g/mol) and the atomic mass of chlorine (35.45 g/mol) and combining them.
This study source was downloaded by 100000857952895 from CourseHero.com on 01-10-2023 11:24:43 GMT -06:00
https://www.coursehero.com/file/119019433/0308-Molecules-and-Compounds-Discussion-Based-Assessmentdocx/
