1.) How does reading across a periodic table compare and contrast with reading down a group on the periodic table?

Reading across a periodic table, also known as reading from left to right, allows you to compare elements in terms of their atomic number, electron configuration, and properties. When reading across, you move through different groups of elements.

By contrast, reading down a group on the periodic table, also known as reading in a column, allows you to see similarities in terms of valence electrons, atomic radius, and chemical reactivity. When reading down a group, you move through different periods of the periodic table.

To understand how reading across and reading down the periodic table compare and contrast, follow these steps:

1. Start by finding a periodic table. You can easily find one online or in a chemistry textbook.

2. To read across the periodic table, start from the leftmost side and move towards the right. As you do this, you will notice that elements in the same group (vertical columns) tend to have similar properties. This is because they have the same number of valence electrons, which influences their reactivity and chemical behavior.

3. While reading across, you will also notice that elements become progressively smaller in size from left to right. This trend is due to an increasing number of protons, which results in a greater positive charge in the nucleus and stronger attraction to the electrons.

4. To read down a group, start from the topmost element in a column and move downwards. As you do this, you will see a recurring pattern of similar chemical properties within the group. This similarity is due to the fact that elements in the same group have the same number of valence electrons, resulting in comparable reactivity.

5. Another trend when reading down a group is an increase in atomic radius as you move lower. This is because additional energy levels are being added to the electron shells, resulting in a larger atomic size.

Remember, these comparisons and contrasts are general trends, and there may be exceptions and variations within certain groups or periods of the periodic table.