HOW TO READ THE PERIODIC TABLE

Each column in the table is referred to as a period. A period’s elements all have the same number of orbitals. This progression begins with a single orbital in the top row and ends with seven orbitals in the bottom row. Each row adds an orbital. Physical properties of elements belonging to the same era are similar.

Each column in a table is referred to as a group. Each set of elements has the same number of electrons in its outer shell, referred to as valence electrons. Elements belonging to the same group respond similarly to other elements.

• Part 1

• A Representative Periodic Table

1.) Recognize the Periodic Table’s Structure

From left to right, read the periodic table. The elements are classified according to their atomic numbers, which grow as the periodic table is traversed. The atomic number indicates the number of protons contained in an element’s atom. Additionally, you’ll notice that the atomic mass of each element grows as you progress across the chart. This means that you can infer a great deal about an element’s weight just by glancing at its position on the table.

The atomic mass of each element grows as you walk across or down the table, as the mass is computed by adding the protons and neutrons in its atom. With each element, the amount of protons increases, which results in an increase in weight.

Electrons are excluded from the atomic mass because they contribute significantly less weight to the atom than protons and neutrons do.

2.)  Note that each element has one additional proton compared to its predecessor. This can be determined by examining the atomic number. Atomic numbers are arranged in ascending order from left to right. Due to the fact that the elements are also grouped, you will see gaps in the table. 

For instance, the first row comprises Hydrogen (atomic number 1) and Helium (atomic number 2). They are, however, at opposing ends of the table due to their membership in distinct groupings.

3.)  Recognize groups that have similar physical and chemical characteristics. Groups, often called families, are arranged vertically. In most circumstances, groupings will also share a common colour. This enables you to determine which elements share comparable physical and chemical properties, allowing you to forecast their behaviour. [3] Each element within a group has an identical number of electrons in its outer orbital. 

While the majority of elements belong to a single group, hydrogen can be classified as a Halogen or an Alkali Metal. It will appear with both on some charts.

Columns are often numbered 1-18, either above or below the table. Roman numerals (IA), Arabic numerals (1A), or numerals may be used to represent the integers (1).

When you read a group down from top to bottom, this is referred to as “reading down a group.”

4.) Consider why the table contains gaps. While elements are classified according to their atomic number, they are also classified into groups and families with similar physical and chemical properties. This assists you in comprehending how each part behaves. Due to the fact that elements do not always neatly organise themselves as their number increases, the periodic table contains gaps. 

For instance, the first three rows are missing, as Transition Metals are not included in the table until atomic number 21.

Similarly, elements 57–71, together referred to as the Rare Earth Elements, are frequently depicted as a subset at the bottom right of the table.

5.) Take note that each row is referred to as a period. Each element inside a period has the same number of atomic orbitals, which are the locations of their electrons. The number of orbitals equals the period. There are seven rows, which indicates that there are seven eras. 

For instance, atoms in period 1 have a single orbital, but elements in period 7 have seven orbitals.

They are often numbered 1-7 along the left hand side of the table.

When you travel from left to right across a row, this is referred to as “reading across a period.”

6.) Separate metals, semimetals, and nonmetals. By identifying the type of element, you can gain a better understanding of its properties. Fortunately, the majority of periodic tables employ colour to identify whether an element is metallic, semi-metallic, or non-metallic. You’ll note that metals are listed on the left, while non-metals are listed on the right. Between them are semi-metals. 

Keep in mind that because hydrogen can be classified as a Halogen or an Alkali Metal based on its properties, it may appear on either side of the table or have a different colour.If an element has lustre, is solid at room temperature, conducts heat and electricity, and is malleable and ductile, it is classified as a metal.

If an element lacks lustre, does not conduct heat or electricity, and is not malleable, it is classified as a non-metal. At room temperature, these elements are usually gases, but can also exist as solids or liquids at specific temperatures.

Semi-metals are elements that exhibit characteristics of both metals and nonmetals.

• Part 2

• Investigating the Elements

1.) Recognize the element’s symbol, which ranges from one to two letters. It is most frequently displayed in a huge font in the box’s centre. The sign represents an abbreviation for the element’s name, which is standardised across languages. When conducting experiments or working with elemental equations, you will almost certainly employ the elements’ symbols, so it is critical to become familiar with them.

While this symbol is typically obtained from the Latin version of the element’s name, it may also be derived from the element’s commonly accepted common name, particularly for younger elements. For instance, Helium’s symbol is He, which nearly reflects its common name. However, the symbol for Iron is Fe, which is first more difficult to detect.

2.) If the element has a whole name, look for it. This is the element’s name as it will be written out. For instance, the elements “Helium” and “Carbon” are given names. This will typically display just beneath the sign, but its location may vary.

Certain periodic tables ignore the whole name in favour of the symbol.

3.) Calculate the atomic number. The atomic number is frequently displayed at the top of the box, in the middle or a corner. It may, however, be situated beneath the element symbol or name. The atomic numbers begin with 1 and end with 118.

The atomic number will be a decimal, not a whole number.

4.) Recognize that the atomic number represents the number of protons contained within an atom. Each atom of an element has the same number of protons. Unlike electrons, protons cannot be gained or lost by an atom. Otherwise, the element would alter its state!

Additionally, you’ll use the atomic number to determine the quantity of electrons and neutrons!

5.) Elements with known electron-proton ratios contain the same number of protons as electrons. If they are ionised, there is an exception. Electrons have a negative charge, while protons have a positive charge. Because ordinary atoms lack an electrical charge, electrons and protons are equal. An atom, on the other hand, can lose or receive electrons, causing it to become ionised.

Ions are charged electrically. If an ion contains more protons than electrons, it is positive, as shown by the presence of a plus sign next to the ion’s symbol. If an ion has more electrons than protons, it is negative, as shown by the negative sign.

If the element is not an ion, there will be no plus or minus symbol.

• Part 3

• Calculating Neutrons Using the Atomic Weight

1.) Calculate the atomic weight. The atomic weight is often listed below the element symbol at the bottom of the box. The atomic weight is the sum of the masses of the protons and neutrons in the nucleus. However, because ions complicate the computation, the atomic weight is calculated as the average of the element’s atomic mass and the atomic mass of its ions.

Due to the averaging of weights, the majority of elements will have atomic weights that include decimals.

While it may appear that the atomic weights grow in number from left to right, this is not always the case.

2.) Determine the element’s mass number. By rounding the atomic mass to the nearest whole number, you can obtain the mass number. This explains why the atomic weight of an element is calculated as the average of all potential atomic masses for that element, including ions. 

Carbon, for example, has an atomic weight of 12.011, which rounds to 12. Iron, on the other hand, has a mass of 55.847, which rounds to 56.

3.) To determine the neutrons, subtract the atomic number from the mass number. The mass number is calculated by combining the protons and neutrons together. This makes it simple to determine the number of neutrons in an atom simply by subtracting the number of protons from the mass number!

Utilize the following formula: Neutrons = Protons – Mass Number

Carbon, for example, has a mass number of 12 and six protons. Carbon contains six neutrons, since 12 – 6 = 6.

Another example is iron, which has a mass of 56 and 26 protons. Because 56 – 26 = 30, we know that Iron contains 30 neutrons.

Each isotope of an atom contains a varied number of neutrons, altering the atom’s weight.

CONCLUSION

From the following article we can conclude that A period is a row in the table. The number of orbitals for each element in a period is the same. The top row has one orbital, and the bottom row has seven. One orbital is added to each row. The physical properties of elements from the same era are similar.

A group is the name given to each column in the table. There are the same number of electrons in the outer shell, or valence electrons, of all the elements in each group The reactions of elements within the same group are very similar.