Question

For each of the following atomic numbers, use the periodic table to write the formula (including the charge) for the simple ion that the element is most likely to form. a. 53 b. 38 c. 55 d. 88 e. 9 f. 13

Short answer

The simple ions that the elements with these atomic numbers are most likely to form are: a. I⁻ (Iodine) b. Sr²⁺ (Strontium) c. Cs⁺ (Cesium) d. Ra²⁺ (Radium) e. F⁻ (Fluorine) f. Al³⁺ (Aluminum)

Step-by-step solution

Identifying the Elements with Given Atomic Numbers

Let's find out which elements represent the given atomic numbers: a. 53 - Iodine (I) b. 38 - Strontium (Sr) c. 55 - Cesium (Cs) d. 88 - Radium (Ra) e. 9 - Fluorine (F) f. 13 - Aluminum (Al)

Group Numbers and Predicting Ion Charge

Now, we need to find the group numbers in the periodic table for each element, which will help us determine the most likely ion charges: a. Iodine (I) - Group 17 (Halogens) – these form -1 anions. b. Strontium (Sr) - Group 2 (Alkaline Earth Metals) – these form +2 cations. c. Cesium (Cs) - Group 1 (Alkali Metals) – these form +1 cations. d. Radium (Ra) - Group 2 (Alkaline Earth Metals) – these form +2 cations. e. Fluorine (F) - Group 17 (Halogens) – these form -1 anions. f. Aluminum (Al) - Group 13 - these form +3 cations.

Writing the Ionic Formula

Now that we have identified the most likely charges for each ion, we can write the formula. a. Iodine (I) - I⁻ b. Strontium (Sr) - Sr²⁺ c. Cesium (Cs) - Cs⁺ d. Radium (Ra) - Ra²⁺ e. Fluorine (F) - F⁻ f. Aluminum (Al) - Al³⁺ So, the simple ions that these elements are most likely to form are: a. I⁻ b. Sr²⁺ c. Cs⁺ d. Ra²⁺ e. F⁻ f. Al³⁺

Key concepts

Periodic Table

The periodic table is a scientific tool that organizes all known chemical elements based on their atomic number, electron configurations, and recurring chemical properties. It helps predict elements' behaviors based on their position. Every element is situated in a specific row or period and column or group.
The periodic table places elements in periods (horizontal rows) and groups (vertical columns).

• Elements in the same group often have similar properties and form similar ions.
• By understanding the table layout, we can deduce how different elements might behave in chemical reactions.

The placement is such that it allows a systematic understanding of element properties, such as electronegativity and ionization energies.
This means one can use the table to make educated guesses about how an element might interact with others.

Atomic Number

The atomic number is a fundamental property of an element that indicates the number of protons in an atom's nucleus. This number decision not only determines the element's identity but also its position on the periodic table.
For example:

• Element 53 is Iodine (I) because it has 53 protons.
• Element 38 is Strontium (Sr), characterized by its 38 protons.

The uniqueness of each element comes from its atomic number, making it a key identifier in chemistry.
Moreover, since the atomic number also equals the number of electrons in a neutral atom, it influences how an element forms ions by gaining or losing electrons.

Ion Charge

Ion charge refers to the electrical charge an atom carries when it gains or loses electrons during ionic bonding. Atoms tend to achieve a full outer electron shell, also known as a noble gas configuration.

• Elements lose electrons: they form positively charged ions or cations.
• Elements gain electrons: they form negatively charged ions or anions.

For example, group 17 elements like Iodine ( I⁻ ) form anions with a charge of -1 by gaining one electron.
Besides, group 1 elements like Cesium ( Cs⁺ ) form cations with a charge of +1 by losing one electron. Recognizing the possible charges aids in predicting chemical reactions and the kind of bonds elements might form.

Chemical Elements

Chemical elements are pure substances that consist of only one type of atom. Here, each element is defined by its atomic number and possesses unique characteristics.
In combining, elements form chemical compounds by entering chemical reactions. Each element has distinct properties that determine how it participates in reactions.

• For instance, Fluorine (F) is known for forming stable compounds like fluorides.
• Aluminum (Al) is known for its strong and lightweight properties, making it valuable in manufacturing.

Understanding the nature of each element helps in predicting the formations of ions and the types of chemical reactions they might undergo.