Question

Group the following electron configurations in pairs that would represent elements with similar chemical properties: (a) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}\) (d) \(1 s^{2} 2 s^{2}\) (b) \(1 s^{2} 2 s^{2} 2 p^{3}\) (e) \(1 s^{2} 2 s^{2} 2 p^{6}\) (c) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6}\) (f) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3}\)

Short answer

Pairs are (a, d), (b, f), and (c, e).

Step-by-step solution

Identify the Element for Each Electron Configuration

Each electron configuration corresponds to an element on the periodic table. We identify the elements as follows: - (a) corresponds to Magnesium (Mg) - (b) corresponds to Nitrogen (N) - (c) corresponds to Krypton (Kr) - (d) corresponds to Beryllium (Be) - (e) corresponds to Neon (Ne) - (f) corresponds to Phosphorus (P)

Determine Chemical Properties Based on Group

Elements with similar chemical properties belong to the same group (column) on the periodic table. We locate the elements on the periodic table: - Magnesium (a) is in Group 2 - Nitrogen (b) is in Group 15 - Krypton (c) is in Group 18 - Beryllium (d) is in Group 2 - Neon (e) is in Group 18 - Phosphorus (f) is in Group 15

Pair Elements with Similar Chemical Properties

Pair elements from the same group, as they share similar chemical properties: - Pair (a) Magnesium with (d) Beryllium, both from Group 2 - Pair (b) Nitrogen with (f) Phosphorus, both from Group 15 - Pair (c) Krypton with (e) Neon, both from Group 18

Key concepts

Periodic Table

The periodic table is like a big chart that organizes all the chemical elements based on their properties. It was invented to make sense of how elements behave and react with each other. Elements on the periodic table are arranged by their atomic number, which is the number of protons in their nucleus. This organizing helps us predict the properties of elements and how they interact.

The layout divides elements into rows, called periods, and columns, known as groups. The position of an element in the periodic table can tell us a lot about its characteristics and chemical behavior. For example, elements in the same group have the same number of valence electrons, which are the electrons in the outermost shell. Valence electrons are critical because they determine an element's reactivity and which chemical bonds they can form.

In summary, the periodic table is an essential tool for chemists. It organizes elements by their properties and helps predict how different substances will react together.

Chemical Properties

Chemical properties of an element refer to the element's ability to undergo chemical changes or reactions based on its electron configuration. These properties are heavily influenced by the arrangement of electrons around an atom. Elements with similar electron configurations tend to have similar chemical properties. This is because similar configurations lead to similar ways of reacting with other elements.

For example, elements in Group 2 of the periodic table, like Magnesium and Beryllium, have two electrons in their outermost shell. This makes them likely to lose these outer electrons in reactions, thus forming similar compounds. In contrast, Group 18 elements like Neon and Krypton have complete outer shells, making them mostly non-reactive, or inert.

Understanding chemical properties is crucial for predicting how substances will behave in chemical reactions, helping us to foresee the results of combining different elements. It provides a fundamental insight into why and how reactions occur, which is essential for studies of materials and chemistry.

Element Groups

Element groups are the columns in the periodic table. Each group contains elements with the same number of valence electrons, which gives them similar chemical properties. This similarity is useful in predicting how elements react with others in chemical reactions.

Elements in the same group are often known as a 'family' of elements due to their similar properties. For instance, Group 1 contains alkali metals like lithium, sodium, and potassium. These metals are highly reactive, particularly with water, due to their single valence electron moving to achieve a stable configuration.

Moving to Group 2, the alkaline earth metals, such as magnesium and beryllium, are slightly less reactive but still easily form compounds by losing their two outer electrons. Another key group is the halogens, found in Group 17, which include fluorine and chlorine. These elements are very reactive, particularly with alkali metals, due to their seven valence electrons.

• Group 1: Highly reactive alkali metals.
• Group 2: Alkaline earth metals, losing two electrons easily.
• Group 17: Reactive halogens needing one more electron for stability.
• Group 18: Noble gases, inert and stable.

Understanding element groups and their characteristics can greatly aid in predicting and explaining chemical reactions.