Question

Which of the following statement is false? (1) An clement having clectronic configuration \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}\) forms basic oxide. (2) Chloride of an clement \(\Lambda\) gave a neutral solution in water. In the periodic table the clement \(\Lambda\) belongs to III group.

Short answer

Statement (2) is false.

Step-by-step solution

Analyze Electronic Configuration

Examine the electronic configuration provided in statement (1):\[ 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{1} \]This configuration corresponds to potassium (K), which is in Group 1 of the periodic table. Elements in Group 1, like potassium, typically form basic oxides.

Assess Chloride of Element in Group III

Consider statement (2) regarding element \( \Lambda \) from Group III. Elements in Group III of the periodic table include boron (B), aluminum (Al), gallium (Ga), indium (In), and thallium (Tl). Typically, chlorides of these elements are acidic or weakly acidic, not neutral.

Determine the False Statement

Based on Steps 1 and 2, it is established that statement (1) is true because potassium forms a basic oxide. In contrast, statement (2) is false because chlorides of Group III elements do not typically form neutral solutions in water. Hence, statement (2) is the incorrect one.

Key concepts

Electronic Configuration

Understanding electronic configuration is vital in chemistry.
This notation describes the arrangement of electrons in an atom's orbitals based on increasing energy levels.
For example, the configuration \(1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{1}\) belongs to potassium (K).
This tells us potassium has 1 electron in the 4s orbital, which informs us about its position and properties.
The configuration reveals that potassium is in Group 1 (alkali metals) and Period 4 of the periodic table.
This arrangement helps predict chemical behaviors, reactivity, and the types of bonds the element can form. Each element’s properties are deeply connected to its electronic structure.

Group Trends in Periodic Table

Elements in the periodic table are organized based on their atomic number, electron configurations, and recurring chemical properties.
One way to predict these properties is by looking at group trends.
Elements in the same group (vertical columns) have similar chemical properties because they have the same number of electrons in their outermost shell.
For instance, Group 1 elements (alkali metals) all have one electron in their outermost shell, making them highly reactive and prone to forming basic oxides.
On the other hand, Group III elements (such as boron, aluminum) typically form acidic or weakly acidic chlorides rather than neutral ones.
By understanding these trends, you can predict an element's behavior, reactivity, and the type of compounds it will form.

Chemical Properties of Elements

The chemical properties of elements depend heavily on their electronic configurations and their position in the periodic table.
For example, potassium (Group 1) forms basic oxides because it readily loses its one valence electron to form positive ions, which then combine with oxygen.
Conversely, Group III elements like aluminum form amphoteric oxides that can act both as acids and bases.
When these elements form chlorides, they often produce solutions that are not neutral.
These chemical properties are essential for understanding reactions, bonding, and how different elements will interact with each other.

• Group 1: highly reactive, form basic oxides
• Group III: form acidic or weakly acidic chlorides, typically not neutral

By grasping these concepts, you can better predict how elements will behave in various chemical reactions.