Chapter 3: Problem 90
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
Expert verified
Statement (2) is false.
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
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.
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.
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.
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
