Sublevel being filled by element with atomic number 47 – In the realm of chemistry, the sublevel being filled by an element plays a crucial role in determining its properties and behavior. This article delves into the captivating case of element with atomic number 47, silver, to unravel the significance of its sublevel filling in shaping its identity.
Silver, a noble metal renowned for its lustrous sheen and exceptional electrical conductivity, owes its unique characteristics to the 4d sublevel being filled during its electron configuration. As we explore the intricate details of this process, we will uncover the profound impact it has on silver’s chemical bonding, physical properties, and diverse applications.
Sublevel Structure
Sublevels are subdivisions within energy levels that describe the specific orbitals occupied by electrons. Each sublevel is characterized by a unique set of quantum numbers, including the azimuthal quantum number (l). The azimuthal quantum number determines the shape and orientation of the orbital and is denoted by letters: s, p, d, f, and so on.
For an element with atomic number 47, the sublevel structure is as follows:
- 1s 2
- 2s 22p 6
- 3s 23p 63d 10
- 4s 24p 64d 9
The sublevel being filled is the 4d sublevel.
Electron Configuration
The electron configuration of the element with atomic number 47 is:
1s 22s 22p 63s 23p 63d 104s 24p 64d 9
The sublevel being filled is the 4d sublevel, which contains 9 electrons.
The element with atomic number 47 is silver (Ag).
Periodic Table Trends
Silver belongs to Group 11 (formerly known as Group IB) and Period 5 of the periodic table.
Across Group 11, the elements show a trend of increasing atomic radius and decreasing ionization energy. This is because as you move down the group, the electrons are added to higher energy levels, which are further away from the nucleus.
The decrease in ionization energy indicates that it becomes easier to remove an electron as you move down the group.
Across Period 5, the elements show a trend of increasing atomic number and effective nuclear charge. This is because as you move from left to right across the period, the number of protons in the nucleus increases, which attracts the electrons more strongly.
The increase in effective nuclear charge leads to an increase in ionization energy.
Chemical Bonding: Sublevel Being Filled By Element With Atomic Number 47
Silver can form various types of chemical bonds, including:
- Ionic bonds: Silver can lose one electron to form a cation with a +1 charge. This cation can then form ionic bonds with anions.
- Covalent bonds: Silver can also share electrons with other atoms to form covalent bonds. Covalent bonds are typically formed between non-metals.
- Metallic bonds: Silver is a metal and can form metallic bonds with other metals. Metallic bonds are formed between metal atoms that share their valence electrons.
Physical Properties
Silver is a white, lustrous metal with a high melting point (961.93 °C) and a high boiling point (2162 °C). It is also a good conductor of heat and electricity.
The 4d sublevel being filled contributes to silver’s physical properties. The 4d electrons are relatively close to the nucleus and are therefore strongly attracted to it. This strong attraction results in a high melting point and boiling point.
Applications
Silver has a wide range of applications, including:
- Jewelry: Silver is commonly used in jewelry making because it is malleable and ductile, making it easy to work with. Silver is also resistant to tarnishing, which makes it a popular choice for jewelry.
- Electronics: Silver is used in electrical contacts and conductors because it is a good conductor of electricity. Silver is also used in batteries and solar cells.
- Photography: Silver is used in photographic film and paper because it is sensitive to light. When light strikes silver, it causes the silver atoms to darken, creating an image.
- Medicine: Silver is used in some medical applications, such as antimicrobial coatings and wound dressings. Silver has antibacterial and antifungal properties, which makes it effective in preventing and treating infections.
Questions Often Asked
What is the significance of the 4d sublevel being filled in silver?
The 4d sublevel being filled in silver determines its position in the periodic table, influences its chemical bonding behavior, and contributes to its unique physical properties.
How does the sublevel filling affect silver’s chemical bonding?
The 4d sublevel being filled gives silver the ability to form various types of chemical bonds, including metallic bonds, covalent bonds, and ionic bonds, enabling it to interact with a wide range of elements.
What are some practical applications of silver?
Silver finds applications in electronics due to its high electrical conductivity, in medicine as an antimicrobial agent, and in photography as a light-sensitive material, among others.
