Answer:
Explanation:
Substances with giant covalent structures are solids with high melting and boiling points due to the nature of the covalent bonds and the three-dimensional network they form within the crystal lattice. This structure is also often referred to as a network covalent structure. Let's break down the key reasons why these substances have such properties:
1. **Strong Covalent Bonds**: In giant covalent structures, each atom forms strong covalent bonds with neighboring atoms. Covalent bonds involve the sharing of electrons between atoms. This sharing results in the formation of very strong and directional bonds, which require a significant amount of energy to break.
2. **Three-Dimensional Network**: In these substances, the covalent bonds extend in a three-dimensional network throughout the entire structure. This means that every atom is bonded to several neighboring atoms in all three spatial dimensions. This extensive network of covalent bonds creates a robust and interconnected structure.
3. **Lack of Weak Intermolecular Forces**: Unlike some other types of solids (e.g., molecular solids or ionic solids), giant covalent structures lack weak intermolecular forces, such as Van der Waals forces. In molecular solids, weak intermolecular forces are responsible for their relatively low melting and boiling points. In giant covalent structures, the primary forces holding the atoms together are the covalent bonds themselves, which are much stronger.
4. **High Bond Energy**: The covalent bonds in giant covalent structures have high bond energies, meaning that a substantial amount of energy is required to break these bonds. When a solid is heated, the energy provided must be sufficient to overcome the covalent bonds' strength, leading to the high melting and boiling points.
5. **Rigidity and Structural Integrity**: The three-dimensional covalent network imparts rigidity and structural integrity to the substance. This network resists deformation and allows the substance to maintain its solid form at high temperatures, as the covalent bonds continuously hold the structure together.
Examples of substances with giant covalent structures include diamond (composed of carbon atoms), graphite (also composed of carbon atoms but arranged differently), and various forms of silica (e.g., quartz and silicon dioxide). Diamond, in particular, is known for its exceptional hardness, high melting point, and remarkable optical properties, all of which are attributed to its giant covalent structure.
In summary, giant covalent structures have high melting and boiling points because of the strong covalent bonds, the three-dimensional network of bonds, and the absence of weak intermolecular forces. These factors combine to create a solid with exceptional stability and resistance to temperature-induced phase changes.
Substances with simple molecular structures are usually gases, liquids, or solids with low melting points due to the intermolecular forces between their molecules. The chemical identities of the molecules determine the types and strengths of these attractions, influencing the physical state of the substance.
Substances with simple molecular structures tend to be gases, liquids, or solids with low melting and boiling points because of the nature of intermolecular forces at play. Intermolecular forces are the attractions between molecules, which determine many of the physical properties of a substance. For instance, small, symmetrical molecules, such as H2, N2, O2, and F2, have weak intermolecular attractive forces and form molecular solids with very low melting points (below -200 °C).
In a liquid, intermolecular attractive forces hold the molecules together, though they still have sufficient kinetic energy to move relative to each other. In gases, the molecules have large separations compared to their sizes due to which the forces between them can be ignored, except during collisions.
Therefore, the chemical identities of the molecules in a substance determine the types and strengths of intermolecular attractions possible; this subsequently influences whether the substance is a gas, liquid, or solid, and its melting and boiling points.
Learn more about Intermolecular Forces here:
#SPJ11
Answer:
Decrease order of speed of atoms in solid state, liquid state and gaseous states: gas > liquid> solid
Decreasing order of space of atoms in solid state, liquid state and gaseous states: gas > liquid> solid
Explanation:
Solid state : In this state, the particles are closely packed and does not have any space between them. They have least kinetic energy due to restricted movement. This state has a definite shape and volume.
Liquid state : In this state, particles are present in random and irregular pattern. The particles are closely arranged but they can move from one place to another and thus have higher kinetic energy as compared to solids. This state has a definite volume but does not have a fixed shape.
Gaseous state : In this state, particles are loosely arranged and have a lot of space between them. They have highest kinetic energy. This state has indefinite volume as well as shape.
Decrease order of speed of atoms in solid state, liquid state and gaseous states: gas > liquid> solid
Decreasing order of space of atoms in solid state, liquid state and gaseous states: gas > liquid> solid
1s2 2s2 2p3
1s2 2s2 2p4
1s2 2s2 2p6
1s², 2s², 2p⁴
Electronic configuration is the distribution of electrons of an atom in atomic orbitals. As we know Oxygen is a non metal and is present in group 6 and period 2 with atomic number 8. The atomic number in fact specifies the number of protons. Hence, for a neutral oxygen atom there must be 8 electrons to balance the charges of protons.
These 8 electrons are distributed in two main energy levels i.e. n = 1 and 2 and sub energy levels i.e. s and p. According to certain rules like Aufbau Principle, Pauli's Exclusion Principle and Hund's Rule the electronic configuration for eight electrons is as,
1s², 2s², 2px², 2p¹, 2p¹
The electronic configuration for oxygen is 1s2 2s2 2p4.
The electron configuration for oxygen is 1s2 2s2 2p4.
In the electron configuration, the numbers represent the energy levels (1s, 2s, 2p), and the superscripts represent the number of electrons in each orbital. The electron configuration follows the Aufbau principle, which states that electrons fill the lowest energy levels first.
In the case of oxygen, there are 8 electrons in total. The first two electrons fill the 1s orbital, the next two fill the 2s orbital, and the remaining four fill the 2p orbital (with two electrons each in the three 2p orbitals).
#SPJ6
Minerals can be described using 7 key characteristics: color, streak, luster, crystal form, hardness, cleavage, and density. These characteristics provide detailed information about a mineral's geological properties.
The characteristics used to describe minerals are generally located in the detail of their geological properties. These characteristics include:
#SPJ2
(B) lattice energy
(C) kinetic energy
(D) activation energy
(E) ionization energy