Answer: Option (c) is the correct answer.
Explanation:
According to Le Chatelier's principle, when a system is in equilibrium for a long time then it will change its concentration, temperature, volume or pressure to attain a new equilibrium that partly counteracts the applied change.
Since it is given that reaction is exothermic therefore, according to Le Chatelier's principle increase in temperature will be opposed so that reaction can proceed in the forward direction. Therefore, temperature has to be decreased to carry the reaction in forward direction.
Whereas pressure has to be increased so that reaction will shift to the forward side where there are less number of molecules.
Thus, we can conclude that to increase the yield of the products for the given reaction decrease the temperature and increase the pressure.
b. oil
c. natural gas
d. uranium
mass
neutrons
electrons
Answer:energy
Explanation:
Energy can be added to an atom to cause a non-valence electron in the atom to temporarily become a valence electron. The correct option is A.
Valence electrons are those electrons that are present in the outermost shell of the atom. These electrons are free to form bonds with another atoms.
Non-valence electrons are preset in the inner shell of the element. These shell are fulfilled with electrons, and these electrons does need to form bonds with other atoms to fulfill their orbit.
The electrons in the orbit have different energies present. The energy change when the electrons transfer from one shell to another shell. When energy is given to the electron, they move to the higher orbit or shell.
Thus, the correct option is A, energy.
To learn more about valence electrons, refer to the link:
#SPJ6
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 giant covalent structures have high melting and boiling points due to the strong covalent bonds that exist throughout their structure. The size of the molecules and the polarizability of the atoms also impact these properties. However, covalent compounds generally have lower melting and boiling points than ionic compounds.
Substances with giant covalent structures are typically solids with high melting and boiling points due to the extensive network of strong covalent bonds that require a lot of energy to break. An example of this would be carbon dioxide (CO₂) and iodine (I₂) which are molecular solids with defined melting points. The size of the molecule impacts the strength of the intermolecular attractions.
Larger atoms have valence electrons that are further from the nucleus and less tightly held, making them more easily distorted to form temporary dipoles leading to stronger dispersion forces. This concept is known as polarizability. Therefore, substances which consist of larger, nonpolar molecules tend to have higher melting and boiling points due to larger attractive forces.
However, compounds with covalent bonds have different physical properties than ionic compounds. Covalent compounds generally have much lower melting and boiling points than ionic compounds, due to the weaker attraction between electrically neutral molecules than that between electrically charged ions.
Learn more about Giant Covalent Structures here:
#SPJ11
will mark brainliest!!
b. protons, electrons and neutrons are evenly distributed throughout the volume of the atom.
c. the nucleus is made of electrons and protons
Electrons are distributed in shells revolving around the nucleus and occupy almost all the volume of the atom.
In the nucleus of an atom, proton and neutron are present whereas electrons are present in shells revolving around the nucleus. Most of the volume of an atom has empty spaces in which shells are present in which electrons are moving.
The number of protons and electrons are the same in an atom but the number of neutrons are different so we can conclude that electrons are distributed in shells that are present around the nucleus.
Learn more: brainly.com/question/3132105
As a consequence of the discovery of the nucleus, the model of the atom that is true is A. electrons are distributed around the nucleus and occupy almost all the volume of the atom.
It should be noted that neutron and proton can be found in the nucleus of an atom. Also, there are electrons that are present in the shells that revolve around the nucleus.
In the atom, the number of electrons and protons are the same but there are different neutrons. Lastly, most of the volume of the atom has empty spaces.
Read related link on: