Well,its because the particles that constitute solids are closer together hence the forces of attraction are greater rising the boiling point and melting points are raised as the heat try to break the bonds
No, the trends for melting points and boiling points in nonmetals are generally different from those in metals. Nonmetals typically have lower melting and boiling points compared to metals, which tend to have high melting and boiling points due to strong metallic bonds. In nonmetals, the melting and boiling points can vary significantly based on molecular structure and intermolecular forces, with noble gases having very low points and some covalent network solids like diamond having high points. Therefore, while both groups exhibit trends, the underlying reasons and values differ significantly.
Electrovalent compounds have high melting and boiling points because they have strong electrostatic forces of attraction between the positively charged metal ions and negatively charged non-metal ions. These forces require a significant amount of energy to overcome, resulting in high melting and boiling points for these compounds.
The structure of a compound will dictate what intermolecular forces hold the molecules together. The stronger these forces, the higher will be the boiling point.
Which metal needs to be specified. Look in a Chemistry book or reference book. All metals have their own melting and boiling points - that's one of the ways we identify which metal the item is made of.
Poor conductors of heat and electricity. Brittle and not malleable. Low melting and boiling points. Dull appearance. Tend to gain electrons in chemical reactions. Mostly gases or solids at room temperature. Generally have high electronegativity.
metals
No, the trends for melting points and boiling points in nonmetals are generally different from those in metals. Nonmetals typically have lower melting and boiling points compared to metals, which tend to have high melting and boiling points due to strong metallic bonds. In nonmetals, the melting and boiling points can vary significantly based on molecular structure and intermolecular forces, with noble gases having very low points and some covalent network solids like diamond having high points. Therefore, while both groups exhibit trends, the underlying reasons and values differ significantly.
Ionic solids typically have high melting points due to the strong electrostatic forces binding the positive and negative ions together in a lattice structure. When heated, these bonds must be overcome, requiring a significant amount of energy, resulting in high melting points.
Boiling point decrease at high altitude.
Simple molecular substances typically have low melting and boiling points. This is because the weak intermolecular forces, such as London dispersion forces, in simple molecular substances are easily overcome compared to the stronger bonds in ionic or metallic substances.
The boiling points of ionic solids tend to be very high.
Electrovalent compounds have high melting and boiling points because they have strong electrostatic forces of attraction between the positively charged metal ions and negatively charged non-metal ions. These forces require a significant amount of energy to overcome, resulting in high melting and boiling points for these compounds.
The structure of a compound will dictate what intermolecular forces hold the molecules together. The stronger these forces, the higher will be the boiling point.
1)brittleness 2)high melting points 3)high boiling points
Metallically bonded compounds have high melting and boiling points due to the strength of their bonds. Metallic bonds are very strong and therefore take a lot of energy to break, which could be heat. This is why lots of heat energy is needed to break down each individual metallic bond
They have low melting points and high reactivity.
Ionic solids exhibit high melting points due to the strong electrostatic forces between the positively and negatively charged ions. These forces require a significant amount of energy to overcome in order to break the crystal lattice structure and transition to the liquid phase.