Ionic compounds are mad by ionic bonding The two parts of the compound ther for become one by means of moving electronioc and beoming stable there fore the bond and the compound is stronger that conalent compounds which just share the electrons needed for the two (or more ) elements to become a compound so they are weaker
Simple molecular compounds have discrete molecules held together by weak intermolecular forces, while giant molecular compounds have repeating units bonded together by strong covalent bonds. Simple molecular compounds typically have low melting and boiling points and are often gases or liquids at room temperature, while giant molecular compounds tend to have high melting and boiling points and are usually solids at room temperature.
No, molecules of alkanes have weak intermolecular forces (London dispersion forces) due to their simple linear structure with only van der Waals interactions. This results in low melting points for alkanes compared to many other types of compounds.
Yes, salts do form covalent bonds. Actually, no bond is 100% ionic or covalent. For example, if you consider NaCl, even though it is considered ionic, it has some amount of covalent character in its bond.
The giant structure involve an enormous number of atoms.
simple molecules are bonds between non-metals and elements, or in some cases, non-metals and non-metals. Things like Water, CO2, I2 are simple moleculars. The single molecules of simple moleculars are held together through covalent bonds, the intermolecular forces that hold together many bonds are weaker, thus simple moleculars have low melting/boiling points. Giant Metallics are bonds between metals, such as Zinc Magnesium, and have strong bonds among and between atoms, with high melting/boiling points and ability to conduct electricity.
No they have high melting and boiling points. Don't get confused with simple molecular structures such as water and carbon dioxide which have simple covalent structures. When you heat them you are overcoming the forces BETWEEN THE MOLECULES (intermolecular/van der waals forces of attraction), NOT the actual covalent bonds themselves, like the bond betwen the C and either O in carbon dioxide.
Simple molecular compounds have discrete molecules held together by weak intermolecular forces, while giant molecular compounds have repeating units bonded together by strong covalent bonds. Simple molecular compounds typically have low melting and boiling points and are often gases or liquids at room temperature, while giant molecular compounds tend to have high melting and boiling points and are usually solids at room temperature.
It is a saturated hydrocarbon. It is a covalent compound and has all properties which are identical to simple covalent compounds. Low boiling and melting points, soluble in organic solvents (most simple covalent compounds are soluble in organic solvent), insoluble in water and does not conduct electricity as in does not have free ions.Its tetrahedral geometry makes it non-polar.It contains four hydrogen atoms
Binary covalent compounds consist of two nonmetals that share electrons to form a covalent bond. They have simple molecular structures with low melting and boiling points. They do not conduct electricity in any state.
Substances that usually contain covalent bonds have a simple molecular structure. Examples include elements like oxygen and compounds like methane. Giant molecular structures are typically found in substances with strong covalent bonds, such as diamond and quartz.
It is a saturated hydrocarbon. It is a covalent compound and has all properties which are identical to simple covalent compounds. Low boiling and melting points, soluble in organic solvents (most simple covalent compounds are soluble in organic solvent), insoluble in water and does not conduct electricity as in does not have free ions.Its tetrahedral geometry makes it non-polar.It contains four hydrogen atoms
Covalent compounds are formed by the sharing of electrons, hence the bonding is relatively weak. On the other hand, ionic compounds are formed by the transferring of electrons thus strong electrostatic forces holds the compound together, the strength in these forces co-existing within the ionic compounds require a large amount of energy to break it apart hence boiling and melting points are high.
Silicon compounds can exhibit both ionic and covalent bonding. Compounds such as silicon dioxide (SiO2) have a covalent structure, while compounds like silicon carbide (SiC) can have more ionic character. The nature of bonding in silicon compounds depends on the electronegativity difference between silicon and the other elements involved.
*soft-tend to be gases, liquids, or gases *poor conductors of heat & electricity *brittle or cleave rather than deform *nonelectrolytes-do not conduct electricity in water
its simple. ionic compounds have strong electrovalent bonds which need more heat to be broken down. hence more heat is needed to convert the solid into its other state. therefore high melting and boiling point.
Simple molecular structures like H2O and CO2 have the following properties: 1) Physical state: usually liquids and gases at room temperature due to weak intermolecular forces 2) Melting and boiling points: low (below 2000 C) melting and boiling points due to weak intermolecular forces 3) Electrical conductivity: cannot conduct electricity because there are no free electrons 4) Solubility: insoluble in water, but soluble in organic substances such as petrol Macromolecular structures such as diamond and SiO2 have the following properties: 1) Physical state: hard solids at room temperature due to the many strong covalent bonds holding the atoms together 2) Melting and boiling points: high melting and boiling points due to the many strong covalent bonds that must be broken before the substance can change state 3) Electrical conductivity: cannot conduct electricity because there are no free electrons 4) Solubility: insoluble
Because although the covalent bonds between the elements are strong, there are only weak forces between the molecules so they have low melting points