The stable balance of attractive and repulsive forces between atoms when they share electrons is known as covalent bonding. As the valency of germanium is 4, it can share 4 electrons of neighboring atom to complete the octet. Hence, Ge has covalent bond.

Examples of covalent compounds include:

• O2 – oxygen.
• Cl2 – chlorine.
• PCl3 – phosphorus trichloride.
• CH3CH2OH – ethanol.
• O3 – ozone.
• H2 – hydrogen.
• H2O – water.
• HCl – hydrogen chloride.

In chemistry, a double bond is a covalent bond between two atoms involving four bonding electrons as opposed to two in a single bond. Double bonds occur most commonly between two carbon atoms, for example in alkenes.

Covalent bonds can be single, double, and triple bonds. Single bonds occur when two electrons are shared and are composed of one sigma bond between the two atoms. Double bonds occur when four electrons are shared between the two atoms and consist of one sigma bond and one pi bond.

Covalent compounds have bonds where electrons are shared between atoms. Due to the sharing of electrons, they exhibit characteristic physical properties that include lower melting points and electrical conductivity compared to ionic compounds.

Covalent bond, in chemistry, the interatomic linkage that results from the sharing of an electron pair between two atoms. The binding arises from the electrostatic attraction of their nuclei for the same electrons.

Ionic bonds form between a metal and a nonmetal, whereas, covalent bonds form between two nonmetals….Complete step by step answer:

A covalent bond is a result of sharing electrons between two atoms. The main difference between electrovalent and covalent bond is that electrovalent bond is formed when two atoms are in an electrostatic attraction whereas covalent bond is formed when two atoms share their electrons with each other.

The key difference between covalent and noncovalent bonds is that covalent bonds form when two atoms share their electrons with each other whereas noncovalent bonds form either by completely exchanging electrons between two atoms or by not exchanging any electron.

There is a couple different ways to determine if a bond is ionic or covalent. By definition, an ionic bond is between a metal and a nonmetal, and a covalent bond is between 2 nonmetals. So you usually just look at the periodic table and determine whether your compound is made of a metal/nonmetal or is just 2 nonmetals.

HCN is a covalent molecule and not ionic. It dissociates in water to give and . The polar covalent compounds only dissociate in water to give ions. Both HCl and HCN are polar compounds and hence, they dissociate in water and give ions.

Ion-ion, dipole-dipole and ion-dipole interactions The strongest type of non-covalent interaction is between two ionic groups of opposite charge (an ion-ion or charge-charge interaction). This is called a dipole-dipole interaction.

ionic bond

London dispersion forces

Van der Waals forces are the weakest intermolecular force and consist of dipole-dipole forces and dispersion forces.

In order from strongest to weakest, the intermolecular forces given in the answer choices are: ion-dipole, hydrogen bonding, dipole-dipole, and Van der Waals forces. Ionic bonding is stronger than any of the given intermolecular forces, but is itself NOT an intermolecular force.

Van der Waals forces (partially known as London forces) are the residual attractive or repulsive forces between molecules or atomic groups that do not arise from a covalent bond, or electrostatic interaction of ions or of ionic groups with one another or with neutral molecules.

Neutral molecules may be held together by a weak electric force known as the van der Waals bond.

The three types of van der Waals forces include: 1) dispersion (weak), 2) dipole-dipole (medium), and 3) hydrogen (strong). Ion-dipole bonds (ionic species to covalent molecules) are formed between ions and polar molecules. These compounds typically form medium to strong bonds.

The structure of the DNA helix is stabilized by van der Waals forces, hydrogen bonds between complementary organic bases (a base pair), and hydrophobic interactions between the nitrogenous bases and the surrounding sheath of water.

Van der Waals forces’ is a general term used to define the attraction of intermolecular forces between molecules. There are two kinds of Van der Waals forces: weak London Dispersion Forces and stronger dipole-dipole forces.

Van der Waals forces may be attractive or repulsive, depending on the distance between the molecules involved. Recall that Van der Waals forces generally refer to intermolecular forces . These forces are generally attractive at normal pressures.

Number of Electrons Held by the Atoms/Molecules The greater the number of (instantaneous) dipoles formed, the greater the strength of the Van der Waals force.