What type of bond holds o2 together

The nature of the interaction between the atoms depends on their relative electronegativity. Atoms with equal or similar electronegativity form covalent bonds, in which the valence electron density is shared between the two atoms. The electron density resides between the atoms and is attracted to both nuclei. This type of bond forms most frequently between two non- metals. When there is a greater electronegativity difference than between covalently bonded atoms, the pair of atoms usually forms a polar covalent bond.

The electrons are still shared between the atoms, but the electrons are not equally attracted to both elements. As a result, the electrons tend to be found near one particular atom most of the time. Again, polar covalent bonds tend to occur between non-metals. Finally, for atoms with the largest electronegativity differences such as metals bonding with nonmetals , the bonding interaction is called ionic, and the valence electrons are typically represented as being transferred from the metal atom to the nonmetal.

Once the electrons have been transferred to the non-metal, both the metal and the non-metal are considered to be ions. The two oppositely charged ions attract each other to form an ionic compound. Covalent interactions are directional and depend on orbital overlap, while ionic interactions have no particular directionality.

Each of these interactions allows the atoms involved to gain eight electrons in their valence shell, satisfying the octet rule and making the atoms more stable. These atomic properties help describe the macroscopic properties of compounds. For example, smaller covalent compounds that are held together by weaker bonds are frequently soft and malleable.

On the other hand, longer-range covalent interactions can be quite strong, making their compounds very durable. Ionic compounds, though composed of strong bonding interactions, tend to form brittle crystalline lattices. Ionic bonds are a subset of chemical bonds that result from the transfer of valence electrons, typically between a metal and a nonmetal. Ionic bonds are a class of chemical bonds that result from the exchange of one or more valence electrons from one atom, typically a metal, to another, typically a nonmetal.

This electron exchange results in an electrostatic attraction between the two atoms called an ionic bond. An atom that loses one or more valence electrons to become a positively charged ion is known as a cation, while an atom that gains electrons and becomes negatively charged is known as an anion. This exchange of valence electrons allows ions to achieve electron configurations that mimic those of the noble gases, satisfying the octet rule.

The octet rule states that an atom is most stable when there are eight electrons in its valence shell. Other examples of covalent bonds are water H2O and carbon dioxide CO2. Covalent compounds are generally liquids or gases with a low melting point. Covalent bonds hold atoms together because the attraction between the positively charged nuclei and the shared negatively charged electrons is greater than the repulsion between the nuclei themselves.

When two atoms come together, the electrons in their outer shell begin to notice the nucleus of the other atom. Covalent Bonds in Water The hydrogen atoms in the H2O water molecule form the same type of covalent bond as the hydrogen gas, but with the oxygen atom. The oxygen atom has six electrons in its outermost electron shell which can hold eight electrons.

The single electron dot diagram indicates that O2 has a double bond a sigma bond and a pi bond between the two oxygen atoms. Each oxygen also has 2 unbound electron pairs.

If we count the shared electrons and the non-bonding electrons for each oxygen atom, we get 8 electrons. Carbon monoxide consists of a carbon atom and an oxygen atom linked by a triple bond, consisting of two covalent bonds and one dative covalent bond.

It is the simplest oxycarbon and isoelectronic with cyanide anion, nitrosonium cation and molecular nitrogen. Explanation: Diatomic oxygen is composed of the same two elements and they also share the 4 electrons which form the double bond between them.

They are also electronegative, which means there are no undercharges for any element. Since none of the atoms pull harder, there is a non-polar covalent bond. The weakest of the intramolecular or chemical bonds is the ionic bond. There are weaker intermolecular bonds or more correct forces. Ionic bonds are created when atoms transfer electrons to each other and form ions that are electrically attracted to each other and form a bond between them.

The shape formed is called tetrahedral. Nitrogen atoms have five outer electrons so needs three more for a full outer shell.

Nitrogen forms three single covalent bonds to hydrogen atoms. The shape formed is called trigonal pyramidal. Oxygen atoms have six outer electrons so need two more for a full outer shell. The oxygen forms two single covalent bonds with the two hydrogen atoms. The shape formed is called angular. More than one bond can be formed between atoms leading to double and triple bonds.

Examples of these are diatomic oxygen double bond or nitrogen triple bond. This could also be written as:. Substances that consist of covalent molecules are usually gases or liquids at room temperature because the attractions between molecules are weak and easy to overcome. Individual H 2 O molecules are V-shaped, consisting of two hydrogen atoms depicted in white attached to the sides of a single oxygen atom depicted in red.

Neighboring H 2 O molecules interact transiently by way of hydrogen bonds depicted as blue and white ovals.