Chemistry Ch. 6

octet rule exceptions

( H, He, B, Al, F, Cl)

what is the difference between a single, double, and triple bond

-a single bond shares 1 pair of electrons -a double bond shares 2 pairs of electrons (greater bond energy and are shorter than single bonds) -a triple bond shares 3 pairs of electrons (strongest and shortest)

list out the bonds in order from strongest to weakest

-polar covalent -nonpolar covalent -ionic -metallic bonds

what are the differences in electronegativity for non polar covalent, polar, and ionic

0-0.3 0.3-1.7 >1.7

Order of strength of intermolecular forces

1. Hydrogen Bonding (strongest) 2. Dipole Dipole 3. London Dispersion (weakest)

Metallic Bonds

Metallic bonds happen due to the attraction between metal atoms and the surrounding "sea of electron". In metallic bonds, large D-orbitals are overlapping each other. This helps create a "sea of electrons" that the electrons are able to travel along easily. It also allows the metals to hold their electrons looser so they are more conductive of electricity. Since the electrons can travel so easily, they can slide past each other, making the metals ductile. Metallic properties include conductivity of electricity, malleability, ductility, luster, and high melting points.

how to form a covalent bond

When atoms are separated by a distance large enough to prevent them from influencing each other, the overall potential energy is zero. As the atoms get closer to each other, their charged particles begin to interact. The approaching nuclei and electrons are attracted to each other. This causes the potential energy to decrease. At the same time, the nuclei and electrons repel each other, creating an increase in potential energy. The attractive force continues to dominate and the total potential energy continues to decrease until a distance is reached at which the repulsion between the like charges equals the attraction of the opposite charges. At this point, the potential energy is at a minimum and a stable molecule forms. The atoms then get even closer which results in a sharp rise in potential energy as repulsion becomes increasingly greater than attraction.

ionic bonds

chemical bonding between cations and anions. They transfer electrons.

octet rule

chemical compounds form so that each atom, by gaining, losing, or sharing electrons, will have an octet of electrons in its highest occupied energy level

non polar covalent

covalent bond that equally share electrons

polar covalent

covalent bond that unequally shares electrons

what kind of reaction occurs when energy is taken in

endothermic

what kind of reaction occurs when energy is released

exothermic

metallic bonding

happens due to the attraction between metal atoms and the surrounding "sea of electrons"

Hybrid Orbitals

orbitals of equal energy produced by the combination of two or more orbitals on the same atom

Intermolecular forces

the forces of attraction between molecules

Hybridization

the mixing of 2 or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energy

Covalent bond

Chemical bonds between 2 atoms that share electron pairs

Difference between non-polar covalent, polar covalent, and ionic

Non-polar covalent and polar covalent are both covalent bonds. This means that they share electrons. This is usually between two nonmetals. However, these bonds differ when it comes to how the electrons are shared. Nonpolar covalent bonds share electrons equally. A nonpolar bond is Methane (CH4). In contrast, polar covalent bonds share electrons unequally. An example of a polar bond is Hydrochloric Acid (HCl). Polar bonds are also stronger than ionic and nonpolar bonds. Non polar bonds are stronger than ionic bonds. In polar bonds the difference the electronegativities of the atoms being bonded is between 0.3-1.7. The difference of electronegativity for nonpolar is 0-0.3. Ionic bonds are weaker than both polar and nonpolar covalent bonds. Ionic bonds also transfer electrons. Ionic bonds typically occur between a metal and a nonmetal. In Ionic bonds the differences of the elctronegativities of the atoms being bonded is greater than 1.7. An example of an ionic bond is Sodium Chloride.

chemical bond

a mutual electronic attraction between the nuclei and valance electrons of different atoms