WK4 - Covalent Bonding

• Covalent bonding is described in terms of electron sharing.
• The Lewis structure of molecular covalent compounds is drawn.
• The properties of covalent molecular compounds are explained in terms of their structure.
• A bond results from the attraction of nuclei for electrons, with all atoms aiming to achieve a stable octet.
• In a bond, the protons in one nucleus are attracted to the electrons of another atom, which is known as Electronegativity.
• Ionic bonding forms ionic compounds through the transfer of valence electrons.
• Metallic bonding is always formed between two metals, such as solid gold, silver, lead, etc.
• Covalent bonding forms molecules by sharing valence electrons.
• Covalent bonding occurs between nonmetal atoms which need to gain electrons to get a stable octet of electrons or a filled outer shell.
• In covalent bonding, a symbol represents the kernel of the atom (nucleus and inner electrons), dots represent valence electrons, and the ones place of the group number indicates the number of valence electrons on an atom.
• In covalent bonding, a valence electron is drawn on each side (top, right, bottom, left) before pairing them.
• Atoms in covalent bonding are trying to complete their valence shell, with 2 electrons being ideal but 8 being great.
• The total number of electrons the atoms need is the total number of bonds they can make.
• Terminal atoms have the fewest unpaired electrons.
• Boron only needs 6 valence electrons, it is an exception.
• Multiple bonds (double and triple bonds) can be formed by C, N, O, P, and S.
• In a triple bond, atoms share three electrons (6 electrons).
• The atoms form a covalent bond by sharing their valence electrons to get a stable octet of electrons, which is a filled valence shell of 8 electrons.
• In a double bond, atoms share two electrons (4 electrons).
• When carbon is one of the atoms, it will always be in the center.
• Electron-Dot Diagrams of the atoms are combined to show the covalent bonds.
• Sometimes you only have two atoms, so there is no central atom.
• Central atoms have the most unpaired electrons.
• Covalently bonded atoms form molecules.
• All valence electrons of the atoms in Lewis structures must be shown.
• The method ANS (Available, Needed, Shared) is used to draw Lewis dot structures for molecules.
• Generally each atom needs eight electrons in its valence shell, except Hydrogen needs only two electrons and Boron needs only 6.