3. Chemical bonds

Question 1

Stable electron configuration (ions)

Answer 1

In group 1 (alkali metals) they form single charged ion, and form a stable octet to adopt stability like noble gases. Lithium ion would be Li 1+ so the elec.config.  would be 1s2.
Same with group 2, they form double charged ion, and form a stable octet to adopt stability. 
Group 4, they can form ions with losing or gaining 4e- to form a stable octet to adopt stability. 
Group 7 (halogen) react with metals, and form single charged ion, to form a stable octet Clorine ion would be Cl 1- so the elec.cogfig. would be1s2 2s2 2p6 3s2 3p6, 3 sublevel has the highest energy so adding 6+2= 8

Question 2

Ionic bond

Answer 2

Ionic: it is bonds forms between metals and non-metals. The nature of bonds can be predicted from the periodic table from the position of the atoms and electronegativity. The further apart the elements are on the periodic table, the more ionic bonds they have. Electronegativity differ by more than about 1.8

Question 3

Covalend bond

Answer 3

Covalent: it is bonds forms between two non-metals. The atoms are held by electrostatic attraction because both nuclei attract the e- to them both. Some atoms share more than pair of e- to form double bond or triple bond. Covalent bond could be polar, when there is difference in electronegativity between the two atoms, they form a polar covalent bonds, the greater electronegative atom has Ȣ- and with less electronegative atom has Ȣ+, ex. H-Cl. Electronegativity difference up to about 1.8 Covalent bond could be non-polar, when there is no difference in electronegativity the compound will have covalent non-polar bonds ex. Cl-Cl.

Question 4

Coordinate

Answer 4

Coordinate: molecules form stable molecule and have central atoms with fewer than eight electrons (incomplete octet) or more than eight electrons (expanded octet) in their valence shell. Molecules with incomplete octet have very small central atoms, and have tendency to form dative compounds, they gain an octet by reacting with lone pair atoms (two e- in their valence shell) ex. BeCl2
Sometimes as the bond forms by both the electrons in the pair from the same atom, this means the other atom accepts and gains a share in a donated electron pair, where they gain an octet by reacting with lone pair.

Question 5

hybridization types sp

Answer 5

Sp: this hybridization produced with triple bond, ex. Ethyne, carbon forms triple bond with the other carbon, each contain 2 sigma bonds one with carbon the other with hydrogen, each carbon has two unhybridized p orbital, as they overlap they form two pi bonds.

Question 6

hybridization types sp2

Answer 6

sp2: this hybridization produced with double bond, ex. Ethane, carbon forms double bond with other carbon, and it forms 3 sigma bonds with carbon and two hydrogen. The carbon each has one unhybridized p orbital that forms the pi bond. This forms planar triangular shape with bond angel 120 degree.

Question 7

hybridization types sp3

Answer 7

sp3: this hybridization produced with single bond, ex. Carbon forms four single bonds with hydrogen forms a tetrahedron shape with bond angel 109.5 degree.