C8|CHEMICAL BONDING

Question 1

Types of bonds

Answer 1

Ionic bonds formed by electrostatic attractions between oppositely charged ions.

Covalent bonds from sharing of electrons

Metallic Bonds usually in solid metals where bonding electrons are relatively free to move throughout 3D structure from delocalized sharing of electrons in metals

Question 2

Ionic bonding

Answer 2

Transfer leads to 3D lattice of charged particles.
Stability result from strong Electrostatic attractions between ions and surrounding opp charge.
Magnitude of these interactions are measured by lattice energy.

Question 3

Lattice Energy

Answer 3

Energy required to separate completely the ions in an ionic solid into its gaseous ions.
Increases with increasing charge on ion and increases with smaller distance between the ion.

Question 4

Bond Polarity

Answer 4

Degree to which electrons are unequally shared between atoms in chemical bond.

Question 5

Bond Polarity in Covalent bonds

Answer 5

Non polar are equally shared
Polar Covalent bond are one where atoms exert greater attraction for electrons than other

Question 6

Electronegativity

Answer 6

Measure of ability of atom bonded to another atom to attract electrons to itself.
Increases across period and up a group.
The greater the EN the more polar the bond

Question 7

Polar molecule

Answer 7

Has positive and negative side as is a molecule that possess non zero moment.

Question 8

Dipole moment (D)

Answer 8

Increase as increasing amt of charge separated and increasing distance of serperation

Question 9

Exceptions to bonding rules

Answer 9

When difference in EN of atoms are relatively small
When Oxidation state of metal becomes large.

Question 10

Resonance structures

Answer 10

Individual Lewis structures in cases where 2 or more lewis structures are equally good descriptions of a single molecule. Resonance structure therefore averaged to give more accurate description of real molecule

Question 11

Exceptions to octet rule

Answer 11

Molecule has odd number of electrons
Impossible to complete octet without forming unfavorable distribution of electrons
Large atom surrounded by atoms with small EN more than an octet of electron around it.

Question 12

Strengths and lengths of Covalent bonds

Answer 12

Avg bond enthalpy measures it.
Greater the bonds=greater Avg bond enthalpy =stronger

Question 13

Valence Bond Theory

Answer 13

Model on chemical bonding in which the electron-pair bond is formed between 2 atoms by the overlap of orbitals on 2 atoms.