Chapter 3 Bonding and Chemical Interaction

Question 1

Ionic Bonding

Answer 1

one or more electrons from an atom with a low ionization energy, typically a metal, are transferred to an atom with a high electron affinity, typically a nonmetal. Form between atoms that have significantly different electronegativities. the difference in electronegativity must be greater than 1.7 on the Pauling scale.

Question 2

Covalent Bonding

Answer 2

an electron pair is shared between two atoms, typically non-metals, that have relatively similar values of electronegativity. The degree to which the pair of electrons is shared equally or unequally between the two atoms determines the degree of polarity in the covalent bond.

Question 3

Coordinate Covalent

Answer 3

If both of the shared electrons are contributed by only one of the two atoms, the bond is called coordinate covalent.

Question 4

Incomplete octet

Answer 4

These elements are stable with fewer than 8 electrons in their valence shell and include hydrogen (stable with 2 electrons), helium (2) lithium(2), beryllium(4), and boron (6).

Question 5

Expanded Octet

Answer 5

Any element in period 3 and greater can hold more than 8 electrons, including phosphorus (10), sulfur (12), chlorine (14), and many others.

Question 6

Odd numbers of Electrons

Answer 6

Any molecule with an odd number of valence electrons cannot distribute those electron to give eight to each atom; for example, nitric oxide (NO) has eleven valence electrons.

Question 7

Cation

Answer 7

An atom that loses an electron and has an overall positive charge.

Question 8

Anion

Answer 8

An atom that gains an electron and has an overall negative charge.

Question 9

Crystalline Lattice

Answer 9

In a solid state, the ionic constituents of the compound form this structure, consisting of repeating positive and negative ions. This arrangement maximizes the attractive forces between oppositely charged ions and minimizes the repulsive forces between ions with similar charges.

Question 10

Ionic Compound Characteristics

Answer 10

-High Melting and boiling points due to electrostatic compounds.
-Solubility of ions in water due to interactions with polar solvents
-Good conductors of heat and electricity.
- Crystal lattice arrangement to minimize repulsive forces.
- Large electronegativity difference between ions.

Question 11

Nonpolar Covalent Bond

Answer 11

Atoms that have identical or nearly identical electronegativities share electron pairs, they do so with equal distribution of the electrons, no separation of charge across the bond. Any bond between atoms with a difference electronegativity less than 0.5 is generally considered nonpolar.

Question 12

Polar Covalent Bond

Answer 12

bonds with atoms that differ moderately in their electronegativities will share electrons unevenly.

Question 13

Dipole Moment

Answer 13

polar bond of polar molecule is a vector quantity given by the equation p=qd. where p is the dipole moment, q is the magnitude of the charge, and d is the displacement vector separating the two partial charges. Measured in Debye units (coulomb-meters).

Question 14

Lewis Base

Answer 14

any compound that will donate a pair of electrons to form a covalent bond

Question 15

Lewis Acid

Answer 15

any compound that will accept a lone pair of electrons

Question 16

VSEPR(valence shell electron pair repulsion theory)

Answer 16

Uses lewis dot structures to predict the molecular geometry of covalently bonded molecules. It states that the three-dimensional arrangement of atoms surrounding a central atom is determined by the repulsion between bonding and nonbonding electron pair in the valence shell of the central atom.

Question 17

Electronic Geometry

Answer 17

describes the spatial arrangement of all pairs of electrons around the central atom, including both the bonding and the lone pairs.

Question 18

Molecular Geometry

Answer 18

Describes the spatial arrangement of only the bonding pairs of electron.

Question 19

The coordination number

Answer 19

Which is the number of atoms that surround and are bonded to a central atom, is the relevant factor when determining molecular geometry.

Question 19

London dispersion forces(van der Waals force)

Answer 19

The attractive or repulsive interactions of these short-lived and rapidly shifting dipoles. LDF’s increase in strength with the size of the atom or molecule. More Electrons= more polarizability