Chapter 8 - Basic Concepts of Chemical Bonding

Question 1

8.1

Define “chemical bond”. What are the 3 types?

Answer 1

Whenever 2 atoms or ions are strongly attached to each other

Ionic, covalent, metallic

Question 2

8.1

Define “ionic bond”.

Answer 2

Electrostatic forces that exist between ions of opposite charge.

• Ions may be formed from atoms by the transfer of 1+ electrons from one atom to another.
• Ionic substances generally result from the interaction of metals on the left side of the periodic table w/ nonmetals on the right side (except for noble gases)

Question 3

8.1

Define “covalent bond”.

Answer 3

Results from the sharing of electrons between 2 atoms.

-Nonmetallic elements with one another

Question 4

8.1

Define “metallic bond”.

Answer 4

Found in metals (ex. Cu, Fe, Al)

• Each atom in a metal is bonded to several neighboring atoms
• Bonding electrons relatively free to move throughout the 3D structure of the metal
• Give rise to typical metallic properties (high electrical conductivity, luster)

Question 5

8.1

Define “valence electrons”.

Answer 5

Electrons involved in chemical bonding, which, for most atoms, are those residing in the outermost occupied shell of an atom.

Question 6

8.1

Define “Lewis symbol”.

Answer 6

Consists of the chemical symbol for the element & a dot for each valence electrno.

Ex. S has the electron configuration [Ne]3s2 3p4, so it’s lewis symbol is an S with 6 electrons around it.

Question 7

8.1

Define “octet rule”.

Answer 7

Atoms tend to gain, lose, or share electrons until they’re surrounded by 8 valence electrons.

Why?

Noble gases (except He) has 8 valence electrons, so atoms undergoing reactions also end up with 8 valence electrons.

Question 8

8.1

An octet of electrons consists of full _ and _ subshells in an atom.

Answer 8

s, p