Chemical Bonding

Question 1

Valence Electrons

Answer 1

• Electrons in the outermost orbit
• Used to bond with other atoms

Question 2

Octet Rule

Answer 2

Atoms tend to gain , loose , or share electrons to fill their outermost energy level with eight valence electrons.

Question 3

Cation

Answer 3

Positive Ion

Question 4

Anion

Answer 4

Negative Ion

Question 5

Polyatomic Ion

Answer 5

When more than one element groups together and has a charge.

Question 6

Intramolecular bonding

Answer 6

• Forces that hold atoms together within a molecule
• 3 types : Ionic , Metallic, Covalent

Question 7

Ductility

Answer 7

Ability to stretch

Question 8

Malleability

Answer 8

Ability to be bent or hammered out of shape

Question 9

Sea of electrons

Answer 9

The body of delocalized electrons that surrounds positive metal ions in metallic bonds

Question 10

Alloy

Answer 10

Formed when other elements are introduced into a metallic crystal.
- have chemical and physical properties that are better suited to certain applications

Question 11

Substitutional alloy

Answer 11

Atoms of the original metal are replaced by other metal atoms of the same size.
( e.g, Brass, Bronze, Sterling Silver)

Question 12

Interstitial alloy

Answer 12

The small holes in the metallic crystal are filled with smaller atoms.
(e.g., Steel)

Question 13

Single bond

Answer 13

Atoms share a single pair of electrons

Question 14

Double bond

Answer 14

Atoms share two pairs of electrons

Question 15

Triple bond

Answer 15

Atom shared three pairs of electrons

Question 16

Network Covalent Crystal

Answer 16

Atoms that are covalently bonded to each other

Question 17

Resonance

Answer 17

Structures that differ only in the position of double or triple bonds (shows all different positions of a bond on an atom)

Question 18

Electron domain

Answer 18

The number of locations on the central atom where bonding can occur

Question 19

Parent geometry

Answer 19

The geometry shape when all possible bonding locations are occupied by bonds (linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral)

Question 20

Intermolecular bonding

Answer 20

The attractive and repulsive forces between covalent molecules

Question 21

What does VSEPR stand for? What does it allow us to do? How?

Answer 21

Valence Shell Electron Pair Repulsion Theory
- allows us to predict 3-D shape of a mole from from its Lewis structure
- Based on geometry that minimizes the repulsion of electrons around the central atom