CHEMISTRY

DEFINITIONS

100

Define:

Covalent Bond

A shared pair of valence electrons that are held together in a covalent bond.

200

Define: 

Anion

A negatively charged ion. 

300

Define: 

Cation

A positively charged ion.

400

Define: 

Valence Electrons

Electrons that exist farthest from the nucleus.

500

Define: 

Polyatomic Ions

Ions that are formed when a group of atoms gains or loses electrons.

LEWIS STRUCTURE

100

What is the Lewis Structure?

The Lewis structure is a diagram that represents the bonding between atoms in a molecule and shows the lone pairs of electrons that may exist in the molecule.

200

What do the dots Represent in the Lewis Structure?

The Valence Electrons 

300

Where do you find the Valence Electrons on the Periodic Table?

The group/column. 

400

Give an example of a group/column, and what it represents.

Group 6A has 6 Valence electrons. 

500

Give the Lewis Structure for Hydrogen

^.H

POLYATOMIC IONS

100

name this polyatomic ion:

NH₄⁺

ammonium

200

name this polyatomic ion:

SO₃^2-

sulfite

300

name this polyatomic ion:

PO₄^3-

phosphate

400

name this polyatomic ion:

CrO₇^2-

dichromate

500

name this polyatomic ion:

C₂H₃O₂^-

Acetate

EVERTHING ELECTRON

100

What charge does the electron have?

A negative charge.

200

In the Plum Pudding Model, where are the electrons?

Inside the positively charged "pudding"

300

In the Rutherford Model, where are the electrons?

The are on the outside, rotating around the nucleus.  

400

What is the Octet Rule?

Most atoms strive to attain, 8 valence electrons.

500

How many electrons should be in the D orbital?

5 electrons per 2 rings